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Chemistry > unit 7 > Flashcards

unit 7 Flashcards

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1
Q

Lewis Dot Models

A

shows valence shells of electrons

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2
Q

Bonding domains

A

in covalent bonds, places where electrons are shared

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3
Q

covalent bond

A

a bond formed when two non-metallic atoms share valence electrons

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4
Q

difference between covalent and ionically bonded electrons

A

in covalent bonds electrons are shared, in ionic bonds electrons are fully transferred

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5
Q

why are bonds formed?

A

to have a full valence shell, the octet rule

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6
Q

nonmetals’ IE and ENEG

A

nonmetals have high IE (easy to lose electrons), (high ENEG (easy to gain electrons) and high Zeff (valence e’s have high attraction to nucleus)

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7
Q

How are shared electrons represented in LDMs

A

a dash between atoms (H-H) or two dots between atoms (H:H) (used on regents)

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8
Q

How to draw LDMs for covalent compounds

A
  1. add total valence e’s
  2. create the structure for the compound
    • least ENEG goes in the middle
    • H RULE: never place hydrogen or a halogen in the middle
  3. subtract e’s for each bond
  4. place e’s around outer atoms to satisfy octet rule
  5. make sure central and other atoms have 8 atoms and if not make multiple bonds
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9
Q

Molecular geometry/molecular structure

A

the structure of atoms in a molecule
- each atom in a molecule wi; achieve a geometry that minimizes repulsion between valence e’s

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10
Q

Polyatomic ions LDMs

A

same thing but if it says ‘ion’ make sure to add or subtract that number of electrons form total before doing anything. After done put brackets around and write the charge
-PAIs bond ionically but internally they have covalent bonds

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11
Q

Resonance

A

theory that there is no single conventional LDM that represents PAIs.

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12
Q

resonance structure

A

a form of an LDM for a PAI. (e.g. NO3- has 3 resonance structures)

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13
Q

Sigma bond

A

only 1 shared pair of electron domain
-the electron density is concentrated
-‘head to head’ along the internuclear axis (the line connecting the nuclei)

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14
Q

pi bond

A

result of multiple bonds
on the outside of sigma bonds
formed by the lateral overlap of parallel p orbitals (side by side) on bonded atoms

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15
Q

Polar covalent bond

A

made when atoms with different electronegativities share electrons in a covalent bond
-shared electron pair is displaced toward the more electronegative atom
-defined by NYS as having a END of 0.5-1.6

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16
Q

nonpolar covalent bond

A

made when electrons shared equally between atoms
both atoms in the bond have the same or similar ENEG
-defined by NYS as having a END of 0.0-0.4

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17
Q

When hydrogen is bonded to any nonmetal, the bond is always ______

A

covalent

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18
Q

ionic bond END

A

≥ 1.7

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19
Q

END

A

Electronegativity difference
-determines bond type

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20
Q

Ionic character

A

the degree of bond polarity shows likeness to an ionic bond

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21
Q

dipoles / partial charges

A

minor charges created at the ends of the shared electron pair
only occurs in polar covalent bonds
represented by lowercase delta s lookin thing

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22
Q

dipole vectors

A

help illustrate bond polarity in a bonding domain
arrows pointing at negative end with ‘+’ at positive end
e.g. H +-> F

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23
Q

steric number

A

of atoms, groups, or lone shared pairs around an atom in a molecule
double and triple bonds count as one domain

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24
Q

electron domain geometry (EDG)

A

molecules get a classification based on the number of electron locations (steric number) of the LDM (domains)

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25
Q

steric number 1 EDG

A

linear

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26
Q

steric number 2 EDG

A

linear

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27
Q

steric number 3 EDG

A

trigonal planar

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28
Q

steric number 4 EDG

A

tetrahedral

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29
Q

steric number 5 EDG

A

trigonal bipyramidal

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30
Q

steric number 6 EDG

A

octahedral

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31
Q

expanded octet

A

stuff above steric number of 4, violates octet rule
uses the d sublevel

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32
Q

bond angle linear

A

180 degrees

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33
Q

bond angle trigonal planar

A

120 degrees

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34
Q

bond angle bent steric number 3

A

less than 120 degrees

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35
Q

bond angle tetrahedral

A

109.5 degrees

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36
Q

bond angle trigonal pyramidal

A

107.3 degrees

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37
Q

bond angle bent steric number 4

A

104.5 degrees

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38
Q

Hybridization for linear steric # 1

A

s (if hydrogen) or sp^3

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39
Q

Hybridization for linear steric # 2

A

sp

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40
Q

Hybridization trigonal planar

A

sp^2

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41
Q

Hybridization for tetrahedral

A

sp^3

42
Q

Hybridization for trigonal bipyramidal

A

sp^3d

43
Q

Hybridization for octahedral

A

sp^3d^2

44
Q

VSEPR for steric number 1 or 2

A

linear

45
Q

VSEPR for steric number 3 no lone pairs

A

trigonal planar

46
Q

VSEPR for steric number 3 one lone pair

A

bent

47
Q

VSEPR for steric number 4 no lone pairs

A

tetrahedral

48
Q

VSEPR for steric number 4 one lone pair

A

trigonal pyramidal

49
Q

VSEPR for steric number 4 two lone pairs

A

bent

50
Q

VSEPR for steric number 5 no lone pairs

A

trigonal bipyramidal

51
Q

VSEPR for steric number 5 one lone pair

A

seesaw

52
Q

VSEPR for steric number 5 two lone pairs

A

t-shaped

53
Q

VSEPR for steric number 5 three lone pairs

A

linear

54
Q

VSEPR for steric number 6 no lone pairs

A

octahedral

55
Q

VSEPR for steric number 6 one lone pair

A

square pyramidal

56
Q

VSEPR for steric number 6 two lone pairs

A

square planar

57
Q

A in ABE

A

central atom

58
Q

B in ABE

A

number of the other element bonded to the central atom

59
Q

E in ABE

A

number of lone pairs on the central atom

60
Q

VSEPR

A

Valence Shell Electron Pair Repulsions
VSEPR theory assumes shape of a molecule based on repulsion between shared and lone electron pairs

