Unit 5 Bonding and Nomenclature

Report
lithium nitrate
lead (II) sulfide
lithium nitride
barium sulfide
lithium nitrite
Chemistry
sulfur dioxide
Unit 5: Bonding and
Inorganic Nomenclature
NaClO3
NO2
Fe(ClO3)2
N2O4
Fe(ClO3)3
N2O5
Bonding Types
1. Ionic Bonding
•
•
•
with ions (+/- charges)
atoms gaining/losing eM + NM
2. Covalent Bonding
•
•
atoms sharing eNM + NM
3. Metallic Bonding
•
•
•
metals share e- freely
“sea of e-”
good conductors
Chemical Bonding
Ionic Bonds: atoms give up or gain e– and
are attracted to each other by
coulombic attraction
Na
loses e–
Na+
Na+ + Cl–
Cl
gains e–
NaCl
ionic compounds = salts
K+ + NO3–
KNO3
Cl–
ionic bonds:
M + NM
cation + anion
where NO3– is a polyatomic ion:
a charged group of
atoms that stay together
Common Polyatomic Ions
Names of Common Polyatomic Ions
Ion
Name
Ion
Name
NH4 +
*NO2 NO3 *SO3 2SO4 2HSO4OH CN C2H3O2MnO4 PO4 3*PO3 3H2PO4 -
ammonium
*nitrite
nitrate
*sulfite
sulfate
hydrogen sulfate
hydroxide
cyanide
acetate
permanganate
phosphate
*phosphite
dihydrogen phosphate
CO3 2HCO3 *IO3*IO4*ClO *ClO2 ClO3 *ClO4 *BrO3C2O42Cr2O7 2CrO4 2O2 2-
carbonate
bicarbonate
*iodate
*periodate
*hypochlorite
*chlorite
chlorate
*perchlorate
*bromate
oxalate
dichromate
chromate
peroxide
Memorize the BOLD ions
Zumdahl, Zumdahl, DeCoste, World of Chemistry 2002, page 100
* = you will also be responsible
for knowing these
Polyatomic Ion Trends
*Charges NEVER change between different forms
+1 oxygen
“Per____ate”
BrO4perbromate
ClO4-
perchlorate
IO4periodate
“Normal”
“–ate” form
BrO3bromate
ClO3chlorate
IO3iodate
NO3nitrate
CO32carbonate
SO42sulfate
PO43phosphate
-1 oxygen
“-ite” form
-2 oxygens
“hypo___ite”
BrO2-
BrO-
bromite
hypobromite
ClO2-
ClO-
chlorite
hypochlorite
IO2-
IO-
iodite
hypoiodite
NO2nitrite
CO22carbonite
SO32sulfite
PO33phosphite
Properties of Ionic Salts
1. very hard
each ion is bonded
to several oppositely
charged ions
2. high melting points
3. brittle
many bonds must be
broken
with sufficient force,
like atoms are
brought next to
each other and repel
calcite
Writing Formulas of Ionic Compounds
chemical formula: has neutral charge;
shows types of atoms
and how many of each
To write an ionic compound’s formula, we need:
1. the two types of ions (i.e., cations and anions)
2. the charge on each ion
Na+
and
F–
NaF
Ba2+
and
O2–
BaO
Na+
Ba2+
and
and
O2–
Na2O
F–
BaF2
K+
e-
e-
potassium atom
BrBr
bromine atom
bromide ion
potassium
potassium
ion
bromide
Notice that the pink
pieces are cations
(metals) and the
blue are anions
(non-metals)
KBr
Br Mg2+
Br 1 Mg2+
2 Br -
MgBr2
magnesium bromide
K+
O2K+
potassium oxide
K2O
Chemical Bonding Activity Examples
N3-
Na+
Pb4+
OH -
1 Na
+
1 OH
N3-
-
N3-
Pb4+
NaOH
Pb4+
OH N3-
Mg2+
OH -
1 Mg2+
2 OH -
Mg OH 2
Pb4+
Pb3N4
N3Pb4+
N3-
criss-cross rule: charge on cation / anion
“becomes” subscript of
anion / cation
** Warning: Reduce to lowest terms
Al3+ and O2–
Ba2+ and S2–
In3+ and Br1–
Al 2 O 3
Ba 2S 2
In 1 Br 3
Al2O3
BaS
InBr3
Writing Formulas w/Polyatomic Ions
Parentheses are required only when you need more
than one “bunch” of a particular polyatomic ion
Ba2+
SO42–
BaSO4
Mg2+ and
NO2–
Mg(NO2)2
NH4+ and
ClO3–
NH4ClO3
Sn4+
and
SO42–
Sn(SO4)2
Fe3+
and
Cr2O72–
Fe2(Cr2O7)3
N3–
(NH4)3N
and
NH4+ and
The Importance of Parentheses
Calcium hydroxide
ide
Ca2+
OH-
CaOH2
Ca - O
H
H
vs.
