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This review test will require the use of a Periodic Table.

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# Atomic Structure - Review (Grades 11-12)

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## Atomic Structure - Review

Instructions: Answer the following questions, based on your knowledge of atomic structure.

1.
Which of the following statements is consistent with Dalton's model of the atom?
1. The atom contains protons, neutrons, and electrons.
2. The atom has a positive nucleus.
3. The atom contains a positive nucleus with electrons in circular pathways called orbits surrounding the nucleus.
4. The atom is indivisible and can't be destroyed.
2.
Which of the following was observed in Thomson's experiments with cathodes and anodes?
1. The cathode rays moved towards the cathode, so they consisted of negatively-charged particles.
2. The cathode rays moved towards the anode, so they consisted of negatively-charged particles.
3. The cathode rays moved towards the cathode, so they consisted of positively-charged particles.
4. The cathode rays moved towards the anode, so they consisted of positively-charged particles.
3.
Which of the following models visualized the atom as being a positive mass with negatively-charged particles spread throughout the mass?
1. Nuclear Model
2. Orbital Model
3. Plum Pudding Model
4. Bohr Model
4.
What happened to some the alpha particles directed at the gold foil in Rutherford's experiment, when they struck the center of the atoms of gold?
1. They passed through.
2. They deflected at different angles.
3. Their motion was disrupted, but they continued through the foil.
4. None of the above
5.
In a famous experiment conducted by Ernest Rutherford, positively charged alpha particles were scattered by a thin gold foil. Which of the following is a conclusion that resulted from this experiment?
1. The nucleus is negatively charged.
2. The atom is a dense solid and is indivisible.
3. The mass is conserved when atoms react chemically.
4. The nucleus is very small and the atom is mostly empty space.
6.
Which of the following conclusions is consistent with the Bohr model of the atom?
1. Electrons exist in fixed circular paths known as orbits.
2. Electrons are most likely to be located in a space known as an orbital.
3. Electrons are randomly spaced out around a positive mass.
4. Electrons are directly adjacent to the nucleus.
7.
Which of the following was observed by Niels Bohr?
1. Heated atoms absorbed energy in the form of light.
2. Atoms lost electrons, when exposed to a stimulus like heat.
3. Atoms gained electrons, when exposed to a stimulus like heat.
4. Heated atoms released energy in the form of light.
8.
Which of the following statements best summarizes the modern model of the atom?
1. Protons travel in circular paths around a charged nucleus.
2. Negative electrons are found in positive matter.
3. Matter is composed of identical and indivisible particles.
4. Electrons are likely to be found in orbitals around the nucleus.
9.
The nucleus is made up of
1. protons and electrons.
2. electrons and neutrons.
3. protons and neutrons.
4. protons, neutrons and electrons.
10.
What is the atomic number of an atom with 20 protons, 20 electrons, and 22 neutrons?
1. 42
2. 22
3. 2
4. 20
11.
A neutral atom contains 12 neutrons and 11 electrons. What is the number of protons in this atom?
1. 12
2. 23
3. 1
4. 11
12.
What is the total number of electrons in an atom of Mn-55?
1. 30
2. 55
3. 25
4. 80
13.
What is the mass number of an atom with 11 protons, 11 electrons, and 12 neutrons?
1. 11
2. 23
3. 22
4. 1
14.
What is the total number of neutrons in an atom with a mass number of 3 and an atomic number of 1?
1. 3
2. 1
3. 2
4. 4
15.
What is the charge of the nucleus of a magnesium-24 atom?
1. +2
2. +24
3. +12
4. +36
16.
Isotopes of an element must have different what?
1. atomic numbers
2. numbers of protons
3. numbers of electrons
4. mass numbers
17.
Which of the following isotopes has the same number of neutrons as phosphorus-31?
1. ${:( ,32),(,16):} S$
2. ${:( ,29),(,14):} Si$
3. ${:( ,32),(,15):} P.$
4. ${:( ,28),(,14):} Si$
18.
Which statement correctly describes the average atomic mass of an element?
1. The average of the two most abundant isotopes of an element
2. The average of all of the naturally-occurring atomic mass values of isotopes
3. The atomic mass of the most abundant isotope of an element
4. The atomic mass of the least abundant isotope of an element
19.
An element has an atomic number of 26 and has isotopes with mass numbers of 56 and 54. Its average atomic mass is 55.845 amu. Based on the average atomic mass, which of the following isotopes is most abundant?
1. The isotope with a mass number of 54
2. The isotope with a mass number of 56
3. Both isotopes have equal abundances
