TRANSPORT OF FOOD MINERALS IN PLANTS
A) Name the following :
a) The membrane which allows the solvent to pass through it but not the solute.
b) The process by which solid, liquid and gases move from a place of higher concentration to a place of lower concentration.
c) The upward movement of water and minerals from roots towards the top of the plant.
d) The pull which helps in have conduction of water in case of tall trees.
e) The tissue which helps in conduction of water minerals in the plant.
f) An apparatus used to measure the rate of transpiration.
g) An antitranspirant.
h) A plant having hydathodes.
i) The tissue which helps in conduction of food in plants.
j) Name the disease caused due to deficiency of nitrogen nutrients in plants.
B) Choose the odd one from each of the following giving reason:
a) Osmosis, Diffusion, Active transport, Transpiration pull.
b) Meristematic zone, Shoot cap, Elongation zone, Maturation zone.
c) Conduction, Rranslocation, Transpiration , Ascent of sap.
d) Root pressure, Transpiration pull, Turgor pressure, Capillary force.
e) Egg-membrane, Parchment paper, Goat's bladder, Litmus Paper.
f) Cooling effect, Ascent of sap, Conduction of minerals, Evaporation.
g) Stomata, Xylem , Lenticel, Hydathodes.
h) Sunlight, Temperature, Humidity , Hydathodes.
i) Tracheids, Teaches, Xylem parenchyma, Sieve plates.
j) Nitrogen , Phosphorus, Potassium , Cooper
C) Fill in the blanks:
a) ____ tissue is involved in the transportation of water in plants.
b) The young growing tip of the root is protected by ____.
c) ____ occurs through a semi permeable membrane.
d) ____ is the major component of protoplasm present in a living cell.
e)A plant cell becomes ____ on absorbing water from the soil.
f) Root hairs absorb____ from the soil by active transport.
g) Upward movement of water takes place through _____.
h) ______system of plants absorb water and minerals from the soil.
i) _____ is the inflow of water molecules form an external solution into a cell.
j) A plasmolysed protoplasm swells photo when it is placed in ____ water.
k) Cactus does not have _____ transpiration.
l) Sunken stomata ____ the rate of transpiration.
D) Write true or false and correct the incorrect statements:
a) Osmosis plays an important role in the absorption of water by plants.
b) A semipermeable membrane allows the passage to only solvent molecules through it.
c) Root hairs do not help in absorption of water and minerals.
d) Water is responsible for developing turgor pressure in the cell.
e) Movement of molecules from the region of lower to that of higher concentration is called diffusion.
E) Choose the correct answer:
1) Ascent of sap occurs due to:
a) root pressure b) transpiration pull c) capillary force d) all of these
2) Movement of molecules from a region of higher concentration to the lower concentration through a membrane.
a) diffusion b) active c) osmosis d) all of these
3) The pressure developed in the root due to continuous inflow water in it
a) Turgor pressure b) root pressure c) transpiration pull d) none
4) The upward movement of cell sap in the plants is called :
a) conduction b) absorption c) transpiration d) none
5) The tissue which helps in conduction of water and minerals in the plant:
a) Phloem b) Xylem c) vein d) none
ENDOCRINE SYSTEM
A) Name the following:
a) Ductless glands which release their secretion into bloodstream .
b) which gland is called master gland ?
c) which gland is called emergency gland .
d) name the disease caused due to the dietary deficiency of iodine
e) Name a gland having dual function
B) Fill in the blanks :
a) deficiency of___ cause diabetes.
b) ____ is called stress hormone.
c) Testes secrete____ in males.
d) _____ is called master gland.
e) _____ regulate the calcium and phosphorus in the ratio body.
C) Write true or false statement and correct the incorrect statements
a) thyroxine hormone causes critination in early growing age.
b) pancreas releases emergency hormone, i.e, Adeline hormone
c) parathyroid glands regulate calcium and phosphorus balance in the body.
d) glucagon lowers blood sugar level.
D) Give one word for the following :
a) Flight or fight hormone.
b) chemical messenger in our body.
c) glands with duct
d) glands without duct.
e) it lowers the level of glucose in the blood
f) it raises the level of glucose in the blood.