Ca(OH)2
HO - Ca - OH
The formulas imply two totally different compounds!
Charges Reminder!
1+
2+
Group 1:
Group 2:
Group 3:
Group 5:
Group 6:
Group 7:
Group 8:
1+
2+
3+
3–
2–
1–
0
0
3+
3– 2– 1–
Inorganic Nomenclature
potassium
nitrate
KNO3
copper (II)
sulfate
CuSO4
dinitrogen monoxide
N2O
sodium
hydroxide
NaOH
Nomenclature - Humor
Fe2+
Fe2+
Fe2+
Fe2+
Fe2+
Fe2+
Fe2+
Fe2+
“Ferrous Wheel”
Fe = iron (Latin = ferrum)
Fe2+ = lower oxidation state = ferrous
Fe3+ = higher oxidation state = ferric
BaNa2
“BaNaNa”
What weapon can you make
from the elements nickel,
potassium and iron?
A KNiFe
Teacher: What is the formula for water?
Student: H, I, J, K, L, M, N, O
Teacher: That’s not what I taught you.
Student: But you said the formula for water was…H to O.
"H-O-H"?! WHAT'S
THAT SPELL?!
mis
WATER?
“Little Johnny took a drink,
Now he shall drink no more.
For what he thought was H2O,
Was H2SO4.”
Under aged Pb walks into a bar and the bartender turns to the gold
Bouncer and says, “Au, get the lead out!”
“Perhaps one of you gentlemen would mind telling me just
what is outside the window that you find so attractive..?”
Image courtesy NearingZero.net
Ionic Compounds (cation/anion combos)
Fixed-Charge Cations with Elemental Anions
i.e., “pulled off the
The fixed-charge cations are:
Table” anions
groups 1, 2, 13, Ag+ and Zn2+
1+
2+
3+
3– 2– 1–
Fixed-Charge Exceptions
3+
• Start with Al
• Go backwards down the stairs
• Decrease the charge after
each stair
3+
Al
13
2+
Zn
30
Ag
47
+
Fixed-charge cations
Variable-charge cations
Elemental anions
1+
1
H
1
2
3
7
2
3- 2- 1-
B
C
N
O
F
Ne
3
4
5
6
7
8
9
10
Al
Si
P
S
Cl
Ar
13
14
15
16
17
18
Na Mg
K
12
Ca Sc
Ti
V
Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br
Kr
23
24
35
36
I
Xe
53
54
20
21
22
Rb Sr
Y
Zr Nb Mo Tc Ru Rh Pd Ag Cd
In
39
40
41
42
49
Hf
Ta
W
72
73
74
37
6
1
Be
19
5
3+
He
Li
11
4
2+
H
38
Cs Ba
55
56
Fr
Ra
87
88
*
W
25
43
26
44
Re Os
75
76
27
28
29
47
30
45
46
Ir
Pt Au Hg
Tl
77
78
81
79
48
31
80
32
33
34
Sn Sb Te
50
51
Pb Bi
82
83
52
Po At Rn
84
85
86
Rf Db Sg Bh Hs Mt
104
105
106
107
108
109
La Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb Lu
57
58
59
Ac Th Pa
89
90
91
60
U
92
61
62
63
64
65
66
Np Pu Am Cm Bk Cf
93
94
95
96
97
98
67
68
69
70
71
Es Fm Md No Lr
99
100
101
102
103
1+
Na
2+
3+
3– 2– 1–
A. To name, given
the formula:
Ba
1. Use name of cation
2. Use name of anion (it has the ending “ide”)
NaF
sodium fluoride
BaO
barium oxide
Na2O
sodium oxide
BaF2
barium fluoride
Ca
Zn
1+
2+
3+
Ag
3– 2– 1–
B. To write formula,
given the name:
1. Write symbols for the two types of ions
2. Balance charges to write formula
silver sulfide
Ag+
S2–
Ag2S
zinc phosphide
Zn2+
P3–
Zn3P2
calcium iodide
Ca2+ I–
CaI2
Variable-Charge Cations with Elemental Anions
i.e., “pulled off the
Table” anions
The variable-charge cations are:
Pb, Sn, and the transition metals
(but – of course! – not Ag or Zn)
A. To name, given the formula:
Fe
Cu
1. Figure out charge on
cation.
