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Chapter 5 Review Quiz Flashcards | StudBud
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Chapter 5 Review Quiz
Chapter 5 Review Quiz
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1
Which color of visible light has the most energy?
Violet
White
Green
Red
2
Max Planck proposed the relationship between a quantum of energy and ______________
Planck's constant
The frequency of radiation
The speed of light
The wavelength of light
3
What is the order of the subleveles from HIGHEST energy to LOWEST?
f, p, d, s
s, d, p, f
s, p, d, f
f, d, p, s
4
What is Hund's rule?
Each orbital may only contain 2 electrons with opposite spins
Electrons fill up the orbitals using the diagnol rule
Each orbital may only contain 2 electrons
All orbitals in a sublevel must fill with one electron before getting more
5
What is the symbol for wavelength? NAME AND SYMBOL
Lambda, λ
Nu, ν
Lambda, ν
Nu, λ
6
What type of electromagnetic radiation has the lowest frequency, longest wavelength, and least energy?
Ultraviolet light
Gamma waves
Radio waves
Microwave rays
7
Which number is closest to the nucleus, and which number has the least energy?
7, 1
1, 1
7, 7
1, 7
8
What is the amplitude?
A wave's height from trough to crest
The distance between wave crests
A wave's heigh from zero to the crest
The number of crests per second
9
What does the E stand for in E=hv?
The frequency of the radiation
The number of photons in a packet
A fundamental physical concept known as "Planck's constant"
The energy, in joules, of quantum radiation
10
As you move right across the period on the periodic table, the size _______
Increases
Decreases
Stays the same
11
What does C stand for in C=λν?
The Speed of light
Amplitude
Wavelength
Frequency
12
Who developed the equation that treats atoms as waves?
Einstein
Shrödinger
Bohr
Heisenberg
13
How many orbitals does the d sublevel have?
3
1
7
5
14
What is the equation for the number of electrons that can fit in each energy level?
2n^2
4n
n^2
2n+2
15
What is ionization energy?
A concept resuting from radiation and nuclear decay
The amount of energy required to add an electron to an atom
The energy released when two atoms bond
The amount of energy required to remove an electron from an atom
16
The shorter the wavelength, the ________ the energy in a photon
Lower
Higher
17
True or false: orbitals help locate the EXACT location of electrons
False
True
18
What is a particle of light called?
Photon
Gamma ray
Electron
Lambdon
19
The shorter the wavelength, the _________ the frequency
Higher
Lower
20
Ionization energy ______ as you move right across the periodic table and _______ as you move down
Decreases, decreases
Increases, decreases
Decreases, increases
Increases, increases
21
What are valence electrons?
Electrons on the innermost level involved in bonding
Electrons without atoms
Electrons on the outermost level involved in bonding
Electrons that are stable and unmoving
22
What does the Heisenberg uncertaity principle state?
It's impossible to determine the position aand velocity of an atom
It's impossible to determine the position and velocity of an electron
Electrons teleport randomly and uncontrollably
It's impossible to determine the position and velocity of a proton
23
Which color of visible light has the least energy?
Red
Green
White
Violet
24
Who's uncertainty principle do we use?
Einstein
Bohr
Shrödinger
Heisenberg
25
What does ν stand for in C=λν?
Wavelength
Frequency
Amplitude
The Speed of light
26
What is the bottom of the wavelength called? Opposite of crest
Base
Trough
Valley
Pit
27
Who's model of the atom had fixed energy levels
Einstein
Bohr
Shrödinger
Heisenberg
28
True or false: electron waves can only exist at certain frequencies
False
True
29
Light has the properties of both particles and:
Waves
Sin(x)
Photons
Electrons
30
What does λ stand for in C=λν?
Wavelength
Frequency
Amplitude
The Speed of light
31
What is frequency?
The number of crests that pass by in a second
The number of particles
The height of the crests
The distance between crests
32
True or false: The number of energy levels = the number of sublevels
False
True
33
What type of radiation is light?
Solar
Gamma
Electro magnetic
Photon
34
What is the speed of light in meters per second?
3x1010
3x108
3x106
6.8x107
35
True or false: Energy increases with the principal quantum number
True
False
36
What is the symbol for frequency? NAME AND SYMBOL
Lambda, λ
Nu, ν
Lambda, ν
Nu, λ
37
What is wavelength?
The distance between crests
The number of waves that pass in a second
The height of the waves
The number of photons
38
What does the principal quantum number specify?
The shell of the orbital
The subshell/sublevel of the orbital and its shape
The velocity of the electrons
The spin of the electrons
39
What color of light has the shortest wavelength?
Red
Black
White
VIolet
40
What are the names of the regions that electrons exist in?
Orbitals
Rings
Quantum zones
Atoms
41
What is the photoelectric effect?
Different colors of light have different electrical charges
When light is shined on metal, electrons may be emitted
Light is created by electricty, and electricity can be created from light
Trick question! "Photoelectric" isn't a word!
42
What does the h stand for in E=hv?
The number of photons in a packet
A fundamental physical concept known as "Planck's constant"
The energy, in joules, of quantum radiation
The frequency of the radiation
43
What type of electromagnetic radiation has the highest frequency, shortest wavelength, and most energy?
Gamma waves
Microwave rays
Ultraviolet light
Radio waves
44
As you move down a column on the periodic table, the size _________
Stays the same
Decreases
Increases
45
How long is a nanometer?
1x10-9
1x108m
1x109m
1x10-10
46
When an electron moves from excited to ground state, it releases energy in the form of:
Electromagnetic radiation
Gamma rays
coinheadsium
Heat
47
True or false: electronegativity follows the trend of ionization energy on the periodic table
True
False
48
What is the Pauli exclusion principle?
All orbitals in a sublevel must fill with one electron before getting more
Each orbital may only contain 2 electrons
Each orbital may only contain 2 electrons with opposite spins
Electrons fill up the orbitals using the diagnol rule
49
What do we think of a photon as?
A bouncy ball, because of the way it refracts
A single packet of light energy
Plum pudding
A type of radiation that is not harmful
50
Which scientist looked at how the energy of an atom changes as it absorbs or emits light?
Heisenberg
Shrödinger
Bohr
Einstein
51
In H as
b
when talking about the electron configuration, what does the b represent?
The shape of the orbital
The spin of the electrons
The orbital
The number of electrons
52
What is the minimum amount of energy that can be gained or lost by an atom?
A photon
A quantum
An electron
A planck
53
True or false: Different subshells within the same principle shell have the same energy levels
False
True
54
What is electronegativity?
The amount of energy it takes to remove an electron
The amount of electrons released in a reaction
A nuclear principle related to how particles have charges
The ability of an atom to attract electrons while in a compound
55
True or false: Quantum theory describes mathematically the wave properties of electrons
True
False
56
What is the electron configuration of an atom with electrons in the 3rd level?
1s22s22p63s23p63d12
Xenon
1s22s22p63s23p63d10
1s2s2p3s3p3d
57
Which of these is NOT a letter for a sublevel?
p
b
s
f
58
Who proposed the idea that elecrons function as both particles and waves?
Einstein
Bohr
Louis de Broglie
Schrödinger
59
When an electron absorbs energy, it moves from its _________ state to its ____________ state.
Ground, excited
Base, excited
Excited, ground
Base, energized
60
What is the name for the amount of energy required to move from one energy level to another?
quantum
Calorie
Joule
calorie
61
What shape do orbitals within the s subshell have?
Donut
Sphere
Cone
Rounded X
