Transcript Nomenclature

Vocabulary
ION
1 atom
2 or more atoms
monatomic
Ion (ex. Cl-)
polyatomic
Ion (ex. SO42-)
+
Na
NO3
Courtesy Christy Johannesson www.nisd.net/communicationsarts/pages/chem
-
Single-charge cations
Multiple-charge cations
Elemental anions
1+
1
H
2+
3+
Li
Be
B
3
4
1
2
3
Na Mg
11
4
K
19
5
7
Ca Sc
C
N
O
F
Ne
5
6
7
8
9
10
Al
Si
P
S
Cl
Ar
13
14
15
16
17
18
Ti
V
Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br
Kr
23
24
35
36
I
Xe
53
54
Rb Sr
Y
Zr Nb Mo Tc Ru Rh Pd Ag Cd
In
39
40
41
42
49
Hf
Ta
W
72
73
74
55
56
Fr
Ra
87
88
*
W
2
1-
22
Cs Ba
1
2-
21
38
He
3-
20
37
6
1+ 2+
12
H
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
Cations and Anions
Common Simple Cations and Anions
Cation
H 1+
Li 1+
Na 1+
K 1+
Cs 1+
Be 2+
Mg 2+
Al 3+
Ag 1+
Name
hydrogen
lithium
sodium
potassium
cesium
beryllium
magnesium
aluminum
silver
Anion
H 1F 1Cl 1Br 1I 1O 2S 2-
Name*
hydride
fluoride
chloride
bromide
iodide
oxide
sulfide
*The root is given in color.
Zumdahl, Zumdahl, DeCoste, World of Chemistry 2002, page 86
Type II Cations
Common Type II Cations
Ion
Stock System
Fe 3+
Fe 2+
Cu 2+
Cu 1+
Co 3+
Co 2+
Sn 4+
Sn 2+
Pb 4+
Pb 2+
Hg 2+
Hg2 2+
iron (III)
iron (II)
copper (II)
copper (I)
cobalt (III)
cobalt (II)
tin (IV)
tin (II)
lead (IV)
lead (II)
mercury (II)
mercury (I)
Traditional System
ferric
ferrous
cupric
cuprous
cobaltic
cobaltous
stannic
stannous
plumbic
plumbous
mercuric
mercurous
*Mercury (I) ions are always bound together in pairs to form Hg2 2+
Zumdahl, Zumdahl, DeCoste, World of Chemistry 2002, page 90
Common Polyatomic Ions
Names of Common Polyatomic Ions
Ion
Name
Ion
Name
NH4+
ammonium
CO32-
carbonate
NO2-
nitrite
HCO3-
NO3-
nitrate
SO32-
sulfite
hydrogen carbonate
(bicarbonate is a widely
used common name)
SO42-
sulfate
ClO-
hypochlorite
HSO4-
hydrogen sulfate
(bisulfate is a widely
used common name)
ClO2-
chlorite
ClO3-
chlorate
ClO4-
perchlorate
OH-
hydroxide
C2H3O2-
acetate
CN-
cyanide
MnO4-
permanganate
PO43-
phosphate
Cr2O72-
dichromate
HPO42-
hydrogen phosphate
CrO42-
chromate
H2PO4-
dihydrogen phosphate
O22-
peroxide
COMPOUND
IONIC
COVALENT
metal to nonmetal or
metal to polyatomic
nonmetal to nonmetal
metalloid to nonmetal
formula
unit
molecular
formula
NaCl
CO2
Courtesy Christy Johannesson www.nisd.net/communicationsarts/pages/chem
IONIC
COMPOUND
ions of 2
elements
(metal +
non metal)
more than 2
elements (metal
+polyatomic)
Binary (ionic)
compound
NaCl
Ternary (ionic)
compound
NaNO3
Courtesy Christy Johannesson www.nisd.net/communicationsarts/pages/chem
Binary Ionic Compounds
Binary compounds contain a metal ion (group 1, group 2, Al, Zn, Ag, etc.),
and a non-metal.
To name these compounds, give the name of metal followed by the
name of the non-metal, with the ending replaced by the suffix –ide.
Examples:
NaCl
sodium chloride
(Na1+ Cl1-)
CaS
calcium sulfide
(Ca2+
AlI3
aluminum iodide
(Al3+ 3 I1-)
S2-)
Writing Binary Ionic Compounds
chemical formula (metal/non-metal):
has neutral charge
shows types of atoms/ions
subscript shows how many of each atom/ion
To write an ionic compound’s formula, we need:
1. the two types of ions
2. the charge on each ion
Na1+
and
F1–
NaF
Ba2+
and
O2–
BaO
Na1+
and
O2–
Na2O
Ba2+
and
F1–
BaF2
Naming Binary Ionic Compounds
Formula
Name
BaO
barium oxide
____________________
NaBr
2 ________________
sodium bromide
1
3
MgI2
magnesium iodide
____________________
4
KCl
potassium chloride
____________________
SrF2
5 ________________
strontium fluoride
CsF
6 ________________
cesium fluoride
Naming Binary Ionic Compounds
Formula
Name
1
Hg2O
mercury (I) oxide
____________________
2