2. Write name of cation.
3. Write Roman numerals
in ( ) to show cation’s charge.
4. Write name of anion.
-6
Stock System
of nomenclature
FeO
2+oxide
?
iron
Fe
O2–
Fe2O3
?
3+oxide
iron
Fe
Fe?3+ O2– O2–O2– iron (III) oxide
CuBr
–
copper
Cu+? Brbromide
copper (I) bromide
CuBr2
– Br –
copper
Cu?2+ Brbromide
copper (II) bromide
iron (II) oxide
B. To find the formula, given the name:
1. Write symbols for the two types of ions.
2. Balance charges to write formula.
Co
Sn
cobalt (III) chloride Co3+ Cl–
CoCl3
tin (IV) oxide
Sn4+ O2–
SnO2
tin (II) oxide
Sn2+ O2–
SnO
Ionic Nomenclature Practice
1. sodium hydroxide NaOH
9. iron (III) oxide
Fe2O3
2. HgSO4
mercury (II) sulfate 10. Mg(NO3)2
magnesium nitrate
3. lead (II) phosphate
4. (NH4)2S
Pb3(PO4)2
ammonium sulfide
5. aluminum chlorate
6. Cu2CO3
Al(ClO3)3
copper (I) carbonate
7. manganese (IV) oxide
8. MnSO4
MnO2
manganese (II) sulfate
11. calcium sulfide
CaS
12. K2O
potassium oxide
13. magnesium chloride
14. Cr2O3
MgCl2
chromium (III) oxide
15. gold (III) bromide
16. Zn(NO2)2
AuBr3
zinc nitrite
Traditional System of Nomenclature
…used historically (and still some today) to name
compounds w/multiple-charge cations
To use: 1. Use Latin root of cation.
2. Use -ic ending for higher charge;
-ous ending for lower charge.
3. Then say name of anion, as usual.
Element
gold, Au
lead, Pb
tin, Sn
copper, Cu
iron, Fe
Latin root
aurplumbstanncuprferr-
Write formulas:
cuprous sulfide
Cu+ S2–
Cu2S
auric nitride
Au3+ N3AuN
ferrous fluoride
FeF2
Fe2+ F–
-ic
Au3+
Pb4+
Sn4+
Cu2+
Fe3+
-ous
Au+
Pb2+
Sn2+
Cu+
Fe2+
Write names:
? P3–
Pb4+
Pb3P4
plumbic phosphide
Pb?2+ P3–
Pb3P2
plumbous phosphide
Sn?4+ Cl–
Sn
SnCl4
stannic chloride
Compounds Containing Polyatomic Ions
Insert name of ion
where it should go
in the compound’s
name.
