A1260284414IyKle

1
Chapter 2 The Components of Matter
2.1 Elements, Compounds, and Mixtures An
Atomic Overview 2.2 The Observations
That Led to an Atomic View of
Matter 2.3 Daltons Atomic Theory 2.4 The
Observations That Led to the Nuclear Atom
Model 2.5 The Atomic Theory Today 2.6
Elements A First Look at the Periodic Table 2.7
Compounds Introduction to Bonding 2.8
Compounds Formulas, Names, and Masses 2.9
Mixtures Classification and Separation
2
Fig. 2.1
3
Definitions for Components of Matter
Pure Substances - Their compositions are fixed!
Elements and
compounds are examples of Pure Substances. Element
- Is the simplest type of substance with unique
physical and chemical
properties. An element consists of only one type
of atom. It cannot be broken
down into any simpler
substances by physical or chemical
means. Molecule - Is a structure that is
consisting of two or more atoms that
are chemically bound together and thus
behaves as an independent
unit. Compound - Is a substance composed of two
or more elements that are
chemically combined. Mixture - Is a group of two
or more elements and/or compounds that
are physically intermingled.
4
Fig. 2.2
5
(p. 43)
6
Separating a Mixture
Fig. 2.3
7
Fig. 2.4
8
Laws of Mass Conservation Definite
Composition
Law of Mass conservation The total mass of
substances does not
change during a chemical reaction. Law of
Definite ( or constant ) composition No matter
what its source, a
particular chemical
compound is composed of the same elements
in the same parts (fractions) by
mass.
9
The Meaning of Mass Fraction and Mass Percent
Fig. 2.5
10
Mass Percent Composition of Na2SO4
Na2SO4 2 atoms of Sodium 1 atom of Sulfur 4
atoms of Oxygen
Elemental masses
Percent of each Element
2 x Na 2 x 22.99 45.98
1 x S 1 x 32.07 32.07
4 x O 4 x 16.00 64.00
142.05
Check
Na S O 100 32.37 22.58 45.05
100.00
11
Mass Percent Composition of Na2SO4
Na2SO4 2 atoms of Sodium 1 atom of Sulfur 4
atoms of Oxygen
Elemental masses
Percent of each Element
2 x Na 2 x 22.99 45.98
Na Mass Na / Total mass x 100 Na (45.98 /
142.05) x 100 32.37 S Mass S / Total mass
x 100 S (32.07 / 142.05) x 100 22.58
O Mass O / Total mass x 100 O (64.00 /
142.05) x 100 45.05
1 x S 1 x 32.07 32.07
4 x O 4 x 16.00 64.00
142.05
Check
Na S O 100 32.37 22.58 45.05
100.00
12
Calculating the Mass of an Element in a Compound
Ammonium Nitrate
How much Nitrogen is in 455 kg of Ammonium
Nitrate?
Ammonium Nitrate NH4NO3
The Formula Mass of Cpd is
4 x H 4 x 1.008 4.032 g 2 x N 2 X 14.01
28.02 g 3 x O 3 x 16.00 48.00 g
Therefore gm Nitrogen/ gm Cpd
80.052 g
13
Calculating the Mass of an Element in a Compound
Ammonium Nitrate
How much Nitrogen is in 455 kg of Ammonium
Nitrate?
Ammonium Nitrate NH4NO3
The Formula Mass of Cpd is
4 x H 4 x 1.008 4.032 g 2 x N 2 X 14.01
28.02 g 3 x O 3 x 16.00 48.00 g
Therefore gm Nitrogen/ gm Cpd
28.02 g Nitrogen
80.052 g
0.35002249 g N / g Cpd
80.052 g Cpd
455 kg x 1000g / kg 455,000 g NH4NO3
455,000 g Cpd x 0.35002249 g N / g Cpd 1.59 x
105 g Nitrogen
28.02 kg
Nitrogen
or
159 kg Nitrogen
455 kg NH4NO3 X
80.052 kg NH4NO4
14
Fig. 2.7
15
Law of Multiple Proportions
If elements A and B react to form two
compounds, the different masses of B that combine
with a fixed mass of A can be expressed as a
ratio of small whole numbers
Example Nitrogen Oxides I II
Nitrogen Oxide I 46.68 Nitrogen and 53.32
Oxygen Nitrogen Oxide II 30.45 Nitrogen and
69.55 Oxygen
in 100 g of each Compound g O 53.32 g 69.55
g
g N 46.68 g 30.45 g
g O /g N 1.142 2.284
2.284 2