CURRENT ELECTRICITY
1) A conductor of resistance 4 Ω can pass a current up 2.5 A through it. Calculate the potential difference required across the conductor. 10V
2) Calculate the amount of work done in moving a charge of 5 C through a potential difference of 25V. What will be the potential difference if this amount of work is done in moving a charge of 10C ? 12.5V
3) A metallic wire of length 1m is stretched to double its length in such a way that there is no change in density of the wire . Calculate the ratio of the final resistance. 1:4
4) A wire of length 15m and uniform cross section of 6x 10⁻⁷m² has a resistance of 5Ω. Calculate the resistivity of the material of the wire. 2 x 10⁻⁷Ωm
5) When a potential difference of 4V is applied across the ends of a wire of 10m length, a current of 2A flows through it. Calculate
a) the resistance per unit length of the wire. 0.2Ω m⁻¹
b) the resistance of 4m length of this wire. 0.8Ω
6) A battery supplies a current of 0.8 A through a 2Ω resistor and a current of 0.4A through a 5Ω resistor. Calculate the internal resistance of the battery. 1Ω
7) What will be the equivalent resistance of three resistors of 4Ω, 8Ω and 16 Ω if these are connected in
a) series. 28Ω
b) parallel. 2.28Ω
8) A lamp of resistance 800 Ω, a fire alarm of resistance 30 Ω and a vacuum cleaner of resistance 200Ω are connected in parallel to the mains supply of 240 V. Calculate the current through each appliance and the total current supplied by the mains. 9.5A
9) The effective resistance of two resistors is 25Ω. If the resistance of one of the resistors is 10 Ω, what is the resistance of the other resistors ? 15Ω
10) The effecttive resistance of three resistors connected to a battery is 5 Ω. If R₁ = 10Ω, R₂ = 15Ω, what will be the value of R₃ ? Draw a circuit diagram with the flow of current across each resistor. 30Ω
11) A parallel pair of resistors of values 4Ω and 12 Ω are together connected in series with another resistors of value 3 Ω and battery of emf 24 V. Draw a circuit diagram and calculate the current across each resistor . 3A, 1A
12) The figure below shows
V-I graphs of two metallic conductors for series and parallel combination. Which graph represents parallel combination ?
13) The lengths of three conducting wires of same materials are in the ratio 1:2:3. The area of cross section of each wire is same, if these wires are joined in parallel across a battery, what will be the ratio of the currents in them ? 6:3:2
14) In the given circuit diagram,
the emf of the cell is 5 V and its an internal resistance is 2.5 Ω. Calculate the current flowing in the circuit. 0.67A
15) Find the current flowing through the given circuit connected to a cell of supply 5V. 
3.75A
16) From the circuit flow diagram given below,
Calculate the current flowing through the circuit. 0.67A
17) Three resistors of 8Ω, 4 Ω and 2 Ω are connected together in such a way that the total resistance is greater than 8Ω but less than 10 Ω. Suggest a suitable arrangement of how these resistors can be possibly combined and calculate the total resistance. 9.33Ω
18) In the given diagram,
A₁, A₂ and A₃ are three ammeters of negligible resistance. The reading of ammeter A₃ is 1A. Calculate
a) the readings of ammeter A₁ and A₂. 3A
b) the total resistance of the circuit. 2Ω
19) The diagram below
shows three resistors of 5Ω, 8Ω and 10Ω connected to a battery of emf 10V. Calculate
a) the potential difference across the parallel resistors 8Ω and 10Ω. 4.7V
b) the current through 8Ω resistors. 0.59A
20) A cell of emf 2.5 V and internal resistance 1.5 Ω is connected to resistors of 5 Ω and 15Ω in series. Draw a circuit diagram and calculate
a) the current in the circuit. 0.116A
b) the potential difference across each resistor. 1.74V
c) the total potential difference across the cell. 2.32V
21) An electric motor draws a current of 5 A from a 220V line. Determine the power of the motor and the energy consumed in 2 hour. 7.92 x 10⁶J
22) A heater has a power of 1.1 kW at 220V.
