1. Ionic Bonding and Ionic Compounds
Chapter 6 and 15
Ionic Bonding and Ionic Compounds

2. Ionic vs. Molecular What is a molecule?
A molecule is the smallest electrically neutral unit of a substance that still has the properties of that substance. Molecules are made up of 2 or more atoms that act as a unit.

3. Ionic vs Molecular:
Can we describe the smallest electrically neutral unit of an ionic compound as a molecule?
Can we describe NaCl as a molecule?

4. Chemical Bonds Revisited:
An electrostatic force of attraction between two atoms, ions, or molecules

5. Why do Atoms Bond?
Octet Rule: Atoms will lose, gain, or share electrons to achieve a stable octet. Stable Octet: 8 valence electrons or a noble gas configuration.

6. Chemical Bonding
Atoms within the same group of the periodic table have the same number of valence electrons.
Valence electrons determine the chemical properties of an element

7. Valence electrons revisited:
Valence electrons are usually the only electrons used in chemical bonds.

8. Valence electrons
How do you determine the number of valence electrons?
The group number
The electron configuration diagram

9. Ions: Particles that have either gained or lose electrons.
Metals lose electrons to make positive ions
Nonmetals gain electrons to make negative ions.

10. Ionic Compounds (Formula Unit)
Ionic compounds do not exist as molecules
Ionic compounds exist as a collection of positively and negatively charged ions arranged in repeating 3-D patterns

11. Ionic Bonds
Ionic Bonds: Bonds formed between positive and negative ions (metals and nonmetals)

12. Properties of ionic compounds
Crystalline Solids

13. Properties of ionic compounds
Electrolytes: Conduct electricity when dissolved in water
Conduct electricity in the liquid state but not the solid state
High Melting points and Boiling points

14. Shows the numbers and types of atoms present in a chemical compound.
Chemical Formula
Shows the numbers and types of atoms present in a chemical compound.

15. Formula Unit: Used to represent an Ionic compound (no molecules)
Lowest whole number ratio of ions in an ionic compound
Examples: MgCl2, KBr, AlF3

16. Monatomic Ions: Ions consisting of one atom Monatomic cations
Sodium( Na+), lithium (Li+), Calcium (Ca2+),
Aluminum (Al 3+)
Monatomic anions
Fluoride (F-), Oxide (O2-), Phosphide (P3-)

17. Ionic Charges: Stock system:
For naming cations with more than one possible charge
Example: Iron
Has two possibilities (II), (III)
Written as Iron(II) ion (Fe2+) and Iron(III) ion (Fe3+)

18. Ionic Charges:
Can also use the root word with a different suffix to designate between multiple charged cations:
Example:
Iron(II): ferrous (Fe2+)
Iron(III): ferric (Fe3+)

19. Ionic Charges Polyatomic ions: More than one atom Tightly bound groups
Behave as one unit

20. Ionic Charges: Polyatomic ions: Most end in –ite, or –ate Exceptions:
Ammonium (NH4+)
Hydroxide (OH-)
Cyanide (CN-)

21. Ionic Charges: Polyatomic ions with hydrogen: Example: HCO3-
Note: the charge of the new ion is the sum of the charges of the composite ions

22. Common Polyatomic Ions
1- charge
2- charge
3- charge
Formula
Name
H2PO4-
Dihydrogen phosphate
HPO42-
Hydrogen phosphate
PO33-
Phosphite
C2H3O2-
Acetate
C2O42-
Oxalate
PO43-
Phosphate
HSO3-
Hydrogen sulfite
SO32-
Sulfite
HSO4-
Hydrogen sulfate
SO42-
Sulfate
HCO3-
Hydrogen carbonate
CO32-
Carbonate
1+ charge
NO2-
Nitrite
Cr2O42-
Chromate
NO3-
Nitrate
Cr2O72-
Dichromate
NH4+
Ammonium
CN-
Cyanide
SiO32-
Silicate
OH-
Hydroxide
MnO4-
Permanganate
ClO-
Hypochlorite
ClO2-
Chlorite
ClO3-
Chlorate
ClO4-
Perchlorate 22

23. Nick the Camel ATE a Clam for Supper in Phoenix
Trick for remembering –ate ions…
Nick the Camel ATE a Clam for Supper in Phoenix
Underlined letter represents the symbol of the element
The #of consonants = the # of oxygen atoms
The # vowels = charge
EX: Nick = nitrogen
N = nitrogen
3 consonants = 3 oxygens
1 vowel = -1 charge
Nitrate = NO3-

24. Nick the Camel ATE a Clam for Supper in Phoenix
Trick for remembering –ate ions…
Nick the Camel ATE a Clam for Supper in Phoenix
EX: Camel
C = carbon
3 consonants = 3 oxygens
2 vowel = -2 charge
carbonate = CO3-2

25. Nick the Camel ATE a Clam for Supper in Phoenix
Trick for remembering –ate ions…
Nick the Camel ATE a Clam for Supper in Phoenix
EX: Clam
Cl = chlorine
3 consonants = 3 oxygens
1 vowel = -1 charge
chlorate = ClO3-1

26. Nick the Camel ATE a Clam for Supper in Phoenix
Trick for remembering –ate ions…
Nick the Camel ATE a Clam for Supper in Phoenix
EX: Supper
S = sulfur
4 consonants = 4 oxygens
2 vowel = -2 charge
sulfate = SO4-2

27. Nick the Camel ATE a Clam for Supper in Phoenix
Trick for remembering –ate ions…
Nick the Camel ATE a Clam for Supper in Phoenix
EX: Phoenix
P = phosphate
4 consonants = 4 oxygens
3 vowel = -3 charge
phosphate = PO4-3

28. Binary Ionic Compounds:
Compounds that are composed of two elements
Electrically neutral (net charge of zero
Ionic Binary compounds are composed of a
1. Cation (+) always written first
2. Anion (-) always written last
Examples:
KCl
NaCl
CaBr2

29. Bionary Ionic Compounds
Writing a balanced formula- Criss Cross Method
Must first find identify charges of ions
Find least common multiple
Example: write the formula for
Iron (III) Oxide
Calcium Sulfide
Alumimum Chloride

30. Naming Binary Ionic Compounds
1. write the name of the metallic cation ion.
Use the stock naming system
2. then write the name of the non-metallic anion.
Examples:
CuO
MgCl2
SnO2

31. Ternary Ionic Compounds
A compound that contains atoms of three different elements
Involves polyatomic ions – usually polyatomic anions
Writing the formula for ternary compounds is the same as binary compounds (criss cross method)
Naming ternary ionic compounds- see Nick the Camel etc…

32. Acids:
Acids are a special group of compounds that release hydrogen ion in solution
When naming, can consider them as ionic compounds (cations and anions)
Hydrogen = cation
Monatomic or polyatomic anion

33. Naming Acids If the anion = monatomic- Start with –hydro (prefix)
drop –ide and add –ic. (root word)
Example: HCl
H = hydro
Cl = chloride  chloric
HCl = hydrochloric acid

34. Naming Acids If the anion = polyatomic- No -hydro
If –ate, drop –ate and add –ic. (root word)
If – ite, drop –ite and add – ous (root word)

35. Naming Acids Example: H2SO4 SO4 = sulfate- drop –ate and add –ic
Add – acid
Sulfuric Acid
Example: H2SO3
SO3 = Sulfite – drop –ite and add –ous
Add – acid
Sulfurous Acid

36. Chapter 15
Electron Configuration in Ionic Bonding

37. Electron Configuration in Ionic Bonding: Cations
Cations(metals) will lose electrons to fulfill their octet.
Examples:
Sodium
Potassium
Calcium
Aluminum

38. Electron Configuration in Ionic Bonding: Anions
Anions or non-metals will accept electrons to fulfill their octet.
Fluorine
Oxygen
Nitrogen
Bromide

39. Formation of Ionic Compounds:
Electrostatic forces of attraction
Attraction of opposite charges
Electrically neutral
Total positives = total negatives
Combine in whole number ratios to satisfy the octet
Examples:
NaCl
Al2O3
MgCl2

40. Coordination Number:
Number of ions of opposite charge that surround the ion in a crystal
Ionic compounds have a crystalline structure
3-D arrangement of alternating positively and negatively charged particles
Example: NaCl
Coordination number of Na = 6
Coordination number of Cl = 6