Ionic Bonds Worksheet Answers can be found in a variety of formats. The most common type of ionic bonds worksheet answer is a PDF. However, you may also find ionic bonds worksheet answers in Excel or Word format. When looking for the correct answer to a bond question, it is important to first determine the type of bond that is being discussed. There are three types of ionic bonds: electrovalent, covalent, and coordinate covalent. Each type has its own unique properties which can be tested using various methods. The best way totest the strength of an ionic bond is usually through melting point or boiling point measurements.
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| Question | Answer |
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| Form Name | Ionic Bonds Worksheet Answers |
| Form Length | 4 pages |
| Fillable? | No |
| Fillable fields | 0 |
| Avg. time to fill out | 1 min |
| Other names | charting oxidation number worksheet, charting oxidation number chapter 7 answers, ionic bonding worksheet answers, charting oxidation number answers |
Bonding Basics - Ionic Bonds |
Name _______________________ |
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Complete the chart for each element. |
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Element |
# of Protons |
# of Electrons |
# of Valence Electrons |
Oxidation Number |
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Sodium |
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Chlorine |
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Beryllium |
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Fluorine |
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Lithium |
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Oxygen |
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Phosphorus |
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Follow your teacher’s directions to complete each ionic bond.
(1) Potassium + Fluorine
(2) Magnesium + Iodine
T. TRIMPE 2002
(3) Sodium + Oxygen
(4) Sodium + Chlorine
(5) Calcium + Chlorine
(6) Aluminum + Chlorine
T. TRIMPE 2002
Bonding Basics - Ionic Bonds |
Answer Key/Teacher Notes |
Complete the chart for each element.
Element |
# of Protons |
# of Electrons |
# of Valence Electrons |
Oxidation Number |
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Sodium |
11 |
11 |
1 |
1+ |
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Chlorine |
17 |
17 |
7 |
1- |
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Beryllium |
4 |
4 |
2 |
2+ |
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Fluorine |
9 |
9 |
7 |
1- |
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Lithium |
3 |
3 |
1 |
1+ |
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Oxygen |
8 |
8 |
6 |
2- |
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Phosphorus |
15 |
15 |
5 |
3- |
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NOTE: I have the students use a red pen/pencil to change the # of electrons to the amount it would be if the valence electrons were removed or added. They can see the difference between the number of protons (+) and electrons
Follow your teacher’s directions to complete each ionic bond.
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Step 2 |
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(1) Potassium + Fluorine |
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Step 3 |
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1- Write the symbols for each element. |
K |
F |
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2 - Use Fruity Pebbles (or other cereal/candy with more |
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than one color) to create the Lewis structure for each. |
Step 1 |
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3 - Draw an arrow (or more if needed) to show the
transfer of electrons and move the cereal to the new location.
4 - Determine the charge for each ion and write the formula.
5 - Make sure the sum of the oxidation numbers is zero and write the chemical formula.
6 - Have the students use a pencil or crayon to draw the electrons as they remove the pieces of cereal.
K1+F1-
KF
K would have a charge of 1+ since it lost an electron
Fluorine would have a charge of 1- since it gained an electron.
(2) Magnesium + Iodine
Mg |
I |
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I
Mg2+ I 12-
MgI2
Mg would have a charge of 2+ since it lost two electrons.
Each I ion would have a charge of 1- since each gained an electron. A subscript “2” is used to show that two ions were used in the bond.
Students will start with one magnesium and one iodine atom. Since the oxidation numbers must equal zero, they will need to add another iodine atom.
T. TRIMPE 2002
(3) Sodium + Oxygen
Na |
O |
Na1+2 O 2- |
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Na |
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Na2O |
Students will start with one sodium and one |
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oxygen atom. Since the oxidation numbers must equal zero, they will need to add another sodium atom.
(4) Sodium + Chlorine
Each Na ion would have a charge of 1+ since each lost an electron. A subscript “2” is used to show that two ions were used in the bond.
The O ion would have a charge of 2- since it gained two electrons.
Na Cl
Na1+Cl1-
NaCl
Na would have a charge of 1+ since it lost an electron
Cl would have a charge of
1- since it
gained an electron.
(5) Calcium + Chlorine
CaCl
Cl
Ca 2+Cl 12-
CaCl2
Ca would have a charge of 2+ since it lost two electrons.
Each Cl ion would have a charge of 1- since each gained an electron. A subscript “2” is used to show that two ions were used in the bond.
(6) Aluminum + Chlorine
Al |
Cl |
Cl |
Cl |
Al3+Cl13-
AlCl3
The Al ion would have a charge of 3+
since it lost three electrons.
Each Cl ion would have a charge of 1- since each gained an electron. A subscript “3” is used to show
that three ions were used in the bond.
T. TRIMPE 2002