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WorksheetsChemistry Unit 3 Review
Total questions: 121
Worksheet time: 2hrs 59mins
1. _____ is the wave's height from rest to crest.
Amplitude
Wavelength
Frequency
Crest
1. _____ is the distance between two consecutive crests.
Amplitude
Wavelength
Frequency
Crest
1. _____ is the number of wave cycles passing a point per unit of time.
Amplitude
Wavelength
Frequency
Crest
1. _____ is the frequencies of light that are emitted by an element in discrete lines.
Pauli Exclusion Principle
Hund's Rule
Atomic orbitals
Atomic emission spectrum
1. _____ is the wave's height from rest to the trough.
Amplitude
Wavelength
Frequency
Crest
1. _____ is the distance between two consecutive troughs.
Amplitude
Wavelength
Frequency
Crest
1. _____ is the bottom of a wave.
Amplitude
Wavelength
Trough
Crest
1. _____ is the arrangement of electrons around the nucleus of an atom.
Spectrum
Atomic emission spectrum
Atomic orbitals
Electron configuration
1. _____ states that each orbital can hold at most two electrons and those two electrons must have opposite spins.
Pauli Exclusion Principle
Hund's Rule
Aufbau Principle
Heisenberg Uncertainty Principle
1. _____ is the distance from the rest point through a crest and a trough back to the rest point.
Amplitude
Wavelength
Frequency
Crest
1. _____ is the top of a wave.
Amplitude
Wavelength
Crest
Trough
1. _____ is the separation of light into different wavelength of colors.
Electron configuration
Atomic emission spectrum
Atomic orbitals
Spectrum
1. _____ is the space or region where there is a high probability of finding an electron.
Atomic orbitals
Atomic emission spectrum
Electron configurations
Spectrum
1. _____ states that electrons enter orbitals with the same energy such that as many electrons have the same spin as possible.
Pauli Exclusion Principle
Hund's Rule
Aufbau Principle
Heisenberg Uncertainty Principle
1. _____ states that electrons enter orbitals of the lowest energy first.
Pauli Exclusion Principle
Hund's Rule
Aufbau Principle
Heisenberg Uncertainty Principle
1. _____ states that it is impossible to know both the velocity and the position of a moving particle at the same time.
Pauli Exclusion Principle
Hund's Rule
Aufbau Principle
Heisenberg Uncertainty Principle
1. _____ are orbitals that have the same energy.
Degenerate orbitals
Atomic orbitals
Valence electrons
Excited state
1. _____ is the lowest energy level that electrons enter.
Lewis Dot Diagrams
Ground state
Valence electrons
Excited state
1. _____ are the electrons in the highest occupied energy level of the atom.
Kernel electrons
Ground state
Valence electrons
Excited state
1. _____ is energy levels that contain electrons with a greater energy than normal.
Lewis Dot Diagrams
Ground state
Valence electrons
Excited state
1. _____ show the organization of the valence electrons around the atom.
Lewis Dot Diagrams
Electromagnetic spectrum
Atomic emission spectrum
Spectrum
1. _____ is the range of waves at all possible energies, frequencies, and wavelengths.
Lewis Dot Diagrams
Electromagnetic spectrum
Atomic emission spectrum
Spectrum
1. _____ is elements that don't have magnetic properties because all electrons have a pair.
Quantum
Photon
Diamagnetic
Paramagnetic
1. _____ is elements that have magnetic properties because there are unpaired electrons.
Quantum
Photon
Diamagnetic
Paramagnetic
1. _____ is the amount of energy needed to move an electron from one energy level to another.
Quantum
Photon
Diamagnetic
Paramagnetic
1. _____ is a packet or bundle of electromagnetic energy that exits or enters the atom at once.
Quantum
Photon
Diamagnetic
Paramagnetic
1. _____ is a negatively charged particle that is located around the outside of the nucleus.
Quantum
Proton
Electron
Neutron
2. _____ has the electron configuration 1s2 2s2 2p6 3s1.
