Unit 2 Flashcards

1
Q

Lattice energy (electrostatic)

A

the energy required to completely separate
one mole of a solid ionic compound into gaseous ions (E = kQ+Q-/ r)
-Lattice energy (E) increases
as Q increases and/or
as r decreases.

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2
Q

covalent bond

A

chemical bond in which two or more
electrons are shared by two atoms.

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3
Q

Polar covalent bond or polar bond

A

covalent
bond with greater electron density around one of the
two atoms

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4
Q

Electronegativity

A

ability of an atom to attract
toward itself the electrons in a chemical bond
-electron affinity (measurable, Cl highest)
-electronegativity (relative, F highest)

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5
Q
A
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6
Q

Classification of bonds by difference in electronegativity

A

0-0.4 non-polar covalent
0.5-1.9 polar covalent
2 or > ionic
(dif in electronegativity from sharing, partial transfer, to transfer)

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7
Q

Writing Lewis Structures

A
  1. Draw skeletal structure of compound showing
    what atoms are bonded to each other. Put least
    electronegative element in the center.
  2. Count total number of valence e-
    . Add 1 for
    each negative charge. Subtract 1 for each
    positive charge.
  3. Complete an octet for all atoms except
    hydrogen
  4. If structure contains too many electrons, form
    double and triple bonds on central atom as
    needed.
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8
Q

formal charge

A

= total # valence electrons in free atom - nonbonded electrons - 1/2 bonded electrons

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9
Q

Formal Charge and Lewis Structures

A
  1. For neutral molecules, a Lewis structure in which there
    are no formal charges is preferable to one in which
    formal charges are present.
  2. Lewis structures with large formal charges are less
    plausible than those with small formal charges.
  3. Among Lewis structures having similar distributions of
    formal charges, the most plausible structure is the one in
    which negative formal charges are placed on the more
    electronegative atoms.
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10
Q

resonance structure i

A

one of two or more Lewis structures for a single molecule that cannot be represented accurately by
only one Lewis structure. (O3, CO3-2, SO2

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11
Q

bond energy

A

The enthalpy change required to break a particular bond in
one mole of gaseous molecules = BE reactants=BE products

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12
Q

bond order

A

bonds/domains

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13
Q
A
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13
Q
A
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13
Q
A
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