Atomic Bonding Test

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Atomic Bonding Test - 6

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Weekly Quiz Competition

Question 1
1 / -0

Which of the following correctly represents the electron dot structure of oxygen molecule?

A

B

C

D

Solution

The correct electron dot structure of oxygen molecule is given in option (4).
Question 2
1 / -0

In which of the following is expanded octet present?

A
NH₃

B
PF₅

C
H₂O

D
O₂

Solution

Expanded octet is formed between that compounds which have more than eight electrons in the valence shell around a central atom. Compounds with expanded octets around the central atoms of elements are in the third period and beyond. For example, phosphorus commonly forms stable molecules and ions in which phosphorus is surrounded by more than an octet of valence electrons. Due to its large size, phosphorus as a central atom can violate the octet rule to form PF₅ and PF₆^-.
Question 3
1 / -0

Which of the following types of bonds is the weakest?

A
Ionic bond

B
Metallic bond

C
Hydrogen bond

D
Covalent bond

Solution

A hydrogen bond is formed by attractive force between the hydrogen attached to an electronegative atom of one molecule and an electronegative atom of a different molecule. Thus, because it is formed by attractive force thus ia a weakest bond.
Question 4
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Whenever a chemical bond is formed, there is

A
a decrease in energy of the system

B
an increase in energy of the system

C
no loss or gain of energy

D
none of these

Solution

Whenever a chemical bond is formed, there is a decrease in energy of the system.
Question 5
1 / -0

The hybridisation of carbon atom in methane is

A
sp²

B
sp

C
sp³

D
dsp²

Solution

In methane (ground state configuration: 1s², 2s², 2px¹ 2py¹), 1 carbon binds with 4 hydrogens. The carbon atom itself has only 2 electrons available for bonding in the 2p subshell.
In order for 4 hydrogens to bind, one electron of carbon gets excited from the 2s subshell into the 2p subshell, where it is available for bonding. Thus, a new 'hybridised orbital' called sp³ is formed.
Question 6
1 / -0

Two atoms in the nitrogen molecule are joined by

A
one sigma and one pi bond

B
one sigma bond

C
one sigma and two pi bonds

D
two sigma and one pi bond

Solution

Two atoms in the nitrogen molecule have three bonds between them and are joined by one sigma and two pi bonds.
Question 7
1 / -0

What is the total number of and bonds in C₂H₂?

A
0 and 4

B
2 and 2

C
3 and 2

D
4 and 2

Solution

Acetylene is formed by three sigma and two pi bonds.
Question 8
1 / -0

Which of the following substances possesses the weakest electrostatic forces of attraction?

A
HCl

B
NaCl

C
NO

D
Cl₂

Solution

From the above given substances chlorine molecule is formed by the weakest electrostatic forces of attraction.
Question 9
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Which of the following is not a correct difference between electrovalent and covalent compounds?

A
Electrovalent compounds have strong electrostatic forces of attraction whereas covalent compounds have weak electrostatic forces of attraction.

B
Electrovalent compounds are volatile whereas covalent compounds are non-volatile.

C
Electrovalent compounds are good conductors of electricity whereas covalent compounds are non-conductors.

D
Electrovalent compounds are soluble in water whereas covalent compounds are insoluble in water.

Solution

The option (2) is incorrect. Because, electrovalent compounds are non-volatile in nature whereas covalent compounds are volatile in nature.
Question 10
1 / -0

How many covalent bonds are present in an ammonia molecule?

A
4

B
3

C
2

D
1

Solution

An ammonia molecule is formed by three covalent bonds. For example:
Question 11
1 / -0

How many lone pairs are there in a molecule of ammonia?

A
1

B
2

C
3

D
0

Solution

A molecule of ammonia has one lone pairs of electrons. For example:
Question 12
1 / -0

The covalency of 'N' in NH₄⁺ ion is equal to number of _________

A
covalent bonds

B
valence bonds

C
ionic bonds

D
covalent and co-ordinate bonds

Solution

The covalency of 'N' in NH₄⁺ ion is equal to number of covalent and co-ordinate bonds.
Question 13
1 / -0

How many electrons are present in the valence shell of the central atom in the molecule of BF₃?

A
1

B
2

C
3

D
0

Solution

The electon configuration of boron is 1s², 2s², 2p¹and three electron in its valence shell. Thus due to three electrons in its valence shells of the central atom it form BF₃ molecule.
Question 14
1 / -0

Which of the following covalent compounds can conduct electricity?

A
NH₃

B
CCl₄

C
CH₄

D
Cl₂

Solution

Electrolyte is a solution and a medium that consists of free ions which help in the conduction of electricity. Ammonia in water is an example for weak electrolyte. It exists as molecule in water and to some extent get dissociated as ion. Since the weak electrolytes have fewer ions in the solution, it acts as weak conductor of electricity.
Question 15
1 / -0

What kind of bond is formed between elements X and Y, if X has low ionization energy and Y has electron affinity?

