AP Chemistry Unit 8 Electrons and Periodicity PRE/POST Test

Neon lighting is one application using concepts from emission spectroscopy. Which of the following best describes how the emission process works in neon lighting?

• Ultraviolet light excites the neon gas to produce emitted white light.

• Energy excites the neon gas to an excited state. The relaxation to ground state causes light to be emitted.

• Neon gas reacts with oxygen in the air, which causes the emission of light.

• none of the above.

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Which of the following regions of the electromagnetic spectrum has the lowest frequency?

• ultraviolet
• infrared
• visible
• x-ray

Which electron transition is an absorption of energy?

• n= 4 to n= 3
• n=2 to n=4
• n=3 to n=1
• n=3 to n=0

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What is the shorthand electron configuration for Sulfur atom?

• [Ar] 3p⁴
• [He] 3s²3p⁴
• [Ne] 3s²3p⁴
• [Na] 3s²3p³
  

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Which of the following will have a larger radius than Zinc?

• Gallium
• Aluminum
• Magnesium
• Strontium

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NGSS.HS-PS1-1

Which of the following will have a higher electron affinity than arsenic (As)?

• Carbon (C)

• Neon (Ne)

• Antimony (Sb)

• Germanium (Ge)

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Which of the following will have a lower ionization energy than Scandium (Sc)?

• Helium (He)
• Titanium (Ti)
• Calcium (Ca)
• Magnesium (Mg)

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NGSS.HS-PS1-1

Which atom has the largest atomic radius?

• potassium

• rubidium

• neon

• cesium

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NGSS.HS-PS1-1

As you move down the periodic table atoms get bigger. This is because ____________.

• The atoms have more mass.

• The atoms have more protons.

• The atoms have more energy levels and the shielding effect

• The atoms have more neutrons

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NGSS.HS-PS1-1

Which statement correctly and completely identifies a trend?

• Atomic radius decreases across a period and increases down a group.
• Electronegativity decreases across a period and decreases down a group.
• Ionization energy increases across a period and increases down a group.
• Ionic radius increases across a period and increases down a group.

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