1.142 1
16
Daltons Atomic Theory
1. All matter consists of atoms.
2. Atoms of one element cannot be converted into
atoms of another element.
3. Atoms of an element are identical in mass and
other properties and are different from atoms
of any other element.
4. Compounds result from the chemical combination
of a specific ratio of atoms of different
elements.
17
The Combining Volumes of Hydrogen and Oxygen in
the Formation of Water Vapor
Fig. 2.8
18
Fig. 2.9
19
Fig. 2.11
20
Rutherford Experiment

• Alpha particles bombarding the atom.
• Rationale - to study the internal structure of
  the atom, and to know more about the mass
  distribution in the atom!
• Bombarded a thin Gold foil with Alpha particles
  from Radium.

21
Fig. 2.12
22
Ernest Rutherford (1871-1937)

• Won the Nobel Prize in Chemistry in 1908
• It was quite the most incredible event..... It
  was almost as if a gunner were to fire a shell at
  a piece of tissue and the shell bounced right
  back!!!!!

23
Fig. 2.13
24
Properties of the Subatomic Particles
Name Charge
Mass
Location (Symbol) Relative Absolute
Relative(amu) Absolute In Atom
Proton 1 1.60218 x 10-19 C 1.00727
1.67262 x 10-24 g Nucleus (P ) Neutron
0 0 1.00866
1.67593 x 10-24 g Nucleus (n o) Electron
1 - -1.60218 x 10-19 C
9.10939 x 10-28g Outside (e -)
0.00054858
Nucleus
the coulomb (C) is the SI unit of Charge
Table 2.2 (p. 53)
25
Atomic Definitions I Symbols, Isotopes,Numbers
A
X
The Nuclear Symbol of the Atom, or Isotope
Z
X Atomic symbol of the element, or element
symbol
A The Mass number A Z N Z The Atomic
Number, the Number of Protons in the Nucleus N
The Number of Neutrons in the Nucleus
Isotopes atoms of an element with the same
number of protons, but
different numbers of Neutrons in the Nucleus
26
Depicting the Atom
Fig. 2.14
27
Neutral ATOMS

• 51 Cr P (24), e- (24),
• N (27)
• 239 Pu P(94), e- (94),
• N (145)
• 15 N P(7), e-(7), N(8)
• 56 Fe P(26), e-(26),
• N (50)
• 235 U P(92), e-(92),
• N (143)

28
Atomic Definitions II AMU, Dalton, 12C Std.
Atomic mass Unit (AMU) 1/12 the mass of a
carbon - 12 atom
on this scale Hydrogen has a mass of 1.008 AMU.
Dalton (D) The new name for the Atomic Mass
Unit, one
dalton one Atomic Mass Unit
on this scale, 12C has a mass
of 12.00 daltons.
Isotopic Mass The relative mass of an Isotope
relative to the
Isotope 12C the chosen standard.
Atomic Mass Atomic Weight of an element is
the average of the
masses of its naturally occurring isotopes
weighted according to
their abundances.
29
Isotopes of Hydrogen

• 11H 1 Proton 0 Neutrons 99.985
  1.00782503 amu
• 21H (D) 1 Proton 1 Neutron 0.015
  2.01410178 amu
• 31H (T) 1 Proton 2 Neutrons
  -------- ----------
• The average mass of
  Hydrogen is 1.008 amu
• 3H is Radioactive with a half life of 12 years.
• H2O Normal water light water
• mass 18.0 g/mole , BP 100.000000C
• D2O Heavy water
• mass 20.0 g/mole , BP 101.42 0C

30
Element 8 Oxygen, Isotopes

• 168O 8 Protons 8
  Neutrons
• 99.759 15.99491462
  amu
• 178O 8 Protons 9
  Neutrons
• 0.037
  16.9997341 amu
• 188O 8 Protons 10
  Neutrons
• 0.204
  17.999160 amu

