Chemical Bonding

Compound X consists of molecule.

(i) Bonding in X will be:

A: ionic
B: electrovalent
C: covalent
D: molecular

Answer

Covalent
Reason — As compound X consists of molecules, it means that compound X is a covalent compound. Electrovalent compounds consist of ions. Hence, bonding in X is covalent.

State what is the term defined in:- a bond formed by shared pair of electrons each bonding atom contributing one electron to the pair.

Answer

Single covalent bond

The molecule which contains a triple covalent bond is:

A: ammonia
B: methane
C: water
D: nitrogen

Answer

Nitrogen
Reason — As the electronic configuration of N is [2,5] so when two nitrogen atoms come closer, each contributes three electrons and they have three shared pair of electrons between them. Therefore, it forms triple covalent bond [N ≡ N].

State what is a lone pair of electrons.

Answer

Lone pair of electrons are valence electrons that in a covalent bond are not shared with another atom.

The electronic configuration of nitrogen is 2,5. How many electrons in the outer shell of a nitrogen atom are not involved in the formation of a nitrogen molecule.

Answer

Nitrogen has 5 electrons in its valence shell. In the formation of a nitrogen molecule, each nitrogen atom shares three electrons to complete its octet. Hence, 2 electrons in the outer shell of each nitrogen atom are not involved in bond formation. Formation of a nitrogen molecule from nitrogen atoms is shown in the diagram below:

Draw the atomic orbit structure of carbon tetrachloride and state the type of bond present in it.

Answer

Atomic orbit structure of carbon tetrachloride is shown below:

Type of bond present in carbon tetrachloride is Covalent Bond

Choose the answer -

(i) Sodium chloride — covalent bond/ionic bond/covalent & coordinate bond.

(ii) Carbon tetrachloride — covalent bond/ionic bond/covalent and coordinate bond.

Answer

(i) Sodium chloride — ionic bond.

(ii) Carbon tetrachloride — covalent bond.

(i) In covalent compounds, the bond is formed due to ............... [sharing/transfer] of electrons.

(ii) A molecule of ............... contains a triple bond. [hydrogen/ammonia/nitrogen]

Answer

(i) In covalent compounds, the bond is formed due to sharing of electrons.

(ii) A molecule of nitrogen contains a triple bond.

State the bonding in methane molecule.

Answer

Methane consists of one carbon atom [2,4] and four hydrogen atoms [1]. Carbon needs four electrons to attain a stable electronic configuration of nearest noble gas - Ne, whereas, hydrogen needs one electron to attain stable electronic configuration of nearest noble gas - He.

Therefore, one atom of carbon shares four electron pairs one with each of the four hydrogen atoms, resulting in formation of methane molecule.

The atomic orbit structure diagram of the formation of methane molecule is shown below:

Name -

(a) an atom with electronic configuration 2, 8, 6

(b) A gaseous covalent molecule with four covalent bonds.

Answer

(a) An atom with electronic configuration 2, 8, 6 is Sulphur.

(b) A gaseous covalent molecule with four covalent bonds is Methane

Define the term 'chemical bond' and 'chemical bonding'.

Answer

The force which acts between two or more atoms to hold them together as a stable molecule is called a chemical bond and the concept is called chemical bonding.

Give a reason why noble gases have stable electronic configuration while atoms of other elements have unstable electronic configuration.

Answer

Octet and duplet structures seem to represent stability and are said to be stable electronic configuration.

Noble gases have their outermost or valence shell complete i.e., they have 2 electrons in outermost shell e.g., helium [electronic configuration 2] or they have 8 electrons in outermost shell e.g., neon [electronic configuration 2,8] or argon [electronic configuration 2,8,8 ]. Hence, they have stable electronic configuration. They do not gain, lose or share electrons and are unreactive or inert.

Atoms of other elements have incomplete valence shell, hence they have unstable electronic configuration. So, they can gain, lose or share electrons to attain the stable electronic configuration of the nearest noble gas.

