Synthesis
1. ____ H2
Decompostion
Single Replacement
Double Replacement
Complete Combustion Incomplete combustion
+ ____O2  ___ H2O
___________
2. ____Zn + ____CuSO4  ___ZnSO4 + ____Cu
___________
3. ____KClO3  ___ KCl + ___ O2
___________
4. ___Pb(NO3)2 + ___ NaI  ____PbI2 + ____ NaNO3
___________
5. ____CH4 + ____O2  ___CO2 + ___ H2O
___________
6. ____Si + ____ Br2  ____SiBr4
___________
7. ___CuCl2 + ___AgNO3  ___ Cu(NO3)2 + ____AgCl
___________
8. ___ HCl + ____ NH3  ____ NH4Cl
___________
9. ____CH4 + ___Cl2  ____ CH3Cl + ___ HCl
___________
10. ___ Rb + ____ Cl2  ___ RbCl
___________
11. ___C2H2 + ____O2  ___CO2 + ____H2O
___________
12. ___ HNO3 + ___ Ca(OH)2  ____Ca(NO3)2 + ___ H2O
___________
13. ___Na + ___NiCl2  ___ NaCl + ___ Ni
___________
14. ___ Cu + ____ I2  ___ CuI
___________
+ ____FeCl3  ___ SrCl2 + ___ Fe(OH)3
15.
___ Sr(OH)2
16.
____ Na2CO3  ___ Na + ___ O2 + ___ CO2
___________
17.
___ Cl2 + ___ BaBr2  ___ BaCl2 + ___ Br2
___________
18.
___ H2 + ___ S + ___ O2  ___ H2SO3
___________
19.
___ N2O4  ___ NO2
___________
20.
___ CaCl2 + ___ O2  ___ CaO + ___ Cl2
___________
21.
___ Al + ___ O2  ___ Al2O3
___________
22.
___ Mg + ___ O2  ____MgO
___________
23.
___ NaOH + ___ H2SO4  ___ Na2SO4 + ___ H2O
___________
24.
____( NH4) 2 CO3  ___ NH3 + ____H2O +___ CO2
___________
25.
____H2O + ___SO3  ____ H2SO4
___________
26.
___ P + ___ Cl2  ____PCl5
___________
27.
___ Al2(SO4)3 + ___Ca(OH)2  ___ CaSO4 + ____ Al(OH)3
___________
28.
____ AgNO3 + ____ CuCl2  ___AgCl + ____Cu(NO3)2
___________
29.
____ Cu(NO3)2 + ____ NaOH  ____ Cu(OH)2 + ____ NaNO3
___________
30. ____ Al + ___ HCl  ____ AlCl3
+ ____ H2
___________
___________
Synthesis
Decompostion
Single Replacement
Double Replacement
Complete Combustion Incomplete combustion
1. __2__ H2
+ __1__O2  __2_ H2O
____SYN_______
2. _1___Zn + __1__CuSO4  __1_ZnSO4 + __1__Cu
____SR_______
3. __2__KClO3  __2_ KCl + __3_ O2
____DEC_______
4. __1_Pb(NO3)2 + __2_ NaI  __1__PbI2 + __2__ NaNO3
_____DR_____
5. ___1_CH4 + ___2_O2  __1_CO2 + _1__ H2O
_____CC______
6. __1__Si + __2__ Br2  __1__SiBr4
_____SYN ______
7. __1_CuCl2 + _2__AgNO3  _1__ Cu(NO3)2 + __2__AgCl
______DR_____
8. _1__ HCl + _1___ NH3  __1__ NH4Cl
____SYN_______
9. ___1_CH4 + _1__Cl2  __1__ CH3Cl + __1_ HCl
______SR_____
10. __2_ Rb + __1__ Cl2  _2__ RbCl
_____SYN______
11. __2_C2H2 + ___5_O2  _4__CO2 + _2___H2O
______CC_____
12. _2__ HNO3 + __1_ Ca(OH)2  __1__Ca(NO3)2 + _2__ H2O
_____DR______
13. _2__Na + _1_NiCl2  __2_ NaCl + _1__ Ni
____SR_______
14. ___2 Cu + ___1_ I2  __2_ CuI
___SYN________
+ __2__FeCl3  _3__ SrCl2 + _2__ Fe(OH)3
15.
_3_ Sr(OH)2
16.
__2__ Na2CO3  __4_ Na + __1_ O2 + _2__ CO2
DEC________
17.
_1__ Cl2 + __1_ BaBr2  __1_ BaCl2 + _1__ Br2
SR________
18.
__2_ H2 + _2__ S + __3_ O2  __2_ H2SO3
SYN________
19.
___ N2O4  __2_ NO2
DEC___
20.
__2_ CaCl2 + __1_ O2  _2__ CaO + _4__ Cl2
SR____
21.
__2_ Al + _3__ O2  __2_ Al2O3
SYN________
22.
_2__ Mg + _1__ O2  _2___MgO
SYN_______
23.
__2_ NaOH + __1_ H2SO4  _1__ Na2SO4 + __2_ H2O
DR_______
24.
__1__( NH4) 2 CO3  __2_ NH3 + __1__H2O +_1__ CO2
DEC________
25.
___1_H2O + __1_SO3  ___1_ H2SO4
SYN_______
26.
___2 P + __5_ Cl2  __2__PCl5
SYN
27.
_2__ Al2(SO4)3 + _3__Ca(OH)2  __3_ CaSO4 + __2__ Al(OH)3
DR_______
28.
__2__ AgNO3 + __1__ CuCl2  _2__AgCl + __1__Cu(NO3)2
DR_________
29.
__1__ Cu(NO3)2 + __2__ NaOH  ___1_ Cu(OH)2 + __2__ NaNO3
DR
30. __2__ Al + _6__ HCl  __2__ AlCl3
+ __3__ H2
DR_____
SYN____
Balancing Equations / Types of Reaction Review
Type SYN, DEC,SR,DR,CC, ICC
1. ___S8 + ___O2 ---> ___SO3
2. ___HgO --->___Hg + ___ O2
3. ___Na + ___H2O ---> ___NaOH + ___H2
4. ___H3PO4 ---> ___H4P2O7 + ___H2O
5. ___Al(OH)3 + ___ H2SO4 ---> ___Al2(SO4)3 +___ H2O
6. ___Fe2(SO4)3 + ___KOH ---> ___ K2SO4 + ____Fe(OH)3
7. ___C7H6O2 + ___ O2 ---> ___ CO2 + ___H2O
8. ___Al + ___ FeO ---> ___ Al2O3 + ___ Fe
9.
