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Chemical Bonds
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What is a chemical bond? Why do chemical bonds form?
• A chemical bond is a type of attractive force that forms between atoms.
• All atoms react to obtain a stable and full outer electron configuration.
• Only noble gases naturally possess a stable arrangement that includes a perfect balance and distance between the positive protons and negative electrons.
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The Octet Rule• All noble gases except He has an s2p6 configuration (Note:
2 + 6 = 8….”octet” means the number 8)
• Octet rule: atoms tend to gain, lose, or share electrons until they are surrounded by 8 valence electrons (4 electron pairs).
• Caution: there are many exceptions to the octet rule. For example; H, He Li and Be follow “duet rule.”
The Octet RuleThe Octet Rule
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How do atoms achieve a full “octet?”
• Atoms will gain, lose or share electrons to achieve a stable, completely full outer electron shell. (called valence shell).
• The gaining or losing of valence electrons is a CHEMICAL REACTION!!
• The difference in electronegativity values of atoms, when placed into contact with each other, determines the loss or gain of electrons.
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Bonding and ElectronegativityBonding and Electronegativity
Electronegativity• Electronegativity: The ability of one atom or group of
atoms to attract electrons to itself.• Pauling set electronegativities on a scale from 0.7 (Cs) to
4.0 (F).• Electronegativity increases
• across a period and • down a group.
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Electronegativities of ElementsElectronegativities of ElementsElectronegativity
http://group.chem.iastate.edu/Greenbowe/sections/projectfolder/flashfiles/reaction/bonding1.swfAnimation of electron transfer between selected atoms.
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Lewis Structures
-Chemical reactions involve valence electrons.
-Lewis structures are shorthand version of atoms showing only their valence electrons.
-Why?? Only valence electrons transferred
during most chemical reactions.
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Lewis Symbols
Examples of Longhand and Lewis Electron SymbolsExamples of Longhand and Lewis Electron Symbols
http://www.mhhe.com/physsci/chemistry/chang7/esp/folder_structure/bo/m2/s1/index.htmAnimation of Lewis Diagrams
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Chemical Bonding
…atoms share electrons to get a full valence shell
Covalent Bonds
C 2s2 2p2 (4 v.e–)
F 2s2 2p5 (7 v.e–)
both need 8 valence electrons for a full outer shell(octet rule)
1s2
1s2
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Covalent bonding
F F
• Fluorine has seven valence electrons• A second F atom also has seven• By sharing electrons• Both end with full orbitals (stable octets)
8 Valence electrons
8 Valence electrons
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Chemical Bonding
Ionic Bonds:atoms give up or gain electrons and are attracted to each other by coulombic attraction
Na loses an e–
Na Na1+ + e–
Cl gains an e–
Cl + e– Cl1–
ionic compounds = salts Na1+ + Cl1– NaCl
K1+ + NO31– KNO3
where NO31– is a polyatomic ion: a charged group of atoms
that stay together
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Ionic Bonding
-
-
-
-
-
- -
-
-
-
-
- -
-
- -
n = 2
Na[Ne]3s1
n = 3
n = 3
+
-
-
-
-
-
- -
--
-
- -
-
- -
-
Cl[Ne]3s23p5
Na+
[Ne]Cl-
[Ne]3s23p6
NaCl
Transfer of electrons to achieve a stable octet (8 electrons in valence shell).
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Copyright © 2007 Pearson Benjamin Cummings. All rights reserved.
Na + Cl2 NaCl
sodium metal and chlorine gas react to form sodium chloride
2 2
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Covalent Bonding
-
-
-
-
n = 1
O[He]2s22p4
n = 2
+
-
----
-
-
O2
Sharing of electrons to achieve a stable octet (8 electrons in valence shell).
-
-
-
-
-
-
-
-
-
-
-
-
-
-
-
-
-
O[He]2s22p4
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Properties of Salts
VERY HARD each ion is bonded to several oppositely-charged ions
HIGH MELTING POINTS many bonds must be broken
BRITTLE with sufficient force, like atoms are brought next to each other and repel
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Vocabulary
• Chemical Bond
– attractive force between atoms or ions that binds them together as a unit
– bonds form in order to…• decrease potential energy (PE)
• increase stability
Courtesy Christy Johannesson www.nisd.net/communicationsarts/pages/chem
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Vocabulary
CHEMICAL FORMULA
molecularformula
formulaunit
IONIC COVALENT
COCO22NaClNaClCourtesy Christy Johannesson www.nisd.net/communicationsarts/pages/chem
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Vocabulary
COMPOUND
ternarycompound
binarycompound
2 elementsmore than 2
elements
NaNONaNO33NaClNaClCourtesy Christy Johannesson www.nisd.net/communicationsarts/pages/chem
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Vocabulary
ION
polyatomicIon
monatomicIon
1 atom 2 or more atoms
NONO33--NaNa++
Courtesy Christy Johannesson www.nisd.net/communicationsarts/pages/chem
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IONIC COVALENT
Bond Formation
Type of Structure
Solubility in Water
Electrical Conductivity
OtherProperties
e- are transferred from metal to nonmetal
high
yes (solution or liquid)
yes
e- are shared between two nonmetals
low
no
usually not
MeltingPoint
crystal lattice true molecules
Types of Bonds
Physical State
solid liquid or gas
odorousCourtesy Christy Johannesson www.nisd.net/communicationsarts/pages/chem
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“electron sea”
METALLIC
bond formation
type of structure
solubility in water
conductivity
other properties
melting point
Types of Bonds
physical state
electrons are delocalized among metal atoms
very high
yes (any form)
no
malleable, ductile, lustrous
solid
Courtesy Christy Johannesson www.nisd.net/communicationsarts/pages/chem
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Ionic Bonding - Crystal Lattice
Types of Bonds
Table salt
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Ionic Bonding - Crystal Lattice
Types of Bonds
Table salt
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Covalent Bonding - True Molecules
Types of Bonds
Diatomic Molecule
Ammonia
Nitrogen
Water
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Lewis Structure
Lewis structure: a model of a covalent molecule thatshows all of the valence electrons
1. Two shared electrons make a single covalent bond,
four make a double bond, etc.
2. unshared pairs: pairs of un-bonded valence electrons
3. Each atom needs a full outer shell, i.e., 8 electrons. Exception: H needs 2 electrons
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Lewis Structure
carbon tetrafluoride (CF4)
o
Co
o
o x
xx
x
x x
F x
o
Co
o
ox
xx
x
x x
F x
x x
x
x
x x
F x
x
xx
x
x
F x
x
x
xx
x x
F x
xCx
xx
x
x x
F
x x
x
x x
F x
x
xx
x F x
x
xx
x x
F x
x
covalent compounds = molecular compounds(have lower melting points than do ionic compounds)
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Lewis Structure
o
Co
o o
x
Ho
Co
o oH x
x
H
xH
x H CH
H
H
H
x
xxx
x x
I x
o
No
o o
o o
No
o ox
xxx
x x
I x
x x
xx
x x
I x
xxx
x x I
x
x
o o
Nx
xxx
x x
I
x xx
x x
I x
xx
x x I
x
x
o
o
Co
o o x
xxx
xO x
x
xxx
xO x
x
xxx
xO x
o
Co
o o O = C = O
x x
x x x x
x x
methane (CH4)
carbon dioxide (CO2)
nitrogen triiodide (NI3)
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Properties of Metalsconduct heat and electricity; ductile; malleable
Other Types of Bondsdipole-dipole forceshydrogen bondsLondon dispersion forces ion-dipole forces (solutions)
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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 ions2. the charge on each ion
Na1+ and F1–
Ba2+ and O2–
Na1+ and O2–
Ba2+ and F1–
NaF
BaO
Na2O
BaF2
sodium fluoride
barium oxide
sodium oxide
barium fluoride
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Ca3P2
Formula Unit
Ca2+
Ca2+
Ca2+
P3-
P 3-
Ca2+
P3- Ca2+
P3- Ca2+
Ca2+ and P3– Ca3P2 calcium phosphide
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InBr3BaS
Criss-Cross Rule
criss-cross rule: charge on cation / anion
“becomes” subscript of anion / cation
** Warning: Reduce to lowest terms.
Al2O3
Al3+ and O2–
Al2 O3
Ba2+ and S2–
Ba2 S2
In3+ and Br1–
In1 Br3
aluminum oxide barium sulfide indium bromide
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(NH4)3N
Fe2(Cr2O7)3
Sn(SO4)2
NH4ClO3
Mg(NO2)2
BaSO4
Writing Formulas w/Polyatomic Ions
Parentheses are required only when you need more than one “bunch” of a particular polyatomic ion.
Ba2+ and SO4
2–
Mg2+ and NO2
1–
NH41+ and ClO3
1–
Sn4+ and SO42–
Fe3+ and Cr2O72–
NH41+ and N3–
barium sulfate
magnesium nitrite
ammonium chlorate
tin (IV) sulfate
iron (III) dichromate
ammonium nitride
?
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Compounds Containing Polyatomic Ions
Insert name of ion where it should go in the compound’s name.
Write formulas:
iron (III) nitrate
ammonium phosphide
ammonium chlorite
zinc phosphate
lead (II) permanganate
Fe(NO3)3
(NH4)3P
NH4ClO2
Zn3(PO4)2
Pb(MnO4)2
Fe3+ NO31–
NH41+ P3–
NH41+ ClO2
1–
Zn2+ PO43–
Pb2+ MnO41–
3
3
3 2
2
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Write names:
(NH4)2S2O3
AgBrO3
(NH4)3N
U(CrO4)3
Cr2(SO3)3
Writing Formulas of Ionic Compounds
ammonium thiosulfate
silver bromate
ammonium nitride
uranium (VI) chromate
chromium (III) sulfite
CrO42–
SO32–
3
32 Cr
U?
?
6+
3+
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Writing Formulas of Covalent Molecules
Covalent Moleculescontain two types of nonmetals
Key: FORGET CHARGES
What to do:Use Greek prefixes to indicate how many atoms
of each element, but don’t use “mono” on first element.
1 – mono 6 – hexa2 – di 7 – hepta3 – tri 8 – octa4 – tetra 9 – nona5 – penta 10 – deca
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Writing Formulas of Covalent Molecules
EXAMPLES:
carbon dioxide
CO
dinitrogen trioxide
N2O5
carbon tetrachloride
NI3
CO2
carbon monoxide
N2O3
dinitrogen pentoxide
CCl4
nitrogen triiodide
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Cu 2 Br1–
Cu Br1–
2 Fe 3 O2–
Fe O2–
Stock Systemof nomenclature
4. Write name of anion.
FeO
Fe2O3
CuBr
CuBr2
iron (II) oxide
iron (III) oxide
copper (I) bromide
copper (II) bromide
?
?
?
?
A. To name, given the formula:
1. Figure out charge on cation.
2. Write name of cation.
3. Write Roman numerals in ( ) to show cation’s charge.
Pb2+/Pb4+,Sn2+/Sn4+,transition elements (not Ag or Zn)
Multiple-Charge Cations with Elemental Anions
2+
3+
1+
2+
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B. To find the formula, given the name:
2. Balance charges to write formula.
cobalt (III) chloride Co3+ Cl1– CoCl3
tin (IV) oxide Sn4+ O2– SnO2
tin (II) oxide Sn2+ O2– SnO
1. Write symbols for the two types of ions.
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Element Latin root -ic -ous
gold, Au aur- Au3+ Au1+
lead, Pb plumb- Pb4+ Pb2+
tin, Sn stann- Sn4+ Sn2+
copper, Cu cupr- Cu2+ Cu1+
iron, Fe ferr- Fe3+ Fe2+
Traditional (OLD) 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 “ “ lower “ 3. Then say name of anion, as usual.
; (“icky” food is good for you!); (“delicious” food is not good for you!)
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Cu2S
AuN
FeF2
plumbic phosphide
plumbous phosphide
stannic chlorideFe2+
Write formulas: Write names:
cuprous sulfide
auric nitride
ferrous fluoride
Pb3P4 3 Pb? 4 P3–
Cu1+
Pb3P2 3 Pb? 2 P3–
Au3+
SnCl4 Sn? 4 Cl1–
S2–
N3–
F1–
copper (I) sulfide
gold (III) nitride
iron (II) fluoride
lead (IV) phosphide
lead (II) phosphide
tin (IV) chloride
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O2-
K1+
K1+
Mg2+
Br1-
Br1-
K Br
potassium atom bromine atom
e- e- Br1-K1+
potassium ion bromide ionpotassium bromide
K Br
potassium atom bromine atom
e-
Br1-K1+
potassium ion bromide ion
KBr
MgBr2 K2Omagnesium bromide potassium oxide
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Ca2+
Al3+
K1+
Pb4+
Br1-
O2-
N3-
K1+
K1+
Mg2+
Br1-
Br1-
PO43-
S2-
Cu2+
OH1-
OH1-NH41+
NO31-
?
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Chemical Bonding Activity
Ca2+
Al3+
Na1+
Pb4+
OH1-
N2-
N3-
M1+
Mg2+
OH1-
OH1-
N3-
Pb4+
N3-
N3-
Pb4+
N3-
Pb4+
N3-
?
(nonmetal)M1+
(metal)
Pb4+ N3-
(metal)(metal)
M2+
(metal)
Pb3N4
lead (IV) nitrideor
plumbic nitride
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Key
Cu2+
Al3+
K1+ Pb4+Br1-
O2-
N3-
K1+
K1+
Mg2+
Br1-
Br1-
N3-
N3-
Pb4+
N3-
Pb4+
N3-
1.
2.
3.
4. 5.
6. OH1-
OH1-
NH41+
NO31-
7.
KBr
K2O
MgBr2
AlN
Cu(OH)2
NH4NO3
Pb3N4
http://www.unit5.org/christjs/4bondingact.doc
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Key
Fe2+
8. 9. 10.
Ca2+
Ca2+
Ca2+
PO43-
PO43-
PO43-
NH41+
NH41+
NH41+
O2-
Al3+
Al3+
O2-
O2-
O2-
11.
Ca3(PO4)2
(NH4)3PO4
FeOAl2O3
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Key
12.
15.
O2-
O2-
Fe3+
Fe3+
O2-
O2-
O2-
13.
