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Chemistry > Chapter 8 > Flashcards

Chapter 8 Flashcards

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1
Q

Covalent bond

A

atoms share electrons

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2
Q

Molecule

A

neutral group of atoms joined by covalent bonds

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3
Q

Diatomic molecule

A

consisting of two atoms (e.g. oxygen molecule)

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4
Q

Molecular compound

A

a compound composed of molecules

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5
Q

Molecular compound melting point

A

relatively lower than those of ionic compounds

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6
Q

Molecular formula

A

chemical formula of a molecular compound, shows how many atoms of each element a molecule contains

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7
Q

Octet rule

A

atoms share to attain the electron configuration of noble gases

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8
Q

Single covalent bond

A

two atoms held by sharing a pair of electrons, shown by a bar

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9
Q

Double and triple covalent bonds

A

formed if the atoms can achieve the electron structure of noble gases

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10
Q

Coordinate covalent bond

A

a covalent bond in which one atom contributes both bonding electrons

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11
Q

Polyatomic ion

A

a tightly bound group of atoms that has a charge and behaves as a unit

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12
Q

Bond dissociation energies

A

the energy needed to break the bond between two covalently bonded atoms, large energy corresponds to a strong bond

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13
Q

A resonance structure

A

a structure that occurs when it’s possible to draw two or more valid electron dot structures that have the same number of electron pairs for a molecule or ion

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14
Q

Exceptions to the octet rule

A

cannot be satisfied in molecules whose total # of valence electron is an odd #

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15
Q

Molecular orbitals

A

when two atoms combine, this model assumes that their orbitals overlap to produce molecular orbitals

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16
Q

Molecular orbitals belong to

A

a molecule as a whole

17
Q

Bonding orbital

A

a molecular orbital that can be occupied by two electrons of a covalent bond

18
Q

Sigma

A

symmetrical molecular orbital

19
Q

Pi

A

sausage-shaped molecular orbital, asymmetrical

20
Q

VSEPR theory

A

the repulsion between electron pairs causes molecular shapes to adjust so that the valence electron pairs stay as far apart as possible

21
Q

Orbital hybridization

A

provides information about both molecular bonding and molecular shape

22
Q

What happens in hybridization?

A

several atomic orbitals mix to form the total # of equivalent hybrid orbitals

23
Q

Non polar covalent bonds

A

when the atoms pull equally in the bond

24
Q

Polar covalent bond

A

when the atoms pull unequally in the bond

25
Q

The more electronegative atom

A

attracts electrons more strongly and gains a slightly negative chard

26
Q

The less electronegative atom

A

has a slightly positive charge

27
Q

Polar molecules

A

one end is slightly negative, the other end is slightly positive

28
Q

Dipole

A

a molecule that has two poles

29
Q

When polar molecules are placed between oppositely charged plates, what happens?

A

they tend to become oriented to the respective positive and negatively charged plates

30
Q

Intermolecular attractions

A

weaker than with ionic or covalent bonds

31
Q

Van der Waals forces

A

the two weakest attractions between molecules

32
Q

Dipole interactions

A

when polar molecules are attracted to one another

33
Q

Dispersion forces

A

weakest of all, caused by the motions of electrons

34
Q

Hydrogen bonds

A

a hydrogen covalently bonded to a very electronegative atom is weakly bonded to an unshared electron pair of another electronegative atom

35
Q

Network solids

A

solids in which all of the atoms are covalently bonded to each other

36
Q

Melting a network solid

A

requires breaking covalent bonds throughout a solid

37
Q

An example of a network solid

A

diamond

38
Q

Widely varying intermolecular attractions cause

A

a great range of physical properties among covalent compounds

Chemistry (13 decks)

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