1. An unknown chemical element is presented by the following formula: 𝐴𝑍𝑋. What is the name of index Z?
A. Atomic mass number B. Atomic number C. Principle quantum number
D. Orbital quantum number E. Magnetic quantum number
2. An unknown chemical element is presented by the following formula: 𝐴𝑍𝑋. What is the name of index A?
A. Atomic mass number B. Atomic number C. Principle quantum number
D. Orbital quantum number E. Magnetic quantum number
3. The atomic number is equivalent to which of the following?
A. The number of neutrons in the atom. B. The number of protons in the atom.
C. The number of nucleons in the atom. D. The number of 𝛼–particles in the atom.
E. None of the above
4. The atomic mass number is equivalent to which of the following?
A. The number of neutrons in the atom. B. The number of protons in the atom.
C. The number of nucleons in the atom D. The number of 𝛼–particles in the atom.
E. None of the above
5. Which of the following particles has the smallest mass?
A. Proton B. Electron C. Neutron D. Nucleus E. Nucleon
6. Which of the following statements about the mass of an atom is true?
A. It is evenly divided between the protons and the orbiting electrons.
B. It is evenly divided between the nucleons and the orbiting electrons.
C. It is concentrated in the electron cloud.
D. It is concentrated in the nucleus.
E. It is evenly divided between protons, neutrons and orbiting electrons.
7. Which of the following is correct for the number of neutrons in the nucleus?
A. N = A –Z B. N = Z – A C. N = Z +A D. N = Z E. N = A
8. How many electrons are in the 126𝐶 atom?
A. 12 B. 6 C. 18 D. 3 E. 9
9. How many nucleons are in the 20
10𝑁𝑒 atom?
A. 12 B. 30 C. 18 D. 10 E. 20
23
10. How many neutrons are in the 11𝑁𝑎 atom?
A. 12 B. 11 C. 18 D. 24 E. 9
, 11. How many protons are in the 147𝑁 atom?
A. 14 B. 6 C. 7 D. 10 E. 9
12. What law did Ernest Rutherford use to estimate the size of the nucleus?
A. Conservation of nucleon number
B. Conservation of angular momentum
C. Conservation of linear momentum
D. Conservation of energy
E. Conservation of charge
13. Why are nuclear energy levels more complex than electron energy levels?
A. Nuclear energy levels depend only on attractive forces.
B. Nuclear energy levels depend on attractive and repulsive forces.
C. Nuclear energy levels are an order of one hundred times as great as electron energy levels.
D. Electron energy levels depend on the interaction between neutrons and electrons.
E. Electron energy levels have greater energy than the nuclear energy levels.
14. Which of the following about the nuclear force is true?
A. It is an attractive force between electrons and protons in an atom.
B. It is an attractive force between electrons and neutrons in an atom.
C. It is much weaker than the electromagnetic force.
D. It is much weaker than the gravitational force.
E. It is a strong, short-range, attractive force between the nucleons.
15. What force is responsible for the radioactive decay of the nucleus?
A. Gravitational force
B. Weak Nuclear force
C. Strong Nuclear force
D. Electromagnetic force
16. Isotopes of an element:
A. have the same number of protons and electrons, but a different number of neutrons.
B. have the same number of protons and neutrons, but a different number of electrons.
C. have different number of protons.
D. have different number of electrons.
E. have the same number of neutrons and protons.
17. Binding energy is:
A. the amount of energy required to break a nucleus apart into protons and neutrons.
B. the amount of energy required to break a nucleus apart into protons and electrons.
C. the amount of energy required to break a nucleus apart into electrons and neutrons.
D. the amount of energy released when neutrons change energy levels.
E. the amount of energy released when protons change energy levels.
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