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Chapter Two:
ATOMS, MOLECULES, AND IONS
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2-1 The Early History of Chemistry
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2-2 Fundamental Chemical Laws
Three Important Laws
 Law
of conservation of mass
Mass
 Law
A
is neither created nor destroyed
of definite proportion
given compound always contains exactly
the same proportion of elements by mass
Three Important Laws (continued)
 Law
of multiple proportions
When two elements form a series of compounds,
the ratios of the masses of the second element
that combine with 1 gram of the first element can
always be reduced to small whole numbers.
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Ex 2.1 Illustrating the Law of Multiple
Proportions
The following data were collected for several compounds of nitrogen
and oxygen:
Sow how these data illustrate the law of multiple proportions.
Solution:
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2-3 Dalton’
s Atomic Theory
Dalton’
s Atomic Theory (1808)
Each
element is made up of tiny particles called
atoms.
Dalton’
s Atomic Theory (1808) (continued)
 The
atoms of a given element are identical; the
atoms of different elements are different in
some fundamental way or ways.
Dalton’
s Atomic Theory (continued)
Chemical
compounds are formed when atoms
combine with each other. A given compound
always has the same relative numbers and types of
atoms.
Dalton’
s Atomic Theory (continued)
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.
Avogadro’
s Hypothesis (1811)
At the same temperature and pressure, equal volumes of
different gases contain the same number of particles.
5
liters of oxygen
5
liters of nitrogen
Same
number of particles!
Representing Gay-Lussac’
s Results
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Representing Gay-Lussac’
s Results
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2-4 Early Experiments to
Characterize the Atom
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The Electron
Figure 2.7 A Cathode-ray tube. The fast-moving electrons excite the
gas in the tube, causing a glow between the electrodes. The green color
in the photo is due to the response of the screen (coated with zinc
sulfide) to the electron beam.
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Early Experiments to Characterize the Atom
 J.
J. Thomson - postulated the existence of
electrons using cathode ray tubes.
 Ernest
Rutherford - explained the nuclear atom,
containing a dense nucleus with electrons
traveling around the nucleus at a large distance.
Cathode Ray Tube
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Milliken Oil Drop Experiment
2-5 The Modern View of Atomic
Structure
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The atom contains:
electrons
protons:
found in the nucleus; positive charge
equal in magnitude to the electron’
s negative
charge.
neutrons:
found in the nucleus; no charge;
virtually same mass as a proton.
The Nuclear Atom
Radioactivity
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Rutherford’
s Gold Foil Experiment
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Nuclear Atom Viewed in Cross Section
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Two Isotopes of Sodium
Ex 2.2 Writing the Symbols for Atoms
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Write the symbol for the atom that has an atomic number
of 9 and a mass number of 19. How many electrons and
how many neutrons does this atom have?
Solution:
2-6 Molecules and Ions
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Formation of Ionic Compounds
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Molecular vs. Ionic Compounds
Covalent Bonding
2-7 An Introduction to the Periodic
Table
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The Periodic Table
2-8 Naming Simple Compounds
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Binary Ionic Compounds (Type I)
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Naming Binary Ionic Compounds
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Ex 2.3 Naming Type I Binary Compounds
Name each binary compound.
a. CsF
Solution
b. AlCl3
c. LiH
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Ex 2.4 Formulas from Names for
Type I Binary Compounds
Given the following systematic names, write the formula
foe each compound:
a. Potassium iodide, b. Calcium oxide, c. Gallium bromide
Solution:
Formulas from Names
Binary Ionic Compounds (Type II)
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Ex 2.5 Naming Type II Binary Compounds
1. Give the systematic name for each of the following
compounds:
a. CuCl
b. HgO
c. Fe2O3
2. Given the following systematic names, write the
formula for each compound:
a. Manganese(IV) oxide
b. Lead(II) chloride
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Solution:
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Ex 2.6 Naming Binary Compounds
1. Give the systematic name for each of the following
compounds:
a. CoBr2
b. CaCl2
c. Al2O3
2. Given the following systematic names, write the
formula for each compound:
a. Chromium(III) chloride
b. Gallium iodide
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S0lution:
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Figure 2.22 The common cations and anions
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Ex 2.7 Naming Compounds Containing
Polyatomic Ions
1. Give the systematic name for each of the following
compounds:
a. Na2SO4, b. KH2PO4, c. Fe(NO3)3,
d. Mn(OH)2, e. Na2SO3, f. Na2CO3
2. Given the following systematic names, write the formula
for each compound:
a. Sodium hydrogen carbonate,
b. Cesium perchlorate
c. Sodium hypochlorite
d. Sodium selenate
e. Potassium bromate
Solution:
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Ex 7.7 Solution (continued)
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Binary Covalent Compounds (Type III)
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N2O
NO
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Ex 2.8 Naming Type III Binary
Compounds
1. Name each of the following compounds:
a. PCl5, b. PCl3, c. SO2
2. From the following systematic names, write the formula
for each compound:
a. Sulfur hexafluoride, b. Sulfur trioxide,
c. Carbon dioxide
Solution:
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Flowchart for Naming Binary Compounds
Figure 2.23
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Overall Strategy for Naming
Chemical Compounds
Figure 2.34
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Ex 2.9 Naming Various Types of
Compounds
1. Give the systematic name for each of the following
compounds:
a. P4O10, b. Nb2O5,
c. Li2O2, d. Ti(NO3)4
2. Given the following systematic names, write the
formula for each compound:
a. Vanadium(V) fluoride, b. Dioxygen difluoride,
c. Rubidium peroxide,
d. Gallium oxide
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Solution:
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Ex 2.9 Solution (continued):
Flowchart for Naming Acids
Figure 2.25
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