Calcium
Potassium
Magnesium
Sodium
2. _____ has the electron configuration 1s2 2s2 2p6 3s2 3p6 4s2 3d1.
Scandium
Potassium
Titanium
Calcium
2. _____ has the electron configuration 1s2 2s2 2p6 3s2 3p6 4s2 3d3.
Scandium
Vanadium
Titanium
Calcium
2. _____ has the electron configuration 1s2 2s2 2p6 3s2.
Calcium
Potassium
Magnesium
Sodium
2. _____ has the electron configuration 1s2 2s2 2p6 3s2 3p6 4s2 3d6.
Copper
Cobalt
Manganese
Iron
2. _____ has the electron configuration 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p5.
Bromine
Arsenic
Gallium
Selenium
2. _____ has the electron configuration 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p3.
Bromine
Arsenic
Gallium
Selenium
2. _____ has the electron configuration 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p1.
Zinc
Arsenic
Gallium
Germanium
2. _____ has the electron configuration 1s2 2s2 2p3.
Sulfur
Oxygen
Carbon
Nitrogen
2. _____ has the electron configuration 1s2 2s2 2p6 3s2 3p4.
Sulfur
Oxygen
Phosphorus
Silicon
2. _____ has the electron configuration 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2 4f14 5d10 6p6.
Astatine
Radon
Francium
Radium
2. _____ has the electron configuration 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2.
Xenon
Lanthanum
Barium
Cesium
2. _____ has the electron configuration 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p2.
Tellurium
Antimony
Indium
Tin
2. Sodium has _____ unpaired electrons.
1
2
3
4
2. Sulfur has _____ unpaired electrons.
1
2
3
4
2. Nitrogen has _____ unpaired electrons.
1
2
3
4
2. Iron has _____ unpaired electrons.
1
2
3
4
2. Scandium has _____ unpaired electrons.
1
2
3
4
2. Radon has _____ unpaired electrons.
1
0
3
4
2. Radon has _____ valence electrons.
5
6
7
8
2. Arsenic has _____ unpaired electrons.
1
0
3
4
2. Bromine has _____ unpaired electrons.
1
0
3
4
2. Barium has _____ unpaired electrons.
1
0
3
4
2. Bromine has _____ valence electrons.
5
6
7
8
2. Tin has _____ unpaired electrons.
1
0
3
2
2. Gallium has _____ unpaired electrons.
1
0
3
2
2. Magnesium has _____ unpaired electrons.
1
0
3
2
2. Vanadium has _____ unpaired electrons.
1
0
3
2
2. Nitrogen has _____ valence electrons.
5
6
7
8
2. Sulfur has _____ valence electrons.
5
6
7
8
2. Gallium has _____ valence electrons.
1
2
3
4
2. Tin has _____ valence electrons.
1
2
3
4
2. Sodium has _____ valence electrons.
4
3
2
1
2. Arsenic has _____ valence electrons.
5
6
7
8
2. Scandium has _____ valence electrons.
1
2
3
4
2. Iron has _____ valence electrons.
4
3
2
1
2. Scandium has _____ as the highest energy level.
1
2
3
4
2. Nitrogen has _____ as the highest energy level.
2
3
4
5
2. Vanadium has _____ valence electrons.
1
2
3
4
2. Barium has _____ valence electrons.
4
3
2
1
2. Tin has _____ as the highest energy level.
2
3
4
5
2. Sodium has _____ as the highest energy level.
3
4
5
6
2. Iron has _____ as the highest energy level.
3
4
5
6
2. Magnesium has _____ valence electrons.
4
3
2
1
2. Radon has _____ as the highest energy level.
3
4
5
6
2. Magnesium has _____ as the highest energy level.
3
4
5
6
2. Bromine has _____ as the highest energy level.
3
4
5
6
2. Vanadium has _____ as the highest energy level.
2
3
4
5
2. Barium has _____ as the highest energy level.
3
4
5
6
2. Sulfur has _____ as the highest energy level.
3
4
5
6
2. Arsenic has _____ as the highest energy level.
3
4
5
6
2. Gallium has _____ as the highest energy level.
2
3
4
5
2. _____ will have one dot on the left-hand side of the symbol.
