Ionic and Molecular Compounds

Name each of the following molecular compounds:

a. $PB{r}_3$ 

b. $C{l}_{2}O$ 

c. $CB{r}_4$ 

d. $HF$ 

e. $N{F}_3$

Name each of the following molecular compounds:

a. $C{S}_2$

b. $P_2{O}_5$

c. $Si{O}_2$

d. $PC{l}_3$

e. $CO$

Name each of the following molecular compounds: 

a. $N_2{O}_3$

b. $S{i}_{2}B{r}_6$

c. $P_4{S}_3$

d. $PC{l}_5$

e. $Se{F}_6$

Write the formula for each of the following molecular compounds:

a. sulfur dioxide

b. silicon tetrachloride

c. iodine trifluoride

d. dinitrogen oxide

Write the formula for each of the following molecular compounds:

a. carbon tetrachloride

b. carbon monoxide

c. phosphorus trifluoride 

d. dinitrogen tetroxide

Name each of the following molecular compounds: 

a. $Si{F}_4$ 

b.$IB{r}_3$ 

c. $C{O}_2$ 

d.$N_2{F}_2$

e. $N_2{S}_3$

Name each of the following ionic or molecular compounds: 

(a) $Al{\left(S{O}_4\right)}_3$, antiperspirant

(b) $CaC{O}_3$, antacid

(c) $N_{2}O$, "laughing gas," inhaled anesthetic

(d) $Mg{\left(OH\right)}_2$, laxative

Name each of the following ionic or molecular compounds: 

(a) $Al{\left(OH\right)}_3$, antacid 

(b) $FeS{O}_4$, iron supplement in vitamins

(c) $NO$, vasodilator

(d) $Cu{\left(OH\right)}_2$, fungicide

Write the formula for each of the following molecular compounds:

a. sulfur dibromide

b. carbon disulfide

c. tetraphosphorus hexoxide

d. dinitrogen pentoxide

Write the formula for each of the following molecular compounds:

a. oxygen difluoride

b. boron trichloride

c. dinitrogen trioxide

d. sulfur hexafluoride

Determine the total number of valence electrons for each of the following.

a. ${\mathrm{H}}_2\mathrm{S}$

b. ${\mathrm{I}}_2$

c. ${\mathrm{CCl}}_4$

Determine the total number of valence electrons for each of the following:

a. ${\mathrm{SBr}}_2$

b. ${\mathrm{NBr}}_3$

c. ${\mathrm{CH}}_3\mathrm{OH}$

Describe the trend in electronegativity as increases or decreases for each of the following:

(a) from B to F     

(b) from Mg to Ba 

(c) from F to I 

Describe the trend in electronegativity as increases or decreases for each of the following: 

(a) from Al to CI 

(b) from Br to K 

(c) from Li to Cs

Using the periodic table, arrange the atoms in each of the following sets in order of increasing electronegativity: 

(a) Li, Na, K 

(b) Na, CI, P 

(c) Se, Ca, O 

Which electronegativity difference (a, b, or c) would you expect for a polar covalent bond?

(a) $0.0$ to $0.4$

(b) $0.5$ to $1.8$

(c) $1.9$ to $3.3$

Which electronegativity difference (a, b, or c) would you expect for a nonpolar covalent bond?

(a) from $0.0$ to $0.4$

(b) from $0.5$ to $1.8$

(c) from $1.9$ to $3.3$

Predict whether each of the following bonds is nonpolar covalent, polar covalent, or ionic:

a. $Si$and$Br$

b. $Li$and$F$

c. $Br$and$F$

d. $I$and$I$

e. $N$and$P$

f.  $C$and$P$

Predict whether each of the following bonds is nonpolar covalent, polar covalent, or ionic:

a. $Si$ and $O$

b. $K$ and $Cl$

c. $S$ and $F$

d. $P$ and $Br$

e. $Li$ and $O$

f.  $N$ and $S$

For each of the following bonds, indicate the positive end with ${\delta }^{+}$and the negative end with ${\delta }^{-}$. Draw an arrow to show the dipole for each.
a. N and F
b. Si and Br
c. C and O
d. P and Br
e. N and P

Using the periodic table, arrange the atoms in each of the following sets in order of increasing electronegativity: 

(a) CI, F, Br 

(b) B, O, N 

(c) Mg, F, S

For each of the following bonds, indicate the positive end with ${\delta }^{+}$and the negative end with ${\delta }^{-}$. Draw an arrow to show the dipole for each.
a. $\mathrm{P}$ and $\mathrm{Cl}$
b. $\mathrm{Se}$ and $\mathrm{F}$
c. $\mathrm{Br}$ and $\mathrm{F}$
d. $\mathrm{N}$ and $\mathrm{H}$
e. $\mathrm{B}$ and $\mathrm{Cl}$

Complete each of the following statements for a molecule of ${\mathrm{H}}_2\mathrm{S}$ :
a. There are          electron groups around the central $\mathrm{S}$ atom.
b. The electron-group geometry is          .
c. The number of atoms attached to the central $\mathrm{S}$ atom is         

d. The shape of the molecule is          .