State how atoms of other elements other than noble gases, attain stable electronic configuration of the nearest noble gas.

Answer

Atoms of elements other than noble gases, attain stable electronic configuration of the nearest noble gas by:

1. Transfer of valence electrons from a metallic atom to a non-metallic atom.
2. Mutual sharing of electrons between two pairs of atoms of non-metallic elements.

Define each of the following terms -

(a) electrovalent bond

(b) electrovalent compound

(c) covalent bond

(d) covalent compound

with suitable examples wherever required.

Answer

(a) The chemical bond formed between the two atoms by transfer of one or more electrons from the atom of a metallic element to an atom of a non-metallic element is called an electrovalent bond.

(b) The chemical compound formed as a result of transfer of one or more electrons from the atom of a metallic element to an atom of a non-metallic element is called an electrovalent compound. e.g., NaCl, CaO

(c) The chemical bond formed due to mutual sharing of electrons between the given pairs of atoms of non-metallic elements is called a covalent bond.

(d) The chemical compound formed due to mutual sharing of electrons between the given pair of non-metallic elements is called a covalent compound. e.g., Chlorine molecule, Oxygen molecule.

State what is meant by - (a) duplet rule (b) octet rule.

Answer

(a) Duplet Rule — For an atom to achieve stable electronic configuration it must have 2 electrons in the first shell [outermost] like that of noble gas Helium.

(b) Octet Rule — For an atom to achieve stable electronic configuration it must have 8 electrons in outermost orbit like that of noble gases other than Helium.

Sodium chloride is formed as a result of - transfer of electrons from metallic sodium atom to non-metallic chlorine atom. With the help of atomic orbit structure diagram - show the formation of sodium chloride [Atomic numbers: Na = 11, Cl = 17].

Answer

Atomic orbit structure diagram of the formation of sodium chloride by transfer of electrons from metallic sodium atom to non-metallic chlorine atom is shown below:

Atomic number of calcium is 20 and of oxygen is 8. State the number of electrons - calcium loses and oxygen gains to attain stable electronic configuration of the nearest noble gas - during formation of electrovalent molecule, calcium oxide.

Answer

Calcium oxide is formed as a result of transfer of two valence electrons

• from metallic calcium atom ⁴⁰₂₀Ca; electronic configuration - 2,8,8,2 ; Nearest noble gas = Argon [2,8,8]
• to non-metallic oxygen atom ¹⁶₈O - electronic configuration - 2,6 ; Nearest noble gas = Neon [2,8]
• calcium loses two electrons - from its outer shell to attain stability of nearest noble gas - argon and becomes a calcium ion [cation] : Ca²⁺
• oxygen accepts two electrons - in outer shell to attain stability of nearest noble gas - neon and becomes an oxide ion [anion] : O^2-

Explain with the help of atomic orbit structure diagram the formation of calcium oxide.

Answer

Atomic orbit structure diagram of the formation of calcium oxide is shown below:

Calcium oxide is formed as a result of transfer of two valence electrons

• from metallic calcium atom ⁴⁰₂₀Ca; electronic configuration - 2,8,8,2 ; Nearest noble gas = Argon [2,8,8]
• to non-metallic oxygen atom ¹⁶₈O - electronic configuration - 2,6 ; Nearest noble gas = Neon [2,8]
• calcium loses two electrons - from its outer shell to attain stability of nearest noble gas - argon and becomes a calcium ion [cation] : Ca²⁺
• oxygen accepts two electrons - in outer shell to attain stability of nearest noble gas - neon and becomes an oxide ion [anion] : O^2-

Give a reason why - in the formation of electrovalent compound - magnesium chloride, one magnesium atom combines with two chlorine atoms to give magnesium chloride. [at. no. Mg=12, Cl=17, ]

Answer

Magnesium [At. no. 12 and electronic configuration 2,8,2] loses two electrons from it's outer shell in order to attain stability of nearest noble gas Neon [2,8] and becomes a magnesium ion [cation] : Mg²⁺.

