Chemical Bonding and Molecular Structure Test -1

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Chemical Bonding and Molecular Structure Test -1

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Weekly Quiz Competition

Question 1
1 / -0

For N₂, bond order is

A
2

B
1

C
4

D
3

Solution

Explanation:

Bond order is the number of chemical bonds between a pair of atoms. in diatomic nitrogen N≡N, Triple covalent bond is present in nitrogen so the bond order is 3.
Question 2
1 / -0

The amount of energy required to break one mole of bonds of a particular type between two atoms in a gaseous state is called

A
ionization enthalpy

B
bond enthalpy

C
lattice enthalpy

D
Electron affinity

Solution

Explanation:

Bond enthalpy, also known as bond energy, is the energy that is needed to break a particular bond in a gaseous compound. The unit that expresses bond enthalpy is kilojoules per mole, or kJ/mol.
Question 3
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Bond angle helps us in

A
determining molecular size

B
determining the stability of the element

C
determining the reactivity of the element

D
determining molecular shape

Solution

Explanation:

Bond angles also contribute to the shape of a molecule. Bond angles are the angles between adjacent lines representing bonds. The bond angle can help differentiate between linear, trigonal planar, tetraheral, trigonal-bipyramidal, and octahedral. The ideal bond angles are the angles that demonstrate the maximum angle where it would minimize repulsion, thus verifying the VSEPR theory.
Question 4
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bond lengths are lower in elements having

A
double bond

B
single bond

C
triple bond

D
crystal structure

Solution

Explanation:

The bond length depends on the strength of the bond. The stronger the bond is, the shorter it will be. The triple bonds are the strongest and hence the shortest. Then comes double bonds which are of intermediate strength between the triple and single bonds. And finally the single bonds are weaker than the other two. This way, Triple bonds are the shortest. Then comes double bonds. Finally, single bonds are the longest among the three.

The order of bond lengths is given as, Triple bond < Double bond < Single bond
Question 5
1 / -0

A qualitative measure of the stability of an ionic compound is provided by

A
electron gain enthalpy

B
ionization enthalpy

C
Electron affinity

D
lattice enthalpy

Solution

Explanation:

Lattice energy is an estimate of the bond strength in ionic compounds. It is defined as the heat of formation for ions of opposite charge in the gas phase to combine into an ionic solid.

The stability of ionic bond is directly propotional to lattice energy.
Question 6
1 / -0

The formation of the Cl₂molecule can be understood in terms of the sharing of a pair of electrons between the two chlorine atoms, each chlorine atom contributing one electron to the shared pair. Choose the most appropriate name of the bond that is formed

A
ionic bond

B
multiple bond

C
a single covalent bond

D
double bond

Solution

Explanation:

Two chlorine atoms will each share one electron to get a full outer shell and form a stable Cl₂ molecule.

By sharing the two electrons where the shells touch each chlorine atom can count 8 electrons in its outer shell. These full outer shells with their shared electrons are now stable and the Cl₂ molecule will not react further with other chlorine atoms. One pair of shared electrons form a single covalent bond.
Question 7
1 / -0

The number of dots around the Lewis symbols for the elements represent

A
group valence of the element

B
electrovalency

C
the number of valence electrons of the element

D
coordinate valency

Solution

Explanation:

Gilbert N. Lewis is widely known for his use of simple symbolic representations of elements that show valence electrons as dots.

The Lewis electron-dot symbols focus on the electrons in the highest principal energy level in the atom, the valence electrons.

After all, these are the electrons that participate in chemical reactions. Lewis electron-dot symbols work well for the representative elements.
Question 8
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The bond formed, as a result of the electrostatic attraction between the positive and negative ions was termed as

A
single covalency

B
covalent bond

C
electrovalent bond

D
coordinate bond

Solution

Explanation:

Chemical bond formed between two atoms due to transfer of electron(s) from one atom to the other. atom is called "Ionic bond" or "electrovalent bond".

in electrovalent bond one atom loses an electron to form a positive ion and the other atom gains the electron to form a negative ion. The resulting ions are held together by electrostatic attraction
Question 9
1 / -0

Stable outer octet of electrons is achieved in chlorine atom during the formation of NaCl by:

A
The formation of a coordinate bond

B
The loss of an electron

C
The formation of a hybrid orbital

D
The gain of an electron

Solution

Explanation:

Na lose its one electron forming Na⁺ while Cl gains the electron formimg Cl^-
Question 10
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By the axial overlapping of two p-orbitals of the same energy, a strong sigma bond is formed.

A
True

B
False

C

Ambiguous

D
None of these

Solution

Sigma bond is formed by the linear or head to head or end on overlapping of orbitals. Sigma bonds are the strong bonds due to maximum overlapping of orbitals. Electron density is maximum around the bond axis. Therefore the axial overlapping of two p-orbitals of the same energy results in a strong sigma bond.