___Fe2O3 + ___ H2 ---> ___ Fe + ___ H2O
10. ___ K + ___ Br2 ---> ___ KBr
11. ___K2O + ___H2O ---> ___ KOH
12. ___H2O2 ---> ___ H2O + ___ O2
13. ___SiO2 + ___ HF ---> ___ SiF4
+ ____ H2O
14. ___H3AsO4 ---> ___As2O5 + ____ H2O
15. ___ C3H8 + ___ O2 ---> ___ C + ___ CO + ___ H2O
16. ____P4O10
+ ____H2O ---> ____ H3PO4
17. ____Sb + ___ O2 ---> ___ Sb4O6
18. ___N2O5 + ___ H2O ---> ___ HNO3
19. ___Fe2O3 + _3_ CO ---> ___ Fe + ___ CO2
20. ___H3BO3 ---> ___ H4B6O11
+ ___ H2O
21. ___H2S + ___Cl2 ---> ___ S8 + ____ HCl
22 ___H2SO3 + ___KOH ---> ___ K2SO3
+ ____ H2O
Balancing Equations / Types of Reaction Review
Type SYN, DEC,SR,DR,CC, ICC
1. _1_S8 + _12__O2 ---> __8_SO3
SYN
2. __2_HgO --->__2_Hg + __1_ O2
DEC
3. __2_Na + __1_H2O ---> __2_NaOH + __1_H2
SR
4. __2_H3PO4 ---> __1_H4P2O7 + __1_H2O
DEC
5. __2_Al(OH)3 + __3_ H2SO4 ---> __1_Al2(SO4)3 +__6_ H2O
DR
6. __1_Fe2(SO4)3 + __2_KOH ---> __1_ K2SO4 + __2__Fe(OH)3
DR
7. __2_C7H6O2 + _16__ O2 ---> __14_ CO2 + __6_H2O
CC
8. _2__Al + _3__ FeO ---> ___1 Al2O3 + __3_ Fe
SR
9. _1__Fe2O3 + __3_ H2 ---> _2__ Fe + __3_ H2O
SR
10.__2_ K + _1__ Br2 ---> __2_ KBr
SYN
11.__1_K2O + __1_H2O ---> __2_ KOH
SYN
12.__2_H2O2 ---> __2_ H2O + __1_ O2
DEC
13.__1_SiO2 + __4_ HF ---> __1_ SiF4
+ __2__ H2O
DR
14.__2_H3AsO4 ---> __1_As2O5 + __3__ H2O
DEC
15. __1_ C3H8 + _3__ O2 ---> __1_ C + _2__ CO + __4_ H2O
ICC
16.__1__P4O10
SYN
+ __6__H2O ---> __4__ H3PO4
17.__4__Sb + _3__ O2 ---> _1__ Sb4O6
SYN
18.__1_N2O5 + _1__ H2O ---> _2__ HNO3
SYN
19. __1_Fe2O3 + __3_ CO ---> _2__ Fe + _3__ CO2
REDOX
20. _6__H3BO3 ---> __1_ H4B6O11
DEC
+ __7_ H2O
21.__8_H2S + __8_Cl2 ---> __1_ S8 + ___16_ HCl
SR
22 __1_H2SO3 + _2__KOH ---> __1_ K2SO3
DR
+ ___2_ H2O
Types of
Reaction
can be
can be
can be
can be
________
__________
___________Reactions
of
is
can be
can be
________
Replacement
___________Replacem ent
Reverse
_________
Reactions
can be
can be
for exam ple
for exam ple
Sodium + chlorine y ields ____________
sodium carbonate +
silver nitrate
iron + copper (II) chloride y ields
___________ + _________
represented as
__________
Combustion
for exam ple
__________
Combustion
for exam ple
y ields
___Na(s) +___ Cl 2(g) --> ________(s)
___________ +
_____________
represented as
m ethane +
oxy gen
for exam ple
follows
m ethane +
oxy gen
y ields
y ields
A + B -- > AB
Fe(s) + CuCl 2 (aq) -> ______(aq) + ___ (s)
_____________ yields hydrogen and oxy gen
can be represented
as
______
+
______
_____
+
-_______
+
_____
follows
Na2CO 3(aq) +
2AgNO3(aq)
represented as
y ields
A + BZ -> AZ + B
________
__________
CH 4(g) +
2O 2(g)
_______ -> 2 H 2 (g) + O 2(g)
can also be
y ields
follows
follows
Y + BZ - > BY + Z
AB - > A + B
for exam ple
AZ + BY -> AY + BZ
Chlorine + sodium bromide yields
__________ + ___________
can be represented
as
Cl 2 (aq) + NaBr(aq) -> _____(aq) +____(aq)
___C0 2(g) +
___H 2O(g)
3CH 4 +
4O2 (g)
y ields
C(s)
+ ___CO(g)
+ __H2O(g)
follows
CnHn + O 2
y ields
____+ _____
CnHn +
O2
y ields
__ +
____+
_____
Nomenclature
Rules
for
for
M etals
________
Nonmetals
to
form
form
form
______
to
form
_________
Compounds
Ionic
comp ounds
does not
contain containing
______
can be
_______
may be
Binary
Prefexes
M ono = 1
di= 2
tri = 3
_____ = 4
p enta = 5
hexa = 6
_____ = 7
octa = 8
is
Roman ______
Stock Sy stem
uses
uses
for examp le
ex
ex
ex ex
to
Indicate
Oxidation State of
________element
ex
NO
NO2
N2O3
N2O4
N2O5
is
is
is
is
is
______________
____________
____________
___________
changes
Roman
Numerals
second
elements
ending to
_____
Nitrogen
oxygen
comp ounds
ex.
