2.An atom with high ionization energy will form a positive ion more easily than an atom
with low ionization energy.
3.On the periodic table, the trend in ionization energy is the opposite of the trend in atomic size.
4.Atomic size increases as you move from left to right across a period of elements.
5.The ionization energy of sodium is higher than that of magnesium.
6.Which of the following possesses the highest first ionization energy value?
7.Which of the following ranks ions from smallest to largest radius?
a. Al3+, Ca2+, Cs+
b.Ca2+, Cs+, Al3+
c. Cs+, Ca2+, Al3+
d. Al3+, Cs+, Ca2+
8.The shorthand electron configuration [Rn]7s25f2 describes the electrons of which element?
9.The 57th electron in an atom's electron configuration will be placed into which orbital?
9.Transition metal elements are in the "d block" on the periodic table, because the electron configuration of every transition metal ends with electrons in "d" atomic orbitals.
10.The full electron configuration for rubidium is 1s22s22p63s23p64s24d104p65s1.