Unit 1 Review Questions

Unit 1 Review Questions

Multiple-choice exercise

Choose the correct answer for each question.

CA Standards

The periodic table displays the elements in increasing atomic number and shows how periodicity of the physical and chemical properties of the elements relates to atomic structure. As a basis for understanding this concept:

Students know how to relate the position of an element in the periodic table to its atomic number and atomic mass.
Students know the nucleus of the atom is much smaller than the atom yet contains most of its mass.

Nuclear processes are those in which an atomic nucleus changes, including radioactive decay of naturally occurring and human-made isotopes, nuclear fission, and nuclear fusion. As a basis for understanding this concept:

Students know protons and neutrons in the nucleus are held together by nuclear forces that overcome the electromagnetic repulsion between the protons.
Students know the energy release per gram of material is much larger in nuclear fusion or fission reactions than in chemical reactions. The change in mass (calculated by E = mc²) is small but significant in nuclear reactions.
Students know some naturally occurring isotopes of elements are radioactive, as are isotopes formed in nuclear reactions.
Students know the three most common forms of radioactive decay (alpha, beta, and gamma) and know how the nucleus changes in each type of decay.
Students know alpha, beta, and gamma radiation produce different amounts and kinds of damage in matter and have different penetrations.

The nucleus of most atoms is made up of:
1. protons and electrons
2. protons and neutrons
3. neutrons and electrons
4. electrons and protons
The laws of electrostatics consistently demonstrate that opposite charges:
1. destroy one another
2. attract
3. repel
The charge and mass number of a proton are:
1. charge = +1, Mass number = 0
2. charge = -1, Mass number = 0
3. charge = 0, Mass number = 1
4. charge = +1, Mass number = 1
The charge and mass number of an electron are:
1. charge = +1, Mass number = 0
2. charge = -1, Mass number = 0
3. charge = 0, Mass number = 1
4. charge = +1, Mass number = 1
The charge and mass number of a neutron are:
1. charge = +1, Mass number = 0
2. charge = -1, Mass number = 0
3. charge = 0, Mass number = 1
4. charge = +1, Mass number = 1
Most of the mass of the atom can be found in the:
1. electron cloud
2. nucleus
3. electrons
4. charges
Which of the following descriptions does not apply to the nucleus?
1. Very dense
2. Mostly empty space
3. Positively charged
4. Very small
Of the basic atomic particles, the one that would be attracted to a negatively charged metallic plate is the:
1. proton
2. neutron
3. electron
The mass number of an atom is determined by:
1. adding the protons and electrons
2. adding the neutrons and electrons
3. adding the neutrons and protons
4. the number of protons only
The _______________ constitute(s) most of the volume of an atom.
1. protons
2. neutrons
3. nucleus
4. electron cloud
The atomic number of an element is equal to:
1. the number of protons in the atom
2. the number of neutrons in the atom
3. the number of protons plus the number of neutrons
4. the number of protons plus the number of electrons
How many electrons, neutrons and protons would be found in an atom of carbon-14 (atomic number 6)?
1. 6 electrons, 6 neutrons, 6 protons
2. 6 electrons, 6 neutrons, 8 protons
3. 8 electrons, 8 neutrons, 6 protons
4. 6 electrons, 8 neutrons, 6 protons
How many electrons would be found in an atom of oxygen (atomic number 8)?
1. 2
2. 4
3. 6
4. 8
An element with nine protons in every atom must:
1. have nine neutrons as well
2. be fluorine
3. have a mass number of nine
4. be unstable
What is the neutron-proton ratio for nitrogen-14?
1. 14:1
2. 2:1
3. 1:2
4. 7:2
5. 1:1
There are three isotopes of the element argon: argon-36, argon-38 and argon-40. These isotopes differ from one another in:
1. their atomic number
2. their number of electrons
3. their number of protons
4. their number of neutrons
5. their mass number
How many neutrons are there in an atom of hydrogen-3?
1. 0
2. 1
3. 2
4. 3
Isotope Mass number Atomic number Protons Neutrons Electrons
Scandium-45
1. The blanks, respectively, would be filled: 21, 45, 21, 21, 24
2. The blanks, respectively, would be filled: 45, 21, 21, 24, 21
3. The blanks, respectively, would be filled: 21, 45, 24, 21, 21
4. The blanks, respectively, would be filled: 24, 21, 45, 21, 21
Isotope Mass number Atomic number Protons Neutrons Electrons
