ALKANES

1. Draw structural formula for:

a) 2,2,4-trimethylpentane b) 3,4-diethylheptane

See 4. a) See 4. b)

c) 3-methylheptane d) 4-ethyl-3-methylheptane

See 4. c) See 4. d)

e) 3-chloro-2-methylhexane f) 2-chloro-2-methylpentane

See 4. e) See 4. f)

g) 4-bromo-5-iodo-2,2,3-trimethylhexane h) 5,6-dichloro-3-ethyl-2,3-dimethyloctane

See 4. g) See 4. h)

2. Draw and name 3 isomers of C5H12.

• have the same chemical formula, but different structures – different branching.

n - pentane 2 – methylbutane 2,2-dimethylpropane

3. Which compound has the higher melting point: propane or pentane? Explain.

n – pentane has the higher melting point as the molecule can pack closer together causing stronger London

Dispersion forces. More energy is needed to overcome these forces and allow the molecules to move

further apart and melt.

C C C C C

C C C C

C

C C C

C

C

4. Name the following:

a)

See 1. a)

b)

See 1. b)

c)

See 1. c)

d)

See 1. d)

e)

See 1. e)

f)

See 1. f)

g)

See 1. g)

h)

See 1. h)

CH3 C CH CH CH CH3

CH3

CH3

CH3 Br

I

CH3 CH CH2 C CH3

CH3

CH3

CH3

CH3 CH2 CH

CH2CH3

CH CH2 CH2 CH3

CH2 CH3

CH3 CH2 CH2 CH2 CH CH3

CH2CH3

CH3 CH2 CH CH CH2 CH2 CH2 CH3

CH3 CH2 CH3

CH3 CH CH CH2 CH2 CH3

CH3

Cl

CH3 C CH2 CH2 CH3

CH3

Cl

CH3 CH C CH2 CH CH CH2 CH3

CH3 CH3

CH2CH3 Cl

Cl

ALKENES

1. Draw structural formula for the following:

a) 2-methylpropene b) trans-2,3-dibromobut-2-ene

See 3. a) See 3. b)

c) cis-hex-3-ene d) 2-ethylpent-1-ene

See 3. c) See 3. d)

e) cis-4-chloro-5-methylhex-2-ene f) 4,4-dimethylhex-1-ene

See 3. e) See 3. f)

g) trans-3-bromo-2-iodo-4,5,5-trimethylhex-2-ene h) trans-3,4-dichloro-6-ethyl-6,7-dimethyloct-3-ene

See 3. g) See 3. h)

2. a) Draw and name the geometric isomers of C2H2Cl2.

C C

H H

Cl Cl or

C C

H H

Cl Cl cis-1,2-dichloroethane

C C

H Cl

Cl H or

C C

H Cl

Cl H trans-1,2-dichloroethane

b) Which of the two compounds above has the higher melting point? Explain.

cis-1,2-dichloroethane has the higher melting point as it is more polar than the trans isomer.

3. Name the following:

a)

See 1. a)

b)

See 1. b)

c)

See 1. c)

d)

See 1. d)

e)

See 1. e)

f)

See 1. f)

g)

See 1. g)

h)

See 1. h)

CH3 C

CH3

CH2

C C

CH3

CH3

Br

Br

CH3 CH2 C C

H H

CH2 CH3

CH3 CH2 C CH2 CH2 CH3

CH2

CH3 CH CH C C CH3

CH3

Cl

H H

CH3 C CH2 CH CH2

CH2 CH3

CH3

CH3 C CH C C CH3

CH3CH3

CH3

Br

I

CH3 CH C CH2 C C CH2 CH3

CH3

CH2CH3 Cl

ClCH3

ALKYNES

1. Draw structural formula for the following:

a) 4,5-dimethyl-2-heptane b) 3,3-dimethyl-1-butyne

See 3. a) See 3. b)

c) 4-methyl-2-pentyne d) 4-ethyl-2-hexyne

See 3. c) See 3. d)

e) 4-chloro-5-methyl-2-hexyne f) 5,5-dimethyl-1-heptyne

See 3. e) See 3. f)

g) 1-iodo-3,4,4-trimethyl-1-pentyne h) 6-ethyl-6,7-dimethyl-3-octyne

See 3. g) See 3. h)

2. a) Draw and name the isomers of C4H5Cl.

