chapter two - 國立臺北科技大學chpro/chem/chap2.pdf · three important laws (continued) law...
TRANSCRIPT
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Chapter Two:
ATOMS, MOLECULES, AND IONS
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2-1 The Early History of Chemistryp39
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2-2 Fundamental Chemical Lawsp41
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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
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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 MultipleProportions
P42
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 Theoryp43
Each element is made up of tiny particles called
atoms.
Dalton’s Atomic Theory (1808)
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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.
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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.
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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.
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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!
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p43Representing Gay-Lussac’s Results
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p45Representing Gay-Lussac’s Results
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2-4 Early Experiments toCharacterize the Atom
p45
The Electron
Figure 2.7 A Cathode-ray tube. The fast-moving electrons excite thegas in the tube, causing a glow between the electrodes. The green colorin the photo is due to the response of the screen (coated with zincsulfide) to the electron beam.
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p47
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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.
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Cathode Ray Tube
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p48
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Milliken Oil Drop Experiment
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2-5 The Modern View of AtomicStructure
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.
p49
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p49The Nuclear Atom
Radioactivity
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Rutherford’s Gold Foil Experiment
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Nuclear Atom Viewed in Cross Sectionp50
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Two Isotopes of Sodiump50
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Ex 2.2 Writing the Symbols for AtomsP52
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:
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2-6 Molecules and Ions p52
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p53
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Formation of Ionic Compounds
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p54
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p55
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Molecular vs. Ionic Compounds
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Covalent Bonding
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2-7 An Introduction to the PeriodicTable
p55
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The Periodic Tablep56
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2-8 Naming Simple Compoundsp57
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Binary Ionic Compounds (Type I)p58
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Naming Binary Ionic Compoundsp58
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Ex 2.3 Naming Type I Binary CompoundsP58
Name each binary compound.
a. CsF b. AlCl3 c. LiH
Solution
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P59
Ex 2.4 Formulas from Names forType I Binary Compounds
Given the following systematic names, write the formula
foe each compound:
a. Potassium iodide, b. Calcium oxide, c. Gallium bromide
Solution:
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Binary Ionic Compounds (Type II)
p59Formulas from Names
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Ex 2.5 Naming Type II Binary CompoundsP59
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: p60
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Ex 2.6 Naming Binary CompoundsP60
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:
p61
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p61
Figure 2.22 The common cations and anions
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p62
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Ex 2.7 Naming Compounds ContainingPolyatomic Ions
P62
1. Give the systematic name for each of the followingcompounds:
a. Na2SO4, b. KH2PO4, c. Fe(NO3)3,d. Mn(OH)2, e. Na2SO3, f. Na2CO3
2. Given the following systematic names, write the formulafor each compound:a. Sodium hydrogen carbonate,b. Cesium perchloratec. Sodium hypochlorited. Sodium selenatee. Potassium bromate
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Solution: p63
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Ex 7.7 Solution (continued)
p63
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Binary Covalent Compounds (Type III)p63
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p64
N2O
NO
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Ex 2.8 Naming Type III BinaryCompounds
P64
1. Name each of the following compounds:
a. PCl5, b. PCl3, c. SO2
2. From the following systematic names, write the formulafor each compound:
a. Sulfur hexafluoride, b. Sulfur trioxide,c. Carbon dioxide
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Solution:p64
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Flowchart for Naming Binary Compounds
Figure 2.23
p65
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Overall Strategy for NamingChemical Compounds
p65
Figure 2.34
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P65
Ex 2.9 Naming Various Types ofCompounds
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:
p66
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Ex 2.9 Solution (continued):p66
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Flowchart for Naming Acids
Figure 2.25
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