HYDROGEN CHLORIDE(1)
A) Answer the following:
1) Why is Hydrogen chloride not collected over water ?
2) Choose the letter A, B C or D to match the description given below:
A) Ammonia
B) Hydrogen chloride
C) Hydrogen sulphide
D) Sulphur dioxide
This has gives a white precipitate when reacted with silver nitrate solution acidified with dilute nitric scid.
3) A colourless gas (G) is passed through a solution of silver nitrate, when a curdy white precipitate (P) is formed. The precipitate is insoluble in di. Nitric acid but soluble in Ammonia solution. Name G and P.
4) Why does hydrogen chloride fume in moist air ?
5) Hydrochloric acid is not very expensive. give reason.
6) Why is high temperature is avoided in the preparation of hydrogen chloride from sodium sulphate and concentrated sulphuric acid.
7) Conc. nitric acid is not used for the preparation of HCl. Why ?
8) Explain why the following statement is not correct ?
"Lead chloride can be prepared by adding dilute hydrochloric acid to lead sulphate solution.
9) From the following list of substances: ammonium chloride, ammonium nitrate, chlorine, dilute hydrochloric acid, iron, lead nitrate, manganese (IV) oxide, silver nitrate, sodium nitrate, Sodium and nitrite and sulphur-
Choose those which meet the description given below:
Two compounds whose aqueous solutions give white percipitate with dilute hydrochloric acid.
10) State what is observed when hydrochloric acid is added to Silver nitrate solution.
11) What do you observe when concentrated hydrochloric acid is added to lead (IV) oxide with the warming ?
12) What would you see when hydrogen chloride is mixed with Ammonia ?
13) What happens when dilute hydrochloric acid is added to lead nitrate solution.
14) Write balanced equation for the following reaction:
Red lead (trilead tetroxide) is warmed with concentrated hydrochloric acid.
15) Write balance chemical equation for the following reaction:
Zinc and dilute hydrochloric acid.
16) Select from the list given below (A to F), the one substance which matches the given description.
A. Ammonia
B. Copper oxide
C. Copper sulphate
D. hydrogen chloride
E. hydrogen sulphide
F. lead bromide
This compound can be oxidised to chlorine.
17) Write a balanced equation for the following reaction:
Sodium chloride from sodium carbonate solution and dilute hydrochloric acid.
F) COMPLETE AND BALANCE THE EQUATION:
1) Pb₃O₄+ + 8HCl(con) --> 3PbCl₂
2) Zn+ 2HCl(dil)----->ZnCl₂
3) KCl + H₂SO₄(ᶜᵒⁿᶜ) -> .... + .....
4) Cu + HCl(dil) --> .... + ......
5) Cuo + HCl(dil) ---> ..... + .....
6) Cuo +[O]+ HCl(conc) -->
...+ .... + ......
7) K₂O + HCl(dil) -> .... + .......
8) HCl <⁵⁰⁰ᶜ=> ...... + .......
9) HNO₃(conc)+ HCl(conc) ----->
........ + ........ + ........
10) Pb(NO₃O)₂ + 2HCl(dil) --> ...
11) MnO₂(aq) + HCl --> ...+ ...+ ....
12) KMnO₄+ HCl(conc) -->
.....+ ..... + 8H₂O + Cl₂
C) NAME THE FOLLOWING :
1) Products obtained by passing Chlorine and sulphur dioxide together through water.
2) Drying agent which is used to dry Hydrogen chloride.
3) A gas Which yields dense white fumes when treated with Hydrogen chloride.
4) The gas obtained by treating metals with Hydrochloric acid.
5) The gas obtained by treating ferrous sulphide with Hydrochloric acid.
6) Covalent compound Which becomes electrovalent when dissolved in water.
7) The anion present in the following: when compound A is warmed with Conc. Sulphuric acid gives a gas Which fumes in moist air and gives dense white fumes with Ammonia.
8) The lead compound that can be used to oxidise Hydrogen chloride to chlorine.
9) A solution which gives Chlorine on oxidation.
10) A substance that turns moist starch iodide paper blue.
D) T/F. CORRECT IF IT IS FALSE :
1) Hydrochloric acid is found in the stomach of mammals.
2) Hydrogen chloride gas is obtained by treating metals with Hydrochloric acid.
3) When moist blue litmus paper is introduced into a jar of HCL, it turns red.
4) HCL gas is not combustible but it supports combustion.
5) HCL gas partially ionized in an aqueous solution.
6) HCL acid is not used to remove rust from iron sheets.
7) HCL acid gives brown fumes of ammonium chloride with Ammonia.
8) In the laboratory, HCL gas is collected by downward displacement of air.
9) HCL gas is a colourless odourless and tasteless gas.
10) HCL gas is insoluble in water.
Each Questions carries 2 marks
1) Identify the substances describe below.
a) Colourless liquid used for the preparation of aqua -regia; turns wet blue litmus red; reacts with silver nitrate solution forming a dense white precipitate .
b) Greenish yellow gas which combines with hydrogen to form hydrogen chloride gas.
2) How would you represent Hydrogen chloride and Hydrochloric acid by chemical formula? Why do they differ ?
3) What must be added to sodium chloride to obtain hydrogen chloride?
b) Write the equation for the reaction which takes place above.
4) Select from the list below, the gas which matches the description given and answer the questions that follow:
Ammonia, chlorine, HCL, Sulphur dioxide.
When gas C is mixed with gas B ( which turns moist red litmus to blue). dense white fumes are seen and there is no other product.
a) What is the name of gas B and gas C ?
b) What is the name of the product of the reaction between gas B and gas C ?
5) Manganese(IV) oxide, lead(IV) oxide and red lead (Pb₃O₄) react with concentrated hydrochloric acid liberating chlorine.
a) What is the common property being by these metal oxides ?
b) Write the equation for the reaction of concentratated Hydrochloric acid with Pb₃O₄.
6) Write the observation and balanced equations for the following reactions:
Excess of ammonia hydroxide is added to a substance obtained by adding hydrochloride acid in silver nitrate solution.
7) Salts A and E undergo reaction (a) and (b) respectively. Identify the anion present in these salts on the basis of these reactions.
a) When Silver Nitrate solution is added to a solution of A, a white precipitate insoluble in dilute nitric acid, is formed.
b) Addition of dilute hydrochloric acid to E produced an effervescence. The gas produced turns lime water milky but does not affect acidified potassium dichromate solution.
8) The following series of reactions is carried out:
a) HCL is passed into cold water.
b) Ammonia is passed into the resulting solution.
c) Sodium hydroxide solution is added to the product of (b) and solution in the warmed.
c) Silver nitrate is added to the solution resulting from (c) (Assume that the sodium hydroxide is not in excess)
Answer the question (i), (ii), (III) and about steps and respectively name (iv) about steps (a),(b), (c) and (d) respectively.
i) 1. Name the product.
2. State whether it is ionic or covalent.
ii) 1. Name the product.
2. State whether it is ionic or covalent.
iii) 1. Name the products.
2. Which of the product/s is/are covalent?
3. Write the equation for the reaction.
iv) 1. What would you see ?
2. Write the equation for the reaction.
HYDROGEN CHLORIDE (2)
1) The gastric juice secreted by the walls of the stomach contains:
a) sulphuric acid b) hydrochloric acid c) nitric acid d) acetic acid
2) When the equal volumes of hydrogen gas and chlorine gas are exposed to diffuse sunlight, the reaction:
a) does not takes place b) takes place at at moderate speed c) is explosive in nature d) none
3) In the preparation of hydrogen chloride gas from common salt the acid used is:
a) dilute sulphuric acid b) glacial Acetic acid c) conc. sulphuric acid d) carbonic acid
4) In the preparation of hydrogen chloride gas in laboratory, the reaction mixture should be:
a) kept below 10°C b) kept below 200°C c) kept above 200°C d) any of these
5) The drying agent used in the laboratory the preparation of dry HCL gas is:
a) Phosphorus pentoxide b) anhydrous calcium sulphate c) calcium oxide d) conc. sulphuric acid
6) The salt formed when sodium chloride and conc. Sulphuric acid are heated below 200°C is :
a) sodium hydrogen sulphate b) sodium sulphate c) sodium bisulphate d) either a or c
7) In order to find that a given jar is filled with HCl gas, a glass rod dipped in ____ solution is held near its mouth.