Aluminum
Magnesium
Neon
Sodium
2. _____ will have two dots on the left-hand side of the symbol.
Scandium
Bromine
Gallium
Potassium
2. _____ will have two dots on the left-hand side of the symbol.
Aluminum
Magnesium
Neon
Sodium
2. _____ will have two dots on the left-hand side of the symbol.
Gallium
Bromine
Iron
Potassium
2. _____ will have two dots on the left-hand side of the symbol.
Gallium
Bromine
Potassium
Vanadium
2. _____ will have two dots on the left-hand side of the symbol.
Barium
Cesium
Xenon
Lead
2. _____ will have two dots on the left-hand side, two on the top, two on the right-hand side, and one on the bottom of the symbol.
Gallium
Bromine
Potassium
Vanadium
2. _____ will have two dots on the left-hand side, one on the top, one on the right-hand side, and one on the bottom of the symbol.
Fluorine
Oxygen
Nitrogen
Carbon
2. _____ will have two dots on the left-hand side, one on the top, one on the right-hand side, and one on the bottom of the symbol.
Germanium
Gallium
Selenium
Arsenic
2. _____ will have two dots on the left-hand side, two on the top, two on the right-hand side, and two on the bottom of the symbol.
Radon
Tin
Radium
Barium
2. _____ will have two dots on the left-hand side and one on the top of the symbol.
Germanium
Gallium
Selenium
Arsenic
2. _____ will have two dots on the left-hand side, one on the top, and one on the right-hand side of the symbol.
Tellurium
Indium
Tin
Antimony
2. _____ will have two dots on the left-hand side, two on the top, one on the right-hand side, and one on the bottom of the symbol.
Phosphorus
Argon
Chlorine
Sulfur
3. What happens to the energy of an electron as it moves farther away from the nucleus?
It gains energy.
It loses energy.
The energy stays the same.
It gains energy and loses energy.
4. What was Max Planck's conclusion about energy?
Energy comes as any multiple of "hv".
Energy is only in whole numbers.
Energy comes as whole-number multiples of "hv".
Energy can come in any amount.
5. Which of the following DOES NOT show the correct atomic orbitals in each of the first four principal energy levels?
4 - s, p, d, e
3 - s, p, d
2 - s, p
1 - s
6. What did Louis de Broglie say about matter?
Matter moves either as particles or waves, but not both.
Matter moves only as waves.
Matter moves only as particles.
Matter moves as particles and waves.
7. How do electrons fill atomic orbitals with more than one orbital?
Two electrons with opposite spin are placed in each orbital before the next orbital gets an electron.
One electron will be placed in each orbital with the same spin before electrons are paired up.
Two electrons with the same spin are placed in each orbital before the next orbital gets an electron.
Electrons will fill each orbital with different spins before any orbital gets a second electron.
8. Which of the following DOES NOT show the correct number of orbitals for the s, p, d, and f orbitals in a principal energy level?
s - 1 orbital
p - 3 orbitals
d - 4 orbitals
f - 7 orbitals
9. In an electron configuration, what does the letter tell you?
the energy level of the orbital
the number of electrons in the orbital
the number of unpaired electrons in the orbital
the type of atomic orbital
10. If one electron has a spin that is clockwise, what is the spin of the other electron in the orbital?
clockwise
counterclockwise
quarter of clockwise
half of clockwise
11. Which of the following DOES NOT show the maximum number of electrons in each of the first four principal energy levels
4 - thirty-two electrons
3 - eighteen electrons
2 - six electrons
1 - two electrons
12. What did Albert Einstein's experiment determine?
Light moves either as particles or waves, but not both.
Light moves only as waves.
Light moves only as particles.
Light moves as particles and waves.
13. When does light get emitted from an atom?
When it drops from a higher energy level to a lower energy level.
When it moves up and down between energy levels.
When it moves from a lower energy level to a higher energy level.
When it stays in the same energy level.
