Download Practice Qs - Unit 6a

Unit 6a Question Packet
Chemical Formulas & Equations
Name ……………………………………………
Period ………….
SKILLS
1.
2.
3.
4.
counting ATOMS IN FORMULAS
counting IONS IN IONIC FORMULAS
identifying MOLECULAR & EMPIRICAL FORMULAS
NAMES TO FORMULAS and FORMULAS TO NAMES
SKILL #1:
5. BALANCING EQUATIONS
6. applying the LAW OF CONSERVATION OF MASS
7. identifying TYPES OF REACTIONS
- refer to your notes & RB p. 73 & 87
COUNTING ATOMS IN FORMULAS
1. Fill in the table below. Put an “M” if the substance is molecular/covalent, an “I” if ionic,
and an “H” if a hydrate.
Total
Total
Formula
Moles of each
moles of
Formula
Moles of each
moles of
atom
atoms
atom
atoms
HClO3
1 mol H atoms
CaCl2
1 mol Ca atoms
a.
1 mol Cl atoms
5
f.
3
2 mol Cl atoms
3 mol O atoms
NH4C2H3O2
1 mol N atoms
Mg3(PO4)2
3 mol Mg atoms
7 mol H atoms
b.
12
g.
2 mol P atoms
13
2 mol C atoms
8 mol O atoms
2 mol O atoms
Mg(OH)2
1 mol Mg atoms
CH3CH2CH3
3 mol C atoms
c.
2 mol C atoms
5
h.
6
8 mol H atoms
2 mol C atoms
LiCl4H2O
1 mol Li atoms
Al(SCN)3
1 mol Al atoms
1 mol Cl atoms
3 mol S atoms
d.
14
i.
10
8 mol H atoms
3 mol C atoms
4 mol O atoms
3 mol N atoms
NH4Cl5H2O
CH3COOH
1 mol N atoms
2 mol C atoms
1 mol Cl atoms
e.
8
j.
21
4 mol H atoms
14 mol H atoms
2 mol O atoms
5 mol O atoms
SKILL #2:
counting IONS IN IONIC FORMULAS
- refer to your notes, RB p. 73, and Table E!
2. Complete the table below. Use Table E!!!
Ionic
Compound
Cation
(+ ion)
Anion
(- ion)
Total moles
of ions
Ionic
Compound
Cation
(+ ion)
Anion
(- ion)
Total moles
of ions
a.
NH4C2H3O2
NH4+
C2H3O2–
2
e.
CaF2
Ca2+
F–
3
b.
Ba(NO3)2
Ba2+
NO3–
3
f.
Al2O3
Al3+
O2–
5
c.
Li2CO3
Li+
CO32–
3
g.
KMnO4
K+
MnO4–
2
d.
NaHCO3
Na+
HCO3–
2
h.
(NH4)3PO4
NH4+
PO43–
4
SKILL #3:
– refer to your notes & RB p. 74
identifying MOLECULAR & EMPIRICAL FORMULAS
3. Below are a list of formulas. Write the empirical formula (if not already empirical).
SKILL #4:
a. C4H10
b. C3H6
c.
N2O4
d. Na2SO4
e.
C6H10
f.
Al2O3
g.
NH4NO3
h.
C11H22O11
i.
K2S2O3
j.
S2O4
k.
CH4
l.
C6H12Cl2O2
– refer to your notes & RB p. 75-78
NAMES TO FORMULAS and FORMULAS TO NAMES
4. Write formulas for the following ionic substances.
Name
Formula
sodium
chloride
aluminum
oxide
barium
iodide
gallium
nitride
Name
Formula
zinc
sulfide
potassium
fluoride
lithium
bromide
strontium
chloride
5. What do the ionic compounds in #4 all have in common? How are they named?
They all contain two elements only.
Metal: always first (element name)
Nonmetal: element root w/ -ide ending
6. Write formulas for the following ionic substances. Use Table E.
Name
Formula
sodium
sulfate
aluminum
chromate
magnesium
hydrogen
carbonate
lithium
permanganate
rubidium
oxalate
Name
Formula
barium
phosphate
calcium
hydroxide
potassium
hydrogen
sulfate
ammonium
chloride
sodium
acetate
7. What do the ionic compounds in #6 all have in common? How are they named?
They all contain polyatomic ions.
+ ion: always first (element name or ammonium)
- ion: second (name on Table E)
8. Write formulas for the following ionic substances. Use Table E if needed.
Name
Formula
Name
lead(II)
iodide
copper(I)
nitrate
iron(III)
sulfate
chromium(V)
chloride
platinum(II)
oxide
Formula
manganese(III)
oxide
copper(II)
nitrate
gold(III)
oxide
titanium(IV)
phosphide
iron(II)
hydroxide
9. What do the ionic compounds in #8 all have in common? How are they named?
They all contain metals w/ more than 1 possible charge (oxidation state).
+ ion: always first (element name or ammonium
Charge of metal ion goes as Roman numeral in ( )
- ion: second (name on Table E or root / ide ending)
10. Write IUPAC names the following ionic compounds.
Name
Formula
Name
Formula
LiBr
PbSO4
Ag2O
NaHCO3
Ba3N2
Ni2(SO4)3
SnO
Ti2O3
Mg(NO3)2
Al2(SO3)3
Cu3P
Al(CN)3
Co2O3
NH4Cl
AgBr
KNO3
NaNO3
CaCO3
KI
(NH4)2CO3
NaClO
NaS2O3
Fe(OH)3
YBr3
11. Write formulas for the following molecular substances.
Name
Formula
dinitrogen
trioxide
diphosphorus
pentoxide
sulfur
dioxide
silicon
dioxide
xenon
hexafluoride
tetraphosphorus
decoxide
Name
Formula
silicon
tetrafluoride
carbon
tetrachloride
boron
triiodide
carbon
disulfide
phosphorus
pentabromide
boron
trihydride
12. Write IUPAC names for the following molecular substances.
Name
SKILL #5:
Formula
Name
Formula
N2O5
H2S
SF6
BF3
PBr3
PH3
SO3
H2O
B2H4
Cl2
– refer to your notes & RB p. 79, 81
BALANCING EQUATIONS
13. Balance the following equations using the smallest, whole-number coefficients.
a.
____Mg
+
____Mn2O3