Write formulas:
iron (III) nitrite
Fe3+ NO2–
Fe(NO2)3
ammonium phosphide
NH4+ P3–
(NH4)3P
ammonium chlorate
NH4+ ClO3–
NH4ClO3
zinc phosphate
Zn2+ PO43–
Zn3(PO4)2
lead (II) permanganate Pb2+ MnO4– Pb(MnO4)2
Write names:
(NH4)2S2O3
ammonium thiosulfate
AgBrO3
silver bromate
(NH4)3N
ammonium nitride
CrO42–
? CrO 2–
uranium (VI) chromate
U(CrO4)3 U6+
4
CrO42–
? SO 2–
Cr2(SO3)3 Cr3+
chromium (III) sulfite
3
Cr?3+SO32– SO32–
Self-Test Quiz
1. lithium nitrate
2. lithium nitride
3. lithium nitrite
4. NaClO3
5. Fe(ClO3)2
6. Fe(ClO3)3
7. lead(II) sulfide
8. barium sulfide
9. Never show charges
in a compound’s formula. (T/F)
10. When writing names with
Group 9 cations, you need to
use Roman numerals. (T/F)
11. When using an anion off the
polyatomic ion sheet, change
name’s ending to “-ide.” (T/F)
12. A Roman numeral indicates
the charge on the anion. (T/F)
Self-Test Quiz
Answers
1. lithium nitrate
LiNO3
2. lithium nitride
Li3N
3. lithium nitrite
LiNO2
4. NaClO3
sodium chlorate
5. Fe(ClO3)2
iron(II) chlorate
6. Fe(ClO3)3
iron(III) chlorate
7. lead(II) sulfide
PbS
8. barium sulfide
BaS
Self-Test Quiz
Answers
T
9. Never show charges
in a compound’s formula.
T
10. When writing names with
Group 9 cations, you need to
use Roman numerals.
11. When using an anion off the
polyatomic ion sheet, change
the name’s ending to “-ide.”
F
F
12. A Roman numeral indicates
the charge on the anion.
Covalent Bonds (2 nonmetals)
…atoms share e– to get a full valence shell
C
1s2 2s2 2p2 4 valence e1s2 2s2 2p5
F
7 valence e-
Both need 8 valence e- for a full outer shell…
otherwise known as the octet rule
o
o
C
o
xx
o
x
x
F
xx
x
Draw the Lewis dot structure for the
following elements:
Si
1s2 2s2 2p6 3s2 3p2
4 valence e-
O
1s2 2s2 2p4
6 valence e-
P
1s2 2s2 2p6 3s2 3p3
5 valence e-
B
1s2 2s2 2p1
3 valence e-
Ar
1s2 2s2 2p6 3s2 3p6
8 valence e-
Br
1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p5
7 valence e-
Notice any trends…?
Drawing Lewis Structures
Lewis structure:
a model of a covalent molecule that
shows all of the valence e–
1. Two shared e– make a single covalent bond,
four make a double bond, etc.
2. unshared pairs: pairs of unbonded valence e–
3. Each atom needs a full outer shell, i.e., 8 e–.
Exception: H needs 2 e–
Let’s bond two F atoms together…
Each F has 7 v.e. and each needs 1 more e-
F
F
F F
F2
Now let’s bond C and F atoms together…
carbon tetrafluoride (CF4)
F
F
C
F
F
F C F
F
F
And now,
a video break…
nitrogen triiodide (NI3)
x x
x
x
x x
x
x
o o
o
N
o
o
I
x x
x x
x
x
x
o o
o
x
I N
o
x x
x
x x
x
x
Ix x
x
x x
x
o
x
x
x
Ix x
I
x x
x
x
x
x
x x
I
carbon dioxide (CO2)
x x
o
o
x
x
o
C
o
x x
x
x
Ox
x
Ox
x
x x
x
x
Ox
o
x
o
o
C
o
xx
x
Ox
xx
x
x
xx
O
=C=O
xx
xx
covalent compounds = molecular compounds
-- have lower melting points
than do ionic compounds
(consist of two or more
nonmetal elements)
butter
Dihydrogen Monoxide:
A Tale of Danger and
Irresponsibility
major component of acid rain
found in all cancer cells
inhalation can be deadly
excessive ingestion results in
acute physical symptoms:
e.g., frequent urination,
bloated sensation,
profuse sweating
often an industrial byproduct of chemical
reactions; dumped wholesale into rivers and lakes
Covalent Compounds
-- contain two types of
nonmetals
** Key:
FORGET CHARGES!
