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CH110CH110Chapter 4: Compounds & BondsChapter 4: Compounds & Bonds
Valence Electrons & eValence Electrons & e–– Dot Structures Dot Structures
Octet RuleOctet Rule & & IonsIons
Ionic CompoundsIonic Compounds
Covalent CompoundsCovalent Compounds
Molecular Shapes & Molecular Shapes & PolarityPolarity
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Electron arrangementElectron arrangement
2288
18183232
Electronsfill layers
around nucleusLow High
Electronsfill layers
around nucleusLow High
Shells = Energy levelsShells = Energy levels
2424
1212MgMg
A new layer isadded for each row or period in the table.
A new layer isadded for each row or period in the table.
2n2
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11
11HH
77
33LiLi
44
22HeHe
99
44BeBe 2020
1010NeNe
2323
1111NaNa
2424
1212MgMg4040
1818ArAr
88881111
2222
2, 12, 12, 12, 1 2, 22, 22, 22, 2 2, 82, 82, 82, 8
2, 8, 12, 8, 12, 8, 12, 8, 1 2, 8, 22, 8, 22, 8, 22, 8, 2 2, 8, 82, 8, 82, 8, 82, 8, 8
Octet RuleOctet Rule
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11
11HH
77
33LiLi
2323
1111NaNa
Lewis StructuresLewis Structures
Show only Valence
Electrons
H
Li
Na
K
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H
Li
Na
K
He
Be B C O F NeN
Mg
Ca
Al
Ga
Si
Ge
P
As
S
Se
Cl
Br
Ar
Kr
1
2 3 4 5 6 7
8
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2323
1111NaNaIonsIons
Metals give eMetals give e--s to make s to make Cations (+)Cations (+)
Na11 +’s11 +’s
11 -’s11 -’s
00
11 +’s11 +’s
11 -’s11 -’s
00
11 +’s11 +’s
10 -’s10 -’s
1 +1 +
11 +’s11 +’s
10 -’s10 -’s
1 +1 +
NaNa1+1+oror Na Na++
2, 8 = [Ne]2, 8 = [Ne]2, 8 = [Ne]2, 8 = [Ne]
2, 8, 1 2, 8, 1 2, 8, 1 2, 8, 1
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IonsIons
Nonmetals take eNonmetals take e--s to make s to make Anions (–)Anions (–)
17 +’s17 +’s
17 -’s17 -’s
00
17 +’s17 +’s
17 -’s17 -’s
00
17 +’s17 +’s
18 -’s18 -’s
1 -1 -
17 +’s17 +’s
18 -’s18 -’s
1 -1 -
Cl
Cl1-1-
3535
1717ClCl
= Cl= Cl1– 1–
2, 8, 8 = [Ar]2, 8, 8 = [Ar]2, 8, 8 = [Ar]2, 8, 8 = [Ar]
2, 8, 72, 8, 72, 8, 72, 8, 7
ClCl––
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Formation of NaClFormation of NaCl
Na + Cl Na+ + Cl
+ and - ions attract to form an ionic bond.
_
e– moves from Metal Nonmetal
Metal Cation
Nonmetal Anion
Stable octets
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Ionic compoundsIonic compounds
• Not individual molecules• Form crystal arrays• Ions touch many others • Formula represents the average ion ratio
NaNaClClsodiumsodium chloridechloride
NaNaClClsodiumsodium chloridechloride
Na
NaNa
Cl
Cl Cl
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Common ionsCommon ions
H
Li
Na
Cs
Rb
K
TlHgAuHfLsBa
Fr
PtIrOsReWTa
He
RnAtPoBiPb
Be
Mg
Sr
Ca
CdAgZrY PdRhRuTcMoNb
AcRa
ZnCuTiSc NiCoFeMnCrV
In XeITeSbSn
Ga KrBrSeAsGe
Al ArClSPSi
B NeFONC
Gd
Cm
Tb
Bk
Sm
Pu
Eu
Am
Nd
U
Pm
Np
Ce
Th
Pr
Pa
Yb
No
Lu
Lr
Er
Fm
Tm
Md
Dy
Cf
Ho
Es4 - 6
1+1+1+1+
2+2+2+2+ 3+3+3+3+
4+4+
4-4-
4+4+
4-4- 3-3-3-3- 2-2-2-2- 1-1-1-1-
Representative ElementsRepresentative ElementsRepresentative ElementsRepresentative Elements
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Ionic FormulasIonic FormulasMetal Cations Metal Cations ++ NonmetalNonmetal AnionsAnions
NaNa1+1+ ClCl1- 1-
NaNaClClSodiumSodium ChlorChlorideide
AlAl3+3+ ClCl1- 1-
AlAlClCl33Aluminum Aluminum ChlorChlorideide
ClCl1- 1-
ClCl1- 1-
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Common ionsCommon ions
H
Li
Na
Cs
Rb
K
TlBa
Fr
He
RnAtPoBiPb
Be
Mg
Sr
Ca
Ra
In XeITeSbSn
Ga KrBrSeAsGe
Al ArClSPSi
B NeFONC
HgAuHfLs PtIrOsReWTa
CdAgZrY PdRhRuTcMoNb
Ac
ZnCuTiSc NiCoFeMnCrV
Gd
Cm
Tb
Bk
Sm
Pu
Eu
Am
Nd
U
Pm
Np
Ce
Th
Pr
Pa
Yb
No
Lu
Lr
Er
Fm
Tm
Md
Dy
Cf
Ho
Es
1+1+1+1+
2+2+2+2+ 3+3+3+3+
4+4+
4-4-
4+4+
4-4- 3-3-3-3- 2-2-2-2- 1-1-1-1-
Transition ElementsTransition ElementsTransition ElementsTransition Elements
VariableVariableVariableVariable
Representative ElementsRepresentative ElementsRepresentative ElementsRepresentative Elements
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Information in the tableInformation in the table
Fe
55.845
Elemental Symbol
Electronic Configuration
Atomic mass (weight)26
Iron
2,3
[Ar]3d64s2
Atomic number
Name of the element
Possible ChargesPossible Charges (Valence)(Valence) Possible ChargesPossible Charges (Valence)(Valence)
No longer discussed in text
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Transition Metal IonsTransition Metal Ions
FeFe2+2+ ClCl1- 1-
FeFeClCl22
Iron(II)Iron(II) ChlorChlorideide
FeFe3+3+ ClCl1- 1-
FeFeClCl33
Iron(III) Iron(III) ChlorChlorideide
ClCl1- 1-
ClCl1- 1- ClCl1- 1-
FerrousFerrous ChlorChlorideide Ferric Ferric ChlorChlorideide
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Polyatomic IonsPolyatomic Ions
NaNa1+1+ SOSO442- 2-
NaNa22SOSO44
SodiumSodium SulfSulfateate
NHNH441+1+ POPO44
3- 3-
(NH(NH44))33POPO44
Ammonium Ammonium PhosphPhosphateate
NHNH441+1+
NHNH441+1+
NaNa1+1+
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Names and Formulas of Common Names and Formulas of Common Polyatomic IonsPolyatomic Ions
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Ionic compoundsIonic compounds
NaNa++
MgMg2+2+
AlAl3+3+
ClCl-- OO2-2- NN3-3-
Some simple ionsSome simple ions
NaClNaCl
Anions
Cat
ion
s
NaNa22OO NaNa33NN
MgClMgCl22
AlClAlCl33
MgOMgO
AlAl22OO33
MgMg33NN22
AlNAlN
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Ionic compoundsIonic compoundsC
atio
ns
Anions
NaNa1+1+
MgMg2+2+
AlAl3+3+
BrBr1-1- OO2-2- NN3-3-
NaBrNaBr NaNa22OO NaNa33NN
MgBrMgBr22
AlBrAlBr33
MgOMgO
AlAl22OO33
MgMg33NN22
AlNAlN
FeFe3+3+
CuCu1+1+
FeBrFeBr33 FeFe22OO33FeNFeN
CuBrCuBr CuCu22OO CuCu33NN
Sodium BromideSodium Bromide Sodium OxideSodium Oxide Sodium NitrideSodium Nitride
Magnesium BromideMagnesium Bromide
Aluminum BromideAluminum Bromide
Iron(III) BromideIron(III) BromideFerric BromideFerric Bromide
