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Honors Chem > Unit 6.1-6.3 Quiz > Flashcards

Unit 6.1-6.3 Quiz Flashcards

1
Q

what is the SI unit of measuring quantity

A

the mole

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2
Q

how many representative particles are in a mole

A

6.02*10^23

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3
Q

what is a representative particle

A

the smallest piece of matter of a substance that has the substance’s chemistry

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4
Q

what is the representative particle for a compound

A

the molecule

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5
Q

what is the representative particle for most elements

A

an atom

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6
Q

what are the diatomic elements

A

h2, n2, o2, f2, cl2, br2, i2

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7
Q

what are the three questions that rutheford’s model exposed?

A

how were the electrons arranged?
Why weren’t they being pulled into the nucleus?
What about atomic structure allowed different elements to give out different colored light?

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8
Q

what is electromagnetic radiation

A

its energy that moves through space like a wave

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9
Q

what is amplitude

A

the wave’s height from zero to crest

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10
Q

what is wavelength

A

the distance between the crests

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11
Q

what is frequency

A

the number of wave cycles to pass a given point per unit of time

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12
Q

the colors we see are called

A

the visible spectrum

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13
Q

the visible spectrum is just a small portion of wat

A

electromagnetic radiation

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14
Q

how fast does all electromagnetic radiation travel in a vacuum

A

at the speed of light

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15
Q

what two questions did scientists ask that couldn’t be explained with light simply as a wave

A

why does the same metal give off only specific wavelengths of light at certain temperatures?
and why do some metals emit electrons when exposed to only certain frequencies of light?

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16
Q

what did mac planck discover

A

he discovered that matter can only gain or lose energy in small specific amounts called quanta

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17
Q

the minimum amount of energy that can be gained or lost by an atom (not a set amount–depends on the atom and circumstances)

A

quantum

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18
Q

in this effect, electrons are emitted from the surface of a metal’s when light of a certain frequency or higher shines on the surface

A

photoelectric effect

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19
Q

who proposed that light isn’t a pure wave of energy

A

alber einstein

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20
Q

a massless particle that carries a quantum of energy and moves with a wavelike motion

A

photon

21
Q

what can be used to separate light into the colors that it contains

A

a prism

22
Q

the set of frequencies of the electromagnetic waves emitted by atoms of that element

A

atomic emission spectrum of an element

23
Q

which model explained the relationship between the atomic structure and light

A

bohr’s model/ the quantum model

24
Q

what did bohr state

A

that electrons moved around the nucleus in specific circular orbitals of defined energy

25
Q

the lowest possible state for an electron

A

ground state

26
Q

anything above the ground state

A

excited state

27
Q

what did bohr’s model explain

A

why the atomic emission spectrum for hydrogen only had certain wavelengths of light

28
Q

what question did bohr ask that allowed him to infer something about how orbitals were arranged

A

if the orbitals were evenly spaced, shouldn’t the wavelengths emitted be simple multiples of each other?

29
Q

what didnt bohrs model explain?

A

It didn’t explain how multiple electrons would not arrange themselves within the energy levels or whether or not you could have more than one electron in an energy level

30
Q

what is the heisenberg uncertainty principle

A

it states that you cannot know the position and velocity of an object at the same time

31
Q

what does the quantum mechanical model give us

A

it gives us an accurate description of how electrons arrange themselves in an atom, how many electrons in an energy level, the shape of the orbitals etc….

32
Q

energy levels

A

an electrons distance from the nucleus

33
Q

the shape of an electron cloud

A

sublevel

34
Q

the probable location for 2e-

A

atomic orbitals

35
Q

what letters describe the sublevel shapes

A

s,p,d,f

36
Q

what shape are s orbitals

A

spherical shape

37
Q

what shape are p orbitals

A

dumbbell shape

38
Q

what don’t we know about p orbitals

A

how the electrons get from one side to the other side

39
Q

what is the order of the sublevels for the little trick thing

A

1s, 2p, 3d, 4f

40
Q

how many electrons in s orbital

A

2e-

41
Q

how many electrons in p orbital

A

6e-

42
Q

how many electrons in d orbital

A

10e-

43
Q

how many electrons in f orbital

A

14e-

44
Q

this shows where each electrons in an atom is located

A

electron configuration

45
Q

states that each electron occupies the lowest energy orbital available

A

aufbau principle

46
Q

states that a maximum of two electrons can occupy a single atomic orbital, but only if the electrons have opposite spins

A

hund’s rule

47
Q

how are orbital diagrams expressed

A

arrows in boxes

48
Q

how are noble gas configurations expressed

A
  1. find preceding noble gas
  2. subtract noble gas electrons from element electrons
  3. start an s orbital with element role number
49
Q

how are electron notations/configurations expressed

A

write it out like 1s^2, 2s^2 etc

Honors Chem (10 decks)

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