313528
What is the formal charge on ' \(\mathrm{N}\) ' atom in \(\mathrm{NH}_{4}^{+}\) ion?
1 +1
2 -3
3 -1
4 Zero
Explanation:
\(\mathrm{NH}_{4}^{+}\)ion \(\Rightarrow\left[\begin{array}{c}\mathrm{H} \\ \mathrm{H}-\mathrm{N}-\mathrm{N}-\mathrm{H} \\ \mathrm{H}\end{array}\right]^{+}\) \(\mathrm{FC}=\mathrm{VE}-\mathrm{NE}-\left(\dfrac{\mathrm{BE}}{2}\right)\) \(\therefore\) Formal charge of ' \(\mathrm{N}\) ' atom \(=5-0-\left(\dfrac{8}{2}\right)=+1\)
MHTCET - 2021
CHXI04:CHEMICAL BONDING AND MOLECULAR STRUCTURE
313529
The formal charge on carbon atom in the following structure is
1 0
2 1
3 -1
4 0.5
Explanation:
The Formal charge on C atom = Valence electrons - Lone pair of electrons - \(\frac{{\rm{1}}}{{\rm{2}}}{\rm{ \times Bonding}}\,\,{\rm{electrons = 4 - 0 - }}\frac{{\rm{1}}}{{\rm{2}}}{\rm{ \times 8 = 0}}\)
CHXI04:CHEMICAL BONDING AND MOLECULAR STRUCTURE
313530
Statement A : The correct Lewis structure of \({{\rm{O}}_{\rm{3}}}\) may be drawn as Statement B : The formal charges on atom 1, 2 and 3 are +1, 0 and -1 respectively
1 Statement A is correct but Statement B is incorrect
2 Statement A is incorrect but Statement B is correct
3 Both statements are correct
4 Both statements are incorrect
Explanation:
Formal charge on \({{\rm{O}}_{\rm{1}}}{\rm{ = 6 - 2 - }}\frac{{\rm{1}}}{{\rm{2}}}{\rm{(6) = + 1}}\) Formal charge on \({{\rm{O}}_{\rm{2}}}{\rm{ = 6 - 4 - }}\frac{{\rm{1}}}{{\rm{2}}}{\rm{(4) = 0}}\) Formal charge on \({{\rm{O}}_{\rm{3}}}{\rm{ = 6 - 6 - }}\frac{{\rm{1}}}{{\rm{2}}}{\rm{ \times 3 = - 1}}\) Hence, correct representation of \({{\rm{O}}_{\rm{3}}}\) is So, the option (3) is correct.
CHXI04:CHEMICAL BONDING AND MOLECULAR STRUCTURE
313531
The formal charge on S-atom in the following structure is:
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CHXI04:CHEMICAL BONDING AND MOLECULAR STRUCTURE
313528
What is the formal charge on ' \(\mathrm{N}\) ' atom in \(\mathrm{NH}_{4}^{+}\) ion?
1 +1
2 -3
3 -1
4 Zero
Explanation:
\(\mathrm{NH}_{4}^{+}\)ion \(\Rightarrow\left[\begin{array}{c}\mathrm{H} \\ \mathrm{H}-\mathrm{N}-\mathrm{N}-\mathrm{H} \\ \mathrm{H}\end{array}\right]^{+}\) \(\mathrm{FC}=\mathrm{VE}-\mathrm{NE}-\left(\dfrac{\mathrm{BE}}{2}\right)\) \(\therefore\) Formal charge of ' \(\mathrm{N}\) ' atom \(=5-0-\left(\dfrac{8}{2}\right)=+1\)
MHTCET - 2021
CHXI04:CHEMICAL BONDING AND MOLECULAR STRUCTURE
313529
The formal charge on carbon atom in the following structure is
1 0
2 1
3 -1
4 0.5
Explanation:
The Formal charge on C atom = Valence electrons - Lone pair of electrons - \(\frac{{\rm{1}}}{{\rm{2}}}{\rm{ \times Bonding}}\,\,{\rm{electrons = 4 - 0 - }}\frac{{\rm{1}}}{{\rm{2}}}{\rm{ \times 8 = 0}}\)
CHXI04:CHEMICAL BONDING AND MOLECULAR STRUCTURE
313530
Statement A : The correct Lewis structure of \({{\rm{O}}_{\rm{3}}}\) may be drawn as Statement B : The formal charges on atom 1, 2 and 3 are +1, 0 and -1 respectively
1 Statement A is correct but Statement B is incorrect
2 Statement A is incorrect but Statement B is correct
3 Both statements are correct
4 Both statements are incorrect
Explanation:
Formal charge on \({{\rm{O}}_{\rm{1}}}{\rm{ = 6 - 2 - }}\frac{{\rm{1}}}{{\rm{2}}}{\rm{(6) = + 1}}\) Formal charge on \({{\rm{O}}_{\rm{2}}}{\rm{ = 6 - 4 - }}\frac{{\rm{1}}}{{\rm{2}}}{\rm{(4) = 0}}\) Formal charge on \({{\rm{O}}_{\rm{3}}}{\rm{ = 6 - 6 - }}\frac{{\rm{1}}}{{\rm{2}}}{\rm{ \times 3 = - 1}}\) Hence, correct representation of \({{\rm{O}}_{\rm{3}}}\) is So, the option (3) is correct.
