MDCAT Chemistry Chapter 4 MCQ Test With Answer for (Chemical Bonding)

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MCQ's Test For MDCAT Chemistry Chapter 4 Chemical Bonding Online Test

Try The MCQ's Test For MDCAT Chemistry Chapter 4 Chemical Bonding Online Test

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MDCAT Chemistry Chapter 4 Chemical Bonding Online Test

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Question # 1

The nature of the attractive force in acetone and chloroform are

Question # 2

H2O and HF are the hydrides of the second period. Fluorine is more electronegative than oxygen. Anyhow, the boiling point of water is greater than that of HF. This is due to:

Question # 3

The boiling of water may be 120°C, when the external pressure is

Question # 4

Which of following factor affect vapour pressure of a liquid?

Question # 5

The nature of crystals formed due to London forces of interaction are

Question # 6

Which of the following liquid has highest bolling point

Question # 7

lce occupies more space than liquid water

Question # 8

The B.P. of compound is mostly raised by

Question # 9

The weakest intermolecular forces present in a liquid may be

Question # 10

Polarizability is responsible for intermolecular forces and it

Question # 11

H-bonding is maximum in:

Question # 12

Vapour pressure of a substance does not depend upon:

Question # 13

At freezing point of water, the density decreases due to

Question # 14

Oxygen and sulphur are present in VI-A group of the periodic table The hydride of oxygen i.e., H2O is liquid at room temperature but the hydride of sulphur (H2S) is a gas. This is due to

Question # 15

The boiling point of H2O is 100°C while that of C2H5-OH is 78.5C°. The reason is that:

Question # 16

Hydrogen bonding is not present in which of following compound?

Question # 17

Saturated hydrocarbons having carbon atoms more than 20 in a molecule are solids due to

Question # 18

Hydrogen bonding is extensively present in proteins which form the spiral. The hydrogen bond being produced is between

Question # 19

Liquids evaporate at every temperature. When the temperature becomes constant for a liquid, then:

Question # 20

Point out the substance which has maximum vapour pressure at a given temperature?

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Prepare Complete Set Wise MDCAT Chemistry Chapter 4 Chemical Bonding Online Test MCQs Online With Answers


In this topic,Student should be able to :

a) Characterize electrovalent (ionic) bond as in sodium chloride and calcium oxide.

b) Use the ‘dot-and-cross’ diagrams to explain: i) Covalent bonding, as in hydrogen(H2); oxygen(O2); chlorine(Cl2); hydrogen chloride; carbon dioxide; methane and ethane. ii) Co-ordinate (dative covalent) bonding, as in the formation of the ammonium ion in H3N+– -BF3 and H3O+.

c) Describe the shapes and bond angles in molecules by using the qualitative model of Valence Shell Electron-Pair Repulsion (VSEPR) theory up to 4 pairs of electron including bonded electron pair and lone pair around central atom. d) Describe covalent bonding in terms of orbital overlap, giving  and  bonds.

e) Explain the shape of and bond angles in ethane, ethene and benzene molecules in terms of  and  bonds.

f) Describe hydrogen bonding, using ammonia and water as simple examples of molecules containing N-H and O-H groups.

g) Explain the terms bond energy, bond length and bond polarity (electronegativity difference) and use them to compare the nature of covalent bonds i.e. polar and non-polar.

h) Describe intermolecular forces (Van der Waal’s forces), based on permanent and induced dipoles, as in HCl, CHCl3, Halogens and in liquid noble gases.

i) Describe metallic bonding in terms of positive ions surrounded by mobile electrons (sea of electrons).

j) Describe, interpret and/or predict the effect of different types of bonding (ionic bonding; covalent bonding; hydrogen bonding; Van der Waal’s forces and metallic bonding) on the physical properties of substances.

k) Deduce the type of bonding present in a substance from the given information

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Sr.# Question Answer
1 The B.P. of compound is mostly raised by
A. dipole-induced dipole interactions
B. london dispersion forces
C. intramolecular H-bonding
D. intermolecular H-bonding
2 The boiling points of the halogens
A. increases down the group
B. decreases down the group
C. remains constant
D. can not be predicted
3 The B.P of glycerine at 760 torr pressure is
A. 200°C
B. 290C°
C. 250C°
D. 262C°
4 Vapour pressure of a substance does not depend upon:
A. physical state of matter
B. temperature
C. intermolecular forces
D. surface area
5 Liquids evaporate at every temperature. When the temperature becomes constant for a liquid, then:
A. rate of evaporation is greater than the rate of condensation
B. the rate of condensation is greater than the rate of evaporation
C. The rate of condensation and evaporation become equal
D. it depends upon the nature of the liquid
6 The long chains of amino acids are coiled around one another into a spiral by
A. ionic bond
B. Van der Waal's forces
C. hydrogen bonding
D. overlapping of orbitals
7 H-bonding is maximum in:
A. ethanol
B. benzene
C. diethyl ether
D. water
8 Dipole-dipole interaction are present in the
A. atoms of the He gas
B. molecules of CCl4
C. molecules of solid iodine
D. molecules of :NH3
9 In order to maintain the boiling point of water at 110 C°, the extemal pressure should be
A. 550 torr
B. between 500 and 760 tor
C. between 760 and 1500 torr
D. any pressure can be maintained
10 The boiling point of higher alkanes are greater than those of lower alkanes due to reason that
A. higher alkanes have greater number of atoms
B. the polarizabilities of higher alkanes are greater
C. higher alkanes have greater hydrogen bonding
D. higher alkanes have zig-zag structures
11 Ice floats on water because
A. the hydrogen bonding in ice is stronger than that of in water
B. empty spaces are left in ice
C. ice has two-dimensional structure
D. the bond length of the oxygen and hydrogen bond is different in water and ice
12 Halogens form halogen acids. HF is the weakest among all of them This is due to the reason that
A. fluorine is a very small-sized atom
B. fluorine is highly electronegative atom
C. there is strong hydrogen bonding in HF
D. the polarity of HF bond is less
13 Oxygen and sulphur are present in VI-A group of the periodic table The hydride of oxygen i.e., H2O is liquid at room temperature but the hydride of sulphur (H2S) is a gas. This is due to
A. greater bond angle of water than Hs
B. greater bond lengths in HS than H2O
C. hydrogen bonding in water
D. acidic character of HS
14 The nature of crystals formed due to London forces of interaction are
A. molecular
B. metallic
C. ionic
D. covalent
15 lce occupies more space than liquid water
A. 9%
B. 10%
C. 11%
D. 12%
16 The forces which are present between the ions and the water molecules are known as
A. dipole-induced dipole forces
B. dipole-dipole forces
C. ion-dipole forces
D. London dispersion forces

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