chapter 2 atoms, molecules, and ions. the early history of chemistry -before 16th century alchemy:...
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Chapter 2Chapter 2
Atoms, Molecules, and IonsAtoms, Molecules, and Ions
The Early History of ChemistryThe Early History of Chemistry
- Before 16th CenturyBefore 16th CenturyAlchemyAlchemy: Attempts (scientific or otherwise) to : Attempts (scientific or otherwise) to change cheap metals into goldchange cheap metals into gold
- 17th Century17th CenturyRobert BoyleRobert Boyle: First “chemist” to perform : First “chemist” to perform quantitative experimentsquantitative experiments
- 18th Century18th CenturyGeorge StahlGeorge Stahl: : PhlogistonPhlogiston flows out of a burning flows out of a burning material.material.Joseph PriestleyJoseph Priestley: Discovers oxygen gas, : Discovers oxygen gas, “dephlogisticated air.”“dephlogisticated air.”
Law of Conservation of MassLaw of Conservation of Mass
- Discovered by Antoine LavoisierDiscovered by Antoine Lavoisier
- Mass is neither created nor destroyedMass is neither created nor destroyed
- Combustion involves oxygen, not Combustion involves oxygen, not phlogistonphlogiston
Other Fundamental Chemical LawsOther Fundamental Chemical Laws
- A given compound always contains exactly A given compound always contains exactly the same proportion of elements by mass.the same proportion of elements by mass.
- Carbon tetrachloride is always 1 atom Carbon tetrachloride is always 1 atom carbon per 4 atoms chlorine.carbon per 4 atoms chlorine.
Law of Definite Proportion
Other Fundamental Chemical LawsOther Fundamental Chemical Laws
- When two elements form a series of compounds, When two elements form a series of compounds, the ratios of the masses of the second element the ratios of the masses of the second element that combine with 1 gram of the first element that combine with 1 gram of the first element can always be reduced to small whole numbers.can always be reduced to small whole numbers.
- The ratio of the masses of oxygen in HThe ratio of the masses of oxygen in H22O and O and
HH22OO22 will be a small whole number (“2”). will be a small whole number (“2”).
Law of Multiple Proportions
Dalton’s Atomic Theory (1808)Dalton’s Atomic Theory (1808)
1 Each element is made up of tiny particles Each element is made up of tiny particles called atoms.called atoms.
2 The atoms of a given element are The atoms of a given element are identicalidentical; the atoms of different elements ; the atoms of different elements are different in some fundamental way or are different in some fundamental way or ways.ways.
Dalton’s Atomic Theory(continued)
Dalton’s Atomic Theory(continued)
3 Chemical compounds are formed when Chemical compounds are formed when atoms combine with each otheratoms combine with each other. . A given A given compound always has the same relative compound always has the same relative numbers and types of atoms.numbers and types of atoms.
4 Chemical reactions involve reorganization Chemical reactions involve reorganization of the atomsof the atoms - changes in the way they are - changes in the way they are bound together. The atoms themselves are bound together. The atoms themselves are not changed in a chemical reaction.not changed in a chemical reaction.
Atomic TheoryAtomic Theory
Alpha, Beta, and GammaAlpha, Beta, and Gamma
Movie
Early Experiments to Characterize the AtomEarly Experiments to
Characterize the Atom
- J. J. Thomson J. J. Thomson - postulated the existence of - postulated the existence of electronselectrons using using cathode ray tubescathode ray tubes..
- Ernest RutherfordErnest Rutherford - explained the - explained the nuclear nuclear atomatom, containing a dense nucleus with , containing a dense nucleus with electrons traveling around the nucleus at a electrons traveling around the nucleus at a large distance.large distance.
J. J. Thompson ExperimentJ. J. Thompson Experiment02_21
Metalelectrode
Metalelectrode
(-)
(+)
(+)
(-)
Appliedelectric field
Millikan Oil Drop ExperimentMillikan Oil Drop Experiment
Movie
Plum Pudding ModelPlum Pudding Model
Rutherford ExperimentRutherford Experiment
Movie
02_25
Electrons scatteredthroughout Diffuse
positivecharge
(a) (b)
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--
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-
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--
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-
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--
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--
--
n+
The Modern View of Atomic Structure
The Modern View of Atomic Structure
- electronselectrons
- protonsprotons: found in the nucleus, they have a : found in the nucleus, they have a positive charge equal in magnitude to the positive charge equal in magnitude to the electron’s negative charge.electron’s negative charge.
- neutronsneutrons: found in the nucleus, virtually : found in the nucleus, virtually same mass as a proton but no charge.same mass as a proton but no charge.
The The atomatom contains: contains:
The Mass and Change of the Electron, Proton, and NeutronThe Mass and Change of the Electron, Proton, and Neutron
Particle Mass (kg) Charge
Electron 9.11 10 31 1
Proton 1.67 10 27 1+
Neutron 1.67 10 27 0
The Chemists’ Shorthand: Atomic Symbols
The Chemists’ Shorthand: Atomic Symbols
K Element Symbol39
19
Mass number
Atomic number
IsotopesIsotopes
Periodic TablePeriodic TableElements classified by:Elements classified by: --propertiesproperties -- atomic numberatomic number
GroupsGroups (vertical) (vertical) 1A = alkali metals1A = alkali metals 2A = alkaline earth metals2A = alkaline earth metals 7A = halogens7A = halogens 8A = noble gases8A = noble gases
PeriodsPeriods (horizontal) (horizontal)
02_29
1H
3Li
11Na
19K
37Rb
55Cs
87Fr
4Be
12Mg
20Ca
38Sr
56Ba
88Ra
21Sc
39Y
57La*
89Ac†
22Ti
40Zr
72Hf
104Unq
23V
41Nb
73Ta
105Unp
24Cr
42Mo
74W
106Unh
25Mn
43Tc
75Re
107Uns
26Fe
44Ru
76Os
108Uno
27Co
45Rh
77Ir
109Une
110Uun
111Uuu
28Ni
46Pd
78Pt
29Cu
47Ag
79Au
30Zn
3 4 5 6 7 8 9 10 11 12
48Cd
80Hg
31Ga
49In
81Tl
5B
13Al
32Ge
50Sn
82Pb
6C
14Si
33As
51Sb
83Bi
7N
15P
34Se
52Te
84Po
8O
16S
9F
17Cl
35Br
53I
85At
10Ne
18Ar
36Kr
54Xe
86Rn
2He
58Ce
90Th
59Pr
91Pa
60Nd
92U
61Pm
93Np
62Sm
94Pu
63Eu
95Am
64Gd
96Cm
65Tb
97Bk
66Dy
98Cf
67Ho
99Es
68Er
100Fm
69Tm
101Md
70Yb
102No
71Lu
103Lr
1A
2A
Transition metals
3A 4A 5A 6A 7A
8A1
2 13 14 15 16 17
18
Alk
ali m
eta
lsAlkalineearth metals Halogens
Noblegases
*Lanthanides
† Actinides
Fill in the TableFill in the Table
Chemical BondsChemical Bonds
The forces that hold atoms together in The forces that hold atoms together in compounds. compounds. Covalent bonds Covalent bonds result from atoms result from atoms sharing electronssharing electrons..
MoleculeMolecule: a collection of covalently-bonded : a collection of covalently-bonded atoms.atoms.
Methane
The Chemists’ Shorthand:Formulas
The Chemists’ Shorthand:Formulas
Chemical Formula:Chemical Formula:
SymbolsSymbols = types of atoms = types of atoms
SubscriptsSubscripts = relative numbers of atoms = relative numbers of atoms
COCO22
Structural Formula:Structural Formula:
Individual bonds are shown Individual bonds are shown by linesby lines..
OO==CC==OO
IonsIons
CationCation: A positive ion: A positive ion
MgMg2+2+, NH, NH44++
AnionAnion: A negative ion: A negative ion
ClCl, SO, SO4422
Ionic BondingIonic Bonding: Force of attraction between : Force of attraction between oppositely charged ions.oppositely charged ions.
Naming CompoundsNaming Compounds
1. Cation first, then anion1. Cation first, then anion
2. Monatomic cation = name of the element2. Monatomic cation = name of the element
CaCa2+2+ = = calciumcalcium ionion
3. Monatomic anion = 3. Monatomic anion = rootroot + + -ide-ide
ClCl = = chlorchlorideide
CaClCaCl22 = = calcium chlorcalcium chlorideide
Binary Ionic Binary Ionic Compounds:Compounds:
Type I – Binary Ionic CmpdsType I – Binary Ionic Cmpds
Name the FollowingName the Following
KIKI
MgBrMgBr22
SrOSrO
Write the Symbols for Write the Symbols for the Followingthe Following
Lithium ChlorideLithium Chloride
Barium FluorideBarium Fluoride
Magnesium OxideMagnesium Oxide
Naming Compounds(continued)
Naming Compounds(continued)
-- metal forms more than one metal forms more than one cationcation
-- use use Roman numeral Roman numeral in namein name
PbClPbCl22
PbPb2+2+ is cationis cation
PbClPbCl22 = lead ( = lead (IIII) chloride) chloride
Binary Ionic Compounds (Type Binary Ionic Compounds (Type II):II):
Type II – Binary Ionic CmpdsType II – Binary Ionic Cmpds
Name the following-Name the following-
CuOCuO
FeFe22OO33
CuFCuF
Write the Formula for Write the Formula for the following-the following-
Iron(III) SulfateIron(III) Sulfate
Zinc OxideZinc Oxide
Naming Compounds(continued)
Naming Compounds(continued)
-- Compounds between two Compounds between two nonmetalsnonmetals-- First element First element in the formula is in the formula is named firstnamed first..-- Second element Second element is named as if it were an is named as if it were an anionanion..-- Use prefixesUse prefixes-- Never use Never use mono-mono-
PP22OO55 = = didiphosphorus phosphorus pentpentoxideoxide
Binary compounds (Type III):Binary compounds (Type III):
AlkanesAlkanes
02_31Binary compound?
Yes
Metal present?
No Yes
Type III:Use prefixes.
Does the metal formmore than one cation?
No Yes
Type I:Use the elementname for the cation.
Type II:Determine the charge of the cation;use a Roman numeral after theelement name for the cation.
02_33
Does the anioncontain oxygen?
No Yes
hydro -+ anion root+ -ichydro (anion root)ic acid
Check the ending of the anion.
-ate
anion or element root+ -ous(root)ous acid
-ite
anion or element root+ -ic(root)ic acid
EndEnd