p38 Chapter Two: ATOMS, MOLECULES, AND IONS
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1 p38 Chapter Two: ATOMS, MOLECULES, AND IONS
2 2-1 The Early History of Chemistry p39
3 2-2 Fundamental Chemical Laws p41
4
5 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
6 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.
7 Ex 2.1 Illustrating the Law of Multiple Proportions The following data were collected for several compounds of nitrogen and oxygen: P42 Sow how these data illustrate the law of multiple proportions. Solution:
8 2-3 Dalton s Atomic Theory p43 Dalton s Atomic Theory (1808) Each element is made up of tiny particles called atoms.
9 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.
10 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.
11 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.
12 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!
13 Representing Gay-Lussac s Results p43
14 Representing Gay-Lussac s Results p45
15 2-4 Early Experiments to Characterize the Atom 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.
16 p47
17 p47
18 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.
19 Cathode Ray Tube
20 p48
21 Milliken Oil Drop Experiment
22 2-5 The Modern View of Atomic Structure p49 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.
23 The Nuclear Atom p49 Radioactivity
24 Rutherford s Gold Foil Experiment
25
26 Nuclear Atom Viewed in Cross Section p50
27 Two Isotopes of Sodium p50
28 Ex 2.2 Writing the Symbols for Atoms 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: P52
29 2-6 Molecules and Ions p52
30 p53
31 Formation of Ionic Compounds
32 p54
33 p55
34 Molecular vs. Ionic Compounds
35 Covalent Bonding
36 2-7 An Introduction to the Periodic Table p55
37 The Periodic Table p56
38 2-8 Naming Simple Compounds p57
39 Binary Ionic Compounds (Type I) p58
40 Naming Binary Ionic Compounds p58
41 Ex 2.3 Naming Type I Binary Compounds Name each binary compound. P58 a. CsF b. AlCl 3 c. LiH Solution
42 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:
43 Formulas from Names p59 Binary Ionic Compounds (Type II)
44 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
45 Solution: p60
46 Ex 2.6 Naming Binary Compounds P60 1. Give the systematic name for each of the following compounds: 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
47 S0lution: p61
48 Figure 2.22 The common cations and anions p61
49 p62
50 Ex 2.7 Naming Compounds Containing Polyatomic Ions 1. Give the systematic name for each of the following compounds: P62 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
51 Solution: p63
52 Ex 7.7 Solution (continued) p63
53 Binary Covalent Compounds (Type III) p63
54 p64 N 2 O NO
55 Ex 2.8 Naming Type III Binary Compounds P64 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
56 Solution: p64
57 Flowchart for Naming Binary Compounds p65 Figure 2.23
58 Overall Strategy for Naming Chemical Compounds p65 Figure 2.34
59 Ex 2.9 Naming Various Types of Compounds 1. Give the systematic name for each of the following compounds: P65 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
60 Solution: p66
61 Ex 2.9 Solution (continued): p66
62 Flowchart for Naming Acids p67 Figure 2.25
63 p67
64 p67
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