N2O
named by
Prefix named by
M ethod
changes
_______________
______________
Second
elements
ending to
_____
_____
Nomenclat ure
Rules
for
for
M etals
form
nonmetal
Nonmetals
to
form
form
nonmetal
to
form
M olecular
Compounds
Ionic
comp ounds
does not
contain containing
hy drogen
hy drogen
named by
Roman _______
Stock Sy st em
changes
uses
Roman
_______
to
Indicate
Oxidation State of
________element
2(
N
)
(-2)
O
(
N
) (-2)
O
2(
N
)
(-2)
O
(
N
) (-2)
O
nitrogen( )oxide
for example
Nitrogen
oxygen
comp ounds
(
N
(
N
) 2(-2)
O
)
Second
elements
ending to
____
N2O3
NO2
NO
nitrogen( )oxide
Acidic
can be
Binary
N2O
may be
2 (-2)
O
nitrogen( )oxide
2(
N
) 3(-2)
O
2( ) 3 (-2)
N
O
nitrogen( )oxide
N2O5
2(
N
) 5(-2)
O
2(
N
) 5 (-2)
O
nitrogen( )oxide
Nomenclature
Rules
for
for
M etals
nonmetal
Nonmetals
to
form
form
form
nonmetal
to
form
M olecular
Compounds
Ionic
comp ounds
does not
contain containing
hy drogen
hy drogen
may be
may be
may be
Binary
contain
_____
Tertiary
contain
contain
_______
_______
_______
change to
change
do not
________
ions
may end in
Ending to
___
_____
Name/
_____
____
change to
change to
______
acid
____
acid
Drop the
hy dro
for examp le
HF
for examp le
HCl
for examp le
for examp le
_________
_________
for examp le
for examp le
for examp le
H2S
SO 32sulfite
__________
may end in
H2SO 3 (aq)
___________
NO2nitrite
______(aq)
______acid
SO 42sulfate
NO3nitrate
________(aq)
_______ acid
_______(aq)
______acid
Formulas of Compounds based on their Oxidation states / charges
Al
0
Copper (II) hydroxide
1.
Cu+2 OH-1
Copper (I) sulfide
2.
Cu+1 S-2
Copper (II) Phosphate
3.
Cu+2 PO4-3
Potassium hydroxide
4.
K+1 OH-1
Potassium phosphate
5.
K+1 PO4-3
Aluminum hydroxide
6.
Al+3 OH-1
Aluminum oxide
7.
Al+3 O-2
vanadium (V) hydroxide
8.
V+5 OH-1
Vanadium (V) sulfide
9.
V+5 S-2
Zirconium (IV) sulfide
10.
Zr+4 S-2
11. potassium nitrate
19. magnesium phosphate
12. aluminium chloride
20. hydrogen phosphate
13. manganese (II) chloride
21. barium oxide
14. hydrogen sulfite
22. phosphorous (V) chloride
15. calcium thiosulfate
23. hydrogen hypochlorite
16. iron (II) chromate
24. cesium fluoride
17. sulfur trioxide
25. hydrogen bromide
18. carbon (II) oxide
26. nickel (III) sulfate
Nomenclature Practice
1. AgCl m
nm
nm polyatomic ions
ionic/molecular/acid prefixes Y/N multiple ox Y/N
nm
nm polyatomic ions
ionic/molecular/acid prefixes Y/N multiple ox Y/N
m
nm
nm polyatomic ions
ionic/molecular/acid prefixes Y/N multiple ox Y/N
4. NaBr m
nm
nm polyatomic ions
ionic/molecular/acid prefixes Y/N multiple ox Y/N
5. ZnCO3 m
Name
nm
nm polyatomic ions
ionic/molecular/acid prefixes Y/N multiple ox Y/N
6. PH3
N
m
nm
nm polyatomic ions
ionic/molecular/acid prefixes Y/N multiple ox Y/N
7. KCN m
Name
nm
nm polyatomic ions
ionic/molecular/acid prefixes Y/N multiple ox Y/N
Name
2. CoBr2 m
Name
3. AuS
Name
Name
Name
8. Fe(OH)2 m
Name
nm
9. Au(NO3)3 m
nm
nm polyatomic ions
nm polyatomic ions
ionic/molecular/acid prefixes Y/N multiple ox Y/N
ionic/molecular/acid prefixes Y/N multiple ox Y/N
Name
10. NiBr3 m
nm
nm polyatomic ions
ionic/molecular/acid prefixes Y/N multiple ox Y/N
11. SO2 m
Name
nm
nm polyatomic ions
ionic/molecular/acid prefixes Y/N multiple ox Y/N
12. Rb2O m
nm
nm polyatomic ions
ionic/molecular/acid prefixes Y/N multiple ox Y/N
Name
Name
13. H2CO3(aq) m
nm
nm polyatomic ions
ionic/molecular/acid prefixes Y/N multiple ox Y/N
14. BaS
m
nm
nm polyatomic ions
ionic/molecular/acid prefixes Y/N multiple ox Y/N
Name
15. HClO3(aq) m
nm
nm polyatomic ions
ionic/molecular/acid prefixes Y/N multiple ox Y/N
Name
16. Cr2O3 m
nm
nm polyatomic ions
ionic/molecular/acid prefixes Y/N multiple ox Y/N
Name
17. CaC2O4 m
nm
nm polyatomic ions
ionic/molecular/acid prefixes Y/N multiple ox Y/N
Name
18. HClO2(aq) m
nm
nm polyatomic ions
ionic/molecular/acid prefixes Y/N multiple ox Y/N
Name
19. PCl5 m
Name
20. Al2SO4 m
nm
nm
nm polyatomic ions
nm polyatomic ions
ionic/molecular/acid prefixes Y/N multiple ox Y/N
ionic/molecular/acid prefixes Y/N multiple ox Y/N
Types of
Reaction
can be
can be
can be
________
Syn
__________
can be
Dec
of
is
Reactions
can be
can be
________
Double
Replacement
___________Replacem ent
Single
Reverse
_________
Combustion
Replacement
___________Reactions
can be
can be
for exam ple
for exam ple
Combustion
Sodium + chlorine y ields ____________
Sodium chloride
sodium carbonate +
silver nitrate
iron + copper (II) chloride y ields
Iron(II)chloride
+ copper
___________ + _________
represented as
Complete
__________
for exam ple
Incomplete
__________
Combustion
for exam ple
y ields
Silver carbonate
___Na(s)
+___
________(s)
2
1 Cl 2(g) --> 2NaCl
_____________
Sodium
nitrate
m ethane +
oxy gen
for exam ple
follows
A + B -- > AB
___________ +
represented as
y ields
FeCl2
y ields
Cu
Fe(s) + CuCl 2 (aq) -> ______(aq) + ___ (s)
Water
_____________ yields hydrogen and oxy gen
m ethane +
oxy gen
can be represented
as
CO
______
2
+
______
H2O
_____
C
CO+
-_______
+
H2O
_____
follows
Na2CO 3(aq) +
2AgNO3(aq)
represented as
y ields
A + BZ -> AZ + B
________
2NaNO
3
__________
Ag
2(CO)3
_______ -> 2 H 2 (g) + O 2(g)
2H2O
can also be
CH 4(g) +
2O 2(g)
y ields
follows
follows
Y + BZ - > BY + Z
AB - > A + B
AZ + BY -> AY + BZ
for exam ple
Chlorine + sodium bromide yields
__________ +
+ ___________
Sodium chloride
bromine
1 2(g) +
___C0
2 2O(g)
___H
CnHn + O 2
CO2 H2O
2NaCl
Br
2
Cl 2 (aq) + NaBr(aq) -> _____(aq) +____(aq)
4O2 (g)
y ields
C(s)
2
+ ___CO(g)
6 2O(g)
+ __H
follows
y ields
____+ _____
can be represented
as
3CH 4 +
CnHn +
O2
y ields
C__ +
____+
CO
_____
H
2O
Ionic
Molecular
Binary
Tertiary
Polyatomic
1st
2nd
No
ide
Excess
Deficiency
+1
+2
2oxide
+3
ending
+2
Lithium oxide
+3
II
III
Ammonium sulfate
Formulas of Compounds based on their Oxidation states / charges
Nomenclature
Rules
for
for
M etals
Nonmetal
________
Nonmetals
to
Nonmetal
______
to
form
form
form
form
_________
molecular
Compounds
Ionic
comp ounds
does not
contain containing
can be
Hydrogen
______
_______ may be
Hydrogen
Binary
Prefexes
M ono = 1
di= 2
tri = 3
Tetra
_____ = 4
p enta = 5
hexa = 6
Penta = 7
_____
octa = 8
is
Roman ______
Numeral
Stock Sy stem
uses
uses
for examp le
ex
ex
ex ex
to
Indicate
Oxidation State of
first
________element
ex
NO
NO2
N2O3
N2O4
N2O5
is
is
is
is
is
Dintrogen monoxide
______________
Nitrogen
monoxide
____________
____________
Dinitrogen
trioxide
___________
Nitrogen
dioxide
changes
Roman
Numerals
second
elements
ending
Ide to
_____
Nitrogen
oxygen
comp ounds
ex.
