Ionic and Molecular Compounds

Using each of the following electron arrangements, give the formulas for the cation and anion that form, the formula for the compound they form, and its name. 

Using each of the following electron arrangements, give the formulas for the cation and anion that form, the formula for the compound they form, and its name. 

State the number of valence electrons, bonding pairs, and lone pairs in each of the following Lewis structures:

State the number of valence electrons, bonding pairs, and lone pairs in each of the following Lewis structures: 

Match each of the Lewis structures (a to c) with the correct diagram (1 to 3) of its shape, and name the shape; indicate if each molecule is polar or non-polar. Assume X and Y are non-metals and all bonds are polar covalent.

Write the name for the following: 

a. $N^{3-}$ 

b. $M{g}^{2+}$

c. $O^{2-}$

d. $A{l}^{3+}$

Write the name for the following: 

a. $K^{+}$

b. $N{a}^{+}$

c. $B{a}^{2+}$

d. $C{l}^{-}$

Write the formula for each of the following ionic compounds: $(6.2,6.3)$

a. tin(II) sulfide

b. lead(IV) oxide

c. silver chloride

d. calcium nitride

e. copper(I) phosphide

f. chromium(II) bromide

Consider the following bonds: $\mathrm{Ca} \mathrm{and} \mathrm{O},\mathrm{C} \mathrm{and} \mathrm{O}, \mathrm{K} \mathrm{and} \mathrm{O}, \mathrm{O} \mathrm{and} \mathrm{O}, \mathrm{N} \mathrm{and} \mathrm{O}$.

(a) Which bonds are polar covalent ?

(b) Which bonds are non polar covalent ?

(c) Which bonds are ionic?

(d) Arrange the covalent bonds in order of decreasing polarity.

Consider the following bonds : $\mathrm{F} \mathrm{and} \mathrm{Cl}, \mathrm{Cl} \mathrm{and} \mathrm{Cl} , \mathrm{Cs} \mathrm{and} \mathrm{Cl} , \mathrm{O} \mathrm{and} \mathrm{Cl}, \mathrm{Ca} \mathrm{and} \mathrm{Cl}.$

(a) Which bonds are polar covalent ?

(b) Which bonds are non polar covalent ?

(c) Which bonds are ionic?

(d) Arrange the covalent bonds in order of decreasing polarity.

Write the formula for each of the following ionic compounds: $(6.2,6.3)$

(a) nickel(III) oxide

(b) iron(III) sulfide

(c) lead(II) sulfate

(d) chromium(III) iodide

(e)  lithium nitride

(f) gold(I) oxide

Name each of the following molecular compounds: $(6.5)$

(a) $NC{l}_3$ (b) $N_2{S}_3$ (c) $N_{2}O$ (d) $IF$ (e) $B{F}_3$ (f) $P_2{O}_5$

Consider an ion with the symbol $X^{2+}$ formed from a representative

element.

a. What is the group number of the element?

b. What is the Lewis symbol of the element?

c. If $X$ is in Period $3$, what is the element?

d. What is the formula of the compound formed from $X$ and

the nitride ion?

Consider an ion with the symbol  $Y^{3-}$formed from a representative element.

a. What is the group number of the element?

b. What is the Lewis symbol of the element?

c. If $Y$ is in Period $3$, what is the element?

d. What is the formula of the compound formed from $Y$and

the barium ion?

One of the ions of tin is tin(IV).

a. What is the symbol for this ion?

b. How many protons and electrons are in the ion?

c. What is the formula of tin(IV) oxide?

d. What is the formula of tin(IV} phosphate?

Name each of the following molecular compounds: (6.5)

(a) $C{F}_4$ (b) $S{F}_6$ (c) $BrCl$ (d) $N_2{O}_4$ (e) $S{O}_2$ (f) $C{S}_2$

Determine the total number of valence electrons in each of the

following:                                                                                                               

a. ${\mathrm{HNO}}_2$

b. ${\mathrm{CH}}_3\mathrm{CHO}$

c. ${\mathrm{CH}}_3{\mathrm{NH}}_2$

Determine the total number of valence electrons in each of the

following:

