chapter 16 covalent bonding milbank high school. section 16.1 the nature of covalent bonding...
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Chapter 16Covalent Bonding
Milbank High School
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Section 16.1The Nature of Covalent Bonding
• OBJECTIVES:– Describe and give examples of
coordinate covalent bonding, resonance structures, and exceptions to the octet rule.
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Section 16.1The Nature of Covalent Bonding
• OBJECTIVES:– Use electron dot structures to show the
formation of single, double, and triple covalent bonds.
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How does H2 form?
• The nuclei repel
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How does H2 form?
++
• The nuclei repel
• But they are attracted to electrons
• They share the electrons
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Covalent bonds• Nonmetals hold on to their valence
electrons.• Get noble gas configuration by sharing
valence electrons with each other.• By sharing, both atoms get to count the
electrons toward a noble gas configuration.
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Covalent bonding
• Fluorine has seven valence electrons
F
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Covalent bonding
• Fluorine has seven valence electrons
• A second atom also has seven
F F
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Covalent bonding Fluorine has seven valence
electrons A second atom also has seven By sharing electrons…
F F
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Covalent bonding Fluorine has seven valence
electrons A second atom also has seven By sharing electrons…
F F
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Covalent bonding Fluorine has seven valence
electrons A second atom also has seven By sharing electrons…
F F
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Covalent bonding Fluorine has seven valence
electrons A second atom also has seven By sharing electrons…
F F
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Covalent bonding Fluorine has seven valence
electrons A second atom also has seven By sharing electrons…
F F
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Covalent bonding Fluorine has seven valence electrons A second atom also has seven By sharing electrons… …both end with full orbitals
F F
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Covalent bonding Fluorine has seven valence electrons A second atom also has seven By sharing electrons… …both end with full orbitals
F F8 Valence electrons
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Covalent bonding Fluorine has seven valence electrons A second atom also has seven By sharing electrons… …both end with full orbitals
F F8 Valence electrons
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A Single Covalent Bond is...
• A sharing of two valence electrons.
• Only nonmetals and Hydrogen.
• Different from an ionic bond because they actually form molecules.
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Water
H
O
Each hydrogen has 1 valence electron
Each hydrogen wants 1 more
The oxygen has 6 valence electrons
The oxygen wants 2 more
They share to make each other happy
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Water
• The oxygen still wants one more
H O
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Water
• The second hydrogen attaches
• Every atom has full energy levels
H OHSample 16-1,
p.440
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Multiple Bonds• Double bonds - share two pairs (4
total) of electrons
• Triple bond - share three pairs (6 total) of electrons
• Table 16.1, p.443 - Know which elements are diatomic (Oxygen?)
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Carbon dioxide• CO2 - Carbon is central
atom ( more metallic )
• Carbon has 4 valence electrons
• Wants 4 more
• Oxygen has 6 valence electrons
• Wants 2 more
O
C
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Carbon dioxide
• Attaching 1 oxygen leaves the oxygen 1 short, and the carbon 3 short
OC
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Carbon dioxide Attaching the second oxygen
leaves both oxygen 1 short and the carbon 2 short
OCO
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Carbon dioxide The only solution is to share more
OCO
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Carbon dioxide The only solution is to share more
OCO
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Carbon dioxide The only solution is to share more
OCO
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Carbon dioxide The only solution is to share more
OCO
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Carbon dioxide The only solution is to share more
OCO
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Carbon dioxide The only solution is to share more
OCO
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Carbon dioxide The only solution is to share more Requires two double bonds Each atom can count all the
electrons in the bond
OCO
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Carbon dioxide The only solution is to share more Requires two double bonds Each atom can count all the electrons in
the bond
OCO8 valence electrons
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Carbon dioxide The only solution is to share more Requires two double bonds Each atom can count all the electrons in
the bond
OCO8 valence electrons
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Carbon dioxide The only solution is to share more Requires two double bonds Each atom can count all the electrons in
the bond
OCO
8 valence electrons
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N HHH
Examples
• Draw in the bonds
• All 8 electrons are accounted for
• Everything is full
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HCN• Put single bond between each atom
• Need to add 2 more bonds
• Must go between C and N
NH C
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HCN Put in single bonds Need 2 more bonds Must go between C and N Uses 8 electrons - 2 more to add to
equal the 10 it has
NH C
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HCN Put in single bonds Need 2 more bonds Must go between C and N Uses 8 electrons - 2 more to add Must go on N to fill octet
NH C
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Another way of indicating bonds
• Often use a line to indicate a bond• Called a structural formula• Each line is 2 valence electrons
H HO = H HO
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Structural Examples
H C N
C OH
H
• C has 8 e- because each line is 2 e-
• same for N
• same for C here
• same for O
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A Coordinate Covalent Bond...
