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Chemistry 103 > Exam 3 > Flashcards

Exam 3 Flashcards

1
Q

how are discrete line spectras produced

A

exciting a gas at a low partial pressure

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2
Q

formula for energy absorbed/emitted

A

hc/wavelength

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3
Q

quantized definition

A

a system is limited to specific energy values

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4
Q

when is a photon emitted

A

when an e- transitions from a ground state to an excited state

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5
Q

energy of a photon formula

A

h * v

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6
Q

relationship between electron energy and distance from nucleus

A

as one increases, so does the other

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7
Q

what is coulomb’s potential?

A

attractive force between a positive nucleus and an electron

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8
Q

important features of all orbital models

A

energies of electrons are quantized
electron energy increases with distance from nucleus
discrete energies (lines) in spectra come from quantized electronic energies

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9
Q

constructive intereference

A

peaks and troughs coincide to amplify

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10
Q

destructive interference

A

peaks and troughs conflict, cancels out

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11
Q

how to obtain probability density

A

square the wavefunction

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12
Q

principle quantum number

A

n
location of energy level/shell number

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13
Q

angular momentum quantum number

A

l
defines shape of orbital
any value from o to n-1

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14
Q

magnetic quantum number

A

m1
defines z component of l
ex. l = 1, m1 = -1, 0, +1

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15
Q

is absorption/emission of light endo or exothermic?

A

absorption: endothermic
emission: exothermic

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16
Q

wavefunction squaured …

A

probability of finding an electron at a given point near the position

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17
Q

radial distribution

A

total probability of finding an electron at a given distance (r) from the nucleus
- r increases with surface area

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17
Q

describe the electron density graph of the 1s orbital

A

starts high, goes lower, no nodes

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18
Q

describe the electron density graph of the 2s orbital

A

starts high, one node, one peak

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19
Q

describe the electron density graph of the 3s orbital

A

starts high, 2 nodes, one large peak, one smaller peak

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20
Q

describe the radial distribution graph of the 1s orbital

A

starts low, not at zero, one massive peak

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21
Q

describe the radial distribution graph of the 2s orbital

A

starts low, closer to zero, one node, two peaks second is larger than the first

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22
Q

describe the radial distribution graph of the 3s orbital

A

starts low, closer to zero, two nodes, three peaks getting progressively larger

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23
Q

orbitals in the nth energy level

A

n^2

24
Q

electrons in the nth energy level

A

2n^2

25
Q

orbitals in the l-subshell

A

2l + 1

26
Q

how many electrons can each orbital hold

A

2

27
Q

what is the pauli exclusion principle

A

no two e- can have the same set of 4 quantum numbers

28
Q

what l values correlate to subshells?

A

l = 0, s
l = 1, p
l = 2, d
l = 3, f

29
Q

difference between surface nodes and radial nodes

A

surface nodes (planar) are found at the original of the radial graphs, while radial nodes are not

30
Q

total nodes (surface + radial) =

A

n - 1

31
Q

surface/planar nodes =

A

l

32
Q

diamagnetic definition

A

all e- are paired

33
Q

paramagnetic definition

A

at least one unpaired e-

34
Q

isoelectronic definition

A

same #e-

35
Q

isovalent definition

A

same #valence e-

36
Q

what are degenerate orbitals

A

having the same energy

37
Q

what is effective nuclear charge

A

Zeff
- strength of the e- – nucleus interaction
- = Z (atomic number) - # core e-
- increases from left to right
- increases as electron subshell level decreases

38
Q

what are the common periodic table trends

A
  • atomic radii (size) increases from right to left and down
  • ionization energy (to remove an e- from a gaseous atom) increases left to right and up
  • electron affinity (energy change with addition of an e- to a neutral gas) more negative left to right and up
  • ionic radii –> anions are larger than cations
39
Q

definition of electronegativity

A

the degree to which an atom can attract an e- in a bond

40
Q

nonpolar covalent bond

A

equal sharing of e- between two identical nonmetal elements

41
Q

polar covalent

A

unequal sharing of e- between two nonmetals
small electronegativity difference

42
Q

ionic

A

metal + nonmetal
e- are transferred to nonmetal
large electronegativity difference

43
Q

as electronegativity increases, what happens to the following?
- bond polarity
- ionic character
- covalent character

A
  • increase
  • increase
  • decrease
44
Q

what is bond order

A

essentially, number of bonds
= # bonds/ # bond locations

45
Q

as bond order increases, what happens to the following?
- bond strength
- bond length
- bond dissociation energy

A
  • increase
  • decrease
  • increase
46
Q

what is formal charge

A

charge on an atom as determined by lewis dot structure
= #valence e- - #e- shown around atom in lewis dot structure

47
Q

what is needed for a lewis dot structure to contribute most in resonance?

A
  • smaller (ideally 0) formal charges
  • more zeros for formal charges
  • if formal charges are equal, the structure with the more negative formal charge on the more electronegative atom
48
Q

electron pair geometry versus molecular geometry

A

EPG:
- geometry including all domains (including lone pairs)
MG:
- refers to actual arrangement of atoms
- does not include lone pairs

49
Q

what is a dipole moment? when does it cancel?

A

dipole moment: measure of molecular polarity
- cancels when bond vectors cancel out –> nonpolar molecule
- when bond vectors create a net vector –> polar molecule

50
Q

relate VSEPR and polarity

A

(#atoms, #lone pairs)
POLAR: (2,1) (3,1) (2,2) (4,1) (3,2) (5,1)
NONPOLAR: (2,0) (3,0) (4,0) (5,0) (2,3) (6,0) (4,2) AND all atoms around central atom are the same

51
Q

are hydrocarbons polar or nonpolar?

A

nonpolar

52
Q

are binary atom molecules polar or nonpolar?

A

nonpolar

53
Q

are X-Y molecules polar or nonpolar?

A

polar

54
Q

where do sigma bonds lie

A

directly between the two nuclei of atoms

55
Q

what type of bond is in all single, double, or triple bond?

A

sigma

56
Q

compare sigma bonds and pi bonds

A

SIGMA
- can rotate
- symmetrical
- stronger
PI
- cannot rotate
- weaker

57
Q

where do pi bonds lie

A

above and below the internuclear axis

58
Q

what is required to make a pi bond?

A

two p-atomic orbitals

Chemistry 103 (1 decks)

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