types of chemical bonds (what holds atoms together): covalent – sharing electrons between non...
TRANSCRIPT
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BONDINGBOND TYPES
BOND ENERGIES
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Types of Chemical Bonds (what holds atoms together):
Covalent – sharing electrons between non metal atoms to form molecules.
Nonpolar – equal sharingPolar – unequal sharing
Ionic – giving or taking electrons between atoms to form compounds.
Metallic – a “sea of electrons” among metal atoms to form the metal solid.
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IONIC COVALENTBond Formation
Type of Structure
Solubility in Water
Electrical Conductivity
OtherProperties
e- are transferred from metal to nonmetal
high
yes (solution or liquid)
yes
e- are shared between two nonmetals
low
no
usually not
MeltingPoint
crystal lattice true molecules
Types of Bonds
Physical State solid liquid or gas
odorous
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“electron sea”
METALLICBond Formation
Type of Structure
Solubility in Water
Electrical Conductivity
OtherProperties
MeltingPoint
Physical State
e- are delocalized among metal atoms
very high
yes (any form)
no
malleable, ductile, lustrous
solid
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Ionic Bonding - Crystal Lattice
Types of Bonds
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Covalent Bonding - True Molecules
Types of Bonds
Diatomic Molecule
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Metallic Bonding - “Electron Sea”
Types of Bonds
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CHEMICAL FORMULA
MolecularFormula
FormulaUnit
IONIC COVALENT
CO2NaCl
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Chemical Bond
attractive force between atoms or ions that binds them together as a unit
bonds form in order to…○decrease potential energy (PE)○ increase stability
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Bond Polarity Most bonds are a
blend of ionic and covalent characteristics.
Difference in electronegativity determines bond type.
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Bond Polarity
ElectronegativityAttraction an atom has for a shared pair of
electrons.higher e-neg atom -
lower e-neg atom +
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Bond Polarity Electronegativity Trend
Increases up and to the right.
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Nonpolar Covalent Bonde- are shared equallysymmetrical e- densityusually identical atoms
Bond Polarity
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+ -
Bond Polarity
Polar Covalent Bonde- are shared unequallyasymmetrical e- densityresults in partial charges (dipole)
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Nonpolar (Pure)
Polar
Ionic
View Bonding Animations.
Bond Polarity
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Bond Polarity
Examples:
Cl2
HCl
NaCl
3.0-3.0=0.0Nonpolar
3.0-2.1=0.9Polar
3.0-0.9=2.1Ionic
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MOLECULAR POLARITY
When does a MOLECULE become polar??
Write some examples:
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ATTRACTIONS BETWEEN ATOMS
INTRAMOLECULAR FORCESCovalent BondsIonic (Electrostatic) BondsMetallic Bonds
Examples:
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8.4 in TEXTBOOK:Attractions between Molecules INTERMOLECULAR FORCES
Van der Waals Forces – weakest attractions○ Result of dipole interactions – when one polar
molecule “lines up” to another molecule○ Dispersion forces – occur between ALL molecules
(polar or not) and are momentaryHydrogen Bonds – strongest type of intermolecular
force○ Always involves hydrogen○ An attraction to a hydrogen atom ALREADY bonded
to another strongly electronegative atom○ Hydrogen becomes strongly polarized with a bond
and will therefore try to compensate when close to another molecule
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BOND ENERGIES
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Energy of Bonding
Endothermic – heat is a reactant heat is absorbed breaking a bond
Reaction 1(endo):
CD + 100kJ C + D
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Energy of BondingExothermic – heat is a product heat is released making a bond less potential energy bond is more stable
Reaction 2 (exo): A + B AB + 100kJ
Reaction 3: E + B EB + 100kJ
Reaction 4: F + G FG + 400kJ
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Reaction 1(endo): CD + 100kJ C + D
Reaction 2 (exo): A + B AB + 100kJ
Reaction 3: E + B EB + 100kJ
Reaction 4: F + G FG + 400kJ
Which bond is more stable, EB or FG?FG, because it takes more energy (300kj more) to break the bond
than EB.
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Energy of Bond Formation
Bond EnergyShort bond = high bond energy
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