Unit 1 Chemistry Review

What causes the emission spectrum of an element? 

• movement of electrons from a lower energy state to a higher energy state.
• movement of protons from a lower energy state to a higher energy state.
• movement of electrons from a high energy state to a lower energy state.
• movement of protons from a high energy state to a lower energy state.

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NGSS.HS-PS4-3

The wavelength of a line in the emission spectrum of an atom is inversely proportional to the

• charge characteristically lost when an electron drops to a lower energy state.
• energy characteristically released when an electron falls to a lower energy state.
• kinetic energy gained by the nucleus when heat energy is added to the atom.
• energy released by the nucleus when heat energy is removed from the atom.

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NGSS.HS-PS4-1

NGSS.HS-PS4-3

Flame tests can be used to identify an element. Each element emits characteristic waves of light when it is heated in a flame. What describes how the light is produced? 

• Protons in the ground state lose energy and give off light
• Protons in the ground state gain energy and are emitted from the nucleus, giving off light.
• Electrons in the ground state lose energy, and move to an excited state, giving off light.
• Electrons in the ground state gain energy, move to an excited state, and give off light when they return to the ground state.

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NGSS.HS-PS4-3

A student has a homework assignment to identify the properties of an element based on its electron configuration. If the element has an electron configuration of 1s²2s²2p⁶3s²3p⁶4s²3d¹⁰4p⁵. Which of the following is most likely a property of this element? 

• has low electronegativity.
• Forms -1 ions
• is malleable
• reacts with fluorine to form a salt

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NGSS.HS-PS1-1

If a radio station were to increase its frequency from 94.5 MHz to 99.1 MHz, what would happen to the station's wavelength?

• The wavelength would not change
• The wavelength would go up
• The wavelength would go down
• The wavelength would double

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NGSS.HS-PS4-1

In the Bohr model of the hydrogen atom, which of the following transitions results in light you can see?

• n=1 to n=2
• n=6 to n=2
• n=6 to n=3
• n=5 to n=3

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NGSS.HS-PS4-1

Which of the following electromagnetic waves has photons of the highest energy?

• microwaves
• infrared
• x-rays
• ultraviolet

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NGSS.HS-PS4-1

NGSS.HS-PS4-3

In the figure above, why are there dots beyond the "boundary of the atomic orbital"?

• the boundary encloses the volume in which the electron is found 90% of the time.
• the boundary is three dimensional, while the picture shows only two dimensions
• experimental error
• the boundary encloses the volume in which the electron is found 50% of the time.

What is the wavelength of the photon emitted when the electron of a hydrogen atom transitions from n=4 to n=1? 

• 97 nm
• 103 nm
• 122 nm
• 410 nm

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NGSS.HS-PS4-1

NGSS.HS-PS4-3

In what part of the electromagnetic spectrum does the photon emitted lie when the electron of a hydrogen atom transitions from n=4 to n=3?

• ultraviolet
• visible
• infrared
• there is not enough information to determine the region.

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NGSS.HS-PS4-1