Use Greek prefixes to indicate how
What to do:
many atoms of each element, but
don’t use “mono” on first element.
1 – mono
2 – di
3 – tri
6 – hexa
7 – hepta
8 – octa
4 – tetra
5 – penta
9 – nona
10 – deca
EXAMPLES:
carbon dioxide
CO2
CO
carbon monoxide
dinitrogen trioxide
N2O3
N2O5
dinitrogen pentoxide
carbon tetrachloride
CCl4
NI3
nitrogen triiodide
Metallic Bonds
In metals, valence shells of atoms overlap, so v.e–
are free to travel between atoms through material.
In insulators (like wood),
the v.e– are attached
to particular atoms.
Not so in metals.
Properties of Metals
ductile
malleable
conduct heat and electricity
All due to
free-moving
v.e–.
Other Types of Forces/Attractions
dipole-dipole forces
hydrogen bonds
London dispersion forces
ion-dipole forces
boiling
H2O
DNA
These are much weaker than ionic, covalent, or
metallic bonds, but very important in determining
states of matter, boiling and melting points, and
molecular shape (among other things).
Empirical Formula and Molecular Formula
lowest-terms
formula
shows the true number
and type of atoms in a m’cule
Compound
Molecular
Formula
Empirical
Formula
glucose
C6H12O6
CH2O
propane
C3H8
C3H8
butane
C4H10
C2H5
naphthalene
C10H8
C5H4
sucrose
C12H22O11
C12H22O11
octane
C8H18
C4H9
Nomenclature Review
Flow Chart
Formula  Name?
Metal + Nonmetal?
(Including NH4+)
Ionic
d,f-block
Pb,Sn
Metal
Type?
Columns 1, 2, 13
Ag+, Zn2+
Variable
Fixed
Two
Nonmetals?
Covalent
Steps 1 & 4 ONLY
1. Write name of cation (metal)
2. Determine the charge on the metal by balancing
the (-) charge from the anion
3. Write the charge of the metal in Roman Numerals
and put in parentheses
4. Write name of anion
(Individual anions need –ide ending!)
Use Prefixes!
*Mono*
Di
Tri
Tetra
Penta
Hexa
Hepta
Octa
Nona
Deca
Add –ide to 2nd element
Name  Formula?
No Prefixes?
Ionic
Prefixes?
Covalent
1. Determine the ions present
and the charge on each
(Roman Numeral = cation
charge, otherwise use PT)
1. FORGET CHARGES!!!
2. Balance formula (criss-cross)
3. Do NOT reduce
subscripts!
3. Reduce subscripts (if needed)
2. Use prefixes to
determine subscripts
Ionic Compounds
Covalent
Two nonmetals
Variable-charge cation
carbon
sulfur
tetrabromide
N
NCl
O35
2dichloride
vanadium
niobiumMn
Pt(IO
(V)
(II)
Sperchlorate
)4
2
53chromate
rubidium
sulfate
NH4KI
ClOoxide
barium
3
Roman numeral
for name only
Roman
numeral
Greek prefixes
Charge
CrissCross
Rule
Roman
numeral
Fixed-charge
Don’t know the charge from Know the charge from
PT
Polyatomic ions OK PT
Polyatomic ions OK
Where would you file this?