a) ammonia b) caustic soda c) caustic potash d) barium chloride
8) Hydrogen chloride gas is collected :
a) by the upward displacement of air b) downward displacement of air c) downward displacement of water d) over the mercury
9) HCL gas extremely soluble in water. One volume up water at 20°C can absorb:
a) 200 volumes of HCL b) 450 volumes of HCL c) 150 volumes of HCL d) 800 volumes of HCL
10) HCl gas turns alkaline phenolphthalein solution from:
a) pink to green b) pink to blue c) pink to colourless d) pink to yellow
11) The advantage of using inverted funnel for the absorption of HCl gas in water is:
a) it prevents back suction into the reaction mixture
b) it provides large surface area of water for absorption
c) it prevents explosion in apparatus d) both a and b
12) A non metallic hydroxide, which forms dense white fumes with HCl gas is compound of:
a) nitrogen and hydrogen b) nitrogen and oxygen c) nitrogen and carbon d) nitrogen and sulphur
13) A metallic carbonates react with dilute hydrochloric acid to form theit respective :
a) chlorides and water b) chloride and carbon dioxide gas c) chlorides, water and carbon dioxide gas d) none
14) When dilute HCl is mixed with clear solution of silver nitrate, a precipitate is formed which is:
a) yellow in colour b) silvery in colour c) curdy white in colour d) blue in colour
15) Aqua region is a mixture of:
a) 3 parts of conc. HCL and 1 part of conc. HNO₃
b) 1 part of conc. HCL and 3 parts of conc.HNO₃
c) equal parts of conc. HCL and conc. HNO₃ d) none
16)) Black copper(II ) oxide is placed in a beaker containing hydrochloric acid. After 1 hour the colour of reaction mixture changes to:
a) grey b) brown c) red d) blue
17) A chemical/chemicals which can dissolve gold is:
a)! Aqua Fortis b) aqua regia c) aqua pure d) none
18) An acid commonly applied on the surface of metal before soldering or welding is:
a) conc. sulphuric acid b) conc. nitric acidic c) conc. acetic acid d) conc. hydrochloric acid
19) The common name of hydrochloric acid is :
a) Marine acid b) muriatic acid c) solution of HCl d) none
20) Traces of hydrochloric acid is present in:
a) pancreatic juice b) gastric juice c) bile secreted by liver d) none
21) When equal volume of a mixture of hydrogen and chlorine are exposed to direct sunlight, they:
a) do not react b) react at a moderate speed c) react violently d) none
22) The acid with reacts with metallic chlorides, either without heating or with heating is:
a) conc. Nitric acid b) glacial acetic acid c) dilute sulphuric acid d) conc. Sulphuric acid
23) conc. sulphuric acid react with the Iron (II) chloride on heating to form:
a) iron(II ) sulphate and HCL only b) iron(II ) sulphate, water and HCL only c) iron(III ) sulphate and HCL gas only d) iron(III ) sulphate, water and HCL gas only
24) concentrated or dilute sulphuric acid does not react with lead chloride, because:
a) lead is lower than hydrogen in electrochemical series
b) lead is higher than the hydrogen in electrochemical series
c)!an insoluble thin layer of lead sulphate is found over lead chloride , which cuts off chemical reaction d) none
25) In laboratory , hydrogen chloride gas is prepared by heating conc. H₂SO₄ with:
a) potassium chloride b) magnesium chloride c) sodium chloride d) ammonium chloride
26) Sodium chloride is used in the preparation of hydrogen chloride gas because:
a) it is cheapest chemical b) it is readily available c) it reacts readily with conc. H₂SO₄ even without heating d) all of these
27) The sodium chloride and conc. Sulphuric acid mixture should not be heated beyond 200°C, because:
a)! sodium sulphate so formed fuses with glass apparatus and makes it useless
b) rate of evolution of HCl gas is very high and hence it is difficult to collect
c) the apparatus may crack because sodium sulphate acts as a bad conductor of heat
d) all of these
28) During the laboratory preparation of hydrogen chloride gas from common salt and conc. H₂SO₄, the salt formed is sodium hydrogen sulphate, only when the temperature of mixture is:
a) 300°C b) 250°C c) 220°C d) below 200°C
29) Hydrogen chloride gas is heavier than air because its vapour density is:
a) 17.75 b) 18.25 c) 36.5 d) 22
30) 1 volume of water at room temperature will absorb :
a) 750 c.c of HCl gas b) 200 c.c of HCl gas c) 450 c.c of HCl gas d) 650 c.c of HCl gas
31) Hydrogen chloride gas is dried by bubbling it through conc.H₂SO₄ because:
a) HCl gas does not react chemically with conc.H₂SO₄
b) conc. H₂SO₄ being dehydrating agent absorbs moisture present in the HCL gas
c) conc.H₂SO₄ is least volatile acid and hence it's vapours do not mix with HCl gas.
d) all of these
32) An Alkaline solution which gives dense white fumes with HCl gas is :
a) sodium hydroxide b) potassium hydroxide solution c) ammonium hydroxide solution d) calcium hydroxide solution
33) When silver nitrate solution is treated with hydrochloric acid a thick curdy white precipitate of silver chloride is formed. This white precipitate dissolves in excess of:
a) sodium hydroxide solution b) ammonium hydroxide solution c) potassium hydroxide solution d) calcium hydroxide solution
34) When hydrochloric acid is added in lead nitrate solution, then a precipitate of lead chloride is formed which is :
a) white in colour b) light yellow in colour c) reddish brown in colour d) deep yellow in colour
35) The precipitate lead chloride in question 34 (above) along with rest of the reaction mixture is boiled. It is seen
a) percipetate changes to orange colour
b) no changes takes in precipitate
c) precipitate redissolves and a colourless liquid is formed d) none
36) The solution of nitrate/s of a metal/s which form white precipitate with dil. HCl are:
a) Zn(NO₃)₂ sol. b) Pb(NO₃)₂ sol. c) AgNO₃ d) both b and c
37) A salt of sodium which on boiling with conc. HCl gives reddish brown fumes of nitrogen gas is :
a) Na₂S b) NaHCO₃ c) Na₂SO₄ d) NaNO₃
38) When calcium hydrogen carbonate is treated with dilute HCl , the products formed are:
a) calcium chloride and water
b) calcium chloride and carbon dioxide
c) calcium chloride, water and CO₂ gas
d) calcium chloride, water and carbon monoxide gas
39) Which is not a correct statement?
When Na₂CO₃ is treated with dilute hydrochloric acid ?
a) a lot of effervescence takes place
b) carbon dioxide gas evolved
c) carbon dioxide and carbon monoxide gas evolved
d) both a and b
40) Iron savings reacts with dilute hydrochloric acid to form:
a) iron(II) chloride and water b) iron(II ) chloride and hydrogen c) Iron(III ) chloride and hydrogen d) Iron (III) chloride and water
41) In a beaker containing dilute HCl is poured 2g of black copper oxide(II ). The beaker is left undisturbed for one hour. After this time interval the colour of reaction mixture is:
a) colourless b) light green c) blue d) yellow
42) The products formed when magnesium sulphide is treated with dil. HCl are:
a) magnesium chloride and hydrogen gas
b) magnesium chloride and sulphur
c) magnesium chloride and hydrogen sulphide gas d) none
43) The product formed when potassium hydroxide sulphide (KHS) is treated with dilute HCl are:
a) KCL and sulphur b) KCL, water and sulphur c) KCL, H₂S and water d) KCL and H₂S gas only
44) The products formed when potassium hydrogen sulphite[KHSO₃] is treated with dilute HCl are:
A) KCL and sulphur b) KCL, water and sulphur c) KCL, SO₂ gas and water d) KCL, H₂S gas and water
45) The products formed when zinc sulphite is treated with HCl are:
a) zinc chloride and SO₂ gas b) zinc chloride and SO₃ gas c) zinc chloride, SO₂ gas and sulphur d) zinc chloride, SO₂ gas and water
46) The products formed when sodium thiosulphate solution is mixed with dilute hydrochloric acid are:
a) sodium chloride, water and SO₂ gas
b) sodium chloride, water and sulphur
c) sodium chloride, water, SO₂ gas and sulphur
d) sodium chloride, SO₂ gas and sulphur
47) When copper nitrate crystals are boiled with conc. HCl, the products formed are:
a) copper(II ) chloride and water
b) copper(I ) chloride and nitric acid
c) copper(II ) chloride and nitric acid
d) copper (II) chloride, water and nitric acid
48) When MnO₂ boiled with conc. HCl, the products formed are:
a) manganese chloride and water
b) manganese chloride and chlorine
c) manganese chloride, water, chlorine d) none
49) When lead dioxide is boiled with conc.HCl, the product formed are:
a) lead (II) chloride and water
b) lead(IV ) chloride and chlorine
c) lead(II ) chloride and chlorine
d) lead+II ) chloride, water and chlorine
50) When red lead oxide [Pb₃O₄] is boiled with conc. HCl, the products formed are:
a) lead(II ) chloride and chlorine b) lead(IV ) chloride and chlorine c) lead (II) chloride and water d) lead(II) chloride, water and chlorine
51) When potassium permanganate [KMnO₄] is treated conc. HCL, the product of reaction are:
a) potassium chloride, manganese chloride and water
b) potassium chloride, manganese chloride and chlorine gas
c) potassium chloride, manganese chloride, water and chlorine gas
d) none of these
52) When potassium dichromate(K₂Cr₂O₇) is boiled with conc.HCl, the products of reaction are:
a) potassium chloride, chromium chloride and water
b) potassium chloride, chromium chloride and chlorine gas
c) potassium chloride, chromium chloride, water and chlorine gas
d) none of these
53) Which is not a correct statement ?
