IBA PUBLIC SCHOOL SUKKUR

Subject: Chemistry

Question bank Class XI

CHAPTER#O1

FUNDAMENTAL CONCEPT IN CHEMISTRY

MCQs

Q1. Choose the correct answer.

Q. 1.The soul of chemistry is its dealing with ___________

a. Internal structural changes in matter

b. Composition of matter

c. Properties of matter

d. Composition and properties of matter

Q. 2.All of the following statements are incorrect for 20 mol of hydrogen peroxide except_________

a. it has 20 mol of hydrogen atoms

b. it has 30 mol of oxygen atoms

c. it has 80 mol of atoms

d. 30 mol of hydrogen atoms

Q. 3.The formula which gives simplest ratio of each kind of atom present in the molecule of compound is

a. Molecular Formula

b. Empirical Formula

c. Structural formula

d. Atomic mass unit

Q. 4.A chemist poured lemon juice on soil, the idea that he may have in his mind is that__________

a. there may be a possibility of a chemical reaction

b. lemon juice is dangerous to health

c. lemon juice is dangerous to health

d. water should be preferred over lemon juice for drinking

Q. 5.Mole is quantity that has __________ particles of the substance.

a. 6.02 ˣ1023

b. 1 billion

c. 12.04ˣ1023

d. 1gram

Q. 6.Which of the following is not related to amu?

a. gram

b. kilogram

c. microgram

d. gram/lit

Q. 7.The number of significant figures in 0.00200 is__________

a. two

b. three

c. five

d. one

Q. 8.All of the following statements are incorrect except_________

a. precision and accuracy should go side by side in a scientific work

b. scientific work must be precise, accuracy is not essential

c. scientific work must be accurate, precision is not essential

d. +calculations must be made before any experiment

Q. 9.Empirical formula and formula unit of an ionic compound__________

a. are always similar

b. are always different

c. may be similar or different

d. ionic compounds don’t’ have any empirical formula

Q. 10.Copper (II) oxide is mixed with organic compound during combustion analysis. The purpose is _______

a. to carry out complete combustion

b. to reduce the economy of the process

c. to reduce the time for completion of the reaction

d. all of the above

Q. 11.Bismarck brown is a dye. Its molar mass is 228.3 g/mol. When the dye was analyzed by a scientist, it was found that it contains 30.68% nitrogen. How many nitrogen atoms are there in each Bismarck brown molecule?

a. 6

b. 5

c. 4

d. 3

Q.12.The mass of 2 mole of sodium hydroxide will be__________

a. 2 g

b. 20 g

c. 40 g

d. 80 g

Q. 13.“A” compound is always consists of the same elements combined in the same fixed ratio”. The statement is ___________

a. a hypothesis

b. a fact

c. a law

d. an observation

Q. 14.2 moles of Cl- ions contain_________ ions.

a. 6.02 ˣ1023

b. 1 billion

c. 12.04ˣ1023

d. 1gram

Q. 15.6600 contains __________ significant numbers.

a. 2

b. 1

c. 4

d. 3

Q. 16.3.7ˣ106 contains _______________ significant numbers.

a. 6

b. 2

c. 8

d. 10

Q. 17.10 moles of H2O contains___________

a. 100 moles of bonds

b. 100 moles of electrons

c. 30 atoms

d. 25 moles of hydrogen bonds

Q. 18.100grams of water is equal to ____________moles

a. 2.56

b. 5.56

c. 6.25

d. 27.78

Q. 19.A compound contains two elements X and Y percentage of X is 20% (At.wt = 40) and that of Y is 80% (At.wt =80). The empirical formula of the compound is _____________

a. XY2

b. X2Y

c. X3Y

d. XY

Q. 20.A piece of paper is burnt in air; the gas produced is passed through distilled water. The PH of water solution will be______________

a. 1

b. 7

c. 2.1

d. 6.8

Q. 21.58.5 are ____________ of NaCl.

a. Atomic weight

b. Molecular weight

c. Formula weight

d. All

Q. 22.Molecular weight is used for the _______________ compounds.

a. Ionic

b. Neutral

c. Electro static

d. Non ionic

Q. 23.One mole of glucose contains ______________grams.

a. 180

b. 250

c. 280

d. 200

Q. 24.A student subtracted 0.00055 from 10.2345678 and reported the result as 10.23401. But his friend told him that the result was wrong. What is the correct result?

a. 10.234017

b. 10.2340178

c. 10.234

d. 10.23

Q. 25.The following statement contained in a student’s laboratory report is a conclusion.

a. a gas is liberated

b. color of the gas is greenish yellow

c. oxide of the gas is strongly acidic

d. the gas is chlorine

Q. 26.If 10g each of uranium and hydrogen are converted into energy according to equation E = mc2

a. energy obtained from uranium will be too much greater than that of hydrogen

b. energy obtained from hydrogen will be a little bit less than that of uranium

c. energy obtained from hydrogen and uranium will always be exactly equal

d. diamond

Q. 27.A student analyzed a sample of sea water and found that it contained 2.3g of NaCl, 0.005g of MgSo4, 0.234g of CaCI2 and 60.12g of H2O. Total mass of the sample is

a. 62.659

b. 62.65

c. 62.70

d. 65.7

Q. 28.A 50.00 mL sample of a cough mixture prepared by a pharmacist was found to have a mass of 46.0g. What is the density (in g/mL) of this mixture. Stated to the correct number of significant figures?