Copper(I) BromideCopper(I) BromideCuprous BromideCuprous Bromide
Magnesium OxideMagnesium Oxide
Aluminum OxideAluminum Oxide
Iron(III) OxideIron(III) OxideFerric OxideFerric Oxide
Copper(I) OxideCopper(I) OxideCuprous OxideCuprous Oxide
Magnesium NitrideMagnesium Nitride
Aluminum NitrideAluminum Nitride
Iron(III) NitrideIron(III) NitrideFerric NitrideFerric Nitride
Copper(I) NitrideCopper(I) NitrideCuprous NitrideCuprous Nitride
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Thanks to Christine Neighbors (Fall 2012)
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Covalent BondsCovalent Bonds
H H+ H H
Cl
O
+ Cl Cl
O +
+N N N N
OO
Cl
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Covalent BondsCovalent Bonds
H H
Cl Cl
N N
OO
H-H HH22 Cl-Cl ClCl22
O=O OO22
N N NN22
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Covalent compoundsCovalent compounds
•Discrete molecular units
•Atoms held together by bonds
•Covalent compounds exist in all states(CO2 - gas, H2O - liquid, SiO2 - solid)
•Formula represents atoms in a molecule
Covalent compoundsCovalent compounds
O=O O=O
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O C
OC
Covalent BondsCovalent Bonds
O=C=O
C O
O
COCOCarbon Carbon monmonoxideoxide
Carbon Carbon didioxideoxide COCO22
May modify rules to improve the sound. ExampleExample - use monoxide not monooxide.
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Naming Covalent CompoundsNaming Covalent Compounds
In the names of covalent compounds, prefixes are used to indicate the number of atoms (subscript) of each element. (mono is omitted for the first element, not the second)
Prefixes Used in Naming Covalent Compounds
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Rules for Naming Binary Compounds Containing Two Nonmetals
1. Write the name of the first nonmetal as it appears on the periodic table. Use a prefix if there is more than one atom.
2. Use a prefix to indicate the number of atoms for the second nonmetal.
3. Write the stem of the second nonmetal. 4. Add the suffix –ide.
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CO
CO2
Cl2O
N2O5
SiO2
ICl3
P2O5
CCl4
Naming covalent compoundsNaming covalent compounds
May modify rules to improve the sound. ExampleExample - use monoxide not monooxide.
carbon tetrachloride
diphosphorous pentoxide
iodine trichloride
silicon dioxide
carbon monoxide
carbon dioxide
dinitrogen pentoxidedichlorine monoxide
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Bond Polarity, ElectronegativityBond Polarity, Electronegativity
ClH
Electrons in covalent bonds rarely get shared equally.
H Cl
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ElectronegativityElectronegativityRelative ability of atoms to attract e-.
At
I
Br
Cl
Po
Te
Se
S
Bi
Sb
As
P
Pb
Sn
Ge
Si
FON
Tl
Na
Cs
Rb
K
Ba
Mg
Sr
Ca
In
Ga
Al
H
Li Be B C
ClH
1.0
0.8
0.9
1.5
1.2
0.7
1.0
2.0
1.5
0.8
1.0
0.9
1.6
1.7
1.8
2.5
1.8
1.8
1.8
1.9
3.0
2.1
2.0
1.9
1.9
3.5
2.5
2.4
2.1
2.0
4.0
3.0
2.8
2.5
2.1
2.1
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This unequal sharing results in polarpolar bonds.This unequal sharing results in polarpolar bonds.
H ClH Cl
•Slight positive side•Smaller electronegativity•Slight positive side•Smaller electronegativity
•Slight negative•Larger electronegativity•Slight negative•Larger electronegativity
++++ ––––
Bond Polarity, ElectronegativityBond Polarity, ElectronegativityClH
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Bond Polarity, ElectronegativityBond Polarity, Electronegativity
H Cl+ –
This unequal sharing results in polarpolar bonds.This unequal sharing results in polarpolar bonds.
