S2-Q8- AR-IP -EA-EN

Which one has the largest radius?

• Lithium (Li, atomic #3)

• Boron (B, atomic #5)

• Neon (Ne, atomic #10)

• Nitrogen (N, atomic #7)

Which of the following elements would have the largest bond length when reacting with chlorine ?

• copper

• zinc

• silver

• cadmium

How does the atomic radius affect the ionization energy?

• Decreasing the atomic radius leads to a higher ionization energy.

• Increasing the atomic radius leads to a higher ionization energy.

• Decreasing the atomic radius leads to a lower ionization energy.

• The atomic radius does not affect ionization energy at all.

Which of the following is the correct order from greatest to least according to the second ionization energy?

• Mg, Na, Ca, K

• Mg, Na, K, Ca

• Mg, Ca, Na, K

• K, Ca, Na, Mg

• Na, K, Mg, Ca

The table shows how electron affinity generally decreases when moving down elements in group 17, the halogens. However, the data shows fluorine to be anomalous. Which of the following provides the correct explanation for the lower electron affinity of fluorine?

• Chlorine is actually the anomalous element, as its electron affinity is greater than it should be because of screening from the 3d electrons.

• An atom of fluorine is smaller than an atom of chlorine, so the extra electron experiences significantly more electron repulsion in fluorine, reducing its electron affinity.

• An atom of chlorine obtains a full outer shell through the addition of an electron, which an atom of fluorine does not.

• There is a stronger attraction between the nucleus and the incoming electron in an atom of chlorine, giving it a greater electron affinity.

Which of the following transition metals atom would you predict to have the lowest electron affinity?

[refer to Electronic configuration]

• iron Fe₂₆

• Cobalt Co₂₇

• Manganese Mn₂₅

• Vanadium V₂₃

Why is there a decrease in electron affinity between carbon and nitrogen?

• The added electron is placed in a shell farther from the nucleus in an atom of nitrogen.

• The addition of an electron to an atom of carbon will create a half-filled 2p subshell, which is energetically unfavorable.

• An atom of nitrogen has a half-filled 2p subshell, so an additional electron will be added to an already filled orbital and stability will decrease.

• An atom of carbon has a half-filled second electron shell, so an additional electron will experience more repulsion compared with that it would experience in an atom of nitrogen.

Which of the following elements has the lowest value of electronegativity according to the Pauling scale?

• S

• Mg

• Al

• Cl

Why do no values exist on the Pauling scale of electronegativity for argon, neon, and helium?

• These noble gases exist as electrically neutral atoms.

• These noble gases require too much energy to be ionized.

• These noble gases have too great an electron density.

• These noble gases do not form bonds; therefore, no bond dissociation energy data is available.

Which letter corresponds to the elements in the periodic table that are the most electronegative?

• A

• B

• C

• D