1. Ionic Bonds and Ionic Bonding
Ms. Samayoa
Chemistry
Birmingham community charter high school

2. Learning Objective & Vocab
Learning Objective: Students will understand that when cations and anions combine they form an ionic bond
Academic vocabulary: anions, cations, ions, ionic bond, electrostatic attraction, and lattice structure

3. There are three types of bonds: Ionic bonds Covalent bonds
Metallic bonds
Today we are going to focus on ionic bonding

4. Ionic Bonding
Ionic bonds are chemical bonds that hold metal atoms and nonmetal atoms together

5. Examples of Ionic Bonds
Silver Chloride
Magnesium Iodide
Aluminum Oxide
Call three students and ask which atom is metal and nonmetal and if they make an ionic bond and why

6. Today we are going to focus on salt
The scientific name for table salt is sodium chloride
Sodium chloride happens when sodium and chlorine are held together through an ionic bond

7. Question What does electronegativity mean?
The ability of an atom to steal electrons
Which atom is more electronegative? Sodium or chlorine?
Chlorine is more electronegative
Sodium and chlorine are on the same period and because chlorine has more protons than sodium, it will have a higher electronegativity.

8. What is the electron configuration of sodium?
1s22s23s1
How many valence electrons does sodium have? 1
What is the electron configuration of chlorine?
1s22s23s23p5
How many valence electrons does chlorine have? 7

9. So why do sodium and chlorine form an ionic bond?
The reason why sodium and chlorine form an ionic bond is because they each want a full octet and end up getting electrical charges
Sodium turns into (cation/anion) with a (positive/negative) charge
Chlorine turns into (cation/anion) with a (positive/negative) charge
What do opposite charges like to do?
They like to attract!

10. 1. Start with separate atoms: nonmetal atom and metal atom
2. Sodium atom gives one electron to chlorine atom which changes the charge of the two atoms
cation
anion
3. Atoms get a charge and become ions. They attract each other because they have opposite charges.
Sodium chloride

11. What patterns do you notice amongst ionic bonds?
Metals
Electron givers
Always lose electrons
Cations
Positive charge (+)
Nonmetals
Electron takers
Always gain electrons
Anions
Negative charge (-)

12. Ionic Bonds: Electrostatic Attraction
Remember that opposites attract!
When metals give up an electron, it becomes positive (cation)
When nonmetals gain an electron, it becomes negative (anion)

13. Ionic Bonds: Electrostatic Attraction
Electrostatic Attraction: The force of attraction between a positive charge and a negative charge

14. Lattice Structure
Opposite charges don’t only attract in groups of two!
They can also attract other sodium chlorides and form what is called a lattice structure

15. Names & Formulas of Compounds
Learning Objective: When students are given the formula of a compound, they would be able to write the name. When students are given the name of a compound, they would be able to write the formula.

16. Chemical Formula  Chemical Name
The name of an ionic compound is made up of just two words:
Name of the cation (metal)
Cations have the same names as the elements
For example, K+ = potassium
Name of the anion
Anions, the name changes to – ide
For example, chlorine becomes chloride
Negative Ions
Fluoride F-
Chloride
Cl-
Bromide
Br-
Iodide I-
Oxide
O2-
Sulfide
S2-
Nitride
N3-
Phosphide
P3-

17. Chemical Formula  Chemical Name Example
K2S
Cation is potassium so leave as is
Anion is sulfur so change from sulfur  sulfide
Potassium Sulfide
CaBr2
Cation is Calcium so leave as is
Anion is Bromine so change from bromine  bromide
Calcium Bromide

18. Practice Chemical Formula Chemical Name NaF NaI CsF CsCl LiF BeS CaO
BaS
LiCl
Na2S
MgCl2
BaF2

19. Practice Chemical Formula Chemical Name NaF Sodium Fluoride NaI
Sodium Iodide
CsF
Cesium Fluoride
CsCl
Cesium Chloride
LiF
Lithium Fluoride
BeS
Berrylium Sulfide
CaO
Calcium Oxide
BaS
Barium Sulfide
LiCl
Lithium Chloride
Na2S
Sodium Sulfide
MgCl2
Magnesium Chloride
BaF2
Barium Fluoride

20. Chemical Name  Chemical Formula
Board
Example:
Lithium Oxide
Potassium Nitride
Sodium Chloride
Aluminum Oxide
On the board have periodic table written on it with charges and show how to do certain ionic bond formuals

21. Practice Chemical Name Chemical Formula Lithium Fluoride
Sodium Bromide
Potassium Chloride
Cesium Fluoride
Cesium Bromide
Beryllium Oxide
Magnesium Oxide
Calcium Oxide
Sodium Sulfide
Lithium Oxide
Potassium Oxide
Calcium Chloride
Barium Iodide

22. Practice Chemical Name Chemical Formula Lithium Fluoride LiF
Sodium Bromide
NaBr
Potassium Chloride
KCl
Cesium Fluoride
CsF
Cesium Bromide
CsBr
Beryllium Oxide
BeO
Magnesium Oxide
MgO
Calcium Oxide
CaO
Sodium Sulfide
Na2S
Lithium Oxide
Li2O
Potassium Oxide
K2O
Calcium Chloride
CaCl2
Barium Iodide
BaI2

23. But what about ionic bonds that contain transition metals?
Number
Roman Numerals 1 I 2 II 3
III 4 IV 5 V 6 VI 7
VII 8
VIII 9 IX 10 X
Remember that transition metals DO NOT ALWAYS HAVE THE SAME CHARGE
For example, Iron can have two possible charges: Fe2+ or Fe3+
In order to tell which iron is in the ionic bond, look at the Roman Numerals
Example: Iron (II) Oxide
Am I using Fe2+ or Fe3+?
Answer: Fe2+

24. Check for Understanding
What charge does Tin have in Tin (II) Bromide?
What charge does Tin have in Tin (IV) Chloride?
What charge does Iron have in Iron (III) Chloride?
What charge does Iron have in Iron (II) Bromide?

25. Chemical Name  Chemical Formula
Tin (II) Bromide
Tin (IV) Chloride
Iron (III) Chloride
Iron (II) Bromide
Board

26. Practice Chemical Name Chemical Formula Nickel (III) Bromide
Cobalt (II) Chloride
Lead (IV) Fluoride
Copper (II) Iodide
Iron (III) Iodide

27. Practice Chemical Name Chemical Formula Nickel (III) Bromide NiBr3
Cobalt (II) Chloride
CoCl2
Lead (IV) Fluoride
PbF4
Copper (II) Iodide
CuI2
Iron (III) Iodide
FeI3

28. Learning Objective
Be able to identify a polyatomic ion and being able to read a chemical formula containing a polyatomic ion

29. What is a polyatomic ion?
Polyatomic Ions
What is a polyatomic ion?
What happens when a bunch of atoms connect together and form a clump that has a positive or negative charge

30. List of Polyatomic Ions

31. Common Polyatomic Ions

32. Ca(NO3)2 ZnSO4 Ba(OH)2 Calcium Nitrate Zinc Sulfate Barium Hydroxide
Example
Ca(NO3)2
Calcium Nitrate
ZnSO4
Zinc Sulfate
Ba(OH)2
Barium Hydroxide

33. Practice Chemical Name Chemical Formula Calcium Carbonate
Calcium Sulfate
Barium Acetate
Barium Phosphate
Magnesium Sulfite

34. Practice Chemical Name Chemical Formula Calcium Carbonate CaCO3
Calcium Sulfate
CaSO4
Barium Acetate
Ba(C2H3O2)2
Barium Phosphate
Ba3(PO4)2 
Magnesium Sulfite
MgSO3 

35. Practice Chemical Formula Chemical Name Ca3(PO4)2 Ba(OH)2 BaSO4
Mg3(PO4)2
Ca(MnO4)2

36. Practice Chemical Formula Chemical Name Ca3(PO4)2 Calcium Phosphate
Ba(OH)2
Barium Hydroxide
BaSO4
Barium Sulfate
Mg3(PO4)2
Magnesium Phosphate 
Ca(MnO4)2
Calcium Permanganate