ECAT Pre Engineering Chemistry Chapter 6 MCQ Test With Answer

MCQ's Test For ECAT Chemistry Chapter 6 Chemical Bonding

Try The MCQ's Test For ECAT Chemistry Chapter 6 Chemical Bonding

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ECAT Chemistry Chapter 6 Chemical Bonding

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Question # 1

Ionization energies increase from left to right along the period due to

Question # 2

In a group the atomic size increase downward due to

Question # 3

Hydrogen chloride molecule contains

Question # 4

In H2O molecule the bond angle is

Question # 5

Mg becomes isoelectronic with neon when it

Question # 6

The formation of compounds like PF5, BCI3, SF6indicates that

Question # 7

Inter molecular forces in solid hydrogen are

Question # 8

The overlapping of two partially filled atomic orbital is in such a way that the probability of finding the electron pair is maximum along the axis joining the two nuclei, the bond is

Question # 9

The Electro-negatively difference for ionic bond must be greater than

Question # 10

All covalent bonds formed between the two atoms are non-polar when

Question # 11

Fluorine molecule is formed by

Question # 12

The electronegativity of elements in a period from left to right

Question # 13

Nitrogen in NH3is sp3hybridized but the bond angle in NH3is 107° and not 109.5° due to

Question # 14

Water H2O is liquid while hydrogen sulphide H2S is a gas beause

Question # 15

On the basis of VSEPR theory SO2is a

Question # 16

The equation for the first ionization energy of hydrogen is

Question # 17

Outer shells of two elements X and Y have two and six electrons respectively. If they combine, the expected formula of compound will be

Question # 18

Question Image
Question # 19

Ionic radius, in a period from left to right

Question # 20

Which one of these is weakest?

Question # 21

Which of the hydrogen halides has the highest percentage of ionic character

Question # 22

When of the following is isolelectronic with krypton

Question # 23

Planar geometry of molecules is due to

Question # 24

Size of an anion is increased as compared to its atom because of the

Question # 25

The electronegativeities of F,Cl,Br and I are 4.0,3.0,2.8,2.5 respectively.Hydrogen halide with a high percentage of ionic character is

Question # 26

Shielding effect intervening electrons causes

Question # 27

Covalent compounds are soluble in

Question # 28

Which of the following statements is not correct regarding bonding molecular orbitals?

Question # 29

The shape of gaseous SnCl2is

Question # 30

Which of the following molecules have multiple bonds

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Sr. # Question Answer
1 The geometry of 4 sp3hybrid orbitals on an atom is

A. Square planar

B. Tetrahedral

C.Trigonal planar

D. Linear

2 Inter molecular forces in solid hydrogen are

A. Covalent forces

B. Van der Waal forces or London dispersion forces

C.Hydrogen bonds

D. All of these

3 Two H-atom combine to form a strong H2molecule due to

A. Increase in potential energy

B. Decrease in potential energy

C.Energy remains unchanged

D. Distance is increased

4 Noble gases have the electronic configuration with their valance shell ns2np6except one

A. He

B. Ne

C.Kr

D. Xe

5 The electron affinity of chlorine may be represented by the equation
6 The bond angle H - O - H in ice ins closest to

A. 120° , 28'

B. 60°

C.90°

D. 109°

7 Which of the hydrogen halides has the highest percentage of ionic character

A. HCl

B. HBr

C.HF

D. HI

8 Generally the bond formed by metals with non-metals is

A. Ionic

B. Covalent

C.Polar

D. Non- polar

9 SnCI2have ______ shape

A. Planner

B. Tetrahedral

C.Angular

D. None

10 Mg becomes isoelectronic with neon when it

A. Loses two electrons

B. Gains two electrons

C.Loses 1 electron

D. Gains 1 electron

11 Which of the following has zero depole-moment?

A. CIF

B. PCl3

C.SiF4

D. CFCl4

12 The structure of ICI2is

A. Trigonal

B. Trigonal bipyramidal

C.Octahedral

D. Square planar

13 The most suitable method of the separation of a mixture of ortho and para-nitrophenol mixed in the ratio of 1: 1 is

A. Distrillation

B. Crystallization

C.Vapourisation

D. Colour spectrum

14 Outer shells of two elements X and Y have two and six electrons respectively. If they combine, the expected formula of compound will be

A. XY

B. X2Y

C.X2Y3

D. XY2

15 N-atom forms three covalent bonds, its electronic configuration is
16 Which of the following molecules have sp3hybridized carbon

A. CH4

B. C2H4

C.C2H2

D. CO2

17 Antibonding MO is formed by

A. Addition of atomic orbitals

B. Substraction of atomic orbitals

C.Multiplication of atomic orbitals

D. None of these

18 Size of an anion is increased as compared to its atom because of the

A. Addition of new shell

B. Repulsion of electrons in the valence shell

C.Decrease in nuclear charge

D. Increase in the unclear charge

19 Which carbon is more electronegative?

A. sp3- hybridized carbon

B. sp-hybridized carbon

C.sp2-hybridized carbon

D. always same irrespective of its hybrid state

20 An ionic compound M2S3is formed by the metal M,, the metal is

A. Ca

B. Ba

C.K

D. Al

21 In a group the atomic size increase downward due to

A. Addition of electronic shells

B. Increase in the proton number

C.Repulsion of electrons

D. All of the above

22 Water H2O is liquid while hydrogen sulphide H2S is a gas beause

A. Water has higher molecular weight

B. Hydrogen sulphide is a weak acid

C.Sulphure has high electronegativity than oxyhe

D. Water molecules associate through hydrogen bonding

23 The number of antibonding electron pairs in O2-molecular ion on the basis of MOT is

A. 4

B. 3

C.2

D. 5

24 Which of the following is a polar molecules

A. Carbon dioxide

B. Carbon tetrachloride

C.Methanol

D. Ethane

25 Coordinate covalent bond is present in the molecules

A. H2O

B. BF3

C.SiO2

D. SO2

26 Which of the following has highest bond order
27 When two hydrogen atoms approach to form a chemical bond

A. The repulsive forces dominate the attractive forces

B. The attractive forces, dominate the repulsive forces

C.The energy of atoms increases

D. The two atoms start ionization

28 The number of electron pairs shared in carbon tetrachloride molecule is

A. 2

B. 3

C.4

D. 1

29 From the difference between expected bond energies for the normal covalent bond and experimentally determined values Pauling calculated the values of

A. Ionization potential of elements

B. Electron affinity of elements

C.Electronegativity of elements

D. Bond length

30 Which of the following molecules have multiple bonds

A. CH4

B. C2H4

C.C2H6

D. CCI4

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