Pb4+
S2-
S2-
Pb4+
S2-
S2-
Pb2+ S2-
14.
Cu2+
Cu1+
Cu1+
16.
Fe2O3
Pb2S3
PbS
CuO
Cu2OPb2S4PbS2
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Binary CompoundsContaining a Metal of Variable Oxidation Number
To name these compounds, give the name of the metal (Type II cations) followed by Roman numerals in parentheses to indicate the oxidation number of the metal, followed by the name of the nonmetal, with its ending replaced by the suffix –ide.
Examples Stock System
FeCl2
(“ic” ending = higher oxidation state; “ous” is lower oxidation state)
SnO Tin oxideSnO2 Tin oxide
(II)
(III)
(II)
(IV)
Traditional (OLD) System
Ferrous chlorideFerric chloride
Stannous oxideStannic oxide
Iron chlorideIron chlorideFeCl3
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Type II CationsCommon Type II Cations
Ion Stock System Traditional System
Fe 3+ iron (III) ferric Fe 2+ iron (II) ferrous Cu 2+ copper (II) cupric Cu 1+ copper (I) cuprous Co 3+ cobalt (III) cobaltic Co 2+ cobalt (II) cobaltous Sn 4+ tin (IV) stannic Sn 2+ tin (II) stannous Pb 4+ lead (IV) plumbic Pb 2+ lead (II) plumbous Hg 2+ mercury (II) mercuric Hg2 2+ mercury (I) mercurous
*Mercury (I) ions are always bound together in pairs to form Hg2 2+
Zumdahl, Zumdahl, DeCoste, World of Chemistry 2002, page 90
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Naming Binary Compounds
Formula Name
1 Hg2O ____________________
2 HgO ____________________
3 ________________ copper (II) fluoride
4 ________________ copper (I) sulfide
5 Cr2O3 ____________________
6 ________________ lead (IV) oxide
mercury (I) oxide
PbO2
mercury (II) oxide
CuF2
Cu2S
chromium (III) oxide
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Li
3
H
1
He
2
C
6
N
7
O
8
F
9
Ne
10
Na
11
B
5
Be
4
H
1
Al
13
Si
14
P
15
S
16
Cl
17
Ar
18
K
19
Ca
20
Sc
21
Ti
22
V
23
Cr
24
Mn
25
Fe
26
Co
27
Ni
28
Cu
29
Zn
30
Ga
31
Ge
32
As
33
Se
34
Br
35
Kr
36
Rb
37
Sr
38
Y
39
Zr
40
Nb
41
Mo
42
Tc
43
Ru
44
Rh
45
Pd
46
Ag
47
Cd
48
In
49
Sn
50
Sb
51
Te
52
I
53
Xe
54
Cs
55
Ba
56
Hf
72
Ta
73
W
74
Re
75
Os
76
Ir
77
Pt
78
Au
79
Hg
80
Tl
81
Pb
82
Bi
83
Po
84
At
85
Rn
86
Fr
87
Ra
88
Rf
104
Db
105
Sg
106
Bh
107
Hs
108
Mt
109
Mg
12
Ce
58
Pr
59
Nd
60
Pm
61
Sm
62
Eu
63
Gd
64
Tb
65
Dy
66
Ho
67
Er
68
Tm
69
Yb
70
Lu
71
Th
90
Pa
91
U
92
Np
93
Pu
94
Am
95
Cm
96
Bk
97
Cf
98
Es
99
Fm
100
Md
101
No
102
Lr
103
La
57
Ac
89
1
2
3
4
5
6
7
Single-charge cationsMultiple-charge cations
Elemental anions
1+
2+
1+ 2+
3+ 1-2-3-
Periodic Table with
charges
Periodic Table with
charges
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Binary Compounds Containing Two Nonmetals
To name these compounds, give the name of the less electronegative element first with the Greek prefix indicating the number of atoms of that element present, followed by the name of the more electronegative non-metal with the Greek prefix indicating the number of atoms of that element present and with its ending replaced by the suffix –ide.
Prefixes you should know:
Mono Di Tri Tetra Penta Hexa Hepta Octa Nona Deca
1 2 3 4 5 6 7 8 9 10
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Binary CompoundsContaining Two Nonmetals (Type III Compounds)
1. ________________ diarsenic trisulfide
2. ________________ sulfur dioxide
3. P2O5 ____________________
4. ________________ carbon dioxide
5. N2O5 ____________________
6. H2O ____________________
As2S3
SO2
diphosphorus pentoxide
CO2
dinitrogen pentoxide
dihydrogen monoxide
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Prefixes – Binary Molecular CompoundsGreek Prefixes for Two Nonmetals
Number Indicated Prefixes
1 mono- 2 di- 3 tri- 4 tetra- 5 penta- 6 hexa- 7 hepta- 8 octa- 9 nona-10 deca-
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Binary Molecular Compounds
N2O dinitrogen monoxideN2O3 dinitrogen trioxideN2O5 dinitrogen pentoxide
ICl iodine monochlorideICl3 iodine trichloride
SO2 sulfur dioxideSO3 sulfur trioxide
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Naming Binary CompoundsBinary Compound?
Metal Present?
Does the metal formmore than one cation?
Type IIIUse Greek
Prefixes
Type IUse the elementname for the cation.
Type IIDetermine the charge of the cation; use a Romannumeral after the cationname.
Yes
Yes
YesNo
No
Zumdahl, Zumdahl, DeCoste, World of Chemistry 2002, page 98
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Ternary Compounds
Ternary compounds are those containing three different elements. (NaNO3, NH4Cl, etc.). The naming of ternary compounds involves the memorization of several positive and negative polyatomic ions, (two or more atoms per ion), and adding these names to the element with which they combine.
i.e., Sodium ion, Na1+ added to the nitrate ion, NO31-, to give
the compound, NaNO3, sodium nitrate.
Binary rules for indicating the oxidation number of metals and for indicating the numbers of atoms present are followed. The polyatomic ions that shouldbe learned are listed in a separate handout.
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(PO4)3-
Phosphate
PO43-
1 P 4 O @ 2- = 8-
@ 3- = 3-
11-
?@ 5+ = 5+
3-
Fluorine and oxygenoxygen are highly electronegative and will attractelectrons very strongly. Generally, phosphorus will be 3- oxidation state: however, when combining with oxygen, phosphorus will lose
five electrons and take on a 5+ oxidation charge.
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phosphate
sulfate
carbonate
chlorate
nitrate
Polyatomic Ions - Memorize
phosphATE
sulfATE
carbonATE
chlorATE
nitrATE
PO43- ……………
SO42- ……………
CO32- …………..
ClO31- …………..
NO31- ………..….
Eight “-ATE’s”
Exceptions:
ammonium
hydroxide
cyanide
NH41+ ……………
OH1- ……………
CN1- …………..
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Pattern to Memorizing Nomenclature
XY“-ide”
XYO3“-ate”
XYO2“-ite”
XYO“hypo___-ite”
XYO4“per___-ate”
normal 1 less oxygen 2 less oxygen1 more oxygen
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Polyatomic Ion: a group of atoms that stay together and have a single, overall charge.
