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Chemistry > Chapter 6 > Flashcards

Chapter 6 Flashcards

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1
Q

chemical bond

A

attraction between nuclei and valence electrons of different atoms

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2
Q

how do atoms form compounds?

A

by gaining, losing, or sharing electrons

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3
Q

ionic bond

A

attraction between cations and anions

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4
Q

cation

A

metal

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5
Q

anion

A

nonmetal

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6
Q

covalent bond

A

sharing electrons between two nonmetals

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7
Q

non-polar covalent

A

bonding electrons are shared equally between bonding atoms

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8
Q

polar covalent

A

bonded atoms have an unequal attraction for shared electrons

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9
Q

list the bonds in order from least to greatest electronegative difference

A

non-polar covalent, polar covalent, ionic

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10
Q

molecule

A

neutral group of atoms held together by covalent bonds

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11
Q

molecular compound

A

chemical compound whose simplest units are molecules

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12
Q

chemical formula

A

indicates relative number of atoms of each kind in a chemical compound

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13
Q

molecular formula

A

shows types and numbers of atoms combined in a single molecule of a molecular compound

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14
Q

when do atoms have lower potential energy?

A

when bonded to other atoms

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15
Q

bond length

A

average distance between two bonded atoms at minimum potential energy

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16
Q

when do atoms release energy?

A

they release energy when forming covalent bonds

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17
Q

energy must be ______ to separate bonded atoms

A

added

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18
Q

when forming a covalent bond…

A

atoms’ shared electrons form overlapping orbitals

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19
Q

why do overlapping orbitals form?

A

achieves noble gas configuration/ stability

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20
Q

why are noble gases unreactive?

A

electron configurations are stable

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21
Q

how do atoms fill outermost p and s orbitals?

A

by sharing electrons through covalent bonding

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22
Q

exceptions to the octet rule?

A

some atoms can’t fit 8 valence electrons; others can fit more

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23
Q

how many electrons does Hydrogen need to form a bond and be stable?

A

only two

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24
Q

expanded valence

A

main group elements in periods three and up can form bonds involving more than 8 electrons

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25
Q

list the number of bonds in order of least to greatest energies

A

single < double < triple

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26
Q

resonance

A

other ways to write a Lewis form

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27
Q

ionic compound

A

cations and ions combined so the number of positive and negative charges are equal

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28
Q

what form do most ionic compounds exist as?

A

crystaline solids

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29
Q

can ionic compounds be separated into independent neutral units?

A

no

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30
Q

empirieal formula

A

simplest ratio of compound’s ions

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31
Q

mula unit

A

simplest collection of atoms from which ionic compound’s formula can be established

32
Q

Avagadro’s number

A

6.022 x 10^23

33
Q

how do ions minimize their potential energy?

A

by forming a crystal lattice

34
Q

crystal lattice

A

attractive forces exist between oppositely charged ions within a lattice; repulsive forces exist between like-charged ions

35
Q

what does combined repulsive forces within crystal lattices determine?

A

distance between ions and pattern of ions’ arrangement in crystal lattice

36
Q

differences between ionic and molecular compounds?

A
  • force that holds ions together in ionic compound is stronger than the one that holds together molecular compounds
  • molecular compounds melt at lower temps
37
Q

ionic compound properties

A
  • solids at room temp
  • very high melting point
  • hard but brittle
  • not electrical conductors in solid state because ions can’t move
38
Q

polyatomic ions

A

charged group of covalently bonded atoms

39
Q

metallic bonding properties

A
  • conductors of electricity
  • conductors of heat
  • malleability
  • ductility
  • shiny appearance
40
Q

metallic properties

A
  • electricity conductors
  • thermal conductors
  • malleable
    = ductile
  • shiny appearance
41
Q

delocalized electrons

A

electrons don’t belong to any one atom but are free to move freely about the metals’ network of empty atomic orbitals; forms a “sea of electrons” which then forms a crystal lattice

42
Q

metallic bonding

A

chemical bodning resulting from attraction between metal atoms and surrounding sea of electrons

43
Q

molecular geometry

A

3 d arrangement of molecules’ atoms with regular patterns and equal distances separating atoms not bonded to each other

44
Q

what two factors determine an electron’s polarity?

A

molecular shape and difference in electronegativity of the atoms

45
Q

VSPER theory

A

in a small molecule, pairs of valence electrons are arranged as far apart from each other as possible

46
Q

what does VSPER stand for?

A

Valence Shell Electron Pair Repulsion

47
Q

bond angle

A

geometric angle between 2 adjacent bonds

48
Q

linear

A

form a straight line; central atom bonded to two atoms with NO unshared pairs
o-o

49
Q

trigonal planar

A

flat triangle; atom has no unshared pairs of electrons o
|
o
/ \
o o

50
Q

bond angle of linear

A

180

51
Q

bond angle of trigonal planar

A

120

52
Q

tetrahedral

A

four surfaces; central angle bonded to four atoms, and central atom has no unshared pairs of electrons o
|
o
/ | \
o o o

53
Q

trigonal-pyramidal

A

central atom bonded to three other atoms and HAS an unshared pair of electrons

54
Q

at is true of trigonal-pyramidal models?

A

unshared pairs of electrons exert greater repulsion force because they’re held by only one atom

55
Q

bond angle of tetrahedral

A

109.5

56
Q

bond angle of trigonal-pyramidal

A

107

57
Q

bent

A

central atom bonded to two other atoms and has TWO unshared pairs of valence electronsq

58
Q

bond angle of bent

A

105

59
Q

atomic orbital

A

region around nucleus where electrons with a given energy are most likely to be found

60
Q

hybrid orbital

A

mixture of atomic orbitals formed when atoms approach each other to form a bond

61
Q

sp orbital

A

formed in linear molecules from mixing s and p orbitals

62
Q

sp^2

A

formed in trigonal planar molecules from mixing s and 2p orbitals

63
Q

sp^3

A

formed in tetrahedral, pyramidal, and bent molecules by mixing s and 3p orbitals

64
Q

intermolecular forces

A

force of attraction between molecules

65
Q

strength of intermolecular forces?

A

generally weaker than ionic, covalent, and metallic

66
Q

what is one measure of intermolecular forces?

A

boiling point; a higher boiling point shows higher attractive forces

67
Q

dipole

A

separation of two opposite charges by some distance

68
Q

induced dipole

A

created by presence of neighboring dipole

69
Q

dispersion force

A

force of attraction between neighboring dipoles

70
Q

do larger or smaller atoms have greater dispersion forces?

A

larger

71
Q

dipole-dipole force

A

attraction between opposite charges of neighboring permanent dipoles

72
Q

polar molecule has _________ dipoles

A

permanent

73
Q

what increases dipole moment?

A

greater difference in electronegativity

74
Q

Hydrogen bonding

A

force of attraction between Hydrogen and either Fluorine, Oxygen, or Nitrogen

75
Q

Hydrogen

A

one of the least electronegative elements

76
Q

Fluorine, Oxygen, NItrogen

A

the most electronegative elements

77
Q

strength of Hydrogen bonds

A

very strong

Chemistry (8 decks)

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