Chlorine [At. no. 17 and electronic configuration 2,8,7] accepts one electron in it's outer shell to attain stability of nearest noble gas Argon [2,8,8] and becomes a chloride ion [anion] : Cl^1-.

Magnesium atom donates two electrons, whereas chlorine accepts one electron to give - chloride ion. Therefore, to accept the other electron donated by magnesium atom there must be another chlorine atom. Thus, one magnesium atom combines with two chlorine atoms to give MgCl₂

'Formation of hydrogen molecule takes place by sharing of electrons'. Give a reason why the molecule of hydrogen is not formed by transfer of electrons.

Answer

Hydrogen is a non-metal and has 1 valence electron. To attain a stable duplet electronic configuration, each hydrogen atom needs one more electron. As both the combining atoms are one electron short, none of them can donate an electron. Hence, they share one pair of electrons and attain a stable duplet configuration.

Draw the atomic orbit structure diagram for formation of -

(a) hydrogen molecule

(b) chlorine molecule

(c) oxygen molecule

(d) nitrogen molecule

[at. no. H=1, Cl=17, O=8, N=7]

Answer

(a) Atomic orbit structure diagram for formation of hydrogen molecule is shown below:

(b) Atomic orbit structure diagram for formation of chlorine molecule is shown below:

(c) Atomic orbit structure diagram for formation of oxygen molecule is shown below:

(d) Atomic orbit structure diagram for formation of nitrogen molecule is shown below:

Give reasons for formation of single covalent bond between two chlorine atoms and a double covalent bond between two oxygen atoms - during formation of respective covalent molecules.

Answer

Atomic number of Cl is 17 and elect. config. is [2,8,7]. As both the Cl atoms require one electron to complete it's octet, hence, they both will share 1 electron and will attain a stable electronic configuration of the nearest noble gas — argon. Therefore, single covalent bond is formed during formation of a chlorine molecule.

Atomic number of O is 8 and elect. config. is [2,6]. As both the O atoms require two electrons to complete their octet, hence, they both will share 2 electrons and will attain a stable electronic configuration of the nearest noble gas — neon. Therefore, double covalent bond is formed during formation of a oxygen molecule.

Draw the atomic orbit structure diagram for formation of a -

(a) water molecule

(b) ammonia molecule

[at. no. H=1, O=8, N=7]

Answer

(a) Atomic orbit structure diagram for formation of water molecule is shown below:

(b) Atomic orbit structure diagram for formation of ammonia molecule is shown below:

With the help of an atomic orbit structure diagram - explain the formation of :

(a) carbon tetrachloride

(b) methane

[at. no. : C=6, Cl=17, H=1]

Answer

(a) Atomic orbit structure diagram for formation of carbon tetrachloride molecule is shown below:

(b) Atomic orbit structure diagram for formation of methane molecule is shown below:

Explain the formation of a radical from a covalent bond with an example.

Answer

Radical formation occurs when a covalent bond breaks symmetrically, with each atom retaining one electron of the shared pair. This results in the formation of two radicals. The process is called bond fission and is initiated by light, heat or certain chemicals.

A—B $\xrightarrow{\text{light energy}}$ A● + B●

Assertion: Noble gases have stable electronic configuration.

Reason: Atoms of elements other than noble gases have incomplete valence shell.

1. Both A and R are true and R is the correct explanation of A.
2. Both A and R are true but R is not the correct explanation of A.
3. A is true and R is false.
4. A is false and R is true.

Answer

Both A and R are true but R is not the correct explanation of A.

Reason — A is true as noble gases have completely filled valence shells making them chemically stable.
R is true as except noble gases, other elements do not have completely filled outermost shells.

Therefore, Both A and R are true but R is not the correct explanation of A is the correct option.

An element 'X' has same number of electrons in its first & in its outermost shell. The electronic configuration of X²⁺ is :

1. 2, 8, 1
2. 2, 8
3. 2, 8, 2
4. 2, 8, 8

Answer

Both 2,8 and 2,8,8 can be correct.