HgO
mercury (II) oxide
____________________
CuF2
3 ________________
copper (II) fluoride
Cu2S
4 ________________
copper (I) sulfide
5
Cr2O3
PbO2
6 ________________
chromium (III) oxide
____________________
lead (IV) oxide
Ternary Ionic Compounds
Ternary compounds contain a metal ion (group 1, group 2, Al, Zn,
Ag, etc.), and a polyatomic ion.
To name these compounds, give the name of metal followed by the
name of the polyatomic ion.
Examples:
NaNO3
sodium nitrate
K2SO4
potassium sulfate
Ca3(PO4)2
calcium phosphate
Fe(OH)3
iron (III) hydroxide
Na2CO3
sodium carbonate
Naming Ternary Ionic Compounds
Ca3(PO4) 2
1. ________________
calcium phosphate
(NH4)2CO3
2. ________________
ammonium carbonate
Al2(SO4)3
3. ________________
aluminum sulfate
4.
Na2SO4
sodium sulfate
____________________
5.
LiCN
lithium cyanide
____________________
6.
Ba2CO3
barium carbonate
____________________
Cu(OH)2
7. ________________
copper (II) hydroxide
Writing Ternary Ionic Compounds
Parentheses are required only when you need more
than one “bunch” of a particular polyatomic ion.
Ba2+
and
SO42–
BaSO4
barium sulfate
Mg2+
and
NO31–
Mg(NO3)2
magnesium nitrate
NH41+
and
PO43–
(NH4)3PO3
ammonium phosphate
Sn4+
and
SO42–
Sn(SO4)2
tin (IV) sulfate
Fe3+
and
CO32–
Fe2(CO3)3
iron (III) carbonate
NH41+
and
OH1–
NH4OH
ammonium hydroxide
Criss-Cross Rule
Example: Aluminum Chloride
Step 1:
Aluminum
Chloride
Step 2:
Al3+
Cl1-
Step 3:
Al 1
Cl 3
Step 4:
AlCl 3
Criss-Cross Rule
Example: Aluminum Oxide
Step 1:
Aluminum
Oxide
Step 2:
Al3+
O2-
Step 3:
Al 2
O3
Step 4:
Al2O3
Criss-Cross Rule
Example: Magnesium Oxide
Step 1:
Magnesium
Step 2:
Mg2+
O2-
Step 3:
Mg 2
O2
Step 4:
Step 5:
Mg2O2
MgO
Oxide
Writing Formulas/Names of Covalent
Compounds
 Covalent Compounds
contain two types of nonmetals, or metalloid and nonmetal
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
2 – di
3 – tri
4 – tetra
5 – penta
6 – hexa
7 – hepta
8 – octa
9 – nona
10 – deca
Binary Covalent Compounds
N2O
N2O3
N2O5
dinitrogen monoxide
dinitrogen trioxide
dinitrogen pentoxide
ICl
ICl3
iodine monochloride
iodine trichloride
SO2
SO3
sulfur dioxide
sulfur trioxide
Writing Formulas/Names of Covalent Compounds
EXAMPLES:
carbon dioxide
CO
dinitrogen trioxide
N2O5
carbon tetrachloride
NI3
CO2
carbon monoxide
N2O3
dinitrogen pentoxide
CCl4
nitrogen triiodide
Naming Binary Covalent Compounds
As2S3
1. ________________
diarsenic trisulfide
SO2
2. ________________
sulfur dioxide
P2O5
diphosphorus pentoxide
____________________
CO2
4. ________________
carbon dioxide
3.
5.
N2O5
dinitrogen pentoxide
____________________
6.
H2O
dihydrogen monoxide
____________________
Exceptions!
Two exceptions to the simple –ide ending are the diatomic oxide ions,
O22- and O21-.
O22- is called peroxide
Note the differences.
O21- is called superoxide.
barium oxide
barium peroxide
BaO
__________
BaO2
__________
sodium oxide
sodium peroxide
Na2O
__________
Na2O2
__________
potassium oxide
potassium superoxide
K2O
__________
KO2
__________
Ba2+
Na1+
Do Not Reduce to lowest terms!
K1+
Binary Hydrogen Compounds
of Nonmetals When Dissolved in Water
(These compounds are commonly called acids.)
The prefix hydro- is used to represent hydrogen, followed by the name
of the nonmetal with its ending replaced by the suffix –ic and the word
Acid added.
Examples:
*HCl
Hydrochloric acid
HBr
Hydrobromic acid
*The name of this compound would be hydrogen chloride if it was NOT dissolved in water.
Naming Ternary Compounds
from Oxyacids
The following table lists the most common families of oxy acids.
one more
oxygen atom
HClO4
perchloric acid
most