Hydrochloric acid is used in:
a) the manufacture of dyes, drugs and paints
b) soldering and welding of metal
c) food preservative industry
d) leather industry
54) The aim of fountain experiment is to prove:
a) HCL turns blue litmus red
b) HCl is denser than air
c) HCl is highly soluble in water
d) HCL fumes in moist air
1) Identify the following :
a) Name of experiment which shows that hydrogen chloride gas is extremely soluble in water.
b) A gas liberated when dilute hydrochloric acid is treated with magnesium.
c) A coloured gas which reacts with hydrogen gas to form hydrogen chloride gas.
d) A gas liberated when calcium hydrogen carbonate is treated with dilute hydrochloric acid.
e) A white percipitate formed when sodium chloride solution is treated with silver nitrate solution.
f) A concentrated acid (1 part) which forms aqua regia, when mixed with three parts of conc. Hydrochloric acid.
g) An element liberated when sodium thiosulphate solution reacts with dilute hydrochloric acid.
h) A salt of sodium on treating with dilute hydrochloric acid liberates Sulphur dioxide gas.
i) A nitrate of a metal (other than silvery nitrate), which forms while precipitate when treated with dilute hydrochloric acid.
j) Name the gas evolved when potassium sulphide is treated with dilute hydrochloric acid
k) Name the gas evolved when hydrochloric acid is made to react with manganese dioxide.
l) Name an acid which on mixing with silver nitrate solution produces a white percipetate which is soluble excess of ammonium hydroxide .
m) Name the gas that is produced by the action of dilute hydrochloric acid on sodium sulphide.
2) Complete the following by choosing the correct answers from the bracket.
a) The common name for hydrochloric acid is ______.(Muriatic acid/Aqua Fortis)
b) The traces of hydrochloric acid are present in ____.(pancreatic juice/ gastric juice)
c) Hydrogen gas and chlorine gas react____ when exposed to direct sunlight.(slowly/ explosively)
d) All metallic chlorides on heating with concentric____liberate hydrogen chloride gas.( nitric acid/sulphuric acid)
e) In laboratory hydrogen chloride gas is prepared by heating_____with conc. Sulphuric acid.(calcium chloride/sodium chloride)
f) During the preparation of hydrogen chloride from common salt and concentric Sulphuric acid, the salt formed is sodium hydrogen sulphate, if the reaction mixture is kept _____200°C (above/below)
g) Hydrogen chloride is collected by the upward displacement of air because its vapour density is____ as compared to air being 14.4. (36.5/18.5)
h) 1 volume up water at room temperature absorbs____ volumes of hydrogen chloride gas. (700/450)
i) Hydrogen chloride gas is dried by passing it through____. (Phosphorus pentoxide/conc. Sulphuric acid)
j) An alkaline solution which gives dense white fumes with hydrochloric acid gas is ____. (Sodium hydroxide/ammonium hydroxide.
k) Quicklime is not used to dry HCL because _____. (CaO is alkaline/ CaO is acidic/ CaO is a neutral)
l) potassium sulphite on reacting hydrochloric acid releases ____gas.(Cl₂/SO₂/ H₂S)
m) dry hydrogen chloride gas can be collected by _____displacement of air.(downward/ upward) is_____. (sodium hydrogen sulphate/sodium sulphate/chlorine)
n) The acid which cannot act as an oxidizing agent is _____.(Conc. H₂SO₄/conc. HNO₃/conc HCL)
3) Give balanced chemical equation for the following:
a) sodium thiosulphate and dilute HCl.
b) Calcium hydrogen carbonate and dilute HCl.
c) Concentrated hydrochloric acid and potassium permanganate crystals.
d) Action of dilute hydrochloric acid on sodium sulphide.
e) Action of hydrochloric acid on sodium bicarbonate .
f) Action of dilute hydrochloric acid and magnesium sulphite.
g) Action of dilute hydrochloric acid on iron.
State one Relevant Observation for each of the following:
1) When dilute hydrochloric acid is added to sodium carbonate crystals.
2) Action of dilute hydrochloric acid on iron(II) sulphide.
3) Lead nitrate solution is mixed with dilute hydrochloric acid and heated.
4) A small piece of zinc is added to dilute hydrochloric acid.
5) Dilute hydrochloric acid is added to silver nitrate solution.
6) hydrogen chloride gas fumes in moist air.
2 Marks questions
1)a) What is the property of concentrated sulphuric acid which allows it to be used in the preparation of hydrogen chloride and nitric acid ?
b) What property of hydrogen chloride is demonstrated when it is collected by the downward)?
2) Write balanced chemical equations for the following the reactions:
a) zinc and dilute hydrochloric acid.
b) calcium bicarbonate and dilute hydrochloric acid.
3) What is observed when dilute hydrochloric acid is added to silver nitrate solution.
a) Name the experiment illustrated above.
b) Which property of hydrogen chloride is demonsrated by this experiment ?
5) a) What happens when dilute hydrochloric acid is added to lead nitrate solution ?
b) Write a balance chemical equation for the action of dilute hydrochloric acid on sodium sulphite.
6) Study the figure given below and answer the questions that follow:
a) Identify the gas Y.
b) What property of gas Y does the experiment demonstrate ?
7) a) Name two acids used in the formation of Aqua regia.
b) What is the ratio of these acids ?
8) In the laboratory preparation of HCl gas from sodium chloride, state, why the following are preferred.
a) conc. H₂SO₄ as reactant.
b) temperature of the reaction mixture below 200°C.
9) The diagram shows a simple arrangement of the fountain experiment:
a) Name the two gases you have studied which can be used in this experiment.
b) What is the common property demonstrated by this experiment?
10) Give an equation of HCl gas by synthesis. State to condition involved in its synthesis.
11) Why are conventional drying agent such as calcium oxide and Phosphorus pentoxide not used for drying moist HCl? Give equations
12) Name two soluble nitrates which can be converted into insoluble chlorides by the use of dilute HCl. Support your answer by chemical equations .
3 Marks Questions
1) The diagram shows an apparatus for the laboratory preparation of hydrogen chloride
a) Identify A and B
b) Write the equation for the reaction.
c) How would you check whether or not the gas jar filled hydrogen chloride ?
2) To a solution of hydrogen chloride, the following substances are added separately in small portions . Copy and complete the table given below.
No. Substance added Gas evolved odour
1. Sodium sulphite ----- ____
2) Calcium carbonate ____ ___
3. Magnesium ribbon. ____. _____
3) In and the laboratory preparation of hydrochloric acid, HCl gas is dissolved in water.
a) Draw a diagram to show the arrangement used for the absorption of HCl in water.
b) Why is such an arrangement necessary? giuve two reasons.
c) Write the chemical equations for the laboratory preparation of HCl gas when the reactants are:
i) below 200°C
ii) above 200°C
4) Answer the following questions pertaining The laboratory person hydrogen chloride.
a) Write an equation for the laboratory refraction of hydrogen chloride.
b) Name the drying agent used.
c) Name the method of collecting hydrogen chloride gas.
5) When concentrated hydrochloric acid is treated with potassium permanganate crystal a greenish yellow gas is given out.
a) Name the gas evolved
b) Write fully balanced chemical equation for the reaction.
c) Is hydrochloric acid acting as oxidizing agent or reducing agent?
6) Hydrogen chloride gas is prepared in the laboratory using concentrated sulphuric acid and sodium chloride. Answer the questions that follow based on the reaction:
a) Give the balanced chemical equation for the reaction with suitable condition/s if any .
b) Why is concentrated sulphuric acid used instead of concentrated nitric acid ?
c) How is the gas collected ?
7) How will you obtain the following from dil. HCL acid ? Given equation
a) hydrogen
b) carbon dioxide
c) sulphur dioxide.
8) a) Hydrogen is burn in a greenish yellow gas A then another gas B is formed . The gas B gives dense white fumes with ammonia liquor . Name the gas A and B.
b) Write the chemicals equations in support of your answer in (a).
9) what is an Aqua regia? How does it help in dissolving gold or platinum? Support your answer with chemical equations.
