4 - 1CH 104 Chapter 4
CH04Chapter 5: Compounds & Bonds
Valence Electrons & e- Dot Structures
Octet Rule & Ions
Ionic Compounds & Formulas
Covalent Compounds & Formulas
Polyatomic Ions
Molecular Shapes & Polarity
Attractive Forces
4 - 2CH 104 Chapter 4
Electron arrangement
28
1832
Electrons
fill layers
around nucleus
Low High
Shells = Energy levels
2412Mg
4 - 3CH 104 Chapter 4
Inner vs. valence electrons
Valence electronsThis is wheremost chemicalreactionsoccur.
Inner electronsNot much happenshere under normalconditions.
4 - 4CH 104 Chapter 4
11H
73Li
42He
94Be
2010Ne
2311Na
2412Mg
4018Ar
Octet Rule
4 - 5CH 104 Chapter 4
11H
73Li
42He
94Be
2010Ne
2311Na
2412Mg
4018Ar
Octet Rule
1s2, 2s11s2, 2s1 1s2, 2s21s2, 2s2
1s11s1 1s21s2
1s2, 2s2 2p61s2, 2s2 2p6
1s2, 2s2 2p6, 3s11s2, 2s2 2p6, 3s1
1s2, 2s2 2p6, 3s21s2, 2s2 2p6, 3s2[Ne] 3s1[Ne] 3s1
1s2, 2s2 2p6, 3s2 3p61s2, 2s2 2p6, 3s2 3p6
4 - 6CH 104 Chapter 4
11H
73Li
2311Na
Lewis Structures
Show only Valence
Electrons
H
Li
Na
K
4 - 7CH 104 Chapter 4
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
4 - 8CH 104 Chapter 4
2311Na
Ions
Metals give e-s to make Cations
Na11 +’s11 -’s 0
11 +’s11 -’s 0
11 +’s10 -’s 1 +
11 +’s10 -’s 1 +
Na1+
2, 8 = [Ne]2, 8 = [Ne]
4 - 9CH 104 Chapter 4
Ions
Nonmetals take e-s to make Anions
17 +’s
17 -’s
0
17 +’s
17 -’s
0
17 +’s
18 -’s
1 -
17 +’s
18 -’s
1 -
Cl
Cl1-
3517Cl
= Cl1-
2, 8, 8 = [Ar]2, 8, 8 = [Ar]
4 - 10CH 104 Chapter 4
Formation 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
4 - 11CH 104 Chapter 4
Ionic compounds
• Not individual molecules• Form crystal arrays• Ions touch many others • Formula represents the average ion ratio
NaClsodium chloride
NaClsodium chloride
Na
NaNa
Cl
Cl Cl
Common 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+
2+2+ 3+3+
4+
4-
4+
4- 3-3- 2-2- 1-1-
Representative ElementsRepresentative Elements
4 - 13CH 104 Chapter 4
Ionic FormulasMetal Cations + Nonmetal Anions
Na1+ Cl1-
NaClSodium Chloride
Al3+ Cl1-
AlCl3Aluminum Chloride
Cl1-
Cl1-
4 - 14CH 104 Chapter 4
Common 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+
2+2+ 3+3+
4+
4-
4+
4- 3-3- 2-2- 1-1-
Transition ElementsTransition Elements
VariableVariable
Representative ElementsRepresentative Elements
4 - 15CH 104 Chapter 4
Information 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
Oxidation states (Valence)Oxidation states (Valence)
4 - 16CH 104 Chapter 4
Transition Metal Ions
Fe2+ Cl1-
FeCl2
Iron (II) Chloride
Fe3+ Cl1-
FeCl3
Iron (III) Chloride
Cl1-
Cl1- Cl1-
Ferrous Chloride Ferric Chloride
4 - 17CH 104 Chapter 4
Ionic compoundsC
atio
ns
Anions
Na1+
Mg2+
Al3+
Br1- O2- N3-
NaBr Na2O Na3N
MgBr2