“common”
HClO3
chloric acid
H2SO4
sulfuric acid
H3PO4
phosphoric acid
HNO3
nitric acid
one less
oxygen
HClO2
chlorous acid
H2SO3
sulfurous acid
H3PO3
phosphorous acid
HNO2
nitrous acid
two less
oxygen
HClO
hypochlorous acid
H3PO2
hypophosphorous acid
(HNO)2
hyponitrous acid
An acid with a
name ending in
A salt with a
name ending in
-ous
forms
-ite
-ic
forms
-ate
Hill, Petrucci, General Chemistry An Integrated Approach 1999, page 60
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 the
salt consists of a metal, a nonmetal, and oxygen it is called an
oxysalt. NaClO4, sodium perchlorate, is an oxysalt.
OXYACID
OXYSALT
HClO4
perchloric acid
NaClO4
sodium perchlorate
HClO3
chloric acid
NaClO3
sodium chlorate
HClO2
chlorous acid
NaClO2
sodium chlorite
HClO
hypochlorous acid
NaClO
sodium hypochlorite
Organic Chemistry
Organic Chemistry: The chemistry of carbon
and carbon-based compounds
Organic Chemistry in everyday life:
Smells & tastes: fruits, chocolate, fish, mint
Medications: aspirin, Tylenol, decongestants, sedatives
Addictive substances: caffeine, nicotine, alcohol, narcotics
Hormones/Neurotransmitters: adrenaline, epinephrine
Food: carbohydrates, protein, fat
Genetics: DNA, RNA
Consumer products: plastics, nylon, rayon, polyester
First Ten Hydrocarbons (Alkanes)
Number of
Carbon Atoms
Molecular
Formula
Melting
Point, oC
Boiling
Point, oC
# of
Isomers
Methane
1
CH4
-182.5
-161.5
0
Ethane
2
C2H6
-183.2
-88.6
0
n-Propane
3
C3H8
-187.7
-42.1
0
n-Butane
4
C4H10
-138.3
-0.5
2
n-Pentane
5
C5H12
-129.7
36.1
3
n-Hexane
6
C6H14
-95.3
68.7
5
n-Heptane
7
C7H16
-90.6
98.4
9
n-Octane
8
C8H18
-56.8
125.7
18
n-Nonane
9
C9H20
-53.6
150.8
35
n-Decane
10
C10H22
-29.7
174.0
75
Name
Molecular Weight and Molar Mass
Molecular weight (or Formula mass) is the sum of atomic weights
of all atoms in the molecule.
example: NaCl has a molecular weight of 58.5 amu.
this is composed of a single molecule of NaCl
Molar mass = molecular weight in grams. Units = g/mol
example: NaCl has a molar mass of 58.5 grams
this is composed of a 6.02 x1023 molecules of NaCl
Counting Atoms
• Chemistry is a quantitative science - we need
a "counting unit."
• The MOLE
• 1 mole is the amount of substance that
contains as many particles (particles, atoms,
molecules) as there are in 12.0 g of C-12.
NOTE: Mole equates a gram to an amu
How Big is a Mole?
One mole of marbles would cover the entire Earth
(oceans included) for a depth of two miles.
One mole of $1 bills stacked
one on top of another would
reach from the Sun to Pluto
and back 7.5 million times.
It would take light 9500 years to travel from the bottom
to the top of a stack of 1 mole of $1 bills.
Particles in a Mole
Amedeo
Avogadro
(1776 – 1856)
?
quadrillions
thousands
trillions
billions
millions
1 mole = 602213673600000000000000
or 6.022 x 1023
There is Avogadro's number of particles in a mole of any substance.
Percentage Composition
(by mass...not atoms)
24.305
35.453
Mg
Cl
12
17
magnesium
chlorine
partg
24
% Mg
% = whole x 100
95 g
25.52% Mg
Mg2+
Cl174.48% Cl
MgCl2
It is not 33% Mg and 66% Cl
1 Mg @ 24.305 amu = 24.305 amu
2 Cl @ 35.453 amu = 70.906 amu
95.211 amu
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 WEIGHT. The
simplest formula is called the Empirical
Formula
Ethanol, C2H6O
52.13% C
13.15% H
34.72% O
Empirical Formula
Quantitative analysis shows that a compound contains 32.38% sodium,
22.65% sulfur, and 44.99% oxygen.
sodium sulfate
Find the empirical formula of this compound.
 1 mol Na 
 =
 23 g Na 
1.408 mol Na / 0.708 mol = 2 Na
32.38% Na
32.38 g Na 
22.65% S
22.65 g S
 1 mol S 


