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Chem 103 > Exam 1 > Flashcards

Exam 1 Flashcards

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1
Q

first controlled reaction

A

fire

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2
Q

Aristotle believed in…

A

unlimited divisions of matter, not true

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3
Q

Democritus believed in…

A

limited divisions, true = atom as smallest fundamental unit

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4
Q

law

A

describes an observation, answers “what”?

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5
Q

theory

A

explains an observation, answers “how” and “why”? (think conspiracy theories)

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6
Q

Law of Conservation of Mass

A

matter is neither created or destroyed

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7
Q

Law of Definite Proportions

A

a substance is always made of the same proportion of elements

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8
Q

Law of Multiple Proportions/Constant Composition

A

elements combine in small whole number ratios (multiples)

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9
Q

Dalton’s Atomic Theory (5 parts, 2 proven wrong)

A
  1. Matter composed of small, indivisible particles (=atoms)
  2. Atoms of a particular element are identical*
  3. Atoms combine in small, whole number ratios
  4. Atoms are neither created or destroyed*
  5. Atoms of different elements are different
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10
Q

J.J. Thomson findings

A
  • discovered the electron (cathode rays are negatively charged particles), creating the plum pudding model in response
  • discovered applying force caused acceleration
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11
Q

Millikan findings

A
  • discovered the mass and charge of an electron

- the electric field must be a multiple of the charge of an electron to suspend particles

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12
Q

Rutherford findings in gold foil experiment

A
  • positive charge located in one dense area: nucleus
  • neutral particles with mass also here: neutrons
  • atom is mostly empty space
  • created the nuclear model of the atom: nucleus as very tiny and atom as huge and largely open space
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13
Q

Mass defect

A

difference between the predicted mass and the actual mass of an atom’s nucleus

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14
Q

Z

A

atomic number, number of protons (and electrons in neutral atom), written on bottom

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15
Q

A

A

atomic mass, # of protons and neutrons, written on top

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16
Q

to determine number of neutrons…

A

mass # - protons

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17
Q

isotopes

A

atoms of the same element with different number of neutrons (as evident through mass number)

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18
Q

ions

A

atoms that are not neutral due to different numbers of protons and electrons

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19
Q

atomic mass

A

weighted average between atomic mass of natural abundance of isotopes of an element

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20
Q

Avogadro’s number

A

6.02 x 10^23 (just a number, no units)

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21
Q

how are E, frequency, wavelength related?

A

as E and frequency increase, wavelength decreases

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22
Q

on color spectrum of light, which colors are high E/low E?

A

Reds are low E, blues are high E

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23
Q

photoelectric effect

A

the emission of electrons when light hits a material

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24
Q

photon

A

particle of light

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25
Q

Planck’s constant relates to…

A

light /E of photon

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26
Q

work function

A

E of a photon necessary to remove an electron from metal via the photoelectric effect

27
Q

What does Rydberg’s equation measure?

A

predicts the transitions between quantized energy levels (n) based off of wavelength (and vice versa)

28
Q

Bohr

A

made first model of the atom with quantized electrons; problems: only works for 1 electron atoms and treats electrons classically

29
Q

de Broglie equation

A

how to find wavelength

30
Q

de Broglie equation

A

how to find wavelength, mass must be in kg and velocity in meters/second

31
Q

microscopic particles are best considered to be

A

waves

32
Q

uncertainty principle

A

it’s impossible to know simultaneously and exactly the position and momentum of a microscopic particle

33
Q

wave function

A

electrons described as standing waves

34
Q

standing waves

A

waves that don’t travel

35
Q

(wave function)^squared

A

describes the likelihood of finding an electron at a particular point in space (a sort of probability density map)

36
Q

quantum numbers

A

describe where a particular electron is within an atom

37
Q

atomic orbital

A

where electrons are likely to be found for each possible quantum state

38
Q

principle quantum number = n

A
  • shells, distance from nucleus
  • coordinates to periods
  • higher n = higher E
39
Q

angular momentum quantum number = l

A
  • subshells
  • describes an orbital’s shape
  • s,p,d,f
40
Q

circle node and how to find

A

radial/spherical, what’s leftover

41
Q

line node and how to find

A

planar/angular; l

42
Q

how to find total nodes

A

n-1

43
Q

magnetic quantum number = m sub l

*helpful for remembering what l corresponds to n if you look at picture/energy table

A
  • number of orbitals in each subshell
  • for l=0, 1 orbital
  • for l=1, 3 orbitals
  • for l-2, 5 orbitals
  • for l=3, 7 orbitals
  • to help remember, look at electron config
44
Q

pauli exclusion principle

A

no 2 electrons in one atom can have same set of quantum numbers, caused spin quantum number to be created

45
Q

spin quantum number = M sub s

A

+1/2, -1/2

spin direction of electron

46
Q

aufbau principle

A

electrons in ground state atom (low E) occupy the lowest energy orbitals available to them first then move up

47
Q

shielding

A

attraction between an electron and the nucleus in an atom with multiple electrons

48
Q

Z effective

A

nuclear charge that electrons feel

49
Q

relationship between Z actual and Z effective in multi electron atom

A

Z effective < Z actual

if there is more than one electron, don’t feel full pull of nucleus = farther away

50
Q

closed shell

A

full outermost shell

51
Q

how to find an elements inner and valence electrons

A
  • inner: look at Z of last noble gas

- valence: what’s left

52
Q

hund’s rule

A

equal E orbitals are singly filled before they are fully filled

53
Q

d-block anomaly #1

A

it is particularly stable for d-orbitals to be half-filled or fully-filled. 1 s-orbital electron is moved to d-orbital to satisfy this

54
Q

isoelectronic

A

atoms/ions with identical electron configurations

55
Q

d-block anomaly #2

A

when losing electrons, d-orbital elements lose both valence shell s-orbital electrons before losing d-orbital electrons (applies to ions)

56
Q

periodic trends: to go up/down table use

A

n

57
Q

periodic trends: to go left/right table use

A

z

58
Q

why use Slater’s Rules

A

to approximate Z effective

59
Q

periodic trends: Z effective

A

up/down table (as n goes up), Z eff goes up

as z goes up (move left to right), Z eff goes up

60
Q

periodic trends: atomic radius

A

as n goes up (move down table), radius goes up

as z goes up (move left to right), radius goes down

61
Q

periodic trends: ionization energy

A
  • as n goes up (move up to down), IE goes down

- as z goes up (move L to R), IE goes up

62
Q

periodic trend: ion radius

A
  • as ions lose electrons, radius decreases ( = less pull)

- as ions gain electrons, radius increases

63
Q

electron affinity (EA)

A

the E released when an electron is added to an atom

  • very general
  • EA increases as you move across and up the periodic table

Chem 103 (1 decks)

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