Answered

1. Fill in the blanks:

- A polar bond results from the ________ sharing of the electrons in a covalent bond between atoms.
- A nonpolar bond results from the ________ sharing of the electrons in a covalent bond between atoms.

2. Complete the Lewis electron-dot symbols and valence electron configuration for elements in the following table.

[tex]\[
\begin{array}{|c|c|c|}
\hline
\text{Group} & \text{1 A} & \text{2 A} \\
\hline
\begin{array}{r}
\text{Valence} \\
\text{electrons}
\end{array} & \text{ns} & \\
\hline
\text{Period 2} & \text{Li} & \text{Be} \\
\hline
\text{Period 3} & \text{Na} & \text{Mg} \\
\hline
\end{array}
\][/tex]

[tex]\[
\begin{array}{|c|c|c|c|c|c|c|}
\hline
\text{3 A} & \text{4 A} & \text{5 A} & \text{6 A} & \text{7 A} & \text{8 A} \\
\hline
& & & & & \\
\hline
\text{s}^2 \text{np}^5 \\
\hline
\text{B} & \text{C} & \text{N} & \text{O} & \text{F} & \text{Ne} \\
\hline
\text{Al} & \text{Si} & \text{P} & \text{S} & \text{Cl} & \text{Ar} \\
\hline
\end{array}
\][/tex]

3. Learn the definitions of the types of intermolecular forces between molecules and/or ions. Fill in the blanks.

[tex]\[
\begin{array}{|c|l|}
\hline
\text{Particles Interact} & \text{via Intermolecular Forces} \\
\hline
\begin{array}{c}
\text{Polar molecules interact} \\
\text{with polar molecules}
\end{array} & \\
\hline
\text{Ions interact with polar molecules} & \\
\hline
\begin{array}{l}
\text{Polar molecules with O-H, N-H, or H-F} \\
\text{groups interact with each other, or with} \\
\text{polar molecules containing O, N, and F}
\end{array} & \\
\hline
\begin{array}{c}
\text{Nonpolar molecules interact} \\
\text{with nonpolar molecules}
\end{array} & \\
\hline
\begin{array}{c}
\text{Nonpolar molecules interact} \\
\text{with polar molecules}
\end{array} & \\
\hline
\end{array}
\][/tex]



Answer :

Sure! Let's break down each part of the question and provide a detailed, step-by-step solution.

### 1. Fill in the blanks:
- A polar bond results from the unequal sharing of the electrons in a covalent bond between atoms.
- A nonpolar bond results from the equal sharing of the electrons in a covalent bond between atoms.

### 2. Complete the Lewis electron-dot symbols and valence electron configuration for elements in the following table:
\begin{tabular}{|c|c|c|}
\hline
Group & 1 A & 2 A \\
\hline
\begin{tabular}{c}
Valence \\
electrons
\end{tabular} & ns & [tex]\([He] 2s^2\)[/tex] \\
\hline
Period 2 & Li & Be \\
\hline
Period 3 & Na & Mg \\
\hline
\end{tabular}
\begin{tabular}{|c|c|c|c|c|c|}
\hline
3 A & 4 A & 5 A & 6 A & 7 A & 8 A \\
\hline
[tex]\( s^2 p^1\)[/tex] & & s^2 n p^5 & & & [tex]\( s^2 np^6\)[/tex] \\
\hline
B & C & N & O & F & Ne \\
\hline
Al & Si & P & S & Cl & Ar \\
\hline
\end{tabular}

### 3. Learn the definitions of the type of intermolecular forces between molecules and/or ions. Fill in the blanks.
\begin{tabular}{|c|l|}
\hline
Particles Interact & via Intermolecular Forces \\
\hline
\begin{tabular}{c}
Polar molecules interact \\
with polar molecules
\end{tabular} & dipole-dipole forces and hydrogen bonds \\
\hline
Ions interact with polar molecules & ion-dipole forces \\
\hline
\begin{tabular}{l}
Polar molecules with O-H, N-H, or H-F \\
groups interact with each other, or with \\
polar molecules containing O, N, and F
\end{tabular} & hydrogen bonds \\
\hline
Nonpolar molecules interact \\
with nonpolar molecules & dispersion forces (London forces) \\
\hline
Nonpolar molecules interact \\
with polar molecules & induced dipole forces \\
\hline
\end{tabular}

### Summary:
1. The sharing of electrons in polar bonds is unequal, leading to partial charges on the atoms involved. In nonpolar bonds, the electron sharing is equal.
2. The valence electron configurations for elements in various groups and periods highlight the distribution of electrons in their outermost shells, influenced by their position on the periodic table.
3. Different types of intermolecular forces act between molecules and/or ions, such as dipole-dipole forces, ion-dipole forces, hydrogen bonds, and dispersion forces (London forces), depending on the nature of the interacting particles.