Question

try again
your answer is incorrect.
. row 1: clo⁻: your answer is incorrect.
. row 2: cocl₂: your answer is incorrect.
. row 3: h₂o: you made several mistakes. please read the explanation.
decide whether these proposed lewis structures are reasonable.
proposed lewis structure | is the proposed lewis structure reasonable?
\\:cl - o:\\^-
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
\\:o:
|
:cl - c - 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:* c
h - h - \\:o:
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:* h, h

• 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 \(ClO^-\)

The valence electrons of \(Cl\) is 7, \(O\) is 6, and + 1 for the negative charge, so \(7 + 6+1 = 14\).

Step2: Check octet rule for \(ClO^-\)

\(Cl\) has 7 electrons around it, violating the octet rule.

Step3: Calculate valence electrons for \(COCl_2\)

\(C\) has 4, \(O\) has 6, and \(2Cl\) have \(2\times7\), so \(4 + 6+14 = 24\).

Step4: Check octet rule for \(COCl_2\)

\(C\) has 6 electrons around it, violating the octet rule.

Step5: Calculate valence electrons for \(H_2O\)

\(2H\) have \(2\times1\) and \(O\) has 6, so \(2 + 6=8\).

Step6: Check octet rule for \(H_2O\)

The \(H - H\) bond is incorrect, and \(O\) does not have a complete octet in this structure.

Answer:

1. For \(ClO^-\):

• No, it has the right number of valence - electrons but doesn't satisfy the octet rule. The symbols of the problem atoms are: \(Cl\)
• Calculate the number of valence electrons: \(Cl\) has 7 valence electrons and \(O\) has 6 valence electrons, and there is an extra electron due to the negative charge. So the total number of valence electrons is \(7 + 6+1=14\). In the given structure, \(Cl\) has only 7 electrons around it (counting bonding and non - bonding electrons), not satisfying the octet rule.

1. For \(COCl_2\):

• No, it has the right number of valence electrons but doesn't satisfy the octet rule. The symbols of the problem atoms are: \(C\)
• Calculate the number of valence electrons: \(C\) has 4, \(O\) has 6, and \(Cl\) has 7. For \(COCl_2\), the total number of valence electrons is \(4 + 6+2\times7=24\). In the given structure, \(C\) has only 6 electrons around it (counting bonding and non - bonding electrons), not satisfying the octet rule.

1. For \(H_2O\):

• No, it has the right number of valence electrons but doesn't satisfy the octet rule. The symbols of the problem atoms are: \(H,H\)
• Calculate the number of valence electrons: \(H\) has 1 valence electron and \(O\) has 6 valence electrons. For \(H_2O\), the total number of valence electrons is \(2\times1 + 6=8\). In the given structure, the two \(H\) atoms are bonded to each other which is incorrect. In a water molecule, the \(H\) atoms should be bonded to the \(O\) atom, and the \(O\) atom should have 8 electrons around it to satisfy the octet rule.