Drawing Ionic Bonds Worksheet Answers

Bonding Basics - Ionic Bonds				Name _______________________
Complete the chart for each element.
	Element	# of Protons	# of Electrons	# of Valence Electrons	Oxidation Number
	Sodium
	Chlorine
	Beryllium
	Fluorine
	Lithium
	Oxygen
	Phosphorus

Follow your teacher's directions to complete each ionic bond.

(1) Potassium + Fluorine

(2) Magnesium + Iodine

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
Sodium	11	11	-> 10	1	1+
Chlorine	17	17	-> 18	7	1-
Beryllium	4	4	-> 2	2	2+
Fluorine	9	9	-> 10	7	1-
Lithium	3	3	-> 2	1	1+
Oxygen	8	8	-> 10	6	2-
Phosphorus	15	15	-> 18	5	3-

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 (-), which relates to the charge or oxidation number. If the ion has more protons (+), it would be a positive ion. If it has more electrons (-), it would be a negative ion.

Follow your teacher's directions to complete each ionic bond.

			Step 2
	(1) Potassium + Fluorine		Step 3
	1- Write the symbols for each element.	K	F
	2 - Use Fruity Pebbles (or other cereal/candy with more
	than one color) to create the Lewis structure for each.	Step 1

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.

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 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-
Na		Na2O
	Students will start with one sodium and one

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

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

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

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

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