____MgO
+
____Mn
b.
_____C6H12O6  _____C2H5OH + _____CO2
c.
_____C3H8 +
____ O2
 ____ H2O
+ ____ CO2
d.
____FeCl3
e.
+ ____Be3(PO4)2
____NH3 +
____O2


____BeCl2
____N2 +
+
____FePO4
____H2O
f.
____ C2H4O2 + ____ PCl3  ____ C2H3OCl + ____ H3PO3
*g.
_____Fe2O3 + _____CO  ____Fe + ____CO2
SKILL #6:
– refer to your notes & RB p. 81
applying the LAW OF CONSERVATION OF MASS
14. Given the reaction:
2H2 + O2  2H2O
What is the total mass of water formed when 8 grams of hydrogen reacts completely
with 64 grams of oxygen?
15. When glucose is fermented, it produces ethanol and carbon dioxide. If 60.0 grams of
glucose is fermented and produces 16.5 grams of carbon dioxide gas, what mass of
ethanol is produced?
16. A 4.86-gram sample of calcium reacted completely with oxygen to form 6.80 grams of
calcium oxide. This reaction is represented by the balanced equation below.
2Ca(s) + O2(g)  2CaO(s)
Determine the total mass of oxygen that reacted.
17. Given the following incomplete equations, write the formula of the molecule represented
by X.
a.
X + Cl2  C2H5Cl + HCl
b.
4Fe + 3O2  2X
18. Which equation represents conservation of mass?
(1) H2 + Cl2  HCl
(2) H2 + Cl2 2HCl
(3) H2 + O2  H2O
SKILL # 7:
(4) H2 + O2  2H2O
– refer to your notes & RB p. 80
identifying TYPES OF REACTIONS
19. Complete the table below.
Equation
a.
Cl2 + 2NaI  2NaCl + I2
b.
HNO3 + LiOH  H2O + LiNO3
c.
2NaN3  2Na + 3N2
d.
Ba(NO3)2 + K2SO4 
2KNO3 + BaSO4
e.
BaO + SO3  BaSO4
f.
2Al + Fe2O3  Al2O3 + 2Fe
g.
P4 + 6Cl2  4PCl3
Reactant(s)
Product(s)
Type of Reaction