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unit 7 Flashcards

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
steric number 1 EDG
linear
26
steric number 2 EDG
linear
27
steric number 3 EDG
trigonal planar
28
steric number 4 EDG
tetrahedral
29
steric number 5 EDG
trigonal bipyramidal
30
steric number 6 EDG
octahedral
31
expanded octet
stuff above steric number of 4, violates octet rule uses the d sublevel
32
bond angle linear
180 degrees
33
bond angle trigonal planar
120 degrees
34
bond angle bent steric number 3
less than 120 degrees
35
bond angle tetrahedral
109.5 degrees
36
bond angle trigonal pyramidal
107.3 degrees
37
bond angle bent steric number 4
104.5 degrees
38
Hybridization for linear steric # 1
s (if hydrogen) or sp^3
39
Hybridization for linear steric # 2
sp
40
Hybridization trigonal planar
sp^2
41
Hybridization for tetrahedral
sp^3
42
Hybridization for trigonal bipyramidal
sp^3d
43
Hybridization for octahedral
sp^3d^2
44
VSEPR for steric number 1 or 2
linear
45
VSEPR for steric number 3 no lone pairs
trigonal planar
46
VSEPR for steric number 3 one lone pair
bent
47
VSEPR for steric number 4 no lone pairs
tetrahedral
48
VSEPR for steric number 4 one lone pair
trigonal pyramidal
49
VSEPR for steric number 4 two lone pairs
bent
50
VSEPR for steric number 5 no lone pairs
trigonal bipyramidal
51
VSEPR for steric number 5 one lone pair
seesaw
52
VSEPR for steric number 5 two lone pairs
t-shaped
53
VSEPR for steric number 5 three lone pairs
linear
54
VSEPR for steric number 6 no lone pairs
octahedral
55
VSEPR for steric number 6 one lone pair
square pyramidal
56
VSEPR for steric number 6 two lone pairs
square planar
57
A in ABE
central atom
58
B in ABE
number of the other element bonded to the central atom
59
E in ABE
number of lone pairs on the central atom
60
VSEPR
Valence Shell Electron Pair Repulsions VSEPR theory assumes shape of a molecule based on repulsion between shared and lone electron pairs
61
each atom will achieve a geometry that ____
minimizes the repulsion between valence electrons, leaving maximum space between orbitals
62
lone pairs create _____ bond angles
lone pairs create smaller bond angles
63
change in bond angle that lone pairs create
roughly 2 degree difference (e.g. 109.5 to 107.3)
64
why do lone pairs change bond angles?
because single electrons repel from each other more
65
hybridization
mixing of s&p orbitals to create new hybrid orbitals (of equal energy) which become available during bonding
66
molecular polarity
NOT bond polarity, instead the polarity of the entire molecule e.g. water
67
how to determine a polar molecule
when a molecule is asymmetrical, the sharing of e's is uneven and molecule is polar bent molecules
68
how to determine a nonpolar molecule
when e's are distributed equally, symmetry bond dipoles cancel and there is no net molecular dipole also all diatomic atoms are nonpolar
69
can a molecule be nonpolar with polar bonds?
yes
70
can a molecule be polar with nonpolar bonds?
only if it also contains polar bonds
71
a lone pair on an atom will ________ the shape
distort
72
why is a molecule polar/nonpolar? (more abstract the answer depends on the molecule)
symmetrical vs nonsymmetrical, linear vs bent, has the same vs different kinds of atoms around center atom, lone pair, diatomic, etc.
73
intermolecular forces (IMF)
attractive forces between molecules
74
van der waals forces
intermolecular forces
75
intramolecular forces
forces which keep molecules together e.g. bonds
76
IMFs are ______ than intramolecular bonds
weaker
77
three types of IMFS
dipoles, hydrogen bonds, london dispersion forces
78
dipole-dipole interactions
IMF, an attraction between two non polar molecules who are oppositely charged partial positive and partial negative attract each other
79
cohesion
attraction between similar molecules
80
adhesion
attraction between different polar molecules
81
the greater the molecule polarity, the ____ the IMFs of the molecule will. be
stronger
82
Hydrogen bonds
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
examples of hydrogen bonds in molecules
NH3, H2O ofc, HF N O F
84
London dispersion forces (LDF)
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
a ______ melting temperature with _______ electrons creates a stronger london dispersion force in elements
higher/more
86
london dispersion forces are the primary IMF for ______
gases and nonpolar molecules
87
factor of LDF strength for molecules (not elements)
size of nonpolar molecules the bigger the size, the stronger the dispersion force
88
do all molecules have LDFs?
yes, but for polar molecules it's not the primary because the dipole-dipole and hydrogen bonds are stronger
89
covalent compounds all properties
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
why do covalent compounds have low MP and BP?
weak IMFs make bonds easy to break
91
why are covalent compounds solid liquid or gas @ room temp?
weak IMFs mean some bonds are broken at room temp and make some liquid or gas
92
why are covalent compounds soft or brittle solids?
weak IMFs make compounds easy to distort or break
93
why do covalent compounds have poor to no electrical/thermal conductivity? (solid or solution)
there are no mobile electrons in the internal structure and solids don't make mobile ions when dissolved
94
why do covalent compounds have variable solubility in water?
because the compound will not dissolve unless the solvent and solute are both nonmetals or both metals
95
network solids
an extended network of either carbon or silicon atoms held together by covalent bonds
96
in a network solid there are ____ individual molecules and it is considered a _______ _______ molecule
no/large macro
97
examples of network solids
diamond, graphite, silicon dioxide, silicon carbide
98
properties of network solids
same as covalent compounds except very hard and high melting/boiling points
99
why do network solids have high melting/boiling points and why are they hard?
the bonds are strong and there are so many bonds in the 'network' that it takes a lot of energy to break them
100
allotropes
different forms of the same element due to different bonding
101
example of allotropes
graphite and diamond (both carbon)

Chemistry (18 decks)

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