Download - Chemical bonding part 2
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CHEMICAL BONDING
• IONIC BONDS
• COVALENT BONDS
• HYDROGEN BONDS
• METALLIC BONDS
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IONIC BONDING
When an atom of a nonmetaltakes one or more electrons
from an atom of a metalso both atoms end up with
eight valence electrons
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IONIC BONDING
IS THE COMPOUND AN IONIC COMPOUND?
METALMETAL NONMETAL
SUBSCRIPTS
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IONIC BOND FORMATION
Neutral atoms come near each other. Electron(s) are transferred from the Metal atom to the Non-metal atom. They stick together because of electrostatic forces, like magnets.
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IONIC BONDING
Metals will tend to lose electrons and become
POSITIVE CATIONS
Normal sodium atom loses one electron to become sodium ion
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IONIC BONDING
Nonmetals will tend to gain electrons and become
NEGATIVE ANIONS
Normal chlorine atom gains an electron to become a chloride ion
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POLYATOMIC IONS--a group of atoms that act like one ion
NH4+1--ammonium ion
CO3-2--carbonate ion
PO4-3--phosphate ion
IONIC BONDING
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IONIC BONDING
SODIUM SULFATE
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Properties of Ionic Compounds
• Crystalline structure.
• A regular repeating arrangement of ions in the solid.
• Ions are strongly bonded.
• Structure is rigid.
• High melting points- because of strong forces between ions.
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Crystalline structure
+
+
+ +
+
+
++
+
--
--
- --
--
The POSITIVE CATIONS stick to the
NEGATIVE ANIONS, like
a magnet.
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Do they Conduct?
• Conducting electricity is allowing charges to move.
• In a solid, the ions are locked in place.• Ionic solids are insulators.• When melted, the ions can move
around.• Melted ionic compounds conduct.• First get them to 800ºC.• Dissolved in water they conduct.
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Ionic solids are brittle
+ - + -+- +-
+ - + -+- +-
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Ionic solids are brittle
+ - + -
+- +-+ - + -
+- +-
• Strong Repulsion breaks crystal apart.
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COVALENT BONDING
When an atom of one nonmetal
shares one or more electrons
with an atom of another
nonmetal so both atoms
end up witheight valence electrons
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COVALENT BOND FORMATION
When one nonmetal shares one or more electrons with an atom of another nonmetal so both atoms end up with eight valence electrons
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COVALENT BONDING
IS THE COMPOUND A COVALENT COMPOUND?
NONMETALNONMETAL NONMETAL
YES since it is made of only nonmetal elementsYES since it is made of only nonmetal elements
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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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Single Covalent Bond
• A sharing of two valence electrons.
• Only nonmetals and Hydrogen.
• Different from an ionic bond because they actually form molecules.
• Two specific atoms are joined.
• In an ionic solid you can’t tell which atom the electrons moved from or to.
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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
• Put the pieces together• The first hydrogen is happy• The oxygen still wants one more
H O
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Water
• The second hydrogen attaches
• Every atom has full energy levels
H OH
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Carbon dioxide• CO2 - Carbon is central atom (
I have to tell you)
• Carbon has 4 valence electrons
• Wants 4 more
• Oxygen has 6 valence electrons
• Wants 2 moreO
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 gets to count all the atoms in
the bond
OCO
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Carbon dioxide The only solution is to share more Requires two double bonds Each atom gets to count all the atoms 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 gets to count all the atoms 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 gets to count all the atoms in
the bond
OCO
8 valence electrons
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How to draw them
• Add up all the valence electrons.• Count up the total number of electrons to
make all atoms happy.• Subtract.• Divide by 2• Tells you how many bonds - draw them.• Fill in the rest of the valence electrons to fill
atoms up.
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Examples
• HCN C is central atom• N - has 5 valence electrons wants 8• C - has 4 valence electrons wants 8• H - has 1 valence electrons wants 2
• HCN has 5+4+1 = 10
• HCN wants 8+8+2 = 18• (18-10)/2= 4 bonds• 3 atoms with 4 bonds -will require multiple bonds -
not to H
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HCN
• Put in single bonds• Need 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
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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Polar Bonds
• When the atoms in a bond are the same, the electrons are shared equally.
• This is a nonpolar covalent bond.• When two different atoms are connected,
the atoms may not be shared equally.• This is a polar covalent bond.• How do we measure how strong the atoms
pull on electrons?
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Electronegativity
• A measure of how strongly the atoms attract electrons in a bond.
• The bigger the electronegativity difference the more polar the bond.
