Chem Vocab quiz April Flashcards

1
Q

Coordination Number

A

the number of ions of opposite charge that surround each ion in a crystal

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2
Q

Electron dot structure

A

Depicts valence electrons as dots around the atomic symbol.

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3
Q

Ionic bond

A

Electrostatic attraction that binds oppositely charged ions together.

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4
Q

Metallic bond

A

An attraction between metal atoms that loosely involves many electrons

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5
Q

Octet rule

A

Atoms react by gaining or losing electrons so as to acquire a stable configuration.

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6
Q

Valence electron

A

Is the highest occupied energy level of an atom.

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7
Q

Bonding orbital

A

A molecular orbital whose energy is lower than that of the atomic orbital from which it is formed.

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8
Q

Dipole

A

A molecule that has two electrically charged regions.

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9
Q

Double covalent bond

A

A bond in which two pairs of electrons are shared by double two atoms.

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10
Q

Hydrogen bond

A

A relatively strong intermolecular force in which a hydrogen atom that is covalently bonded to a very electronegative atom.

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11
Q

Molecular orbital

A

An orbital resulting from the overlapping of atomic orbital when two atoms combine.

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12
Q

Non polar covalent bond

A

The weakest kind of intermolecular attraction; this attraction is thought to be caused by the motion of electrons.

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13
Q

Polar covalent bond

A

two different atoms are joined by a covalent bond unequally

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14
Q

Polar molecule

A

A molecule in which one or more atoms is slightly negative and one or more is slightly positive.

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15
Q

Single covalent bond

A

a type of chemical bond formed by the sharing of one pair of electrons between two atoms. It is a strong bond that holds atoms together in molecules.

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16
Q

Structural formula

A

A chemical formula that shows the arrangement mof atons in a molecule or a polyatomic ion.

17
Q

Tetrahedral angle

A

a bond angle of 109.5

18
Q

Triple covalent bond

A

A covalent bond in which three pairs of electrons are shared by two atoms.

19
Q

Vander Waals force

A

Weakest intermolecular attractions; includes dispersion forces and dipole interactions.

20
Q

VSEPR Theory

A

Molecules adjust their shapes so that valence-electron pairs are as far apart as possible.