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+
Chemical Bonding
Chm 1.2.1 and 1.2.2
CuN
ArF
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+Chemical Bond
A mutual attraction for electrons on adjacent atoms
Atoms bond in different ways in order to achieve stability
Stability = lowest energy
e- involved in bonding = valance e-
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+Valance Electrons
e- in the outermost energy level (n)
Determined by electron configuration
Determined by group #s block valance e- = group #p block valance e- = group # - 10
d and f block = 2 valance e-
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+Types of Chemical Bonds
1. Metallic BondingBetween metal atomsOverlapping of outer orbitalsSharing of all valance e- between all atoms
“sea of electrons”Reason for conductivity
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+Types of Chemical Bonds
2. Ionic BondingBond between ions Attraction between + cation and – anion
Metals lose e- = cationsNonmetals gain e- = anions
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+Ions
Cations (+ charged)Metals become cationsLose valance e- to become stable
The octet rule Chemical stability = 8 valance e-
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+Ions
Anions (- charged)Non-Metals become anionsGain valance e- to become stable
The octet rule Chemical stability = 8 valance e-
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+Ionic Charge
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+Ionic Bond: e- transfer
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+Types of Chemical Bonds
3. Covalent BondsBetween nonmetal atomsOverlap of outer orbitals valance e- are sharedEach atom can achieve stability8 valance e-2 valance e- (Hydrogen)6 valance e- (Boron)
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+Covalent Bonding
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+Types of Covalent Bonds1. Nonpolar Covalent Bonds
e- are being shared equallyno electronegativity difference between atoms (ΔEN < 0.3)
least ionic character diatomic molecules
atoms that cannot exist aloneAlways exist bonded to themselves
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+Types of Covalent Bonds2. Polar Covalent Bonds
e- are not being shared equallyLarger electronegativity difference between atoms (ΔEN > 0.3)
Higher ionic characterResults in + and – partial charges on atoms
* Bonds with ΔEN > 1.7 = ionic bonds (100% ionic character)
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+Non Polar Covalent Bond
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+Polar Covalent Bond
δ
δ
δ