31
Formation of a Positively Charged Neon Particle
in a Mass Spectrometer
Fig. 2.A
32
Fig. 2.B part A
33
Calculating the Average Atomic Mass of an
Element
Problem Calculate the average atomic mass of
Magnesium! Magnesium Has three
stable isotopes, 24Mg ( 78.7)
25Mg (10.2) 26Mg (11.1).
24Mg (78.7) 23.98504 amu x 0.787
18.876226 amu 25Mg (10.2) 24.98584
amu x 0.102 2.548556 amu 26Mg (11.1)
25.98636 amu x 0.111 2.884486 amu

24.309268 amu
With Significant Digits 24.3 amu
34
Calculate the Average Atomic Mass of
Zirconium, Element 40
Zirconium has five stable isotopes 90Zr, 91Zr,
92Zr, 94Zr, 96Zr.
Isotope ( abd.) Mass (amu) ()
Fractional Mass 90Zr (51.45)
89.904703 amu X 0.5145 46.2560 amu 91Zr
(11.27) 90.905642 amu X 0.1127
10.2451 amu 92Zr (17.17) 91.905037 amu X
0.1717 15.7801 amu 94Zr (17.33)
93.906314 amu X 0.1733 16.2740 amu 96Zr
(2.78) 95.908274 amu X 0.0278
2.6663 amu
91.2215 amu
With Significant Digits 91.22 amu
35
Problem Calculate the abundance of the two
Bromine isotopes 79Br 78.918336 g/mol
and 81Br 80.91629 g/mol , given that
the average mass of Bromine is 79.904 g/mol.
Plan Let the abundance of 79Br X and of 81Br
Y and X Y 1.0
Solution X(78.918336) Y(80.91629)
79.904 X Y 1.00 therefore X
1.00 - Y (1.00 - Y)(78.918336)
Y(80.91629) 79.904 78.918336 -
78.918336 Y 80.91629 Y 79.904 1.997954 Y
0.985664 or Y 0.4933 X 1.00 -
Y 1.00 - 0.4933 0.5067 X
79Br 0.5067 x 100 50.67 79Br
Y 81Br 0.4933 x 100 49.33 81Br
36
Modern Reassessment of the Atomic Theory
1. All matter is composed of atoms. Although
atoms are composed of smaller particles
(electrons, protons, and neutrons), the atom
is the smallest body that retains the unique
identity of the element. 2. Atoms of one element
cannot be converted into atoms of another
element in a chemical reaction. Elements can only
be converted into other elements in Nuclear
reactions in which protons are changed. 3. All
atoms of an element have the same number of
protons and electrons, which determines the
chemical behavior of the element. Isotopes
of an element differ in the number of neutrons,
and thus in mass number, but a sample of the
element is treated as though its atoms have
an average mass. 4. Compounds are formed by the
chemical combination of two or more elements
in specific ratios, as originally stated by
Dalton.
37
Definitions

• ELEMENT - A substance that cannot be separated
  into simpler substances by chemical means
• COMPOUND - A substance composed of atoms of two
  or more elements chemically united in fixed
  proportions
• PERIODIC TABLE - MENDELEEV TABLE - A tabular
  arrangement of the elements, vertical groups or
  families of elements based upon their chemical
  properties - actually combining ratios with
  oxygen

