Practice Questions for Chp 7.1 to 7.3
Multiple Choice
1. This diagram represents:
a. a cation
b. an anion
c. a neutral atom
2. Of the following, which is a molecular element?
a. carbon dioxide c. nitrogen gas
b. table salt
d. ice
3. A potassium ion has
a. 18 protons and 19 electrons
b. 19 protons and 19 electrons
c. 18 protons and 18 electrons
d. 19 protons and 18 electrons ** note change**
4. If an element has an atomic number of 13 and
an atomic mass of 27, how many neutrons does
it have?
a. 13
b. 14
c. 27
5. The Bohr-Rutherford diagram of oxygen suggests
that in ionic compounds, oxygen would have a
charge of :
a. 0
b. -2
c. +2
d. -1
6. The Bohr-Rutherford diagram shown represents a
a. neutral atom
b. neutral molecule
c. -1 ion
d. +1 ion
7. The diagram shows
8. Which would be a correct name for the compound Li2O?
a. lithium oxygen
c. dilithium oxygen
b. lithium oxide
d. lithide dioxygen
9. In the chemical formula NaHCO3, there are
a. four different elements
b. four non-metallic elements
c. three atoms in total
d. twelve atoms in total
10.
The chemical formula KNO3 indicates there are:
a. 3 potassium, 1 nitrogen and 3 oxygen atoms
b. 1 potassium, 1 nitrogen and 3 oxygen atoms
c. 3 potassium, 3 nitrogen and 3 oxygen atoms
11. Which is the number of sulfur atoms in K2SO4
a. 2
b. 1
c. 4
12. The correct name for CaBr2 is:
a. calcium bromide
b. calcium dibromide
c. monocalcium dibromide
13. The correct chemical formula for
diphosphorus pentaoxide is:
a. PO5
b. P2O5
c. P5O2
14.
Which of the following is a compound?
a. H2
b. NaCl
c. Mg
15.
Which of the following elements has 6 electrons in
its second shell?
*Hint: draw a Bohr-Rutherford diagram.*
a. O
b. F
c. S
16. Which two ions have the same number of electrons?
a. sodium and potassium
b. fluorine and chlorine
c. sodium and fluorine
d. none of the above
17. Of the following, which represents the most stable
element?
a. how sodium and chlorine form a covalent bond
b. how sodium and chlorine become new elements
by exchanging an electron
c. how sodium and chlorine form an ionic bond
a. Diagram 1
b. Diagram 2
c. Diagram 3
d. Diagram 4
18.
Complete the following table:
Chemical
formula
Composition
Type of compound
Name
SO3
1 sulfur atom
3 oxygen atoms
Both non-metals
 Molecular compound
Sulfur trioxide
CaCl2
1 calcium ion
2 chloride ions
Metal with non-metal
 Ionic compound
Calcium chloride
MgO
1 magnesium ion
1 oxide ion
Metal with non-metal
 Ionic compound
Magnesium oxide
CF4
1 carbon atom
4 fluorine atoms
Both non-metals
 Molecular compound
Carbon tetrafluoride
Li2O
2 lithium ions
1 oxide ion
Metal with non-metal
 Ionic compound
Lithium oxide
Na2S
2 sodium ions
1 sulfide ion
Metal with non-metal
 Ionic compound
Sodium sulfide
BeF2
1 beryllium ion
2 fluoride ions
Metal with non-metal
 Ionic compound
Beryllium fluoride
N2O
2 nitrogen atoms
1 oxygen atom
Both non-metals
 Molecular compound
Dinitrogen monoxide
CaO
1 calcium ion
1 oxide ion
Metal with non-metal
 Ionic compound
Calcium oxide
P4O10
4 phosphorus atoms
10 oxygen atoms
Both non-metals
 Molecular compound
Tetraphosphorus decaoxide
Na3N
3 sodium ions
1 nitride ion
Metal with non-metal
 Ionic compound
Sodium nitride
N2O4
2 nitrogen atoms
4 oxygen atoms
Both non-metals
 Molecular compound
Dinitrogen tetraoxide
Al2O3
2 aluminum ions
3 oxide ions
Metal with non-metal
 Ionic compound
Aluminum oxide
Mg3P2
3 magnesium ions
2 phosphide ions
Metal with non-metal
 Ionic compound
Magnesium phosphide
IF7
1 iodine atom
7 fluorine atoms
Both non-metals
 Molecular compound
Iodine heptafluoride
KI
1 potassium ion
1 iodide ion
Metal with non-metal
 Ionic compound
Potassium iodide
H2 S
2 hydrogen atoms
1 sulfur atom
Both non-metals
 Molecular compound
Dihydrogen monosulfide
MgCl2
1 magnesium ion
2 chloride ions
Metal with non-metal
 Ionic compound
Magnesium chloride
1 carbon atom
1 oxygen atom
Both non-metals
 Molecular compound
Carbon monoxide
CO
Chemical
formula
Composition
Type of compound
Name
SO2
1 sulfur atom
2 oxygen atoms
Both non-metals
 Molecular compound
Sulfur dioxide
PF5
1 phosphorus atom
5 fluorine atoms
Both non-metals
 Molecular compound
Phosphorus pentafluoride
LOSE electrons; while non-metals tend to ________
GAIN electrons.
19. In forming ionic compounds, metals tend to ________
20. When magnesium reacts with fluorine to form an ionic compound, what is the expected chemical formula for the
compound? Explain how you got your answer.
Either draw the bohr Rutherford diagrams OR the Lewis dot diagrams for both Magnesium and Fluorine.
Mg
F
F
Because magnesium will need to lose 2 electrons,
and each fluorine can only gain 1 electron….……
so you will need 2 fluorine for every 1 magnesium
Chemical formula (metal always goes first!):
MgF2