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Chapter 11: Problem 57

Give the total number of valence electrons in each of the following molecules. a. \(\mathrm{CBr}_{4}\) b. \(\mathrm{NO}_{2}\) c. \(C_{6} H_{6}\) d. \(\mathrm{H}_{2} \mathrm{O}_{2}\)

Short Answer

Expert verified
The total number of valence electrons in each molecule are as follows: a. \(\mathrm{CBr}_{4}\): 32 valence electrons b. \(\mathrm{NO}_{2}\): 17 valence electrons c. \(C_{6} H_{6}\): 30 valence electrons d. \(\mathrm{H}_{2} \mathrm{O}_{2}\): 14 valence electrons

Step by step solution

01

Identify the valence electrons of each atom in the molecule

First, we need to identify the number of valence electrons for each atom in the molecule. Carbon (C) has 4 valence electrons, and bromine (Br) has 7 valence electrons.
02

Calculate the total valence electrons

Now, we can calculate the total valence electrons in the molecule by adding the valence electrons of each atom, multiplied by the number of atoms in the molecule: \(1 \times 4 + 4 \times 7 = 4 + 28 = 32\). Therefore, there are 32 valence electrons in \(\mathrm{CBr}_{4}\). #b. \(\mathrm{NO}_{2}\)#
03

Identify the valence electrons of each atom in the molecule

For this molecule, nitrogen (N) has 5 valence electrons, and oxygen (O) has 6 valence electrons.
04

Calculate the total valence electrons

We can calculate the total valence electrons in the molecule by adding the valence electrons of each atom, multiplied by the number of atoms in the molecule: \(1 \times 5 + 2 \times 6 = 5 + 12 = 17\). Therefore, there are 17 valence electrons in \(\mathrm{NO}_{2}\). #c. \(C_{6} H_{6}\)#
05

Identify the valence electrons of each atom in the molecule

In this molecule, carbon (C) has 4 valence electrons, and hydrogen (H) has 1 valence electron.
06

Calculate the total valence electrons

We can calculate the total valence electrons in the molecule by adding the valence electrons of each atom, multiplied by the number of atoms in the molecule: \(6 \times 4 + 6 \times 1 = 24 + 6 = 30\). Therefore, there are 30 valence electrons in \(C_{6} H_{6}\). #d. \(\mathrm{H}_{2} \mathrm{O}_{2}\)#
07

Identify the valence electrons of each atom in the molecule

For this molecule, hydrogen (H) has 1 valence electron, and oxygen (O) has 6 valence electrons.
08

Calculate the total valence electrons

We can calculate the total valence electrons in the molecule by adding the valence electrons of each atom, multiplied by the number of atoms in the molecule: \(2 \times 1 + 2 \times 6 = 2 + 12 = 14\). Therefore, there are 14 valence electrons in \(\mathrm{H}_{2} \mathrm{O}_{2}\).

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Most popular questions from this chapter

Write a Lewis structure for each of the following polyatomic ions. Show all bonding valence electron pairs as lines and all nonbonding valence electron pairs as dots. For those ions that exhibit resonance, draw the various possible resonance forms. a. sulfate ion, \(\mathrm{SO}_{4}^{2-}\) b. phosphate ion, \(\mathrm{PO}_{4}^{3-}\) c. sulfite ion, \(\mathrm{SO}_{3}^{2-}\)

Write the Lewis structure for each of the following atoms. a. He \((Z=2)\) b. \(\operatorname{Br}(Z=35)\) c. \(\operatorname{Sr}(Z=38)\) d. \(\operatorname{Ne}(Z=10)\) e. I \((Z=53)\) f. Ra \((Z=88)\)

Write a Lewis structure for each of the following polyatomic ions. Show all bonding valence electron pairs as lines and all nonbonding valence electron pairs as dots. For those ions that exhibit resonance, draw the various possible resonance forms. a. nitrate ion b. carbonate ion c. ammonium ion

Explain how the atoms in covalent molecules achieve configurations similar to those of the noble gases. How does this differ from the situation in ionic compounds?

Which of the following molecules contain polar covalent bonds? a. phosphorus, \(P_{4}\) b. oxygen, \(\mathrm{O}_{2}\) c. ozone, \(\mathrm{O}_{3}\) d. hydrogen fluoride, HF
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