There are several, here are a few:

C C C CCl

H

H

H

H

H

C C C CH

Cl

H

H

H

H

1-chlorobut-1-ene 3-chlorobut-1-ene

C C C CH

H

H

H

H

Cl

C C C CH

H

H

Cl

H

H 4-chlorobut-1-ene 1-chlorobut-2-ene

C C C C

HH

H

H H

Cl

C C

H

H C C

H

H

Cl

H 1-chlorobuta-1,3-diene 4-chloro-1,2-butadiene

C C

H

H C C

H

H

H

Cl

C C

Cl

H C C

H

H

H

H 3-chloro-1,2-butadiene 1-chloro-1,2-butadiene

b) Which of the isomer compounds above has the higher melting point? Explain.

The dienes have more electrons and 1-chlorobuta-1,3-diene has the closest packing.

3. Name the following:

a)

See 1. a)

b)

See 1. b)

c)

See 1. c)

d)

See 1. d)

e)

See 1. e)

f)

See 1. f)

g)

See 1. g)

h)

See 1. h)

CH3 C C CH CH CH3

CH2 CH3CH3

CH C C CH3

CH3

CH3

CH3 C C CH CH3

CH3

CH3 CH2 CH C C CH3

CH2 CH3

CH3 CH CH C C CH3

Cl

CH3

CH3 C CH2 CH2 C CH

CH2 CH3

CH3

CH3 C CH C C

CH3

CH3 CH3

I

CH3 CH C CH2 C C CH2 CH3

CH3 CH3

CH2CH3

Practice Intermolecular Forces

1. For each of the molecules below complete the following:

a) Are the bonds polar?

b) Pick the most polar bond in each and indicate the positive and negative portion of the bond by using a

vector.

c) Which of these are polar molecules (have a net dipole moment)?

CH4 (a) ΔEN (CH) = 0.4 non-polar (b) no polar bonds (c) non-polar molecule

C

H

HH

H CH3OH (a) ΔEN (CO) = 1.0 ; polar, ΔEN (OH) = 1.4 ; polar (b) O-H

(c) polar molecule

C

H

OH

H

H

CO2 (a) ΔEN (CO) = 1.0 ; polar (b) both C-O (c) non-polar molecule

CO O

C2H6 (a) ΔEN (CH) = 0.4 ; non-polar (b) non-polar (c) non-polar molecule

C C

H H

H

H

H

H

CCl4 (a) ΔEN (CCl) = 0.5 ; polar (b) all C-Cl (c) non-polar molecule

C

Cl

ClCl

Cl CH3Cl (a) ΔEN (CCl) = 0.5 ; polar (b) one C-Cl (c) polar molecule

C

H

ClH

H CH3CN (a) ΔEN (CN) = 0.5 ; polar (b) C-N (c) polar molecule

C

H

CH

HN

2. a) Rank the following from substances from strongest to weakest intermolecular forces.

CH4 Cl2 CH3Cl

LD LD LD, D-D

ΔEN = 0.4 ΔEN = 0 ΔEN = 0.5

weak weakest strongest

b) What features must a molecule have to exhibit the above attractive forces?

Non-polar molecule – non-polar bond or symmetrical shape – LD only

Polar molecule – polar bond(s) and a nonsymmetrical shape – LD and D-D

c) What type of intermolecular attraction would occur between identical molecules of the following?

CH3Cl CH2CH2

D-D LD

CH3CH3 CH3OH CH3CH2OH

LD HB HB

3. Are ammonia (NH3) and water miscible? Explain

Yes, ammonia will dissolve in water as both are polar molecules and the dipoles will attract each other.

4. Indicate which compound in the following pairs would have the higher boiling point and greater water

solubility. Explain your order.

a)

HB D-D

Higher b.p.

Greater H2O solubility

b)

LD D-D

Higher b.p.

Greater H2O solubility

c) CH3CH2CH2Cl vs CH3CH2CH3

D-D LD

Higher b.p.

