Study Guide
Unit III – Chapter 11
Answer Key
Review questions Write all the work for these problem on separate paper.
1.
2.
3.
4.
5.
What is the Law of Conservation of Mass (Matter) and why is it important to chemist:
Mass cannot be created or destroyed, but atoms can only be rearranged. Chemists keep track of
all atoms in a system (Chemical Reaction) and use Coefficients to balance the reactants and
products to have equal atoms on the reactant and product side of the equation.
List the four signals of a chemical reaction:
a. Color Change
b. Precipitate formed (solid)
c. Gas evolved (no heating)
d. Temperature Change (kinetic energy is released from or absorbed into the chemical
bonds)
Compounds and/or elements before the arrow (to the left) are called _Reactants_________
Compounds and/or elements after the arrow (to the right) are called __Products________
Which elements are diatomic in nature: Hydrogen (H2), Nitrogen (N2), Oxygen (O2), all VII A
(Halogens), Fluorine (F2), Chlorine (Cl2), Bromine (Br 2), Iodine (I2).
How is an ionic compound different from an acid compound?
An Ionic is a metal (+) cation with a non-metal (-) anion. An Acid is a Hydrogen ion (H1+) with an
anion (-)
6.
What are the rules for naming acids?
Ending
ate
ic
ite
ous
ide
7.
9.
10.
hydro
ic
What does each symbol mean:
+
→
∆
─ Pt →
8.
change to
And
Yields
Heat
catalysts
(s)
(l)
(g)
(aq)
Solid
Liquid
Gas
aqueous
What is a catalyst? It is a substance that speeds up a chemical reaction, but it is not a reactant
or a product (it is not used up when the reaction occurs).
Which element has the highest electronegativity? Fluorine
Which group of elements does not have electronegativity? Nobel Gases
Explain the trend for electronegativity for a group (from top to bottom) gets lower (less able to
gain an electron during bonding) and for a period (left to right). Electronegativity gets larger
(more able to gain an e- during bonding)
Know the difference between a Cation (+) and an Anion (-). Cation is made from metals (mostly)
and it is an atom that has lost e- and has become a positively charged ion. An Anion is a usually a
non-metal atom that has gained e- to become a negatively charged ion.
Be sure to know what happens to the charge of an atom, when the electrons are lost or gained
respectively. Answered above
10.
O2
HClO
Fe(SO4)
I2
Al2(CO3)3
Na(C2H3O2)
H2SO4
CO2
K2CrO4
Ag(NO3)
ZnO
H 2O
Name
_________Oxygen_________________________
_________Hypochlorous Acid_________________
______Iron(II) Sulfate_______________
_______________________Iodine____
_______Aluminum Carbonate_____________
_____________Sodium Acetate_______
_______Sulfuric Acid________________
_________________Carbon Dioxide___
_____Potassium Chromate______________
_______________Silver Nitrate______
_____Zinc Oxide___________________
_____________Water______________
Then you will also need to be able to write the formula from the name!
11.
Thinking
Formula
Silver hydroxide
________________
____Ag(OH)_
Nitrous Acid
________________
_______HNO2___
Carbonic acid
________________
____H2CO3____
Carbon Dioxide
________________
CO2_________
Hydrochloric acid
________________
_______HCl___
Calcium carbonate
________________
__CaCO3_____
Lithium chlorate
________________
_______LiClO3_
Hydrogen gas
________________
_______H2____
Lead (II) phosphate
________________
_Pb3(PO4)2____
Barium sulfate
________________
_____BaSO4_____
12.
List all of the compounds from question #10 and #11 that would dissociate in water?
[Hint: use the solubility table]:All of the following would become [aqueous (aq)]
#11. HClO, Fe(SO4), Na(C2H3O2), H2SO4, K2CrO4, Ag(NO3), and for # 12. Nitrous Acid (HNO2),
Carbonic Acid (H2CO3), Hydrochloric Acid (HCl), Lithium Chlorate (LiClO3),
13.
From the pairs given below choose the metal that is more reactive. [Hint use the reactivity of
metals table (back of periodic table or p. 333)]
a. Li or Cu
b. Ag or Cu
c. Mg or K
14.
d. Al or Zn
e. Pb or Ca
f. Hydrogen (H2) or Cu
a.
Balance the following equations, using coefficients. Also identify the type of chemical reaction it
equation represents (combination, decomposition, single replacement, double replacement, or
combustion).
__2_ H2O2

__2__ H2O + ____ O2
type: __Decompostion___
b.
_3_ Zn + _2__ H3(PO4) 
c.
__2_ Ag(NO3) + __ PbI2
d.
_4__Al
+
_3__ O2
___ Zn3(PO4)2
 __ Pb(NO3)2
 __2_ Al2O3
+ _3_ H2
+ _2_ AgI
__Single Replacement__
_Double Replacement__
___Combination_______
e._ Ca(OH)2
f.
+ _2_ HCl
 __ CaCl2
+ _2_ H(OH)
___ Na2O +
___ H2O ——→
metal oxide and water yields
(actually H2O) __Double Replacement___
__2_ Na(OH)
a base
t
_____Decompostion_____
Practice Chemical Equations
(finishing, balancing and identifying)
Type:
15.
Al(s) +
__Combination_____
16.
Mg
17.
Ca(s) +
18.
Cu(NO3)2 (aq) +
19.
O2 (g)
+
Ca(NO3)2  __NO Reaction _ + Check Activity Series _ _Single Replacement___
N2O3
Mg(NO3)2(aq)  ___Ca(NO3)2 (aq) +
+
H 2O
K2CO3(s) 
21.
Zn
22.
Al2(SO4)3(aq) +
23.
24.
+
__HNO2 (aq)____