BrO41-
Perbromate ion
BrO31-
Bromate ion
BrO21-
Bromite ion
BrO1-
Hypobromite ion
CO42- CO3
2-
Carbonate ion
CO22- CO2-
ClO41- ClO3
1-
Chlorate ion
ClO21- ClO1-
IO41- IO3
1-
Iodate ion
IO21- IO1-
NO41- NO3
1-
Nitrate ion
NO21- NO1-
PO53- PO4
3-
Phosphate ion
PO33- PO2
3-
SO52- SO4
2-
Sulfate ion
SO32- SO2
2-
1 more oxygen “normal” 1 less oxygen 2 less oxygen
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Polyatomic Ion: a group of atoms that stay together and have a single, overall charge.
BrO41-
Perbromate ion
BrO31-
Bromate ion
BrO21-
Bromite ion
BrO1-
Hypobromite ion
CO42- CO3
2-
Carbonate ion
CO22- CO2-
ClO41- ClO3
1-
Chlorate ion
ClO21- ClO1-
IO41- IO3
1-
Iodate ion
IO21- IO1-
NO41- NO3
1-
Nitrate ion
NO21- NO1-
PO53- PO4
3-
Phosphate ion
PO33- PO2
3-
SO52- SO4
2-
Sulfate ion
SO32- SO2
2-
1 more oxygen “normal” 1 less oxygen 2 less oxygen
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Ternary Compounds
NaNO2 sodium nitrite
KClO3 potassium chlorate
Ca3(PO4)2 calcium phosphate
Fe(OH)3 iron (III) hydroxide
NaHCO3 sodium bicarbonate ‘sodium hydrogen carbonate’
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ideCalcium hydroxide
Ca2+ OH1-
CaOH2
Ca(OH)2
Ca - OH
H
HO - Ca - OH
vs.
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Common Polyatomic Ions
Names of Common Polyatomic Ions
Ion Name Ion Name
NH4 1+ ammonium CO3 2- carbonate
NO2 1- nitrite HCO3 1- hydrogen carbonate NO3 1- nitrate (“bicarbonate” is a widely SO3 2- sulfite used common name) SO4 2- sulfate ClO 1- hypochlorite HSO4 1- hydrogen sulfateClO2 1- chlorite
(“bisulfate” is a widely ClO3 1- chlorate used common name) ClO4 1- perchlorate OH 1- hydroxide C2H3O2 2- acetate CN 1- cyanide MnO4 1- permanganate PO4 3- phosphate Cr2O7 2- dichromate HPO4 2- hydrogen phosphate CrO4 2- chromate H2PO4 1- dihydrogen phosphate O2 2- peroxide
Zumdahl, Zumdahl, DeCoste, World of Chemistry 2002, page 100 Print Version
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Ternary Compounds
1. ________________ calcium phosphate
2. ________________ ammonium carbonate
3. ________________ aluminum sulfate
4. Na2SO4 ____________________
5. LiCN ____________________
6. Ba(ClO3)2 ____________________
7. ________________ copper (II) hydroxide
Ca3(PO4) 2
(NH4)2CO3
Al2(SO4)3
sodium sulfate
lithium cyanide
barium chlorate
Cu(OH)2
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Magnesium Phosphate
Step 1: Magnesium Phosphate
Step 2: Mg2+ PO43-
Step 3: Mg (PO4)3 2
Step 4: Mg3(PO4)2
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fluoride
sulfide
sulfide
chloride
bromide
phosphide
fluoride
iodide
chloride
oxide
phosphide
iridium (III)
calcium
titanium (IV)
platinum (II)
barium
strontium
potassium
zinc
manganese (IV)
gold (III)
sodium
dichromate
hydroxide
chromate
acetate
bromate
sulfate
cyanide
nitrite
chlorate
phosphate
nitrate
2(Cr2O7)3
(OH)2
(CrO4)2
(CH3COO)2
(BrO3)2
SO4
CN
(NO2)2
(ClO3)4
PO4
NO3
Ir
Ca
Ti
Pt
Ba
Sr
K
Zn
Mn
Au
Na
F3
S
S2
Cl2
Br2
3P2
F
I2
Cl4
2O3
3P
Ir2+,3+,4+,6+
Ca2+
Ti3+,4+
Pt2+,4+
Ba2+
Sr2+
K1+
Zn2+
Mn2,3,4,6,7+
Au1+,3+
Na1+
variable
fixed
variable
variable
fixed
fixed
fixed
fixed
variable
variable
fixed
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fluoride
sulfide
sulfide
chloride
bromide
phosphide
fluoride
iodide
chloride
oxide
phosphide
iridium (III)
calcium
titanium (IV)
platinum (II)
barium
strontium
potassium
zinc
manganese (IV)
gold (III)
sodium
Ir
Ca
Ti
Pt
Ba
Sr
K
Zn
Mn
Au
Na
F3
S
S2
Cl2
Br2
3P2
F
I2
Cl4
2O3
3P
Ir2+,3+,4+,6+
Ca2+
Ti3+,4+
Pt2+,4+
Ba2+
Sr2+
K1+
Zn2+
Mn2,3,4,6,7+
Au1+,3+
Na1+
variable
fixed
variable
variable
fixed
fixed
fixed
fixed
variable
variable
fixed
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dichromate
hydroxide
chromate
acetate
bromate
sulfate
cyanide
nitrite
chlorate
phosphate
nitrate
iridium (III)
calcium
titanium (IV)
platinum (II)
barium
strontium
potassium
zinc
manganese (IV)
gold (III)
sodium
2(Cr2O7)3
(OH)2
(CrO4)2
(CH3COO)2
(BrO3)2
3SO4
CN
(NO2)2
(ClO3)4
PO4
NO3
Ir
Ca
Ti
Pt
Ba
Sr
K
Zn
Mn
Au
Na
Ir2+,3+,4+,6+
Ca2+
Ti3+,4+
Pt2+,4+
Ba2+
Sr2+
K1+
Zn2+
Mn2,3,4,6,7+
Au1+,3+
Na1+
variable
fixed
variable
variable
fixed
fixed
fixed
fixed
variable
variable
fixed
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Two nonmetals Multiple-charge cation Everything else
Romannumeral
Polyatomic ions OK
Roman numeralfor name only
Polyatomic ions
Greek prefixes
Charge
Criss-CrossRule
Romannumeral
OK
Where would you file this?
VCrO4
BaO
CBr4
Nb(ClO4)5
SCl2
Rb2SO4
dinitrogen pentoxide
platinum (IV) iodate
ammonium chlorate
potassium iodide
nitrogen trichloride
manganese (V) sulfide
vanadium (II) chromate
VCrO4
N2O5
dinitrogen pentoxide
barium oxide
BaO
Pt(IO3)4
platinum (IV) iodate
carbon tetrabromide
CBr4
NH4ClO3
ammonium chlorate
niobium (V) perchlorate
Nb(ClO4)5
KI
potassium iodide
sulfur dichloride
SCl2
NCl3
nitrogen trichloride
rubidium sulfate
Rb2SO4
Mn2S5
manganese (V) sulfide
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Two nonmetals Multiple-charge cation Everything else
Romannumeral
Polyatomic ions
Roman numeralfor name only
Polyatomic ions
Greek prefixes
Charge
Criss-CrossRule
Romannumeral
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
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Write the total number of atoms that make up each compound.