a. 0.92

b. 0.920

c. 0.9200

d. 1.087

Q. 29.Ozone (O3) filters the cosmic rays of sunlight. How many oxygen atoms are there in 0.2 mole of ozone (O3, molar mass 48.0 g/mol)?

a. 6.02 x 1022

b. 6.02 x 1023

c. 3.61 x 1023

d. 6 x 1023

Q. 30.On heating, the hydrated salt CaSO4, xH2O loses its water of crystallization. In an experiment it was found that when 0.2 mol of the hydrated salt was heated 0.10 mol of water was lost. What is the molecular formula of the hydrated compound?

a. CaSO4

b. CaSO3. ½ H2O

c. CaSO4.H2O

d. CaSO4.2H2O

Q. 31.Zirconium chloride reacts with magnesium to produce Zirconium. The process is called Knoll process.

ZrCI4 + 2MgZr + 2MgCI2

How many moles Zr would be produced if 0.2 mol of Mg metal is used in the reaction?

a. 0.1

b. 0.01

c. 0.20

d. 0.05

Q. 32.Tobacco contains a poisonous alkaloid called Nicotine. The molecular formula of nicotine is C10H14N2 (molar mass = 162.23g). The mass percentage of nitrogen in nicotine, is?

a. 4.32%

b. 8.23%

c. 12.4%

d. 17.3%

Q. 33.A sample of an ionic compound contains 2.82 g Na, 4.35 g CI, and 7.83 g O. The empirical formula of this compound is___________

a. NaCIO2

b. NaCIO3

c. NaCIO

d. NaCIO4

Q. 34. The numbers of moles in 23g of Na are ___________

(a) 2 moles

(b) 3 moles

(c) 1 mole

(d) Non of above

Q. 35. Number of molecules in 36g of water is ___________

(a) 6.02*1023

(b) 1.204*1024

(c) 3.01*1023

Q. 36. Number of Na ions and Cl ions in 58.5g of NaCl

(a) 6.02*1023 Na ions, 3.01*1023 Cl ions

(b) 6.02*1023Na ions, 6.02*1023 Cl ions

(c) Both (a) and (b)

Q. 37. Number of atoms in 12g of Mg

(a) 6.02*1023

(b) 1.204*1024

(c) 3.01*1023

(d) None of above

Q. 38. A compound contains 60 % Mg and calculates the mole ratio

(a) 2

(b) 2.5

(c) 3

(d) 5

Q. 39. The empirical formula of a compound is CH2O, the value of n= 6 the molecular formula is___________

(a) C12H22O11

(b) C6H12O6

(c) C6H22O6

(d) None of above

Q. 40. One mole of any gas at S.T.P occupies the volume

(a) 44.8 dm3

(b) 22.4 dm3

(c) 66.9 dm3

(d) Non of above

Q. 41. Na2S4O6is represented by__________

(a) Both empirical and molecular formulae

(b) Only by molecular formulae

(c) Only by empirical formulae

(d) None of above

Q. 42. 6 moles of H2 on complete consumption produce __________ dm3of ammonia

N2 + 3H2 ………………> 2NH3

(a) 22.4dm3

(b) 44.8dm3

(c) 89.6dm3

(d) none of above

Q. 43. Limiting reactant is_________

(a) which is in excess quantity

(b) which consumes earlier

(c) which never consumes

(d) none of above

Q. 44. According to gay lussac law gases reacts in a volume of ______________ under the similar conditions of temperature and pressure

(a) fractions

(b) small whole number ratio

(c) large whole number ratio

(d) both (b) and (c)

Q. 45. What volume of CO2 will be formed by consuming 96g of O2

C + O2……………………> CO2

(a) 22.4 dm3

(b) 44.8 dm3

(c) 67.2 dm3

(d) Non of above

Q. 46. 32g of S react with 1g of H2 produce 17g of H2S, which reactant is limiting reactant and which one is in excess

S +H2 ……………> H2S

(a) S in limiting reactant and H2is in excess

(b) H2 in limiting reactant and S is in excess

(c) H2and S both are limiting reactant

(d) Non of above

Q. 47. Assumptions of stoichiometry are ___________ in number

(a) 1

(b) 2

(c) 3

(d) Non of above

Q. 48. Calculate the mass of C in 6.24g of CO2. And mass of H2in 5.8g of H2O

(a) 8g C and 6g H2

(b) 7g C and 0.64g H2

(c) 7g H and 0.64g C

(d) None of above

Q. 49. A compound consists of C, H and O % of C is 20. % of H is 3.06. % of O will be______________

(a) 76.00

(b) 76.94

(c) 0.9476

(d) Non of above

Q. 50. A compound has empirical formula mass is 30; its molecular mass is 60. The value of “n” will be_________

(a) 0.5

(b) 1

(c) 2

(d) None of above

Q. 51. A gas occupies a volume of 67.2 dm3 at S.T.P how many number of moles are there?

(a) 1

(b) 2

(c) 3

(d) None of above

Q. 52. A mole can be defined as__________

(a) Mass of substance expressed in grams

(b) Mass of substance contains Avogadro number of particles

(c) Both (a) and (b)

(d) Non of above

Q. 53. Relative atomic mass can be defined as _____________

(a) Mass of one atom of an element compared to mass of one atom of C

(b) Mass of one atom of an element compared to mass of 1g of C

(c) Mass of one atom of an element compared to mass of one atom of H

(d) None of above.