Greater H2O solubility

CH3 CH2 OH CH3 CH

O

vs

CH3 CH2 CH3 vs CH3 C CH3

O

BALANCING SKELETAL EQUATIONS

Balance the following skeletal equations:

a) 2 Li + 2 H2O 2 LiOH + H2

b) 2 Mg + Pb(SO4)2 2 MgSO4 + Pb

c) FeSO4 + 2 HCN Fe(CN)2 + H2SO4

d) 3 H2S + Al2(CO3)3 Al2S3 + 3 H2O + 3 CO2

e) 2 H3PO4 + 3 Ca(OH)2 Ca3(PO4)2 + 6 H2O

f) Na2O + H2O 2 NaOH

g) 4 Fe + 3 O2 2 Fe2O3

h) 2 Fe(OH)3 Fe2O3 + 3 H2O

i) C12H22O11 + 12 O2 12 CO2 + 11 H2O

BALANCING WORD EQUATIONS

Balance the following word equations:

j) iron + oxygen iron (III) oxide

4 Fe + 3 O2 2 Fe2O3

k) sodium chlorate sodium chloride + oxygen

2 NaClO3 2 NaCl + 3 O2

l) copper (II) oxide + hydrogen copper + water

CuO + H2 Cu + H2O

m) sodium hydroxide + carbon dioxide sodium carbonate + water

2 NaOH + CO2 Na2CO3 + H2O

n) hydrogen + nitrogen ammonia

3 H2 + N2 2 NH3

o) tin (IV) oxide + carbon tin + carbon monoxide

SnO2 + 2 C Sn + 2 CO

p) calcium chloride calcium + chlorine

CaCl2 Ca + Cl2

A) Synthesis Reactions For each of the following, complete and give the Balanced Chemical equation: 1. sodium + iodine sodium iodide

2 Na (s) + I2 (s) 2 NaI (s)

2. carbon + oxygen carbon dioxide

C (s) + O2 (g) CO2 (g)

3. carbon dioxide + water carbonic acid

CO2 (g) + H2O (l) H2CO3 (aq)

4. calcium + oxygen calcium oxide

2 Ca (s) + O2 (g) 2 CaO (s)

5. dinitrogen pentoxide + water nitric acid

N2O5 (g) + H2O (l) 2 HNO3 (aq)

6. calcium oxide + water calcium hydroxide

2 CaO (s) + H2O (l) Ca(OH)2 (aq)

7. sodium oxide + sulfur trioxide sodium sulfate

Na2O (s) + SO3 (g) Na2SO4 (s)

B) Decomposition Reactions

8. carbonic acid carbon dioxide + water

H2CO3 (l) CO2 (g) + H2O (l)

9. copper (II) carbonate

heat

copper (II) oxide + carbon dioxide

CuCO3 (s) CuO (s) + CO2 (g)

10. sodium bicarbonate

heat

sodium oxide + carbon dioxide + water

2 NaHCO3 (s) Na2O (s) + 2 CO2 (g) + H2O (l)

11. magnesium chloride

iselectrolys magnesium + chlorine

MgCl2 (s) Mg (s) + Cl2 (g)

C) Single Displacement Reactions For each of the following, complete and give the Balanced Chemical equation: 1. nickel + copper (II) nitrate sol’n nickel (II) nitrate sol’n + copper

Ni (s) + Cu(NO3)2 (aq) Ni(NO3)2 (aq) + Cu (s)

2. zinc + hydrochloric acid zinc chloride sol’n + hydrogen

Zn (s) + 2 HCl (aq) ZnCl2 (aq) + H2 (g)

3. barium + iron (III) chloride sol’n barium chloride sol’n + iron

3 Ba (s) + 2 FeCl3 (aq) 3 BaCl2 (aq) + 2 Fe (s)

4. aluminum + zinc hydroxide sol’n aluminum hydroxide sol’n + zinc

2 Al (s) + 3 Zn(OH)2 (aq) 2 Al(OH)3 (aq) + 3 Zn (s)

5. lead + magnesium sulfate sol’n no reaction (NR)

Pb (s) + MgSO4 (aq) NR

6. chlorine + sodium iodide sol’n sodium chloride sol’n + iodine

Cl2 (g) + 2 NaI (aq) 2 NaCl (aq) + I2 (s)