Write the compound formed by the following ions:1) Al3+ S2-
2) 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
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+)
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Write the total number of atoms that make up each compound.
Write the compound formed by the following ions:1) Al3+ S2-
2) 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
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+)
POP QUIZ
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Write the total number of atoms that make up each compound.
Write the compound formed by the following ions:1) Al3+ S2-
2) 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
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
Al2S3
Mg3(PO4)2
barium oxide
nickel (III) sulfide
LiBr
dinitrogen pentoxide
MoN2
8
21
PbI4
P3O7
aluminum sulfide
magnesium phosphate
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Polyatomic Ions - Quiz
oxalate
chromate
dichromate
permanganate
acetate
C2O42- ……………
CrO42- ……………
Cr2O72- …………..
MnO41- …………..
CH3COO1- …….
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K2O
Exceptions!Two exceptions to the simple –ide ending are the diatomic oxide ions, O2
2- and O21-.
O22- is called peroxide
O21- is called superoxide.
Note the differences.
barium oxide __________barium peroxide __________
sodium oxide __________sodium peroxide __________
potassium oxide __________potassium superoxide __________
BaO
Na2O
Do Not Reduce to lowest terms!
KO2
Ba2+
Na1+
K1+
BaO2
Na2O2
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Naming Chemical Compounds
Binary Compound?
Use the strategysummarized
earlier
Polyatomic ions present?
This is a compound for which naming procedures have not yet been considered.
Name the compound using procedures similar to those for naming binary ionic compounds.
Yes
YesNo
No
Zumdahl, Zumdahl, DeCoste, World of Chemistry 2002, page 102
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Nomenclature Review Flow Chart
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Metal + Nonmetal?
Formula Name?
Ionic
Covalent
Two Nonmetals?
Multiple Single
Use Prefixes!!!
*Mono* HexaDi HeptaTri OctaTetra NonaPenta Deca
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!)
Steps 1 & 4 ONLY
d,f-blockPb,Sn
Columns 1, 2, 13Ag+, Zn2+
(Except: NH4+)
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Name Formula?
No Prefixes? Prefixes?
1. Determine the ions present and the charge on each (Roman Numeral = cation charge, otherwise use PT)
2. Balance formula (criss-cross)
3. Reduce subscripts (if needed)
1. FORGET CHARGES!!!
2. Use prefixes to determine subscripts
3. Do NOT reduce subscripts!
Ionic Covalent
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Binary Hydrogen Compoundsof Nonmetals When Dissolved in Water
(These compounds are commonly called acids.)
The prefix hydro- is used to represent hydrogen, followed by the nameof the nonmetal with its ending replaced by the suffix –ic and the wordacid added.
Examples:
*HCl
HBr
*The name of this compound would be hydrogen chloride if it was NOT dissolved in water.
Hydrochloric acid
Hydrobromic acid
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Naming Simple Chemical Compounds
Ionic (metal and nonmetal) Covalent (2 nonmetals)
Metal
Formsonly onepositive
ion
Formsmore than
one positiveion
Nonmetal
Use the name of element
Use elementname followed
by a Romannumeral to
show the charge
Firstnonmetal
Secondnonmetal
Beforeelement name
use a prefixto matchsubscript
Use a prefixbefore
element name and end with ide
SingleNegative
Ion
Polyatomic Ion
Use the nameof the
element, butend with ide
Use thename of
polyatomicion (ate or
Ite)
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Naming Ternary Compounds from Oxyacids
The following table lists the most common families of oxy acids.
one moreoxygen atom
most“common”
one lessoxygen
two lessoxygen
HClO4
perchloric acid
HClO3
chloric acid
HClO2
chlorous acid
HClOhypochlorous acid
H2SO4
sulfuric acid
H2SO3
sulfurous acid
H3PO4
phosphoric acid
H3PO3
phosphorous acid
H3PO2
hypophosphorous acid
HNO3
nitric acid
HNO2
nitrous acid
(HNO)2
hyponitrous acid
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An acid with aname ending in
A salt with aname ending in
-ic
-ous
-ate
-iteforms
forms
Hill, Petrucci, General Chemistry An Integrated Approach1999, page 60
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Oxyacids Oxysalts If you replace hydrogen with a metal, you have formed an oxysalt.A salt is a compound consisting of a metal and a non-metal. If thesalt consists of a metal, a nonmetal, and oxygen it is called anoxysalt. NaClO4, sodium perchlorate, is an oxysalt.
HClO4
perchloric acid
HClO3
chloric acid
HClO2
chlorous acid
HClOhypochlorous acid
NaClO4
sodium perchlorate
NaClO3
sodium chlorate
NaClO2
sodium chlorite
NaClOsodium hypochlorite
OXYACID OXYSALT
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ACID SALT
per stem ic changes to per stem ate
stem ic changes to stem ate
stem ous changes to stem ite
hyper stem ous changes to hypo stem ite
HClO3 + Na1+ NaClO3 + H1+
acid cation salt
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Suffixes have meaning“-ide” binary compound
sodium chloride (NaCl)
“-ite” or “-ate” polyatomic compoundsulfite (SO3
2-)
sulfate (SO42-) “-ate” means one more
oxygen than “-ite”
“-ol” alcoholmethyl alcohol (methanol)
“-ose” sugarsucrose
“-ase” enzymesucrase
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Oxidation States in Formulas and Names
dinitrogen monoxide N2O nitrogen (I) oxide
dinitrogen trioxide N2O3 nitrogen (III) oxide
dinitrogen pentoxide N2O5 nitrogen (V) oxide
sulfur dioxide SO2 sulfur (IV) oxide
sulfur trioxide SO3 sulfur (VI) oxide
Traditional System Stock System
+1 -2
+3 -2
+5 -2
+4 -2
+6 -2
(Two non-metals)
stock system is NOT preferred for two non-metals
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% Mg = x 10024 g95 g
Percentage Composition
Mg
magnesium
24.305
12
Cl
chlorine
35.453
17
Mg2+ Cl1-
MgCl2
1 Mg @ 24.305 amu = 24.305 amu2 Cl @ 35.453 amu = 70.906 amu 95.211 amu
25.52% Mg
74.48% Cl
(by mass...not atoms)
It is not 33% Mg and 66% Cl
% = x 100part
whole
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Empirical and Molecular Formulas
A pure compound always consists of the same elements combined in the same proportions by weight.
Therefore, we can express molecular composition as PERCENT BY WEIGHTPERCENT BY WEIGHT.
Ethanol, C2H6O 52.13% C 13.15% H 34.72% O
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Empirical FormulaQuantitative analysis shows that a compound contains 32.38% sodium, 22.65% sulfur, and 44.99% oxygen.
Find the empirical formula of this compound.
= 1.408 mol Na
= 0.708 mol S
= 2.812 mol O
/ 0.708 mol
/ 0.708 mol
/ 0.708 mol
= 2 Na
= 1 S
= 4 O
Na2SO4
32.38% Na
22.65% S
44.99% O
32.38 g Na
22.65 g S
44.99 g O
Na g 23
Na mol 1
S g 32
S mol 1
O g 16
O mol 1
sodium sulfate
Step 1) % g Step 2) g molStep 3) mol mol
Na2SO4
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Empirical FormulaA sample weighing 250.0 g is analyzed and found to contain the following:
27.38% sodium 1.19% hydrogen14.29% carbon57.14% oxygen
Determine the empirical formula of this compound.
