AP Chemistry Review

How many protons are in this element?

• 79

• 196

• 117

• Cannot be determined

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Atoms of the same element which have a different number of neutrons are called _________________.

• ions

• isotopes

• quarks

• molecules

Calculate the average atomic mass of silver.

• 106.38649amu

• 111.91896amu

• 107.8677amu

• 121

The Periodic Table of Elements is most related to...

• Chemistry

• Geology

• Astronomy

• Biology

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What is the study of matter and how it changes?

• Biology

• Physics

• Chemistry

• Geology

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What is the electron configuration for this PES graph?

• 1s²2s²2p⁶3s²3p²

• 1s²2s²2p⁶3s²3p¹

• 1s²2s²2p⁶3s²3p³

• 1s²2s²2p⁶3s²

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Which element is represented by this PES graph?

• calcium

• potassium

• titanium

• scandium

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The photoelectron spectra above show the energy required to remove a 1s electron from a nitrogen atom and from an oxygen atom. Which of the following statements best accounts for the peak in the upper spectrum being to the right of the peak in the lower spectrum?

• Nitrogen atoms have a half-filled p subshell.

• There are more electron-electron repulsions in oxygen atoms than in nitrogen atoms.

• Electrons in the p subshell of oxygen atoms provide more shielding than electrons in the p sub shell of nitrogen atoms.

• Nitrogen atoms have a smaller nuclear charge than oxygen atoms.

Answer explanation

"Nuclear charge" = charge of the nucleus. A greater nuclear charge will result in a greater attraction to the 1s electrons, and therefore more energy will be required to remove those electrons.

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A sample containing atoms of C and F was analyze using x-ray photoelectron spectroscopy. The portion of the spectrum showing the 1s peaks for atoms of two elements is shown above. Which of the following correctly identifies the 1s peak for the fluorine atoms and provides an appropriate explanation?

• Peak X, because F has a smaller first ionization energy than C has.

• Peak X, because F has a greater nuclear charge than C has.

• Peak Y, because F is more electronegative than C is.

• Peak Y, because F has a smaller atomic radius than C has.

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Francium (Fr) has the lowest ionization energy in Group 1 because - 

• it has the smallest number of valence electrons

• it has the greatest atomic mass

• it has the greatest number of protons, so it attracts its electrons the strongest

• its 1 valence electron is very far from the nucleus, so little energy is needed to remove it

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