• When one atom donates both electrons in a covalent bond.
• Carbon monoxide
• CO
OC
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Coordinate Covalent Bond When one atom donates both
electrons in a covalent bond. Carbon monoxide CO
OC
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Coordinate Covalent Bond When one atom donates both
electrons in a covalent bond. Carbon monoxide CO
OCC O
Shown as:
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Bond Dissociation Energies...
• The total energy required to break the bond between 2 covalently bonded atoms
• High dissociation energy usually means unreactive
• Table 16.3, p448
• Sample: Calculate the kJ to dissociate the bonds in 0.5 mol CO2
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Resonance is...
• When more than one valid dot diagram is possible.
• Consider the two ways to draw ozone (O3)
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Exceptions to Octet rule
• When there is an odd number of valence electrons– NO2 has 17 valence electrons,
because the N has 5, and each O contributes 6
• impossible to satisfy octet, yet the stable molecule does exist
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Section 16.2Bonding Theories
• OBJECTIVES:– Describe the molecular orbital theory of
covalent bonding, including orbital hybridization.
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Section 16.2Bonding Theories
• OBJECTIVES:– Use VSEPR theory to predict the
shapes of simple covalently bonded molecules.
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VSEPR: stands for...
• Valence Shell Electron Pair Repulsion
• Predicts three dimensional geometry of molecules.
• The name tells you the theory:
• Valence shell - outside electrons.
• Electron Pair repulsion - electron pairs try to get as far away as possible.
• Can determine the angles of bonds.
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VSEPR• Single bonds fill all
atoms.• There are 4 pairs of
electrons pushing away.
• The furthest they can get away is 109.5º
C HH
H
H
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4 atoms bonded• Basic shape is
tetrahedral.
• A pyramid with a triangular base.
• Same shape for everything with 4 pairs. CH H
H
H 109.5º
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Other angles…p.456
• Ammonia (NH3) = 107o
• Water (H2O) = 105o
• Carbon dioxide (CO2) = 180o
• Note shapes in Fig. 16.16, p.457
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Section 16.3Polar Bonds and Molecules
• OBJECTIVES:– Use electronegativity values to classify a
bond as nonpolar covalent, polar covalent, or ionic.
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Section 16.3Polar Bonds and Molecules
• OBJECTIVES:– Name and describe the weak attractive
forces that hold groups of molecules together.
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Bond Polarity
• Refer to Table 14.2, p.405
• Consider HClH = electronegativity of 2.1
Cl = electronegativity of 3.0
– the bond is polar
– the chlorine acquires a slight negative charge, and the hydrogen a slight positive charge
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Bond Polarity• Only partial charges, much less than
a true 1+ or 1- as in ionic bond• Written as:
HCl
• the positive and minus signs (with the lower case delta) denote partial charges.
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Bond Polarity• Can also be shown:
• the arrow points to the more electronegative atom.
• Table 16.4, p.462 shows how the electronegativity can also indicate the type of bond that tends to form
H Cl
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Attractions between molecules
• They are what make solid and liquid molecular compounds possible.
• The weakest called van der Waal’s forces - there are two kinds:
1. Dispersion forces
weakest of all, caused by motion of e-
increases as # e- increases
halogens start as gases; bromine is liquid; iodine is solid
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2. Dipole interactions
• Occurs when polar molecules are attracted to each other.
• Fig. 16.23, p.464• Dipole interaction happens in water
– positive region of one water molecule attracts the negative region of another water molecule.