Atoms, Molecules, and Ions - PowerPoint PPT Presentation

About This Presentation
Title:

Atoms, Molecules, and Ions

Description:

Atoms, Molecules, and Ions Computer simulation of the interior view of a twisted nanotube. Priestley Medal Figure 2.2: John Dalton Figure 2.3 (P19): Combining gases ... – PowerPoint PPT presentation

Number of Views:594
Avg rating:3.0/5.0
Slides: 116
Provided by: Zol6
Category:

less

Transcript and Presenter's Notes

Title: Atoms, Molecules, and Ions


1
Chapter 2
  • Atoms, Molecules, and Ions

2
Chapter 2 Atoms, Molecules and Ions
2.1 The Early History of Chemistry 2.2
Fundamental Chemical laws 2.3 Daltons Atomic
Theory 2.4 Cannizzaros Interpretation 2.5 Early
experiments to Characterize the Atom 2.6 The
Modern View of Atomic Structure An
Introduction 2.7 Molecules and Ions 2.8 An
Introduction to the Periodic Table 2.9 Naming
Simple Compounds
3
Computer simulation of the interior view of a
twisted nanotube.
4
(No Transcript)
5
Priestley Medal
Source Roald Hoffman, Cornell University
6
(No Transcript)
7
Laws of Mass Conservation Definite
Proportions (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.

8
(No Transcript)
9
Figure 2.2 John Dalton
Source Manchester Literary Philosophical
Society
10
Mass of Oxygen that Combines with 1.00g
of Carbon
Compound 1
1.33g Compound 2
2.66g
11
(No Transcript)
12
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 Cpd 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
13
Mass of Nitrogen that Combines with
1.00g of Oxygen
Compound 1 1.750
g Compound 2 0.8750
g Compound 3 0.4375 g
I 1.750 2 Cpd 1
N2O NO N4O2 II
0.8750 1 II
0.8750 2 Cpd 2 NO
or NO2 or N2O2 III 0.4375
1 I 1.750 4
Cpd 3 NO2 NO4
N2O4 III 0.4375 1


14
Daltons Atomic Theory
Postulates 1. Each element is made up of
tiny particles called atoms. 2. The atoms of
a given element are identical the atoms
of different elements are different in some
fundamental way or ways. 3. Chemical
compounds are formed when atoms combine
with each other. A given compound always has the
same relative numbers and types of
atoms. 4. Chemical reactions involve
reorganization of the atoms changes in
the way they are bound together. The atoms
themselves are not changed in a chemical
reaction.
15
(No Transcript)
16
Figure 2.3 (P19) Combining gases on a Molecular
Level
17
Avogadros Hypothesis
At the same temperature and Pressure, equal
volumes of different gases contain the same
number of particles (Molecules).
18
Stanislao Cannizzaro
Source Corbis
19
Cannizzaros Relative Atomic(Molecular)
Masses of Carbon and Hydrogen
Compound Relative
Percent Carbon Relative mass of
Molecular Mass
by Mass Carbon
Present Methane 16
75
12 Ethane
30 80
24 Propane
44
82
36 Butane 58
83
48 Carbon Dioxide
44 27
12 Compound
Relative Percent
Hydrogen Relative mass of
Molecular Mass
by Mass Hydrogen Present Methane
16
25
4 Ethane 30
20
6 Propane
44 18
8 Butane
58
17
10
20
Comparison of Several of Berzeliuss Atomic
Masses with Current Values
Element
Atomic Mass
Berzeliuss Value Current
Value Chlorine
35.41
35.45 Copper 63.00
63.55 Hydrogen
1.00
1.01 Lead
207.12
207.2 Nitrogen
14.05
14.01 Oxygen
16.00
16.00 Potassium 39.19
39.10 Silver
108.12
107.87 Sulfur
32.18
32.07
21
Figure 2.4 An STM image of nickel atoms placed
on a copper surface.
Source IBM Research
22
Figure 2.5 Image of a ring of cobalt atoms
placed on a copper surface.
Source IBM Research
23
Figure 2.6 A cathode-ray tube. The fast-moving
electrons
24
Figure 2.7 Deflection of cathode rays by an
applied electric field.
25
(No Transcript)
26
(No Transcript)
27
Figure 2.8 (P24)ThomsonsPlum Pudding model
28
Figure 2.9 Schematic representation of the
apparatus Millikan
29
(No Transcript)
30
(No Transcript)
31
Marie Sklodowska Curie
Source Corbis
32
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.

33
Figure 2.11 (P25) Rutherfords experiment
34
Figure 2.12 The expected results of the metal
foil experiment
35
(No Transcript)
36
(No Transcript)
37
(No Transcript)
38
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!!!!!

39
Figure 2.13 (P26) Nuclear atom cross section
40
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.
41
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
42
Table 2.2 (P 27) The Masses and Charges of
the Electron Proton and Neutron
  • Particle Mass
    Charge
  • Electron 9.11 x 10 31
    kg -1
  • Proton 1.67 x 10 27
    kg 1
  • Neutron 1.67 x 10 27
    kg none
  • The magnitude of the charge on the electron and
    proton is
  • 1.60 x 10-19 coulombs .

43
(No Transcript)
44
Figure 2.14(P28) Isotopes of sodium
45
(No Transcript)
46
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 (30)
  • 235 U P(92), e-(92),
  • N (143)

47
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.
48
Figure 2.15 Space-filling model of the methane
molecule
49
Figure 2.17 Ball-and-stick model
50
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.
51
Definitions
Chemical Bonds The forces that hold atoms
together in compounds Covalent Bonds The
sharing of electrons in a chemical bond Molecule
A group of atoms held together by covalent
bonds Chemical Formula The symbols of for the
elements are used to
indicate the types of atoms present, and
the
subscripts are used to indicate the relative
numbers of atoms
present Structural Formula a Formula in which
the bonds are shown along
with the elemental symbols and
order of atom
arrangement
52
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
53
(No Transcript)
54
Molecular model Electron transferred from
sodium to chlorine (neutral sodium to neutral
sodium ion)
55
Molecular model Electron added to chlorine
(neutral chlorine to chloride ion)
56
Figure 2.18 Sodium metal reacts with chlorine
gas
57
Figure 2.19 (P31) Na/Cl arrangement
58
Figure 2.16 Space-filling models of various
molecules.
59
Figure 2.20 Ball-and-stick models of the
ammonium ion and nitrate ion.
60
(No Transcript)
61
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

62
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
Db
Bh
Hs
Mt
Ds
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
63
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
Db
Bh
Hs
Mt
Ds
The Halogens
The Alkali Metals
The Alkaline Earth Metals
The Noble Gases
64
Samples of the alkai metals
Source Tom Pantages
65
Three members of the halogen family
Source Tom Pantages
66
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
Db
Sg
Bh
Hs
Mt
Ds
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
67
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
Ds
Fr
Ra
Ac
Rf
Sg
Hs
Db
Bh
Mt
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
68
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
69
Figure 2.21 The periodic table continues to
expand as new elements are synthesized
70
The Periodic Table of the Elements
H
He
Date of Discovery of the Elements
Li
Be
B
N
O
F
Ne
C
Na
Mg
Ar
Al
Si
Cl
S
P
K
Ca
Sc
Ti
V
Cr
Mn
Co
Ni
Zn
Ga
Ge
Se
Br
Kr
Fe
As
Cu
Rb
Sr
Y
Zr
Nb
Mo
Tc
Ru
Rh
Pd
Cd
Xe
I
Te
In
Sb
Sn
Ag
Cs
Ba
La
Hf
Ta
W
Re
Os
Ir
Pt
Rn
At
Po
Tl
Bi
Pb
Hg
Au
Fr
Ra
Ac
Rf
Db
Sg
Bh
Hs
Mt Ds
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
1850 - 1900
1700 - 1750
Before 1600
1750 - 1800
1900 - 1950
1600 - 1700
1800 - 1850
1950 - 2000
71
The Periodic Table of the Elements
He
Date of Discovery of the Elements
H
B
N
O
F
Ne
C
Li
Be
Ar
Al
Si
Cl
S
Na
Mg
P
Sc
Ti
V
Cr
Mn
Ni
Ga
Ge
Se
Br
Kr
Fe
As
Cu
Ca
K
Zn
Co
Rb
Sr
Y
Zr
Nb
Mo
Tc
Ru
Rh
Pd
Cd
Xe
I
Te
In
Sb
Sn
Ag
Cs
Ba
La
Hf
Ta
W
Re
Os
Ir
Rn
At
Po
Tl
Bi
Pb
Hg
Au
Pt
Fr
Ra
Ac
Rf
Db
Sg
Bh
Hs
Mt Ds
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
1850 - 1900
1700 - 1750
Before 1600
1750 - 1800
1900 - 1950
1600 - 1700
1800 - 1850
1950 - 2000
72
The Periodic Table of the Elements
He
Date of Discovery of the Elements
H
B
F
Ne
C
Li
Be
N
O
Ar
Al
Si
S
Na
Mg
Cl
P
Sc
V
Ga
Ge
Se
Br
Kr
Fe
As
Cu
Ca
K
Zn
Co
Ti
Cr
Mn
Ni
Rb
Nb
Tc
Ru
Rh
Pd
Cd
Xe
I
In
Sb
Sn
Ag
Sr
Y
Zr
Mo
Te
Cs
Ba
La
Hf
Ta
Re
Os
Ir
Rn
At
Po
Tl
Bi
Pb
Hg
Au
Pt
W
Fr
Ra
Ac
Rf
Db
Sg
Bh
Hs
Mt Ds
Ce
Pr
Nd
Pm
Sm
Eu
Gd
Tb
Dy
Ho
Er
Tm
Yb
Lu
Th
Pa
Np
Pu
Am
Cm
Bk Cf
Es
Fm
Md
No
Lr
U
1850 - 1900
1700 - 1750
Before 1600
1750 - 1800
1900 - 1950
1600 - 1700
1800 - 1850
1950 - 2000
73
The Periodic Table of the Elements
He
Date of Discovery of the Elements
H
F
Ne
C
Be
N
O
Li
B
Ar
S
Mg
Cl
P
Na
Al
Si
Sc
Ga
Ge
Kr
Fe
As
Cu
Zn
Co
Ti
Cr
Mn
Ni
K
Ca
V
Se
Br
Rb
Tc
Xe
In
Sb
Sn
Ag
Sr
Y
Zr
Mo
Te
Nb
Rh
Pd
Cd
I
Ru
Cs
Hf
Re
Rn
At
Po
Tl
Bi
Pb
Hg
Au
Pt
W
Ba
La
Ta
Os
Ir
Fr
Ra
Ac
Rf
Db
Sg
Bh
Hs
Mt Ds
Pr
Pm
Sm
Eu
Gd
Dy
Ho
Tm
Yb
Lu
Ce
Nd
Tb
Er
Pa
Np
Pu
Am
Cm
Bk Cf
Es
Fm
Md
No
Lr
Th
U
1850 - 1900
1700 - 1750
Before 1600
1750 - 1800
1900 - 1950
1600 - 1700
1800 - 1850
1950 - 2000
74
The Periodic Table of the Elements
Date of Discovery of the Elements
H
He
C
Be
N
O
Li
B
F
Ne
S
Mg
Cl
P
Na
Al
Si
Ar
Fe
As
Cu
Zn
Co
Ti
Cr
Mn
Ni
K
Ca
V
Se
Br
Sc
Ga
Ge
Kr
Tc
Sb
Sn
Ag
Sr
Y
Zr
Mo
Te
Nb
Rh
Pd
Cd
I
Ru
Rb
In
Xe
Hf
Re
At
Bi
Pb
Hg
Au
Pt
W
Ba
La
Ta
Os
Ir
Cs
Tl
Po
Rn
Fr
Rf
Sg
Ra
Ac
Bh
Db
Hs
Mt Ds
Pm
Lu
Ce
Nd
Tb
Er
Pr
Sm
Eu
Gd
Dy
Ho
Tm
Yb
Pa
Np
Pu
Am
Cm
Bk Cf
Es
Fm
Md
No
Lr
Th
U
1850 - 1900
1700 - 1750
Before 1600
1750 - 1800
1900 - 1950
1600 - 1700
1800 - 1850
1950 - 2000
75
The Periodic Table of the Elements
Date of Discovery of the Elements
H
He
C
Be
N
O
Li
B
F
Ne
S
Mg
Cl
P
Na
Al
Si
Ar
Fe
As
Cu
Zn
Co
Ti
Cr
Mn
Ni
K
Ca
V
Se
Br
Sc
Ga
Ge
Kr
Sb
Sn
Ag
Sr
Y
Zr
Mo
Te
Nb
Rh
Pd
Cd
I
Ru
Rb
In
Xe
Tc
At
Bi
Pb
Hg
Au
Pt
W
Ba
La
Ta
Os
Ir
Cs
Tl
Po
Rn
Re
Hf
Rf
Db
Sg
Ra
Ac
Fr
Bh
Hs
Mt Ds
Ce
Nd
Tb
Er
Pr
Sm
Eu
Gd
Dy
Ho
Tm
Pm
Yb
Lu
Es
Fm
Md
No
Lr
Th
U
Pa
Np
Pu
Am
Cm
Bk
Cf
1850 - 1900
1700 - 1750
Before 1600
1750 - 1800
1900 - 1950
1600 - 1700
1800 - 1850
1950 - 2000
76
The Periodic Table of the Elements
Date of Discovery of the Elements
H
He
C
Be
N
O
Li
B
F
Ne
S
Mg
Cl
P
Na
Al
Si
Ar
Fe
As
Cu
Zn
Co
Ti
Cr
Mn
Ni
K
Ca
V
Se
Br
Sc
Ga
Ge
Kr
Sb
Sn
Ag
Sr
Y
Zr
Mo
Te
Nb
Rh
Pd
Cd
I
Ru
Rb
In
Xe
Tc
Bi
Pb
Hg
Au
Pt
W
Ba
La
Ta
Os
Ir
Cs
Tl
Po
Rn
At
Re
Hf
Ra
Ac
Fr
Rf
Sg
111
Db
Bh
Hs
Mt
Ds
Ce
Nd
Tb
Er
Pr
Sm
Eu
Gd
Dy
Ho
Tm
Pm
Yb
Lu
Th
Pa
U
Np
Pu
Am
Cm
Bk
Cf
Lr
Es
Fm
Md
No
1850 - 1900
1700 - 1750
Before 1600
1750 - 1800
1900 - 1950
1600 - 1700
1800 - 1850
1950 - 2000
77
(No Transcript)
78
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 Darmstadium Darmstadium
Darmstadium
111 ?
? GSI
Final Slate 9/12/04
112 ?
? GSI
79
The Periodic Table of the Elements
H
He
1997- 2004
Li
Be
B
C
N
O
F
Ne
Na
Mg
Ar
Al
Si
P
S
Cl
K
Ca
Sc
Ti
V
Cr
Mn
Fe
Co
Ni
Cu
Zn
Ga
Ge
As
Se
Br
Kr
Rb
Sr
Y
Zr
Nb
Mo
Tc
Ru
Rh
Pd
Ag
Cd
Xe
I
Te
Sb
Sn
In
Cs
Ba
La
Hf
Ta
W
Re
Os
Ir
Pt
Au
Hg
Rn
At
Po
Bi
Pb
Tl
Mt
Ds
Fr
Ra
Ac
Rf
Db
Sg
Bh
Hs
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
80
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
2
1
5
Na
Mg
Al
Si
Cl
S
P
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
Mt
Ds
Fr
Ra
Ac
Rf
Db
Sg
Bh
Hs
3
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
3
81
(No Transcript)
82
Table 2.3(P35) Common Monatomic
Cations and Anions
Cation Name
Anion Name
H hydrogen
H- hydride Li
lithium F-
fluoride Na
sodium Cl-
chloride K
potassium Br-
bromide Cs cesium
I-
iodide Be2 beryllium
O2- oxide
Mg2 magnesium
S2- sulfide
Ca2 calcium
N3- nitride Ba2
barium P3-
phosphide Al3
aluminum Ag silver
Zn2 zinc
83
Table 2.4(P36) Common Type II Cations
Ion Systematic Name
Alternate Name Fe3
iron (III)
ferric Fe2
iron (II)
ferrous Cu2
copper (II)
cupric Cu
copper (I)
cuprous Co3
cobalt (III)
cobaltic Co2
cobalt (II)
cobaltous Sn4
tin (IV)
stannic Sn2
tin (II)
stannous Pb4
lead (IV)
plumbic Pb2
lead (II)
plumbous Hg2
mercury (II)
mercuric Hg22
mercury (I)
mercurous Note that mercury (I) ions always
occur bound together to form Hg22
84
A dish of copper (II) sulfate.
Source Tom Pantages
85
Crystals of copper (II) sulfate
86
Like Example 2.2 (P 37)
  • Give the systematic name of each of the following
    compounds
  • Fe Cl3 d) B2O3
    g) Na2O
  • SrF2 e) SnBr4
    h) CsBr
  • c) MgS f ) Ca3N2
  • Solution
  • a) iron (III) chloride e)
    Tin (IV) bromide
  • b) Strontium fluoride f )
    Calcium Nitride
  • c) Magnesium Sulfide g)
    Sodium Oxide
  • d) Boron Oxide h)
    Cesium bromide

87
Does the compound contain Type I or Type II
cations
88
Various chromium compounds dissolved in water
Cr(NO3)3
CrCl3
K2Cr2O7
K2CrO4
CrCl2
89
Table 2.5 (P 38) Common Polyatomic Ions
Ion Name
Ion Name
NH4 ammonium CO32-
carbonate NO2-
nitrite HCO3-
hydrogen carbonate NO3- nitrate

(bicarbonate is a SO32- sulfite
used
common name) SO42- sulfate
ClO-
hypochlorite HSO4- hydrogen sulfate
ClO2- chlorite
(bisulfate is a widely ClO3-
chlorate used
common name) ClO4-
perchlorate OH- hydroxide
C2H3O2- acetate CN-
cyanide MnO4-
permanganate PO43-
phosphate Cr2O72-
dichromate HPO42- hydrogen phosphate
CrO42- chromate H2PO4-
dihydrogen phosphate O22-
peroxide
90
Table 2.6 (P 39) Prefixes Used to Indicate
Number in Chemical Names
Prefix
Number Indicated mono-

1 di-
2 tri-

3 tetra-

4 penta-
5 hexa-

6 hepta-
7 octa-

8 nana-
9 deca-

10
91
Figure 2.22 Flowchart for naming binary
compounds
92
Figure 2.23 Flowchart for overall strategy for
naming chemical compounds
93
Microtaggants
Source Microtrace, Minneapolis, MN 55449
94
Like Example 2.3 (P 40) Give the systematic name
of
each of the following compounds

Compounds a. Na3PO4
d. KClO4 g. NaIO3
b. K2SO4 e.
KHCO3 h. NaOH
c. CuCO3 f. Cs2SO3

Names a. Sodium
Phosphate e. Potassium Hydrogen
Carbonate b. Potassium Sulfate
f. Cesium Sulfite
c. Copper (II) Carbonate
g. Sodium Iodate d. Potassium Perchlorate
h. Sodium Hydroxide
95
Like Example 2.4 (P 42) Give the chemical formula
of
each of the following compounds

Names a. Sodium Peroxide e.
Lithium Hydrogen Carbonate b. Chromium (VI)
Oxide f. Calcium Carbonate
c. Aluminum Oxide g.
Copper (II) Chloride d. Ammonium
Carbonate h. Magnesium Perchlorate

Compounds a. Na2O2
e. LiHCO3 b. CrO3
f. CaCO3
c. Al2O3
g. Cu(Cl)2 d. (NH4)2CO3
h. Mg(ClO4)2
96
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.
97
Figure 2.24(P44) Naming acids
98
Table 2.7 (P 44) Names of Acids that do not

Contain Oxygen
Acid
Name
HF
hydrofluoric acid HCl
hydrochloric acid HBr
hydrobromic acid HI

hydroiodic acid HCN
hydrocyanic acid H2S
hydrosulfuric acid
99
Table 2.8 (P 44) Names of some Oxygen-
Containing
Acids
Acid
Name
HNO3
nitric acid HNO2
nitrous acid H2SO4
sulfuric acid H2SO3
sulfurous
acid H3PO4
phosphoric acid HC2H3O2
acetic acid
100
Naming of the Oxoacids of Chlorine
Acid Anion
Name
HClO4 perchlorate
perchloric acid HClO3 chlorate
chloric acid HClO2
chlorite chlorous
acid HClO hypochlorite
hypochlorous acid
101
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.
102
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
103
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
lose 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 lose 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
lose 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!
104
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
105
Determining Names and Formulas of Ionic
Compounds 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
106
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
107
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

108
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

109
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
110
Determining Names and Formulas ofAnions 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 Bromate and the acid is
    Bromic acid, HBrO3
  • 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

111
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)
112
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 ___________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
____________ amu
113
Calculate the Molecular Mass of Glucose C6H12O6
  • Carbon 6 x 12.01 g/mol 72.06 g
  • Hydrogen 12 x 1.008 g/mol 12.096 g
  • Oxygen 6 x 16.00 g/mol 96.00 g


g
114
(No Transcript)
115
A space-filled model of C60 containing a "caged"
methanol molecule
Source Photo Researchers
Write a Comment
User Comments (0)
About PowerShow.com