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

b. ${\mathrm{N}}_2\mathrm{O}$

c. ${\mathrm{SeCl}}_2$

Write the formula for each of the following molecular compounds: $(6.5)$

a. carbon sulfide

b. diphosphorus pentoxide

c. dihydrogen sulfide

d. sulfur dichloride

Write the formula for each of the following molecular compounds: $(6.5)$

a. silicon dioxide

b. carbon tetrabromide

c. diphosphorus tetraiodide

d. dinitrogen trioxide

Classify each of the following as ionic or molecular, and give its name: (6.3,6.5)

a. $FeC{l}_3$ b. $N{a}_{2}S{O}_4$ c. $N{O}_2$ d. $R{b}_{2}S$ e. $P{F}_5$ f. $C{F}_4$

Classify each of the following as ionic or molecular, and give its name: $(6.3,6.5)$

(a) $A{l}_2{\left(C{O}_3\right)}_3$ (b) $CI{F}_5$ (c) $BC{l}_3$ (d) $M{g}_3{N}_2$ (e) $CI{O}_2$ (f) $CrP{O}_4$

Match each of the formulas (a to c) with the correct diagram (1 to 3) of its shape, and name the shape; indicate if each molecule is polar or non-polar. 

Write the formula for each of the following: $(6.3,6.4,6.5)$

a. tin(II) carbonate

b. lithium phosphide

c. silicon tetrachloride

d. manganese(III) oxide

e. tetraphosphorus triselenide 

f. calcium bromide 

Write the formula for each of the following: $(6.3,6.4,6.5)$

a. sodium carbonate

b. nitrogen dioxide

c. aluminum nitrate

d. copper(I) nitride

e. potassium phosphate

f. cobalt(III) sulfate

Identify the major intermolecular forces between each of the following atoms or molecules: ($6.9$)

a. data-custom-editor="chemistry" $\mathrm{He}$

b. $HBr$

c. $Sn{H}_4$

d. data-custom-editor="chemistry" ${\mathrm{CH}}_3-{\mathrm{CH}}_2-{\mathrm{CH}}_2-\mathrm{OH}$

One of the ions of gold is gold($III$). ($6.1, 6.2, 6.3, 6.4$)

a. What is the symbol for this ion?

b. How many protons and electrons are in the ion?

c. What is the formula of gold($III$) sulfate? 

d. What is the formula of gold($III$) nitrate?

Identify the major intermolecular forces between each of the

following atoms or molecules:

a. $P{H}_3$

 b. $N{O}_2$

c. $C{H}_{3_{}}N{H}_2$

d. $Ar$

Select the more polar bond in each of the following pairs.$\left(6.7\right)$

a. $\mathrm{C}-\mathrm{C} \mathrm{or} \mathrm{C}-\mathrm{O}$

b. $\mathrm{P}-\mathrm{Cl} \mathrm{or} \mathrm{P}-\mathrm{Br}$

c. $\mathrm{Si}-\mathrm{S} \mathrm{or} \mathrm{Si}-\mathrm{Cl}$

d. $\mathrm{F}-\mathrm{Cl} \mathrm{or} \mathrm{F}-\mathrm{Br}$

e. $\mathrm{P}-\mathrm{O} \mathrm{or} \mathrm{P}-\mathrm{S}$

Draw the Lewis structure for each of the following:

a. ${\mathrm{Cl}}_2\mathrm{O}$

b. ${\mathrm{H}}_2\mathrm{NOH}$($\mathrm{N}$ is the central atom)

c. ${\mathrm{H}}_2{\mathrm{CCCl}}_2$

Calculate the electronegativity difference and classify each of the following bonds as nonpolar covalent, polar covalent, or ionic:

a. $Si and Cl$                  b. $C and C$                c. $Na and Cl$

d. $C and H$                  e. $F and F$.

Calculate the electronegativity difference and classify each of the following bonds as nonpolar covalent, polar covalent, or ionic: 

a. $C and N$                b. $Cl and Cl$                 c. $K and Br$

d. $H and H$                e. $N and F$.

Show the dipole arrow for each of the following bonds: $(6.7)$

a. $Si-Cl$

b. $C-N$

c. $F-Cl$

d. $C-F$

e. $N-O$

Show the dipole arrow for each of the following bonds:  $(6.7)$

a. $P-O$

b. $N-F$

c. $O-Cl$

d. $S-Cl$

e. $P-F$

Predict the shape and polarity of each of the following molecules, which have polar covalent bonds:$(6.8 , 6.9)$

a. A central atom with three identical bonded atoms and one lone pair.

b. A central atom with two bonded atoms and two lone pairs.