N2O
named by
Prefix named by
M ethod
changes
_______________
dinitrogen pentoxide
Dinitrogen
tetraoxide
______________
Second
elements
ending to
ide
_____
_____
acidic
Nomenclat ure
Rules
for
for
M etals
form
nonmetal
Nonmetals
to
form
form
nonmetal
to
form
M olecular
Compounds
Ionic
comp ounds
does not
contain containing
hy drogen
hy drogen
named by
Roman _______
Numeral
Stock Sy st em
changes
uses
Roman
Number
_______
to
Indicate
Oxidation State of
First
________element
2(
N
)
(-2)
O
2( +1) (-2)
N
O
nitrogen(I )oxide
) (-2)
O
(+2 ) (-2)
N
O
nitrogen( II)oxide
for example
Nitrogen
oxygen
comp ounds
(
N
) 2(-2)
O
(+4 ) 2 (-2)
N
O
nitrogen(IV)oxide
Second
elements
ending to
____
Ide
N2O3
NO2
NO
(
N
Acidic
can be
Binary
N2O
may be
2(
N
) 3(-2)
O
N2O5
2(
N
) 5(-2)
O
2(+3) 3 (-2)
N
O
2(+5 ) 5 (-2)
N
O
nitrogen(III )oxide
nitrogen(V )oxide
Nomenclature
Rules
for
for
M etals
nonmetal
Nonmetals
to
form
form
form
nonmetal
to
form
M olecular
Compounds
Ionic
comp ounds
does not
contain containing
hy drogen
hy drogen
may be
may be
may be
Binary
contain
Tertiary
contain
_______
Hydrogen
_____
Acidic
contain
_______
nonmetal
________
polyatomic
_______
Hydrogen
ions
may end in
change to
change
do not
Hydro
_____
Ending to
___
Name/
Ic
for examp le
HF
for examp le
HCl
ite
_____
ate
____
change to
change to
______
Ous
acid
ic
____
acid
for examp le
for examp le
Drop the
hy dro
for examp le
Hydrochloric
_________
Acid
Hydrosulfuric
_________
Acid
for examp le
for examp le
H2S
SO 32sulfite
Hydrofluoric
__________
Acid
may end in
H2SO 3 (aq)
___________
sulfurous
NO2nitrite
______(aq)
HNO
2
______acid
nitrous
SO 42sulfate
H________(aq)
2SO4
_______ acid
sulfuric
NO3nitrate
_______(aq)
HNO
3
______acid
nitric
Al+3
0-2
Al2O3
2Al+3
3O2-
Aluminium has a combining power of 3 therefore it attracts
three oxygen ions. The oxygen has a combining power of 2
therefore it attracts two aluminium ions.
Copper (II) hydroxide
1.
Cu+2+2 OH-1-1 Cu(OH)2
Copper (I) sulfide
2.
Cu+1+1 S-2-2 CCu2S
Copper (II) Phosphate
3.
Cu+2 PO43--3 Cu3(PO4)2
Potassium hydroxide
4.
K+1+1 OH-1- KOH
Potassium phosphate
5.
K+1+1 PO43--3 K3PO4
Aluminum hydroxide
6.
Al+33 OH1-1 Al(OH)3
Aluminum oxide
7.
Al+3 O-2
vanadium (V) hydroxide
8.
V+5+5 OH1—1 V(OH)5
Al2O3
Vanadium (V) sulfide
9.
V5+5 S2-2
V2S5
Zirconium (IV) sulfide
10.
