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

00:00
Question # 1

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

Question # 2

The forces which are present between the ions and the water molecules are known as

Question # 3

Ice floats on water because

Question # 4

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

Question # 5

The boiling point of higher alkanes are greater than those of lower alkanes due to reason that

Question # 6

The nature of the attractive force in acetone and chloroform are

Question # 7

Vapour pressure of a substance does not depend upon:

Question # 8

Hydrogen bonding is not present in which of following compound?

Question # 9

The boiling points of the halogens

Question # 10

Halogens form halogen acids. HF is the weakest among all of them This is due to the reason that

Question # 11

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 # 12

The B.P. of compound is mostly raised by

Question # 13

Liquid hydrocarbon is

Question # 14

H-bonding is maximum in:

Question # 15

The polarizabilities of elements mostly increase down the group due to the reason that

Question # 16

Dipole-dipole interaction are present in the

Question # 17

Dipole-induced dipole forces are also called

Question # 18

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

Question # 19

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

Question # 20

Strong dipole-dipole forces among the liquid molecules are responsible for

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


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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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MCAT Chemistry Chapter 4 Important MCQ's

Sr.# Question Answer
1 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
2 Polarizability is responsible for intermolecular forces and it
A. increases down the group
B. decreases down the group
C. almost remains the same
D. increased along a period
3 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
4 lce occupies more space than liquid water
A. 9%
B. 10%
C. 11%
D. 12%
5 The boiling point of H2O is 100°C while that of C2H5-OH is 78.5C°. The reason is that:
A. H2O molecules are small-sized
B. the bond angles at oxygen atom are different
C. C2H5-group is electron donating
D. the number of H-bonds are greater in H20, than C2H5-OH
6 Hydrogen bonding is not present in which of following compound?
A. Ammonia
B. Ethanol
C. Ether
D. Water
7 The polarizabilities of elements mostly increase down the group due to the reason that
A. the atomic numbers increase
B. number of protons increase
C. number of shells increase along with increase of shielding effect
D. the behaviour of the elements remain the same
8 Hydrogen bonding is extensively present in proteins which form the spiral. The hydrogen bond being produced is between
A. nitrogen and hydrogen atom
B. oxygen and hydrogen atom
C. carbon and hydrogen atom
D. oxygen and carbon atom
9 Dipole-induced dipole forces are also called
A. dipole-dipole forces
B. ion-dipole forces
C. Debye forces
D. London-dispersion forces
10 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:
A. water is more polar than HF
B. water has a bent structure
C. HF has a zig zag structure after making hydrogen bonding
D. the number of hydrogen bonds produced by water are greater than that of HF

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