D) Double Displacement Reactions NOTE: Due to lack of space, assume all products and reactants are solutions (aq) unless

otherwise stated For each of the following, complete and give the Balanced Chemical equation: 1. silver nitrate + iron (III) chloride silver chloride solid + iron (III) nitate

3 AgNO3 (aq) + FeCl3 (aq) 3 AgCl (s) + Fe(NO3)3 (aq)

2. nitric acid + sodium carbonate sodium nitrate + carbon dioxide

+ water

2 HNO3 (aq) + Na2CO3 (aq) 2 NaNO3 (aq) + CO2 (g)

+ H2O (l)

3. phosphoric acid + potassium hydroxide potassium phosphate + water

H3PO4 (aq) + 3 KOH (aq) K3PO4 (aq) + 3 H2O (l)

4. lithium hydroxide + sulfuric acid lithium sulfate + water

2 LiOH (aq) + H2SO4 (aq) Li2SO4 (aq) + 2 H2O (l)

5. ammonium nitrate + sodium hydroxide sodium nitrate + ammonia

+ water

NH4NO3 (aq) + NaOH (aq) NaNO3 (aq) + NH3 (g)

+ H2O(l)

6. barium hydroxide + ammonium sulfate barium sulfate + ammonia

+ water

Ba(OH)2 (aq) + (NH4)2SO4 (aq) BaSO4 (aq) + 2 NH3 (g)

+ 2H2O(l)

Organic Reactions

Alkanes

1. What is the equation for the complete combustion of pentane?

C5H12 (l) + 8 O2 (g) → 5 CO2 (g) + 6 H2O (l)

2. Give an example of a cracking of an alkane.

C15H32 (l) + H2 (g) → C7H16 (l) + C8H18 (l)

3. Give the equation of the reaction of bromine with ethane.

C2H6 (g) + Br2 (l) → C2H5Br (l) + HBr (l)

C C C C C C

H

H

H

H

H

H

H

H

H

H

H H

H

H + Br Br C C C C C C

H

H

H

H

H

H

H

H

H

H

H H

H

Br + BrH

Alkenes

4. What is the equation for the complete combustion of 2-pentene?

2 C5H10 (l) + 10 O2 (g) → 5 CO2 (g) + 10 H2O (l)

5. Give the equation of the reaction of bromine with 2-hexene.

C6H12 (l) + Br2 (l) → C6H12Br2 (l)

C C C C C

H H H

H H

H

H

H

C H

H

H

H

+ Br Br C C C C C

H H H

H H

H

H

H

C H

H

H

H

Br Br

6. Give the equation of the reaction of water with propene.

C3H6 (g) + H2O (l) → C3H7OH (l)

C CH C

H

H

H

H

H + O HH C C C

H

H

H

H

OH

H

H

H

Alkynes

7. What is the equation for the complete combustion of propyne?

C3H4 (l) + 4 O2 (g) → 3 CO2 (g) + 2 H2O (l)

8. Give the equation of the reaction of hydrogen chloride with 2-hexyne.

C6H10 (l) + HCl (l) → C6H11Cl (l)

C C C C C C

H

H

H

H

H

H

H H

H

H

+ H Cl C C C C C C

H

H

H

H Cl H

H

H

H H

H

H

9. Give the equation of the reaction of water with propyne.

C3H4 (g) + H2O (l) → C3H5OH (l)

C C CH

H

H

H

+ O HH C C C

OHH

H

H

H

H

EQUATION DRILL WORKSHEET For each of the following, give the:

a) completed word equation

b) the balanced chemical equation

c) electron dot diagrams for all reactants and products d) reaction type(s) [as many classes as possible] 1. barium + iodine → barium iodide

Ba (s) + I2 (s) → BaI2 (s)

Ba I I

Synthesis, exothermic

2. dinitrogen pentoxide + water → nitric acid

N2O5 (g) H2O (l) 2 HNO3 (aq)

NO O

O

N O

O

O HH

NO O

O

H

Synthesis, exothermic

3. eg. carbon dioxide + water → carbonic acid

CO2 (g) + H2O (l) → H2CO3 (aq)

