p38

2-1
p39

2-2
p41

Three Important Laws
 Law of conservation of mass
 Mass is neither created nor destroyed
 Law of definite proportion
 A 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.

Ex 2.1
Illustrating the Law of Multiple
Proportions
The following data were collected for several compounds of nitrogen
P42 and oxygen:
Sow how these data illustrate the law of multiple proportions.
Solution:

2-3
Dalton ’
 Each element is made up of tiny particles called atoms .
p43

Dalton ’
 The atoms of a given element are identical; the atoms of different elements are different in some fundamental way or ways .

Dalton ’
 Chemical compounds are formed when atoms combine with each other. A given compound always has the same relative numbers and types of atoms.

Dalton ’
 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 ’
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 ’ p43

Representing Gay-Lussac
’ p45

2-4
The Electron p45
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.

p47

p47

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

p48

Milliken Oil Drop Experiment

2-5
The atom contains:
 electrons
 protons : found in the nucleus; positive charge equal in magnitude to the electron ’ charge.
 neutrons : found in the nucleus; no charge; virtually same mass as a proton.
p49

The Nuclear Atom
Radioactivity p49

Rutherford ’

Nuclear Atom Viewed in Cross Section p50

Two Isotopes of Sodium p50

Ex 2.2
Writing the Symbols for Atoms
Write the symbol for the atom that has an atomic number
P52 of 9 and a mass number of 19. How many electrons and how many neutrons does this atom have?
Solution:

2-6
p52

p53

Formation of Ionic Compounds

p54

p55

Molecular vs. Ionic Compounds

Covalent Bonding

2-7
p55

The Periodic Table p56

2-8
p57

p58

Naming Binary Ionic Compounds p58

Ex 2.3
Naming Type I Binary Compounds
Name each binary compound.
P58 a. CsF
Solution b. AlCl
3 c. LiH

Ex 2.4
Formulas from Names for
Type I Binary Compounds
Given the following systematic names, write the formula foe each compound:
P59 a. Potassium iodide, b. Calcium oxide, c. Gallium bromide
Solution:

p59

Ex 2.5
Naming Type II Binary Compounds
P59
1. Give the systematic name for each of the following compounds: a. CuCl b. HgO c. Fe
2
O
3
2. Given the following systematic names, write the formula for each compound: a. Manganese(IV) oxide b. Lead(II) chloride

Solution: p60

Ex 2.6
Naming Binary Compounds
1. Give the systematic name for each of the following compounds:
P60 a. CoBr
2 b. CaCl
2 c. Al
2
O
3
2. Given the following systematic names, write the formula for each compound: a. Chromium(III) chloride b. Gallium iodide

S0lution: p61

Figure 2.22 The common cations and anions p61

p62

P62
Ex 2.7
Naming Compounds Containing
Polyatomic Ions
1.
Give the systematic name for each of the following compounds: a. Na
2
SO
4
, b. KH
2
PO
4
, c. Fe(NO
3
)
3
, d. Mn(OH)
2
, e. Na
2
SO
3
, f. Na
2
CO
3
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: p63

Ex 7.7
Solution (continued) p63

p63

N
2
O
NO p64

Ex 2.8
Naming Type III Binary
Compounds
1.
Name each of the following compounds: a.
PCl
5
, b.
PCl
3
, c.
SO
2
2.
From the following systematic names, write the formula for each compound: a.
Sulfur hexafluoride, b.
Sulfur trioxide, c.
Carbon dioxide
P64

Solution: p64

Flowchart for Naming Binary Compounds p65
Figure 2.23

Figure 2.34
Overall Strategy for Naming
Chemical Compounds p65

Ex 2.9
Naming Various Types of
Compounds
1. Give the systematic name for each of the following compounds: a. P
4
O
10
, b. Nb
2
O
5
, c. Li
2
O
2
, d. Ti(NO
3
)
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
P65

Solution: p66

Ex 2.9
Solution (continued): p66

Figure 2.25
Flowchart for Naming Acids p67

p67

p67