Q. 54. Molecular formula is___________

(a) Fractional multiple of empirical formula

(b) Integral multiple of empirical formulae

(c) Square root of empirical formulae

(d) None of above

Q. 55. A compound consist of 2.4g of Mg and 1.6g of O. % of Mg and O will be__________

(a) 40% Mg, 60% O

(b) 60% Mg, 40% O

(c) both of above

(d) none of above

Q. 56. 100g of CaCO3 on decomposition produce 56g of CaO, 50 g of CaCO3 on decomposition produce 28g of CaO. Is an example of __________

(a) mass volume relationship

(b) volume volume relationship

(c) mass mass relationship

(d) none of above

Q. 57. Uncertain digit in the given significant number 0.000034571

(a) 3

(b) 7

(c) 1

(d) None of above

Q. 58. Very large number and very small number are expressed by _____________

(a) Significant number

(b) Exponential notation

(c) Avogadro number

(d) Non of above

Q. 59. Chemistry is the branch of science which deals with the study of ____________

(a) World

(b) The materials of which world is made up of

(c) Non of above

Q. 60. Evaporation of spirit is_________

(a) Physical change

(b) Chemical change

(c) Non of above

Q. 61. Burning of coal _________

(a) Physical change

(b) Chemical change

(c) Non of above

Q. 62. Reliable digits which are known with certainly are called_________

(a) Significant figures

(b) Non significant

(c) Non of above

Q. 63. Every last digit in the significant figures is__________

(a) Certain

(b) Un certain

(c) Non of above

Q. 64. Rounding off data is carried out

(a) To drop significant digit

(b) To get the desired number of significant digits

(c) Both of these

Q. 65. There are _____________ types of errors

(a) Three

(b) Two

(c) Four

Q. 66. Systematic errors are __________

(a) Due to the machine

(b) Due to the lack of expertise

(c) Due to the environment

Q. 67. Random errors are__________

(a )Due to the machine

(b) Due to the lack of expertise

(c) Due to the environment

Q. 68. Change from original__________

(a) Error

(b) Deviation

(c) Non of above

Q. 69. Mass of an atom of an element compared to mass of one atom of C12

(a) Atomic number

(b) Atomic mass

(c) Molecular mass

Q. 70. Carbon dating involves __________

(a) C13

(b) C12

(c) C14

Q. 71. The sum of atomic masses of all the atoms present in the formula unit of the substance is_______________

(a) Molecular formula

(b) Formula mass

(c) Molecular mass

Q. 72. The sum of atomic masses of all the atoms present in the molecule or compound is ______________

(a) Empirical formula

(b) Formula mass

(c) Molecular mass

Q. 73. Formula which is found by experiment__________

(a) Molecular formula

(b) Empirical formula

(c) Non of above

Q. 74. Integral multiple of empirical formula is_____________

(a) Molecular mass

(b) Molecular formula

(c) Molar mass

Q. 75. All ionic compounds except one are represented by____________

(a) Molecular formulae

(b) Empirical formula

(c) Non of above

Q. 76. Ionic compounds do not exist in the form of ____________

(a) Compounds

(b) Molecules

(c) Non of above

Q. 77. Empirical formula of water is_________

(a) H2O

(b) OH2

(c) HO

Q. 78. The relative number of atoms present in the molecule represented by_________

(a) Empirical formula

(b) Molecular formula

(c) Non of above

Q. 79. H2O, CH4 have_____________

(a) Same molecular mass

(b) Same formula mass

(c) Same empirical and molecular formula

Q. 80. Na2S4O6 is___________

(a) Covalent compound

(b) Ionic compound

(c) Non of above

Q. 81. Molecular formula is the____________

(a) Fractional multiple of empirical formula

(b) Integral multiple of empirical formula

(c) Non of above

Q. 82. Molecular formulae is __________

(a) n/ empirical formulae

(b) n* Empirical formulae

(c) non of above

Q. 83.emprrical formula of glucose is___________

(a) CH2O

(b) COH2

(c) C2H4O2

SUBJECTIVE

1. Calculate the mass of 10-3 moles of MgSO4

2. State why empirical formula called simplest formula?

3. Calculate the number of moles in 120g of glucose.

4. Ionic compounds are represented by empirical formula. Why?

5. Na2S4O6 is an ionic compound but represents by molecular formula. Why?

6. Calculate the mass of 3.01 ˣ 1020 atoms of Na.

7. Calculate the volume of CO2 gas at S.T.P by the combustion of 40 g of CH4.

8. A compound of C, H and N contains 66.70 % carbon, 7.41 % hydrogen and 25.90 % nitrogen. The molecular mass of compound was found to be 108. Find the empirical and molecular formula of the compound.

9. Round off the data up to four, three and two significant digits.

(a) 5.9876459 _________________, __________________, _________________

(b) 2.987605 __________________, __________________, __________________

10. Write the exponential notation of the following.

a) 123000000000000000000000000. ____________________.

b) 0.0000000000000000005460. _______________________.

11. How many moles are present in 5gms of the following?

a) CO2 b) Mg c) C6H76 d) CuSO4

CHAPTER#02

STATES OF MATTER

MCQs

Choose the correct answer.