Step 1) convert % gram
Step 2) gram moles
Step 3) mol / mol
Assume sample is 100 g.
27.38 g Na 1.19 g H14.29 g C57.14 g O
Na mol 1.1904 Na g 23Na mol 1Na g 27.38 Na molx
H mol 1.19 H g 1H mol 1H g 1.19 H molx
C mol 1.1908 C g 12C mol 1C g 14.29 C molx
O mol 3.5712 O g 16O mol 1O g 57.14 O molx
/ 1.19 mol = 1 Na
/ 1.19 mol = 1 H
/ 1.19 mol = 1 C
/ 1.19 mol = 3 O
NaHCO3
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Empirical & Molecular FormulaA 175 g hydrocarbon sample is analyzed and found to contain ~83% carbon.The molar mass of the sample is determined to be 58 g/mol. Determine the empirical and molecular formula for this sample.
Determine the empirical formula of this compound.
Step 1) convert % gram
Step 2) gram moles
Step 3) mol / mol
Assume sample is 100 g.
C mol 6.917 C g 12C mol 1C g 83 C molx
H mol 17 H g 1H mol 1H g 17 H molx
/ 6.917 mol = 1 C
/ 6.917 mol = 2.5 H (2.4577 H)
CH2.5
Then, 83 g carbon and 17 g hydrogen.
C2H5
MMmolecular = 58 g/mol
58/29 = 2
Therefore 2(C2H5) = C4H10
MMempirical = 29 g/mol
2 C @ 12 g = 24 g5 H @ 1 g = 5 g 29 g
butane
(~17% hydrogen)(contains only hydrogen + carbon)
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1 mol S
1 mol Zn
Common Mistakes when Calculating Empirical Formula
Given: Compound consists of 36.3 g Zn and 17.8 g S.
Find: empirical formula
36.3 g Zn
65.4 g Zn
= 2 Zn
17.8 g S
17.8
17.8= 1 S
Zn2S
36.3 g Zn
17.8 g S
32.1 g S
= 0.555 mol Zn
= 0.555 mol S
Chemical formulaindicates MOLE ratio,
not GRAM ratio
0.555 mol
0.555 mol
1
1
Zn
SZnS
zinc sulfide
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Empirical Formula of a Hydrocarbon
CxHy
g H2O
g CO2
mol H2O
mol CO2
mol Cmol H
burnin O2
1 mol CO2
44.01 gx
1 mol H2O 18.02 g
x 2 mol H 1 mol H2O
x
2 mol C 1 mol CO2
x
Empiricalformula
Kotz & Treichel, Chemistry & Chemical Reactivity, 3rd Edition , 1996, page 224
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Find the molar mass and percentage composition of zinc acetate
acetate = CH3COO1-
Zn2+ CH3COO1-
Zn(CH3COO)2
1 Zn @ 65.4 g/mol = 65.4 g
4 C @ 12 g/mol = 48 g
6 H @ 1 g/mol = 6 g
4 O @ 16 g/mol = 64 g
Zn(CH3COO)2183.4 g
/ 183.4 g x 100% = 35.6 % Zn
/ 183.4 g x 100% = 26.2 % C
/ 183.4 g x 100% = 3.3 % H
/ 183.4 g x 100% = 34.9 % O
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1 mol Cl
35.5 g Cl
1 mol Y
88.9 g Y
A compound is found to be 45.5% Y and 54.5% Cl.
Its molar mass (molecular mass) is 590 g.
a) Find its empirical formula
b) Find its molecular formula
Assume a 100 g sample sizeAssume a 100 g sample size
45.5 g Y
54.5 g Cl
= 0.5118 mol Y
= 1.535 mol Cl
/ 0.5118 mol
/ 0.5118 mol
= 1 Y
= 3 Cl
YCl3
1 Y @ 88.9 g/mol = 88.9g
3 Cl @ 35.5 g/mol = 106.5 g
YCl3 195.4 g590 / 195.4 = 3
3 (YCl3) Y3Cl9
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Molar Mass vs. Atomic Mass
6.02x1023
H2 = _______H2 = _____
H2O = ________H2O = _____
MgSO4 = ________MgSO4 = _____
(NH4)3PO4 = _____ (NH4)3PO4 = ________
Percentage Composition
Empirical vs. Molecular Formula
% g g mol mol mol
Empirical Formula
2 amu
18 amu
120 amu
149 amu
2 g
18 g
120 g
149 g
% = x 100 % partwhole
(lowest ratio)
(by mass)
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Subscripts, Superscripts and Coefficients
Al3(SO4 )2coefficient
subscripts
superscripts
ALUMINUM SULFATE
SO43- Al2+
5
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Subscripts, Superscripts and Coefficients
MgSO4 MAGNESIUM SULFATE
SO42- Mg2+
3
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Subscripts, Superscripts and Coefficients
subscript
MAGNESIUM NITRATE
NO31- Mg2+
42
MgNO3 Mg(NO3)2
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Interpretation of a Chemical Formula
Sulfuric Acid
H2SO4
Two atomsof hydrogen
One atom of sulfur
Four atoms of oxygen
S
O
O
O
O H
H
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Chemical Formulas
C8H18 Subscript indicates that there are 8 carbon atoms in a molecule of octane.
Subscript indicates thatthere are 18 hydrogen atoms
in a molecule of octane.
Davis, Metcalfe, Williams, Castka, Modern Chemistry, 1999, page 203
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Stock System of Nomenclature
CuCl2 Name of Roman cation numeral
indicating charge
Name of anion+
copper (II) chloride
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Chemical Formulas
Al2(SO4)3Subscript 2
refers to2 aluminum
atoms.
Subscript 4refers to4 oxygenatoms in
sulfate ion.
Subscript 3 refers toeverything inside parentheses.Here there are 3 sulfate ions, with a total of 3 sulfur atoms
and 12 oxygen atoms.
Davis, Metcalfe, Williams, Castka, Modern Chemistry, 1999, page 204
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Naming Binary Ionic Compounds
Al2O3
Name of cation Name of anion
aluminum oxide
Davis, Metcalfe, Williams, Castka, Modern Chemistry, 1999, page 207
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The OLD System of Nomenclature
CuCl2Name of Name of anion cation
Cupric chloride
-ic higheroxidation #
-ous loweroxidation #
+
Davis, Metcalfe, Williams, Castka, Modern Chemistry, 1999, page 208
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Centrum Multi-VitaminIngredients: ascorbic acid, beta carotene, biotin, calcium pantothenate, calciumphosphate, carnauba wax, chromium chloride, crospovidone, cupric sulfate,cyanocobalamin, dl-alpha tocopheryl acetate, FD & C blue no. 2 aluminum lake,hydroxypropyl cellulose, ferrous fumarate, hydroxypropyl methylcellulose, lactose, Magnesium oxide, magnesium stearate, manganese sulfate, microcrystalline cellu-lose,niacinamide, nickel sulfate, phytonandione, polyethylene glycol, potassium chloride, potassium citrate, potassium iodide, povidone, pyridoxine hydrochloride, riboflavin, silica gel, sodium borate, sodium metavanadate, sodium molybdate,sodium selenate, stannous chloride, stearic acid, thiamin mononitrate, titaniumdioxide, triacetin, vitamin A acetate, vitamin D3, zinc oxide. PC7563-46-00
Warning: Accidental overdose of iron-containing products is a leading cause of fatal poisoning in children under 6. Keep this product out of reach of children.In case of accidental overdose, call a doctor or poison control immediately.