Hence, the correct option is $$\text{A}$$
Question 11
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The number of lone pairs of electron on $$Xe$$ in $$XeO{F}_{4}$$ is:

A
$$1$$

B
$$2$$

C
$$3$$

D
$$4$$

Solution

The number of lone pairs of electron on $$Xe$$ in $$XeO{F}_{4}$$ is 1. $$Xe$$ in $$XeO{F}_{4}$$ has $${ sp }^{ 3 }{d}^{2}$$-hybridization having one lone pair on $$Xe$$-atom and is square pyramidal in shape.
Question 12
1 / -0

The ratio of lone pair and bond pair electrons on central $$I$$ atom in $${I}_{3}^{-}$$:

A
$$1$$

B
$$1.5$$

C
$$0.6$$

D
$$0.5$$

Solution

The ratio of lone pair and bond pair electrons on central $$I$$ atom in $${I}_{3}^{-}$$ is $$1.5$$.
Thus, No. of lone pair of electrons $$=3$$
No. of bond pair of electrons $$=2$$
The ratio of lone pair and bond pair electrons $$= 3/2 = 1.5$$
Question 13
1 / -0

Number of bond pair and lone pair of electrons in $${OF}_{2}$$ are:

A
$$2,6$$

B
$$2,8$$

C
$$2,10$$

D
$$1,9$$

Solution

Number of bond pair and lone pair of electrons in $$OF_2$$ are $$2,8$$.
Question 14
1 / -0

Calculate the steric numbers for iodine in $$(IF_4^-)$$ and for bromine in $$(BrO_4^-)$$.

A
$$6$$ and $$4$$

B
$$5$$ and $$6$$

C
$$4$$ and $$6$$

D
$$3$$ and $$4$$

Solution

The central $$I^-$$ has eight valence electrons
Each $$F$$ atom has seven valence electrons of its own and needs to one of the electrons from $$I^-$$ to attain noble-gas configuration $$(s^2p^6)$$. Thus, four, of the $$I^-$$ valence electrons take part in covalent bonds, leaving the remaining four to form two lone pairs. Thus,
$$S_N =$$ 4 (bonded atoms) + 2 (lone pairs) $$= 6$$
The central $$Br^-$$ has also eight electrons. In $$BrO_4^-$$, each oxygen atom needs to share two of electrons from $$Br^-$$ to attain noble-gas configurations thus all the electrons are used in bonding and no lone pair exists.
Thus, $$S_N = $$ 4 (bonded pair) + 0 (lone pairs) $$=4$$.
Question 15
1 / -0

In the cyanide ion the formal negative charge is on:

A
$$C$$

B
$$N$$

C
both $$C$$ and $$N$$

D
resonate between $$C$$ and $$N$$

Solution

In the cyanide ion the formal negative charge resonates between $$C$$ and $$N$$. Cyanide ion has resonating structure, $$-\overset { \_ }{ C } \equiv N\longleftrightarrow \overset { \_ }{ N } \underrightarrow { = } C$$
Question 16
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What is the value of $$1D$$ in $$SI$$ units ?

A
$$3.336\, \times 10^{-30}\, cm$$

B
$$33.36\, \times\, 10^{-30}\, cm$$

C
$$333.6\, \times\, 10^{-30}\, cm$$

D
None of these

Solution

The debye is a CGS unit of electric dipole moment.
It is defined as $$1 \times 10^{−18}$$ statcoulomb-centimetre and $$ 3.33564\times 10^{−30} C.m$$.
Question 17
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Select the correct statement about chemical bond.

A
It is attraction between atoms

B
It is caused by the electrostatic force of attraction

C
The strength of chemical bonds varies considerably

D
All of the above

Solution

A chemical bond is an attraction between atoms that allows the formation of chemical substances that contain two or more atoms. The bond is caused by the electrostatic force of attraction between opposite charges, either between electrons and nuclei, or as the result of a dipole attraction.
Question 18
1 / -0

Which of the following has higher bond dipole moment ?

A
$$H-C$$

B
$$N-O$$

C
$$P-H$$

D
None of these

Solution

Higher Bond dipole moment
a) $$H-C=(2.20-2.55)=0.35$$
b) $$N-O=(3.04-3.44)=0.40$$
c) $$P-H=(2.19-2.20)=0.10$$
Higher the difference in electro negativity between the two atoms, higher the dipole moment.
The higher dipole is found in NO. Here bond dipole moment is 0.40
Question 19
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Which of the following species has four lone pairs of electrons in its outer shell ?

A
$$I$$

B
$$O^-$$

C
$$Cl^-$$

D
$$He$$

Solution

Consider the electronic configuration of each of these options:-

A) $$ I $$ - $$ [Kr] 4d^{10} 5s^2 5p^5 \rightarrow$$ 3 lone pairs.

B) $$O^-$$ - $$ 1s^2 2s^2 2p^5 \rightarrow$$ 3 lone pairs.

C) $$Cl^-$$ - $$1s^2 2s^2 2p^6 3s^2 3p^6\rightarrow$$ 4 lone pairs.

D) $$He$$ - $$ 1s^2\rightarrow$$ 1 lone pair.

Hence option C is the right answer.

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Chemical Bonding and Molecular Structure Test -1

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Question 1

2

1

4

3

Solution

Question 2

ionization enthalpy

bond enthalpy

lattice enthalpy

Electron affinity

Solution

Question 3

determining molecular size

determining the stability of the element

determining the reactivity of the element

determining molecular shape

Solution

Question 4

double bond

single bond

triple bond

crystal structure

Solution

Question 5

electron gain enthalpy

ionization enthalpy

Electron affinity

lattice enthalpy

Solution

Question 6

ionic bond

multiple bond

a single covalent bond

double bond

Solution

Question 7

group valence of the element

electrovalency

the number of valence electrons of the element

coordinate valency

Solution

Question 8

single covalency

covalent bond

electrovalent bond

coordinate bond

Solution

Question 9

The formation of a coordinate bond

The loss of an electron

The formation of a hybrid orbital

The gain of an electron

Solution

Question 10

True

False

Ambiguous

None of these

Solution

Question 11

$$1$$

$$2$$

$$3$$

$$4$$

Solution

Question 12

$$1$$

$$1.5$$

$$0.6$$

$$0.5$$

Solution