Chapter 8.4, Problem 35LC

(a)

Interpretation Introduction

Interpretation: The electron dot structure of HOOH needs to be drawn. Also, the polar covalent bonds need to be identified by assigning partial positive and negative charges on atoms.

Concept Introduction: A covalent bond can be polar if the two atoms bonded together have electronegativity differences. Here, an atom with more electronegativity has a partial negative charge, and an atom with less electronegativity has a partial positive charge.

Explanation of Solution

The given molecule is HOOH. Here, oxygen atoms are bonded together with one hydrogen atom. The number of valence electrons in an oxygen atom is 6 and that in the hydrogen atom is 1; thus, the total number of valence electrons will be:

  $\begin{array}{c}2\left(6\right)+2\left(1\right)=12+2\\ =14\end{array}$

The arrangement of electrons around an atom can be represented as follows:

  

In the above molecule, the oxygen atom is more electronegative than the hydrogen atom. Thus, the oxygen atom will have a partial negative charge and the hydrogen atom will have a partial positive charge. This is represented as follows:

  

(b)

Interpretation Introduction

Interpretation: The electron dot structure of BrCl needs to be drawn. Also, the polar covalent bonds need to be identified by assigning partial positive and negative charges on atoms.

Concept Introduction: A covalent bond can be polar if the two atoms bonded together have electronegativity differences. Here, the atom with more electronegativity has a partial negative charge, and the atom with less electronegativity has a partial positive charge.

Explanation of Solution

The given molecule is BrCl. Here, Br and Cl are bonded via a single covalent bond. There are 7 valence electrons on Br and Cl atoms. Thus, the total number of valence electrons in the molecule will be:

  $7+7=14$

The arrangement of electrons around the atom in the molecule can be represented as follows:

  

In the above molecule, the Cl atom is more electronegative than the Br atom. Thus, the Cl atom will have a partial negative charge and the Br atom will have a partial positive charge. This can be represented as follows:

  

(c)

Interpretation Introduction

Interpretation: The electron dot structure of HBr needs to be drawn. Also, the polar covalent bonds need to be identified by assigning partial positive and negative charges on atoms.

Concept Introduction: A covalent bond can be polar if the two atoms bonded together have electronegativity differences. Here, the atom with more electronegativity has a partial negative charge, and the atom with less electronegativity has a partial positive charge.

Explanation of Solution

The given molecule is HBr. Here, H and Br are bonded via a single covalent bond. There are 7 valence electrons in the Br atom and 1 valence electron in the H atom. Thus, the total number of valence electrons in a molecule will be:

  $1+7+8$

The arrangement of electrons around an atom in the molecule can be represented as follows:

  

In the molecule, the Br atom is more electronegative than the H atom thus, there will be a partial negative charge on Br and a partial positive charge on the H atom. This can be represented as follows:

  

(d)

Interpretation Introduction

Interpretation: The electron dot structure of ${\text{H}}_{\text{2}}\text{O}$ needs to be drawn. Also, the polar covalent bonds need to be identified by assigning partial positive and negative charges on atoms.

Concept Introduction: A covalent bond can be polar if the two atoms bonded together have electronegativity differences. Here, the atom with more electronegativity has a partial negative charge, and the atom with less electronegativity has a partial positive charge.

Explanation of Solution

The given molecule is ${\text{H}}_{\text{2}}\text{O}$ . Here, the oxygen atom is bonded with two hydrogen atoms via a single covalent bond. The number of valence electrons on O and H atoms is 6 and 1 respectively. Thus, the total number of valence electrons in the molecule will be:

  $\begin{array}{c}2\left(1\right)+6=2+6\\ =8\end{array}$

The arrangement of electrons around atoms in the molecule can be represented as follows:

  

In the above molecule, the oxygen atom is more electronegative than the hydrogen atom. Thus, the oxygen atom will have a partial negative charge and the hydrogen atom will have a partial positive charge. This is represented as follows: