Modern Periodic Table
1) 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 elements 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 the period-2 and period-3.
f) The non metallic elements in the period-2 and period-3.
g) The elements in periods-2 and periods-3 having stable electronic configuration.
h) The element in period-3 having 5 valence electronics.
i) The elements in period -2 having electronic configuration 2,4.
j) The period/s having 8 element.
k) The elements having one shell and one valence electron.
l) The period containing
i) rate earth elements
ii) radioreactive elements.
m) The bridge elements in period-2 which has a diagonal relationship with aluminium in period-3.
n) A metalloid in period-3.
o) The valency of the elements in period-2
i) group V
ii) group 0.
p) The type of bonding of the chloride of the element in period-3, group IIA .
q) The type of bonding of the oxide of the element in period-3, group IIIA and VIA.
r) The state of the chloride of the element in period-3 group VIA.
s) The character of the oxide of the element in period-3 group IIA and IIIA.
t) The character of the hydroxide of the element in period-3 group IIA.
u) The element in period-3 whose hydride is a strong acid.
v) Two property trends of elements which increase from left to right in a period.
2) Name or state the following pertaining to elements in groups of the periodic table.
a) The number of valence 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 non metals only.
f) The group number to which elements with 7 valence electrons belong.
g) The type of elements present in group IB to VIIB and VIII.
h) The group to which innert, 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.
j) The two property trends which increase down a sub group.
k) A non metal in group VIIA which is a liquid at room temperature.
l) Two non metals which react with a group VIIA element forming liquid Chlorides.
m) An elements from group IA which reacts with an element of group VIIA forming a soluble electrovalent compound.
n) An element from group IA which dissolves in water to give caustic potash .
o) A strong reducing agent from the elements -- sodium of group IA and fluorine of group VIIA.
p) The element in group VIIA with the highest electronegativity.
ELECTROLYSIS
1) Name the following:
a) An organic compound which is a non-electrolyte.
b) An inorganic liquid which in the pure state is almost a non-conductor of electricity.
c) An acidic gas whose aqueous solution is a week electrolyte.
d) A salt of an active metal which conducts electricity in its molten state.
e) A monobasic acid other than dilute hydrochloric and nitric acid which is a weak electrolyte.
f) A gas whose aqueous alkaline solution is a weak electrolyte.
g) A covalent acidic gas which ionises in aqueous solution.
h) A metal which forms a strong electrolyte on reaction with water.
i) A neutral liquid which contains almost only molecules.
j) A substance in the molten state which contains almost only ions.
k) An acidic solution which contains ions and molecules.
l) A basic gas which contains molecules but its aqueous solution contains ions.
m) A diabasic non-volatile acid which is a strong electrolyte.
2) The diagram represents the arrangement for electrorefining of copper.
Name the following:
a) The electrolyte used in the above electrorefining .
b) The product at the anode.
c) The product at the cathode.
d) the monovalent metal recovered from the anode mud.
e) A divalent metal other than copper refined by electrolysis.
AMMONIA
1) Name the following:
a) An acidic solid drying agent not used for drying ammonia gas.
b) A metallic nitride of a trivalent metal which on reaction with warm water evolves ammonia gas.
c) A drying agent which forms an addition compound with ammonia.
d) The catalyst other than iron which may be used in Haber's process.
e) The promoter other than molybdenum used for assisting the catalyst in Haber's process.
f) Two acidic gases which tend to poison the catalyst, used in Haber's process.
g) A solvent for Ammonia gas.
h) A salt which reacts with an alkali liberating ammonia on heating.
2) Name the following:
a) The liquid component of liquor Ammonia fortis.
b) The ion responsible for the alkaline nature of Ammonium hydroxide.
c) An amphoteric oxide which cannot be reduced by Ammonia.
d) A metallic chloride insoluble in sodium hydroxide but soluble in Ammonium hydroxide.
e) A metallic hydroxide soluble in excess of sodium hydroxide but insoluble in excess of ammonia hydroxide.
f) The gases product of catalytic oxidation of ammonia.
g) A yellow liquid obtained when excess chlorine is bubbled through a solution of ammonia.
h) The neutral liquid obtained when ammonia is passed over heated lead monoxide.
i) A nitrogenous fertilizer obtained when Ammonia reacts with an acidic gas at elevated temperature.
j) The neutral gas obtained when excess of ammonia reacts with chlorine.
