ATOMIC STRUCTURE QUIZ – Test Your Knowledge and ability today.
At the end, Score yourself over 20 after testing your knowledge:
1. Which of the following best describes an atom?
A. The smallest particle of an element that can exist
B. The smallest particle of a compound
C. The smallest unit of a mixture
D. The smallest particle of a molecule
2. Who proposed the atomic theory that states matter is made of indivisible particles?
A. J.J. Thomson
B. John Dalton
C. Ernest Rutherford
D. Niels Bohr
3. Which subatomic particle carries a positive charge?
A. Electron
B. Neutron
C. Proton
D. Nucleus
4. The subatomic particle with no electrical charge is called the
A. Proton
B. Electron
C. Neutron
D. Ion
Atomic structure Quiz
5. Where are protons and neutrons found in an atom?
A. In the electron shell
B. In the nucleus
C. In the outer orbit
D. In the valence shell
6. Electrons are mainly found
A. Inside the nucleus
B. Around the nucleus in shells
C. Inside protons
D. Inside neutrons
7. The atomic number of an element represents the number of
A. Neutrons only
B. Electrons only
C. Protons only
D. Protons and neutrons
8. What is the mass number of an atom?
A. Number of electrons only
B. Number of protons only
C. Number of neutrons only
D. Number of protons and neutrons
9. The number of neutrons in an atom is calculated by
A. Atomic number minus mass number
B. Mass number minus atomic number
C. Atomic number plus mass number
D. Atomic number divided by mass number
10. Isotopes are atoms that have the same
A. Mass number but different atomic number
B. Atomic number but different mass number
C. Number of neutrons and electrons
D. Chemical formula only
Atomic structure Quiz
11. Why do isotopes have similar chemical properties?
A. They have different nuclei
B. They have the same number of protons
C. They have the same number of electrons
D. They have the same mass
12. The relative atomic mass of an element is based on
A. Only the lightest isotope
B. Only the heaviest isotope
C. The average mass of its isotopes
D. The mass of hydrogen
13. Rutherford’s atomic model shows that the atom has
A. A solid structure
B. No nucleus
C. A central nucleus
D. No electrons
14. Which experiment led to Rutherford’s discovery of the nucleus?
A. Cathode ray experiment
B. Oil drop experiment
C. Gold foil experiment
D. Electrolysis experiment
Atomic structure Quiz
15. One major weakness of Rutherford’s model was that it could not explain
A. Atomic mass
B. Atomic stability
C. Atomic number
D. Atomic volume
16. Bohr’s model improved Rutherford’s model by introducing
A. Random electron movement
B. Fixed energy levels
C. Solid electrons
D. No nucleus
17. Electron shells are also known as
A. Orbits
B. Protons
C. Nuclei
D. Ions
18. The electronic configuration of sodium (Na) is
A. 2,7,1
B. 2,8,1
C. 2,6,3
D. 2,5,4
19. Valence electrons are found in the
A. Nucleus
B. Innermost shell
C. Middle shell
D. Outermost shell
20. Elements are chemically reactive mainly because of their
A. Number of neutrons
B. Mass number
C. Valence electrons
D. Atomic size
ANSWERS AND EXPLANATIONS on Atomic structure Quiz
1. A – An atom is the smallest particle of an element that can exist and still retain its properties.
2. B – John Dalton proposed the first modern atomic theory.
3. C – Protons carry a positive electrical charge.
4. C – Neutrons have no electrical charge.
5. B – Protons and neutrons are located in the nucleus.
6. B – Electrons move around the nucleus in shells.
7. C – Atomic number is equal to the number of protons.
8. D – Mass number is the total of protons and neutrons.
9. B – Neutrons are found by subtracting atomic number from mass number.
10. B – Isotopes have the same atomic number but different mass numbers.
11. C – They have the same number of electrons, which determines chemical behavior.
12. C – Relative atomic mass is the weighted average of isotopes.
13. C – Rutherford discovered the central nucleus.
14. C – The gold foil experiment revealed the nucleus.
15. B – Rutherford’s model could not explain why electrons do not fall into the nucleus.
16. B – Bohr introduced fixed energy levels for electrons.
17. A – Electron shells are also called orbits.
18. B – Sodium has 11 electrons arranged as 2,8,1.
19. D – Valence electrons are in the outermost shell.
20. C – Chemical reactivity depends mainly on valence electrons.
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