61
Q

each atom will achieve a geometry that ____

A

minimizes the repulsion between valence electrons, leaving maximum space between orbitals

62
Q

lone pairs create _____ bond angles

A

lone pairs create smaller bond angles

63
Q

change in bond angle that lone pairs create

A

roughly 2 degree difference (e.g. 109.5 to 107.3)

64
Q

why do lone pairs change bond angles?

A

because single electrons repel from each other more

65
Q

hybridization

A

mixing of s&p orbitals to create new hybrid orbitals (of equal energy) which become available during bonding

66
Q

molecular polarity

A

NOT bond polarity, instead the polarity of the entire molecule e.g. water

67
Q

how to determine a polar molecule

A

when a molecule is asymmetrical, the sharing of e’s is uneven and molecule is polar
bent molecules

68
Q

how to determine a nonpolar molecule

A

when e’s are distributed equally, symmetry
bond dipoles cancel and there is no net molecular dipole
also all diatomic atoms are nonpolar

69
Q

can a molecule be nonpolar with polar bonds?

A

yes

70
Q

can a molecule be polar with nonpolar bonds?

A

only if it also contains polar bonds

71
Q

a lone pair on an atom will ________ the shape

A

distort

72
Q

why is a molecule polar/nonpolar? (more abstract the answer depends on the molecule)

A

symmetrical vs nonsymmetrical, linear vs bent, has the same vs different kinds of atoms around center atom, lone pair, diatomic, etc.

73
Q

intermolecular forces (IMF)

A

attractive forces between molecules

74
Q

van der waals forces

A

intermolecular forces

75
Q

intramolecular forces

A

forces which keep molecules together e.g. bonds

76
Q

IMFs are ______ than intramolecular bonds

A

weaker

77
Q

three types of IMFS

A

dipoles, hydrogen bonds, london dispersion forces

78
Q

dipole-dipole interactions

A

IMF, an attraction between two non polar molecules who are oppositely charged
partial positive and partial negative attract each other

79
Q

cohesion

A

attraction between similar molecules

80
Q

adhesion

A

attraction between different polar molecules

81
Q

the greater the molecule polarity, the ____ the IMFs of the molecule will. be

A

stronger

82
Q

Hydrogen bonds

A

strongest IMF
an abnormally strong dipole-dipole attraction
hydrogen gives away their only electron in bonding, leaving a very positive nucleus with no shielding

83
Q

examples of hydrogen bonds in molecules

A

NH3, H2O ofc, HF
N O F

84
Q

London dispersion forces (LDF)

A

weakest IMF
at random electrons move to create a momentary dipole, which causes the nearby molecules to create dipoles as well in repulsion/attraction and creates an IMF

85
Q

a ______ melting temperature with _______ electrons creates a stronger london dispersion force in elements

A

higher/more

86
Q

london dispersion forces are the primary IMF for ______

A

gases and nonpolar molecules

87
Q

factor of LDF strength for molecules (not elements)

A

size of nonpolar molecules
the bigger the size, the stronger the dispersion force

88
Q

do all molecules have LDFs?

A

yes, but for polar molecules it’s not the primary because the dipole-dipole and hydrogen bonds are stronger

89
Q

covalent compounds all properties

A

low MP and BP, gas liquid or solid @ room temp, soft and brittle solids, variable solubility in water, poor to no electrical/thermal conductivity

90
Q

why do covalent compounds have low MP and BP?

A

weak IMFs make bonds easy to break

91
Q

why are covalent compounds solid liquid or gas @ room temp?

A

weak IMFs mean some bonds are broken at room temp and make some liquid or gas

92
Q

why are covalent compounds soft or brittle solids?

A

weak IMFs make compounds easy to distort or break

93
Q

why do covalent compounds have poor to no electrical/thermal conductivity? (solid or solution)

A

there are no mobile electrons in the internal structure and solids don’t make mobile ions when dissolved

94
Q

why do covalent compounds have variable solubility in water?

A

because the compound will not dissolve unless the solvent and solute are both nonmetals or both metals

95
Q

network solids

A

an extended network of either carbon or silicon atoms held together by covalent bonds

96
Q

in a network solid there are ____ individual molecules and it is considered a _______ _______ molecule

A

no/large macro

97
Q

examples of network solids

A

diamond, graphite, silicon dioxide, silicon carbide

98
Q

properties of network solids

A

same as covalent compounds except very hard and high melting/boiling points

99
Q

why do network solids have high melting/boiling points and why are they hard?

A

the bonds are strong and there are so many bonds in the ‘network’ that it takes a lot of energy to break them

100
Q

allotropes

A

different forms of the same element due to different bonding

101
Q

example of allotropes

A

graphite and diamond (both carbon)

Chemistry (18 decks)

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