4. An isotope with a mass number other than 56 or 54
20.
Mg has three different isotopes. Mg-24 has an abundance of 78.70%, Mg-25 has an abundance of 10.13%, and Mg-26 has an abundance of 11.17%. Which setup is correct for calculating the atomic mass of magnesium?
1. (78.70)(24 u)+(10.13)(25 u)+(11.17)(26 u)
2. (78.70)(24 u)+(11.17)(25 u)+(10.13)(26 u)
3. (0.7870)(24 u)+(0.1013)(25 u)+(0.1117)(26 u)
4. (0.7870)(24 u)+(0.1117)(25 u)+(0.1013)(26 u)
21.
Which two orbitals have the same shape?
1. 2s and 2p
2. 2s and 3s
3. 3p and 3d
22.
How many total electrons can the d sublevel hold?
1. 2
2. 6
3. 10
4. 14
23.
What is the maximum number of unpaired electrons that can be placed in a 3p sublevel?
1. 1
2. 2
3. 3
4. 4
24.
How many total electrons can the f sublevel hold?
1. 2
2. 6
3. 10
4. 14
25.
What is the total number of electrons in a completely filled sixth shell of an atom?
1. 50
2. 32
3. 72
4. 18
26.
The maximum number of electrons that can be found in any atom's third principal energy level is
1. 5.
2. 18.
3. 10.
4. 20.
27.
What is the total number of protons in an atom with two electrons in the first shell, eight electrons in the second shell, and seven electrons in the third shell?
1. 7
2. 8
3. 10
4. 17
28.
Which orbital notation represents an s block element in Period 3?
1. $(uarrdarr)/(1s)$$(uarrdarr)/(2s)$
2. $(uarrdarr)/(1s)$$(uarrdarr)/(2s)$ $(uarrdarruarrdarruarrdarr)/(2p)$ $(uarrdarr)/(3s)$
3. $(uarrdarr)/(1s)$$(uarrdarr)/(2s)$ $(uarrdarruarrdarruarrdarr)/(2p)$ $(uarrdarr)/(3s)$ $(uarrdarruarrdarruarr)/(3p)$
4. $(uarrdarr)/(1s)$$(uarrdarr)/(2s)$ $(uarrdarruarrdarruarrdarr)/(2p)$ $(uarrdarr)/(3s)$ $(uarrdarruarrdarruarrdarr)/(3p) (uarrdarr)/(4s) (uarr uarr)/(3d)$
29.
Which element has an atom with the electron configuration 2-8-1?
1. magnesium
2. sodium
3. calcium
4. beryllium
30.
Which of the following represents a correct ground-state electron configuration for a silicon atom?
1. $1s^2 2s^2 2p^6 3s^2 3p^6 4s^2$
2. $1s^2 2s^2 2p^4 3s^2 3p^4$
3. $1s^2 2s^2 2p^6 3s^2 3p^2$
31.
Which represents an atom of an element in an excited state?
1. 2-1
2. 2-8-15-2
3. 2-8-10-2
4. 2-7-10-2
32.
An atom's valence electrons are those in its                       .
1. outermost energy level
2. lowest energy level
3. electron clouds
4. inner energy level
33.
Given the number of valence electrons shown in the diagram, what can you conclude about this element?
1. It is nonreactive.
2. It only reacts with elements with 6 valence electrons.
3. It is reactive with elements that have 1 valence electron.
4. None of the above
34.
Which of the following noble gases does not have an octet of valence electrons?
1. neon
2. argon
3. krypton
4. helium
35.
If an atom loses a valence electron, what will happen?
1. The charge of the atom does not change because an electron has no charge.
2. The atom will lose the same amount of protons to keep the charge neutral.
3. The atom will become positively charged because it has lost an electron.
4. The atom will become negatively charged because it has lost an electron.
36.
What must magnesium do in order to have a complete outer shell of electrons?
1. lose 1 electron
2. gain 1 electron
3. lose 2 electrons
4. gain 2 electrons
37.
What is the total number of electrons in a $"Cr"^"3+"$ ion?
1. 21
2. 18
3. 24
4. 27
38.
Which ion's configuration matches that of the noble gas whose electron-dot diagram is below?
1. $"N"^"3-"$
2. $"Rb"^"+"$
3. $"Ca"^"2+"$
4. None of the above
39.
How many protons and electrons are in a $Cu^(+2)$ ion?
1. 27 protons, 29 electrons
2. 27 protons, 31 electrons
3. 29 protons, 27 electrons
4. 29 protons, 31 electrons
40.
What is the total number of protons in an ion with 10 electrons, a charge of +2, and an atomic number of 12?
1. 10
2. 9
3. 12
4. 2
41.
What were the limitations of Democritus's ideas about atoms?

42.
How many protons are in the nuclei of the following atoms?

a. phosphorus (P)
b. molybdenum (Mo)
c. Aluminum (Al)

43.
There are three isotopes of silicon. Si-28 has an atomic mass of 27.98 amu and an abundance of 92.21%, Si-29 has an atomic mass of 28.98 amu and an abundance of 4.70%, and Si-30 has an atomic mass of 29.97 amu and an abundance of 3.09%. Calculate the average atomic mass of silicon.

44.
A correct excited state electron configuration for nickel contains 1 electron in the first shell, 8 electrons in the second shell, 17 electrons in the third shell, and 2 electrons in the fourth shell.
1. True
2. False
45.
Write the electron configuration of an $Mg^{2+} "ion"$.

46.
Write the electron configuration for an $F^-$ ion.

47.
Write the electron configuration for a lithium ion.

48.
In the space provided below, write the full electron configuration for an atom of cobalt.

49.
Write the electron configuration for an atom of selenium.

50.
Write the electron configuration for an atom of cobalt.

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