Reason — The first shell can have a maximum of 2 electrons. Since element X has the same number of electrons in its first shell and in its outermost shell, its outermost shell also contains 2 electrons.

Thus, X may have electronic configuration:

• 2,8,2 — on losing 2 electrons, X²⁺ becomes 2,8
• 2,8,8,2 — on losing 2 electrons, X²⁺ becomes 2,8,8

Hence, both 2,8 and 2,8,8 are possible electronic configurations of X²⁺. Therefore, the question has two correct options unless the atomic number or period of element X is specified.

An element 'A' needs 4 electrons to attain stable electronic configuration of the nearest noble gas — Neon. An element 'B' needs 1 electron to attain stable electronic configuration of the nearest noble gas — Argon.
The covalent compound formed between A & B is :

1. AB₃
2. A₄B
3. A₂B₄
4. AB₄

Answer

AB₄

Reason — Electronic configuration of A = 2, 4
Element A needs 4 electrons to attain Neon configuration as it has 4 valence electrons. Therefore, valency of A = 4.

Electronic configuration of B = 2, 8, 7
Element B needs 1 electron to attain Argon configuration as it has 7 valence electrons. Therefore, valency of B = 1.

$\overset{\phantom{4}{4}}{\text{A}} \space {\searrow}\mathllap{\swarrow} \space \overset{1}{\text{B}} \Rightarrow \underset{\phantom{1}{1}}{\text{A}} \space {\searrow}\mathllap{\swarrow} \space \underset{4}{\text{B}} \\[0.5em]$

AB₄ is the correct formula.

State why water has two lone pairs of electrons in it's covalent molecule, ammonia has one lone pair & methane has no lone pairs in its molecule.

Answer

Water contains two hydrogen atoms and one oxygen atom. The hydrogen atom [1] has one electron in it's valence shell while the oxygen atom [2,6] has 6 electrons in it's valence shell. Two hydrogen atom share one electron each and two unshared pairs of electrons are left as lone pairs as shown in the diagram below :

In the case of ammonia, it contains three hydrogen atoms and one nitrogen atom. Nitrogen atom [2,5] has five valence electrons and hydrogen atom [1] has one valence electron. In ammonia, each of the three hydrogen atoms are bonded to the nitrogen atom by a pair of shared electrons. Thus, the nitrogen atom in ammonia is left with one lone pair of electrons as shown in the diagram below:

In methane, carbon has 4 valence electrons. All four electrons are used in forming four covalent bonds with hydrogen atoms, so no electrons remain unshared. Hence, methane has no lone pairs.

Name the following:

1. An electrovalent compound formed by transfer of one electron from a metallic atom to a non-metallic atom.
2. A covalent hydrocarbon molecule, having four single covalent bonds.
3. A covalent molecule, having two lone pair of electrons.
4. A covalent molecule having a triple covalent bond.
5. A covalent molecule having two shared pairs of electrons in its molecule.

Answer

1. Sodium chloride [NaCl]
2. Methane [CH₄]
3. Water [H₂O]
4. Nitrogen [N ≡ N]
5. Oxygen [O = O]

Give reasons for the following :

To attain stable electronic configuration of the nearest noble gas —

1. Hydrogen atom ¹₁H — needs one electron.
2. Oxygen atom ¹⁶₈O — needs two electrons.
3. Nitrogen atom ¹⁴₇N — needs three electrons.
4. Carbon atom ¹²₆C — needs four electrons.
5. Chlorine atom ³⁵₁₇Cl — needs one electron.