CHXI04:CHEMICAL BONDING AND MOLECULAR STRUCTURE
313531
The formal charge on S-atom in the following structure is:
313528
What is the formal charge on ' \(\mathrm{N}\) ' atom in \(\mathrm{NH}_{4}^{+}\) ion?
1 +1
2 -3
3 -1
4 Zero
Explanation:
\(\mathrm{NH}_{4}^{+}\)ion \(\Rightarrow\left[\begin{array}{c}\mathrm{H} \\ \mathrm{H}-\mathrm{N}-\mathrm{N}-\mathrm{H} \\ \mathrm{H}\end{array}\right]^{+}\) \(\mathrm{FC}=\mathrm{VE}-\mathrm{NE}-\left(\dfrac{\mathrm{BE}}{2}\right)\) \(\therefore\) Formal charge of ' \(\mathrm{N}\) ' atom \(=5-0-\left(\dfrac{8}{2}\right)=+1\)
MHTCET - 2021
CHXI04:CHEMICAL BONDING AND MOLECULAR STRUCTURE
313529
The formal charge on carbon atom in the following structure is
1 0
2 1
3 -1
4 0.5
Explanation:
The Formal charge on C atom = Valence electrons - Lone pair of electrons - \(\frac{{\rm{1}}}{{\rm{2}}}{\rm{ \times Bonding}}\,\,{\rm{electrons = 4 - 0 - }}\frac{{\rm{1}}}{{\rm{2}}}{\rm{ \times 8 = 0}}\)
CHXI04:CHEMICAL BONDING AND MOLECULAR STRUCTURE
313530
Statement A : The correct Lewis structure of \({{\rm{O}}_{\rm{3}}}\) may be drawn as Statement B : The formal charges on atom 1, 2 and 3 are +1, 0 and -1 respectively
1 Statement A is correct but Statement B is incorrect
2 Statement A is incorrect but Statement B is correct
3 Both statements are correct
4 Both statements are incorrect
Explanation:
Formal charge on \({{\rm{O}}_{\rm{1}}}{\rm{ = 6 - 2 - }}\frac{{\rm{1}}}{{\rm{2}}}{\rm{(6) = + 1}}\) Formal charge on \({{\rm{O}}_{\rm{2}}}{\rm{ = 6 - 4 - }}\frac{{\rm{1}}}{{\rm{2}}}{\rm{(4) = 0}}\) Formal charge on \({{\rm{O}}_{\rm{3}}}{\rm{ = 6 - 6 - }}\frac{{\rm{1}}}{{\rm{2}}}{\rm{ \times 3 = - 1}}\) Hence, correct representation of \({{\rm{O}}_{\rm{3}}}\) is So, the option (3) is correct.
CHXI04:CHEMICAL BONDING AND MOLECULAR STRUCTURE
313531
The formal charge on S-atom in the following structure is:
313528
What is the formal charge on ' \(\mathrm{N}\) ' atom in \(\mathrm{NH}_{4}^{+}\) ion?
1 +1
2 -3
3 -1
4 Zero
Explanation:
\(\mathrm{NH}_{4}^{+}\)ion \(\Rightarrow\left[\begin{array}{c}\mathrm{H} \\ \mathrm{H}-\mathrm{N}-\mathrm{N}-\mathrm{H} \\ \mathrm{H}\end{array}\right]^{+}\) \(\mathrm{FC}=\mathrm{VE}-\mathrm{NE}-\left(\dfrac{\mathrm{BE}}{2}\right)\) \(\therefore\) Formal charge of ' \(\mathrm{N}\) ' atom \(=5-0-\left(\dfrac{8}{2}\right)=+1\)
MHTCET - 2021
CHXI04:CHEMICAL BONDING AND MOLECULAR STRUCTURE
313529
The formal charge on carbon atom in the following structure is
1 0
2 1
3 -1
4 0.5
Explanation:
The Formal charge on C atom = Valence electrons - Lone pair of electrons - \(\frac{{\rm{1}}}{{\rm{2}}}{\rm{ \times Bonding}}\,\,{\rm{electrons = 4 - 0 - }}\frac{{\rm{1}}}{{\rm{2}}}{\rm{ \times 8 = 0}}\)
CHXI04:CHEMICAL BONDING AND MOLECULAR STRUCTURE
313530
Statement A : The correct Lewis structure of \({{\rm{O}}_{\rm{3}}}\) may be drawn as Statement B : The formal charges on atom 1, 2 and 3 are +1, 0 and -1 respectively
1 Statement A is correct but Statement B is incorrect
2 Statement A is incorrect but Statement B is correct
3 Both statements are correct
4 Both statements are incorrect
Explanation:
Formal charge on \({{\rm{O}}_{\rm{1}}}{\rm{ = 6 - 2 - }}\frac{{\rm{1}}}{{\rm{2}}}{\rm{(6) = + 1}}\) Formal charge on \({{\rm{O}}_{\rm{2}}}{\rm{ = 6 - 4 - }}\frac{{\rm{1}}}{{\rm{2}}}{\rm{(4) = 0}}\) Formal charge on \({{\rm{O}}_{\rm{3}}}{\rm{ = 6 - 6 - }}\frac{{\rm{1}}}{{\rm{2}}}{\rm{ \times 3 = - 1}}\) Hence, correct representation of \({{\rm{O}}_{\rm{3}}}\) is So, the option (3) is correct.
CHXI04:CHEMICAL BONDING AND MOLECULAR STRUCTURE
313531
The formal charge on S-atom in the following structure is:
