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Ch02 121227103353-phpapp02
1.
Prentice-Hall ©General Chemistry:Slide
1 of 25 Chapter 2: Atoms and the Atomic Theory Philip Dutton University of Windsor, Canada Prentice-Hall © 2002 General Chemistry Principles and Modern Applications Petrucci • Harwood • Herring 8th Edition
2.
Prentice-Hall ©General Chemistry:Slide
2 of 25 Contents • Early chemical discoveries • Electrons and the Nuclear Atom • Chemical Elements • Atomic Masses • The Mole
3.
Prentice-Hall ©General Chemistry:Slide
3 of 25 Early Discoveries Lavoisier 1774 Law of conservation of mass Proust 1799 Law of constant composition Dalton 1803-1888 Atomic Theory
4.
Prentice-Hall ©General Chemistry:Slide
4 of 25 Dalton’s Atomic Theory Each element is composed of small particles called atoms. Atoms are neither created nor destroyed in chemical reactions. All atoms of a given element are identical Compounds are formed when atoms of more than one element combine
5.
Prentice-Hall ©General Chemistry:Slide
5 of 25 Consequences of Dalton’s theory In forming carbon monoxide, 1.33 g of oxygen combines with 1.0 g of carbon. In the formation of hydrogen peroxide 2.66 g of oxygen combines with 1.0 g of hydrogen. Law of Definite Proportions: combinations of elements are in ratios of small whole numbers.
6.
Prentice-Hall ©General Chemistry:Slide
6 of 25 Behavior of charges
7.
Prentice-Hall ©General Chemistry:Slide
7 of 25 Cathode ray tube
8.
Prentice-Hall ©General Chemistry:Slide
8 of 25 Properties of cathode rays Electron m/e = -5.6857 x 10-9 g coulomb-1
9.
Prentice-Hall ©General Chemistry:Slide
9 of 25 Charge on the electron From 1906-1914 Robert Millikan showed ionized oil drops can be balanced against the pull of gravity by an electric field. The charge is an integral multiple of the electronic charge, e.
10.
Prentice-Hall ©General Chemistry:Slide
10 of 25 Radioactivity Radioactivity is the spontaneous emission of radiation from a substance. X-rays and γ-rays are high-energy light. α-particles are a stream of helium nuclei, He2+. β-particles are a stream of high speed electrons that originate in the nucleus.
11.
Prentice-Hall ©General Chemistry:Slide
11 of 25 The nuclear atom Geiger and Rutherford 1909
12.
Prentice-Hall ©General Chemistry:Slide
12 of 25 The α-particle experiment Most of the mass and all of the positive charge is concentrated in a small region called the nucleus . There are as many electrons outside the nucleus as there are units of positive charge on the nucleus
13.
Prentice-Hall ©General Chemistry:Slide
13 of 25 The nuclear atom Rutherford protons 1919 James Chadwick neutrons 1932
14.
Prentice-Hall ©General Chemistry:Slide
14 of 25 Atomic Diameter 10-8 cm Nuclear diameter 10-13 cm Nuclear Structure Particle Mass Charge kg amu Coulombs (e) Electron 9.109 x 10-31 0.000548 –1.602 x 10-19 –1 Proton 1.673 x 10-27 1.00073 +1.602 x 10-19 +1 Neutron 1.675 x 10-27 1.00087 0 0 1 Å
15.
Prentice-Hall ©General Chemistry:Slide
15 of 25 Scale of Atoms Useful units: 1 amu (atomic mass unit) = 1.66054 x 10-24 kg 1 pm (picometer) = 1 x 10-12 m 1 Å (Angstrom) = 1 x 10-10 m = 100 pm = 1 x 10-8 cm The heaviest atom has a mass of only 4.8 x 10-22 g and a diameter of only 5 x 10-10 m. Biggest atom is 240 amu and is 50 Å across. Typical C-C bond length 154 pm (1.54 Å) Molecular models are 1 Å /inch or about 0.4 Å /cm
16.
Prentice-Hall ©General Chemistry:Slide
16 of 25 Isotopes, atomic numbers and mass numbers To represent a particular atom we use the symbolism: A= mass number Z = atomic number
17.
Prentice-Hall ©General Chemistry:Slide
17 of 25 Measuring atomic masses
18.
Prentice-Hall ©General Chemistry:Slide
18 of 25 The Periodic tableAlkali Metals Alkaline Earths Transition Metals Halogens Noble Gases Lanthanides and Actinides Main Group Main Group
19.
Prentice-Hall ©General Chemistry:Slide
19 of 25 The Periodic Table • Read atomic masses. • Read the ions formed by main group elements. • Read the electron configuration. • Learn trends in physical and chemical properties. We will discuss these in detail in Chapter 10.
20.
Prentice-Hall ©General Chemistry:Slide
20 of 25 The Mole • Physically counting atoms is impossible. • We must be able to relate measured mass to numbers of atoms. – buying nails by the pound. – using atoms by the gram
21.
Prentice-Hall ©General Chemistry:Slide
21 of 25 Avogadro’s number The mole is an amount of substance that contains the same number of elementary entities as there are carbon-12 atoms in exactly 12 g of carbon-12. NA = 6.02214199 x 1023 mol-1
22.
Prentice-Hall ©General Chemistry:Slide
22 of 25 Molar Mass • The molar mass, M, is the mass of one mole of a substance. M(g/mol 12 C) = A(g/atom 12 C) x NA (atoms 12 C /mol 12 C)
23.
Prentice-Hall ©General Chemistry:Slide
23 of 25 Combining Several Factors in a Calculation—Molar Mass, the Avogadro Constant, Percent Abundance. Potassium-40 is one of the few naturally occurring radioactive isotopes of elements of low atomic number. Its percent natural abundance among K isotopes is 0.012%. How many 40K atoms do you ingest by drinking one cup of whole milk containing 371 mg of K? Want atoms of 40 K, need atoms of K, Want atoms of K, need moles of K, Want moles of K, need mass and M(K). Example 2-9
24.
Prentice-Hall ©General Chemistry:Slide
24 of 25 Convert strategy to plan mK(mg) x (1g/1000mg) mK (g) x 1/MK (mol/g) nK(mol) Convert mass of K(mg K) into moles of K (mol K) Convert moles of K into atoms of 40 K nK(mol) x NA atoms K x 0.012% atoms 40 K nK = (371 mg K) x (10-3 g/mg) x (1 mol K) / (39.10 g K) = 9.49 x 10-3 mol K and plan into action atoms 40 K = (9.49 x 10-3 mol K) x (6.022 x 1023 atoms K/mol K) x (1.2 x 10-4 40 K/K) = 6.9 x 1017 40 K atoms
25.
Prentice-Hall ©General Chemistry:Slide
25 of 25 Chapter 2 Questions 3, 4, 11, 22, 33, 51, 55, 63, 83.
Editor's Notes
Often do not specify Z when writing. For example 14C, C specifies Z = 12. Special names for some isotopes. For example hydrogen, deuterium, tritium.
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