Q. 1.Professor Qawwi told his students that air is a mixture because: suddenly a student raised his hand and said

a. it is colorless

b. oxygen can be removed from it

c. its composition is different at different altitudes

d. it has different properties from its constituents

Q. 2.Imagine Dr. Rehan is sitting in a room. The room is closed from all sides, no entry, and no exit of any gas. If the room expands suddenly then

a. he will be frightened

b. his blood pressure will decrease

c. he will feel cool

d. he will feel warmth

Q. 3.Which of the following elements will have strongest Van Der Waal force of attraction between its molecules?

a. hydrogen

b. oxygen

c. chlorine

d. nitrogen

Q. 4.The beaker shown in the figure contains slurry of ice and water, the three thermometers Fahrenheit, Kelvin and Centigrade placed in it. The thermometers are represented by A, B and C respectively. The lowest reading will be on thermometer.

a. A

b. B

c. C

d. Both A and C

Q. 5.Which thermometer will have its reading 273 degrees greater than that of thermometer C?

a. A

b. B

c. C has greater reading than all other thermometer

d. B has 273 degrees greater reading than A

Q. 6.The temperature recorded by Kelvin scale is

a. 0K

b. 273K

c. 373K

d. Absolute scale is unable to record this temperature

Q. 7.If three birds called O2, CI2 and H2 were flying in the garden of Iba public school then,

I. Fastest birds are O2 and CI2

II. Slowest bird is CI2

III. Bird called O2 is in the middle.

a. I only

b. II and III only

c. I and III only

d. III only

Q. 8.One liter of an unknown gas weighs 1.25 grams at S.T.P, one possible formula for the gas is

a. CO2

b. CO

c. O2

d. SO2

Q. 9.If pressure on a gas is increased from 2 atm to 4 atm than its volume will decrease from

a. 6L to 4L

b. 8L to 2L

c. 3L to 1L

d. 4L to 2L

Q. 10.An unknown gas has a density of 2.45 g/L at 1.5atmospheric pressure and 25oC. The gas is

a. Kr

b. CI2

c. SO2

d. Ar

Q. 11.This is a known fact that the molar volumes of different gases at S.T.P are

a. little bit greater than the molar volumes of liquids

b. little bit less than the molar volumes of solids

c. about the same as the molar volumes of liquids

d. much larger than the molar volumes of liquids and solids

Q. 12.The behavior of a gas is non-ideal at

a. lo2w temperature and low pressure

b. high temperature and high pressure

c. high temperature and low pressure

d. low temperature and high pressure

Q. 13.Ammonium Per chlorate is used as solid fuel in rockets. During the process it decomposes according to the reaction given below

4NH4CIO4 (g) 2CI2 (g) +8H2O (g) +2N2O (g) +3O2 (g)

The total volume of all the gases produced at S.T.P by the decomposition of 8 moles of Ammonium Per chlorate will be

a. 30 L

b. 672 L

c. 179.0 L

d. 60 L

Q. 14.Compressed natural gas (CNG) contains mainly methane CH4. Methane gas burns in air according to the following reaction.

CH4 (g) + 2O2 (g)CO2 (g) + 2H2O (g)

If 8 g of methane is burnt, what volume of CO2 measured at S.T.P. will be produced?

a. 0.5 L

b. 22 L

c. 22.4 L

d. 11.2 L

Q. 15.A kid has a helium filled balloon which deflates at the rate of 1.00 liter/day by He gas leaking through the relatively porous skin of the balloon. How fast would carbon dioxide (CO2) leak from a balloon made of the same material?

a. 3.0 L/day

b. 0.3 L/day

c. 1.33 L/day

d. 3.33 L/day

Q. 16.All of the following statements are false except

a. gas molecules do not attract each other at very low temperature

b. all of the gases cannot be liquefied

c. increase in pressure will not decrease the intermolecular distance in a gas

d. actual volume of a gas is not negligible at very high pressure

Q. 17.At the same temperature and pressure helium is more ideal than hydrogen due to

a. greater molar mass

b. less molar mass

c. greater molecular size

d. less molecular size

Q. 18.A container with a porous wall has a mixture of H2, He, N2 and O2. Which of these gases will take maximum time in getting out of the container?

a. H2

b. He

c. N2

d. O2

Q. 19.The value of for an unknown gas is equal to

a. 0.082 L.atm.mol-1.K

b. 0.082 L.atm.mol-1.K-1

c. 0.82 L.atm.mol.K-1

d. 0.82 L.atm.mol.K-1

Q. 20.If the temperature of the atmosphere is 30oC then which of the following will have highest average speed

a. O2

b. H2

c. Ne

d. N2

Q. 21.The volume of one kilogram of water at 4oC is equal to one litre. The temperature of water is kept at 4oC because water

