Chapter 4 - Electrons in Atoms

What is the lowest possible energy level that an electron can occupy?

• Lower energy level

• Ground State

• Excited State 

• Depressive State

The blue section of the wave is measuring _________________.

• wavelength
• crest
• trough
• amplitude 

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According to the Bohr Model, electrons are only found in specific orbits around the nucleus called __________________________

• Energy Levels
• Electron Lanes
• Electron Places
• Atomic Mass

When atoms _____________ energy, their electrons move to higher energy levels. These electrons _____________ energy by emitting light when they return to lower energy levels.

• lose, absorb

• absorb, lose

• lose, lose

• absorb, absorb

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Emission spectra (bright line spectra) are created when electrons move from ___.

• higher to lower energy levels.

• lower to higher energy levels.

• s orbitals to p orbitals.

• one atom to a different atom.

Emission spectra emitted by an element (or compound) will produce ___ through a spectroscope.

• discrete bright lines

• a continuous rainbow

• dark lines

• white light

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NGSS.HS-PS4-3

Which wave in the diagram has the highest frequency?

• 1

• 2

• 3

• 4

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For an electron to change from ground state to an excited stated it must...

• Absorb energy
• Release energy

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Why are line emission spectra of elements called "atomic fingerprints"?

• They are all the same
• They are all unique
• They are all similar
• They all contain colored light

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NGSS.HS-PS4-3

What does energy have to do with wavelength and frequency?

• The higher the frequency the less energy the wave has.

• The lower the frequency the more energy the wave has.

• The shorter the wavelength the more energy the wave has.

• The longer the wavelength the more energy the wave has.

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