• 0.0 - 0.3 Covalent nonpolar
• 0.3 - 1.67 Covalent polar
• >1.67 Ionic
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How to show a bond is polar• Isn’t a whole charge just a partial chargemeans a partially positivemeans a partially negative
• The Cl pulls harder on the electrons• The electrons spend more time near the Cl
H Cl
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Polar Molecules
Molecules with ends
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Polar Molecules
• Molecules with a positive and a negative end• Requires two things to be true The molecule must contain polar bonds
This can be determined from differences in electronegativity.
Symmetry can not cancel out the effects of the polar bonds.
Must determine geometry first.
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Is it polar?
• HF
• H2O
• NH3
• CCl4
• CO2
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Intermolecular Forces
What holds molecules to each other
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Intermolecular Forces
• They are what make solid and liquid molecular compounds possible.
• The weakest are called van der Waal’s forces - there are two kinds
• Dispersion forces• Dipole Interactions
– depend on the number of electrons – more electrons stronger forces– Bigger molecules
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Dipole interactions
• Depend on the number of electrons
• More electrons stronger forces
• Bigger molecules more electrons
• Fluorine is a gas
• Bromine is a liquid
• Iodine is a solid
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Dipole interactions
• Occur when polar molecules are attracted to each other.
• Slightly stronger than dispersion forces.
• Opposites attract but not completely hooked like in ionic solids.
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Dipole interactions
• Occur when polar molecules are attracted to each other.
• Slightly stronger than dispersion forces.
• Opposites attract but not completely hooked like in ionic solids.
H F
H F
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Dipole Interactions
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Hydrogen bonding
• Are the attractive force caused by hydrogen bonded to F, O, or N.
• F, O, and N are very electronegative so it is a very strong dipole.
• The hydrogen partially share with the lone pair in the molecule next to it.
• The strongest of the intermolecular forces.
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Hydrogen Bonding
HH
O+ -
+
H HO+-
+
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Hydrogen bonding
HH
O H HO
HH
O
H
H
OH
HO
H
HO HH
O
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MOLECULAR SHAPES
OFCOVALENT
COMPOUNDS
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VSepR tHEORY
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What Vsepr means
Since electrons do not like each other, because of their negative charges, they orient themselves as far apart as possible, from each other.
This leads to molecules having specific shapes.
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Things to remember
•Atoms bond to form an Octet (8 outer electrons/full outer energy level)
•Bonded electrons take up less space then un-bonded/unshared pairs of electrons.
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Linear
•Number of Bonds = 2
•Number of Shared Pairs of Electrons = 2
•Bond Angle = 180°
EXAMPLE:
BeF2
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Trigonal Planar
•Number of Bonds = 3
•Number of Shared Pairs of Electrons = 3
•Number of Unshared Pairs of Electrons = 0
•Bond Angle = 120°
EXAMPLE:
GaF3
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Bent #1
•Number of Bonds = 2
•Number of Shared Pairs of Electrons = 2
•Number of Unshared Pairs of Electrons = 2
•Bond Angle = < 120°
EXAMPLE:
H2O
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Bent #2
•Number of Bonds = 2
•Number of Shared Pairs of Electrons = 2
•Number of Unshared Pairs of Electrons = 1
•Bond Angle = >120°
EXAMPLE:
O3
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Tetrahedral
•Number of Bonds = 4
•Number of Shared Pairs of Electrons = 4
•Number of Unshared Pairs of Electrons = 0
•Bond Angle = 109.5°
EXAMPLE:
CH4
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Trigonal Pyramidal
•Number of Bonds = 3
•Number of Shared Pairs of Electrons = 4
•Number of Unshared Pairs of Electrons = 1
•Bond Angle = <109.5°
EXAMPLE:
NH3
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Trigonal bIPyramidal
•Number of Bonds = 5
•Number of Shared Pairs of Electrons = 5
•Number of Unshared Pairs of Electrons = 0
•Bond Angle = <120°
EXAMPLE:
NbF5
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OCTAHEDRAL
•Number of Bonds = 6
•Number of Shared Pairs of Electrons = 6
•Number of Unshared Pairs of Electrons = 1
•Bond Angle = 90°
EXAMPLE:
SF6
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Metallic Bonds
• How atoms are held together in the solid.
• Metals hold onto there valence electrons very weakly.
• Think of them as positive ions floating in a sea of electrons.
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Sea of Electrons
+ + + ++ + + +
+ + + +
• Electrons are free to move through the solid.
• Metals conduct electricity.
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Metals are Malleable
• Hammered into shape (bend).
• Ductile - drawn into wires.
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Malleable
+ + + ++ + + +
+ + + +
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Malleable
+ + + +
+ + + ++ + + +
• Electrons allow atoms to slide by.
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