a. has no dissolved gasses at this temperature

b. has maximum density at this temperature

c. polarity of water molecule is least at this temperature

d. dipole moment has maximum value at this temperature

Q. 22.Which of the following is a substance?

a. sea water

b. Brass

c. tape water

d. graphite

Q. 23.Freezing point of a substance is a temperature at which a liquid substance is converted to solid, it is

a. always lower than its melting point

b. usually a little lower than its melting point

c. always higher than its melting point

d. exactly the same as its melting point

Q. 25.The content of the matter in a body is called_________

a. Inertia

b. Energy

c. Weight

d. Mass

Q. 26.A liquid has its own volume because of _________

a. Less random motion of molecules as compared to gases

b. High kinetic energy between molecules

c. The liquid molecules are free to move

d. The liquid molecules consist of clusters

Q. 27.Kinetic theory is named so because____________

a. Molecules have high kinetic energy

b. Molecules are in constant motion

c. Molecules show mean free path

d. Molecules collide against container

Q. 28.The forces of attraction are weaker between the molecules of_________

a. Oxygen

b. Chlorine

c. Zinc

d. Bromine

Q. 29.The three states of matter solid, liquid and gas are due to_________

a. Physical properties

b. Chemical properties

c. Different arrangement of atoms

d. Pressure exerted by the atoms

Q.30.The gases diffuse rapidly due to _________

a. Free movement of molecules

b. Free motion of molecules

c. Large empty space between molecules

d. All

Q. 31.A real gas has less pressure than ideal gas because of_________

a. Finite size of molecules

b. Increase in kinetic energy

c. Intermolecular forces

d. Increased number of collisions

Q. 32.An ideal gas is defined as which obeys_________

a. Boyles Law

b. Charles law

c. Avogadro’s Law

d. Gas Law

Q. 33.The pressure of the gas increase when temperature_________

a. Increase

b. Decrease

c. Remain constant

d. With condition

Q. 34.Which one of the following describe STP_________

a. 25C and 1 atm

b. 0C and 1 atm

c. 273K and 1 Pa

d. 0C and 1 Pa

Q. 35.1 atm is equal to all except_________

a. 760 mm Hg

b. 14.7 lb/inch2

c. 101625 Pa

d. 700 torr

Q. 36.The value of gas constant ‘R’ in Cal/deg/mol is_________

a. 0.0821

b. 8.314

c. 1.987

d. 22.4

Q. 37.At Absolute zero gases exists as_________

a. Solid

b. Liquid

c. Gas

d. Plasma

Q. 38.The gas which diffuses with slowest rate _________

a. CO2

b. NO

c. SO2

d. NH3

Q. 39.No diffusion in one of the following take place_________

a. In a mixture of NH3 and HCl

b. Saturates solution of CuSO4 and water

c. A mixture of air and NO2

d. Copper sulfate solution and graphite

Q. 40.With the increase in temperature the decrease in viscosity is_________

a. 1%

b. 2%

c. 3%

d. 3.5%

Q. 41.The gas molecules exert pressure on the walls of container because of_________

a. Attraction

b. Adhesive

c. Collision

d. Strong forces

Q. 42.The droplets are spherical because of_________

a. Viscosity

b. Tendency to acquire minimum surface

c. Tendency to acquire maximum surface

d. Pressure

Q. 43.The force of attraction b/w liquid and another surface _________

a. Cohesive forces

b. Adhesive forces

c. London forces

d. Hydrogen bonding

Q. 44.A crystalline solid shows the properties that vary with direction_________

a. Anisotropy

b. Allotropy

c. Isotropy

d. All

Q. 45.Amorphous solids do not have _________

a. Sharp melting point

b. Geometrical shape

c. Regular structure

d. All

Q. 46.The volume occupied by 9grams of H2O at 0C and 760 torr _________

a. 22.4 dm3

b. 11.2 dm3

c. 44.8 dm3

d. 5.6 dm3

Q. 47.When water is cooled from 4C to 0C then it _________

a. Contracts

b. Expand

c. Diffuse

d. No change

Q. 48.The cohesive forces are weakest among the molecules of _________

a. Solids

b. Liquids

c. Gases

d. Colloids

Q. 49.Ice is an example of _________type of crystal

a. Ionic

b. Atomic

c. Covalent

d. molecular

Q. 50.The empirical formula of benzene is _________

a. C6H12O6

b. CH2O

c. CH

d. C6H6

SUBJECTIVE

1. By which formula densities of ideal gases are calculated?

2. A mixture of gases at 760 torr contains 2 moles of hydrogen and 4 moles of carbon dioxide. What is the partial pressure of each gas in torr?

3. Calculate the rate of diffusion of the following,

(a) CO2 (b) SO2 (c) NO (d) CO

4. The substances contain atoms, ions or molecules but why some materials are solid, some liquid and some gases at

room temperature?

5. Gases compressed more than liquids. Why?

6. Honey is more viscous than water. Why?

7. The boiling point of water remains same although heat is continuously supplied to the liquid. How?

8. Why the properties of gases cannot be studied at Absolute zero?

9. Why Cooker pressure is valuable at Mount Everest?

10. Why Real gases deviate from ideal gases.

11. Why does water spilled on floor evaporate more rapidly than the same amount of water in a jug?

12. According to Boyle’s law, when volume is reduced, the gas molecules come closer to each other and collide more

frequently produce high pressure but velocity of the particles will remain same. Why?

13. How Kinetic energy and intermolecular forces between molecules determine the physical state of substance. (Solid,

liquid and gas)?

14. Why liquids do not flow as liquids and gases do?

15. Cooker pressure cooks food more quickly as compare to covered pot?

16. A falling drop of a liquid is spherical?

17. A drop of ink spreads on a blotting paper?

18. How Evaporation is a cooling process?

19. Why mercury has its meniscus upward?

20. Why Graphite conducts electricity when it is placed parallel to the direction of current.

21. Why crystalline solids have characteristic shape but amorphous solids do not have the same.

22. The melting point of diamond is high but that of graphite is low. How?

CHAPTER#03

ATOMIC STRCTURE

Choose the correct answer.