10) Write balanced chemical reaction for the reaction of dilute hydrochloric acid with each of the following:
a) iron
b) sodium hydrogen carbonate
c) iron (III) sulphide
11) The diagram shows an apparatus for the laboratory preparation hydrogen chloride.
a) identify A and B.
b) Write the equation for the reaction.
c) How would you check whether or not the gas is filled with hydrogen chloride ?
12) a) Name the acid used for the preparation of hydrogen chloride gas in the laboratory. Why is this particular acid preferred to other acids ?
b) Write the balanced chemical equation for the laboratory preparation hydrogen chloride gas.
b) For the preparation of hydrochloric acid in laboratory:
i) Why is direct absorption of hydrogen chloride gas in water not feasible ?
ii) What arrangement is done to dissolve hydrogen chloride gas in water ?
PERIODIC TABLE
A) FILL IN THE BLANKS :
1) The serial number of an element in the pieriodic Table is also its____. (Atomic number /mass number )
2) The metallic character_____in a Group as one moves from top to bottom. (Increases/decreases.
3) The metallic character____ in a Period as one moves from left to right. (Increases/decreases).
4) _____is the most active nonmetal.(Chlorine/ Iodine)
5) _____is the most active metal.(Magnesium/ sodium)
6) An increase in nuclear charge____ the tendency of an atom to accept electrons. (Increases/ decreases)
7) The atomic size____as one moves from left to right across a Period.(Increases/ decreases)
8) The element in Group VIIA which is a liquid at room temperature is____. (F/ Cl/ Br)
9) Nuclear charge of an atom is the____(negative/positive) charge on the nucleus of an atom, equivalent to the atomic____(numbers/mass) of an atom.
10) Atomic size of neon is_____than the atomic size of fluorine.(More/ less)
11) With increase in nuclear charge the nuclear attraction for outer electron____(increasees/ decreases), Hence ionisation potential____(increases/ decreases).
12) If an element has one electron in its outermost shell. Then it is likely to be____. (Non metallic/ metallic)
13) The Properties of elements are periodic functions of their____. (Atomic numbers/ mass numbers)
14) The element below sodium in the same Group would be expected to have a___. (Lower / higher) electronegativity than sodium and the element above chlorine would be expected to have a_____(lower / higher) ionisation potential than chlorine.
15) On moving from left to right in a given Period, the number of shells___. (Remains the same/ increases/ decreases)
16) On moving down a Group, the number of valence electrons_____( remains the same/ increase/ decreases)
B) CHOOSE CORRECT OPTION:
1) The chemical properties of an element depends on its:
a) atomic mass
b) atomic number
c) atomic energy
d) atomic volume
2) Total number of vertical columns (Groups) in the Long Form of the Periodic Table is :
a) 8 b) 18 c) 17 d) 16
3) The element having the lowest ionisation potential in period 3 is:
a) Na b) K c) Mg d) A
4) The number of elements present in Period 3 is :
a) 6 b) 32 c) 18 d) 8
5) On going down a Group, the number of valence electrons.
a) increases b) decreases
c) remains the same
d) varies irregularly
6) The number of Periods in the Long Form of Periodic Table is:
a) 6 b) 7 c) 8 d) 10
7) On moving down a Group, the size of atoms :
a) increases b) decreases
c) remains the same
d) varies irregularly
8) Which one of the following ions has the smallest radius ?
a) Cl⁻ b) K⁺ c) S²⁻ d) Ca²⁺
9) On moving from left to right in a Period the metallic character of elements:
a) increases
b) decreases
c) remains the same
d) varies irregularly
10) The correct order of decreasing first ionisation potential is :
a) C > B > Be > Li
b) C > Be > B > Ki
c) B > C > Be > Li
d) Be > Li > B > C
11) Which halogen has the highest electron affinity ?
a) F b) Cl c) Be d) I
12) The most electronegative element in the Period Table is:
a) N b) O c) Cl d) F
13) Which has the smallest size?
a) Na⁺ b) Al³⁺ c) Mg²⁺ d) P⁵⁺
14) Which of the following is the correct order of ionisation potential in the Periodic Table?
a) F > O > N > C
b) O > F > N > C
c) O > N > F > C
d) C > N > O > F
15) The electron affinity for noble gases is likely to be:
a) high b) small c) zero d) Positive
16) Which of the following has the highest electron affinity?
a) F b) O c) O⁻ d) Na⁺
17) The size of a positive ion is:
a) more than its atom.
b) less than its atom
c) equal to its atom
d) none of the above
18) Which one of the following is correct order of the size ?
a) I > I⁻> I⁺
b) I > I⁺> I⁻
c) I⁺ > I⁻> I
d) I⁻ > I > I⁺
19)The size of chloride ion (Cl⁻) is
a) smaller than chlorine atom
b) bigger than chlorine atom
c) equal to that of chlorine atom
d) none of the above
20) The ionic radii of N³⁻ , O²⁻ , F⁻ and Na⁺ follow the order
a) N³⁻ > O²⁻ > F⁻ > Na⁺
b) N³⁻ > Na⁺ > O²⁻ > F⁻
c) Na⁺> O²⁻ > N³⁻ > F⁻
d) O²⁻ > F⁻ > Na⁺ > N³⁻
C) NAME THE FOLLOWING:
1) The element present in the first Period.
2) The biggest atom in the third Period.
3) A solid halogen.
4) The smallest element of third Period.
5) The family of elements to which chlorine belongs.
6) The family of elements to which sodium belongs.
7) The family of elements to which argon and neon belongs.
8) Least electronegative element of halogen family.
9) A non metal which has three electrons in its outermost shell.
10) The smallest atom in the third Period.
11) The least reactive elements in Group IA.
12) The most metallic element in the third Period.
13) The most nonmetallic element in the third Period.
14) The element which is most electronegative in the third Period.
15) A greenish yellow gas other than chlorine.
16) The most abundant halide salt.
17) The element which has the highest ionisation potential.
18) The element of third Period which has least ionisation potential.
19) The most electronegative element of second period.
20) An element in period 3 with electronegativity 3.0.
21) The element with the least ionisation potential in the 2nd period.
22) The element which has the highest electron affinity in the third Period.
23) The noble gas having an electronic configuration 2,8,8.
24) The valency of elements in Group I.
25) An element of group VIIA, solid at room temperature.
D) TRUE/FALSE
1) The electron present in the outermost shell are called valence electrons.
2) In a group, atomic and ionic radii decrease from top to bottom due to increase in the number of shells.
3) The electron affinity of elements increases in a group from top to bottom and decreases along a Period from left to right.
4) The amount of energy required to remove a loosely bound electron from the outermost shell of an isolated atom is called ionisation potential.
5) Electron affinity is the property of an atom to attract electrons towards itself, when combined to form a compound.
6) Lithium resembles radium and potassium in electropositive character and univalency.
7) The element in a Group have consecutive atomic Numbers.
8) On going down in a Group of the Modern Periodic Table, the metallic character of elements increases.
9) The tendency of an atom of an element to donate or lose electrons is called electropositivity.
10) Iron is a non-metal.
E) DEFINE:
1) Periods in Periodic table
2) Group in Periodic table
3) Periodicity
E) ANSWER THE FOLLOWING:
1) What are Periods ?
2) How many electrones are present in the valency shell of the element with the atomic number 18 ?
3) Explain why electron affinity of an atoms increases from left to right along a Period in the Modern Periodic Table.
3) What happens in the number of valence electrons in the atoms of elements as we go down in a Group of the Modern Periodic Table ?.
4) From amongst Be, B, and C, choose the element with the highest ionisation potential.
5) What is similar in the electronic structure of Li, Na, and K ?
6) Which of the following elements are in the same Group of the Periodic table ? Magnesium, Nitrogen, Beryllium, Sulphur
7) Which group of elements was missing from Mendeleev's original Periodic table
8) State the Periodic law on which Mendeleev's Periodic table was based ?
9) In the Long Form of the Periodic Table. the elements are arranged according to their mass numbers. Is this statement correct ? if not, correct it.
10) How could the atomic radius of a noble gas compered with other elements in a Period ?
11) What similarity do halogen show in their molecular state ?
12) Why is ionization potential of O less that of N ?
13) Explain why the elements with low ionisation potential exhibit metallic properties.
14) Account for the difference in size of Fe²⁺ and Fe³⁺ as Fe²⁺ = 0.76 A° and Fe³⁺ = 0.64 A°.
15) Give the formula of one species positively charged and one negativity charged that will be iso-electronic with Ne.
16) Mg²⁺ ion is smaller than O³ ion althrough both are iso-electronic. Explain.
17) What is the probable formula of the oxide of silicon ? (Silicon occurs below carbon in the Periodic Table)
18) What would you expect the formula of a compared of hydrogen with an element I to be ? ( use I as the symbol of the element.)
