Unit 6.1-6.3 Quiz

Question 1

what is the SI unit of measuring quantity

Answer 1

the mole

Question 2

how many representative particles are in a mole

Answer 2

6.02*10^23

Question 3

what is a representative particle

Answer 3

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

Question 4

what is the representative particle for a compound

Answer 4

the molecule

Question 5

what is the representative particle for most elements

Answer 5

an atom

Question 6

what are the diatomic elements

Answer 6

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

Question 7

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

Answer 7

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?

Question 8

what is electromagnetic radiation

Answer 8

its energy that moves through space like a wave

Question 9

what is amplitude

Answer 9

the wave’s height from zero to crest

Question 10

what is wavelength

Answer 10

the distance between the crests

Question 11

what is frequency

Answer 11

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

Question 12

the colors we see are called

Answer 12

the visible spectrum

Question 13

the visible spectrum is just a small portion of wat

Answer 13

electromagnetic radiation

Question 14

how fast does all electromagnetic radiation travel in a vacuum

Answer 14

at the speed of light

Question 15

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

Answer 15

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?

Question 16

what did mac planck discover

Answer 16

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

Question 17

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

Answer 17

quantum

Question 18

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

Answer 18

photoelectric effect

Question 19

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

Answer 19

alber einstein

Question 20

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

Answer 20

photon

Question 21

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

Answer 21

a prism

Question 22

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

Answer 22

atomic emission spectrum of an element

Question 23

which model explained the relationship between the atomic structure and light

Answer 23

bohr’s model/ the quantum model

Question 24

what did bohr state

Answer 24

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

Question 25

the lowest possible state for an electron

Answer 25

ground state

Question 26

anything above the ground state

Answer 26

excited state

Question 27

what did bohr's model explain

Answer 27

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

Question 28

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

Answer 28

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

Question 29

what didnt bohrs model explain?

Answer 29

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

Question 30

what is the heisenberg uncertainty principle

Answer 30

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

Question 31

what does the quantum mechanical model give us

Answer 31

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….

Question 32

energy levels

Answer 32

an electrons distance from the nucleus

Question 33

the shape of an electron cloud

Answer 33

sublevel

Question 34

the probable location for 2e-

Answer 34

atomic orbitals

Question 35

what letters describe the sublevel shapes

Answer 35

s,p,d,f

Question 36

what shape are s orbitals

Answer 36

spherical shape

Question 37

what shape are p orbitals

Answer 37

dumbbell shape

Question 38

what don't we know about p orbitals

Answer 38

how the electrons get from one side to the other side

Question 39

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

Answer 39

1s, 2p, 3d, 4f

Question 40

how many electrons in s orbital

Answer 40

2e-

Question 41

how many electrons in p orbital

Answer 41

6e-

Question 42

how many electrons in d orbital

Answer 42

10e-

Question 43

how many electrons in f orbital

Answer 43

14e-

Question 44

this shows where each electrons in an atom is located

Answer 44

electron configuration

Question 45

states that each electron occupies the lowest energy orbital available

Answer 45

aufbau principle

Question 46

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

Answer 46

hund's rule

Question 47

how are orbital diagrams expressed

Answer 47

arrows in boxes

Question 48

how are noble gas configurations expressed

Answer 48

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

Question 49

how are electron notations/configurations expressed

Answer 49

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