Zr+4+4 S-2 Zr2S4  ZrS2
19. potassium nitrate
K+1 NO31KNO3
19. magnesium phosphate
Mg2+PO43- Mg3(PO4)2
20. aluminium chloride
Al+3Cl-1
AlCl3
20. hydrogen phosphate
H+1PO43- H3PO4
21. manganese (II) chloride
Mn+2Cl1MnCl2
21. barium oxide
Ba+2 O2- BaO
22. hydrogen sulfite
H+1 SO32H2SO3
22. phosphorous (V) chloride
P+5Cl1PCl5
23. calcium thiosulfate
Ca+2 C2S22- CaC2S2
23. hydrogen hypochlorite
H1 ClO1- HClO
24. iron (II) chromate
Fe+2 CrO42- FeCrO4
24. cesium fluoride
Cs+1F-1
CsF
25. sulfur trioxide
SO3
25. hydrogen bromide
H+1Br-1 HBr
26. carbon (II) oxide
C+2O2CO
26. nickel (III) sulfate
Ni3+SO42- Ni2(SO4)3
Nomenclature Practice
21. AgCl m
nm
nm polyatomic ions
ionic/molecular/acid prefixes Y/N multiple ox Y/N
Name silver chloride
22. CoBr2 m
nm
nm polyatomic ions
ionic/molecular/acid prefixes Y/N multiple ox Y/N
Name cobalt (II) bromide
23. Au2S m
nm
nm polyatomic ions
ionic/molecular/acid prefixes Y/N multiple ox Y/N
Name gold (I) Sulfide
24. NaBr m
nm
nm polyatomic ions
ionic/molecular/acid prefixes Y/N multiple ox Y/N
Name sodium bromide
25. ZnCO3 m nm nm polyatomic ions
Name zinc carbonate
ionic/molecular/acid prefixes Y/N multiple ox Y/N
26. PH3
ionic/molecular/acid prefixes Y/N multiple ox Y/N
m
nm
nm polyatomic ions
Name phosphorous trihydride
27. KCN m nm nm polyatomic ions
Name potassium cyanide
ionic/molecular/acid prefixes Y/N multiple ox Y/N
28. Fe(OH)2 m nm nm polyatomic ions
Name iron (II) hydroxide
ionic/molecular/acid prefixes Y/N multiple ox Y/N
29. Au(NO3)3 m
ionic/molecular/acid prefixes Y/N multiple ox Y/N
nm
nm polyatomic ions
Name gold (III) nitrate
30. NiBr3 m
nm
nm polyatomic ions
ionic/molecular/acid prefixes Y/N multiple ox Y/N
Name nickel (III) bromide
31. SO2 m nm nm polyatomic ions
Name sulfur dioxide
ionic/molecular/acid prefixes Y/N multiple ox Y/N
32. Rb2O m
ionic/molecular/acid prefixes Y/N multiple ox Y/N
nm
nm polyatomic ions
Name rubidium oxide
33. H2CO3(aq) m nm nm polyatomic ions ionic/molecular/acid prefixes Y/N multiple ox Y/N
Hydrogen carbonate  drop the hydro  ate  ic acid  carbonic acid
34. BaS
m
nm
nm polyatomic ions
ionic/molecular/acid prefixes Y/N multiple ox Y/N
Name barium sulfide
35. HClO3(aq) m
nm
nm polyatomic ions
ionic/molecular/acid prefixes Y/N multiple ox Y/N
Name hydrogen chlorate  drop hydro  ate  ic acid  chloric acid
36. Cr2O3 m
nm
nm polyatomic ions
ionic/molecular/acid prefixes Y/N multiple ox Y/N
Name chromium (III) oxide
37. CaC2O4 m
nm
nm polyatomic ions
ionic/molecular/acid prefixes Y/N multiple ox Y/N
Name calcium oxalate
38. HClO2(aq) m
nm
nm polyatomic ions
ionic/molecular/acid prefixes Y/N multiple ox Y/N
Name hydrogen chlorate  drop hydro  chlorite  ous acid  chlorous acid
39. PCl5 m nm nm polyatomic ions
Name phosphorous pentachloride
ionic/molecular/acid prefixes Y/N multiple ox Y/N
40. Al2 ( SO4) m
ionic/molecular/acid prefixes Y/N multiple ox Y/N
nm
nm polyatomic ions
Name aluminium sulfate
Nomenclature Practice
calcium iodide
CaI2
Mg(NO3)2
magnesium nitrate
iron(II) ethanoate
Fe(C2H3O2)2
PbO2
lead(IV) oxide
calcium hydride
CaH2
CuS
copper(II) sulfide
Ammonia ( nitrogen
trihydride)
NH3
H2SO3(aq)
Sulfurous acid (g)
magnesium nitrate
Mg(NO3)2
Co(C2H3O2)2 Cobalt (II) ethanoate
calcium iodide
CaI2
H2S(aq)
Hydrosulfuric acid
calcium hydride
CaH2
PbO2
lead(IV) oxide
potassium chromate
K2CrO4
CdBr2
cadmium bromide
copper(II) sulfide
CuS
Al(C2H3O2)3 aluminum ethanoate
Phoshorous(III)hydride (g)
PH3
SbP
antimony(III) phosphide
antimony(V) sulfite
Sb2(SO3)5
V2(CO3)5
vanadium(V) carbonate
nickel(II) sulfate
NiSO4
AsSO3
arsenic(II) sulfite
tin(II) fluoride
SnF2
PbS
lead(II) sulfide
Hyrobromic acid
HBr(aq)
Pb(ClO3)2
lead(II) chlorate
manganese(II) oxalate
MnC2O4
CCl4
carbon tetrachloride
manganese(III) dichromate
Mn2(Cr2O7)3
(NH4)2SO4
ammonium sulfate
Nitrous acid
HNO2(aq)
HNO3(aq)
cobalt(II) hydroxide
Co(OH)2
SnS2
tin(IV) sulfide
lithium perchlorate
LiClO4
Mn(MnO4)3
manganese(III)
permanganate
tungsten(VI) phosphate
W(PO4)2
SO2
sulfur dioxide
copper(II) sulfate
CuSO4
Au3P
gold(I) phosphide
zinc nitrite
Zn(NO2)2
RbH
rubidium hydride
mercury(I) phosphate
(Hg2)3(PO4)2
Ba3N2
barium nitride
mercury(II) phosphate
Hg3(PO4)2
CsCN
cesium cyanide
tetraphosphorus decoxide
P4O10
AgCN
silver cyanide
Oxalic acid
H2C2O4(aq)
CS2
carbon disulfide
cesium dihydrogen phosphate CsH2PO4
Rb2CrO4
rubidium chromate
tungsten(VI) sulfite
W(SO3)3
(NH4)3PO4
ammonium phosphate
disulfur dichloride
S2Cl2
Na2HPO4
sodium hydrogen
phosphate
platinum(IV) oxide
PtO2
HF(aq)
hydrogen fluoric acid
(g)
Nomenclature Answers
calcium iodide
CaI2
Mg(NO3)2
magnesium nitrate
iron(II) ethanoate
Fe(C2H3O2)2
PbO2
lead(IV) oxide
calcium hydride
CaH2
CuS
copper(II) sulfide
Ammonia ( nitrogen
trihydride)
NH3
H2SO3(aq)
Sulfurous acid (g)
magnesium nitrate
Mg(NO3)2
Co(C2H3O2)2 Cobalt (II) ethanoate
calcium iodide
CaI2
H2S(aq)
Hydrosulfuric acid
calcium hydride
CaH2
PbO2
lead(IV) oxide
potassium chromate
K2CrO4
CdBr2
cadmium bromide
copper(II) sulfide
CuS
Al(C2H3O2)3 aluminum ethanoate
Phoshorous(III)hydride (g)
PH3
SbP
antimony(III) phosphide
antimony(V) sulfite
Sb2(SO3)5
V2(CO3)5
vanadium(V) carbonate
nickel(II) sulfate
NiSO4
AsSO3
arsenic(II) sulfite
tin(II) fluoride
SnF2
PbS
lead(II) sulfide
Hyrobromic acid
HBr(aq)
Pb(ClO3)2
lead(II) chlorate
manganese(II) oxalate
MnC2O4
CCl4
carbon tetrachloride
manganese(III) dichromate
Mn2(Cr2O7)3
(NH4)2SO4
ammonium sulfate
Nitrous acid
HNO2(aq)
HNO3(aq)
cobalt(II) hydroxide
Co(OH)2
SnS2
tin(IV) sulfide
lithium perchlorate
LiClO4
Mn(MnO4)3
manganese(III)
permanganate
tungsten(VI) phosphate
W(PO4)2
SO2
sulfur dioxide
copper(II) sulfate
CuSO4
Au3P
gold(I) phosphide
zinc nitrite
Zn(NO2)2
RbH
rubidium hydride
mercury(I) phosphate
(Hg2)3(PO4)2
Ba3N2
barium nitride
mercury(II) phosphate
Hg3(PO4)2
CsCN
cesium cyanide
tetraphosphorus decoxide
P4O10
AgCN
silver cyanide
Oxalic acid
H2C2O4(aq)
CS2
carbon disulfide
cesium dihydrogen phosphate CsH2PO4
Rb2CrO4
rubidium chromate
tungsten(VI) sulfite
W(SO3)3
(NH4)3PO4
ammonium phosphate
disulfur dichloride
S2Cl2
Na2HPO4
sodium hydrogen
phosphate
platinum(IV) oxide
PtO2
HF(aq)