CO O O HH

CO O

O

H H

Synthesis, exothermic

4. eg. sodium oxide + water → sodium hydroxide

Na2O (s) + H2O (l) → NaOH (aq)

Synthesis, exothermic

5. sodium oxide + sulfur trioxide → sodium sulfate Na2O (s) + SO3 (g) → Na2SO4 (s)

Synthesis, exothermic

6. aluminum hydroxide

heat

aluminum oxide + water

2 Al(OH)3 (s) → Al2O3 (s) + 2 H2O (l)

Ba 2+

I -

2

Na +

O 2-

2Na

+OH

-

O HH

Na +

O 2-

2SO O

O

SO O

O

O

Na+

2

Decomposition, endothermic

7. copper (II) carbonate

heat

copper (II) oxide + carbon dioxide

CuCO3 (s) → CuO (s) + CO2 (g)

Decomposition, endothermic 8. nickel + copper (II) nitrate sol’n → nickel (II) nitrate + copper

Ni (s) + Cu(NO3)2 (aq) → Ni(NO3)2 (aq) + Cu (s)

Single Displacement 9. zinc + potassium hydroxide sol’n → No Reaction (NR)

Zn (s) + KOH (aq) → NR

Single Displacement 10. chlorine + gallium iodide sol’n → gallium chloride + iodine

Cl2 (g) + 2 GaI3 (s) → GaCl3 (s) + 3 I2 (s)

Single Displacement 11. magnesium sulfide sol’n + iron (III) chloride sol’n → iron (III) sulfide + magnesium chloride sol’n

3 MgS (aq) + FeCl3 (aq) → Fe2S3 (s) + 3 MgCl2 (aq)

Double Displacement

12. aluminum chloride sol’n + sodium carbonate sol’n → sodium chloride sol’n + aluminum oxide +

carbon dioxide “boiled dry and then heated”

Al 3+

3OH

-Al

3+O

2-

2 3O HH

CO O

O 2-

Cu 2+ Cu

2+O

2-CO O

Ni Cu 2+

2NO O

O 1-

Ni 2+

2NO O

O 1-

Cu

Zn K +

OH -

Cl Cl Ga 3+ Cl

-

3Ga

3+ I -

3

Mg 2+

S 2-

Fe 3+ Cl

-

3Fe

3+S

2-

2 3Mg

2+Cl

-

2

I I

Na +

Cl -

2 AlCl3 (aq) + 3 Na2CO3 (aq)

heat

6NaCl (s) + Al2O3 (s) + 3 CO2

(g)

Double Displacement, Decomposition

13. phosphoric acid + potassium hydroxide sol’n → potassium phosphate + water H3PO4 (aq) + 3 KOH (aq) → K3PO4 (aq) + 3 H2O (l)

Double Displacement 14. lithium hydroxide sol’n + sulfur trioxide gas → lithium hydrogen sulfate

LiOH (aq) + SO3 (g) → LiHSO4 (s)

Synthesis, Exothermic 15. ammonium chloride sol’n + calcium hydroxide sol’n → calcium chloride sol’n + ammonium + water

2 NH4Cl (aq) + Ca(OH)2 (aq) → CaCl2 (aq) + 2 NH3 (g) + 2 H2O (l)

Double Displacement, Decomposition 16. barium hydroxide sol’n + ammonium sulphate sol’n → barium sulfate + ammonia + water

Ba(OH)2 (aq) + (NH4)2SO4 (aq) → BaSO4 (s) + 2 NH3 (g) + 2 H2O (l)

Double Displacement, Decomposition

Al 3+ Cl

-

3CO O

O 2-

Na+

2

Al 3+

O 2-

2 3

PO O

O

O

H H

H

K +

OH -

PO O

O

O

3-

K +

3

O HH

Li +

OH -

SO O

O

SO O

O

O

H

1-

Li +

CO O

N+

H

H

H

H

Cl - Ca

2+

2OH

- Ca 2+

Cl -

2N H

H

H O HH

N+

H

H

H

H

2

SO O

O

O

Ba 2+

2OH

-N H

H

HSO O

O

O

2-

Ba 2+

O HH