19) How do the nature of oxides of the elements change on moving from top to bottom in a Group of the Periodic Table?
Give example.
20) What is the common feature of the electronic configuration of the elements at the end of Period 2 and Period 3 ?
21) if an element is in group 7(or group 7A). is it likely to be metallic or nonmetallic in character ?
22) What is meant by a group in a Periodic Table ?
23) theelectronegativities of the elements in period 3 of the Periodic Table are as follows with elements arranged in alphabetical order:
Al Cl Mg Na P S Si
1.5 3.0 1.2 0.9 2.1 2.5 1.8
Arrange the elements in the order in which they occur in the Periodic Table from left to right. ( The group 1 element first, followed by the group 2 element and so on, up to Group 7.)
24) Predict the Group of an element X if its atomic number is 16.
25) Select the correct order of radii of three species Ca, Ca⁺ and Ca²⁺
a) Ca > Ca⁺ > Ca²⁺
b) Ca²⁺ > Ca⁺ > Ca
c) Ca⁺ > Ca > Ca²⁺
d) Ca⁺ > Ca²⁺ > Ca
Assign suitable reason.
26) Electron affinities of two elements A and B are as follows:
A=3.79 eV and B= 3.56 eV
Which of them will ionise more easily and why ?
27) How does the number of valence electrons vary on moving from left to right:
a) in the first Period of the Periodic Table?
b) in the second Period of the Periodic Table?
c) in the second Period of the Periodic Table?
28) The elements lithium, sodium and potassium were put in one Group on the basis of their similar properties.
a) What are those similar properties
b) What is the usual name of this Group or family.?
29) Which is larger, Na⁺ or K⁺ ? Why?
30) Chlorine , bromine and iodine elements were put in one Group on the basis of their similar properties:
a) What are those similar properties ?
b) What is the common name of this Group or family ?
31) In the following set of elements, one element does not belong to the set. Select this element. Give reason in support of your answer.
Calcium, Magnesium, Sodium, Beryllium .
32) Consider the following elements: Na, Ca, Al, K, Mg, Li
a) Which of these elements belongs to the same Period of the Modern Periodic Table ?
b) Which of these elements belongs to the same Group of the Modern Periodic Table ?
33) What is the cause of periodicity of elements in the Periodic Table?.
34) What are the following Groups known as?
a) Group IA
b) Group VIIA
c) Group Zero
35) How did the following properties vary in a Period, say Period 3 ?
a) Atomic size
b) Metallic character
c) Non-metallic character
d) Ionisation potential
e) Electron affinity
f) Electronegativity
36) a) Name the elements of Period 3.
b) Which element in Period three is likely to react most violently with chlorine.
c) Of the 8 elements in Period 3, which is likely to form a compound of the formula XCl₃ with chlorine.
37) Match the following
Column A
a) Proton
b) Sodium
c) Barium
d) Chlorine
e) Electron
f) Completed shell
Column B
i) An alkaline earth metal
ii) halogen
iii) noble gas
iv) An alkaline metal
v) Responsible for nuclear charge
vi) Occupied subshell
38) Among the elements of the second Period (Li to Ne), pick out the element.
a) with the largest atomic size.
b) with the highest ionisation potential.
c) with highest electron affinity.
d) With highest electronegativity.
e) which is the most reactive metal.
f) which is the most reactive nonmetal.
39)a) How many Groups and Periods are there in the Modern Periodic Table ?
b) On what basis is an element placed in a particular Period in a Group ?
c) The electronic configuration of three elements A, B and C are as follows:
A-- 2 8 18 18 8 1
B-- 2 8 18 18 7
C-- 2 8 18. 32 18 8
Find the respective Period and Group to which each of them belongs.
40) For each of the following pairs, predict which one has a greater ionization potential and greater electron affinity ?
a) I, I⁻
b) B, C
c) Li, Li⁺
41) What is the number of elements in:
a) first Period of the Modern Periodic Table ?
b) 2nd Period of the Modern Periodic Table ?
c) 3rd Period of the Modern Periodic Table?
42) a) What are alkali metals ?
b) In which Group and Sub groups are they are placed ?
c) What is their valency ?
d) Why do they not occur free in nature?
43) This question refery to the elements of the Periodic Table with atomic numbers from 3 to 18. Some of the elements are shown by letters, but the letters are not the usual symbols of the elements.
3 4 5 6 7 8 9 10
A B C D E F G H
11 12 13 14 15 16 17 18
I J K L M N O P
Which of these elements:
a) are noble gases ?
b) are halogens ?
c) are alkali metals ?
d) are elements with valency 4?
44) An element X belongs to Period 3 and Group II of the Periodic Table . State :
a) the number of valence electrons .
b) valency of the element.
c) is it metal or nonmetal.
d) the name of the element
45) The atoms A and B have electronic configuration (2, 8, 2) and (2,6) respectivaly.
a) to which Period do A and B belong ?
b) to which group do A and B belong ?
c) What are the valencies of A and B with respect to hydrogen ?
d) What is the formula of the compound of A and B ? Is the compound ionic or covalent in nature ?
46) An element X belongs to Period 2 and another element Y belongs to Group 15 of the Periodic Table.
a) What is the number of valence electrons in X ,?
b) What is Valency of X ?
c) What is the number of valence electrons in Y ?
d) What is the valency of Y?
47) In any vertical column of elements in the sub group A of the Periodic Table , as you go from top to bottom :
a) the elements become ____metallic (less /more)
b) the number of electronic shells ____ (increases/decreases)
c) The ionization potential ______. (decreases/ increases)
d) the electronegativity_______ (decreases/ increases).
48) a) What are noble gases ?
b) What is the speciality of the their outermost shells ?
c) in which group are they placed ?
d) why is that Group referred to as Zero Group ?
e)why are they referred to as inert gases
49) a) What are halogens ?
b) in which Group and Sub groups are they placed ?
c) What is their valency ?
d) Why are they called halogens ?
e) why do they not occur free nature ?
50) Arrange the elements of Group VIIA according to the given conditions:
a) increasing order of atomic size.
b) Increasing non metallic character.
c) increasing ionization potential.
d) increasing electron affinity.
e) decreasing electronegativity .
51) The electronic configuration of an elements T is 2, 8, 7.
a) What is the Group number of T ?
b) What is the Period number of T ?
c) How many valence electrons are there in an atom of T ?
d) What is the valency of T ?
e) is it a metal or nonmetal ?
52) Arrange the following elements as per the guidelines in brackets.
a) Cl, Mg, Na, P( in increasing order of atomic size)
b) Al, Cl, Na, S ( in increasing order of ionization potential)
c) Ar, He, Ne (in decreasing order of number of electronics shells).
d) C, Li, F, N, (in increasing order of electronegativity)
e) C, F, Li, O, (in increasing order of electron affinity)
53) The table given below shows the mass number and the number of neutrons in 4 elements -- P,Q, R, S
Elements: P Q R S
Mass number: 12 20 23 35
No of neutrons: 6 10 12 18
a) Write down the atomic number of S.
b) Write down the electronic configuration of S.
c) To which Group S belongs ?
d) To which Period S belongs ?
e) What will be the nature (ionic or covalent) of the compound formed by
i) R and S
ii) P and S
54) The position of three elements X, Y and Z in the Periodic Table is as shown below:
Group 16 Group 17
--- X
---- -----
Y Z
a) What will be the valency of Z ?
b) What is the name of the family to which element Z belongs ?
c) State whether Z is a metal or nonmetal.
d) will Z be larger or smaller than Y ?
e) State whether Z is more or less reactive than X.
55) Fill in the blanks:
a) Group 3A elements have____ electrons in their outermost shells.
b) Nitrogen has ____electrons in its outermost shell.
c) Group zero elements have_____ electrons in their outermost shells except ____.
d) The outermost shell electrons are also known as____ electrons.
e) When an atom of magnesium unites with another to form a compound. ____electrons of magnesium are primarily involved.
56) Question (a) to (e) refer to change in the properties of elements on moving left to right across a Period of the Periodic Table . For each property, choose the letter corresponding to the correct answer from choices (i), (ii), (iii) and (iv).
a) The non metallic character of the element:
i) decreases ii) increases iii) remain the same iv) depends on the Period
b) The electronegativity :
i) depends on the member of valence electrons.
ii) remains the same
iii) decreases iv) increases
c) The ionization potential
i) goes up and down
ii) decreases iii) increases iv) remains the same
d) The atomic size:
i) decreases ii) increases iii) remains the same iv) sometimes increasees and sometimes decreases
e) The electron affinity of the elements in Group 1 to 7;
i) goes up and then down
ii) decreases and then increases
iii( increases iv) decreases
57) REASON BEHIND:
a) Sodium is referred to as a normal element.
b) Sodium and potassium are placed in Group I.
c) Noble gases have zero electron affinity values. Explain ?
d) Why is larger Na⁺ or K⁺ ? Why ?
e) Why is the electron affinity for F Less than that of Cl?
f) Why electron affinity of halogen is comparatively high. Give reason.
g) Ionisation potential of alkali metals is comparatively low.
h) Electronegativity of chlorine is higher than that of sulphur. Why ?
i) Sodium and potassium are called alkali metals . Why ?
j) Why is chlorine more reactive than bromin ?
k) Why Potassium is more reactive than sodium.
