Periodic Trends - AP Question Preview (ID: 57194)
Periodic Trends.
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How does the ionic radius of F- compare to that of O-2?
a) Smaller, because oxygen has more electron repulsions.
b) Smaller, because it has one additional proton.
c) Smaller, because it has only gained one electron.
d) Larger, because it is more electronegative.
How does the atomic radius of Ba compare to Sr, and why?
a) Smaller, because it has more protons in the nucleus.
b) Smaller, because it has a greater electronegativity.
c) Larger, because it has one additional occupied shell of electrons.
d) Larger, because its electrons experience more shielding.
How does the atomic radius of Ca compare to K, and why?
a) Smaller, because calcium has 1 additional proton in the nucleus.
b) Smaller, because its electrons experience less shielding.
c) Larger, because calcium has 1 additional proton in the nucleus.
d) Larger, because it has more electron repulsions.
How does the first ionization energy of Ca compare to Be?
a) Smaller, because it has more protons.
b) Smaller, because the valence electrons experience less shielding.
c) Smaller, because the valence electrons experience more shielding.
d) Larger, because it has more occupied shells of electrons.
Which element below is the most metallic?
a) Li
b) Na
c) K
d) Rb
Which halogen below is the most reactive?
a) Cl
b) Br
c) I
d) At
Which element would have a substantial increase between its 2nd and 3rd ionization energy value?
a) Na
b) Sr
c) Al
d) S
When compared to Ca, an atom of K would have a _____ radius and a ____ first ionization energy.
a) larger; lower
b) larger; greater
c) smaller; lower
d) smaller; greater
How would the ionic radius of Na+ compare to Na?
a) smaller, because it has one less occupied shell of electrons.
b) smaller, because there is less electron repulsion.
c) larger, because it has one additional proton.
d) larger, because it has a lower first ionization energy.
Yo momma is so ugly, not even _______ would bond with her.
a) Fluorine
b) Helium
c) Chlorine
d) Carbon
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