AlBr3
MgO
Al2O3
Mg3N2
AlN
Fe3+
Cu1+
FeBr3 Fe2O3FeN
CuBr Cu2O Cu3N
Sodium Bromide Sodium Oxide Sodium Nitride
Magnesium Bromide
Aluminum Bromide
Iron (III) BromideFerric Bromide
Copper (I) BromideCuprous Bromide
Magnesium Oxide
Aluminum Oxide
Iron (III) OxideFerric Oxide
Copper (I) OxideCuprous Oxide
Magnesium Nitride
Aluminum Nitride
Iron (III) NitrideFerric Nitride
Copper (I) NitrideCuprous Nitride
4 - 18CH 104 Chapter 4
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
Metals give e-s to nonmetalsMetals give e-s to nonmetals
Nonmetals Share e-s
with other nonmetals
Nonmetals Share e-s
with other nonmetals
4 - 19CH 104 Chapter 4
Covalent Bonds
H H+ H H
Cl
O
+ Cl Cl
O +
+N N N N
OO
Cl
4 - 20CH 104 Chapter 4
Covalent Bonds
H H
Cl Cl
N N
OO
H-H H2 Cl-Cl Cl2
O=O O2
N N N2
4 - 21CH 104 Chapter 4
O C
OC
Covalent Bonds
O=C=O
C O
O
COCarbon monoxide
Carbon dioxide CO2
May modify rules to improve sound. ie - monoxide not monooxide.
4 - 22CH 104 Chapter 4
CO
CO2
N2O5
SiO2
ICl3
P2O5
CCl4
Naming covalent compounds
May modify rules to improve the sound. Example - use monoxide not monooxide.
carbon tetrachloride
diphophorous pentoxide
iodine trichloride
silicon dioxide
carbon monoxidecarbon dioxide
dinitrogen pentoxide
4 - 23CH 104 Chapter 4
Covalent 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
Properties of ionic and covalent compounds
O=O
4 - 24CH 104 Chapter 4
Lewis Structures for Molecules & Polyatomic Ions
Practice drawing electron dot (Lewis) structures for the following:
H2O
OH1-
CO32-
PO43-
Notice options for Resonance Structures:
4 - 25CH 104 Chapter 4
Polyatomic Ions
Na1+ SO42-
Na2SO4
Sodium Sulfate
NH41+ PO4
3-
(NH4)3PO4
Ammonium Phosphate
NH41+
NH41+
Na1+
4 - 26CH 104 Chapter 4
Polyatomic Ions
Ca2+ C2H3O21-
Calcium Acetate
Sn2+ NO21-
Sn(NO2)2
Tin (II) Nitrite
C2H3O21-
Ca(C2H3O2)2
NO21-
Stannous Nitrite
4 - 27CH 104 Chapter 4
Naming Practice
Aluminum Flouride
FeF3
NF3
SO3
Mg2C
CaCO3
NaHCO3
K2SO3
AlF3
Iron (III) Flouride or Ferric Flouride
Nitrogen Triflouride
Sulfur Trioxide
Potassium Sulfite
Magnesium Carbide
Calcium CarbonateSodium Hydrogen CarbonateSodium Bicarbonate
4 - 28CH 104 Chapter 4
Bond Polarity, Electronegativity
ClH ClH
Electrons in covalent bonds rarely get shared equally.
Electronegativity
Relative 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
4 - 50
4 - 32CH 104 Chapter 4
Electronegativity
Relative 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
4 - 50
4.03.53.0
3.0
2.8
2.5
2.1
2.1 2.5
2.5
2.1
0.8
0.8
0.7
1.2
1.0
0.9 1.8
1.5 2.0
1.5
2.4
2.1
2.0
4 - 33CH 104 Chapter 4
ElectronegativityRelative ability of atoms to attract electrons.