32
g
S


= 0.708 mol S / 0.708 mol
=1S
44.99% O
44.99 g O
 1 mol O 


16
g
O


= 2.812 mol O / 0.708 mol
=4O
Step 1) %  g
Step 2) g  mol
Step 3) mol
mol
Na2SO4
Empirical Formula
A sample weighing 250.0 g is analyzed and found to contain the following:
27.38 g
27.38%
1.19%
1.19
g
14.29%
14.29
g
57.14%
57.14
g
Na
sodium
H
hydrogen
C
carbon
O
oxygen
Assume sample is 100 g.
Determine the empirical formula of this compound.
Step 1) convert %  gram
Step 2) gram  moles
  1.1904 mol Na
x mol Na  27.38 g Na1mol Na
/ 1.19 mol = 1 Na
23 g Na 

  1.19 mol H / 1.19 mol = 1 H
x mol H  1.19 g H1mol H

1
g
H


  1.1908 mol C / 1.19 mol = 1 C
x mol C  14.29 g C1mol C

12
g
C



  3.5712 mol O / 1.19 mol = 3 O
x mol O  57.14 g O1mol O

16
g
O


Step 3) mol / mol
NaHCO3
Empirical & Molecular Formula
(contains only hydrogen + carbon)
(~17% hydrogen)
A 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
Assume sample is 100 g.
Then, 83 g carbon and 17 g hydrogen.
Step 2) gram  moles
  6.917 mol C
x mol C  83 g C1mol C

/ 6.917 mol = 1 C
12
g
C


  17 mol H / 6.917 mol = 2.5 H
x mol H  17 g H1mol H

1
g
H


(2.4577 H)
2 C @ 12 g = 24 g
5H@ 1g = 5g
29 g
MMempirical = 29 g/mol
CH2.5
C2H5
MMmolecular = 58 g/mol
Step 3) mol / mol
58/29 = 2
Therefore 2(C2H5) = C4H10
butane
Find the molar mass and percentage composition of zinc acetate
Zn2+ CH3COO1acetate = CH3COO1-
Zn(CH3COO)2
1 Zn @ 65.4 g/mol = 65.4 g / 183.4 g x 100% = 35.6 % Zn
4 C @ 12 g/mol
6 H @ 1 g/mol
= 48 g
= 6g
4 O @ 16 g/mol
= 64 g
Zn(CH3COO)2
183.4 g
/ 183.4 g x 100% = 26.2 % C
/ 183.4 g x 100% = 3.3 % H
/ 183.4 g x 100% = 34.9 % O
A compound is found to be 45.5% Y and 54.5% Cl.
Its molar mass (molecular mass) is 590 g.
Assume a 100 g sample size
a) Find its empirical formula
45.5 g Y
1 mol Y
88.9 g Y
= 0.5118 mol Y / 0.5118 mol = 1 Y
YCl3
54.5 g Cl
1 mol Cl
35.5 g Cl
= 1.535 mol Cl / 0.5118 mol = 3 Cl
1 Y @ 88.9 g/mol = 88.9g
3 Cl @ 35.5 g/mol = 106.5 g
b) Find its molecular formula
590 / 195.4 = 3
3 (YCl3)
YCl3
Y3Cl9
195.4 g
6.02x1023
Molar Mass
Atomic Mass
vs.
2g
H2 = _____
H2 = _______
2 amu
18 g
H2O = _____
H2O = ________
18 amu
120 g
MgSO4 = _____
MgSO4 = ________
120 amu
g
(NH4)3PO4 = 149
_____
(NH4)3PO4 = ________
149 amu
Percentage Composition (by mass)
% =
part
x 100 %
whole
Empirical vs.
(lowest ratio)
Molecular Formula
Empirical Formula



% g
g  mol
mol
mol