bui (ab35974) – Atoms & Electrons – bowers – (136001A)
This print-out should have 27 questions.
Multiple-choice questions may continue on
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What is the order of decreasing atomic radius?
1. titanium, chromium, cobalt
2. chromium, titanium, cobalt
3. cobalt, titanium, chromium
4. chromium, cobalt, titanium
5. cobalt, chromium, titanium
6. titanium, cobalt, chromium
Which of the following correctly rationalizes
the increase in atomic radii down and to the
left on the periodic table, based on what we
discussed in class?
1. Because the elements are easier to ion-
ize, they have a larger electronegativity, and
therefore their electron affinity is not suffi-
cient to reduce atomic radii.
2. None of these. Atomic radii increase up
and to the right.
3. As you move to the left across a period,
decreasing ENC means the outer electrons
are less tightly held and can move further
from the nucleus. As you move down a group,
the electrons occupy orbitals that are further
from the nucleus.
4. Larger elements have an increasing pro-
portion of d and f orbitals, which are intrinsi-
cally larger than all of the s and p orbitals.
5. The elements are simply larger due to
more protons and neutrons.
6. The periodic table was set up to group
atoms by size to facilitate comparisons.
In the neutral Al atom, what are the effective
nuclear charges for a 1s electron and a valence
1. +12; +3
2. +10; +13
3. +13; +3
4. +3; +3
5. +12; +12
Consider the most stable ions which are
formed by the elements Cs, Ba, Te and I.
Which element will form the ion with the
largest radius? (Hint: the ions will be isoelec-
Why is it harder to remove an electron from
fluorine than from carbon, or, to put it an-
other way, why are the valence electrons of
fluorine more strongly bound than those of
1. Fluorine has a nearly filled octet, which
is always more stable