Unit 1 - General Chemistry Review

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24 Terms

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atomic number (Z)

# p+ (in neutral atoms)

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mass number (A)

p+ + nº (in neutral atoms)

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isotopes

atoms with same #p+ but different # nº

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orbital e- capacity

2 e-

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shell e- capacity

2n2

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orbital shapes

S: spherical

P: dumbbell (3D)

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ions

charged atoms

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ionization energy

energy needed to remove e- from atoms in gaseous state

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electron affinity

energy released after addition of e- to atom in gaseous state

  • larger energy → stronger product

  • groups 16 & 17 have highest EA

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ionic bonding

metal transfers e- to nonmetal, both end up with noble gas configuration

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polyatomic ions

charged molecules

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covalent bonding

sharing of e- between anions to achieve full octet

exceptions (H, Be, B, P, S)

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most stable bonding patterns

atom

H

C

N

O

# bonds

1

4

3

2

# lone pairs

0

0

1

2

total # e-

2

8

8

8

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formal charge of atom

# Valence e- - (unbonded e- + # bonds)

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pos/neg formal charge of atom

  • if atom has more bonds than that #, atom has + formal charge

  • if atom has less bonds than that #, atom has - formal charge

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VSEPR theory

e- in bonds and lone pairs repel producing 30º molecular shape

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steps to predict VSEPR shapes

  1. draw lewis structure

  2. count # of e- regions on atom

  3. use table

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wedge dash system

  • line bond: in plane of paper

  • wedge bond: toward you

  • dash bond: away from you/into the paper

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orbital hybridization theory

shows that we can create hybrid orbitals (C-H bond is SP³ orbital)

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sigma bond

created by bonds with at least one hybrid orbital

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electronegativity

e- negatively affects ability of atom to pull e- density towards itself in a covalent bond (fluorine is most electronegative element)

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polar bond

permanent bond dipole created by difference in electronegativity between atoms and asymmetric distribution of e- density (C-H is effectively non polar)

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non polar bond

atoms are identical (a molecule can be non polar even if polar molecules are present)

ex: CF^4 (polar CF bonds cancel out)

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electrostatic potential maps

show e- density distribution

  • red: e- rich areas

  • Blue: e- deficient area

  • green: non polar area