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Chromium (III) Chloride
Step 1: Chromium (III) Chloride
Step 2: Cr3+ Cl1-
Step 3: Cr Cl1 3
Step 4: CrCl3
RECALL: Chromium forms oxides in which metal exhibits oxidationstates of +3 and +2. STOCK system indicates oxidation state of compound. Assume Cr3+ (chromium (III) chloride).
Return to Centrum Bottle
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Cupric Sulfate
Step 1: Cupric Sulfate
Step 2: Cu2+ SO42-
Step 3: Cu (SO4)2 2
Step 4: Cu2(SO4)2
Step 5: CuSO4
RECALL: “ic” higher oxidation & “ous” lower oxidation Cu2+ (higher) Cu1+ (lower)
Return to Centrum Bottle
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Manganese (III) Sulfate
Step 1: Manganese (III) Sulfate
Step 2: Mn3+ SO42-
Step 3: Mn (SO4)2 3
Step 4: Mn2(SO4)3
RECALL: Manganese forms oxides in which metal exhibits oxidationstates of +2, +3, +4, and +7. STOCK system indicates oxidation state of compound. Assume Mn3+ (manganese (III) sulfate).
Return to Centrum Bottle
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Stannous Chloride
Step 1: Stannous (tin) Chloride
Step 2: Sn2+ Cl1-
Step 3: Sn Cl1 2
Step 4: SnCl2
RECALL: “ic” higher oxidation & “ous” lower oxidation Sn4+ (higher) Sn2+ (lower)
Return to Centrum Bottle
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Stannic Chloride
Step 1: Stannic (tin) Chloride
Step 2: Sn4+ Cl1-
Step 3: Sn Cl1 4
Step 4: SnCl4
RECALL: “ic” higher oxidation & “ous” lower oxidation Sn4+ (higher) Sn2+ (lower)
Return to Centrum Bottle
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Chromium Chloride
Step 1: Chromium (II) Chloride
Step 2: Cr2+ Cl1-
Step 3: Cr Cl1 2
Step 4: Cr1Cl2
Step 5: CrCl2
RECALL: Chromium has multiple oxidation states. Name with STOCK system.
Assume Chromiun (II).
Return to Centrum Bottle
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Calcium Phosphate
Step 1: Calcium Phosphate
Step 2: Ca2+ PO43-
Step 3: Ca (PO4)3 2
Step 4: Ca3(PO4)2
Return to Centrum Bottle
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Zinc Oxide
Step 1: Zinc Oxide
Step 2: Zn2+ O2-
Step 3: Zn O2 2
Step 4: Zn2O2
Step 5: ZnO
Return to Centrum Bottle
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Common Polyatomic Ions
Ion Name Ion Name
NH4+ ammonium
nitrite
nitrate
phosphate
hydrogen phosphate
dihydrogen phosphate
carbonate
hydrogen carbonate(bicarbonate is a widelyused common name)
sulfite
sulfate
hydrogen sulfate(bisulfate is a widelyused common name)
hydroxide
cyanide
hypochlorite
chlorite
chlorate
perchlorate
acetate
permanganate
dichromate
chromate
peroxide
NO2-
NO3-
SO32-
HSO4-
OH-
CN-
PO43-
CO32-
SO42-
MnO4-
O22-
Cr2O72-
HPO42-
H2PO4-
ClO2-
ClO3-
ClO-
HCO3-
ClO4-
C2H3O2-
CrO42-
Names of Common Polyatomic Ions
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1
2
3
4
5
6
1
2
3
4
5
6
Electronegativities
7
Be
1.5
Al
1.5
Si
1.8
Ti
1.5
V
1.6
Cr
1.6
Mn
1.5
Fe
1.8
Co
1.8
Ni
1.8
Cu
1.9
Zn
1.7
Ga
1.6
Ge
1.8
Nb
1.6
Mo
1.8
Tc
1.9
Ag
1.9
Cd
1.7
In
1.7
Sn
1.8
Sb
1.9
Ta
1.5
W
1.7
Re
1.9
Hg
1.9
Tl
1.8
Pb
1.8
Bi
1.9
1.5 - 1.9
N
3.0
O
3.5
F
4.0
Cl
3.0
3.0 - 4.0
C
2.5
S
2.5
Br
2.8
I
2.5
2.5 - 2.9
Na
0.9
K
0.8
Rb
0.8
Cs
0.7
Ba
0.9
Fr
0.7
Ra
0.9
Below 1.0
H
2.1
B
2.0
P
2.1
As
2.0
Se
2.4
Ru
2.2
Rh
2.2
Pd
2.2
Te
2.1
Os
2.2
Ir
2.2
Pt
2.2
Au
2.4
Po
2.0
At
2.2
2.0 - 2.4
Per
iod
Actinides: 1.3 - 1.5
Li
1.0
Ca
1.0
Sc
1.3
Sr
1.0
Y
1.2
Zr
1.4
Hf
1.3
Mg
1.2
La
1.1
Ac
1.1
1.0 - 1.4
Lanthanides: 1.1 - 1.3
1A
2A
3B 4B 5B 6B 7B 1B 2B
3A 4A 5A 6A 7A
8A
Hill, Petrucci, General Chemistry An Integrated Approach 2nd Edition, page 373
8B
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Metal (fixed) + Non-metal
binary -ide NaCl sodium chloride
Metal (variable) + Non-metal
STOCK system (Roman Numeral)
CrCl2 chromium (II) chloride
OLD system [-ic (higher) & -ous (lower)]
CuCl2 cupric chloride
Sn stannumPb plumbumCu cuprumAu aurumFe ferrum
Polyatomic Ions [-ate (one more O) & -ite (one less O)]
LiNO3 lithium nitrate
LiNO2 lithium nitrite
Li3N lithium nitride
TWO Elements
Three or more Elements
ReviewReview
Cu1+ or Cu2+
Group 1, Group 2, Ag, Zn, Al
Transition Elements
Cr2+ Cl1-
Ternary Compounds
(binary compound)
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Polyatomic Ions [-ate (one more O) & -ite (one less O)]
per____ate NORMAL _____ite hypo_____ite
chloratenitratecarbonatesulfatephosphate
ammonium, cyanide, hydroxide
Nonmetal & Nonmetal (Greek prefixes)……DO NOT REDUCE!