_______________-27 13
1. The blanks, respectively, would be filled: aluminum, 27, 13, 13, 14
2. The blanks, respectively, would be filled: cobalt, 40, 27, 13, 27
3. The blanks, respectively, would be filled: aluminum, 27, 13, 14, 13
4. The blanks, respectively, would be filled: silicon, 27, 14, 13, 13
A process in which a very heavy nucleus splits into more-stable nuclei of intermediate mass.
1. nuclear fusion
2. nuclear fission
3. radioactive decay
4. a chain reaction
5. radiocarbon dating
An electron emitted from the nucleus during some kinds of radioactive decay is known as:
1. An alpha (a) particle
2. A beta (b) particle
3. A positron
4. A gamma ray
An alpha (a) particle is essentially a ____________________ nucleus.
1. hydrogen
2. uranium
3. carbon-12
4. helium
5. plutonium
Gamma (g) rays are:
1. neutrons
2. protons
3. electrons
4. pure energy waves
Very large nuclei tend to be unstable because of the:
1. repulsive forces between electrons
2. attraction of electrons for the positively charged nucleus
3. repulsive forces between neutrons
4. repulsive forces between protons
5. attraction of protons for neutrons
For the most common types of radioactive decay, the order of mass from heaviest to lightest is:
1. gamma, alpha, beta
2. beta, alpha, gamma
3. beta, gamma, alpha
4. alpha, beta, gamma
For the most common types of radioactive decay, the order of least penetrating to human tissue, to most penetrating to human tissue is:
1. gamma, alpha, beta
2. alpha, beta, gamma
3. beta, gamma, alpha
4. gamma, beta, alpha
For the most common types of radioactive decay, the order of least dangerous to most dangerous is:
1. gamma, alpha, beta
2. alpha, beta, gamma
3. beta, gamma, alpha
4. gamma, beta, alpha
In nuclear reactions:
1. small amount of mass are converted to large amounts of mass
2. large amount of energy are converted to small amount of mass
3. small amounts of mass are converted to large amount of energy
4. mass and energy are destroyed
Compared to chemical reactions, nuclear reactions produce:
1. proportionally far less energy
2. proportionally far more energy
3. fewer changes in the nucleus
4. more vegetables
Which of the following statements is true?
1. All man-made isotopes are radioactive
2. Some man-made isotopes are radioactive
3. None of the man-made isotopes are radioactive
Which of the following statements is true?
1. All naturally occurring isotopes are radioactive
2. Some naturally occurring isotopes are radioactive
3. No naturally occurring isotopes are radioactive
If we assume that pink represents protons, and green represents neutrons, the nucleus depicted here is:
1. ⁷₆C
2. ⁶₁₃C
3. ⁷₁₃C
4. ¹³₆C
If we assume that pink represents protons, and green represents neutrons, the nucleus depicted here is:
1. Boron-6
2. Boron-11
3. Boron-10.81
4. Boron-5
If we assume that pink represents protons, and green represents neutrons, which nucleus does not represent one of the isotopes of hydrogen?
Which of the following is/are true of the region of the atom labeled "X":
1. It is negatively charged
2. It contains most of the mass of the atom
3. It contains protons
4. It contains neutrons
5. It contains electrons
Which of the following is/are true of the region of the atom labeled "Y"
1. It is negatively charged
2. It contains most of the mass of the atom
3. It contains protons
4. It contains neutrons
5. contains electrons
Alpha decay is generally represented by the symbol _________ on the product side of the equation.
1. ⁴₂He
2. ⁰_-1He
3. ⁰_-1e
4. ⁰₀g
Beta decay is generally represented by the symbol _________ on the product side of the equation.
1. ⁴₂He
2. ⁰_-1He
3. ⁰_-1e
4. ⁰₀g
Gamma decay is generally represented by the symbol _________ on the product side of the equation.
1. ⁴₂He
2. ⁰_-1He
3. ⁰_-1e
4. ⁰₀g
Identify the missing particle in the following nuclear reaction:

²³⁹₉₃Np → ²³⁹₉₄Pu + _____
1. ¹₀n
2. ⁰₁e
3. ⁰_-1e
4. ¹₁H
What type of decay is taking place in the nuclear reaction shown below?

²³⁹₉₃Np → ²³⁹₉₄Pu + ⁰_-1e
1. alpha
2. beta
3. gamma
4. none of these
Which of the following statements best describes the changes occuring in the reaction below?

²³⁹₉₃Np → ²³⁹₉₄Pu + ⁰_-1e
1. a proton has been converted to an electron
2. a proton has been converted to a neutron
3. a neutron has been converted to an electron
4. a neutron has been converted to a proton
Identify the missing particle in the following nuclear reaction:

¹₀n + ²³⁵₉₂U → 2 ¹₀n + _____ + ¹³⁷₅₂Te + ⁰₀g
1. ⁴₂He
2. ⁹⁷₃₈Sr
3. ⁹⁶₄₀Zr
4. ⁹⁷₄₀Zr
What type of decay is evident in the nuclear reaction shown below?