a) Find the resistance of the heater. 44Ω
b) Calculate the energy in kWh consumed in a week if the heater is used daily for 4h. 30.8 kWh
23) An electric heater draws 5A of current for 10 minute when connected to 230V power supply. Find the heat energy developed. 690 kJ
24) Find the current flowing through an electric bulb rated as 100W, 220V when connected to a 110 V supply. What will be the power consumed now? 25W
25) Three bulbs, A, B and C, are connected in parallel across 110V source . The rating of bulb is 5oW, 110V, bulb B is 20W,110 V and bulb C is 100 W, 110V
a) Calculate the current flowing in each bulb. 0.45A, 0.18A, 0.9A
b) Which bulb will glow the brightest ? C
26) Two resistors with resistance R₁ = 5Ω and R₂=7Ω are connected in series across a battery of emf of 16V. Draw a circuit diagram and find
a) the electrical energy consumed by each resistor in 30 second.265.33J, 371.47 J
b) total power developed in the circuit. 21.28 W
27) In the previous example, if the resistors are connected in parallel instead of series, what would be the electrical energy consumed by each resistor. Draw a circuit diagram for the same. 1536 J, 1097.14 J
28) two bulbs are rated as 40W, 220 V and 40W, 110 V, respectively. Compare the resistance of two bulbs. 4:1
29) A geyser is rated 1.5kW, 250V. It is connected to 250V mains. Calculate
a) the current drawn by the geyser. 6A
b) electrical energy consumed in 10h in joules. 54 x 10⁶ J
c) cost of energy consumed at Rs3.50 per kWh. Rs52.50
30) Four tube lights of 40 W each, two fans of 100W each and three bulbs of 60W each operate on an average of 8h per day. If the cost of energy is Rs2.50 per kWh, calculate the monthly bill. Rs324
BOOSTER
* In every chemistry classroom and laboratory, you will see Periodic Table of the elements on the wall, because in learning chemistry and in solving chemistry problems, no other source of information is used as often. In its symbols and numbers, and most of all in its structure, the Periodic Table contains information about the chemical behaviour of the elements and about the masses, compositions and structures of their atoms.
* In the beginning of the development of chemistry only a few elements were known. But with the discovery of new elements their number went on increasing gradually and it became inconvenient to remember and study the chemistry of so many elements. This condition led to the necessity of classification of elements so as to facilitate the study of chemistry. The arrangement of the elements according to their similarities and dissimilarities resulted in the formation of Periodic Table . The periodic arrangement of known elements according to their properties in a tabular form is known as Periodic Table.
* The Modern Periodic Law states that the physical and chemical properties of elements are periodic functions of their atomic numbers.
* In the Modern Periodic Table , there are 7 Periods and 18 Groups .
* Groups I, II, III, IV, V, VI, VII, VIII and 0 (zero) represent various Groups. Groups I to VII are divided in sub-groups A and B.
* Elements of zero Group are called Nobel gases and or inert gases.
* Electron shells increase progressively by one down a Group .
* Elements in the same Group have the same number of electrons in their outermost shells. As a result, elements in the same Group have similar chemical properties.
* Elements in the same Period have the same number of electron shells. Electrons in the outermost shell increases progressively by one across a Period.
Periodic properties and their Variations in Periods and Groups
Atomic size or Atomic Radius:
Atomic radius is the distance between the centre of the nucleus of an atom and its outermost shell containing the electrons. It is measured in Angstrom, abbreviated as A°. 1 A°= 10⁻¹⁰m. The atomic size of the elements decreases in a Period from left to right. The atomic size of elements increases from top to bottom in a Group .
* Ionization Potential (I. P) or Ionization Energy (I. E):
Ionization potential is the amount of energy required to remove a loosely bound electron from the outermost shell of an isolated gaseous atom. it is measured in electron volt (eV). The energy required to remove the first electron is called first ionization potential. The energy required to remove the second electron is called the second ionization potential. Second ionisation potential is more than the first ionization potential. The ionization potential increases on moving from left to right in a Period. It decreases on moving from top to bottom in a Group .
* Electron affinity(E. A) or Electron Gain Enthalpy:
Electron affinity is the amount of energy released when an electron is added to the outermost shell of an isolated gaseous neutral atom. It is measured in electron volt (eV). Since energy liberated, we use minus (-1) . For example, the electron affinity of chlorine is -3.82 eV. The electron affinity increases in a Period on moving from left to right. It decreases in a Group when we move from top to bottom .