VCrO4
dinitrogen pentoxide
BaO
platinum (IV) iodate
CBr4
ammonium chlorate
Nb(ClO4)5
potassium iodide
SCl2
nitrogen trichloride
Rb2SO4
manganese (V) sulfide
Overall Nomenclature Practice
Ionic/variable
Ir F3
iridium (III) fluoride
Ca S
calcium sulfide
Ti S2
titanium (IV) sulfide
HCl(aq)
hydrochloric acid
Acid
BaBr2
barium bromide
Ionic/fixed
N3P2
trinitrogen diphosphide
Covalent
HF(aq)
hydrofluoric acid
Zn I2
zinc iodide
Ionic/fixed
NCl4
nitrogen tetrachloride
Covalent
Au 2O3
gold (III) oxide
Na 3P
sodium phosphide
Ionic/fixed
Ionic/variable
Acid
Ionic/variable
Ionic/fixed
Ionic Nomenclature Practice
Ionic/variable
Ir2 (Cr2O7)3
iridium (III) dichromate
Ca (OH)2
calcium hydroxide
HNO3 (aq)
nitric acid
Pt (CH3COO)2
platinum (II) acetate
HBrO2(aq)
bromous acid
Sr SO4
strontium sulfate
Ionic/fixed
KCN
potassium cyanide
Ionic/fixed
Zn (NO2)2
zinc nitrite
Ionic/fixed
Mn (ClO3)4
manganese (IV) chlorate
Ionic/variable
Au PO4
gold (III) phosphate
Ionic/variable
H2 SO3 (aq)
sulfurous acid
Ionic/fixed
Acid
Ionic/variable
Acid
Acid
Write the compound formed by the following ions:
1) Al3+ S22) Mg2+
PO43-
When a formula is given…write the proper name.
When a name is given…write the proper formula.
3) BaO
4) lithium bromide
5) Ni2S3
6) triphosphorus heptoxide
7) N2O5
8) molybdenum (VI) nitride
Write the total number of atoms that make up each compound.
9) trinitrotoluene (TNT)… CH3C6H2(NO2)3
10) phosphoric acid H3PO4
Extra credit: What is the formula for plumbic iodide? (Hint: lead is Pb2+ or Pb4+)
Write the compound formed by the following ions:
1) Al3+ S22) Mg2+
PO43-
When a formula is given…write the proper name.
When a name is given…write the proper formula.
3) BaO
POP
QUIZ
4) lithium bromide
5) Ni2S3
6) triphosphorus heptoxide
7) N2O5
8) molybdenum (VI) nitride
Write the total number of atoms that make up each compound.
9) trinitrotoluene (TNT)… CH3C6H2(NO2)3
10) phosphoric acid H3PO4
Extra credit: What is the formula for plumbic iodide? (Hint: lead is Pb2+ or Pb4+)
Answer Key
Write the compound formed by the following ions:
1) Al3+ S22) Mg2+
Al2S3
Mg3(PO4)2
PO43-
When a formula is given…write the proper name.
When a name is given…write the proper formula.
3) BaO
barium oxide
LiBr
4) lithium bromide
5) Ni2S3
nickel (III) sulfide
P3O7
6) triphosphorus heptoxide
7) N2O5
dinitrogen pentoxide
8) molybdenum (VI) nitride
MoN2
Write the total number of atoms that make up each compound.
9) trinitrotoluene (TNT)… CH3C6H2(NO2)3
10) phosphoric acid H3PO4
21
8
Extra credit: What is the formula for plumbic iodide? (Hint: lead is Pb2+ or Pb4+)
PbI4
Writing Chemical Names
Use poly.
Formula RN/GP/neither ion sheet?
Name
1. Ni2 S3
RN
no
nickel (III) sulfide
2. N F3
GP
no
nitrogen trifluoride
3. Na BrO3
neither
yes
sodium bromate
4. S F6
GP
no
sulfur hexafluoride
5. Fe (NO3)3
RN
yes
iron (III) nitrate
6. Sr SO4
neither
yes
strontium sulfate
Writing Chemical Formulas
Use poly.
Name
Charges matter? ion sheet?