38
Fig. 2.16
39
Fig. 2.17
40
The Periodic Table of the Elements
Most Probable Oxidation State
1
0
2
3
_4
- 3
- 2
- 1
H
He
Li
Be
B
C
F
O
N
Ne
3
4
Na
Mg
Al
Si
Cl
S
P
2
1
5
Ar
K
Sc
Ca
Ga
Ti
Ge
Br
Se
As
Zn
Cu
V
Kr
Cr
Mn
Fe
Co
Ni
Rb
Sr
Zr
I
Ag
Nb
Xe
Mo
Tc
Ru
Rh
Pd
Y
In
Sn
Te
Sb
Cd
Ba
Hg
Au
Rn
W
Re
Os
Ir
Pt
Cs
La
Tl
Hf
Pb
At
Po
Bi
Ta
Fr
Ra
Ac
Rf
Du
Sg
Bo
Ha
Me
Ce
Pr
Nd
Pm
Sm
Eu
Gd
Tb
Dy
Ho
Er
Tm
Yb
Lu
3
Th
Pa
U
Np
Pu
Am
Cm
Bk
Cf
Es
Fm
Md
No
Lr
3
41
Newly Discovered Elements
1994
Revised IUPAC Slate
Atomic No.
ACS Slate
IUPAC Slate
104 Rutherfordium Dubnium
Rutherfordium
105 Hahnium Joliotium
Dubnium
106 Seaborgium Rutherfordium
Seaborgium
107 Neilsbohrium Bohrium
Bohrium
108 Hassium Hahnium
Hassium
109 Meitnerium Meitnerium
Meitnerium
110 ?
? 3 Labs
111 ?
? GSI
Final Slate 9/12/97
112 ?
? GSI
42
Groups in the Periodic Table
Main Group Elements (Vertical Groups) Group
IA - Alkali Metals Group IIA - Alkaline Earth
Metals Group IIIA - Boron Family Group
IVA - Carbon Family Group VA - Nitrogen
Family Group VIA - Oxygen Family (Calcogens)
Group VIIA - Halogens Group VIIIA - Noble
Gases Other Groups ( Vertical and Horizontal
Groups) Group IB - 8B - Transition Metals Period
6 Group - Lanthanides (Rare Earth
Elements) Period 7 Group - Actinides
43
The Periodic Table of the Elements
H
He
O
N
C
B
Li
Be
Ne
F
S
P
Si
Al
Na
Mg
Ar
Cl
Se
As
Ge
Ga
Zn
Cu
Ni
Co
Fe
Mn
Cr
V
Ti
Sc
K
Ca
Kr
Br
Te
Sb
Sn
In
Cd
Ag
Pd
Rh
Ru
Tc
Mo
Nb
Zr
Y
Rb
Sr
Xe
I
Po
Bi
Pb
Tl
Hg
Au
Pt
Ir
Os
Re
W
Ta
Hf
La
Cs
Ba
Rn
At
Ac
Fr
Ra
Rf
Sg
Du
Bo
Ha
Me
The Halogens
The Alkali Metals
The Alkaline Earth Metals
The Noble Gases
44
The Periodic Table of the Elements
H
He
Li
Be
F
Ne
B
C
N
O
Na
Mg
Ar
Cl
Al
Si
P
S
K
Ca
Sc
Ti
V
Cr
Mn
Fe
Co
Ni
Cu
Zn
Br
Kr
Ga
Ge
As
Se
Rb
Sr
Y
Zr
Nb
Mo
Tc
Ru
Rh
Pd
Ag
Cd
Xe
I
In
Sn
Sb
Te
Cs
Ba
La
Hf
Ta
W
Re
Os
Ir
Pt
Au
Hg
Rn
At
Tl
Pb
Bi
Po
Fr
Ra
Ac
Rf
Du
Sg
Bo
Ha
Me
Ce
Pr
Nd
Pm
Sm
Eu
Gd
Tb
Dy
Ho
Er
Tm
Yb
Lu
Th
Pa
U
Np
Pu
Am
Cm
Bk Cf
Es
Fm
Md
No
Lr
Boron family
Nitrogen family
Carbon Family
Oxygen Family
45
The Periodic Table of the Elements
H
He
O
N
C
B
F
Ne
Li
Be
S
P
Si
Al
Cl
Ar
Na
Mg
Se
As
Ge
Ga
Br
Kr
K
Ca
Sc
Ti
V
Cr
Mn
Fe
Co
Ni
Cu
Zn
Te
Sb
Sn
In
I
Xe
Rb
Sr
Y
Zr
Nb
Mo
Tc
Ru
Rh
Pd
Ag
Cd
Po
Bi
Pb
Tl
At
Rn
Cs
Ba
La
Hf
Ta
W
Re
Os
Ir
Pt
Au
Hg
Fr
Ra
Ac
Rf
Sg
Ha
Du
Bo
Me
The Transition Metals
Ce
Pr
Nd
Pm
Sm
Eu
Gd
Tb
Dy
Ho
Er
Tm
Yb
Lu
Th
Pa
U
Np
Pu
Am
Cm
Bk
Cf
Es
Fm
Md
No
Lr
Lanthanides The Rare Earth Elements
The Actinides
46
The Periodic Table of the Elements
He
H
B
C
N
O
F
Ne
Be
Li
Si
P
S
Cl
Ar
Al
Mg
Na
Ge
As
Se
Br
Kr
Ga
Zn
Cu
Ni
Co
Fe
Mn
Cr
V
Ti
Sc
Ca
K
Sb
Te
I
Xe
Sn
In
Cd
Ag
Pd
Rh
Ru
Tc
Mo
Nb
Zr
Y
Sr
Rb
At
Rn
Po
Bi
Pb
Tl
Hg
Au
Pt
Ir
Os
Re
W
Ta
Hf
La
Ba
Cs
Sg
Rf
Ac
Ra
Fr
Du
Bo
Ha
Me
Ce
Pr
Nd
Pm
Sm
Eu
Gd Tb
Dy
Ho Er
Tm
Yb
Lu
Th
Pa
U
Np
Pu
Am
Cm
Bk
Cf
Es
Fm
Md
No
Lr
Metals
Semi - metals Metalloids
Non Metals
47
Fig. 2.18
48
Fig. 2.19
49
Fig. 2.20
50
Predicting the Ion an Element Will Form in
Chemical Reactions
Problem What monoatomic ions will each of the
elements form? (a) Barium(z56) (b) Sulfur(z16)
(c) Titanium(z 22) (d) Fluorine(z9) Plan We