NITRIC ACoxide
1) Name the following:
a) A metal other than iron rendered passive with concentrated nitric acid.
b) An organic liquid which bursts into flames on addition of concentrated nitric acid.
c) A metal other than magnesium which reacts with very dilute nitric acid to liberate hydrogen.
d) An acid which dissolves zinc but not platinum.
e) The acid formed when dilute nitric acid reacts with the skin.
f) The acidic gas responsible for the yellowish colour of nitric acid.
g) The oxidized product formed when concentrated nitric acid reacts with sulphur.
h) The nascent gas formed on decomposition of nitric acid responsible for the oxidising nature of nitric acid.
i) The nascent gas formed when concentrated hydrochloric acid reacts with concentrated nitric acid when added in the appropriate ratio.
j) The gas obtained when zinc reacts with concentrated nitric acid.
k) The brown compound formed when iron (II) sulphate solution absorbs matric oxide.
2) Name the following chemical compounds obtained from nitric acid.
a) A nitrogenous fertilizer.
b) An organic explosive.
c) A solvent for platinum.
d) A non volatile mineral acid.
e) A coloured nitrate.
3) Name the following nitrates .
a) A white metallic nitrate which leaves a shiny mirror on the cold parts of the test tube on heating.
b) A nitrate which evolves two neutral products on heating, leaving no residue .
c) A nitrate of a heavy metal which evolves two gases on heating one of which is acidic.
d) A nitrate of an alkali metal which evolves only one gas on heating .
e) A nitrate of a divalent metal which leaves a black residue on heating.
f) A nitrate of a monovalent metal which evolves an acidic gas of heating.
g) A nitrate which acts as a strong oxidizing agent.
h) A nitrate which forms an important constituent of gun powder.
i) A nitrate deliquescent in nature.
j) A nitrate which decrepitates on heating.
SULPHURIC ACID
1) Name the following:
a) An acid hygroscopic in nature.
b) An acidic gas which is not dried by passing through concentrated sulphuric acid.
c) A metallic sulphide which reacts with dilute sulphuric acid evolving a foul smelling acidic gas.
d) The black residue obtained when hydrogen sulphide gas is passed through a solution of lead acetate.
e) The gas evolved when zinc reacts with concentrated sulphuric acid.
f) The gas evolved when zinc reacts with dilute sulphuric acid.
g) The volatile acid obtained when sodium nitrate reacts with concentrated sulphuric acid.
h) The residue obtained when the rock salt reacts with concentrated sulphuric acid low temperatures .
i) The ions present in an aqueous solution of sulphuric acid.
j) The neutral gas obtained when concentrated sulphuric acid reacts oxalic acid.
2) Name the following:
a) The white precipitate obtained when dilute sulphuric acid reacts with barium Chloride.
b) The gas evolved when copper is heated with concentrated sulphuric acid.
c) The acidic vapours evolved when concentrated sulphuric acid is heated with sodium chloride.
d) A fertilizer manufactured using sulphuric acid during the process of manufacture.
e) An explosive prepared using concentrated sulphuric acid.
f) An acidic other than Hydrochloric and nitric acid prepared in the laboratory using sulphuric acid.
g) The anhydride of sulphuric acid used during the manufacture of explosives.
3) Name the products, state it's colour and give a balanced equation for the reaction taking place when H₂S gas is bubbled through each of the following solutions.
a) Lead acetate.
b) Copper sulphate.
c) Silver nitrate.
d) Zinc nitrate.
