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Chemical Bonding and Molecular Structure

11903 Which of the following hydrides are ionic

1

C a H_{2}

2

B a H_{2}

3

S r H_{2}

4 All of above

Explanation:

(d) $C a H_{2}, B a H_{2}, S r H_{2}$ are ionic hydride.

Chemical Bonding and Molecular Structure

11904 Which of the following conduct electricity in the fused state

1

B e C l_{2}

2

M g C l_{2}

3

B a C l_{2}

4

(b)

and

(c)

Explanation:

(d) Generally $M g C l_{2}, S r C l_{2},$ $B a C l_{2}$ are ionic compounds so they conduct electricity in fused state.

Chemical Bonding and Molecular Structure

11905 The valency of sulphur in sulphuric acid is

1

2

2

4

3

6

4

8

Explanation:

The correct option is $C 6$
The lewis dot structure of Sulphuric acid $(H_{2} S O_{4})$ is:
$S$ forms $6$ covalent bonds with its neighbouring oxygen atoms and hence the valency of $S$ is $6.$ 205-s1

Chemical Bonding and Molecular Structure

11906 The number of electrons involved in the bond formation of $N_{2}$ molecule

1

2

2

4

3

6

4

10

Explanation:

(c) In $N_{2}$ molecule each Nitrogen atom contribute $3 e^{-}$ so total no. of electron’s are $6.$

Chemical Bonding and Molecular Structure

11907 The electronic configuration of four elements are given in brackets $L (1 s^{2}, 2 s^{2} 2 p^{1}); M (1 s^{2}, 2 s^{2} 2 p^{5})$ $Q (1 s^{2}, 2 s^{2} 2 p^{6}, 3 s^{1}); R (1 s^{2}, 2 s^{2} 2 p^{2})$ The element that would most readily form a diatomic molecule is

1

Q

2

M

3

R

4

L

Explanation:

(b) Non-metals readily form diatomic molecules by sharing of electrons. Element $M (1 s^{2} 2 s^{2} 2 p^{5})$ has seven electrons in its valence shell and thus needs one more electron to complete its octet. Therefore, two atoms share one electron each to form a diatomic molecule $(M_{2})$ 205-s3

Chemical Bonding and Molecular Structure

11903 Which of the following hydrides are ionic

1

C a H_{2}

2

B a H_{2}

3

S r H_{2}

4 All of above

Explanation:

(d) $C a H_{2}, B a H_{2}, S r H_{2}$ are ionic hydride.

Chemical Bonding and Molecular Structure

11904 Which of the following conduct electricity in the fused state

1

B e C l_{2}

2

M g C l_{2}

3

B a C l_{2}

4

(b)

and

(c)

Explanation:

(d) Generally $M g C l_{2}, S r C l_{2},$ $B a C l_{2}$ are ionic compounds so they conduct electricity in fused state.

Chemical Bonding and Molecular Structure

11905 The valency of sulphur in sulphuric acid is

1

2

2

4

3

6

4

8

Explanation:

The correct option is $C 6$
The lewis dot structure of Sulphuric acid $(H_{2} S O_{4})$ is:
$S$ forms $6$ covalent bonds with its neighbouring oxygen atoms and hence the valency of $S$ is $6.$ 205-s1

Chemical Bonding and Molecular Structure

11906 The number of electrons involved in the bond formation of $N_{2}$ molecule

1

2

2

4

3

6

4

10

Explanation:

(c) In $N_{2}$ molecule each Nitrogen atom contribute $3 e^{-}$ so total no. of electron’s are $6.$

Chemical Bonding and Molecular Structure

11907 The electronic configuration of four elements are given in brackets $L (1 s^{2}, 2 s^{2} 2 p^{1}); M (1 s^{2}, 2 s^{2} 2 p^{5})$ $Q (1 s^{2}, 2 s^{2} 2 p^{6}, 3 s^{1}); R (1 s^{2}, 2 s^{2} 2 p^{2})$ The element that would most readily form a diatomic molecule is

1

Q

2

M

3

R

4

L

Explanation:

(b) Non-metals readily form diatomic molecules by sharing of electrons. Element $M (1 s^{2} 2 s^{2} 2 p^{5})$ has seven electrons in its valence shell and thus needs one more electron to complete its octet. Therefore, two atoms share one electron each to form a diatomic molecule $(M_{2})$ 205-s3

Chemical Bonding and Molecular Structure

11903 Which of the following hydrides are ionic

1

C a H_{2}

2

B a H_{2}

3

S r H_{2}

4 All of above

Explanation:

(d) $C a H_{2}, B a H_{2}, S r H_{2}$ are ionic hydride.

Chemical Bonding and Molecular Structure

11904 Which of the following conduct electricity in the fused state

1

B e C l_{2}

2

M g C l_{2}

3

B a C l_{2}

4

(b)

and

(c)

Explanation:

(d) Generally $M g C l_{2}, S r C l_{2},$ $B a C l_{2}$ are ionic compounds so they conduct electricity in fused state.

