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17 Terms
1
What is the main similarity among ionic, covalent, and metallic bonds?
They all occur to satisfy the octet rule or fulfill the outer shell.
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2
What occurs in ionic bonds?
Metals (cations) give up valence electrons to non-metals (anions) which receive the valence electrons.
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3
What characterizes covalent bonds?
Non-metals (anions) bond with each other by sharing valence electrons.
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4
What is the nature of metallic bonds?
Metals (cations) are attracted to delocalized valence electrons shared in a sea of electrons among surrounding metal atoms.
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5
What are some properties of ionic compounds?
They form crystal lattices, are hard and brittle, conduct electricity when dissolved in water, and have high melting and boiling points.
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6
What are the properties of covalent compounds?
They form non-uniform crystal structures, do not conduct electricity if dissolved, have low melting and boiling points, are soft as solids, and can be flammable.
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7
What characterizes metallic compounds?
They are durable, ductile, malleable, conduct electricity and heat, and have moderate to high melting and boiling points.
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8
What is lattice energy?
The energy required to break an ionic bond.
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9
What is bond dissociation?
The energy required to break a covalent bond.
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10
How many valence electrons are required for a single bond?
2 valence electrons.
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11
What distinguishes a double bond from a single bond?
A double bond requires 4 valence electrons and consists of one sigma bond and one pi bond.
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12
What characterizes a triple bond?
A triple bond requires 6 valence electrons, is short in length, and is the strongest bond, consisting of one sigma and two pi bonds.
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13
What is a polar covalent bond?
An unequal sharing of valence electrons.
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14
What is a non-polar covalent bond?
An equal sharing of valence electrons.
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15
What is the London dispersion force?
The weakest intermolecular force; a temporary attractive force resulting from temporary dipoles in adjacent atoms.
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16
What are dipole-dipole forces?
Attractive forces between the positive end of one polar molecule and the negative end of another polar molecule.
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17
What defines a hydrogen bond?
The attractive force between hydrogen attached to an electronegative atom in one molecule and an electronegative atom in a different molecule, usually O, N, or F.
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