Quiz on Electron Behavior and Atomic Structure

Which of the following best explains both the wave and particle natures of electrons?

• Electrons exhibit wave-like behavior in diffraction and interference patterns, and particle-like behavior in photoelectric effect and collisions.

• Electrons only exhibit wave-like behavior in all experiments.

• Electrons only exhibit particle-like behavior in all experiments.

• Electrons do not exhibit any wave or particle-like behavior.

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NGSS.HS-PS4-3

Explain the relationship between electrons, energy, and electromagnetic radiation.

• Electrons absorb energy and emit electromagnetic radiation when they move to a higher energy level.

• Electrons release energy and absorb electromagnetic radiation when they move to a lower energy level.

• Electrons neither absorb nor emit energy when interacting with electromagnetic radiation.

• Electrons only emit energy without any interaction with electromagnetic radiation.

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NGSS.HS-PS4-1

NGSS.HS-PS4-3

Summarize the mathematical relationship between the speed, wavelength, and frequency of electromagnetic radiation.

• The speed of electromagnetic radiation is the product of its wavelength and frequency.

• The speed of electromagnetic radiation is the sum of its wavelength and frequency.

• The speed of electromagnetic radiation is the difference between its wavelength and frequency.

• The speed of electromagnetic radiation is the ratio of its wavelength to frequency.

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NGSS.HS-PS4-1

Which of the following correctly lists the types of radiant energy in the electromagnetic spectrum in order of increasing wavelength?

• Gamma rays, X-rays, Ultraviolet, Visible, Infrared, Microwaves, Radio waves

• Radio waves, Microwaves, Infrared, Visible, Ultraviolet, X-rays, Gamma rays

• X-rays, Gamma rays, Ultraviolet, Visible, Infrared, Microwaves, Radio waves

• Infrared, Visible, Ultraviolet, X-rays, Gamma rays, Microwaves, Radio waves

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NGSS.HS-PS4-1

What makes an atom stable and what might an atom do to become stable? Identify which elements are already stable and why.

• An atom is stable when it has a full outer electron shell, and it may gain, lose, or share electrons to achieve this. Noble gases are already stable because they naturally have full outer electron shells.

• An atom is stable when it has an equal number of protons and neutrons, and it may change its number of protons to achieve this. Alkali metals are already stable because they have one electron in their outer shell.

• An atom is stable when it has more electrons than protons, and it may gain protons to achieve this. Halogens are already stable because they have seven electrons in their outer shell.

• An atom is stable when it has a full inner electron shell, and it may lose electrons to achieve this. Transition metals are already stable because they have partially filled d subshells.

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NGSS.HS-PS1-1

NGSS.HS-PS1-2

What is the main difference between cations and anions?

• Cations are positively charged, while anions are negatively charged.

• Cations are negatively charged, while anions are positively charged.

• Cations have no charge, while anions have a charge.

• Cations and anions both have the same charge.

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NGSS.MS-PS2-3

Which of the following best illustrates the valence electrons of atoms using Lewis structures?

• Dot symbols around the element symbol

• Lines connecting element symbols

• Numbers indicating electron count

• Arrows showing electron movement

Draw a Bohr model and a Lewis structure for sulfur on scratch paper.

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NGSS.HS-PS1-1

Differentiate between Bohr’s model of the atom and the quantum model of the atom.

• Bohr's model describes electrons in fixed orbits, while the quantum model describes electron probabilities in orbitals.

• Bohr's model is based on electron clouds, while the quantum model uses fixed paths for electrons.

• Bohr's model incorporates the uncertainty principle, while the quantum model does not.

• Bohr's model uses wave functions, while the quantum model uses particle trajectories.

Summarize the organization of the first three shells of the electron cloud. Include their orbitals and how many total electrons they can hold.

• The first shell has 1s orbital and holds 2 electrons; the second shell has 2s and 2p orbitals and holds 8 electrons; the third shell has 3s, 3p, and 3d orbitals and holds 18 electrons.

• The first shell has 1s orbital and holds 2 electrons; the second shell has 2s and 2p orbitals and holds 8 electrons; the third shell has 3s and 3p orbitals and holds 8 electrons.

• The first shell has 1s orbital and holds 2 electrons; the second shell has 2s, 2p, and 2d orbitals and holds 10 electrons; the third shell has 3s, 3p, and 3d orbitals and holds 18 electrons.

• The first shell has 1s orbital and holds 2 electrons; the second shell has 2s and 2p orbitals and holds 8 electrons; the third shell has 3s, 3p, and 3d orbitals and holds 10 electrons.