Answer

1. As the atomic number of H is 1 and its electronic configuration is 1, it needs one electron to attain the nearest noble gas He configuration, i.e. 2 electrons in the first shell (duplet rule).
2. As the atomic number of O is 8 and its electronic configuration is 2,6, it needs two electrons to attain the nearest noble gas Ne configuration, i.e. 8 electrons in the valence shell (octet rule).
3. As the atomic number of N is 7 and its electronic configuration is 2,5, it needs three electrons to attain the nearest noble gas Ne configuration, i.e. 8 electrons in the valence shell (octet rule).
4. As the atomic number of C is 6 and its electronic configuration is 2,4, it needs four electrons to attain the nearest noble gas Ne configuration, i.e. 8 electrons in the valence shell (octet rule).
5. As the atomic number of Cl is 17 and its electronic configuration is 2,8,7, it needs one electron to attain the nearest noble gas Ar configuration, i.e. 8 electrons in the valence shell (octet rule).

Complete the table given below, pertaining to formation of covalent compounds :

Answer

Differentiate between the following with a suitable example :

Lone pair & shared pair of electrons.

Answer

Differentiate between the following with a suitable example :

Duplet rule & octet rule.

Answer

Differentiate between the following with a suitable example :

Stable electronic configuration & unstable configuration.

Answer

Differentiate between the following with a suitable example :

Electrovalent bond & covalent bond

Answer

Differentiate between the following with a suitable example :

Single covalent bond & triple covalent bond.

Answer

Atomic numbers of the following elements are given below:

A = 8; B = 7; C = 17; D = 11; E = 20

1. State which of the above is a divalent metal.
2. State which of the above is a non-metal.
3. State the type of bonding between two atoms of 'A'.
4. State the type of bonding between 'D' & 'C'.
5. State the number of covalent bonds formed in a molecule of 'B₂'.

Answer

1. E is a divalent metal as it has 2 electrons in the valence shell [electronic configuration 2,8,8,2] and it tends to lose two electrons in order to gain a stable octet configuration.
2. C is a non-metal as it's electronic configuration is 2,8,7 and it tends to gain one electron to attain a stable state.
3. Double covalent bond as the electronic configuration of A is 2,6 [non-metal], both A atoms will try to gain 2 electrons to attain a stable octet and none of the combining atoms are in a position to donate. Hence, they form the bond by sharing of 2 valence electrons and form a double covalent bond.
4. Electrovalent bond as the elect. configuration of D = [2,8,1] and C = [2,8,7], hence, D donates one electron and becomes a cation whereas C takes up one electron and becomes an anion. The attractive force between a cation and anion results in formation of an electrovalent bond.
5. Triple covalent bond as the electronic configuration of B is [2,5], hence, B needs 3 electrons to attain a stable octet configuration and hence forms a triple covalent bond.

The representation below shows the outline formation of an electrovalent compound.

If the atomic number of element 'X' is 11 and of element 'Y' is 17 —

1. State why an electron is transferred from 'X' to 'Y' during the formation of 'X Y'
2. Give a reason why electrons are not shared between 'X' & 'Y' — during the formation of 'XY'
3. State the difference between 'X' and 'X¹⁺'
4. Does 'Y^1-' have a stable or an unstable electronic configuration.
5. If a compound is formed from atom A [at. no.19] and an atom Y [at. no. 17], would the compound 'AY' be an electrovalent or covalent compound. Give reasons.

Answer

1. As the electronic configuration of X is [2,8,1] and Y is [2,8,7], hence X donates one electron and Y accepts one electron in order to attain stable octet configuration. Hence, electron is transferred from X to Y.
2. Sharing of electrons mainly takes place between a pair of non-metals and as X [2,8,1] is a metal and Y is a non-metal [2,8,7]. Hence, electrons are not shared between 'X' & 'Y' during the formation of 'XY'
3. X is an atom and has no charge, whereas X¹⁺ is a cation and has a unit positive charge.
4. Y^1- has a stable electronic configuration [i.e., 2,8,8] as there are 8 electrons in the valence shell.
5. Electronic configuration of A is [2,8,8,1] and Y is [2,8,7], Hence, A is a metal and Y is a non-metal. Therefore, there will be transfer of 1 valence electron from A to Y and the compound formed will be an electrovalent compound.