Periodic trends
4 - 34CH 104 Chapter 4
ClH
ClH2.1 3.0
d-
Polar Covalent
d+
Electronegativity Difference
< 0.5 Nonpolar
0.5-1.7 Polar
>1.8 Ionic
Bond Polarity, Electronegativity
4 - 35CH 104 Chapter 4
C
Polarity, Shape
3.5 3.52.5
O=C=Od+ d-d-
Polar Covalent Bonds
Linear Shape (180o)Linear Shape (180o)
Electronegativity Difference
< 0.5 Nonpolar
0.5-1.7 Polar
>1.8 Ionic
Nonpolar Compound
CO2
O O
4 - 37CH 104 Chapter 4
CH H
O
Polarity, Shape (VSEPR)
O=C=Od+ d-d-
e-’s in 2 directions = 180o
Linear
e-’s in 3 directions = 120o
d+
d- Trigonal planar
Nonpolar Compound
Polar Compound
4 - 38CH 104 Chapter 4
CH HH
Cl
CH H
H
Cl HC
H
ClH
2.1
2.12.1
2.5
3.0
d+d-
(~109o)Tetrahedral
(~109o)Tetrahedral
Polarity, Shape (VSEPR)
e-’s in 4 directions = 109.5o
4 - 39CH 104 Chapter 4
Polarity, Shape (VSEPR)
OH H
H-O-H
O
H
H
2.1
2.1
3.5
d+
d+d-
(105o)Tetrahedral Configuration of Electrons
Bent Configuration of Atoms
(105o)Tetrahedral Configuration of Electrons
Bent Configuration of Atoms
e-’s in 4 directions = 109.5o
4 - 41CH 104 Chapter 4
NH HH d+
d-e-’s in 4 directions = 109.5o
Pyramidal
NH H
HH
NHHd+
d+
(~109.5o 107o)Tetrahedral Configuration of Electrons
Trigonal Pyramid Configuration of Atoms
(~109.5o 107o)Tetrahedral Configuration of Electrons
Trigonal Pyramid Configuration of Atoms
Polarity, Shape (VSEPR)
4 - 42CH 104 Chapter 4
Tetrahedral electron-pair Geometries
Tetrahedral
PyramidalBent
4 - 43CH 104 Chapter 4
FF B
Exceptions to Octet Rule
4.0
4.0
2.0 d+d- d-
Polar Covalent Bonds
(120o)Trigonal Planar
(120o)Trigonal Planar
Nonpolar Compound
BF3
F4.0F
B
F
Fd-
4 - 44CH 104 Chapter 4
Exceptions to Octet Rule
Trigonal BipyramidTrigonal Bipyramid
PCl5
P
Cl
Cl
ClClCl
S
F
F
FF
FFSF6
OctahedralOctahedral
4 - 46CH 104 Chapter 4
Some common geometries
e- pairs aroundShape central atom Example
Linear 2 BeH2, HF
Trigonal plane 3 BF3
Tetrahedral 4 CH4
Pyramidal 4 NH3
Bent 4 H2O
4 - 47CH 104 Chapter 4
Geometry and polar molecules
For a molecule to be polar- must have polar bonds- must have the proper geometry
CH4 non-polarCH3Cl polarCH2Cl2 polarCHCl3 polarCCl4 non-polar
WHY?
4 - 48CH 104 Chapter 4
Properties of ionic & covalent compounds
Ionic compounds•Exist as 3-D network of ions•Held together by electrostatic attraction
•Ionic compounds are solids at room temp.
•Formula is simple average
Covalent compounds•Discrete molecular units•Atoms held together by covalent bonds
•Covalent compounds exist in all states(CO2 - gas, H2O - liquid, SiO2 - solid)
•Formula represents atoms in a molecule
O=O
4 - 49CH 104 Chapter 4
Covalent 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
Properties of ionic and covalent compounds
O=O
4 - 50CH 104 Chapter 4
Attractive ForcesIonic Bonds 150 - 3000 kcal
mol150 - 3000 kcalmol
Melting PointNaCl 801oC
Na2S 920oC
MgF2 1248oC
Melting PointNaCl 801oC
Na2S 920oC
MgF2 1248oC
Ionic compounds•Held together by electrostatic attraction
•Ionic compounds are solids at room temp
Boiling PointNaCl 1413oC
Boiling PointNaCl 1413oC
4 - 51CH 104 Chapter 4
H
H
Od-d+
d+
H HOd-
d+d+
Attractive ForcesIon-Dipole
HH
Od-d+
d+HH
O d-
d+
d+
HHOd-
d+d+
H
H
Od
-d
+
d+
H
H
Od
-d
+
d+
H
H
Od- d+
d+
4 - 52CH 104 Chapter 4
H Cld+ d-
H Cld+ d-
Attractive Forces
Dipole-Dipole 0.1 - 1 kcalmol0.1 - 1 kcalmol
Melting PointHCl -114oC
CH3F -142oC
Melting PointHCl -114oC
CH3F -142oC
H Cld+ d-
H Cld+ d-
Boiling PointHCl -85oC
Boiling PointHCl -85oC
4 - 53CH 104 Chapter 4
F Fd+ d-
Fd+ d-
F
Attractive ForcesInduced dipole – Induced dipole(Dispersion Forces) 0.01 kcal
mol0.01 kcalmol
Melting Point
F2 -220oC
CH4 -183oC
Melting Point
F2 -220oC
CH4 -183oC
Fd+ d-
F
Fd+ d-
F
Boiling Point
F2 -188oC
CH4 -162oC
Boiling Point
F2 -188oC
CH4 -162oC
4 - 54CH 104 Chapter 4
Dipole-Induced Dipole Attractive Forces
Id+ d-
I
H HOd-
d+d+
H
HOd-
d+
d+
H
H
O d-
d+
d+
H
H Od
-
d+
d+
4 - 55CH 104 Chapter 4
H
HO
d+
d+d-
H H
Od+ d+
d-
H
H
Od+
d+
d-
H H
Od+ d+
d-
Polar Attraction
Attractive Forces
Hydrogen Bonds
4 - 56CH 104 Chapter 4
Hydrogen Bonding of Water
Hydrogen Bonds
5 - 10 kcalmol5 - 10 kcalmol
Melting Point
H2O 0oC
NH3 -78oC
Melting Point
H2O 0oC
NH3 -78oC
Boiling Point
H2O 100oC
NH3 -33oC
Boiling Point
H2O 100oC
NH3 -33oC
4 - 57CH 104 Chapter 4
Frozen H2O: Slow moving moleculesH-Bond in patterns
Hydrogen Bonding of Water
4 - 60CH 104 Chapter 4
Boiling and melting points
Chemical Bond Mp Bp N2 Nonpolar -210 -196 O2 Nonpolar -219 -183 NH3 Polar -78 -33 H2O Polar 0 100NaCl Ionic 804 1413
Melting and Boiling points•Very high for ionic compounds•Typically lower for covalent compounds
4 - 61CH 104 Chapter 4
Polarity and solubilitySolubility 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-Dipole• Hydrogen bonding• Van der Wall forces
General rule“Like dissolves like”
4 - 62CH 104 Chapter 462
Flowchart for Naming Ionic Compounds
4 - 63CH 104 Chapter 463
A. The Group number for sulfur is
1) 4A(14) 2) 8A(18) 3) 6A(16)
B. The number of valence electrons in sulfur is
1) 4e 2) 6e 3) 8e
C. The change in electrons for an octet requires a
1) gain of 2e 2) loss of 2e 3) a gain of 4e
D. The ionic charge of sulfur is
1) 2+ 2) 2 3) 4
Learning Check
4 - 64CH 104 Chapter 4
A. The Group number for sulfur is
1) 4A(14) 2) 8A(18) 3) 6A(16)
B. The number of valence electrons in sulfur is
1) 4e 2) 6e 3) 8e
C. For Sulfur to form an octet requires a
1) gain of 2e 2) loss of 2e 3) a gain of 4e
D. The ionic charge of sulfur is
1) 2+ 2) 2 3) 4 64
Solution
4 - 65CH 104 Chapter 465
Select the larger atom or ion in the following:
1. A.) Mg or B.) Mg2+
2. A.) S or B.) S2
3. A.) Br or B.) Br
Learning Check
4 - 66CH 104 Chapter 466
Solution
Select the larger atom or ion in the following:
1. A.) Mg or B.) Mg2+
2. A.) S or B.) S2
3. A.) Br or B.) Br
4 - 67CH 104 Chapter 467
Select the correct formula for each of the following ionic compounds:
A. Na+ and S2–
1) NaS 2) Na2S 3) NaS2
B. Al3+ and Cl–
1) AlCl3 2) AlCl 3) Al3Cl
C. Mg2+ and N3–
1) MgN 2) Mg2N3 3) Mg3N2
Learning Check
4 - 68CH 104 Chapter 468
Select the correct formula for each of the following ionic compounds:
A. Na+ and S2–
1) NaS 2) Na2S 3) NaS2
B. Al3+ and Cl–
1) AlCl3 2) AlCl 3) Al3Cl
C. Mg2+ and N3–
1) MgN 2) Mg2N3 3) Mg3N2
Solution
4 - 69CH 104 Chapter 469
Give the names of the following ions: Ba2+ Al3+ K+
_________ __________ _________
N3 O2 F
_________ __________ _________
P3 S2 Cl
_________ __________ _________
Learning Check
4 - 70CH 104 Chapter 470
Give the names of the following ions: Ba2+ Al3+ K+
barium aluminum potassium_____ ____ __________ _________
N3 O2 F
nitride oxide fluoride_________ __________ _________
P3 S2 Cl
phosphide sulfide chloride_________ __________ _________
Solution
4 - 71CH 104 Chapter 471
Write the names of the following compounds:
1) CaO ___________
2) KBr ___________
3) Al2O3 ___________
4) MgCl2 ___________
Learning Check
4 - 72CH 104 Chapter 472
Write the names of the following compounds:
1) CaO calcium oxide
2) KBr potassium bromide
3) Al2O3 aluminum oxide
4) MgCl2 magnesium chloride
Solution
4 - 73CH 104 Chapter 473
Learning Check
Write the formulas and names for compounds of the following ions:
Br– S2− N3−
Na+
Al3+
4 - 74CH 104 Chapter 474
Solution
Br− S2− N3−
Na+
Al3+
NaBrsodium bromide
Na2S
sodium sulfide
Na3N
sodium nitride
AlBr3
aluminum bromide
Al2S3
aluminum sulfide
AlNaluminum nitride
Write the formulas and names for compounds of the following ions:
4 - 75CH 104 Chapter 475
Learning Check
Select the correct name for each.A. Fe2S3
1) iron sulfide 2) iron(II) sulfide 3) iron(III) sulfide
B. CuO 1) copper oxide 2) copper(I) oxide 3) copper(II) oxide
4 - 76CH 104 Chapter 476
Solution
Select the correct name for each.A. Fe2S3
1) iron sulfide 2) iron(II) sulfide 3) iron(III) sulfide Fe3+ S2–
B. CuO 1) copper oxide 2) copper(I) oxide 3) copper(II) oxide Cu2+ O2–
4 - 77CH 104 Chapter 477
Learning Check
The correct formula for each of the following is:
A. copper(I) nitride 1) CuN 2) CuN3 3) Cu3N
B. lead(IV) oxide 1) PbO2 2) PbO 3) Pb2O4
4 - 78CH 104 Chapter 478
Solution
The correct formula for each of the following is:
A. copper(I) nitride 1) CuN 2) CuN3 3) Cu3N
3Cu+ + N3– = 3(1+) + (3–) = 0
B. lead(IV) oxide 1) PbO2 2) PbO 3) Pb2O4
Pb4+ + 2O2– = (4+) + 2(2–) = 0
4 - 79CH 104 Chapter 479
Match each formula with the correct name:
A. MgS 1) magnesium sulfite
MgSO3 2) magnesium sulfate
MgSO4 3) magnesium sulfide
B. Ca(ClO3)2 1) calcium chlorate
CaCl2 2) calcium chlorite
Ca(ClO2)2 3) calcium chloride
Learning Check
4 - 80CH 104 Chapter 480
Match each formula with the correct name:
A. MgS 1) magnesium sulfite
MgSO3 2) magnesium sulfate
MgSO4 3) magnesium sulfide
B. Ca(ClO3)2 1) calcium chlorate
CaCl2 2) calcium chlorite
Ca(ClO2)2 3) calcium chloride
Solution
4 - 81CH 104 Chapter 481
Learning Check
Name each of the following compounds:
A. Mg(NO3)2
B. Cu(ClO3)2
C. PbO2
D. Fe2(SO4)3
E. Ba3(PO3)2
4 - 82CH 104 Chapter 482
Solution
Name each of the following compounds:
A. Mg(NO3)2
B. Cu(ClO3)2
C. PbO2
D. Fe2(SO4)3
E. Ba3(PO3)2
magnesium nitrate
copper(II) chlorate
lead(IV) oxide
iron(III) sulfate
barium phosphite
4 - 83CH 104 Chapter 483
Select the correct formula for each:A. aluminum nitrate 1) AlNO3 2) Al(NO)3 3) Al(NO3)3
B. copper(II) nitrate 1) CuNO3 2) Cu(NO3)2 3) Cu2(NO3)
C. iron(III) hydroxide 1) FeOH 2) FeOH3 3) Fe(OH)3
D. tin(IV) hydroxide 1) Sn(OH)4 2) Sn(OH)2 3) Sn4(OH)
Learning Check
4 - 84CH 104 Chapter 484
Select the correct formula for each:A. aluminum nitrate 1) AlNO3 2) Al(NO)3 3) Al(NO3)3
B. copper(II) nitrate 1) CuNO3 2) Cu(NO3)2 3) Cu2(NO3)
C. iron(III) hydroxide 1) FeOH 2) FeOH3 3) Fe(OH)3
D. tin(IV) hydroxide 1) Sn(OH)4 2) Sn(OH)2 3) Sn4(OH)
Solution
4 - 85CH 104 Chapter 485
Learning Check
Write the correct formula for each:
A. potassium bromate
B. calcium carbonate
C. sodium phosphate
D. iron(III) oxide
E. iron(II) nitrite
4 - 86CH 104 Chapter 486
Solution
Write the correct formula for each:
A. potassium bromate
B. calcium carbonate
C. sodium phosphate
D. iron(III) oxide
E. iron(II) nitrite
KBrO3
CaCO3
Na3PO4
Fe2O3
Fe(NO2)2
4 - 87CH 104 Chapter 487
Learning Check
Name the following compounds:A. Ca3(PO4)2
B. FeBr3
C. Al2S3
D. Zn(NO2)2
E. NaHCO3
4 - 88CH 104 Chapter 488
Solution
Name the following compounds:A. Ca3(PO4)2 Ca2+ PO4
3− calcium phosphate
B. FeBr3 Fe3+ Br− iron(III) bromideC. Al2S3 Al3+ S2− aluminum sulfideD. Zn(NO2)2 Zn2+ NO2
− zinc nitriteE. NaHCO3 Na+ HCO3
− sodium hydrogen carbonate
orsodium
bicarbonate
4 - 89CH 104 Chapter 489
Learning Check
Write the formulas for the following:A. calcium nitrateB. iron(II) hydroxideC. aluminum carbonateD. copper(II) bromideE. lithium phosphate
4 - 90CH 104 Chapter 490
Solution
Write the formulas for the following:A. calcium nitrate Ca2+, NO3
− Ca(NO3)2
B. iron(II) hydroxide Fe2+, OH− Fe(OH)2
C. aluminum carbonate Al3+, CO32− Al2(CO3) 3
D. copper(II) bromide Cu2+, Br− CuBr2
E. lithium phosphate Li+, PO43−
Li3PO4
4 - 91CH 104 Chapter 491
What is the name of each of the following diatomic molecules?H2 _______________
N2 _______________
Cl2 _______________
O2 _______________
I2 _______________
Learning Check
4 - 92CH 104 Chapter 492
What is the name of each of the followingdiatomic molecules?
H2 hydrogenN2 nitrogenCl2 chlorine O2 oxygenI2 iodine
Solution
4 - 93CH 104 Chapter 493
FNO2, a rocket propellant, has two resonance structures. One is shown below. What is the other resonance structure?
Learning Check
4 - 94CH 104 Chapter 494
FNO2, a rocket propellant, has two resonance structures. One is shown below. What is the other resonance structure?
Solution
4 - 95CH 104 Chapter 495
Select the correct name for each compound.A. SiCl4 1) silicon chloride
2) tetrasilicon chloride3) silicon tetrachloride
B. P2O5 1) phosphorus oxide2) phosphorus pentoxide3) diphosphorus pentoxide
C. Cl2O7 1) dichlorine heptoxide2) dichlorine oxide3) chlorine heptoxide
Learning Check
4 - 96CH 104 Chapter 496
Select the correct name for each compound.A. SiCl4 3) silicon tetrachlorideB. P2O5 3) diphosphorus pentoxideC. Cl2O7 1) dichlorine heptoxide
Solution
4 - 97CH 104 Chapter 497
Write the name of each covalent compound.
CO _____________________
CO2 _____________________
PCl3 _____________________
CCl4 _____________________
N2O _____________________
Learning Check
4 - 98CH 104 Chapter 498
Write the name of each covalent compound.CO carbon monoxideCO2 carbon dioxidePCl3 phosphorus trichlorideCCl4 carbon tetrachlorideN2O dinitrogen oxide
Solution
4 - 99CH 104 Chapter 4
Guide to Writing Formulas for Covalent Compounds
99
4 - 100CH 104 Chapter 4100
Write the formula for carbon disulfide.
STEP 1 Elements are C and SSTEP 2 No prefix for carbon means 1 C
Prefix di = 2 Formula: CS2
Writing Formulas of Covalent Compounds
4 - 101CH 104 Chapter 4101
Write the correct formula for each of the following:A. phosphorus pentachloride
B. dinitrogen trioxide
C. sulfur hexafluoride
Learning Check
4 - 102CH 104 Chapter 4102
Write the correct formula for each of the following:A. phosphorus pentachloride
1P penta = 5Cl PCl5
B. dinitrogen trioxidedi = 2N tri = 3 O N2O3
C. sulfur hexafluoride1S hexa = 6F SF6
Solution
4 - 103CH 104 Chapter 4103
Learning Check
Identify each compound as ionic or covalent, and give its correct name.A. SO2
B. BaCl2
C. (NH4)3PO4
D. Cu2CO3
E. N2O4
4 - 104CH 104 Chapter 4104
Solution
Identify each compound as ionic or covalent, and give its correct name.
A. SO2 covalent; sulfur dioxide
B. BaCl2 ionic; barium chloride
C. (NH4)3PO3 ionic; ammonium phosphite
D. Cu2CO3 ionic; copper(I) carbonate
E. N2O4 covalent; dinitrogen tetroxide
4 - 105CH 104 Chapter 4105
Learning Check
Name the following compounds:A. Ca3(PO4)2
B. FeBr3
C. SCl2
D. Cl2O
4 - 106CH 104 Chapter 4106
Solution
Name the following compounds:
A. Ca3(PO4)2 ionic Ca2+, PO43− calcium
phosphate
B. FeBr3 ionic Fe3+, Br − iron(III) bromide
C. SCl2 covalent 1S, 2Cl sulfur dichloride
D. Cl2O covalent 2Cl, 1 O dichlorine oxide
4 - 107CH 104 Chapter 4107
Learning Check
Write the formulas for the following:A. calcium nitrateB. boron trifluorideC. aluminum carbonateD. dinitrogen tetroxideE. copper(I) phosphate
4 - 108CH 104 Chapter 4108
Solution
Write the formulas for the following:
A. calcium nitrate Ca2+, NO3−
Ca(NO3)2
B. boron trifluoride 1B, 3F BF3
C. aluminum carbonate Al3+, CO32− Al2(CO3) 3
D. dinitrogen tetroxide 2N, 4 O N2O4
E. copper(I) phosphate Cu+, PO43−
Cu3PO4
4 - 109CH 104 Chapter 4109
Use the electronegativity difference to identify the type of bond between the following:nonpolar covalent (NP), polar covalent (P), or
ionic (I) A. K–N
B. N–OC. Cl–ClD. B–Cl
Learning Check
4 - 110CH 104 Chapter 4110
Use the electronegativity difference to identify the type of bond between the following:nonpolar covalent (NP), polar covalent (P), or
ionic (I)A. K–N 2.2 ionic (I)
B. N–O 0.5 polar covalent (P)C. Cl–Cl 0.0 nonpolar covalent (NP)
D. B–Cl 1.0 polar covalent (P)
Solution
4 - 111CH 104 Chapter 4111
Learning Check
The shape of a molecule of N2O (N N O) is1) linear2) trigonal planar3) bent (120°)
4 - 112CH 104 Chapter 4112
Solution
The shape of a molecule of N2O (N N O) is1) linear
In the electron-dot structure with 16 e–, octets are acquired using two double bonds to the
central N atom. The shape of a molecule with two electron groups and two bonded atoms (no lone pairs on N) is linear.
two electron groups
• • • •
: N :: N :: O :
• • • •
: N = N=O : linear, 180°
4 - 113CH 104 Chapter 4113
Learning Check
State the number of electron groups and lone pairs, and use VSEPR theory to determine the shape of the following molecules or ions.
1) tetrahedral 2) pyramidal 3) bent
A. PF3
B. H2SC. CCl4
4 - 114CH 104 Chapter 4114
Solution
State the number of electron groups and lone pairs, and use VSEPR theory to determine the shape of the following molecules or ions. A. PF3
4 electron groups, 1 lone pair, (2) pyramidalB. H2S
4 electron groups, 2 lone pairs, (3) bentC. CCl4
4 electron groups, 0 lone pairs, (1) tetrahedral
4 - 115CH 104 Chapter 4115
Polar Molecules
A polar molecule contains polar bonds has a separation of positive and negative charge
called a dipole, indicated with + and –
has dipoles that do not cancel + –
• •
H–Cl H—N—H dipole
H dipoles do not cancel
4 - 116CH 104 Chapter 4116
Nonpolar Molecules
A nonpolar molecule contains nonpolar bonds
Cl–Cl H–H
or has a symmetrical arrangement of polar bonds
4 - 117CH 104 Chapter 4
Determining Molecular Polarity
Determine the polarity of the H2O molecule.
Solution: The four electron groups of oxygen are bonded to two H atoms. Thus the H2O molecule has a net dipole, which makes it a polar molecule.
117
4 - 118CH 104 Chapter 4118
Learning Check
Determine the shape of each of the following molecules and whether they are polar or nonpolar. Explain.A. PBr3
B. HBrC. Br2
D. SiBr4
4 - 119CH 104 Chapter 4119
Solution
Determine the shape of each of the following molecules and whether they are polar or nonpolar. Explain.A. PBr3 1) pyramidal; polar; dipoles don’t
cancelB. HBr 1) linear; polar; one polar bond (dipole)C. Br2 2) linear; nonpolar; nonpolar bondD. SiBr4 2) tetrahedral; nonpolar; dipoles cancel
4 - 120CH 104 Chapter 4120
Learning Check
Identify the main type of attractive forces for each:1) ionic 2) dipole–dipole 3) hydrogen bonds 4) dispersion
A. NCl3
B. H2OC. Br–BrD. KClE. NH3
4 - 121CH 104 Chapter 4121
Solution
Identify the main type of attractive forces for each:1) ionic 2) dipole–dipole3) hydrogen bonds 4) dispersion
2 A. NCl3
3 B. H2O 4 C. Br–Br 1 D. KCl 3 E. NH3