CHEMISTRY
Midterm Review, Chapters 5, 6
1.
2.
Indicate whether each statement is true or false.
__T_
A sodium ion (Na+) has the same electron configuration as the fluoride ion (F–).
__F_
A positive ion (cation) has a larger atomic radius than the neutral atom of the same element
__F_
A chlorine atom has a larger atomic radius than a potassium atom.
__F_
A neon atom has a larger atomic radius than a lithium atom.
Arrange the elements, Na, Li, F, Sr, Ne in order of increasing atomic radius (start with the smallest atomic
radius on the left and end with the largest atomic radius on the right).
smallest atomic radius
Sr  Na  Li  F  Ne
3.
4.
Circle the larger particle in each pair.
a.
N
N 3
b.
Ca
Ca 2
c.
Cl
Br
d.
Cu 
Cu 2
Arrange the following elements from left to right in order of increasing electronegativity (starting with the least
electronegative element on the left). Oxygen, magnesium, fluorine, phosphorus.
Least electronegative
5.
Mg  P  O  F
most electronegative
Circle the particle in each pair with the greater ionization energy for the outermost electron.
a.
b.
c.
d.
6.
largest atomic radius
Na
Ar
Mg
F
Na 
Mg
Ca
I
Give an example element from each group listed.
Transition metals Fe
Alkalai metals Na
Halogens F
Nobel gases, which do not tend to form ions. He
The nonmetal group that tends to form ions with a negative two (–2) charge O
A nonmetal Cl
1
7.
8.
9.
Identify the group and period for each element or identify the element for the given group and period.
Element Symbol
Group Number
Period Number
Br
17
4
Mg
2 (2A)
3
S
16
3
F
17 (7A)
2
Write the electron configuration for each ion.
a.
Mg 2 1s 2 2s 2 2 p 6   Ne
b.
F  1s 2 2s 2 2 p 6   Ne
Write the ion, including the charge, that each atom is most likely to form.
Ca
Ca
O
2
O
S
2
S
Cs
2
10. What is the electric charge on
a. An ion with nine protons and ten electrons
b. An ion with 12 protons and 10 electrons
c. An ion with 34 protons and 36 electrons
11. Name each ion.
Formula
Cs 
1−
2+
2−
Name
PO 43
Phosphate
SO 4 2
Sulfate
NO3
Nitrate
OH 
Hydroxide
Cl 
Chloride
N 3
Nitride
2
12. How many valence electrons does each atom have?
O, 6
S, 6
Ca, 2
Na, 1
13. Write the electron configuration for each ion.
a.
Mg 2
1s 2 2 s 2 2 p 6   Ne 
b.
O 2
1s 2 2 s 2 2 p 6   Ne 
c.
Cu 2
 Ar  3d 9
14. Write the ion typically formed by each atom.
Atom
Typical Ion
O
O 2
S
S2 
Ba
Ba 2 
Br
Br 
P
P 3
Na
Na 
15. Name each ionic compound, and write the ions from which it is made.
Ionic Compound
Compound Name
Ions
Ca  OH 2
Calcium hydroxide
Ca 2
OH 
Al2 O3
Aluminum oxide
Al3
O 2
Ag 2O
Silver oxide
Ag 
O2
3
16. Write the correct formula of the compound formed by each pair of ions and write the name of the compound
Cation
Anion
Compound Formula
Compound Name
Ba 2 
PO 43
Ba 3  PO4 2
Barium phosphate
Ca 2 
SO 4 2
CaSO4
Calcium sulfate
Na 
NO3
NaNO3
Sodium nitrate
Al3
NO3
Al  NO3 3
Aluminum nitrate
Ag 
Cl 
AgCl
Silver chloride
Li 
PO 43
Li3PO4
Lithium phosphate
K
N 3
K3 N
Potassium nitride
Ag 
S2 
Ag 2S
Silver sulfide
4