1/ Atom is

(a) Indivisible (b) divisible (c) do not exist

2/ electron, proton, neutron are

(a) Individual atom (b) sub atomic particle (c) do not exist

3/ faraday’s experiment shows the existence of

(a) Electron (b) proton (c) neutron

4/ crook’s tube experiment shows the discovery of

(a) Proton (b) neutron (c) electron

5/ fast moving electrons are

(a) Anode rays (b) cathode rays (c) x- rays

6/ positive rays are

(a) Anode rays (b) cathode rays (c) x- rays

7/ Anode rays are

(a) Negatively charged gas(b) positively charged gas (c) fast moving electrons

8/ properties of cathode rays were described by

(a) Goldstein (b) faraday (c) Thomson

9/ cathode rays move in

(a) Random direction (b) straight path (c) no path

10/ cathode rays have

(a) Potential energy (b) no energy (c) mechanical energy

11/ charge to mass ratio of cathode rays depends upon

(a) Nature of gas (b) do not depend upon nature of gas (c) both (a) and (b)

12/ charge to mass ratio of anode rays depends upon

(a) Nature of gas (b) do not depend upon nature of gas (c) both (a) and (b)

13/ proton have

(a) Greatest charge to mass ratio (b) least charge to mass ratio (c) none of above

14/ radioactivity was discovered by

(a) Marie curie (b) parie curie (c) hennery bacquriel

15/ radioactivity shows the evidence for

(a) Electron (b) proton (c) neutron (d) all of above

16/ Radium was discovered by

(a) Marie curie parie curie (b) hennery bacquriel(c) faraday

17/ Hennery bacquriel used the uranium ore named

(a) Bauxite (b) corundum (c) pitchblende

18/ alpha particle are

(a) Positively charged (b) negatively charged (c) neutral

19/ beta particles are

(a) Positively charged (b) negatively charged (c) neutral

20/ gamma particles are

(a) Positively charged (b) negatively charged (c) neutral

21/ x rays emerge from

(a) Cathode (b) anode (c) both (a) and (b)

22/ x-rays emit from electron of

(a) Outermost shell of atom (b) inner most shell of atom (c) middle shell of an atom

23/ gamma rays emerge from

(a) Shell of the atom (b) nucleus of the atom (c) both (a) and (b)

24/ gamma rays are

(a) Electron (b) proton (c) energy

25/ electricity can be conducted from air

(a) At high pressure (b) at low pressure (c) at very low pressure

26/ neutron was discovered by

(a) Gold stein (b) Chadwick(c) faraday

27/ highest frequency wave in visible region is

(a) Red (b) violet (c) green (d) yellow

28/ light bent at greatest angle is

(a) Red (b) violet (c) green(d) yellow

29/ white light is mixture of ------------ colors

(a) One (b) two (c) three (d) seven

30/ prism cause

(a) Conversion of light (b) dispersion of light (c) do nothing

31/ prism is

(a) Denser medium than air (b) less denser medium then air (C) least denser medium then air

32/ spectrum that is finger print of all the elements

(a) Continuous spectrum (b) line spectrum (c) both (a) and (b)

33/ sodium lamp emit ------------- colored light

(a) Blue (b) red (c) yellow

34/ wavelength of violet and red lights are

(a) 4000 to 7000 A (b) 7000 to 4000 A (c) 3000 to 2000 A

35/ Rutherford bombard ____________ particles with gold foil

(a) Alpha (b) beta (c) gamma

36/ concentrated part of atom is

(a) Shell (b) nucleus (c) orbital

37/ modern periodic table was made after the discovery of

(a) Alpha rays (b) beta rays(c) x rays

38/ Mosley arranged the elements on the basis of increasing atomic ___________ of elements

(a) Weight(b) number (c) number of neutron

39/ according to Bohr the possible energy levels are only those orbits in which product of angular momentum and circumference are equal to

(a) h/2π (b) nh/2π (c) both (a) and (b)

40/ the radius of first orbit of hydrogen atom is equal to

(a) 0.521 A (b) 0.522 A (C) 0.529 A

41/ Value for Rhydberg constant is

(a) 109675 cm-1(b) 109678 cm-1(c) 109670 cm-1

42/ Balmer series are in

(a) UV region (b) visible region (c) IR region

43/ position and momentum of electron

(a) Can be found simultaneously (b) cannot be found simultaneously (c) both (a) and (b

44/ energy levels are expressed by

(a) S,p,d,f(b) K,L,M,N (c) 1,2,3,4 (c) both (b) and (c)

45/ number of sub energy levels present in each energy level are

(a) Less than the number of energy level

(b) Equal to number of energy level

(c) Non of above

46/ number of electron in energy level can be find by formula

(a) n2(b) 2n2(c) (2l +1)

47/ number of sub shell in main shell can be calculated by formula

(a) (2l +1)(b) 2(2l +1) (c) n2

48/ half of the distance between two homo nuclear diatomic molecules

(a) Ionic radius (b) atomic radius (c) both (a) and (b)

49/ distance from nucleus to valance shell electron of and ion

(a) Ionic radius (b) atomic radius (c) both (a) and (b)

50/ size of cat ion is

(a) Greater than parent atom (b) smaller than parent atom (c) same as parent atom

51/ size of anion is

(a) Greater than parent atom (b) smaller than parent atom (c) same as parent atom

52/minimum amount of energy required to remove an electron from the valance shell of an atom is

