Chapter 4 Flashcards
(90 cards)
1
Q
wave motion
A
frequency and wavelength
2
Q
wavelength
A
- the distances between corresponding points on a wave
- Units: meters/nanometers
3
Q
frequency
A
- the number of waves that pass a given point in a specific time
- Units: Hz or 1/s
4
Q
relation of wavelength and frequency
A
inversely proportional
5
Q
relation of wavelength and energy
A
inversely proportional
6
Q
relation of frequency and energy
A
directly proportional
7
Q
electromagnetic radiation
A
form of energy that exhibits wavelength behavior as it travels through space
8
Q
electromagnetic spectrum
A
all forms of electromagnetic radiation combined
9
Q
constant velocity
A
what all types of electromagnetic radiation travel at
10
Q
speed of light(c)
A
3.00 x 10^8 m/s
11
Q
formula for speed of light
A
c = wavelength x frequency
12
Q
formula for energy (using frequency)
A
E = planks constant x frequency
13
Q
formula for energy (NOT using frequency)
A
E = (Plancks x speed of light) / wavelength
14
Q
electromagnetic spectrum in order from least to most energy
A
Radio
Microwave
Infared
Visible
Ultraviolet
X-ray
Gamma Ray
15
Q
Visible light travels at what speed
A
speed of light(c)
16
Q
Photoelectric effect
A
- shine light at different metals and they emit electricity
- electricity is only emitted when the frequency of light is high enough
- Light is acting like a particle
- Max Planck came up with it
17
Q
Who came up with the dual-wave particle theory
A
Albert Einstein
18
Q
why were scientists surprised from the photoelectric effect?
A
They expected that eventually you could shine lower frequency light long enough that enough energy would accumulate but you can’t
19
Q
quanta
A
small amounts of energy
20
Q
photon
A
a particle of electromagnetic radiation that has zero mass and carries a quantum of energy
21
Q
planks constant
A
6.626 x 10^-34 Joules
22
Q
frequency units
A
Hz or 1/s
23
Q
energy unit
A
Joules or J
24
Q
ground state
A
the lowest energy state of an atom
25
excited state
the higher energy when atoms gain energy, and have a higher potential energy than the ground state
26
when an excited atom returns to the ground state, it gives off energy in the form of...
electromagnetic radiation
27
line-emission spectrum
the bands of light that are visible
28
how are atoms like a fingerprint?
excited atoms exhibit a specific portion of the visible spectrum; unique.
29
Why do we see distinct colors or different elements?
There are different amounts of energy that is released depending on the frequency
30
what does Niels Bohr suggest about electrons?
* electrons could circle the nucleus in a fixed path
* electrons could move up and down to higher or lower orbits
31
absorption
photon is absorbed
electron is emitted
32
emission
photon is emitted
electron is absorbed
33
what has to happen for an electron to "jump" from the ground state to an excited state?
Absorption of energy leads to photon getting excited and released a proton
34
1 meter = ? nanometers
1 x 10^-9 nm
35
1 kJ = ? J
1000 J
36
quanta = (Planck constant)(frequency)
TRUE
37
According to Bohrs model of the atom, which particles are allowed to exist in any one of a number of energy levels?
Electrons
38
The line-emission spectrum of an atom is caused by the energies released when electrons...
"jump" from a higher energy level to a lower energy level
39
because excited hydrogen atoms always produced the same line-emission spectrum, scientists concluded that hydrogen...
releases energy of only certain values
40
color of light from longest to shortest wavelength
Red
Orange
Yellow
Green
Blue
Purple
41
When light is envisioned as a particle, it is called what?
a photon
42
In the equation E = hf, what does h represent
Planck's constant
43
What form of energy exhibits wave behavior as it travels through space
all types of electromagnetic radiation
44
the photoelectric effect is when...
light is shone at a substance and the element emits electrons
45
In the Bohr model of the atom, in which orbit is an electron in its lowest energy level?
the orbit closest to the nucleus
46
wave theory of The atom was created by who?
de Broglie and
Schrodinger
47
Wave theory of an atom
* described electrons as particles that behave like waves
* knew electrons had a certain amount of energy and NOTHING in between
*still didn't explain everything
48
quantum theory of an atom
describes mathematically the LIKELY behavior of electrons
Uses the 4 quantum numbers to describe them in their MOST LIKELY location in an atom
49
Heisenberg uncertainty principle
you can't know the exact position of an electron at the same time as the velocity of an electron
50
velocity
speed and direction
51
the exact position and motion of an electron is...
unknowable
52
you can only describe the probable places to find electrons using:
orbitals
53
orbital
a 3D region around the nucleus where an electron will likely be
54
what is the name of the first quantum number?
Principle quantum number
55
Principle Quantum number
* Abbreviation: n
* Tells us the energy level the electrons are
56
what is the highest energy level they go up to?
7 energy levels
57
As n increases:
electrons energy and average distance from nucleus increase too
58
what is the name of the second quantum number?
Angular momentum quantum number
59
Angular momentum quantum number
* Abbreviation: l
* Tells us the sub level the electron is in within the energy levels
60
are sub levels equal in size?
NO
61
What number do sublevels start at?
0
Go up by 1
62
1st sub level = ?
0
63
Sublevel 1 = ?
p or 2nd sublevel
64
what 2 things does the 2nd quantum number tell us?
* shape of orbital
* sublevel it is in
65
what is the name of the 3rd quantum number?
Magnetic quantum number
66
Magnetic quantum number
* Abbreviation: m
* Tells us the designation for which specific orbital within the sublevel
*Tells us the the orientation of orbital around the nucleus
67
what are orbitals labeled as?
(- l ... + l )
68
p sublevel has how many orbitals?
3 orbitals
69
d sublevel has how many orbitals?
5 orbitals
70
s sublevel has how many orbitals?
1 orbital
71
possible orbitals (m values) equation:
2l + 1
72
what is the name of the 4th quantum number?
Spin Quantum Number
73
Spin Quantum Number
* Abbreviation: s
* Tells us the one of two possible spin states
74
what are the two possible spin states?
+ 1/2
- 1/2
75
if the electron is spinning in a positive direction, does it mean it has a positive charge?
NO
76
electron configuration
electrons will fill up rows various spots in the atom from least to most energy
77
ground state configuration
natural state at lowest energy
78
valence electrons
outermost electrons in the highest energy levels
79
orbital filling notation
* based on energy of orbitals, filling the lowest first
* every orbital is designated with a horizontal line
* arrows on top are electrons pointing up and down
80
electron configuration notation
shortened notation
all sublevel superscripts should be full UNLESS its the last one
81
noble gases
the gaseous elements on the periodic table that have full outer electron shells
82
noble gases are what orbitals?
s and p
83
noble gases DO NOT react with other elements to form compounds
TRUE
84
what are the noble gases
Helium
Neon
Argon
Krypton
Xenon
Radon
85
aufbrau principle
lowest energy orbitals will be first filled
86
Hunds rule
* when orbitals of identical energy are available, electrons enter these orbitals singly before a second electron will fill each orbital
* orbitals in the same sublevel are degenerate
87
degenerate
have identical energy
88
Pauli Exclusion Principle
* orbitals can only contain a maximum of two electrons and when two electrons enter the same orbital they must have opposite spins so that each electron has a unique set of quantum numbers.
89
how many electrons are in each orbital?
2 electrons
90
Why do we see colored lights during the flame test experiment?
* The flame adds energy to the electrons
* They get excited and jump to higher energy levels
* Then, they get pulled back towards the nucleus and the extra energy gets emitted as light.