THE PERIODIC TABLE - PERIODIC PROPERTIES (2)
1) Complete the statements given below by the filling in the correct word in the blank from the word/s in bracket.
a) The periodic table based on the basic fundamental property______ (atomic weight/ atomic number/electronic configuration).
Modern Periodic Table has :
b) Elements arranged increasing order in atomic___ (numbers/weights).
c) _____horizontal rows called_____(5/7/18/ periods/groups).
d) ____ vertical columns called____ (6/8/18/ period/ groups).
e) Transition from ____to _&&_character across a period.( metallic/ non metallic).
f) Groups___ to___ sub-divided into A and B.( I/II/VI/VII)
g) Group ____to____are called 'normal' - ' representative elements'. (IA/II A/VIA/VIIA)
h) Group ____to____and____ are called 'transition elements'. (I B/VIB/VIIB/VIII)
i) Group _____at extreme____ contains 'noble gases' (I A/0/VIIA/right/left)
j) _______elements placed in group I A & II A. (reactive, metallic/reactive, non-metallic)
k) _____ elements placed in the upper right hand corner. (Non-metallic/metallic)
Periodicity in Properties:
l) Periodicity in Properties i.e., recurrence in properties are seen with elements belonging to the same____ (period/groups/sub-groups) in the periodic table after difference of _____ , ____ , _____ , or ____ , (18/2/32/8) in atomic numbers due to recurrence of similar ____.(atomic weights /number of shells/valence electronic configuration)
Position of Elements:
m) Alkali metals Li, Na are present in group_____(IB/IA/IIA)
n) Alkaline earth metal Be, Mg are present in group ____(IA/IIA/IVA)
o) Post-transitional metal - Al is present in group ____(IIA/IIIA/VIA)
p) Transition metal - Fe is present in group ____(VIIB/VIII/IB).
q) Transition metal - Zn is present in group ___ (IB/IIB/IIIB).
r) Lanthanide series are present in period _____(2/3/6/7)
s) Actinide series are present in period ____(2/3/6/7).
2) Name or state the following, pertaining to elements of the first three periods.
a) The number of electron shells in period- 1, 2 and 3 respectively.
b) The period number of the element 'X' having electronic configuration 2, 8, 8, 1.
c) The number of elements in the shortest period.
d) The number of short periods of the periodic table.
e) The metallic elements in period-2 and period-3.
f) The non-metallic elements in period-2 and period-3.
g) The element in period-2 and period-3 having stable electronic configuration.
h) The element in period-3 having 5 valence electrons.
i) The element in period-2 having electronic configuration 2, 4.
j) The period/s having 8 elements.
k) The element having one shell and one valence electron.
l) The period containing
i) rate earth elements
ii) radioactive elements.
m) The bridge element in period-2 which has a diagonal relationship with aluminium in period -3.
n) A metalloid in period -3.
o) The valency of the element in period-2
i) group- V
ii) group- 0.
p) The type of bonding of the chloride of the element in periodic-3, group- IIA.
q) The type of bonding of the oxide of the element in period-3, group IIIA & VIA.
r) The state of the chloride of the element in period-3 group VIA.
s) The characteristics of the oxide of the element in period-3 group IIIA & IIIA.
t) The character of the hydroxide of the element in the period-3 group -IIA.
u) The element in period-3 whose hydride is strong acid.
v) Two property trends of elements which increase from left to right in a period.
3) Name or state the following for pertaining to elements in groups of the periodic table.
a) The number of valance electrons of the elements in group IA and in IIA.
b) The group number of the group having 3 columns of elements.
c) The group number to which lithium and sodium belong.
d) The group number to which magnesium and calcium belong.
e) The group containing highly reactive, electronegative nonmetals only.
f) The group number to which elements with 7 valence electron belong.
g) The type of elements present in group I to VIIB & VIII.
h) The group to which inert, unreactive elements belong.
i) The group to which the most reactive metals belong.
j) The two property trends which remain same or similar down a subgroup.
k) The two property trends which increase down a subgroup.
l) A non-metal in group VIIA which is a liquid at room temperature.
m) Two non-metals which react with a group VIIA element forming liquid chlorides.
n) An element from group IA which reacts with an element of group VIIA forming a soluble electrovalent compound.
o) An element from group IA which dissolves in water to give caustic potash .
p) A strong reducing agent from the elements - sodium of group IA and fluorine of group VIIA.
q) The element in group VIIA with the highest electronegativity.
4) Complete the table pertaining to periodicity of elements by selecting the correct term/s in each case:
a) The Modern Periodic Law states that properties of elements are periodic functions of their _____. (atomic mass/ molecular mass/ atomic numbers)
b) The properties which reappear at regular intervals in the periodic table are called ____(atomic/ period/periodic properties)
c) _______ is one of the periodic properties, periodic in nature. (electronic configuration/ atomic radius/ electron pull)
d) ____is the energy required to remove an electron from the outermost shell of a gaseous atom . (Ionisation potential/ electron affinity)
e) The unit of ionization potential is____(mV/eV/iV)
f) ______ is the amount of energy released when an atom in the gaseous state accepts an electron to form an anion. (Ionisation potential/electronegativity / electron affinity)
g) Electronegativity is the tendency of an atom to attract____ to itself when combined in a compound.( protons/ electrons/ ions)
h) If the electronegativity difference between two combining atoms is small the bond between them is_____( electrovalent/covalent/co-ordinate covalent)
i) An element is said to be a______ if it loses one or more electron when supplied with energy. (Non-metal /metal/metalloid)
j) The unit of atomic radii is _____. (0°C/A°/eV)
k) A______ is formed from a metal by loss of electrons.(Anion/cation/proton)
l) Electron affinity of an atom is expressed in _____(A°/eV/mV)
m) An element X gains an electron when supplied with energy. The electronic configuration of X is _____(2, 8/2, 8, 1/2, 8,7)
n) An element Y has atomic number 7 and mass number 14. It's neutron/ proton (n/p) ratio is_____ 3/1.5/1)
o) In the same period or sub group, increase or decrease in a particular (periodic) property is due to gradual charge in _____.(at. wr:/atomic size/ electronic configuration) in the arranged elements.
5) Select the correct element in each case:
a) Select the elements with the largest atomic radii- C, Be, N, F, Li.
b) Select the element with the smallest atomic radii- F, Ne, O
c) Select the element which has a higher electronegativity- N, F, Cl.
d) Select the element which has zero electron affinity- C, Li, O, Ne.
e) Select the elements which show metallic character- Na, Al, Si, P
f) Select the elements which show non-metallic character- Be, C, Li, Cl.
g) Select the elements which show metalloid character-- Be, B, C, N, F, Si.
h) Select the elements which have three electron shells - Li, B, Al, S.
i) Select the element which has the common valency 3- Li, Be, B, C, Al.
j) Select the element having the least electronegativity-- F, Cl, Br.
k) Select the element having the smallest atomic size-- F, Cl, Br.
l) Select the element having the largest atomic radii- N, P, As.
m) Select two elements whose electronegativity difference is large -- Na, C, Cl.
n) Select two element whose electronegativity is almost the same --Li, F, Na, Ne.
o) Select the element with the least electron affinity-- O, C, Ne, F
p) Select the element with the highest ionization potential-- O, F, Ne.
6) Arrange the following elements of different periods As per A and B:
A: ELEMENTS C O N Li F Ne B Be
B: ELEMENTS: Mg Si S Al Cl Na Ar P
a) According to their decreasing atomic radii.
b) According to their decreasing ionization potential.
c) According to their increasing electronegativity.
d) According to their increasing electron affinity.
e) According to their metallic, non-metallic and noble gas character.
7) Arrange the following elements of different groups as per A and B:
A B
Na Br
K F
Li Cl
a) According to their decreasing atomic radii.
b) According to their increasing electronegativity.
c) According to their decreasing ionization potential.
8) Match the Columns:
COLUMN A COLUMN B
The factor which affects the
a) atomic size- down a group i) No. of shells, Nuclear charge
b) Ionization potential-down a group ii) Nuclear charge, Atomic radii
c) electron affinity-down a group iii) number of shells, Nuclear charge
d) metallic character-down a group iv) ionization potential, electron affinity
9) Select the correct reason for the each of the statements given below from the choice of reasons A and B.
i) Characteristics properties occur at definite integrals in the Modern Table
A: The definite intervals are after difference of either 1 or 8 or 16 or 32 in atomic numbers.