(a) Electro negativity (b) electron affinity (c) ionization potential

53/ energy change occur when an electron is added to an atom is

(b) Electro negativity (b) electron affinity (c) ionization potential

54/ 1st I.P is

(a) Greater than 2nd(b) less than 2nd(c) equal to 2nd

55/ 2nd electron affinity is always

(a) Exothermic (b) endothermic (d) both (a) and (b)

56/ In an atom two electron can have maximum ______ quantum number same

(a) 1 (b) 2 (c) 3 (d) 4

57/ electron present in the same orbital have ______ quantum number different

(a) n (b) l (c) m (d) s

58/ electrons present in the same orbital have

(a) same spins(c) opposite spins(c) can be same can be opposite spins

59/ maximum number of electrons present in s,p,d, f sub shell can be

(a) 2,2,10,14 (b) 2,4,10.14 (c) 2,6, 10.14

60/ maximum number of orbital in s,p,d, f sub shell can be

(a) 1.3,5,7 (b) 2,6, 10.14 (c) 1.6,5,14

61/ shapes of s,p orbital are _________ respectively

(a) Dumb-bell, spherical (b) spherical , Dumb-bell (c) spherical, complicated

62/ p orbital has ________ lobes

(a) One (b) two (c) three

63/ nodal plane is

(a) Where no electron is found (b) where maximum number of electrons are present

(b) (c) none of above

64/ orbital of p sub shell are directed in

(a) Only one axis (b) in two axis(c) in three axis

65/ “S” orbital is directed in

(a) Only one axis (b) in two axis(c) in three axis

66/ degenerate orbital are

(a) Orbital of same energy (b) orbital of different energy (d) both (a) and (b)

67/ orbital whose n+l value is smaller should be filled ___________

(a) Later (b) first (c) keep empty

68/ according to Hund’s rule electrons in the degenerate orbital be first filled _____________ and then ____________ respectively

(a) Paired, singly (b) singly , Paired (c) Paired,Paired

69/ region in which probability of finding out electron is maximum is

(a) Orbit (b) orbital (c) sub shell

70/ orbital are the part of

(a) Main shell (b) sub shell (c) both (a) and (b)

SUBJECTIVE

(1) Explain the significance of Pauli’s principle in relation to the electronic configuration of atoms.

(2) What are iso electronic ions?

(3) Write the electronic configuration of the following elements according to Aufbau and Hund rule.

(a) Be (b) Xe (c) Mg (d) B

(4) Write the number of electrons proton and neutrons of the following elements.

(a) 8O16 (b) 17Cl35 (c) 20Ca40

(5) Which orbital will fill first with electrons?

(a) 3p, 2s (b) 3d, 4s (c) 5p, 6s

(6) Write the trends of the following in periodic table?

(a) Ionization potential (b) Electro negativity (c) Atomic radius

(7) Define the energy with four quantum numbers of hydrogen atom.

CHAPTER#04

CHEMICAL BONDING

Choose the correct answer

1/ atoms form bond

(a) To gain stability

(b) To gain inert gas configuration

(c) Both (a) and (b)

2/ every atom want to have ___________ electron in its valance shell

(a) 2 (b) 8 (c) 2 or 8 (c) none of above

3/ bond is

(a) Force of attraction between two atoms

(b) Force of repulsion between two atoms

(c) Linkage

(d) Both (a) and (c)

4/ types of chemical bonds are

(a) One (b) two (c) three

5/ ionic bond is formed by

(a) Loss of electron (b) gain of electron (c) gain or loss of electron

6/ the atom in ionic bond which gain electron become

(a) Positively charged (b) negatively charged (c) neutral

7/ the atom in ionic bond which lose electron become

(b) Positively charged (b) negatively charged (c) neutral

8/ during the formation of ionic bond

(a) Cat ion gains energy to lose electron

(b) Anion lose energy to gain electron

(c) Both (a) and (b)

9/ ionic compounds are

(a) Soft and brittle (b) hard and brittle (c) can easily melt

10/ the melting and boiling point of ionic compounds are

(a) Low (b) high (c) very high

11/ ionic compounds are easily soluble in

(a) Non polar solvents (b) polar solvents (c) water (d) both (b) and (c)

12/ polar solutes are soluble in water

(a) If hydration energy is less than bond energy

(b) If hydration energy is more than bond energy

(c) If hydration energy is equal to bond energy

13/ Ionic compounds are __________ electrolytes

(a) Bad (b) poor (c) good

14/ covalent compounds are formed by

(a) Transfer of electron (b) two sided sharing of electron (c) one sided sharing of electron

15/ covalent bond is formed between

(a) Metal and non metal(b) non metal and non metal(c) metal and metal

16/ covalent bond formed between non metals of different electro negativities are

(a) Polar in nature (b) non polar in nature (c) neutral in nature

17/ water molecule have

(a) Ionic bond (b) covalent bond (c) polar covalent bond

18/on the basis of number of electron shared between non metals covalent bonds are _______ types

(a) One (b) two (c) three

19/ increasing order of bond length in covalent bond are

(a) Triple < double < single (b) single < double< triple (c) double < single< triple

20/ increasing order of bond energy

(b) Triple < double < single (b) single < double< triple (c) double < single< triple

21/ increasing order of bond distance in covalent bond

(c) Triple < double < single (b) single < double< triple (c) double < single< triple

22/ greater the electro negativity difference between the bonded atoms

(a) Weaker the bond lesser the bond energy

(b) Stronger the bond greater the bond energy

(c) Smaller the bond length greater the bond energy

(d) Both (b) and (c)

23/ increasing order of polarity

(a) HF>HCl>HBr>HI (b) HI

24 bond energy of HF is __________ than HCl

(a) Smaller (b) greater (c) equal

25/ HF is ________ % polar

(a) 17% (b) 64% (c ) 100%

26/covalent compounds are

(a) Non directional (b) directional (c) having many directions

27/ covalent bond formed between two same atoms is

(a) Polar (b) non polar (c) highly polar

28/ the product of charge and distance between charge is

(a) I.P (b) E.N (c) dipole moment

29/ S.I unit of dipole moment is

(a) Debye (b) coulomb meter (c) ampere meter

30/ molecules are of ___________ types on the basis of number of atoms combined with each other.