Chemical Bonding and Molecular Structure

11905 The valency of sulphur in sulphuric acid is

1

2

2

4

3

6

4

8

Explanation:

The correct option is $C 6$
The lewis dot structure of Sulphuric acid $(H_{2} S O_{4})$ is:
$S$ forms $6$ covalent bonds with its neighbouring oxygen atoms and hence the valency of $S$ is $6.$ 205-s1

Chemical Bonding and Molecular Structure

11906 The number of electrons involved in the bond formation of $N_{2}$ molecule

1

2

2

4

3

6

4

10

Explanation:

(c) In $N_{2}$ molecule each Nitrogen atom contribute $3 e^{-}$ so total no. of electron’s are $6.$

Chemical Bonding and Molecular Structure

11907 The electronic configuration of four elements are given in brackets $L (1 s^{2}, 2 s^{2} 2 p^{1}); M (1 s^{2}, 2 s^{2} 2 p^{5})$ $Q (1 s^{2}, 2 s^{2} 2 p^{6}, 3 s^{1}); R (1 s^{2}, 2 s^{2} 2 p^{2})$ The element that would most readily form a diatomic molecule is

1

Q

2

M

3

R

4

L

Explanation:

(b) Non-metals readily form diatomic molecules by sharing of electrons. Element $M (1 s^{2} 2 s^{2} 2 p^{5})$ has seven electrons in its valence shell and thus needs one more electron to complete its octet. Therefore, two atoms share one electron each to form a diatomic molecule $(M_{2})$ 205-s3

Chemical Bonding and Molecular Structure

11903 Which of the following hydrides are ionic

1

C a H_{2}

2

B a H_{2}

3

S r H_{2}

4 All of above

Explanation:

(d) $C a H_{2}, B a H_{2}, S r H_{2}$ are ionic hydride.

Chemical Bonding and Molecular Structure

11904 Which of the following conduct electricity in the fused state

1

B e C l_{2}

2

M g C l_{2}

3

B a C l_{2}

4

(b)

and

(c)

Explanation:

(d) Generally $M g C l_{2}, S r C l_{2},$ $B a C l_{2}$ are ionic compounds so they conduct electricity in fused state.

Chemical Bonding and Molecular Structure

11905 The valency of sulphur in sulphuric acid is

1

2

2

4

3

6

4

8

Explanation:

The correct option is $C 6$
The lewis dot structure of Sulphuric acid $(H_{2} S O_{4})$ is:
$S$ forms $6$ covalent bonds with its neighbouring oxygen atoms and hence the valency of $S$ is $6.$ 205-s1

Chemical Bonding and Molecular Structure

11906 The number of electrons involved in the bond formation of $N_{2}$ molecule

1

2

2

4

3

6

4

10

Explanation:

(c) In $N_{2}$ molecule each Nitrogen atom contribute $3 e^{-}$ so total no. of electron’s are $6.$

Chemical Bonding and Molecular Structure

11907 The electronic configuration of four elements are given in brackets $L (1 s^{2}, 2 s^{2} 2 p^{1}); M (1 s^{2}, 2 s^{2} 2 p^{5})$ $Q (1 s^{2}, 2 s^{2} 2 p^{6}, 3 s^{1}); R (1 s^{2}, 2 s^{2} 2 p^{2})$ The element that would most readily form a diatomic molecule is

1

Q

2

M

3

R

4

L

Explanation:

(b) Non-metals readily form diatomic molecules by sharing of electrons. Element $M (1 s^{2} 2 s^{2} 2 p^{5})$ has seven electrons in its valence shell and thus needs one more electron to complete its octet. Therefore, two atoms share one electron each to form a diatomic molecule $(M_{2})$ 205-s3

Chemical Bonding and Molecular Structure

11903 Which of the following hydrides are ionic

1

C a H_{2}

2

B a H_{2}

3

S r H_{2}

4 All of above

Explanation:

(d) $C a H_{2}, B a H_{2}, S r H_{2}$ are ionic hydride.

Chemical Bonding and Molecular Structure

11904 Which of the following conduct electricity in the fused state

1

B e C l_{2}

2

M g C l_{2}

3

B a C l_{2}

4

(b)

and

(c)

Explanation:

(d) Generally $M g C l_{2}, S r C l_{2},$ $B a C l_{2}$ are ionic compounds so they conduct electricity in fused state.

Chemical Bonding and Molecular Structure

11905 The valency of sulphur in sulphuric acid is

1

2

2

4

3

6

4

8

Explanation:

The correct option is $C 6$
The lewis dot structure of Sulphuric acid $(H_{2} S O_{4})$ is:
$S$ forms $6$ covalent bonds with its neighbouring oxygen atoms and hence the valency of $S$ is $6.$ 205-s1

Chemical Bonding and Molecular Structure

11906 The number of electrons involved in the bond formation of $N_{2}$ molecule

1

2

2

4

3

6

4

10

Explanation:

(c) In $N_{2}$ molecule each Nitrogen atom contribute $3 e^{-}$ so total no. of electron’s are $6.$

Chemical Bonding and Molecular Structure

11907 The electronic configuration of four elements are given in brackets $L (1 s^{2}, 2 s^{2} 2 p^{1}); M (1 s^{2}, 2 s^{2} 2 p^{5})$ $Q (1 s^{2}, 2 s^{2} 2 p^{6}, 3 s^{1}); R (1 s^{2}, 2 s^{2} 2 p^{2})$ The element that would most readily form a diatomic molecule is

1

Q

2

M

3

R

4

L

Explanation:

(b) Non-metals readily form diatomic molecules by sharing of electrons. Element $M (1 s^{2} 2 s^{2} 2 p^{5})$ has seven electrons in its valence shell and thus needs one more electron to complete its octet. Therefore, two atoms share one electron each to form a diatomic molecule $(M_{2})$ 205-s3

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