Chapter 8: Basic Concepts of Chemical Bonding

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Ionic Bond

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20 Terms

1

Ionic Bond

An electrostatic attraction between ions, typically formed between metals and nonmetals.

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2

Covalent Bond

A bond formed when nonmetals share electrons.

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3

Octet Rule

A chemical rule that reflects the observation that atoms tend to bond in such a way that they each have eight electrons in their valence shell.

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4

Lewis Symbols

Symbols that represent the valence electrons of an atom as dots surrounding the element's symbol.

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5

Lone pairs

Electrons located on only one atom in a Lewis structure.

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6

Bonding pairs

Shared electrons in a Lewis structure, represented by two dots or one line.

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7

Electronegativity

The ability of an atom in a molecule to attract electrons to itself.

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8

Non-polar covalent bond

A covalent bond where the electrons are shared equally.

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9

Polar covalent bond

A covalent bond where the electrons are not shared equally, resulting in a dipole.

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10

Dipole Moment (Ī¼)

A measure of the separation of positive and negative charges in a molecule.

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11

Formal Charge

The charge an atom would have if all electrons in a covalent bond were shared equally.

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12

Resonance

The concept that some molecules can be represented by two or more structures that differ only in the placement of electrons.

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13

Hypervalent

Referring to atoms that can accommodate more than eight electrons in their valence shell.

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14

Localized electrons

Electrons that are specifically on one atom or shared between two atoms.

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15

Delocalized electrons

Electrons that are spread over several atoms and can move around.

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16

Electronegativity trend

Electronegativity increases from left to right and decreases from bottom to top on the periodic table.

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17

Multiple Bonds

Bonds formed when atoms share more than one pair of electrons; includes single, double, and triple bonds.

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18

Lewis Structure

A diagram that shows the arrangement of atoms and the distribution of electrons in a molecule.

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19

Bound pairs

Pairs of electrons that are shared between atoms in a covalent bond, contributing to bond formation.

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20

Octet exceptions

Ions or molecules that do not follow the octet rule, including those with odd electron counts, fewer or more than eight electrons.

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