•Slight positive side•Smaller electronegativity•Slight positive side•Smaller electronegativity
•Slight negative side•Larger electronegativity•Slight negative side•Larger electronegativity
ClH
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ClH
ClH2.12.1 3.03.0
––
Polar Covalent
++
Electronegativity Electronegativity DifferenceDifference
< 0.5< 0.5 Nonpolar Nonpolar
0.5-1.70.5-1.7 Polar Polar
>>1.81.8 Ionic Ionic
Bond Polarity, ElectronegativityBond Polarity, Electronegativity
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CO O
Polarity, ShapePolarity, Shape
3.53.5 3.53.52.52.5
O=C=O++ ––––
Polar Covalent Bonds
Linear Shape (180Linear Shape (180oo))Linear Shape (180Linear Shape (180oo))
Electronegativity Electronegativity DifferenceDifference
< 0.5< 0.5 Nonpolar Nonpolar
0.5-1.70.5-1.7 Polar Polar
>>1.81.8 Ionic Ionic
Nonpolar CompoundNonpolar Compound
COCO22
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Polar and Non-PolarPolar and Non-Polar
Thanks to Paula H. & Judy M. (Summer 1976)
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CH H
O
Polarity, ShapePolarity, Shape
O=C=O++ ––––
e–’s in 2 directions = 180o
LinearLinear
e–’s in 3 directions = 120o
++
–– Trigonal planarTrigonal planar
Nonpolar CompoundNonpolar Compound
Polar CompoundPolar Compound
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Polarity, ShapePolarity, Shape
CH HH
Cl
CH H
H
ClH
C
H
ClH
OH H
H-O-H
O
H
H
++
++––
++
––
e–’s in 4 directions = 109.5o
TetrahedralTetrahedral
BentBent
4 directions = 109.5o
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Polarity, ShapePolarity, Shape
NH HH ++
--e–’s in 4 directions = 109.5o
PyramidalPyramidal
NH H
HH
NHH++
++
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Some common geometriesSome common geometries e- directions arounde- directions aroundShape central atomShape central atom Example___ Example___ e- directions arounde- directions aroundShape central atomShape central atom Example___ Example___
Linear 2 O=C=O
Tetrahedral 4
HC
H
ClH
Trigonal Planar 3 C
H H
O
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O
H H HH
H H
H
H
H
CN
Tetrahedral electron-pair Geometries
TetrahedralTetrahedralPyramidalPyramidalBentBent
Methane, CH4
4 bond pairsAmmonia, NH3
3 bond pairsWater, H2O2 bond pairs
109.5º
107º
105º
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Molecular geometryMolecular geometry
Molecules have specific shapes.
•Determined by the number of electron pairs around the central atom
•Bonded and unbonded pairs
Geometry affects factors like polarity and solubility.
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Geometry Geometry and polar moleculesand polar molecules
For a molecule to be polarFor a molecule to be polar- must have polar bonds- must have the proper geometry
CH4 non-polarCH3Cl polarCH2Cl2 polarCHCl3 polarCCl4 non-polar
WHY?WHY?
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Polarity and solubilityPolarity and solubilitySolubilitySolubility The maximum amount of a solute
that dissolves in a given solvent
Depends on the forces of attraction between molecules - intermolecular
Types of intermolecular attractions most often encountered• Dipole-DipoleDipole-Dipole• Hydrogen bondingHydrogen bonding• Van der Wall forcesVan der Wall forces
General rule“Like dissolves likeLike dissolves like”
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Boiling and melting pointsBoiling and melting points
Chemical Bond Mp Bp N2 Nonpolar -210 -196 O2 Nonpolar -219 -183 NH3 Polar -78 -33 H2O Polar 0 100NaCl IonicIonic 804 ?
Melting and Boiling pointsMelting and Boiling points
•Very high for ionic compounds
•Typically lower for covalent compounds