Chapter 2: Atomic Structure & Interatomic Bonding 1.
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Transcript of Chapter 2: Atomic Structure & Interatomic Bonding 1.
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Chapter 2: Atomic Chapter 2: Atomic Structure & Interatomic Structure & Interatomic
BondingBonding
1
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Lesson Learning Outcomes (LLO’s)Lesson Learning Outcomes (LLO’s)Upon completion of this topic, student should be able to1. Name/ tell the two atomic models cited and note the
differences between them C12. Describe the important quantum –mechanical principle
that relates to electron energies C13. a) Schematically plot attractive, repulsive, and net
energies versus interatomic separation for two atomic atoms or ions (C4)
b) note on this plot the equilibrium separation and the bonding energy
4. a) Briefly describe ionic, covalent, metallic, hydrogen, and van der waals bonds
b) note which materials exhibit each of these bonding types
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ISSUES TO ADDRESS...
• What promotes bonding?
• What types of bonds are there?
• What properties are inferred from bonding?
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Atomic Structure (Freshman Chem.)Atomic Structure (Freshman Chem.)atom – electrons – 9.11 x 10-31 kg
protons neutrons
atomic number = # of protons in nucleus of atom = # of electrons of neutral
species A [=] atomic mass unit = amu = 1/12 mass of 12C
Atomic wt = wt of 6.022 x 1023 molecules or atoms
1 amu/atom = 1g/mol
C 12.011H 1.008 etc.
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} 1.67 x 10-27 kg
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Atomic StructureAtomic Structure Valence electrons determine all of the
following properties1) Chemical2) Electrical 3) Thermal4) Optical
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Electronic StructureElectronic Structure
Electrons have wavelike and particulate properties. ◦This means that electrons are in orbitals
defined by a probability.◦Each orbital at discrete energy level is
determined by quantum numbers. Quantum # Designation
n = principal (energy level-shell) K, L, M, N, O (1, 2, 3, etc.)
l = subsidiary (orbitals) s, p, d, f (0, 1, 2, 3,…, n -1)
ml = magnetic 1, 3, 5, 7 (-l to +l)
ms = spin ½, -½
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Electron Energy StatesElectron Energy States
71s
2s2p
K-shell n = 1
L-shell n = 2
3s3p M-shell n = 3
3d
4s
4p4d
Energy
N-shell n = 4
• have discrete energy states• tend to occupy lowest available energy state.
Electrons...
Adapted from Fig. 2.4, Callister & Rethwisch 8e.
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SURVEY OF ELEMENTSSURVEY OF ELEMENTS
• Why? Valence (outer) shell usually not filled completely.
• Most elements: Electron configuration not stable.Electron configuration
(stable)
...
...
1s22s 22p 63s23p 6 (stable)... 1s22s 22p 63s23p 63d 10 4s 24p 6 (stable)
Atomic #
18...36
Element1s1 1Hydrogen1s22Helium1s22s 1 3Lithium1s22s24Beryllium1s22s 22p 15Boron1s22s 22p 26Carbon
...
1s22s 22p 6 (stable)10Neon1s22s 22p 63s111Sodium1s22s 22p 63s2 12Magnesium1s22s 22p 63s23p 113Aluminum
...
Argon...Krypton
Adapted from Table 2.2, Callister & Rethwisch 8e.
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Electron ConfigurationsElectron ConfigurationsValence electrons – those in unfilled
shellsFilled shells more stableValence electrons are most available for
bonding and tend to control the chemical properties
◦example: C (atomic number = 6)
1s2 2s2 2p2
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valence electrons
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Electronic ConfigurationsElectronic Configurationsex: Fe - atomic # =
10
26
valence electrons
Adapted from Fig. 2.4, Callister & Rethwisch 8e.
1s
2s2p
K-shell n = 1
L-shell n = 2
3s3p M-shell n = 3
3d
4s
4p4d
Energy
N-shell n = 4
1s2 2s2 2p6 3s2 3p6 3d 6 4s2
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The Periodic TableThe Periodic Table
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• Columns: Similar Valence Structure
Adapted from Fig. 2.6, Callister & Rethwisch 8e.
Electropositive elements:Readily give up electronsto become + ions.
Electronegative elements:Readily acquire electronsto become - ions.
giv
e u
p 1
e-
giv
e u
p 2
e-
giv
e u
p 3
e- ine
rt g
ase
s
acc
ept
1e
-
acc
ept
2e
-
O
Se
Te
Po At
I
Br
He
Ne
Ar
Kr
Xe
Rn
F
ClS
Li Be
H
Na Mg
BaCs
RaFr
CaK Sc
SrRb Y
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ElectronegativityElectronegativity
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• Ranges from 0.7 to 4.0,
Smaller electronegativity Larger electronegativity
• Large values: tendency to acquire electrons.
Adapted from Fig. 2.7, Callister & Rethwisch 8e. (Fig. 2.7 is adapted from Linus Pauling, The Nature of the Chemical Bond, 3rd edition, Copyright 1939 and 1940, 3rd edition. Copyright 1960 by Cornell University.
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Ionic bond – Ionic bond – metalmetal + nonmetal + nonmetal
donates accepts electrons electrons
Dissimilar electronegativities
ex: MgO Mg 1s2 2s2 2p6 3s2 O 1s2 2s2 2p4
[Ne] 3s2
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Mg2+ 1s2 2s2 2p6 O2- 1s2 2s2 2p6 [Ne] [Ne]
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Ionic BondingIonic Bonding• Occurs between + and - ions.
• Requires electron transfer.
• Large difference in electronegativity required.
• Example: NaCl
Na (metal) unstable
Cl (nonmetal) unstable
electron
+ - Coulombic Attraction
Na (cation) stable
Cl (anion) stable
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Ionic BondingIonic Bonding
Energy – minimum energy most stable◦Energy balance of attractive and repulsive
terms
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Attractive energy EA
Net energy EN
Repulsive energy ER
Interatomic separation r
rA
nrBEN = EA + ER =
Adapted from Fig. 2.8(b), Callister & Rethwisch 8e.
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Examples: Ionic BondingExamples: Ionic Bonding• Predominant bonding in Ceramics
Adapted from Fig. 2.7, Callister & Rethwisch 8e. (Fig. 2.7 is adapted from Linus Pauling, The Nature of the Chemical Bond, 3rd edition, Copyright 1939 and 1940, 3rd edition. Copyright 1960 by Cornell University.
Give up electrons Acquire electrons
NaCl
MgO
CaF2CsCl
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Covalent BondingCovalent Bonding
C: has 4 valence e-, needs 4 more
H: has 1 valence e-, needs 1 more
Electronegativities are comparable.
Adapted from Fig. 2.10, Callister & Rethwisch 8e.
• similar electronegativity share electrons• bonds determined by valence – s & p orbitals
dominate bonding
• Example: CH4shared electrons from carbon atom
shared electrons from hydrogen atoms
H
H
H
H
C
CH4
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Primary BondingPrimary BondingMetallic Bond -- delocalized as electron cloud
Ionic-Covalent Mixed Bonding
% ionic character =
where XA & XB are Pauling electronegativities
18
%)100( x
1 e
(XA XB )2
4
ionic 73.4% (100%) x e1 characterionic % 4)2.15.3(
2
Ex: MgO XMg = 1.2XO = 3.5
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SECONDARY BONDINGSECONDARY BONDINGArises from interaction between dipoles
• Permanent dipoles-molecule induced
• Fluctuating dipoles
-general case:
-ex: liquid HCl
-ex: polymer
Adapted from Fig. 2.13, Callister & Rethwisch 8e.
Adapted from Fig. 2.15, Callister & Rethwisch 8e.
asymmetric electron clouds
+ - + -secondary
bonding
HH HH
H2 H2
secondary bonding
ex: liquid H2
H Cl H Clsecondary bonding
secondary bonding+ - + -
secondary bondingsecondary bonding
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Summary: BondingSummary: BondingType
Ionic
Covalent
Metallic
Secondary
Bond Energy
Large!
Variablelarge-Diamondsmall-Bismuth
Variablelarge-Tungstensmall-Mercury
smallest
Comments
Nondirectional (ceramics)
Directional(semiconductors, ceramicspolymer chains)
Nondirectional (metals)
Directionalinter-chain (polymer)inter-molecular
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Properties From Bonding: Properties From Bonding: TTmm
• Bond length, r
• Bond energy, Eo
• Melting Temperature, Tm
Tm is larger if Eo is larger.
r o r
Energyr
larger Tm
smaller Tm
Eo =
“bond energy”
Energy
r o r
unstretched length
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Properties From Bonding : Properties From Bonding : • Coefficient of thermal expansion,
• ~ symmetric at ro
is larger if Eo is smaller.
= (T2 -T1)LLo
coeff. thermal expansion
L
length, Lo
unheated, T1
heated, T2
r or
smaller
larger
Energy
unstretched length
Eo
Eo
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Summary: Primary BondsSummary: Primary Bonds
Ceramics(Ionic & covalent bonding):
Large bond energylarge Tm
large Esmall
Metals(Metallic bonding):
Variable bond energymoderate Tm
moderate Emoderate
Polymers(Covalent & Secondary):
Directional PropertiesSecondary bonding dominates
small Tm
small E large
secondary bonding
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ANNOUNCEMENTSANNOUNCEMENTSReading:
Core Problems:
Self-help Problems: