Drill: Calculate the
volume of hydrogen gas
o
produced at -23 C under
83.1 kPa pressure when
7.0 g of ammonia is
decomposed.
Homework
•Read Chapter 7
•Review PP-15
Bonding
Types of Bonds
•Ionic
•Covalent
•Metallic
Metallic Bonds
•Electrons are shared by
many atoms
•Electrons free to move
•Two or more metals
Metallic Compounds
•Generally high MP
•Hard & lusterous
•Less brittle
•Conductors
Metallic Bonds
•No debate about
metallic bonds
•Easy to identify
Ionic Bonds
•Electrons are
transferred from one
atom to another
creating (+) & (-) ions
•Metal & nonmetal
Ionic Compounds
•Held together by
electrostatic charge
•Very high MP
•Brittle
Covalent Bonds
•Electrons are shared
by two atoms
•Two nonmetals
•Weaker than ionic
Covalent Compounds
•Low MP
•Two nonmetals
•Flexible
Molecule
•Any compound
that can exist as an
entity by itself
Distinguishing Bonds
• Distinguishing ionic &
covalent bonds can be
difficult, but generally
determined by
differenceelectronegativity
Bonds Types
•Ionic
•Polar covalent
•Non polar covalent
Bond Types
• Ionic: DEN > 1.5-1.8
• Covalent: DEN < 1.5-1.8
• Polar Covalent: 0.5<DEN<1.5
• Non polar covalent :DEN< 0.5
• Not absolute
Coordinate Covalent
Bonds
•A covalent bond in
which the two
electrons are donated
by one atom
Classify Bonds
•Na-F
•C-O
•Fe-Fe
H-Cl
Mg-O
Dipole
•Polar bonds
•Polar molecules
Dipole
H F
d+
d-
Ionic Bonding
+
Covalent Bonding
Occurs when
electron orbitals
overlap
Homework
•Work problems 47,
49, & 51 on pages
204 & 205
List & describe
the three types
of bonds
Orbitals
On the board
Max 2 e per
orbital
Hybridization
• When s, p, and/or d
orbitals (electron
clouds) mix to make a
new type of multilobed orbital
Hybrid Orbitals
•sp
2
•sp
3
•sp
3
dsp
2
3
d sp
Homework
•Work problems 53,
55, 57, & 59 on
page 205
Electron Cloud
Repulsion
• In molecules each electron
cloud repels other clouds
enough to spread as far
apart as possible
VSEPR
• Valance Shell Electron
Pair Repulsion
• Electron pairs repel each
other to spread out as
much as possible
Bonding Orbitals
Type
Hybrid
• 2 lobes
sp
2
• 3 lobes
sp
3
• 4 lobes
sp
3
• 5 lobes
dsp
2
3
• 6 lobes
d sp
VSEPR
AX2
AX3
AX4
AX5
AX6
VSEPR Orbitals
Bonding Orbital Shape
• 2 lobes: Linear 180o
• 3 lobes: Trigonal planar 120o
o
• 4 lobes: Tetrahedral 109.5
• 5 lobes: Hexahedral 120&180o
• 6 lobes: Octahedral 90&180o
Drill: Calculate
the density SO2 at
o
47 C under 83.1
kPa Pressure:
Types of Bonds
•Ionic
•Covalent
•Metallic
Draw the Bonding
Electron Dot
Diagrams for Each
Element
Bonding Electron
Dot Diagrams
•Electron dot diagrams
that go through 4
singles before any
electrons are paired up
1A: 1 single
2A: 2 singles
3A: 3 singles
4A: 4 singles
5A: 1 pair & 3 singles
6A: 2 pair & 2 singles
7A: 3 pair & 1 single
8A: 4 pair
Drill: Equate each of the following:
3
sp
sp
3
dsp
2
sp
2
3
d sp
AX2
AX3
AX4
AX5
AX6
2 lobes
4 lobes
6 lobes
3 lobes
5 lobes
Lewis Dot Diagrams
•Representation of
valence electrons and
bonds in a molecule
or polyatomic ion
Drawing LDDs
Draw the bonding electron dot
diagram for each element in
the molecule with the
element with the most
unpaired e near the center
Drawing LDDs
• If there is more than one
carbon, connect the
carbons by connecting
single dots between one
carbon & another
Drawing LDDs
• Connect a single dot on
one atom to a single dot on
another (never two on the
same atom)(never connect
one dot to more than one
other dot)
Drawing LDDs
• Repeat connecting the
dots until all singled
dots are connected
making sure to obey the
octet rule if possible
Drawing LDDs
• Recognize polyatomic ions
-2
• H2CO3: CO3
is a
polyatomic ion; thus,
the three Os must
connect to the C
Drawing LDDs
•Redraw the molecule
neatly making sure to
include all dots
Draw LDDs for:
•BeCl2
•BF3
•CH4
•NH3
H2 O
C2H6
C3H6
CH2O
AP Homework
•Work problems 1,
3, 5, & 7 on pages
202 & 203
Chm II Homework
•Work problems 9,
10, 35, & 37 on
page 301
Lab 07 on Atomic
& Molecular
Orbitals will be
done tomorrow.
Drill: Draw the
LDD for:
C4 H 8
H2CO3
Resonance
Structures
Equally valid Lewis Dot
Diagrams for molecule
or polyatomic ion.
O
O N
-1
O
O
O N
-1
O
Homework
•Work problem 23
on page 203.
Drill: Draw LDDs
for:
•PH3
•HCN
-3
PO3
C 4 H8 O
Draw LDDs for:
CO2
-2
CO3
H2O
C2H6O
Coordinate
Covalent Bond
A covalent bond in
which both electrons
are donated by one
atom
Draw LDDs for:
SO2
-2
SO4
Draw LDDs for:
•PO4
-3
•K2SO4
P2O7
-4
C5H8O
Drill: Draw LDDs for:
C4H6O SCl2
C3H6O2 SiOF2
Draw LDDs for:
BeH2 AlCl3 SO2
CF4
NH3 H2O
Hybridizations
•sp
2
•sp
3
•sp
2 lobes
3 lobes
4 lobes
Bond Angles
•sp
2
•sp
3
•sp
o
~180
o
~120
o
~109.5
Sigma Bonds(s)
• End to end orbital overlap
• All single bonds are
sigma bonds
• All multiple bonds
contain one sigma bond
Pi Bonds (p)
•Side by side orbital
overlap
•Multiple bonds
contain p bonds
Multiple Bonds
•Double: 1 s & 1 p
•Triple: 1 s & 2 p
AP Homework
•Work problems 67,
71 on page 205
Expanded Octets
•Sometimes atoms
can be surrounded by
more than 8 electrons
• Columns 5A-8A
Draw LDDs for:
•PH5
-1
•SCl5
Drill: Draw LDDs:
•SiF6
•XeF4
-2
AP Homework
•Problem 17 & 19
Page 203
Drill: Draw LDDs:
•ICl3
+1
•IF4
Draw LDDs:
HNO3
C4H5NO
Homework
•Work problem 41,
45, 51, & 53 on
page 301 & 302.
Drill: Draw LDDs:
•P3O10
-5
•K2SO4
SCl5
-1
C5H8O
Drill: Predict the type
hybridization & VSEPR
type for central atoms
containing 2, 3, 4, 5, or 6
lobes of electron clouds
Molecular Orbital Theory
• Count valence e-s
• Draw orbital diagram (s & p e s)
• Draw bonding & anti-bonding Os
• Fill in the chart with total # of e s
• Add the total bonding &
antibonding orbital to get bond
order
Each line represents an orbital that
can contain up to two electrons
2p_ _ _
_ _ _2p
N
2s_
N
_2s
2p
_ _ _ anti-bonding
_ _ _2p
2p_ _ _
X
2p _ _ _ bonding
2s _ anti-bonding
_2s
2s_
2s
_ bonding
X
Determine the Bond
Order of N2
•Each N has 5 valence
•The total valence e s = 10
es
2p
___
_ _ _2p
2p_ _ _
N
2p _ _ _
2s _
N
_2s
2s_
2s
_
2p
___
_ _ _2p
2p_ _ _
N
2p _ _ _
2s _
N
_2s
2s_
2s
_
2p
___
_ _ _2p
2p_ _ _
N
2p _ _ _
2s _
N
_2s
2s_
2s
_
2p
___
_ _ _2p
2p_ _ _
N
2p _ _ _
2s _
N
_2s
2s_
2s
_
2p
___
_ _ _2p
2p_ _ _
N
2p _ _ _
2s _
N
_2s
2s_
2s
_
2p
___
_ _ _2p
2p_ _ _
N
2p _ _ _
2s _
N
_2s
2s_
2s
_
2p
___
_ _ _2p
2p_ _ _
N
2p _ _ _
2s _
N
_2s
2s_
2s
_
2p
___
_ _ _2p
2p_ _ _
N
2p _ _ _
2s _
N
_2s
2s_
2s
_
2p
___
_ _ _2p
2p_ _ _
N
2p _ _ _
2s _
N
_2s
2s_
2s
_
2p
___
_ _ _2p
2p_ _ _
N
4 bonding
- 1 anti
2p _ _ _
2s _
N
_2s
2s_
2s
_
Bond Order of
N2 = 3
Determine the bond
order of:
H2
F2
He2 O2
CO Xe2
Intermolecular Forces
• Weak temporary
attractions between atoms
from one molecule to
another or another part of
a larger molecule
Intermolecular Forces
• Hydrogen-bond
• Dipole-dipole
• Dipole-induced dipole
• London dispersion forces
Hydrogen Bond
• Strongest of the
intermolecular forces
• Occurs when H is bound
to one highly EN element
& connects to another
Dipole-Dipole
•When two polar
molecules connect
Dipole-Induced Dipole
•When a polar molecule
gets near a non-polar one,
it induces the non-polar
one to become polar;
thus, they connect
London Dispersion
• Instantaneous attraction
for fractions of seconds in
which non-polar
molecules connect
• Very weak force
Draw Lewis Dot Diagram for:
ICl5
Determine: bond
s, hybridization,
VSEPR, & shape
Draw the bonding electron
dot diagrams for one
element in each of the
columns that go to the top
of the chart, one transition
element, & one inner
transition element.
Identify as ionic, covalent,
or metallic bonds
Na-Cl
S-Cl
Mg-S
N-O
Fe-Cr
H-Cl
C-C
Fe-Fe
Draw LDDs for:
HONO H3PO4
SiO2 C3H4O2
Draw Lewis Dot Diagrams of:
CF4
BF3
H2CO3
NH3
CO2
C3H6O2
Draw Lewis Dot Diagrams of:
H3PO4
IF3
SeCl4
ICl5
CO
C4H6O2
Draw Lewis Dot Diagrams of:
H3AsO4 ICl5
ICl3
CO
C4H9NO2 SeF4
Draw LDDs & predict
VSEPR, Hybridization,
bond s, & shape of:
XeF4
SCl4
XeO4
List & describe
the four types of
intermolecular
forces
Draw Lewis Dot
Diagrams of:
C4H5NO2