hydrofluoric acid
Name _______________
Chemical Equation 2012 Review
____ Na(s) + _____ N2 (g) -----> _____ NaN3 (s)
a) Balance the equation 3pts
b) What type of reaction is it and why? 2pts
2. Given the following reaction answer questions 2a--2d.
2 Al (s) +
2H2SO3 (aq) ----> Al2 (SO3)3 (aq) +
3 H2 (g) This is not balanced
a) What type of reaction is this? __________________ and why 2pts
b) How many atoms of aluminum react? _____ 1pt each
How many molecules of H2SO3react? _____
How many aluminum sulfite form? _____
How many hydrogen molecules form? ______
c) What is the total number of aluminum atoms which react? ______aluminum in the products? ____
What is the total number of hydrogens which react? _____ hydrogens in the products? ______
What is the total number of oxygens which react? ______ oxygens in the products ? _______
What is the total number of sulfurs which react? ________ sulfurs in the products ? _______
.
d) According to the Standard Electrode Potential or activity of metals chart does this reaction take place.
How do you know this from the charts given? 2pts
5. (1pt each) What type of reaction does it represent?
a
b
C
d
6. Balance the following reaction and identify what type of reaction it is and why? 3pts
_____ C6H14 (g) + _____ O2 (g) -----> ______ CO2 (g) + _____ H2O (g)
a) Type of reaction: ___________________ Why?2pts
b) How does the potential energy of the C6H14 (g) + O2 (g) compare to the potential energy of
the CO2 (g) + H2O (g). How do you know this? What is the primary purpose of this type of
reaction? Why do we burn hydrocarbons?3pts
c) What has a greater affinity for hemoglobin 1pt
a) oxygen
b) nitrogen c) carbon dioxide
d) Why is it important to know this? 2pts
6. a) Na2C2O4
d) HCl
a) sulfurous acid
d) cesium sulfide
d) carbon monoxide
b) MnBr2
c) P2O5
e) HClO4
b) nitric acid
f) HClO
c)
e) Vanadium (III) oxide
f) ammonium sulfate
g) dinitrogen trioxide
8. a) Finish the following word equation:
An aqueous iron (III) chloride reacts with an aqueous solution of manganese (II) hydroxide to
produce ___________ ______________ and _____________ __________________.2pts
b) What type of reaction is it? ____________________ and why? 2pts
c) Write a balanced symbol equation including subscripts, coefficients and phases. The product that
forms a precipitate is the compound containing the hydroxide ion? 12 pts
iv) symbols, subscripts, coefficients, and phases of matter
8. Balance the following reaction 3pts
______ Fe2O3 (g) -----> ____Fe (s) + ____ O2 (g)
Type of reaction: ________________________ Why? 2pts
9.
Aluminium Strip
V
Silver (Ag) Strip
Aluminium
chloride solution
Silver nitrate
solution
Porous Ceramic Container
a) Which metals is more reactive? Loses electrons? Is oxidized? Is the source of electrons? Is the negative
electrode? Is the anode? Produces Positive Ions? Mass decreases?
b) Which metal is less reactive? Gains Electrons? Is Reduced? Attracts Positive Ions? Mass increases?
Is the positive electrode? Is the cathode?
e) What are the “half reactions which develop a potential difference between these metals and their ions?
( Use your standard electrode potential chart ) 4pts
f) What is the electrode potential between the aluminium / aluminium ions and the silver / silver
ions? 2pts
g) Which way do the negative ions travel through the porous ceramic container?
h) Which way do the positive ions travel through the porous ceramic container?