use the z value to find the element in the
periodic table and which is the nearest noble
gas. Elements that lie after a noble gas will
loose electrons, and those before a noble gas
will gain electrons. Solution (a) Ba2,
Barium is an alkaline earth element, Group 2A,
and is expected to loose two electrons to
attain the same number of electrons as the
noble gas Xenon! (b) S -2, Sulfur is in the
Oxygen family, Group 6A, and is expected to
gain two electrons to attain the same number of
electrons as the noble gas Argon! (c)
Ti4, Titanium is in Group 4B, and is expected to
loose 4 electrons to attain the same
number of electrons as the noble gas Argon!
(d) F -, Fluorine is in a halogen, Group 7A, and
is expected to gain one electron, to attain
the same number of electrons as the noble gas
Neon!
51
Chemical Compounds and Bonds
Chemical Bonds - The electrostatic forces that
hold the atoms of elements
together in the compound.
Covalent Compounds - Electrons are shared
between atoms of different elements to
form Covalent Cpds.
Ionic Compounds - Electrons are transferred from
one atom to
another to form Ionic Cpds.
Cations - Metal atoms lose electrons to form
ions.
Anions - Nonmetal atoms gain electrons to form
- ions.
Mono-atomic ions form binary ionic compounds
52
Formation of a Covalent Bond between Two
Hydrogen Atoms
Fig. 2.21
53
A Polyatomic Ion
Fig. 2.22
54
Chemical Formulas
Empirical Formula - Shows the relative number of
atoms of each element in the compound.
It is the simplest formula, and is
derived from masses of the elements. Molecular
Formula - Shows the actual number of atoms
of each element in the molecule of the
compound. Structural Formula - Shows the actual
number of atoms, and the bonds between
them that is, the arrangement of
atoms in the molecule.
55
Fig. 2.23
56
Table 2.3 (p. 67) Common Monoatomic Ions
Cations
Anions
Charge Formula Name Charge
Formula Name
1 H hydrogen
1- H - hydride
Li lithium
F - fluoride
Na sodium
Cl - chloride
K potassium
Br - bromide
Cs cesium
I - iodide
Ag silver 2 Mg2
magnesium 2- O 2 -
oxide Ca2 calcium
S2 -
sulfide Sr2 strontium
Ba2 barium
Zn2 zinc Cd2
cadmium 3 Al3 aluminum
3- N 3 -
nitride
Listed by charge those in boldface are most
common
57
Give the Name and Chemical Formulas of the
Compounds Formed from the Following Pairs of
Elements
a) Sodium and Oxygen
Na2O Sodium Oxide b) Zinc and
Chlorine ZnCl2
Zinc Chloride c) Calcium and Fluorine
CaF2 Calcium
Fluoride d) Strontium and Nitrogen
Sr3N2 Strontium Nitride e)
Hydrogen and Iodine
HI Hydrogen Iodide f) Scandium and
Sulfur Sc2S3
Scandium Sulfide
58
Some Metals That Form More than One Oxidation
State
Element Ion Formula
Systematic Name Common Name
Chromium Cr2
Chromium (II)
Chromous Cr3
Chromium (III)
Chromic Cobalt Co2
Cobalt (II)
Co3
Cobalt (III) Copper
Cu1 Copper (I)
Cuprous
Cu2
Copper (II) Cupic Iron
Fe2
Iron (II)
Ferrous Fe3
Iron (III)
Ferric Lead
Pb2 Lead (II)
Pb4
Lead (IV) Manganese
Mn2
Manganese (II)
Mn3 Manganese
(III) Mercury Hg22
Mercury (I)
Mercurous
Hg2 Mercury (II)
Mercuric Tin
Sn2 Tin (II)
Stannous
Sn4
Tin (IV)
Stannic