Use VSEPR theory to predict the shape of each of the following:
a. ${\mathrm{Cl}}_4$
b. ${\mathrm{NCl}}_3$
c. ${\mathrm{SeBr}}_2$
d. ${\mathrm{CS}}_2$

Use VSEPR theory to predict the shape of each of the following:
a. ${\mathrm{GaH}}_3$
b. ${\mathrm{OF}}_2$
c. $\mathrm{HCN}$
d. ${\mathrm{CCl}}_4$

Compare the Lewis structures of ${\mathrm{CH}}_4$ and ${\mathrm{H}}_2\mathrm{O}$. Why do these molecules have similar bond angles but different molecular shapes?

Compare the Lewis structures of ${\mathrm{CF}}_4$ and ${\mathrm{NF}}_3$. Why do these molecules have different shapes?

Complete each of the following statements for a molecule of ${\mathrm{SeO}}_3$ :
a. There are              electron groups around the central $\mathrm{Se}$ atom.
b. The electron-group geometry is            .
c. The number of atoms attached to the central $\mathrm{Se}$ atom is           
d. The shape of the molecule is           .

1. linear
2. bent $(109°)$
3. trigonal planar
4. bent $(120°)$
5. trigonal pyramidal
6. tetrahedral 

(a) A molecule with a central atom that has four electron groups and four bonded atoms.

(b) A molecule with a central atom that has four electron groups and three bonded atoms

(c) A molecule with a central atom that has three electron groups and three bonded atoms

 Choose the shape (1 to 6 ) that matches each of the following descriptions (a to c):

1. linear
2. bent (109∘)
3. trigonal planar
4. bent (120∘)
5. trigonal pyramidal
6. tetrahedral

a. A molecule with a central atom that has four electron groups and two bonded atoms
b. A molecule with a central atom that has two electron groups and two bonded atoms
c. A molecule with a central atom that has three electron groups and two bonded atoms

Identify the major type of intermolecular forces between the particles of each of the following:
a. $BrF$

b.$KCl$

 c. $N{F}_3$

d.$C{l}_2$

Identify the major type of intermolecular forces between the particles of each of the following:
 a. $HCl$
 b. $Mg{F}_2$
 c. $PB{r}_3$
 d. $N{H}_3$

Identify the strongest intermolecular forces between the particles of each of the following:
 a. $C{H}_{3}OH$
 b.$CO$ 
 c. $C{F}_4$
 d. $C{H}_{3}C{H}_3$

Identify the strongest intermolecular forces between the particles of each of the following:
a. $O_2$
b. $Si{H}_4$
 c.$C{H}_{3 }Cl$ 
 d. $H_2{O}_2$

The molecules ${\mathrm{CH}}_4$ and ${\mathrm{CH}}_3\mathrm{Cl}$ both have tetrahedral shapes. Why is ${\mathrm{CH}}_4$ nonpolar whereas ${\mathrm{CH}}_3\mathrm{Cl}$ is polar?

Why is ${\mathrm{F}}_2$ a nonpolar molecule, but $\mathrm{HF}$ is a polar molecule?

Why is ${\mathrm{CCl}}_4$ a nonpolar molecule, but ${\mathrm{PCl}}_3$ is a polar molecule?

Identify each of the following molecules as polar or nonpolar:
a. ${\mathrm{CS}}_2$
b. ${\mathrm{NF}}_3$
c. ${\mathrm{CHF}}_3$
d. ${\mathrm{SO}}_3$

Identify each of the following molecules as polar or nonpolar:
a. ${\mathrm{SeF}}_2$
b. ${\mathrm{PBr}}_3$
c. ${\mathrm{SiF}}_4$
d. ${\mathrm{SO}}_2$

The molecule ${\mathrm{CO}}_2$ is nonpolar, but $\mathrm{CO}$ is a polar molecule. Explain.

Write the chemical formula for each of the following:
 a. Magnesium sulfate
 b.  Tin(II) fluoride
 c. Aluminum hydroxide

Write the chemical formula for each of the following:
 a. Calcium carbonate
 b. Carbon dioxide
 c. Iron(II) sulfate

Identify each of the compounds in problem 6.89 as ionic or molecular.

Identify each of the compounds in problem 6.90 as ionic or molecular.

a. How does the octet rule explain the formation of a magnesium ion? 
 b. What noble gas has the same electron arrangement as the magnesium ion?
c. Why are Group $1A\left(1\right)$ and Group $\left(2\right)$ elements found in many compounds, but not Group $8A\left(18\right)$ elements?

Identify each of the following atoms or ions: $(6.1)$

Identify each of the following atoms or ions: $(6.1)$

a. How does the octet rule explain the formation of a chloride ion? 
 b. What noble gas has the same electron arrangement as the chloride ion?
c. Why are Group $7A\left(17\right)$  elements found in many compounds, but not Group   $8A\left(18\right)$ elements?

Consider the following Lewis symbols for elements X and Y: 

a. What are the group numbers of X and Y?

b. Will a compound of X and Y be ionic or molecular?

c. What ions would be formed by X and Y?

d. What would be the formula of a compound of X and Y?

e. What would be the formula of a compound of X and sulfur?

f. What would be the formula of a compound of Y and chlorine?

g. Is the compound in part f ionic or molecular?

Consider the following Lewis symbols for elements X and Y: 

a. What are the group numbers of X and Y?

b. Will a compound of X and Y be ionic or molecular?

c. What ions would be formed by X and Y?

d. What would be the formula of a compound of X and Y?

e. What would be the formula of a compound of X and sulfur?

f. What would be the formula of a compound of Y and chlorine?

g. Is the compound in part f ionic or molecular?