Nomenclature Review
1. Why is the name of MgCl2 magnesium chloride not:
a) magnesium (II) chloride
b) magnesium dichloride
c) magnesium chlorine
d) magnesium chlorate
2. Why is the name of Co(NO3)3 cobalt (III) nitrate not
a) cobalt nitrate
b) cobalt (II) nitrate
c) cobalt trinitrogen nano oxide
d) cobalt (III) nitrite
3. Why is the name of Li3PO4 lithium phosphate not
a) lithium (I) phosphate
b) trilithium monophosphourous tetraoxide
c) lithium phosphide
d) lithium (III) phosphate
4. Why is the name of FeS2O3 iron (II) thiosulfate not
a) iron thiosulfate
b) iron (I) thiosulate
c) iron disulfur trioxide
d) iron (III) sulfate
5. Why is the name CuS copper (II) sulfide not
a) copper sulfide
b) copper (I) sulfide
c) copper (II) sulfate
d) copper (II) sulfite
6. Why can CO2 have two names ( carbon dioxide and carbon (IV) oxide)?
7. Why can P2O5 have two names phosphorous (V) oxide and diphosphorous pentoxide?
8,
Why is name of Al2O3 aluminim oxide not
a) aluminium (III) oxide
b) dialuminium trioxide
c) aluminium oxalate
d) aluminium nitrate
9. Why is the name of HF (aq) hydrofluoric acid not
a) fluoric acid
b) fluorous acid
10. Why is the name of HClO2 (aq) chlorous acid not
a) hydrochlorous acid
b) chloric acid
c) hypochlorous acid
11. Why is the name of HClO4 (aq) perchloric acid not
a) hydroperchloric acid
b) perchlorous acid
c) hydrochloric acid
12. Why is the name of C2H5OH ethanol not
a) dicarbon hexahydrogen monooxide
b) ethanoic acid
c) carbon hydrogen oxide
13. The formula of lithium sulfate is Li2SO4 not
a) Li (SO4)2
b) Li2S
14. The formula of Copper (I) oxide is Cu2O not
a) CuO
b) CuCO3
15. The formula of Iron (II) sulfite is FeSO3 not
a) Fe2(SO3)2
b) Fe2SO3
16. The formula of nickel (III) carbonate is Ni2(CO3)3 not
a) Ni3C
b) Ni3(CO3)2
17. The formula of hydrosulfuric acid is H2S not
a) H2SO3
a) H2SO4
18. The formula of chloric acid is HClO3 not
a) HCl
b) HClO
c) HClO2
d) HClO4
19. The formula of nitrous acid is HNO2 (aq) not
a) H3N (aq)
b) HNO3 (aq)
20 a) What is the name of each of the following
KClO2
BaO
MnO2
Ca(CN)2
Cu(NO2)2
N2 O
HNO2(aq)
H2CO3(aq)
b) What is the formula of each?
Lead(II) iodide
calcium chloride
phosphoric acid
sulfurous acid
hydroiodidic acid
cobalt (III) sulfite
HBr(aq)
ammonium carbonate
strontium thiosulfate
Name _______________
__2__ Na(s) + __3___ N2 (g) -----> ___2__ NaN3 (s)
a) Balance the equation 3pts
b) What type of reaction is it and why? 2pts
A synthesis reaction because a single compound is formed A + B  AB. The sodium reacts with
nitrogen to form the compound known with the common name of sodium azide.
2. Given the following reaction answer questions 2a--2d.
2 Al (s) +
2H2SO3 (aq) ----> Al2 (SO3)3 (aq) +
3 H2 (g) This is not balance
a) What type of reaction is this? ______SR____________ and why 2pts
An element replaces another element that is part of a compound. It follows the A + BZ -> AZ + B./
The Aluminium replaces the hydrogen in the compound H2SO3
b) How many atoms of aluminum react? _2____ 1pt each
How many molecules of H2SO3react? ___2__
How many aluminum sulfite form? __1___
How many hydrogen molecules form? ___3___
c) What is the total number of aluminum atoms which react? __2____aluminum in the products? __2___
What is the total number of hydrogens which react? __4___ hydrogens in the products? __6____
What is the total number of oxygens which react? ___6___ oxygens in the products ? ___9____
What is the total number of sulfurs which react? ____2____ sulfurs in the products ? _____3__
This reaction is therefore not balanced. Balanced equations indicate that matter can not be
created nor destroyed.
5. (1pt each)
a) SR, element replaces another element that was part of a compound Follows A + BZ  AZ + B
b) DR, two compounds reacting to form two new compounds. Follows AZ + BY -> AY + BZ
c)DEC – single reactant forms multiple products AB  A + B
d) Syn, - single product type formed
A + B  AB
6. Balance the following reaction and identify what type of reaction it is and why? 3pts
___2__ C6H14 (g) + __19___ O2 (g) -----> ___12___ CO2 (g) + __14___ H2O (g)
a) Type of reaction: _____CC______________ Why?2pts
Hydrocarbon reacts with oxygen and combusts to from carbon dioxide and water
___CnHn + ___O2  ___CO2 + H2O
b) How does the potential energy of the C6H14 (g) + O2 (g) compare to the potential energy of
the CO2 (g) + H2O (g). How do you know this? What is the primary purpose of this type of
reaction? 3pts Since their is a release of energy the potential energy of the hexane and
oxygen are greater than the potential energy of the carbon dioxide and water. The primary
purpose of this reaction is to release energy in order to heat or propel an object.
c) What has a greater affinity for hemoglobin 1pt
a) oxygen
b) nitrogen c) carbon dioxide
d) carbon monoxide
d) Why is it important to know this? 2pts
Because hemoglobin has a greater affinity for CO it will not transport oxygen to our cells which
quickly die without a supply of oxygen.
6. a) Na2C2O4 sodium oxalate b) MnBr2 manganese(II)bromide c) P2O5 diphosphorous pentaoxide
d) HCl hydrochloric acid
a) sulfurous acid H2SO3
e) HClO4 perchloric acid f) HClO hypochlorous acid
b) nitric acid
HNO3 c) hydrosulfuric acid H2S
d) cesium sulfide Cs2S e) Vanadium (III) oxide V2O3
f) ammonium sulfate (NH4)2SO4
g) dinitrogen trioxide N2O3
8. a) Finish the following word equation:
An aqueous iron (III) chloride reacts with an aqueous solution of manganese (II) hydroxide to
produce ___iron (III) hydroxide______________ and ___manganese (II) chloride_____.2pts
b) What type of reaction is it? ____DR________________ and why? 2pts
The iron ions switch with the manganese ions and therefore the hydroxide ions switch with the
chloride ions
c) Write a balanced symbol equation including subscripts, coefficients and phases. The product that
forms a precipitate is the compound containing the hydroxide ion? 12 pts
i) symbols
Fe+3 Cl -1 + Mn+2 OH-1
Fe+3 OH-1
Mn+2Cl-1
ii) symbols with subscripts: FeCl3 + Mn(OH)2 ---> Fe(OH)3 + MnCl2
iii) symbols, subscripts and coefficients 2 FeCl3 + 3Mn(OH)2 ---> 2Fe(OH)3 + 3MnCl2
iv) symbols, subscripts, coefficients, and phases of matter
2 FeCl3(aq) + 3Mn(OH)2(aq) ---> 2Fe(OH)3(s) + 3MnCl2(aq)
8. Balance the following reaction 3pts
___2___ Fe2O3 (g) -----> _4___Fe (s) + __3__ O2 (g)
Type of reaction: ____DEC________________ Why? 2pts AB A + B , the iron(III)oxide
decomposes into iron and oxygen
Decomposition because the iron (III) hydroxide is the only reactant that produces two
types of products in the solid iron and the oxygen gas
Aluminium Strip
V
Silver (Ag) Strip
Aluminium
chloride solution
Silver nitrate
solution
Porous Ceramic Container
a) Which metals is more reactive? Loses electrons? Is oxidized? Is the source of electrons? Is the negative
electrode? Is the anode? Produces Positive Ions? Mass decreases? The Al is above the silver in the
metal reactivity series and therefore is more reactive, loses electrons, is said to be oxidized, is the
source of electrons and therefore considered to be the negative electrode called the anode. The Al
will produce Al+ ions and therefore its mass will decrease.
b) Which metal is less reactive? Gains Electrons? Is Reduced? Attracts Positive Ions? Mass increases?
