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WorksheetsUnit 2 Review Game
Total questions: 26
Worksheet time: 7hrs 30mins
Given the following information:
Atomic number: 17
Number of Protons: 17
number of Neutrons: 19
Number of Electrons: 18
What is the mass number of the given atom?
34
35
36
37
Given the following information:
Atomic number: 17
Number of Protons: 17
number of Neutrons: 19
Number of Electrons: 18
What is the charge of the given atom?
+2
+1
0
-1
-2
Given the following information, what is the average atomic mass of the unknown atom?
Isotope 1 with a mass of 23.985 and an abundance of 78.90%
Isotope 2 with a mass of 24.986 and an abundance of 10.00%
Isotope 3 with a mass of 25.983 and an abundance of 11.10%
23.31
24.31
25.31
26.31
How do isotopes differ from one another?
Different Charge
Different Atomic Number
Different Mass Number
Which of the following is the best definition of an ion?
An atom with a charge due to a gain or loss of one or more electrons
An atom with a charge due to a gain or loss of one or more protons
An atom with a charge due to a gain or loss of one or more neutrons
How many grams are in 3.64x1025 atoms of phosphorus?
Answer in scientific notation.
6.79x1050 grams
7.08 x 1047 grams
1.95x100 grams
1.13x105 grams
How many moles are in 62.889 grams of Tc?
0.63582 moles
6220.4 moles
0.62204 moles
6358.2 moles
How does an electron produce light?
An electron will take in energy and jump up to a higher energy orbital (stable) then it will fall back to the ground state (stable) and give off a photon in a release of energy.
An electron will take in energy and jump up to a higher energy orbital (unstable) then it will fall back to the ground state (stable) and give off a photon in a release of energy.
An electron will take in energy and jump up to a higher energy orbital (stable) then it will fall back to the ground state (unstable) and give off a photon in a release of energy.
An electron will take in energy and jump up to a higher energy orbital (unstable) then it will fall back to the ground state (unstable) and give off a photon in a release of energy.
There are two light waves, one with a wavelength of 450 nm and a second with 550 nm, which of the two waves will have a higher frequency?
Both will have the same frequency
450 nm
550 nm
What is the relationship between energy, frequency and wavelength?
As the wavelength increases, the frequency decreases and the energy increases
As the wavelength increases the frequency and the energy increase
As the wavelength increases the energy and the frequency both decrease
As the wavelength increases the frequency increases and the energy decreases
What are the possible sublevels in the 3rd energy level?
s
s, p
s, p, d
s, p, d, f
What is a possible quantum number set for the circled electron shown?
n: 1
l: 0
ml: -1, 0, 1
ms: +1/2
n: 2
l: 1
ml: 0
ms: -1/2
n: 1
l: 1
ml: -1, 0, 1
ms: +1/2
n: 2
l: 1
ml: -1, 0, 1
ms: -1/2
Which of the following is the correct ELECTRON CONFIGURATION for Arsenic?
A
B
C
D
Which of the following Orbital notations for Nitrogen are correct?
A
B
C
D
Which of the following short hand configurations are correct for Tin?
A
B
C
D
What is the energy of a photon with a wavelength of 553 nm?
E = hν
C = λν
C = speed of light = 3.00x108 m/s
h = Planck's Constant = 6.626x10-34 Js
8.19x1047
1.22x10-48 J
2.50x1053 J
3.59x10-19 J
What are valence electrons?
Electrons that are closest to the nucleus and can participate in chemical bonding
Electrons that are found on an atoms outermost shell and can participate in chemical bonding
Electrons that are closest to the nucleus and cannot participate in chemical bonding
Electrons that are found on an atoms outermost shell and cannot participate in chemical bonding
How many valence electrons does Silicon have?
2
3
4
5
Which of the following has the largest atomic radius?
Fluorine, Nitrogen, Carbon, Lithium
Fluorine
Nitrogen
Carbon
Lithium
Which of the following has the largest ionization energy?
Aluminum, Gallium, Silicon, Phosphorus
Aluminum
Gallium
Silicon
Phosphorus
Which of the following have the largest electronegativity?
Cesium, Vanadium, Tin, Fluorine
Fluorine
Vanadium
Cesium
Tin
Why do nonmetals have a high electronegativity?
They are more stable atoms and they are close to having a full octet. They do not want to lose an electron so they hold onto it tighter due to the small atomic radii
They are less stable atoms and they are close to having a full octet. They do not want to lose an electron so they hold onto it tighter due to the small atomic radii
They are more stable atoms and they are close to having a full octet. They do want to lose an electron so they hold onto it looser due to the small atomic radii
They are less stable atoms and they are close to having a full octet. They do want to lose an electron so they hold onto it looser due to the small atomic radii
What is ionization energy?
The amount of energy needed for an atom to gain an electron
The amount of energy needed to remove an electron from an atom
The amount of energy needed to remove a proton from an atom
The amount of energy needed for an atom to gain a proton
Why does Lithium have a higher ionization energy than Rubidium?
Lithium has a larger atomic radii which pulls the electrons closer to the nucleus with less shielding occurring, and Rubidium has a larger atomic radii has a higher shielding effect than Lithium.
Lithium has a smaller atomic radii which pulls the electrons closer to the nucleus with more shielding occurring, and Rubidium has a larger atomic radii has a higher shielding effect than Lithium.
Lithium has a smaller atomic radii which pulls the electrons closer to the nucleus with less shielding occurring, and Rubidium has a larger atomic radii has a higher shielding effect than Lithium.
Lithium has a larger atomic radii which pulls the electrons closer to the nucleus with more shielding occurring, and Rubidium has a smaller atomic radii has a smaller shielding effect than Lithium.
Why does Magnesium have a larger atomic radii than Sulfur?
There is less pull on the electrons of the magnesium atom making the atomic radii smaller than sulfurs.
There is less pull on the electrons of the magnesium atom making the atomic radii larger than sulfurs.
There is more pull on the electrons of the magnesium atom making the atomic radii smaller than sulfurs.
There is more pull on the electrons of the magnesium atom making the atomic radii larger than sulfurs.
How many valence electrons are on Cs?
1
2
3
4