Predict the shape and polarity of each of the following molecules, which have polar covalent bonds: $(6.8 , 6.9)$

a. A central atom with four identical bonded atoms and no lone pairs.

b. A central atom with four bonded atoms that are not identical and no lone pairs.

Identify the group number in the periodic table of $X$, a representative element, in each of the following ionic compounds:$(6.2)$

a. $X_2{O}_3$

b. $X_{2}S{O}_3$

c. $N{a}_{3}X$

Identify the group number in the periodic table of $X$ , a representative element, in each of the following ionic compounds: $(6.2)$

a. $XC{l}_3$

b. $A{l}_2{X}_3$

c. $XC{O}_3$

Complete the following table for atoms or ions: 

Complete the following table for atoms or ions: $(6.1)$

For each of the following, draw the Lewis structure and determine the shape: $(6.6 , 6.8)$

a. $N{F}_3$

b. $SiB{r}_4$

c. $CS{e}_2$

Draw the Lewis structure for each of the following: ($6.6$)

a. data-custom-editor="chemistry" ${\mathrm{H}}_3{\mathrm{COCH}}_3$(the atoms are in the order data-custom-editor="chemistry" $\mathrm{C} \mathrm{O} \mathrm{C}$)

b. data-custom-editor="chemistry" ${\mathrm{HNO}}_2$ (the atoms are in the order data-custom-editor="chemistry" $\mathrm{HONO}$)

c. $OB{r}_2$

Use the periodic table to arrange the following atoms in order of increasing electronegativity: ($6.7$) 

a. data-custom-editor="chemistry" $\mathrm{I}, \mathrm{F}, \mathrm{Cl}$

b.  $\mathrm{Li}, \mathrm{K}, \mathrm{S}, \mathrm{CI}$

c. data-custom-editor="chemistry" $\mathrm{Mg}, \mathrm{Sr}, \mathrm{Ba}, \mathrm{Be}$

Use the periodic table to arrange the following atoms in order of increasing electronegativity: ($6.7$) 

a. data-custom-editor="chemistry" $\mathrm{Cl}, \mathrm{Br}, \mathrm{Se}$ 

b. data-custom-editor="chemistry" $\mathrm{Na}, \mathrm{Cs}, \mathrm{O}, \mathrm{S}$

c. data-custom-editor="chemistry" $\mathrm{O}, \mathrm{F}, \mathrm{B}, \mathrm{Li}$

Select the more polar bond in each of the following pairs: ($6.7$) 

a. data-custom-editor="chemistry" $\mathrm{C}-\mathrm{N}$ or data-custom-editor="chemistry" $\mathrm{C}-\mathrm{O}$ 

b. data-custom-editor="chemistry" $\mathrm{N}-\mathrm{F}$ or data-custom-editor="chemistry" $\mathrm{N}-\mathrm{Br}$

c. data-custom-editor="chemistry" $\mathrm{Br}-\mathrm{Cl}$ or data-custom-editor="chemistry" $\mathrm{S}-\mathrm{Cl}$

d. data-custom-editor="chemistry" $\mathrm{Br}-\mathrm{Cl}$ or data-custom-editor="chemistry" $\mathrm{Br}-\mathrm{I}$

e. data-custom-editor="chemistry" $\mathrm{N}-\mathrm{F}$ or data-custom-editor="chemistry" $\mathrm{N}-\mathrm{O}$

For each of the following, draw the Lewis structure and determine the shape:  $(6.6, 6.8)$

a. $COC{l}_2$($C$ is the central atom)

b. $HCCH$

c. $S{O}_2$

Use the Lewis structure to determine the shape of the following: $(6.6 ,6.8)$

a. $CB{r}_4$

b. $H_{2}O$

Use the Lewis structure to determine the shape of the following: $(6.6 , 6.8 )$

a. $P{H}_3$

b. $HCN$

Classify each of the following as ionic or molecular, and name each.

a. Li₃HPO₂

b. ClF₃

c. Mg(ClO₃)₂

d. NF₃

e. Ca(HSO₄)₂

f. KClO₂

g. Au₂(SO₃)₃

Complete the Lewis structure for each of the following: $(6.6)$

a.

b. 

c.

d.