Is the positive electrode? Is the cathode? The Ag which is below the Al is less reactive, will gain
electrons and therefore will be reduced, will attract positive ions and therefore gain mass. It will be
the positive electrode which is called a cathode.
c) What are the “half reactions which develop a potential difference between these metals and their ions?
( Use your standard electrode potential chart ) 4pts
Al(s) --> Al3+(aq)+3e- (LEO) {Which is reverse of reaction written)
Ag+(aq) + e- ---> Ag(s)(GER)
d) What is the electrode potential between the aluminium / aluminium ions and the silver / silver
ions? 2pts
-1.66 V Aluminium  0 V  + .80 V (Silver) = 2.46 V
e) Which way do the negative ions travel through the porous ceramic container?
The electrons travel from the Al to the Ag and the negative ions travel from the Ag solution
Through the porous ceramic container to the Al solution.
f) Which way do the positive ions travel through the porous ceramic container?
The positive ions travel from the Al solution to the Ag solution through the porous ceramic
Container.
Nomenclature Review
1. Why is the name of MgCl2 magnesium chloride not:
a) magnesium (II) chloride Mg only has a +2 charge
b) magnesium dichloride prefixes are not used with metal to nonmetal compounds
c) magnesium chlorine you need to change ending to ide
d) magnesium chlorate ate endings are used for polyatomic ions
2. Why is the name of Co(NO3)3 cobalt (III) nitrate not
a) cobalt nitrate cobalt needs a roman numeral
b) cobalt (II) nitrate it picks up three nitrates not two nitrates
c) cobalt trinitrogen nano oxide it is an ionic compound and prefixes are not needed
d) cobalt (III) nitrite NO3 is a nitrate ion not a nitrite ion
3. Why is the name of Li3PO4 lithium phosphate not
a) lithium (I) phosphate Li only has a +1 charge
b) trilithium monophosphourous tetraoxide it is ionic and no prefixes are needed
c) lithium phosphide PO4 is a polyatomic not a nonmetal ion
d) lithium (III) phosphate Li only has a +1 charge
4. Why is the name of FeS2O3 iron (II) thiosulfate not
a) iron thiosulfate iron has multiple oxidation numbers therefore it needs a roman numeral
b) iron (I) thiosulfate wrong oxidation number
c) iron disulfur trioxide ionic – no prefixes
d) iron (III) sulfaten – wrong polyatomic ion
5. Why is the name CuS copper (II) sulfide not
a) copper sulfide Cu has multiple oxidation states
b) copper (I) sulfide – wrong oxidation #
c) copper (II) sulfate – it does not contain a polyatomic ion
d) copper (II) sulfite –it does not contain a polyatomic ion
6. Why can CO2 have two names ( carbon dioxide and carbon (IV) oxide)?
Nonmetal to nonmetal compounds can have prefix or roman numeral – stock system name
7. Why can P2O5 have two names phosphorous (V) oxide and diphosphorous pentoxide?
Nonmetal to nonmetal compounds can have prefix or roman numeral – stock system name
8,
Why is name of Al2O3 aluminum oxide not
a) aluminium (III) oxide – aluminum does not need a roman numeral because it has only one
oxidation number
b) dialuminium trioxide – aluminum is a metal oxygen is a nonmetal therefore it is ionic which
are named without prefixes
c) aluminium oxalate – aluminium oxide does not contain carbon found in the oxalate polyatomic
ion
d) aluminium nitrate aluminium oxide does not contain nitrogen
9. Why is the name of HF (aq) hydrofluoric acid not
a) fluoric acid – the hydro is needed because it is not an oxygen containing acid
b) fluorous acid- the hydro is needed and the ending must be ic
10. Why is the name of HClO2 (aq) chlorous acid not
a) hydrochlorous acid - hydro is not needed because it is an oxygen containing acid
b) chloric acid- ite become ous acids
c) hypochlorous acid – ClO2- is a chlorite ion
11. Why is the name of HClO4 (aq) perchloric acid not
a) hydroperchloric acid – hydro is not needed
b) perchlorous acid – ate ions become ic acids
c) hydrochloric acid- hydro is not needed and ClO4- is a perchlorate ion not a chlorate ion
12. Why is the name of C2H5OH ethanol not
a) dicarbon hexahydrogen monoxide-ethanol is an organic compound named by the number of
carbons and its functional group
b) ethanoic acid – OH is an alcohol functional group not an acid functional group
c) carbon hydrogen oxide ethanol is an organic compound named by the number of carbons and
its functional group
13. The formula of lithium sulfate is Li2SO4 not
a) Li (SO4)2 Criss cross oxidation numbers
b) Li2S – lithium sulfide
14. The formula of Copper (I) oxide is Cu2O not
a) CuO
copper (II) oxide
b) CuCO3
copper (II) carbonate
15. The formula of Iron (II) sulfite is FeSO3 not
a) Fe2(SO3)2 reduce subscripts
b) Fe2SO3 the 2 subscripts is not needed
16. The formula of nickel (III) carbonate is Ni2(CO3)3 not
a) Ni3C carbonate is CO3 not a C
b) Ni3(CO3)2 criss cross
17. The formula of hydrosulfuric acid is H2S not
a) H2SO3 sulfurous acid
a) H2SO4 sulfuric acid
18. The formula of chloric acid is HClO3 not
a) HCl hydrochloric acid
b) HClO hypochlorous acid
c) HClO2 chlorous acid
d) HClO4 perchloric acid
19. The formula of nitrous acid is HNO2 (aq) not
a) H3N (aq) NH3 nitrogen trihydride with a common name of ammonia
b) HNO3 (aq) nitric acid
20 a) What is the name of each of the following
KClO2
potassium chlorate
Cu(NO2)2
Copper (II) nitrite
BaO
barium oxide
N2 O
dinitrogen monoxide
HBr(aq) hydrobromic acid
( ) 2(-2)
MnO2
manganese(IV)oxide
HNO2(aq)
nitrous acid
Ca(CN)2
calcium cyanide
H2CO3(aq)
carbonic acid
b) What is the formula of each?
Lead(II) iodide
calcium chloride
PbI2
CaCl2
hydroiodidic acid
HI(aq)
ammonium carbonate
(NH4)2CO3
strontium thiosulfate
SrS2O3
phosphoric acid
H3PO4
cobalt (III) sulfite
Co2(SO4)3
sulfurous acid
H2SO3(aq)