METALLURGY
1) Name a 'metal' which has the following properties.
a) Is a liquid at ordinary temperatures .
b) Has a low boiling point but does not float on water.
c) Is a light, soft metal which can be cut with a knife.
d) Does not give a note on striking.
e) Is found in the native state in nature.
f) Is Brittle at ordinary tempratures.
g) Is divalent and forms a white amphoteric oxide.
h) Has variable valency and forms a black basic oxide.
i) Is neither malleable nore ductile at particular temperatures .
j) Forms an alloy which is a liquid at ordinary temperatures .
k) Has a low density but does not float on water.
l) Is a soft metal whose oxide is amphoteric.
2) Name a 'nonmetal' which has the following properties.
a) Volatizes at low temperatures and burns in air with a pale blue flame.
b) Has a very high density.
c) Conducts electricity and is lustrous.
d) Does not conduct electricity but it is lustrous .
e) Has luster but does not sublime on heating.
f) Has high melting point.
g) Is the present in the alloy stainless steel.
h) Is liquid at ordinary tempratures.
i) Forms a gaseous poisonous neutral oxide and a gaseous acidic oxide which turns line water milky.
j) Forms a gaseous neutral oxide and a gaseous coloured acidic oxide.
k) Forms a neutral oxide, liquid at ordinary temperature.
l) Form a volatile chloride, liquid at ordinary temperatures.
3) Name a metal from the activity series which itself or its compounds show the following characteristic properties.
K a) oxide and nitric reduced to metal by heat alone.
Na b) Forms an oxide on exposure to air.
Mg c) Does not react with cold, boiling water or steam.
Al d) Displaces hydrogen from dilute sulphuric acid and forms a coloured salt,
Zn
Fe e) Reacts with concentrated Sulphuric acid but not with concentrated hydrochloric acid.
Sn
Pb f) oxide, hydroxide and carbon do not decompose on heat
[H]
Cu. g) Hydroxide on thermal decomposition gives a residual coloured basic oxide.
Hg h) Has no action on dil HCl or dil sulphuric acid.
Ag i) nitrate gives only one gas on Thermal decomposition.
Pt
Au j) nitrate leaves a coloured amphoteric oxide of heating.
4) Name the metal which finds application in the following:
a) i) As a cathode plate in dry cells
ii) as a negative plate in storage batteries.
b) i) as an anti corrosive paint in the powder form.
ii) for making compounds used as a pigment in paints.
c) i) in metallurgy as a reducing agent.
ii) in metallurgy to free metals from dissolved oxides in sulphides.
d) i) in the amalgamated form as a reducing agent in the neutral medium.
ii) In the amalgamated form in voltaic cells.
e) i) for covering underground telephone cables and wire systems .
ii) for making electrical cables and transmission wires.
f) i) In the manufacturer of the ammunition.
ii) in the manufacture of the calorimeters and condenser tubes.
5) Name the alloy of the respective metals which finds application in the following:
a) Lead used in making blocks for printing.
b) copper used in hardware and in scientific instruments.
c) Aluminium used in the manufacture of pressure cookers.
d) copper used in gun barrel.
e) Aluminium used in making beams of a balance.
f) copper used in plating and resistance wires.
g) Lead used in soldering and fuse.
h) Steel used in cutlery.
i) copper used in silverwere and jewellery.
ACID BASE AND SALTS
1) Name the following acids:
a) A mineral oxidizing acid.
b) A strong monobasic acid
c) A corrosive mineral acid.
d) A non-corrosive weak acid.
e) An organic acid.
f) An inorganic acid derived from rock salt.
g) A weak monobasic acid.
h) A strong dibasic acid.
i) An unstable oxy-acid.
j) An acid solid in nature.
2) Name or state the ions formed in each of the following dissociations:
a) A manual monobasic acid formed as the displaced volatile acid on reaction of concentric sulphuric acid with Sodium Chloride.
b) a mineral dibasic non-volatile acid which forms two types of salts with NAOH one of which is sodium bisulphate.
c) A tribasic acid which forms two acid salts and one normal salt with a base.
d) A mineral monobasic acid formed by action of a concentric non-volatile acid with the normal salt-nitre.
e) A weak monobasic acid containing four hydrogen atoms.
f) An unstable acid formed by reaction of a metallic bicarbonate with dilute hydrochloric acid.