(a) One (b) three (c) two

31/ symmetrical polyatomic molecules have dipole moment equal to ____________

(a) 0 (b) have some value of dipole moment (c) none of above

32/ greater the polarity of molecule ________________ the dipole moment

(a) Lesser (b)greater (c) 0

33/ dipole moment of CO2 is ___________

(b) 0 (b) have some value of dipole moment (c) none of above

34/ dipole moment of SO2is

(c) 0 (b) have some value of dipole moment (c) none of above

35/ SO2is

(a) Non symmetrical (b) symmetrical (c) partially symmetrical

36/ sigma bond is formed by

(a) Head to head overlap of atomic orbitals

(b) Side to side overlap of atomic orbitals

(c) do not exist

37/ pi bond is formed by

(a) Head to head overlap of atomic orbitals

(b) Side to side overlap of atomic orbitals

(c) do not exist

38/ according to valance bond theory the shared electrons are attracted by

(a) atomic orbitals (b) molecular orbitals (c) not attracted by any nucleus

39/ the anti bonding molecular orbitals have ____________ electron probability

(a) highest (b) lowest (c) moderate

40/ The bonding molecular orbitals have ____________ electron probability

(b) highest (b) lowest (c) moderate

41/ strength of bond in increasing order

(a) s-s, p.p, s-p (b) s-s, s-p, p-p (c) p-p, s-p, s-s

42/ pi bonds are formed

(a) below s orbital (b) above S orbitals (c) near S orbital

43/ shape of BeCl2 is

(a) Trigonal (b) linear (c) tetrahedral (c) angular

44/ hybridization in C2H2 is

(a) SP (b) SP2 (c) SP3 (d) SP3d2

45/ C atom possess

(a) Only one hybridization (b) two hybridization (c) three hybridization

46/ VESPER theory defines

(a) Covalent nature of molecules (b) shape of molecules (c) nature of molecules

47/ energy of anti bonding molecular orbitals is

(a) Equal to bonding molecular orbitals (b) lower than bonging molecular orbitals (c) greater than bonding molecular orbitals.

48/ anti bonding molecular orbitals are formed

(a) By nuclear nuclear repulsion (b) electron electron attraction (d) ) electron electron repulsion

49/ the probability of finding out electron is

(a) Minimum in bonding molecular orbitals

(b) Maximum in bonding molecular orbitals

(c) Minimum in antibonding molecular orbitals

(d) Maximum in antibonding molecular orbitals

50/ valancy of C in excited state is

(a) 2 (b) 3 (c) 4 (d) 5

51/ C take part in bonding in

(a) Ground state (b) excited state (c) do not take part in bonding

52/ According to molecular orbital theory the bonding electrons are attracted by

(a) Only one nucleus (b) By multi nuclei (c) by no any nuclei

53/ the active set of electron are

(a) All valance electron (b) only unpaired electrons (c) only paired electrons

54/ Hydrogen bonding is

(a) Primary bong (b) secondary bond (c) no bond

55/ ___________ properties of compounds are affected by hydrogen bonding

(a) Chemical properties (b) physical properties (c) no any property

56/ boiling point of HF is lower than water because

(a) Greater number of hydrogen bonding per molecule that water

(b) Lesser number of hydrogen bonding per molecule that water

(c) No hydrogen bonding

57/ PCl3O the coordinate bond is between

(a) P and Cl (b) P and O (b) Cl-Cl (c) O-O

58/ coordinate covalent bond is formed by one sided sharing of

(a) Bond pair electrons (b) lone pair of electrons (c) no electrons

59/ Electro negativity difference between bonded atoms induces

(a) Non polarity in molecule (b) polarity in molecule (c) do nothing

60/ greater the electro negativity difference between bonded atoms

(a) Shorter the bond length (b) greater the bond length (c) no any effect on bond length.

61/ covalent bond is formed between

(a) Two metals (b) two nonmetals (c) metal and non metal

62/ elements of group IA, IIA, IIIA involves in the formation of

(a) Covalent bond (b) coordinate bond (c) ionic bond

SUBJECTIVE

1. Explain the sigma and pi bonding

2. What is the affect of ionic character on covalent compounds?

3. What is the difference between polar and non polar?

4. What are the factors on which dipole moment of molecules depend upon?

5. How ionic bond is formed in NaCl bond formation?

6. Draw the shapes of the following molecules.

(a) H2O (b) BeCl2 (c) NH3

7. Explain the structure of CH4 with the help of hybridization.

8. Explain sp2 and sp hybridization with examples.

9. Draw the shape of BF3 and explain it with hybrid orbital model

10. What is hydrogen bond? Why water, ammonia and fluoric acid form hydrogen bond?

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