CHEM
35
General
Chemistry
November 10, 2000
Name:
Largo, Key
1.
Atomic size decreases
across a period, even though the number of electrons increases. Explain
why this trend is observed.
As
you go across a period, the atomic number (Z) increases indicating similar
increases in the number of protons and electrons. The added electrons, however,
experience an increased electrostatic attraction due to the increased positive
charge, as the degree of shielding remains constant. Thus, Zeff increases
as you go across a period, resulting in a greater attractive force on the
valence electrons, pulling them in closer to the nucleus. Thus, atomic radii decrease
as you go across a period.
2.
Titanium (Z = 22) is a
transition metal. What is the ground state electron configuration for the Ti2+
ion?
For
the neutral Ti atom:
1s22s22p63s23p64s23d2
We
remove electrons, however, from the 4s orbital first, giving the
following for Ti2+:
1s22s22p63s23p63d2
3.
O2- and Na+
and Al3+ are all isoelectronic with Ne. Arrange these four
isoelectronic species in order of increasing radius. Give a very brief
justification for your answer.
Atomic
number increases as we go from O2- to Ne to Na+ to Al3+,
so Zeff increases (number of electrons are same for all, so shielding
is the same). Thus, species radius will decrease with increasing Zeff.
In
order of increasing radius: Al3+
< Na+ < Ne < O2-