14. Who developed the Quantum Mechanical Model?
Werner Heisenberg
Ernest Rutherford
Erwin Schrodinger
Niels Bohr
14. The _____ has a mathematical equation that determines the probability of an electron's position around the nucleus of an atom.
Quantum Mechanical Model
Bohr Model
Plum Pudding Model
Rutherford's Model
15. Which of the following DOES NOT match the orbital and the shape correctly?
d - four-leaf clover
f - complicated
s - cubic
p - dumb bell
16. The Bohr model only explained how _____ atoms worked.
Beryllium
Lithium
Helium
Hydrogen
17. How are frequency and wavelength connected?
They are inversely proportional so as one goes up, the other goes down.
They are directly proportional, so as one goes up, the other goes up.
They are inversely proportional so as one goes up, the other goes up.
They are directly proportional, so as one goes up, the other goes down.
18. When do exceptions occur when drawing orbital diagrams and writing electron configurations?
Ultimately, electrons move to become less stable with less energy. Partially-filled energy levels are examples of this.
Ultimately, electrons move to become more stable with more energy. Partially-filled energy levels are examples of this.
Ultimately, electrons move to become more stable with less energy. Half-filled and filled energy levels are examples of this.
Ultimately, electrons move to become less stable with more energy. Half-filled and filled energy levels are examples of this.
19. In an electron configuration, what does the number in front of the letter tell you?
the energy level of the orbital
the number of electrons in the orbital
the number of unpaired electrons in the orbital
the type of atomic orbital
20. The _____ states that protons and neutrons are in the nucleus and the electrons move around the nucleus in orbits with fixed energies.
Quantum Mechanical Model
Bohr Model
Plum Pudding Model
Rutherford's Model
21. How are frequency and energy connected?
They are inversely proportional so as one goes up, the other goes down.
They are directly proportional, so as one goes up, the other goes up.
They are inversely proportional so as one goes up, the other goes up.
They are directly proportional, so as one goes up, the other goes down.
22. The Heisenberg Uncertainty Principle states that one cannot know the _____ of an electron and the _____ of the electron.
location, force
velocity, force
position, force
location, velocity
23. What happens when an electron moves from a higher energy level to a lower energy level?
It gains energy.
It loses energy.
The energy stays the same.
It gains energy and loses energy.
24. What is different between the energy difference in high energy levels and the energy difference in lower energy levels?
The energy difference is greatest at the middle energy levels.
The energy difference is smaller at higher energy levels than at lower energy levels.
The energy difference is larger at higher energy levels than at lower energy levels.
The energy difference is the same at higher energy levels than at lower energy levels.
25. In an electron configuration, what does the subscript tell you?
the energy level of the orbital
the number of electrons in the orbital
the number of unpaired electrons in the orbital
the type of atomic orbital
26. Which of the following DOES NOT show the sublevels in each of the first four principal energy levels?
1 - 1 sublevel
2 - 2 sublevels
3 - 5 sublevels
4 - 4 sublevels
27. Who made the first "quantum" model of the atom?
Werner Heisenberg
Ernest Rutherford
Erwin Schrodinger
Niels Bohr
28. How do atomic emission spectra compare from element to element? Why are they useful for identification?
Some elements have different atomic emission spectra, so they can be compared for identification.
No elements have different atomic emission spectra, so they can't be compared for identification.
Most elements have different atomic emission spectra, so some can be compared for identification.
Each element has a different atomic emission spectrum, so they can be compared for identification.
29. How are wavelength and energy connected?
They are inversely proportional so as one goes up, the other goes down.
They are directly proportional, so as one goes up, the other goes up.
They are inversely proportional so as one goes up, the other goes up.
They are directly proportional, so as one goes up, the other goes down.
30. Why do electrons have "wavelike" motion while basketballs don't?
Basketballs do have "wavelike" motion, but it is so small we can't see it due to the larger mass of the object.
Basketballs don't have "wavelike" motion because of the larger mass of the object.
Basketballs do have "wavelike" motion, but it is so small we can't see it due to the small mass of the object.
Basketballs don't have "wavelike" motion because of the smaller mass of the object.
