AP Chemistry Unit 4

Which of the following explains why atomic radius increases as you go down a group?

• The number of particles in the nucleus of the atom increases

• The number of electrons in the outermost shell of the atom increases

• The attractive force between the valence electrons and the nuclei of the atoms decreases

• the repulsive force between the valence electrons and the electrons in the inner shell decreases.

Which of the following explains why sulfur has a lower first ionization energy than phosphorus in spite of the typical periodic trend? (draw an orbital diagram)

• The atomic radius of sulfur is greater than fluorine.

• Sulfur has a set of paired electrons in 3p which repel the other 3p electrons

• Phosphorus has a greater nuclear charge than sulfur and holds its electrons tighter

• Sulfur on average has more neutrons than phosphorus which interrupt and weaken the coulombic attraction between protons and electrons.

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The mass, in grams, of 1.35 x 10^26 molecules of water is equal to

• 114.78 mol PbI₂

• 0.904 grams PbI₂

• 0.904 mol PbI₂

• 114.78 grams PbI₂

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NGSS.HS-PS1-7

• 408 g KClO₃

• 804 g KClO₃

• 598 g KClO₃

• There is not enough information.

Which electron configuration belongs to a Chloride (Cl^-) ion?

• 1s² 2s² 2p⁶ 3s² 3p⁵

• 1s² 2s² 2p⁶ 3s² 3p⁶

• 1s² 2s² 2p⁶ 3s² 3p⁷

• 1s² 2s² 2p⁶ 3p⁷

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NGSS.HS-PS1-1

Using the table, how many valence electrons does unknown element P have? ***P IS NOT PHOSPHORUS IN THIS CASE!***

• 5

• 2

• 3

• 4

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NGSS.HS-PS1-1

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What would the charge of Q be if it were to become an ion?

• 3-

• 3+

• 5-

• 5+

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NGSS.HS-PS1-1

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Calculate the number of sulfate ions in 100.0 grams of Aluminum Sulfate.

• 3.519 x 10^23 sulfate ions

• 2.639 x 10^23 sulfate ions

• 6.121 x 10^24 sulfate ions

• 2.057 x 10^24 sulfate ions

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NGSS.HS-PS1-7

The graph shows the successive ionization energies of an unknown element. In which group would you expect to find this element?

• 7

• 6

• 16

• 17

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NGSS.HS-PS1-1

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