A
Ionic

B
Polar covalent

C
Co-ordinate covalent

D
Non-polar covalent

Solution

Ionic bond is formed when atoms of an element (usually metal), whose ionization energy is low, release some of their electrons to achieve a stable electron configuration. In doing so, cations are formed. The atom of another element (usually non-metal), whose electron affinity is positive, then accepts the electron(s), again to attain a stable electron configuration, and after accepting electron(s) the atom becomes an anion.
Question 16
1 / -0

Which of the following is an ionic hydride?

A
MgH₂

B
SiH₄

C
BH₃

D
PH₃

Solution

MgH₂ is an ionic hydride because hydride formed by alkali metals are known as ionic hydride.
Question 17
1 / -0

Which of the following is not an ionic compound?

A
CaF₂

B
CH₄

C
KCl

D
MgO

Solution

Metals can form ionic hydride by the lose of electrons. But CH₄ is a covalent molecule as it is formed by only sharing of electrons.
Question 18
1 / -0

Which of the following is a good conductor of electricity?

A
NaCl (s)

B
MgCl₂(aq)

C
CH₄(g)

D
Cl₂(g)

Solution

Covalent bonds are formed by sharing of electrons. They do not have a free electron that is required for electricity transfer (electricity is the flow of free electrons. Thus, they are bad conductors of electricity, e.g. CH₄ and Cl₂.
Whereas, ionic compounds are good conductors of electricity only in molten state and in their aqueous solutions. This is because in molten state/aqueous solution, the free ions move around freely and conduct electricity, e.g. MgCl₂(aq).
Moreover, NaCl(s) is an ionic compound but is a bad conductor because it is in its solid state as the ions are not free to move.
Question 19
1 / -0

Which of the following is a polar compound?

A
CCI₄

B
CH₄

C
HCI

D
C₂H₆

Solution

Polar compound is a compound in which the electric charge is not symmetrically distributed, so that there is a separation of charge or partial charge and formation of definite positive and negative poles, H₂O and HCl.
Question 20
1 / -0

Which of the following correctly explains the reason for lesser covalency of FeCl₂ over FeCl₃?

A
Lower polarizing power of Fe⁺²than that of Fe⁺³ ion.

B
Lower polarizing power of Fe⁺³ than that of Fe⁺².

C
Higher polarizability of Fe⁺² than that of Fe⁺³ ion.

D
Co-ordinate bonding of FeCl_3.

Solution

In FeCl₃, Fe exist in +3 state as Fe³⁺ cation while in FeCl₂, Fe exist in +2 state as Fe²⁺ cation. As we know greater the charge greater will be the covalent nature. Thus, in Fe³⁺cation, due to the greater charge greater will be the polarizibility and so it has more covalent character. Hence, FeCl₃ has more covalent character than in FeCl₂.

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Atomic Bonding Test - 6

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Atomic Bonding Test - 6

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Question 1

Solution

Question 2

NH3

PF5

H2O

O2

Solution

Question 3

Ionic bond

Metallic bond

Hydrogen bond

Covalent bond

Solution

Question 4

a decrease in energy of the system

an increase in energy of the system

no loss or gain of energy

none of these

Solution

Question 5

sp2

sp

sp3

dsp2

Solution

Question 6

one sigma and one pi bond

one sigma bond

one sigma and two pi bonds

two sigma and one pi bond

Solution

Question 7

0 and 4

2 and 2

3 and 2

4 and 2

Solution

Question 8

HCl

NaCl

NO

Cl2

Solution

Question 9

Electrovalent compounds have strong electrostatic forces of attraction whereas covalent compounds have weak electrostatic forces of attraction.

Electrovalent compounds are volatile whereas covalent compounds are non-volatile.

Electrovalent compounds are good conductors of electricity whereas covalent compounds are non-conductors.

Electrovalent compounds are soluble in water whereas covalent compounds are insoluble in water.

Solution

Question 10

4

3

2

1

Solution

Question 11

1

2

3

0

Solution

Question 12

covalent bonds

valence bonds

ionic bonds

covalent and co-ordinate bonds

Solution

Question 13

1

2

3

NH₃

PF₅

H₂O

O₂

sp²

sp³

dsp²

Cl₂

NH₃

CCl₄

CH₄

Cl₂

MgH₂

SiH₄

BH₃

PH₃

CaF₂

CH₄

MgCl₂(aq)

CH₄(g)

Cl₂(g)

CCI₄

CH₄

C₂H₆

Lower polarizing power of Fe⁺²than that of Fe⁺³ ion.

Lower polarizing power of Fe⁺³ than that of Fe⁺².

Higher polarizability of Fe⁺² than that of Fe⁺³ ion.

Co-ordinate bonding of FeCl_3.