Table 2.4 (p. 69)
59
Some Common Polyatomic Ions
Formula Name Formula
Name
Cations
Anions Ctd.
NH4 Ammonium H3O
Hydronium
MnO4- Permanganate CO3-2
Carbonate HCO3- Hydrogen Carbonate CrO4-2
Chromate Cr2O7-2 Dichromate O2-2
Peroxide PO4-3
Phosphate HPO4-2 Hydrogen Phosphate H2PO4-
Dihydrogen Phosphate SO3-2
Sulfite SO4-2 Sulfate HSO4-
Hydrogen Sulfate
Anions
CH3COO- Acetate CN-
Cyanide OH- Hydroxide ClO-
Hypochlorite ClO2-
Chlorite ClO3- Chlorate ClO4-
Perchlorate NO2-
Nitrite NO3- Nitrate
60
Determining Names and Formulas of Ionic
Com-pounds of Elements That Form More than One Ion
Give the systematic names for the formulas or the
formulas for the names of the following
compounds.
a) Iron III Sulfide - Fe is 3, and S is -2
therefore the compound is
Fe2S3 b)
CoF2 - the anion is Fluoride (F -1) and there
are two F -1, the cation is
Cobalt and it must be Co2 therefore the
compound is
Cobalt (II) Fluoride c) Stannic Oxide - Stannic
is the common name for Tin (IV), Sn4, the
Oxide ion is O-2, therefore the
formula of the compound is
SnO2 d)
NiCl3 - The anion is chloride (Cl-1), there are
three anions, so the Nickel
cation is Ni3, therefore the name of the
compound is
Nickel (III) Chloride
61
Rules for Families of Oxoanions
Families with Two Oxoanions
The ion with more O atoms takes the nonmetal root
and the suffix -ate. The ion with fewer O
atoms takes the nonmetal root and the suffix
-ite.
Families with Four Oxoanions (usually a Halogen)
The ion with most O atoms has the prefix per-,
the nonmetal root and the suffix -ate. The
ion with one less O atom has just the suffix
-ate. The ion with two less O atoms has the
just the suffix -ite. The ion with three less
O atoms has the prefix hypo- and the suffix
-ite.
62
Naming Oxoanions - Examples
Prefixes Root Suffixes
Chlorine Bromine Iodine
per ate
perchlorate perbromate periodate

