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Subatomic Particles Quiz
This A-Level Chemistry quiz assesses your knowledge of subatomic particles and their properties. Review the topic before the quiz here: Subatomic particles revision notes and worksheet.
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1. Which of the following statements about subatomic particles is correct?
d) Protons, located in the nucleus, define the element. The number of protons is the atomic number.
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2. An atom of an element has a mass number of 40 and an atomic number of 18. Which of the following represents the number of protons, neutrons, and electrons in this atom?
a) Mass number (40) = protons (18) + neutrons. Neutrons = 40 - 18 = 22. The atom is neutral, so the number of protons equals the number of electrons.
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3. Which of the following pairs represents isotopes of the same element?
a) Isotopes have the same number of protons (same element) but different numbers of neutrons (different mass numbers).
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4. The relative atomic mass of chlorine is 35.5. This indicates that:
b) A non-whole number relative atomic mass indicates the presence of isotopes, as it's a weighted average.
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5. Which of the following best explains why isotopes of the same element have the same chemical properties?
c) Chemical properties are determined by the number and arrangement of electrons, which are the same for isotopes of an element.
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6. An ion of element X has a charge of +2 and contains 10 electrons. How many protons are in the nucleus of element X?
c) The ion has a +2 charge, meaning it has lost 2 electrons. Since it has 10 electrons, it must have 10 + 2 = 12 protons.
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7. Which of the following is not a use of radioactive isotopes?
d) Relative atomic mass is determined using stable (non-radioactive) isotopes.
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8. Which subatomic particle contributes negligibly to the mass of an atom?
c) Electrons have a mass of approximately 1/1836 amu, which is negligible compared to protons and neutrons.
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9. Which statement is incorrect regarding relative atomic mass?
d) Relative atomic mass is usually not a whole number because it's a weighted average of isotopic masses.
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10. Element Y has two isotopes: ⁷⁰Y (20% abundance) and ⁷²Y (80% abundance). What is the relative atomic mass of Y?
b) Relative Atomic Mass (Ar) = (70 × 20) + (72 × 80) / 100 = 71.6
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