___K2O(s)_____ +
HCl
(aq)
 ___ZnCl2 (aq) +
_H2 (g)_
25.
2 NH3 (g)
26.
NaCl(aq) +

N2 (g)
H 2O
+
O2
+
3 H2 (g)
K(NO3)(aq)  NaCl(aq) +
__Double Replacement____
___Decomposition___
_Single Replacement __
3 Ca(OH)2(aq)  _2_Al(OH)3(s) + 3 Ca(SO4)(s)
----Fe3+--
___Single Replacement____
__Combination_______
__CO2 (g)____
C12H22O11 (s) + 12 O2(g)  _12_CO2 (g)_ +
H2O2 (aq)
___Mg(s)___
Na2S(aq)  ___CuS (s)__ + __2_NaNO3 (aq)
20.
(s)
___Al2O3 (s)_

_11_H2O (l)_
_Double Replacement___
___Combustion __
__Decomposition___
(g)
__Decompostion____
KCl(aq)
No Reaction, because all the reactants and
products are aqueous.
Double Check – for questions 15 – 25 were there some combinations that would be No Reaction?
[Hint use the Solubility Table and Activity Series of Metals Table]
Word Equations:
Write the reactants and the products and then balance, also list the type of reaction that each is:
27.
Solid Copper, plus Oxygen gas in a flame yields –
2 Cu (s) + O2 (g)

2 CuO (s)
Combination
28.
Zinc metal and Sulfuric Acid yields –
Zn(s) + H2(SO4) (aq) 
Zn(SO4) (aq) +
H2 (g)
Single Replacement
29.
Magnesium nitrate solution and Sodium hydroxide solution placed together in a test tube yields –
Mg(NO3)2(aq) + 2 Na(OH) (aq)

Mg(OH)2 (s) + 2 Na(NO3) (aq)
Double Replaement
30.
Copper (II) Carbonate is heated and yields –
Cu(CO3) (s)
 CuO (s) + CO2(g)
Decomposition
31.
Methane from the Bunsen burner is reacted with oxygen in the air and yields
CH4 (g)
+
2 O2 (g)

CO2 (g)
+
2 H2O (l)
Combustion
32.
Lithium metal and water yields –
Li(s) +
H2O (l)
Think of water as
H(OH)
33.
34.
35.
36.
Li(OH)

Hydrochloric acid and aluminum hydroxide yields –
3 HCl (aq) +
Al(OH)3

3 H(OH)
+
Water
(aq)
+
H2 (g)
AlCl3
Sulfur dioxide gas (SO2) and water yields –
SO2 (g)
+
H2O (l) 
H2SO3 (aq)
Non-metal plus water
makes an acid
Oxide
Copper Hydroxide is heated and yields –
Cu(OH)2 (s) 
CuO (s) + H2O(l)
Burning sugar (C12H22O11) produces –
C12H22O11 + 12 O2(g)  11 H2O(l)
+
Single Replacement
Double Replacment
Combination
Decomposition
12 CO2(g)
Combustion
37.
Calcium nitrate solution is mixed with sodium phosphate solution and yields 3 Ca(NO3)2 (aq) + 2 Na3(PO4) (aq) 
Ca3(PO4)2 (s)
+
6Na(NO3) (aq)
38.
Explain how to test for each of the following gases:
Hydrogen (H2): Use a lit wooden splint if it pops (explodes) it is hydrogen.
Oxygen (O2): Use a glowing splint if it relights it is oxygen.
Carbon Dioxide (CO2): Use a lit or glowing splint if it goes out it is carbon dioxide.
39.
c.
Sn + 4HNO3 
 SnO2 + 4NO2 + 2H2O
40.
a.
Fluorine
41.
c.
helium
42.
c.
Pb(SO4)
43.
The following reaction is balanced
Sn + 4HNO3 → SnO2 + 4NO2 + 2H2O
true
44.
d.
combination
45.
d.
rearranged or spread apart but can be accounted for
46.
NaI (aq)
+
Pb(NO3)2 (aq)

PbI2 (s) +
Na(NO3) (aq)
+
47.

Correctly balance the equation below and then draw the way the particles are arranged in the
provided beakers.
Mg (s)
+
+
HCl
(aq)
MgCl2 (aq)

+
H2 (g)

SOLUBILITY RULES
(solubility in water)
All alkali metal compounds are soluble in water.
All nitrates are soluble in water.
All acetates are soluble in water, except when they contain Ag +1.
All NH4+ compounds are soluble.
All chlorates are soluble.
All chlorides, bromides, and iodides are soluble except those containing Ag+, Hg+2, and Pb+2.
All sulfates are soluble except those containing Sr +2, Ba+2, and Pb+2.
All carbonates and phosphates are insoluble in water, except those containing alkali metals and NH 4+1.
All hydroxides and sulfides are insoluble, except those containing alkali metals and ones containing NH 4+1,
Sr+2, Ba+2, and Ca+2.
PREDICTING CHEMICAL REACTIONS
Metallic carbonates break into metallic oxides and carbon dioxide.
Metallic chlorates break into metallic chlorides and oxygen.
Cation (+) Peroxides break into Cation oxides and oxygen.
A non-metal oxide and water produce an acid.
Some acids break into non-metallic oxides and water (H2CO3 and H2SO3)
A metal oxide and water produce a base or a hydroxide.
Metallic hydroxides break into metallic oxides and water.
A metal oxide and a non-metal oxide produce an ionic compound.