Mono Di Tri Tetra Penta Hexa Hepta Octa Nona Deca
1 2 3 4 5 6 7 8 9 10
ClO31-
NO31-
CO32-
SO42-
PO43-
NH41+ CN1- OH1-
chloritenitritecarbonitesulfitephosphite
ClO21-
NO21-
CO22-
SO32-
PO33-
perchloratepernitratepercarbonatepersulfateperphosphate
ClO41-
NO41-
CO42-
SO52-
PO53-
2 less oxygen1 less oxygen1 more oxygen
ClO1-
NO1-
CO2-
SO22-
PO23-
hypochloritehyponitritehypocarbonitehyposulfitehypophosphite
Memorize
How many atoms are in a formula unit of ammonium hypophosphite?NH4
1+ PO23-
(NH4)3PO2
318
_____ate
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Molecular Models Activity
ammonia
hydrogen monochloride
trichloromethane
urea
propane
butane
nitrogen triiodide (video)
carbon tetrachloride
methane
water
ethane
ethyne
dihydrogen monosulfide
carbon dioxide
supplies
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Bonding and Shape of Molecules
Number of Bonds
Number of Unshared Pairs Shape Examples
2
3
4
3
2
0
0
0
1
2
Linear
Trigonal planar
Tetrahedral
Pyramidal
Bent
BeCl2
BF3
CH4, SiCl4
NH3, PCl3
H2O, H2S, SCl2
-Be-
B
C
N
:
O
:
:
CovalentStructure
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Lewis Structures
1) Count up total number of valence electrons
2) Connect all atoms with single bonds
- “multiple” atoms usually on outside
- “single” atoms usually in center;
C always in center,
H always on outside.
3) Complete octets on exterior atoms (not H, though)
4) Check
- valence electrons match with Step 1
- all atoms (except H) have an octet; if not, try multiple bonds
- any extra electrons? Put on central atom
- no unpaired electrons (free radicals)
Gilbert Lewis
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Carbon tetrachloride
C ClClCl
Cl
CCl4
C109.5o
Cl
ClClCl
Carbon tetrachloride – “carbon tet” had been used as dry cleaning solventbecause of its extreme non-polarity.
Tetrahedral geometry
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Methane
CHH
HH
C109.5o
H
HHH
Methane –The first member of the paraffin (alkane) hydrocarbons series. a.k.a. (marsh gas, CH4).
Tetrahedral geometry
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Water
....
H HOBent
geometry
SO2
(-)
(+)
Polar molecule
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Ethane
CH
CHH
HHH
space-filling molecule
ball-and-stickLewis dot notation
C2H6
molecular formula
C = 1s22s22p2
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Ethene
CH
CHH
HHH
space-filling molecule
ball-and-stickLewis dot notation
C2H4
molecular formula
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Ethyne
CCH H CCH H
No octet
Stable octet
6 electrons = triple bond
CCH H
C2H2
CCH H
each C “feels” 6 electrons
each C “feels” 7 carbons
Ethyne – a.k.a. “acetylene”
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Dihydrogen monosulfide
....
H HS
Bent
SO2
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Carbon dioxide
O OC
Lineargeometry
C OOCO2
C OO
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Ammonia
NH HH
N107o HH
H
..
NH3
..
HH
H
N
TrigonalPyramidalgeometry
NH HH
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H
Amino Acids – Functional Groups
Amine Carboxylic AcidBase Pair
NH21- R- COOH
NH3NH21- NH4
1+
amine ammonia ammonium ion
NH
HH
:
NH
HH
H : 1+
NH
H
:
1-
:
H+ lose H+ H+
+
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Hydrogen monochloride
H ClHCl
H Cl
(-)(+)
H Cl
Polar molecule
HCl(g) + H2O(l) HCl(aq)
hydrogenchloride
water hydrochloric acid
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Trichloromethane
C ClClCl
H
CHCl3
C109.5o
H
ClClCl
C ClClCl
H
(-)
(+)
Polar molecule
Tetrahedral geometry
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Urea
CON HH
NH H
CON HH
NH H
CO(NH2)2
NOT “di-urea”
Urea – The first organic compound to be synthesized (Wohler, 1828).
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Propane
CH
CHH
CH
HHHH
C C C
HH
H
HH H H
H
C3H8
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Butane
CH
CHH
CH
C HH
HHHHH - C - C - C - C - H
H H H H
H H H H
C4H10 C C C
HH
H
HH H H
HC
H
H
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Nitrogen triiodide
NI II N
107o III
..
NI3
TrigonalPyramidalgeometry
Video clip:
(slow motion)
detonation of NI3
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Supplies
15 black (carbon) 8 green (chlorine and iodine) 1 yellow (sulfur) 4 blue (oxygen) 4 red (nitrogen) 42 hydrogen (hydrogen) 67 bonds (bonds)
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C Cl I S O N H
C ClClCl
ClCH
H HH
C OO
SH HC C HH
C ClClCl
H
H Cl
CCl4 CH4
CO2
C2H2
HClCHCl3
SH2
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CH
CHH
CH
C HH
HHHHCH
CHH
CH
HHHH
NH HH
NI II
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Decomposition of Nitrogen Triiodide
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Decomposition of Nitrogen Triiodide
2 NI3(s) N2(g) + 3 I2(g)
NI3 I2
N2
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C109.5o
H
HHH
N107o HH
H
..
O104.5o H
H
..
..
CH4, methane NH3, ammonia H2O, water
..
O
O
O
lone pairelectrons
OOO
O3, ozone
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......
The VSEPR Model
O OC
Linear
The Shapes of Some Simple ABn Molecules
O OS
BentO O
S
O
Trigonalplanar
FF
F
N
Trigonalpyramidal
T-shaped Squareplanar
F FCl
F
F F
Xe
F FF
F
FP
F
F
Trigonalbipyramidal
Octahedral
FF
F
S
F
F
F
AB6
SO2
Brown, LeMay, Bursten, Chemistry The Central Science, 2000, page 305
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Resources - Nomenclature
ObjectivesObjectives
Worksheet - binary cmpds: single charge cationWorksheet - binary cmpds: single charge cation
Worksheet - ions in chemical formulasWorksheet - ions in chemical formulas
Worksheet - ionic cmpds: polyatomic ions w multiple-charge cationWorksheet - ionic cmpds: polyatomic ions w multiple-charge cation
Worksheet - ionic formulas (binary, polyatomic, transition)Worksheet - ionic formulas (binary, polyatomic, transition)
Worksheet - traditional system of nomenclatureWorksheet - traditional system of nomenclature
Worksheet - covalent binary cmpds: non-metal - non-metal Worksheet - covalent binary cmpds: non-metal - non-metal
Worksheet - ionic cmpds: polyatomic ionsWorksheet - ionic cmpds: polyatomic ions
Outline (general)(general)
Worksheet - empirical and molecularWorksheet - empirical and molecular
Worksheet - vocab (bonding)Worksheet - vocab (bonding)
Activity - bonding piecesActivity - bonding pieces
Activity - molecular modelsActivity - molecular models
Activity - mole patternActivity - mole pattern
Worksheet - binary compoundsWorksheet - binary compounds
Worksheet - ions in chemical compoundsWorksheet - ions in chemical compounds
Textbook - questionsTextbook - questions
Worksheet - ionic binary cmpds: multiple charge cationWorksheet - ionic binary cmpds: multiple charge cation
Worksheet - oxidation numbers and ionic cmpdsWorksheet - oxidation numbers and ionic cmpds
Worksheet - names and formulas of cmpdsWorksheet - names and formulas of cmpds
Worksheet - errors in chemical formulas and nomenclatureWorksheet - errors in chemical formulas and nomenclature
General Chemistry PP