3) Name the acid used in:
a) cooking.
b) removing ink stains.
c) food preservation
d) eye wash.
e) Flavouring drinks.
f) baking powder
g) Health salts.
h) cleaning tiles.
i) pickling of metals.
j) for testing gold ornaments.
4) Name and acid prepared by the following reactions and give a balanced equation for each method of preparation.
a) An acidic gas and a neutral liquid.
b) A volatile acid and a nonmetal.
c) A non-volatile acid and a salt.
d) A neutral gas, an acidic gas and water.
e) An acidic solid and a neutral liquid.
5) Name the following :
a) A neutral gas liberated when an active metal reacts with dilute acid.
b) Am indicator which is Colourless and remains colourless on addition of a few drop of acid.
c) A dibasic acid other than sulphuric acid.
d) A Ammonia acid other than halogen acid or nitric acid.
e) the positive ion formed when nitric acid is dissolved in water.
f) An oxy-acid formed when chlorine is dissolved in water.
g) An inorganic acid derived from nitre.
h) An acid which is an aqueous solution of a weak acidic gas.
i) An acidic gas liberated when a metallic sulphide reacts with the dilute acid.
j) An example of an acid having basicity of three.
6) Name the following bases:
a) A strong base of a monovalent metal.
b) a week base of a divalent metal.
c) A tribasic base of a trivalent metal other than almunium.
d) A metallic oxide which is an alkali.
e) a metallic oxide which is a base but not an alkali.
f) a base which is amphoteric in nature.
g) A base that doesn't contain a metal.
h) A hygroscopic base.
i) An alkali deliquescent in nature.
j) An example of a base having acidity of two.
7) Name the base/alkali used:
a) as an antacid to neutralize the enhanced acidity.
b) in the manufacture of soaps .
c) in the softening of water.
d) for cleaning glass surfaces and porcelain.
e) to neutralize the acidity of the soil.
f) as a foaming agent in fire extinguishers.
g) for removing grease stains from warm clothes.
h) for whitewashing of buildings.
i) in the manufacture of bleaching powder.
j) in the purification of bauxite.
8) Name or state the Ion formed in each of the following dissociations :
a) A minoacidic strong alkali used in the manufacture of soaps.
b) A diabasic base containing ions which form a blue aqueous solution.
c) A weak alkali formed by action of a strong monobasic base on an ammonium salt.
d) A diabasic base used in the manufacture of a chlorine compound which is a mixed salt.
9) Name the following:
a) a base which reacts with an acid to give a salt which decrepitates on heating.
b) Two bases which react together to give a normal salt.
c) An alkali which liberates a basic gas on reacting with a normal salt.
d) A diabasic base which reacts with an acid forming a salt insoluble in water.
e) An alkali which reacts with an acidic gas forming a salt soluble in water.
f) a colored nitrate which on thermal decomposition forms a base as the residual product.
g) A colorless indicator which produces a colour on addition of a drop of an alkali.
h) An alkali which reacts with an acidic gas forming a salt insoluble in water.
i) An alkali which reacts with a metal liberating hydrogen gas.
j) An indicator which gives a yellow colour both with a drop of alkali and with a drop of water.
10) Name the following:
a) An acid salt of a dibasic weak acid.
b) A normal salt of a monobasic mineral acid.
c) A normal salt obtained from α basic salt.
d) A hexahrated double salt.
e) A deliquescent salt obtained by reaction between a metal and a coloured acidic gas.
f) A Decahydrate efflorescent salt.
g) the salt formed when zinc sulphate reacts with sodium hydroxide in excess .
h) the insoluble dirty green participitate formed when iron (II) sulphate reacts with ammonium Hydroxide.
i) A hydroxide formed from a salt and an alkali, insoluble in excess of ammonium Hydroxide but soluble in excess of NaOH.
j) A pale blue precipitate formed when copper sulphate reacts with either NaOH or NH₄OH.
k) A salt which forms a gelatinous white precipitate in excess of NaOH or NH₄OH on reaction with either of them.
ORGANIC CHEMISTRY
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
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.
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