* Electronegativity (E. N): Electronegativity is the tendency of an atom in a molecule to attract shared pair of electronr towards itself. Electronegativity increases across a Period. It decreases from top to bottom in a Group.
* Metallic Character: It is the property of an atom to lose one or more electrons on heating. It decreases on moving left to right across a Period, and increasees from top to bottom on moving down a Group.
* Non-metallic Character: It is the property of an atom to gain one or more electrons in order to attain octate in their outermost shell, when supplied with energy. Non-metallic character increases in a Period as we move from left to right, and it decreases in a Group on moving down from top to bottom.
* Alkali Metals : Alkali metals are those elements which follow immediately after the inert gases in the Periodic Table. They consist of 6 elements, Li( lithium), Na(sodium), K(potassium), Rb(Rubidium), Cs(Cesium) and Fr(Francium).
Physical Properties:
a) Commonly found in a combined state.
b) Soft and can be cut with a knife, except Li(lithium).
c) Silvery-white and shining metals.
d) Excellent conductors of heat and electricity.
e) Emit electrons under the influence of light.
f) Low melting and boiling points.
g) Low density. ( the density increases on moving down the Group .)
Chemical properties:
a) Highly reactive.
b) React with water to form hydroxides with the liberation of hydrogen and heat.
For example, 2Na+ 2H₂O ---> 2NaOH + H₂ + Heat.
c) React with halogen to form a stable binary compound.
For example, 2Na + Cl₂ ---> 2NaCl.
d) React with hydrogen to form white crystalline compounds.
For example, 2Na + H₂ ---> 2NaH.
e) React with oxygen to form oxides.
For example, 4Na + O₂ ---> 2Na₂O.
f) React with non metals to form electrovalent compounds.
For example, Na+ Cl ---> NaCl.
g) Strong reducing agents.
Halogens:
Elements of Group VIIA are called halogens . They consist of 4 elements. F( fluorine), Cl( chlorine), Br(Bromine) , I(iodine).
Physical Properties:
a) Commonly occurs as salts.
b) Bad conductors of heat and electricity.
c) Atomic size increases on moving down the Group .
d) Electronegativity decreases on moving down the Group .
e) Electron affinity decreases on moving down the Group .
f) Melting and boiling points increases on moving down the Group .
Chemical properties:
a) Reactivity decreases on moving down the Group .
b) React with hydrogen to form covalent hydrides.
For example, H₂ + I₂ ---> 2HI
c) React with non metals to form covalent compounds.
For example, 2P+ 3Cl₂ ---> 2PCl₃
d) React with metals to form metal halides.
For example, Ca + Cl₂ ---> CaCl₂
e) Strong oxidizing agents. The oxidising property decreases down the Group.
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 noblw 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.
10) 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.
11) 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 ?
12) 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?
13) 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.?
14) Which is larger, Na⁺ or K⁺ ? Why?
15) 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 ?
16) 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 .
17) 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 ?
18) What is the cause of periodicity of elements in the Periodic Table?
19) What are the following Groups known as?
a) Group IA
b) Group VIIA
c) Group Zero
20) 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
21) 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.
22) 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
23) 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.
24)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.
25) 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⁺
26) 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?
27) 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?
28) 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?
29) 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.
30) 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 ?
31) 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?
32) 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).
33) 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 ?
34) 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 ?
35) 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 .
36) 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 ?
37) 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)
38) 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
39) 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.
40) 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.
41) 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
F) REASON BEHIND:
1) Sodium is referred to as a normal element.
2) Sodium and potassium are placed in Group I.
3) Noble gases have zero electron affinity values. Explain ?
4) Why is larger Na⁺ or K⁺ ? Why ?
5) Why is the electron affinity for F Less than that of Cl?
6) Why electron affinity of halogen is comparatively high. Give reason.
7) Ionisation potential of alkali metals is comparatively low.
8) Electronegativity of chlorine is higher than that of sulphur. Why ?
9) Sodium and potassium are called alkali metals . Why ?
10) Why is chlorine more reactive than bromin ?
11) Why Potassium is more reactive than sodium.
