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Copy - Chemistry 0569 > Chapter 4 Pt.2 Test > Flashcards

Chapter 4 Pt.2 Test Flashcards

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1
Q 
greek philosopher
did experimenting of cutting object in half
called this the atomus
(model is round and plain)
he dissappeared, along with his theories
A

Democritus

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2
Q

british
all matter is made up of atoms
all atoms of an element are exactly alike
they’re different than the atomus of any other element
matter is neither created nor destroyed in a chemical reaction
model of atom = spherical

A

Dalton

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3
Q

realized there are + and - charges in an atom
he believed the whole atom was solid w/ all positives
called “-“ charges, electrons

A

J.J. Thomson

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4
Q

propelled alpha particles through gold foil
some alpha particles went through, or bounced back
ATOM IS EMPTY SPACE
DENSE CENTER
ELECTRONS MOVE RANDOMLY AROUND NUCLEUS

A

Rutherford

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5
Q

it acts like a wave.

it reflects and refracts

A

light

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6
Q

what does every element produce when being burned?

A

light

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7
Q

when light is passed through a prism, it separates into what?

A

wave-lengths

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8
Q

these wavelengths are ….

A

discrete

unique pattern

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9
Q

german
in an element, light is given off or absorbed as packets of energy
packets are “quantized”
they come in different sizes

A

Max Plank

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10
Q

a fan has 3 speeds

fast food meals come in regular or extra large sizes

A

Analogies for Quantize

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11
Q

example: “slider” for brightness on ipad -

A

nonanologies

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12
Q

packet of light energy -

A

Quantum

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13
Q

Quantum’s also know as …

A

photons

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14
Q

who created the Quantum Theory?

A

Max Plank

Albert Einstein

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15
Q

every electron has a fixed orbit
every electron has a location
every orbit has a # of electrons
farther from nucleus the more energy it takes to stay in orbits

A

Bohr

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16
Q

normal location of an electron =

A

ground state

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17
Q

farther from nucleus…. the __________________ it takes to stay in orbit

A

more energy

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18
Q

can higher orbits exists even if there are no electrons located there?

A

yes

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19
Q

what happens at step one of energy levels?

A

photon hits electron

electron absorbs and absorbs energy

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20
Q

Step two:

A

electron absorbs energy

electron jumps to higher energy level

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21
Q

Step three -

A

unstable electron loses energy & returns to ground state

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22
Q

published Heisenberg Uncertainty Principle

said you can know electrons location&momentum, but not at same time -

A

Heisenberg

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23
Q

showed that u can calculate the probability of an electron being in a certain location

  • don’t know exactly the location of electron
  • you can know probability of area where it should be
A

Schrodinger and Born?

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24
Q

Quantum mechanical model… also known as -

A

wave mechanical model

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25
Q

Quantum mechanical model combines ideas from ….

A

scientists

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26
Q

Quantum Mechanical Model:

electrons are in the ______ ________.

A

energy level

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27
Q

Quantum Mechanical Model:

-limited _________ in energy level

A

electrons

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28
Q

energy levels have sub levels called …

A

orbitals

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29
Q

what are the 4 different quantities -

A

n
l
m
s

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30
Q

n = ?

A

which energy level?

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31
Q

L = ?

A

shape of orbital

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32
Q

m = ?

A

where on x & y axis?

33
Q

s = ?

A

spin up or down

34
Q

Principle Energy Level = ….

A

N

35
Q

n describes how ______ an electrons orbit is from the _________.

A

far

nucleus

36
Q

N can be divided into sublevels ….

A

L

37
Q

sub level … = ….

A

orbitals

38
Q

it’s the region of space where there is 90% chance of finding the electron -

A

orbital

39
Q

orbital and orbits do NOT mean the same thing.

A

true

40
Q

energy level # of orbitals Orbital Names
n= 4 L=4 4s 4p 4u 4f
n=1 L=1 1s

A

just example

41
Q

every energy level (n) has same number of _________ (l).

A

orbitals

42
Q

s goes with the ______ orbital

A

1st

43
Q

p goes with the _______ orbital

A

2nd

44
Q

u goes with the _______ orbital

A

3rd

45
Q

f goes with the _______ orbital

A

4th

46
Q

who did Einstein disagree with??

A

Heisenberg and Bohr

47
Q

they held conferences. and there was a lot of tension between who?

A

Bohr and Einstein

48
Q

S looks like a ….

A

sphere

49
Q

p = “pinched” so looks like….

A

8

50
Q

d = “down on the ground” =

A

four leaf clover

51
Q

f = …

A

far too complicated

52
Q

1s…

A

small

53
Q

2s…

A

medium

54
Q

3s…

A

large

55
Q

Px =

A

8 going sideways (acrossed the x-axis)

56
Q

Py =

A

8

57
Q

how many orbitals in “d” orbital?

A

5

58
Q

how many f orbitals are therE?

A

7

59
Q

what orbital tells u the orientation in space of each orbitals -

A

m

60
Q

what orbital tells u the spin of the electrons movement?

A

s orbital

61
Q

1/2 -

A

up

62
Q

-1/2 =

A

down

63
Q

each orbital can hold no more than ________ electrons

A

2

64
Q

electrons must have ___________ spin

A

opposite

65
Q

one _______, and one _________.

A

up / down

66
Q

electrons fill in orbitals starting at the lowest energy level
“electrons are lazy”

A

Aufbau Principle

67
Q

place one electron in each empty orbital in an energy level before you add a second electron to that orbital -

A

Hunds Rule

68
Q

no more than 2 electrons may occupy an orbital & must have opposite spins -

A

Pauli Exclusion Act

69
Q

a maximum of ______ electrons may occupy a single orbital, but only if the electrons have __________ spins

A

2

opposite

70
Q

Quantum Mechanical Model of the Atom =

A

electrons located in energy levels

71
Q

electrons are located by 4 _________ ___________.

A

different quantities

72
Q

limited # of ___________ per energy __________.

A

electrons

level

73
Q

its the fixed amount of energy -

A

energy levels

74
Q

what are the 4 quantum #’s -

A

n
m
l
s

75
Q

define orbitals -

A

sublevels in energy levels

76
Q

what is the relationship between the principle energy level and the number of orbitals -

A

n = l

77
Q

what orbitals are present if n = 3

A

s3
p3
u3

78
Q

what orbitals are present if n = 4

A

4s
4p
4u
4f

Copy - Chemistry 0569 (22 decks)

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