ClO4- BrO4- IO4-
ate
chlorate bromate iodate

ClO3- BrO3- IO3-
ite
chlorite bromite iodite

ClO2- BrO2- IO2- hypo
ite
hypochlorite hypobromite hypoiodite

ClO - BrO - IO -
No. of O atoms
63
Numerical Prefixes for Hydrates and Binary
Covalent Compounds
NUMBER PREFIX NUMBER
PREFIX
1 mono- 6
hexa- 2 di-
7
hepta- 3 tri-
8 octa- 4
tetra- 9
nona- 5 penta-
10 deca-
Table 2.6 (p. 70)
64
Hydrates Compounds
Containing Water Molecules
MgSO4 7H2O Magnesium Sulfate
heptahydrate
CaSO4 2H2O Calcium Sulfate dihydrate
Ba(OH)2 8H2O Barium Hydroxide octahydrate
CuSO4 5H2O Copper II Sulfate
pentahydrate
Na2CO3 10H2O Sodium Carbonate decahydrate
65
Examples of Names and Formulas of Oxoanions and
Their Compounds - I

• KNO2 Potassium Nitrite
  BaSO3 Barium Sulfite
• Mg(NO3)2 Magnesium Nitrate Na2SO4
  Sodium Sulfate
• LiClO4 Lithium Perchlorate Ca(BrO)2
  Calcium Hypobromite
• NaClO3 Sodium Chlorate
  Al(IO2)3 Aluminum Iodite
• RbClO2 Rubidium Chlorite KBrO3
  Potassium Bromate
• CsClO Cesium Hypochlotite LiIO4
  Lithium Periodate

66
Examples of Names and Formulas ofOxoanions and
Their Compounds - II

• Calcium Nitrate Ca(NO3)2 Ammonium
  Sulfite (NH4)2SO3
• Strontium Sulfate SrSO4
  Lithium Nitrite LiNO2
• Potassium Hypochlorite KClO Lithium
  Perbromate LiBrO4
• Rubidium Chlorate RbClO3
  Calcium Iodite Ca(IO2)2
• Ammonium Chlorite NH4ClO2 Boron
  Bromate B(BrO3)3
• Sodium Perchlorate NaClO4 Magnesium
  Hypoiodite Mg(IO)2

67
Determining Names and Formulas of Ionic
Compounds Containing Polyatomic Ions
Ba2 is the cation Barium, Cl- is the Chloride
anion. There are five water molecules
therefore the name is Barium Chloride
Pentahydrate
a) BaCl2
5 H2O
b) Magnesium Perchlorate Magnesium is the
Mg2 cation, and
perchlorate is the ClO4- anion, therefore we
need two
perchlorate anions for each Mg cation
therefore the formula is
Mg( ClO4)2
c) (NH4)2SO3 NH4 is the ammonium ion,
and SO3-2 is the
sulfite anion, therefore the name is
Ammonium
Sulfite
d) Calcium Nitrate Calcium is the Ca2 cation,
and nitrate is the
NO3- anion, therefore the formula is

Ca(NO3)2
68
Naming Acids
1) Binary acids solutions form when certain
gaseous compounds dissolve in water. For
example, when gaseous hydrogen chloride
(HCl) dissolves in water, it forms a solution
called hydrochloric acid. Prefix hydro-
anion nonmetal root suffix -ic the word acid

hydrochloric acid
2) Oxoacid names are similar to those of the
oxoanions, except for two suffix changes
Anion -ate suffix becomes an -ic suffix in
the acid. Anion -ite suffix becomes an
-ous suffix in the acid. The oxoanion
prefixes hypo- and per- are retained. Thus,
BrO4- is perbromate, and HBrO4 is perbromic
acid IO2- is iodite, and HIO2 is iodous
acid.
69
Determining Names and Formulas of Anions and Acids

• Problem Name the following anions and give the
  names and
• formulas of the acid
  solutions derived from them
• a) I - b) BrO3- c) SO3-2
  d) NO3- e) CN -
• Solution
• a) The anion is Iodide and the acid is
  Hydroiodic acid, HI
• b) The anion is Bromite and the acid is
  Bromous acid, HBrO2
• c) The anion is Sulfite and the acid is
  Sulfurous acid, H2SO3
• d) The anion is Nitrate and the acid is
  Nitric acid, HNO3
• e) The anion is Cyanide and the acid is
  Hydrocyanic acid, HCN

