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Chem 110 > Exam 1 (chapters 1-4) > Flashcards

Exam 1 (chapters 1-4) Flashcards

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1
Q

10^6

A

mega- (M)

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2
Q

10^-6

A

micro- (µ)

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3
Q

10^-9

A

nano- (n)

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4
Q

Aufbau Principle

A

e- fills the lowest energy level first

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5
Q

3*10^8 m/s

A

Speed of light

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6
Q

Hund’s Rule

A

-e filled in the same energy level in 1 orbital at a time and is oriented in the same direction

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7
Q

no two e- in an orbital can have the same spin

A

Pauli Exclusion Principle

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8
Q

the ion with the most protons is the smallest b/c there are more protons in the nucleus to pull fewer e- in the shells

A

for ions of an isoelectric series:

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9
Q

How can you tell if an element is in an excited state from the electron configuration?

A

subshells that are not the last sub shell are not filled

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10
Q

ℓ =0

A

Sub-shell s
-spherical

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11
Q

ℓ=1

A

sub-shell p
3 orbitals
dumbbell shape

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12
Q

ℓ=2

A

Sub-shell d
5 orbitals
cloverleaf shaped

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13
Q

ℓ=3

A

Sub-shell f
7 orbitals

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14
Q

Cr electron configuration

A

[Ar]4s^1 3d^5

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15
Q

(2 *ℓ)+1

A

number of orbital or _ in a configuration

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16
Q

Cu electron configuration

A

[Ar] 4s^1 3d^10

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17
Q

Electron affinity (EA)

A

The energy change associated with the addition of an electron to a gaseous atom

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18
Q

energy absorbed during the gain of an e-

A

EA is endothermic

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19
Q

energy is released during the gain of an e-

A

EA is exothermic

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20
Q

an atom is ionized when

A

an e- is leaving an atom; n(final)=∞

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21
Q

attractive interactions are

A

negative

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22
Q

repulsive interactions are

A

positive

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23
Q

atoms of the same element with different neutrons

A

isotopes

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24
Q

mechanical kinetic energy

A

-moving mass
-mechanical pot. energy
-stored mass in a place where a force acts

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25
Q

electrical kinetic energy

A

-moving charge
-electrostatic pot. energy b/c or the interaction of charged particles

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26
Q

light kinetic energy

A

-moving photons
-chemical pot. energy
-stored in bonds

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27
Q

heat enters a system

A

+q

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28
Q

heat leaves a system

A

-q

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29
Q

work is done on a system

A

+w

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30
Q

work is done by the system

A

-w

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31
Q

state function

A

a function that depends only on the initial and final states of a system, not the path in between.
-represented by uppercase letters, P, V, H, T

32
Q

electrostatic energy

A

proportional to the magnitude of the charges
inverse to the distance between particles

33
Q

enthalpy

A

heat transferred at a constant pressure

34
Q

exothermic process

A

when energy (often as heat) leaves a system into the surroundings

35
Q

endothermic process

A

energy (as heat) is added to a system

36
Q

hc/λ

A

E(photon)=

37
Q

Gamma ray wavelength range

A

<10^-8

38
Q

UV and visible wavelength range

A

10^-8 to 10^-6

39
Q

infrared wavelength range

A

10^-6 to 10^-4

40
Q

microwave wavelength range

A

10^-4 to 10^-1

41
Q

radio wavelength range

A

10^0 to 10^4

42
Q

black body radiaiton

A

radiation emitted by an object

43
Q

when light is reflected or transmitted…

A

the complementary color is absorbed

44
Q

transmitted light

A

is not absorbed, passes through

45
Q

when interacting with matter, gamma rays, x rays, UV rays…

A

-ionize atoms and molecules
-break chemical bonds

46
Q

when visible spectrum rays interact with matter (electronic transitions)

A

e- is promoted to higher energy

47
Q

when infrared rays interact w matter

A

increased amplitude of vibrations (KE goes up)

48
Q

microwave interactions with matter

A

rotations increase

49
Q

radio waves…

A

flip nuclear spin

50
Q

lowest energy is when

A

closest to p+ (ground state)

51
Q

electron transition causes

A

e- moves from one allowed energy state to another
e- changes energy levels emitting/absorbing photons

52
Q

principle quantum number (n)

A

-info on orbital size
-defines what shell e- is in
info on orbital energy

53
Q

quantum number ℓ

A

determines shape

54
Q

magnetic quantum number (mℓ)

A

-describes orientation of orbital in 3D space
- ranges from -ℓ to ℓ

55
Q

node

A

no electrons
n-1=nodes

56
Q

core shielding

A
  • inner e- shield valence e- from nucleus
  • outer e- experience less Ze and have a weak attraction
  • outer e- have less energy
57
Q

atomic radius

A

increases down a group
decreases across a period

58
Q

ionization energy

A

energy needed to remove e- in gaseous state
always positive
increases across a period
decreases down a group

59
Q

Zeff for valence e-

A

increases down a group and across a period

60
Q

EA is more negitive

A

across a period

61
Q

size of ion relative to parent atom

A

anion>parent>cation

62
Q

isoelectic series

A

group of atoms or ions that have the same number of e- (same ground state configuration)

63
Q

effective nuclear charge (Zeff)

A

net positive charge experienced by valence e-

64
Q

when valence e- are further from the nucleus

A

more reactive

65
Q

metallic character and reactivity increase

A

as ionization energy decreases

66
Q

IE=

A

energy needed to form a positive ion

67
Q

E(g) –> (E+) + (e-)

A

ionization energy representation

68
Q

electron affinity representation

A

E(g) + (e-) –> E(g)-

69
Q

p block elements, nonmetals

A

elements that have ionization energies > 1000

70
Q

metals s,d,f block elements

A

elements that IE<1000

71
Q

potential energy

A

-stored energy
- not a state function (path matters)

72
Q

1000J

A

1KJ

73
Q

Planck’s Constant

A

6.63*10^-34 m^2kg/s

74
Q

Avogadro’s Number

A

6.02*10^23

75
Q

Moles to grams conversion

A

of moles * molar mass

Chem 110 (2 decks)

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