12200
The states of hybridazation of boron and oxygen atoms in boric acid \(({H_3}B{O_3})\) are respectively
1 \(s{p^3}\) and \(s{p^2}\)
2 \(s{p^2}\) and \(s{p^3}\)
3 \(s{p^2}\) and \(s{p^2}\)
4 \(s{p^3}\)and \(s{p^3}\)
Explanation:
(b)
Chemical Bonding and Molecular Structure
12084
The mode of hybridisation of carbon in \(C{O_2}\) is
1 \(sp\)
2 \(s{p^2}\)
3 \(s{p^3}\)
4 None of these
Explanation:
The carbon atom in \(CO _2\) has two double bonds, one with each atom of oxygen. Therefore, the carbon's hybridization is \(sp\). Determine the hybridization for the other atoms in the molecule. Each oxygen atom in \(CO _2\) has a single double bond with the carbon.
Chemical Bonding and Molecular Structure
12085
In which of the following the central atom does not use \(s{p^3}\) hybrid orbitals in its bonding
1 \(Be{F_3}^ - \)
2 \(OH_3^ + \)
3 \(N{H_2}^ - \)
4 \(N{F_3} \)
Explanation:
(a) In \(BeF_3^ - \), \(Be\) is not \(s{p^3}\)-hybridised it is \(s{p^2}\) hybridised.
Chemical Bonding and Molecular Structure
12220
Which of the following molecule contains one pair of non-bonding electrons
1 \(C{H_4}\)
2 \(N{H_3}\)
3 \({H_2}O\)
4 \(HF\)
Explanation:
(b) In \(N{H_3}\) nitrogen has one lone pair of electron.
12200
The states of hybridazation of boron and oxygen atoms in boric acid \(({H_3}B{O_3})\) are respectively
1 \(s{p^3}\) and \(s{p^2}\)
2 \(s{p^2}\) and \(s{p^3}\)
3 \(s{p^2}\) and \(s{p^2}\)
4 \(s{p^3}\)and \(s{p^3}\)
Explanation:
(b)
Chemical Bonding and Molecular Structure
12084
The mode of hybridisation of carbon in \(C{O_2}\) is
1 \(sp\)
2 \(s{p^2}\)
3 \(s{p^3}\)
4 None of these
Explanation:
The carbon atom in \(CO _2\) has two double bonds, one with each atom of oxygen. Therefore, the carbon's hybridization is \(sp\). Determine the hybridization for the other atoms in the molecule. Each oxygen atom in \(CO _2\) has a single double bond with the carbon.
Chemical Bonding and Molecular Structure
12085
In which of the following the central atom does not use \(s{p^3}\) hybrid orbitals in its bonding
1 \(Be{F_3}^ - \)
2 \(OH_3^ + \)
3 \(N{H_2}^ - \)
4 \(N{F_3} \)
Explanation:
(a) In \(BeF_3^ - \), \(Be\) is not \(s{p^3}\)-hybridised it is \(s{p^2}\) hybridised.
Chemical Bonding and Molecular Structure
12220
Which of the following molecule contains one pair of non-bonding electrons
1 \(C{H_4}\)
2 \(N{H_3}\)
3 \({H_2}O\)
4 \(HF\)
Explanation:
(b) In \(N{H_3}\) nitrogen has one lone pair of electron.
12200
The states of hybridazation of boron and oxygen atoms in boric acid \(({H_3}B{O_3})\) are respectively
1 \(s{p^3}\) and \(s{p^2}\)
2 \(s{p^2}\) and \(s{p^3}\)
3 \(s{p^2}\) and \(s{p^2}\)
4 \(s{p^3}\)and \(s{p^3}\)
Explanation:
(b)
Chemical Bonding and Molecular Structure
12084
The mode of hybridisation of carbon in \(C{O_2}\) is
1 \(sp\)
2 \(s{p^2}\)
3 \(s{p^3}\)
4 None of these
Explanation:
The carbon atom in \(CO _2\) has two double bonds, one with each atom of oxygen. Therefore, the carbon's hybridization is \(sp\). Determine the hybridization for the other atoms in the molecule. Each oxygen atom in \(CO _2\) has a single double bond with the carbon.
Chemical Bonding and Molecular Structure
12085
In which of the following the central atom does not use \(s{p^3}\) hybrid orbitals in its bonding
1 \(Be{F_3}^ - \)
2 \(OH_3^ + \)
3 \(N{H_2}^ - \)
4 \(N{F_3} \)
Explanation:
(a) In \(BeF_3^ - \), \(Be\) is not \(s{p^3}\)-hybridised it is \(s{p^2}\) hybridised.
Chemical Bonding and Molecular Structure
12220
Which of the following molecule contains one pair of non-bonding electrons
1 \(C{H_4}\)
2 \(N{H_3}\)
3 \({H_2}O\)
4 \(HF\)
Explanation:
(b) In \(N{H_3}\) nitrogen has one lone pair of electron.
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Chemical Bonding and Molecular Structure
12200
The states of hybridazation of boron and oxygen atoms in boric acid \(({H_3}B{O_3})\) are respectively
1 \(s{p^3}\) and \(s{p^2}\)
2 \(s{p^2}\) and \(s{p^3}\)
3 \(s{p^2}\) and \(s{p^2}\)
4 \(s{p^3}\)and \(s{p^3}\)
Explanation:
(b)
Chemical Bonding and Molecular Structure
12084
The mode of hybridisation of carbon in \(C{O_2}\) is
1 \(sp\)
2 \(s{p^2}\)
3 \(s{p^3}\)
4 None of these
Explanation:
The carbon atom in \(CO _2\) has two double bonds, one with each atom of oxygen. Therefore, the carbon's hybridization is \(sp\). Determine the hybridization for the other atoms in the molecule. Each oxygen atom in \(CO _2\) has a single double bond with the carbon.
Chemical Bonding and Molecular Structure
12085
In which of the following the central atom does not use \(s{p^3}\) hybrid orbitals in its bonding
1 \(Be{F_3}^ - \)
2 \(OH_3^ + \)
3 \(N{H_2}^ - \)
4 \(N{F_3} \)
Explanation:
(a) In \(BeF_3^ - \), \(Be\) is not \(s{p^3}\)-hybridised it is \(s{p^2}\) hybridised.
Chemical Bonding and Molecular Structure
12220
Which of the following molecule contains one pair of non-bonding electrons
1 \(C{H_4}\)
2 \(N{H_3}\)
3 \({H_2}O\)
4 \(HF\)
Explanation:
(b) In \(N{H_3}\) nitrogen has one lone pair of electron.