70
Names and Formulas of Binary Covalent Compounds
1) The element with the lower group number in the
periodic table is the first word in the name
the element with the higher group number is the
second word. (Important exception When the
compound contains oxygen and a halogen, the
halogen is named first.) 2) If both elements are
in the same group, the one with the higher
period number is named first. 3) The second
element is named with its root and the suffix
-ide. 4) Covalent compounds have Greek
numerical prefixes (table 2.6) to indicate the
number of atoms of each element in the compound.
The first word has a prefix only when more than
one atom of the element is present the second
word always has a numerical prefix.
71
Determining Names and Formulas of Binary
Covalent Compounds
Problem
What are the name or Chemical formulas of the
following Chemical compounds
a) Carbon dioxide b) PCl3 c) Give the name and
chemical formula of the compound formed from two
P atoms and five O atoms.
Solution
a) The prefix di- means two. The formula is
CO2 b) P is the symbol for phosphorous there
are three chlorine atoms which require the
prefix tri-. The name of the compound is
phosphorous trichloride c) P
comes first in the name (lower group number). The
compound is diphosphorous pentaoxide
( commonly called phosphorous
pentaoxide)
72
Naming Alkanes
Alkanes are hydrocarbons that are called
saturated hydrocarbons, they contain only
single bonds, no multiple bonds ! Alkanes have
the general formula --- C n H 2n2 Each carbon
atom has four bonds to others atoms ! The names
for alkanes all end in -ane Alkanes are found in
three distinct groups a) Straight
chain hydrocarbons b) Branched
chain hydrocarbons c) Cyclic
hydrocarbons
73
The First 10 Straight-Chain Alkanes
Name Formula
Structural Formulas
H
H
H
Methane CH4 Ethane
C2H6 Propane
C3H8 Butane
C4H10 Pentane
C5H12 Hexane
C6H14 Heptane C7H16 Octane
C8H18 Nonane
C9H20 Decane
C10H22
C
H
H
H
H
C C
H
H
H
CH3-CH2-CH3
CH3-(CH2)2-CH3
CH3-(CH2)3-CH3
CH3-(CH2)4-CH3
CH3-(CH2)5-CH3
CH3-(CH2)6-CH3
CH3-(CH2)7-CH3
CH3-(CH2)8-CH3
Table 2.7
74
Calculating the Molecular Mass of a Compound
Problem Using the data in the periodic table,
calculate the molecular
mass of the following compounds a)
Tetraphosphorous decoxide b) Ammonium sulfate
Plan We first write the formula, then multiply
the number of atoms (or ions) of each
element by its atomic mass, and find the sum.
Solution
a) The formula is P4O10. Molecular mass (4 x
atomic mass of P ) (10 x atomic mass of O )
( 4 x 30.97 amu) ( 10
x 16.00 amu)
283.88 283.9 amu b) The formula is (NH4)2SO4
Molecular mass ( 2 x atomic mass of N ) ( 8 x
atomic mass of H)
( 1 x atomic mass of S ) ( 4 x atomic mass of
O) ( 2 x 14.01 amu)
( 8 x 1.008 amu)
( 1 x 32.07 amu) ( 4 x 16.00 amu)
132.154 amu 132.15 amu
75
Calculate the Molecular Mass of Glucose C6H12O6

• Carbon 6 x 12.011 g/mol 72.066 g
• Hydrogen 12 x 1.008 g/mol 12.096 g
• Oxygen 6 x 15.999 g/mol 95.994 g
• 
  

180.156 g
76
Fig. 2.25
77
Mixtures
Heterogeneous mixtures has one or more visible
boundaries between the components. Homogeneo
us mixtures has no visible boundaries
because the components are mixed as individual
atoms, ions, and molecules. Solutions A
homogeneous mixture is also called a solution.
Solutions in water are called aqueous solutions,
and are very important in chemistry. Although
we normally think of solutions as liquids,
they can exist in all three physical states.

78
Separating Mixtures
Filtration Separates components of a mixture
based upon differences in particle
size. Normally separating a
precipitate from a solution, or particles from an
air stream. Crystallization
Separation is based upon differences in
solubility of components in a
mixture. Distillation separation is based upon
differences in volatility. Extraction
Separation is based upon differences in
solubility in different solvents (major
material). Chromatography Separation is based
upon differences in solubility
in a solvent versus a stationary phase.
79
Filtration
Fig. 2.D
80
Crystallization
Fig. 2.E
81
Fig. 2.F
82
Fig. 2.G
83
Procedure for Column Chromatography
Fig. 2.H
84
Fig. 2.I AB