B: The definite intervals are after differences of either 2 or 18 or 18 or 32 in atomic number.
ii) Fluorine in group VIIA has a smaller atomic size than neon is group 0.
A: Outer shell in neon is completely filled, resulting in a form of repulsion .
B: Nuclear charge in fluorine atom is more than in the neon atom.
iii) First ionization potential of an atom is less than the second ionization potential.
A: Energy required to remove first electron is more than that required to remove second electron.
B: Energy required to remove first electron is less than that required to remove 2nd electron .
iv) Electron affinity of group 0 elements is zero.
A: Elements with stable electronic configuration find it difficult to accept electrons.
B: Elements with stable electronic configuration find it difficult to lose electrons.
v) Elements with high electronegativity are usually non-metallic.
A: non-metallic elements tend to gain electrons when supplied with energy.
B: non-metallic elements tend to lose electrons when supplied with energy.
vi) Down a group, metallic character increases since ionization potential decreases.
A: Nuclear attraction for valence electrons decreases and electrons are loosely held.
B: Nuclear attraction for valence electrons increases & electrons are strongly held.
10)
P\G G1 2 3 4 5 6 7 0
P-2 Li Be B C N O F Ne
2,1 2,2 2,3 2,4 2,5 2,6 2,7 2,8
P-3 Na Mg Al Si P S Cl Ar
2.8,1 2,8,2 2,8,32,8,4 2,8,5 2,8,6 2,8,72,8,8
Complete the tables given below by choosing the correct words from the list :
• decreases •increases •remains the same
a) Across a period in a periodic table
i) ionization potential______
ii) Electron affinity______
iii) electronegativity_______
iv) non-metallic character______
v) Density and melting point______
vi) Acidic nature of oxy-acids_____
b) Down a group in a periodic table
i) Ionization potential ______
ii) Electron affinity_______
iii) Electronegativity ______
iv) non metallic character______
v) Density and melting point _______
vi) Acidic nature of hydrides_____
Reasons for increase or decrease in periodic properties :
c) Across a period in a periodic table
i) Atomic size___ because nuclear charge___number of shells ____.
ii) Ionization potential ______because nuclear charge ____, atomic radii _____.
iii) Non-metallic characters____because ionization potential___ atomic radii ____.
iv) Electron affinity____because, nuclear charge_____, atomic radii_____.
v) Electronegativity_____ because, atomic radii _____, nuclear charge_____
vi) Metallic character_____ because, ionization potential ______, atomic radii ____.
d) Down a group in a periodic table
i) Atomic size_____ because number of shells _____nuclear charge ______.
ii) Ionization potential ____because atomic radii _____nuclear charge____.
iii) Non-metallic character___ because ionization potential ____, atomic radii ____.
iv) Electron affinity ______because, atomic radii _____,nuclear charge_____.
v) Electronegativity____ because, nuclear charge-----, atomic radii ______.
vi) Metallic character ______ because, atomic radii ____, ionization potential _____.
1) State the salient features of the Modern Periodic Table , with special reference arrangement of the periods and groups in the periodic table p. State how separation and periodicity of elements forms a special feature of the Modern Periodic Table .
2) State what are
a) periods
b) period number
c) Group number
in the Modern Periodic Table.
3) State the elements in correct order of increasing atomic number in period 1, 2 and 3 of the Modern Periodic Table .
4) State the property of trends of elements
a) from left to right in a period.
b) on moving down a sub group
5) State the position of the following elements in the Modern Periodic Table .
a) normal or representative elements.
b) bridge elements.
c) transition and inner transition elements.
d) alkali metals.
e) halogens
f) noble or inert gases.
6) compare the group elements with 7 a group elements still what is the means by the terms periodic properties explain the terms properties explain with reason
TEST PAPER - 1
SECTION A
(Attempt all questions from this section)
Question 1:
Choose the correct answer to the questions from the given options: (15)
(Do not copy the question, write the correct answers only)
i) An aqueous solution of copper sulphate turns colourless on electrolysis.
which of the following could be alectrodes ?
P. anode: copper; cathode: copper
Q. anode: platinum; cathode: copper
R. anode: copper; cathode : platinum
a) only P
b) only Q
c) only R
d) both Q and R
ii) A compound P is heated in a test tube with the Sodium hydroxide solution. A red litmus paper held at the mouth of the test tube turns blue .
Which of the following could be compound P be ?
a) zinc sulphate
b) copper sulphate
c) ferrous sulphate
d) Ammonium sulphate
iii) The atomic mass of a sulphur(S), Oxygen(O), and helium(He) are approximately 32, 16 and 4 respectively.
Which of the following statements regarding the numbers of elements in 32 g of sulphur, 16 g of oxygen, and 4g of helium is correct?
P. 16g of oxygen contains four times the number of atoms as 4g of helium.
Q. 16g of oxygen contains half the number of atoms as 32g of sulphur.
a) Only P b) only Q c) both P and Q d) neither P nor Q
iv) Ammonia gas is passed through a quicklime and then collected in a jar. Red and blue litmus paper are placed in the jar. W, X, Y and Z are the four observations .
Which of the above observation correctly shows the reaction of the litmus paper to ammonia ?
Red litmus paper Blue litmus paper
W turns blue remains blue
X remains red remains blue
Y remains red turns red
Z turns blue turns red
a) W b) X c) Y d) Z
v) Glucose reacts with concentrated sulphuric acid to give a very pure form of carbon called sugar charcoal.
The reaction taking place is:
a) oxidation b) combusion c) dehydration d) combination
vi) In which of the following electrolytic cells (P,Q,R or S) will silver plating be done on the spoon ?
a) P b) Q c) R d) S
vii) The basicity of acetic acid is
a) 1 b) 2 c) 3 d) 4
viii) A --> A⁺³ ; B ---> B⁻¹
Number of electrons present in the outermost shell of atoms A and B respectively are:
a) 5,1 b) 3,1 c) 3,7 d) 5,7
ix) A_____solution is observed after placing Magnesium metal in a solution of Copper sulphate for half an hour .
a) blue b) colourless c) reddish brown d) dirty green
x) An element with atomic number____ will form an acidic oxide.
a) 3 b) 17 c) 11 d) 13
xi) Which of the following is NOT true with respect to nitric acid ?
a) It is strong reducing agent
b) It is a strong oxidizing agent
c) it is unstable to heat
d) It liberates Sulphur dioxide gas when treated with potassium sulphite
xii) ____ is the functional group in methanol.
a) > C= O b) --OH c) --CHO d) --COOH
xiii) The process of electrolysis is an example of:
a) oxidation reaction
b) reduction reaction
c) redox reaction
d) displacement reaction
xiv) The catalyst used in the Oswald's process is ____.
a) finely divided iron b) graphite
c) Vanadium pentoxide d) platinum
xv) An element belongs to third Period and sixteenth group. It will have____ electrons in its valence shell .
a) 2 b) 5 c) 6 d) 3
Question -2
i) The setup shown below is that of the fountain experiment with hydrogen chloride gas in the flask. (5)
The fountain starts when a few drops of water from the dropper are introduced into the flask . Instead of the drops of water, Pooja started the fountain by introducing a few drops of Sodium hydroxide into the flask.
a) Explain why the litmus solution gets sucked up whrSodium hydroxide is used.
b) What will be the colour of the fountain when in Sodium hydroxide is used ? justify your answer.
c) if instead of HCL gas, ammonia gas is filled in the flask and water is introduced from the dropper, will there be a different observation ? justify your answer.
ii) Match the following columns A with Column B. (5)
Column A
a) aluminium
b) sulphuric acid
c) calcination
d) calcium chloride
e) carbon tetrachloride
Column B
1. covalent compound
2. carbon ore
3. Hall Heroult's process
4. Contact Process.
5. Electrovalent compound
iii) Complete the following by choosing the correct answer from the bracket: (5)
a) if an element has one electron in the outermost shell then it is likely to have the ______(smallest/largest) atomic size among all the elements in the same period.
b) ____ (sulphuric acid/hydrochloric acid) does not form an acid salt.
c) A _____(reddish brown/dirty green) colored precipitate is formed when ammonium hydroxide is added to a solution of ferric chloride.
d) Alkenes undergo____(addition/substitution) reactions .
e) An _____(alkaline/acidic) solution will turn methyl orange solution pink.
iv) Identify the following: (5)
a) A bond formed between two atoms by sharing of a pair of electrons, with both electrons being provided by the same atoms.
b) A salt formed by the complete neutralization of an acid by a base.