¹₀n + ²³⁵₉₂U → 2 ¹₀n + ⁹⁷₄₀Zr + ¹³⁷₅₂Te + ⁰₀g
1. alpha
2. beta
3. gamma
4. none of these
Which of the following statements best describes the changes occuring in the reaction below?

¹₀n + ²³⁵₉₂U → 2 ¹₀n +⁹⁷₄₀Zr + ¹³⁷₅₂Te + ⁰₀g
1. uranium is undergoing nuclear fission
2. uranium is converted to neutrons and energy
3. uranium has been converted to zirconium
4. zirconium has been converted to neutrons
Identify the missing particle in the following nuclear reaction:

²³⁹₉₂U + ⁴₂He → _____ + ¹₀n
1. ²⁴²₉₄Pu
2. ²⁴³₉₄Pu
3. ²⁴³₉₂U
4. ²⁴¹₉₂U
What type of decay is evident in the nuclear reaction shown below?

²³⁹₉₂U + ⁴₂He → ²⁴²₉₄Pu + ¹₀n
1. alpha
2. beta
3. gamma
4. none of these
Which of the following statements best describes the changes occuring in the reaction below?

²³⁹₉₂U + ⁴₂He → ²⁴²₉₄Pu + ¹₀n
1. uranium is being converted to plutonium
2. helium is being converted to neutrons
3. helium is being converted to plutonium
4. nuclear fission is taking place
Identify the missing particle in the following nuclear reaction:

²⁷₁₃Al + _____ → ²⁴₁₁Na + ⁴₂He
1. ¹₀n
2. ¹₀H
3. ⁰_-1e
4. ²⁸₁₃Al
What type of decay is evident in the nuclear reaction shown below?

²⁷₁₃Al + ¹₀n → ²⁴₁₁Na + ⁴₂He
1. alpha
2. beta
3. gamma
4. none of these
Which of the following statements best describes the changes occuring in the reaction below?

²⁷₁₃Al + ¹₀n → ²⁴₁₁Na + ⁴₂He
1. aluminum decays into sodium
2. a neutron becomes an alpha particle
3. aluminum decays into a neutron
4. aluminum produces a beta particle
Identify the missing particle in the following nuclear reaction:

⁹₄Be + ¹₁H → _____ + ⁴₂He
1. ⁶₃Li
2. ¹⁴₇N
3. ⁵₂He
4. ⁴₁H
What type of decay is evident in the nuclear reaction shown below?

⁹₄Be + ¹₁H → ⁶₃Li + ⁴₂He
1. alpha
2. beta
3. gamma
4. none of these
Identify the missing particle in the following nuclear reaction:

_____ → ⁴₂He + ²⁰⁸₈₁Tl + ⁰₀g
1. ²¹²₈₃Bi
2. ²⁰⁴₇₉Au
3. ²⁰⁴₈₃Bi
4. ²¹²₇₉Au
What type of decay is evident in the nuclear reaction shown below?

²¹²₈₃Bi → ⁴₂He + ²⁰⁸₈₁Tl + ⁰₀g
1. alpha
2. beta
3. gamma
4. none of these
Which of the following statements best describes the changes occuring in the reaction below?

²¹²₈₃Bi → ⁴₂He + ²⁰⁸₈₁Tl + ⁰₀g
1. bismuth is converted to thallium
2. bismuth is converted to thulium
3. bismuth is converted to helium
4. helium produces thallium
Identify the missing particle in the following nuclear reaction:

¹⁴₆C → ⁰_-1e + _____
1. ¹⁴₇N
2. ¹⁴₅B
3. ¹⁴₆C
4. ¹⁵₇N
What type of decay is evident in the nuclear reaction shown below?

¹⁴₆C → ⁰_-1e + ¹⁴₇N
1. alpha
2. beta
3. gamma
4. none of these
Which of the following statements best describes the changes occuring in the reaction below?

¹⁴₆C → ⁰_-1e + ¹⁴₇N
1. carbon-14 decays to become nitrogen-14
2. one isotope of carbon becomes another isotope of carbon
3. carbon turns into an electron
4. nitrogen decays to form an electron
Identify the missing coefficient in the following nuclear reaction:

²³⁵₉₂U + ¹₀n → ____¹₀n + ¹³⁹₅₃I + ⁹⁵₃₉Y + ⁰₀g
1. 1
2. 2
3. 3
4. 4