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Sophomore- Spring 2024- Mac > Chem 111- Test 3- St. Thomas > Flashcards

Chem 111- Test 3- St. Thomas Flashcards

1
Q

absorbance

A

+

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2
Q

emission

A

-

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3
Q

orbital diagram

A

the thing w the lines

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4
Q

electron configuration

A

[the last nobel gas in row 18] and then the d, s, and p’s

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5
Q

what doesn’t need 8 around central atom

A

B and Be

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6
Q

principle quantum number

A

n. the shells

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7
Q

angular momentum or azimuthal quantum number

A

L, subshell (shape of orbital)

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8
Q

l=what on s orbital

A

0

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9
Q

l=what on p orbital

A

1

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10
Q

l=what on d orbital

A

2

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11
Q

magnetic quantum number

A

m(l), orientation of orbital (d- -2 to 2; s= 0, p= -1 to 1)

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12
Q

l=what on f orbital

A

3

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13
Q

spin quantium number

A

direction of the spin (+1/2 or -1/2)

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14
Q

transition metals in electron configuration

A

s and d orbitals only. also electron is removed from s orbital first

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15
Q

negative ion

A

= MORE electrons

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16
Q

positive ion

A

= LESS electrons

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17
Q

atomic radius

A

smaller left to right, larger top to bottom

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18
Q

ionization energy

A

energy required to move one elctron from an atom. higher left to right, lower top to bottom.

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19
Q

electron affinity

A

increase left to right, lower top to bottom

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20
Q

nonpolar covalent

A

electrons shared equally

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21
Q

polar covalent

A

electrons not shared equally

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22
Q

polar and nonpolar depend on what

A

electronegativity

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23
Q

electronegativity

A

increasing left to right, decreasing top to bottom

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24
Q

pure covalent number

A

less than 0.4

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25
Q

polar covalent number

A

between 0.4 and 1.8

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26
Q

ionic number

A

greater than 1.8

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27
Q

formal charge

A

valence electrons- (lone pair electrions + 1/2 bonding electrons)

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28
Q

bond order

A

sum of indiviedual bond orders/ mumber of bond groups

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29
Q

individual bond order

A

of bonds connecting atoms

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30
Q

breaking bonds ____ energy

A

requires (endothermic)

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31
Q

building bonds ____ energy

A

releases (exothermic)

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32
Q

size pattern

A

decreases up and decreases left to right

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33
Q

ionic bond strength

A
  1. charge
  2. size
34
Q

charge ionic bond strength

A

higher charge= higher bond strength (aka lattice energy)

35
Q

size bond strength

A

smaller ion = higher bond strength (lattice energy)

36
Q

____ bonds = higher melting points

A

stronger

37
Q

covalent bond strength

A
  1. # of bonds
  2. size
38
Q

reaction enthalpy

A

Ebonds broken- Ebonds formed

39
Q

bonds broken are the ____

A

reactants

40
Q

bonds formed are the____

A

products

41
Q

more bonds = ____ length

A

shorter

42
Q

electronic geometry-2 bonds + lone pairs

A

linear, 180 angle

43
Q

electronic geometry-3 bonds + lone pairs

A

trigonal planar, 120 degrees

44
Q

electronic geometry- 4 bonds + lone pairs

A

tetrahedral, all 109.5 degrees

45
Q

electronic geometry- 5 bonds + lone pairs

A

trigonal bipyramidal , angles of 90 or 120

46
Q

electronic geometry- 6 bonds + lone pairs

A

octahedral, angles 90 or 180

47
Q

trigonal planar with 1 lone pair

A

bent, angles left are less than 120 degrees

48
Q

tetrahedral one lone pair

A

trigonal pyramid, angles left are less than 109

49
Q

tetrahedral with 2 lone pairs

A

bent, but angles are less than 109

50
Q

trigonal bipyramid, one lone pair

A

seesaw, angles of less than 90 (straight to bottom) and less than 120 (between bottom 2)

51
Q

trigonal bipyramid, 2 lone pairs

A

t shape, angles of less than 90 degrees

52
Q

trigonal bipyramid, 3 lone pairs

A

linear, 180 degrees

53
Q

octahedral, 1 lone pair

A

square pyramid, ALL angles less than 90

54
Q

octahedral, 2 lone pair

A

square planar, 90 degrees

55
Q

octahedral, 3 lone pair

A

t shaped, less than 90 degrees

56
Q

octahedral, 4 lone pair

A

linear, 180 degrees

57
Q

localized

A

electrons in bonds. they take up less space because they are shared

58
Q

delocalized

A

lone pair electrons. they take more space because they are not shared

59
Q

angle distortion

A

lone pairs on central atoms will distort bond angles

60
Q

when is a it polar

A

when EG and MG are NOT the same. (this means there IS a dipole moment), OR if there are different bond types, it is also polar

61
Q

when is it nonpolar

A

when EG and MG are the same (no dipole moment)

62
Q

be able to write the s, d, and p orbitals

A

s on left (1 on top + helium on left), d in middle (3 on top (NOT 4)), p on right, (2 on top- not including helium)

63
Q

EG= linear, what is hybridization?

A

sp

64
Q

EG= trigonal planar, what is hybridization?

A

sp2

65
Q

EG= tetrahedral, what is hybridization?

A

sp3

66
Q

EG= trigonal bipyramidal, what is hybridization?

A

sp3d

67
Q

EG= octahedral, what is hybridization?

A

sp3d2

68
Q

hybrid orbital what do you do

A

the hybridization = the # of regions (i.e. sp2= 3 regions), then valence electrons = the spins (start with up, then go back with the extras as down spins)

69
Q

single bond (sigma and pi)

A

sigma bond

70
Q

double bond (sigma and pi)

A

1 sigma, 1 pi

71
Q

triple bond (sigma and pi)

A

1 sigma and 2 pi

72
Q

when can molecules rotate?

A

only in a single bond

73
Q

energy units

A

J/photon

74
Q

energy symbol

A

change in E

75
Q

wavelength

A

(the weird one)

76
Q

frequency

A

v

77
Q

when does it come out of s orbital first?

A

transition metals

78
Q

what takes 1 s and 10 d (the exceptions)

A

Cr and Cu

79
Q

shielding

A

electrons are repelled by other electrons in lower shells (so when its up vs down idk)

80
Q

the more negative energy is…

A

the higher electron affinity it has

81
Q

a high electron affinity has ____ energy value

A

negative

Sophomore- Spring 2024- Mac (11 decks)

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