c) A reaction in which the hydrogen of an alkane is replaced by a halogen.
d) The energy required to remove an electron from a neutral gaseous atom.
e) A homologous mixture of two or more metals or a metal and non-metal in a definite proportion in their molten state.
v) a) Draw the structural diagram for the following compounds: (5)
1. 1- propanal
2. 1,2 dichloro ethane
3. But-2-ene.
b) Give the IUPAC name of the following organic compounds:
1. H H OH
| | |
H---C--C----C---H
| | |
H H H
2. H H H H H
| | | | |
H--C----C----C----C----C----H
| | | |
H H H H
SECTION - B
(Attempt any four questions)
Question 3:
i) Identify the reactant and write the balanced equation for the following:
Nitric acid reacts with compound Q to give a salt Ca(NO₃)₂, water and carbon dioxide. (2)
ii) What property of sulphuric acid is exhibited in each of the following cases ? (2)
a) In the preparation of HCL gas when it react with Sodium chloride.
b) When concentric sulphuric acid reacts with Copper to produce Sulphur dioxide gas.
iii) The electron affinity of an element X is greater than that of element Y. (3)
a) How is the oxidizing power of X likely to compare with that of Y ?
b) How is the electronegativity of X likely to compare with that of Y ?
c) State whether X is likely to be placed to the left or to the right of Y in the periodic table.
iv) a) State whether the following statements are TRUE or FALSE. justify your answer. (3)
1. In an electrovalent compound, the cation attains the electronic configuration of the noble gas that comes after it in the periodic table.
2. In the formation of a compound PQ₂, atom P gives one electron to each atom of Q. The compound PQ₂ is a good conductor of electricity.
b) Calculate the number of moles in 22 grams of carbon dioxide.
Question 4
i) The following questions related to extraction of Aluminium by electrolysis. (2)
a) Name the other Almunium containing compound added to alumina.
b) Give a balanced equation for the reaction that takes place at the cathode
ii) A gas cylinder of capacity 40 dm³ is filled with gas X the mass of which is 20g. When the same cylinder is filled with hydrogen gas at the same temperature and pressure the mass of hydrogen is 2g. Find the relative molecular mass of the gas.
iii) Give balanced equations for each of the following:
a) action of warm water on aluminium nitride.
b) oxidation of carbon with concentrated nitric acid.
c) dehydration of ethanol by concentric sulphuric acid at a room temperature of 170°C.
iv) with respect to Haber's process answer the following:
a) temperature of the reaction
b) catalyst used
c) balanced the equation for the reaction occuring .
Question 5
i) a) Ranjana wants to prove that ammonia is a reducing agent. To demonstrate this , she passes Ammonia gas over heated copper oxide. What will she observe ? (2)
b) Write a balanced chemical equation for the above reaction.
ii) Name the alloy which is made up of: (2)
a) copper, zinc and tin
b) lead and tin
iii) Seema takes a blue crystalline salt P in a test tube. On heating it produces a white anhydrous powder. P is dissolved in water. Zinc is added to one part of the solution and to another part of the solution Barium Chloride is added . (3)
a) Name the compound P.
b) Mention one observation of the zinc is added to the solution of P.
c) State the colour of the percipitated formed when the blue chloride is added to the solution of P.
iv) Give reasons : (3)
a) Ethane undergoes addition reaction.
b) hydrocarbon can be used as a fuels .
c) hydrogen chloride gas cannot be collected over Water.
Question 6
i) Name the following: (2)
a) the ore of zinc containing its sulphide.
b) The most commonly used oxides ore of aluminium.
ii) State one observation in the following cases. (2)
a) sodium chloride solution is added to the solution of lead nitrate .
b) Barium Chloride solution is added to a solution of zinc sulphate.
iii) copper sulphate solution is electrolysed using copper electrodes. (3)
a) which electrodes (cathode or anode) is the oxidising electrode? Why?
b) Write the equation for the reaction occuring at the above electrode .
iv) X[2, 8, 7] and Y[2, 8, 2] are two elements. Using this information complete the following: (3)
a) ____ is the metallic element.
b) metal atoms tend to have a maximum of ____electrons in the outermost shell.
c) ____ is the reducing agent.
Question 7
i) The empirical formula of an organic compound is C₃H₄N. Its molecular weight is 108.
Find the amount of carbon in one mole of the compound. Show all the steps involved.
( atomic weight C=12, H= 1, N=4). (3)
ii) a) Mahesh prepared a basic solution X. that has a pH 7. (3)
How will the pH of the solution C change on addition of the following?
1. hydrochloric acid 2. a solution of a base.
b) The atomic number of an element is 15. To which group will this element belong to ?
iii) 8.2 grams of calcium nitrate is composed by heating according to the equation
2Ca(NO₃)₂----> 2CaO+ 4NO₂ + O₂. (3)
Calculate the following:
a)!volume of nitrogen dioxide obtained at STP.
b) Mass of CaO formed
(Atomic weight: Ca=40, N=14, O= 16)
Question 8
i) State giving reason if : (2)
a) zinc and Aluminium can be distinguish by heating the metal powder with concentrated sodium hydroxide solution.
b) calcium nitrate and lead nitrate can be distinguished by adding Ammonium hydroxide solution to the salt solution.
ii) draw an electron dot diagram hydronium ion. (2)
iii) give balanced equation for the following: (3)
a) laboratory preparation of ethyne from calcium carbide.
b) conversion of acetic Acid to ethyle acetaye.
c) laboratory preparation of nitric acid.
iv) identify the following substances : (3)
a) An Alkaline gas which produces dense white fumes when reacted with HCl gas.
b) The anion present in the salt, which produces a gas with the smell of rotten eggs when reacted with dilute HCl.
c) the particle present in strong electrolytes.
1) What is the mass, charge and nature of charge on an electron ? 9.1x31⁻³¹kg, 1.59x 10⁻¹⁹C, negative,
4) Name two characteristics of substances which depend upon the number of free electrons contained in a substance.
7) Express 1 electron volt in terms of joule and erg. 1eV= 1.59 x 10⁻¹⁹J, 1eV= 1.59x 10⁻¹³ erg
10) State the factors which govern rate of emission of electrons due to heating.
14) Draw a diagram of cathode ray tube and label its different parts.
ii) Y-Y plates in a cathode ray tube.
19) Describe three important uses of cathode ray tube.
24) What is the meant by the nucleus of an atom.
26) Which particles are contained inside the nucleus of an atom and what are their masses and charges ?
27) What are isotopes ? illustrate with an example.
28) Name the different types of forces between nucleons.
31) Draw a graph showing variation of average binding energy per nucleon of a nucleus with the atomic number.
32) Give two important conclusiond drawn from the binding energy curve.
36) Following equations relate to the phenomenon of radioactivity. Determine the missing part of the equation.
37) Electric field is applied between two plates P and Q. A radio-active radiation passes through it as an shown. Identify the ray .
38) An α-particle passes through a uniform electric field as shown in the figure. Trace the path of the particle. deflected towards negative plate
38) Radioactive radiations emitted from a radio-active source pass through a uniform electric field as shown in diagram. Draw the course of radiations.
39) State two units for measuring radioactivity of a radioactive sample. How are these two units related with each other ?
41) What are radioactive tracers. Give two examples .
42) Give two examples of the use of the radio-isotopes in medicine.
a) An electron has a negative charge of___coulomb.
b) Proton is a ____'charged particle.
c) Neutron is an _____charged particle.
d) Atomic number of an atom is equal to the number of____ contained inside the nucleus.
e) An increase in the number of neutrons inside a nucleas does not affect its ______number.
f) Electron volt(eV) is the unit of_____.
g) Thermion is a ____charged particles .
h) Chlorine 35 chlorine 37 are the____of chlorine.
i) Isotopes have same ____number.
j) _____ force is the strongest force between two nucleons.
k) _____force between two nucleons is maas independent.
l) _____ force between two nucleons is spin dependent.
m) ____ rays are the heaviest of all the radioactive rays.
n) ____' rays are most penetating of all the radioactive rays.
a) Atomic number is equal to the number of protons in an atom.
b) Atomic number is equal to the number of electrons in an atom.
c) Thermions are positively charged particles.
d) α-rays pass undeflected through an electric field.
e) β-rays are effected by an electric field.
f) Emission of α-rays results in decrease of atomic weight of atom by 4.
g) Due to emission of γ-rays neither atomic weight nor atomic number of the atom is affected.
h) Unit of Radioactivity is roentgen.
i) Radioactivity was discovered by Marie Curie.
j) Rutherford is the unit of radioactivity.
k) Curie is the unit of radioactivity.
State the number of neutrons in each of the atoms A to E. Also state which of the atoms A to E is a metal.
