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Chemistry > Chapter 6 > Flashcards

Chapter 6 Flashcards

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
list the number of bonds in order of least to greatest energies
single < double < triple
26
resonance
other ways to write a Lewis form
27
ionic compound
cations and ions combined so the number of positive and negative charges are equal
28
what form do most ionic compounds exist as?
crystaline solids
29
can ionic compounds be separated into independent neutral units?
no
30
empirieal formula
simplest ratio of compound's ions
31
mula unit
simplest collection of atoms from which ionic compound's formula can be established
32
Avagadro's number
6.022 x 10^23
33
how do ions minimize their potential energy?
by forming a crystal lattice
34
crystal lattice
attractive forces exist between oppositely charged ions within a lattice; repulsive forces exist between like-charged ions
35
what does combined repulsive forces within crystal lattices determine?
distance between ions and pattern of ions' arrangement in crystal lattice
36
differences between ionic and molecular compounds?
- 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
ionic compound properties
- solids at room temp - very high melting point - hard but brittle - not electrical conductors in solid state because ions can't move
38
polyatomic ions
charged group of covalently bonded atoms
39
metallic bonding properties
- conductors of electricity - conductors of heat - malleability - ductility - shiny appearance
40
metallic properties
- electricity conductors - thermal conductors - malleable = ductile - shiny appearance
41
delocalized electrons
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
metallic bonding
chemical bodning resulting from attraction between metal atoms and surrounding sea of electrons
43
molecular geometry
3 d arrangement of molecules' atoms with regular patterns and equal distances separating atoms not bonded to each other
44
what two factors determine an electron's polarity?
molecular shape and difference in electronegativity of the atoms
45
VSPER theory
in a small molecule, pairs of valence electrons are arranged as far apart from each other as possible
46
what does VSPER stand for?
Valence Shell Electron Pair Repulsion
47
bond angle
geometric angle between 2 adjacent bonds
48
linear
form a straight line; central atom bonded to two atoms with NO unshared pairs o-o
49
trigonal planar
flat triangle; atom has no unshared pairs of electrons o | o / \ o o
50
bond angle of linear
180
51
bond angle of trigonal planar
120
52
tetrahedral
four surfaces; central angle bonded to four atoms, and central atom has no unshared pairs of electrons o | o / | \ o o o
53
trigonal-pyramidal
central atom bonded to three other atoms and HAS an unshared pair of electrons
54
at is true of trigonal-pyramidal models?
unshared pairs of electrons exert greater repulsion force because they're held by only one atom
55
bond angle of tetrahedral
109.5
56
bond angle of trigonal-pyramidal
107
57
bent
central atom bonded to two other atoms and has TWO unshared pairs of valence electronsq
58
bond angle of bent
105
59
atomic orbital
region around nucleus where electrons with a given energy are most likely to be found
60
hybrid orbital
mixture of atomic orbitals formed when atoms approach each other to form a bond
61
sp orbital
formed in linear molecules from mixing s and p orbitals
62
sp^2
formed in trigonal planar molecules from mixing s and 2p orbitals
63
sp^3
formed in tetrahedral, pyramidal, and bent molecules by mixing s and 3p orbitals
64
intermolecular forces
force of attraction between molecules
65
strength of intermolecular forces?
generally weaker than ionic, covalent, and metallic
66
what is one measure of intermolecular forces?
boiling point; a higher boiling point shows higher attractive forces
67
dipole
separation of two opposite charges by some distance
68
induced dipole
created by presence of neighboring dipole
69
dispersion force
force of attraction between neighboring dipoles
70
do larger or smaller atoms have greater dispersion forces?
larger
71
dipole-dipole force
attraction between opposite charges of neighboring permanent dipoles
72
polar molecule has _________ dipoles
permanent
73
what increases dipole moment?
greater difference in electronegativity
74
Hydrogen bonding
force of attraction between Hydrogen and either Fluorine, Oxygen, or Nitrogen
75
Hydrogen
one of the least electronegative elements
76
Fluorine, Oxygen, NItrogen
the most electronegative elements
77
strength of Hydrogen bonds
very strong

Chemistry (8 decks)

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