Question

try again
your answer is incorrect.

• row 1: clo⁻ your answer is incorrect.
• row 3: n₃⁻ your answer is incorrect.

decide whether these proposed lewis structures are reasonable.
proposed lewis structure is the proposed lewis structure reasonable?
yes.
no, it has the wrong number of valence electrons.
the correct number is:
no, it has the right number of valence electrons but doesnt satisfy the octet rule.
the symbols of the problem atoms are: cl
yes.
no, it has the wrong number of valence electrons.
the correct number is:
no, it has the right number of valence electrons but doesnt satisfy the octet rule.
the symbols of the problem atoms are:
yes.
no, it has the wrong number of valence electrons.
the correct number is:
no, it has the right number of valence electrons but doesnt satisfy the octet rule.
the symbols of the problem atoms are:

• if two or more atoms of the same element dont satisfy the octet rule, just enter the chemical symbol as many times as necessary. for example, if two oxygen atoms dont satisfy the octet rule, enter \o,o\.

Explanation:

Step1: Calculate valence - electrons of ClO⁻

Chlorine (Cl) has 7 valence electrons and oxygen (O) has 6 valence electrons. The ion has a - 1 charge, so the total number of valence electrons is \(7 + 6+1=14\).
For the first proposed structure \([:Cl = O:]^{-}\), the number of valence - electrons shown is \(2\times4 + 2=10\) (2 lone - pairs on Cl and O, and a double - bond), which is incorrect. The correct number of valence electrons is 14.

Step2: Check octet rule for the first proposed structure

In \([:Cl = O:]^{-}\), Cl has 6 electrons around it (2 lone - pairs and 2 electrons in the double - bond), so it does not satisfy the octet rule. The problem atom is Cl.

Step3: Calculate valence - electrons of the second proposed structure \([:Cl - O:]^{-}\)

The number of valence electrons shown is \(3\times2+2 = 8\) (3 lone - pairs and a single - bond). The correct number of valence electrons is 14.

Step4: Check octet rule for the second proposed structure

In \([:Cl - O:]^{-}\), Cl has 7 electrons around it (3 lone - pairs and 1 electron in the single - bond) and O has 7 electrons around it (3 lone - pairs and 1 electron in the single - bond), so both do not satisfy the octet rule. The problem atoms are Cl and O.

Step5: Calculate valence - electrons of \(N_3^{-}\)

Nitrogen (N) has 5 valence electrons. For \(N_3^{-}\), the total number of valence electrons is \(3\times5 + 1=16\).
For the proposed structure \([:N - N = N:]^{-}\), the number of valence electrons shown is \(2\times2+3\times2=10\) (2 lone - pairs and 3 bonds), which is incorrect. The correct number of valence electrons is 16.

Step6: Check octet rule for the \(N_3^{-}\) structure

In \([:N - N = N:]^{-}\), the left - most N has 7 electrons around it (2 lone - pairs and 3 electrons in the bonds), so it does not satisfy the octet rule. The problem atom is the left - most N.

Answer:

For the first ClO⁻ structure:
No, it has the wrong number of valence electrons. The correct number is 14.
For the second ClO⁻ structure:
No, it has the wrong number of valence electrons. The correct number is 14. The problem atoms are Cl, O.
For the \(N_3^{-}\) structure:
No, it has the wrong number of valence electrons. The correct number is 16. The problem atom is the left - most N.