1. copper (II) phosphide yes
no
2. lithium phosphate
yes
yes
Formula
Cu3P2
Li3PO4
3. phosphorus triiodide
no
no
PI3
4. zinc arsenate
yes
yes
Zn3(AsO4)2
5. silver nitride
yes
no
Ag3N
6. sulfur dibromide
no
no
SBr2
7. dinitrogen pentasulfide no
8. tin (IV) nitride
yes
no
no
N2S5
Sn3N4
9. rubidium nitrite
yes
yes
RbNO2
10. oxygen difluoride
no
no
OF2
11. iron (III) sulfite
12. ammonium oxide
yes
yes
yes
yes
Fe2(SO3)3
(NH4)2O
Writing Chemical Names
Use poly.
Formula RN/GP/neither ion sheet?
Name
7. S O3
8. Sn Br4
GP
neither
no
no
sulfur trioxide
tin (IV) bromide
9. K3 PO4
neither
yes
potassium phosphate
10. NH4 OH
neither
yes yes
ammonium hydroxide
11. C S2
12. Cu F
GP
RN
no
no
carbon disulfide
copper (I) fluoride
Writing Chemical Formulas
Use poly.
Name
Charges matter? ion sheet?
1. copper (II) phosphide yes
no
2. lithium phosphate
yes
yes
Formula
Cu3P2
Li3PO4
3. phosphorus triiodide
no
no
PI3
4. zinc arsenate
yes
yes
Zn3(AsO4)2
5. silver nitride
yes
no
Ag3N
6. sulfur dibromide
no
no
SBr2
7. dinitrogen pentasulfide no
8. tin (IV) nitride
yes
no
no
N2S5
Sn3N4
9. rubidium nitrite
yes
yes
RbNO2
10. oxygen difluoride
no
no
OF2
11. iron (III) sulfite
12. ammonium oxide
yes
yes
yes
yes
Fe2(SO3)3
(NH4)2O
Writing Chemical Formulas
Use poly.
Name
Charges matter? ion sheet?
1. copper (II) phosphide yes
no
2. lithium phosphate
yes
yes
Formula
Cu3P2
Li3PO4
3. phosphorus triiodide
no
no
PI3
4. zinc arsenate
yes
yes
Zn3(AsO4)2
5. silver nitride
yes
no
Ag3N
6. sulfur dibromide
no
no
SBr2
7. dinitrogen pentasulfide no
8. tin (IV) nitride
yes
no
no
N2S5
Sn3N4
9. rubidium nitrite
yes
yes
RbNO2
10. oxygen difluoride
no
no
OF2
11. iron (III) sulfite
12. ammonium oxide
yes
yes
yes
yes
Fe2(SO3)3
(NH4)2O
Writing Chemical Names
Use poly.
Formula RN/GP/neither ion sheet?
Name
1. Ni2 S3
RN
no
nickel (III) sulfide
2. N F3
GP
no
nitrogen trifluoride
3. Na BrO3
neither
yes
sodium bromate
4. S F6
GP
no
sulfur hexafluoride
5. Fe (NO3)3
RN
yes
iron (III) nitrate
6. Sr SO4
neither
yes
strontium sulfate
7. S O3
8. Sn Br4
GP
neither
no
no
sulfur trioxide
tin (IV) bromide
9. K3 PO4
neither
yes
potassium phosphate
10. NH4 OH
neither
yes
ammonium hydroxide
11. C S2
12. Cu F
GP
RN
no
no
carbon disulfide
copper (I) fluoride
Writing Chemical Formulas
Name
Charges matter?
1. copper (II) phosphide yes
2. lithium phosphate
yes
Use poly.
ion sheet?
no
yes
Formula
Cu3P2
Li3PO4
3. phosphorus triiodide
no
no
PI3
4. zinc arsenate
yes
yes
Zn3(AsO4)2
5. silver nitride
yes
no
Ag3N
6. sulfur dibromide
no
no
SBr2
7. dinitrogen pentasulfide no
8. tin (IV) nitride
yes
no
no
N2S5
Sn3N4
9. rubidium nitrite
yes
yes
RbNO2
10. oxygen difluoride
no
no
OF2
11. iron (III) sulfite
12. ammonium oxide
yes
yes
yes
yes
Fe2(SO3)3
(NH4)2O

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