Name Date Class
Ionic Bonds
A fluorine (F) ion has a charge of 1–. An aluminum (Al) ion has a charge of 3+. On a
separate sheet of paper, explain how fluorine and aluminum would exchange valence
electrons to form an ionic compound. Then write the compound’s chemical formula and
name the compound.
137D
Name Date Class
Ionic Bonds
1. Negative ions form when atoms valence electrons.
2. In the formation of an ionic compound, a metal atom is most likely to
valence electrons.
3. Ionic compounds form because charges
attract.
Answer the following questions in the spaces provided. You may use a periodic table.
4. A potassium ion has a charge of 1+. A sulfide ion has a charge of 2−.
What is the chemical formula for potassium sulfide?
5. Name the following compound: MgO.
6. ion
7. polyatomic ion
8. ionic bond
9. ionic compound
10. chemical formula
137E
Name Date Class
Ionic Bonds
Pulling Away Electrons
You know that the metals in Group 1 and 2 are quite reactive. They combine
easily with certain other elements to form compounds. Atoms from Group 1 react
by losing one electron; atoms from Group 2 lose two electrons. It takes energy to
remove an electron from an atom. Some atoms hold their electrons tighter than
other atoms do. Also, an individual atom holds some of its electrons tighter than
other electrons.
The size of an atom’s radius affects how tightly it holds its electrons. The larger
the radius of an atom, the farther away from the nucleus some of its electrons
are. The electron held the least tightly is easiest to remove. To remove yet
another electron requires more energy than was needed to remove the first.
The figure below compares the atomic radii of the elements in Groups 1 and 2.
The number underneath each element represents the atomic radius measured
in picometers (pm).
1. What do you notice about atomic radius as you look down a group?
As you look across a period from Group 1 to Group 2?
2. Which element would you expect to be the most reactive in Group 1?
In Group 2? Explain your answer.
3. Within each period, which element of the two groups would you
expect to be more reactive? Explain your answer.
4. Across the periodic table, atomic radius continues to decrease
through Group 17. How does this fact help explain why the
metals in Groups 3 through 13 are less reactive than the metals
in Group 1 and 2?
137F
Name Date Class
Ionic Bonds
Write the letter of the correct answer on the line at the left.
1. Ionic bonds form between two ions that
have
A ionic compounds
B negative charges
C positive charges
D opposite charges
3. Which is most likely to form a negative
ion?
a an element from Group 17
b a metal
C an element from Group 1
d an element with atoms that have eight
valence electrons
2. Ions that are made of more than
one atom are called
A ionic compounds
B crystals
C polyatomic atoms
D ionic bonds
4. Which of the following is the
correct name for MgCl2?
a magnesium chlorine
b magnesium dichlorine
C magnesium chloride
d magnesium dichloride
Fill in the blank to complete each statement.
5. A(n) is an atom or group of atoms that has an electric charge.
6. The attraction between oppositely charged ions is called a(n)
.
7. When an atom loses a valence electron, it becomes a(n) ion.
8. In order to have a stable arrangement of 8 valence electrons, metal atoms are likely
to electrons.
9. In an ionic compound, the total positive charge of all the positive ions
the total negative charge of all the negative ions.
10. Because the force of attraction between the positive and negative ions is so strong,
ionic compounds have melting points.
137