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: 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 for ClO⁻

Chlorine (Cl) has 7 valence electrons and oxygen (O) has 6 valence electrons. The ion has a - 1 charge, so we add 1 electron. 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 \(2\times2 + 6 = 10\) (2 from the double - bond and 6 non - bonding electrons on O), which is incorrect.

Step2: Check octet rule for first ClO⁻ structure

The chlorine atom in \([:Cl = O:]^{-}\) has 4 electrons (2 from the double - bond and 2 non - bonding electrons), which does not satisfy the octet rule. The problem atom is Cl.

Step3: Calculate valence - electrons for the second ClO⁻ structure \([:Cl - O:]^{-}\)

The number of valence electrons shown is \(2+6 + 6=14\) (2 from the single - bond, 6 non - bonding electrons on Cl and 6 non - bonding electrons on O), which is correct.

Step4: Check octet rule for second ClO⁻ structure

Both Cl and O in \([:Cl - O:]^{-}\) have 8 electrons (Cl has 7 non - bonding + 1 bonding, O has 6 non - bonding+2 bonding), so it satisfies the octet rule.

Step5: Calculate valence - electrons for \(N_{3}^{-}\)

Nitrogen has 5 valence electrons. For \(N_{3}^{-}\), with 3 nitrogen atoms and a - 1 charge, 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 \(2+4 + 6=12\) (2 from the single - bond, 4 non - bonding electrons on the left N and 6 non - bonding electrons on the right N), which is incorrect.

Step6: Check octet rule for \(N_{3}^{-}\) structure

The left - most nitrogen atom in \([:N - N = N:]^{-}\) has 4 electrons (2 non - bonding and 2 bonding), which does not satisfy the octet rule. The problem atom is N.

For the first ClO⁻ structure:

Answer:

No, it has the wrong number of valence electrons. The correct number is: 14. The symbols of the problem atoms are: Cl
For the second ClO⁻ structure: