1. BELL RINGER: Write the charges for the following elements/polyatomic ionsMg Li P K Ba I Cl O S
Nitrate
Sulfate
Acetate
Chromate
Carbonate
Cyanide

2. Ionic compounds

3. What is a bond?
A ______________________________between the nuclei and valence electrons of different atoms that ________ them together.
Can be formed by atoms _______, ________, or ___________ electrons.
Why do atoms form chemical bonds?
To become more stable (___________ potential energy)
ONLY ___________ electrons are used for bonding.

4. Ionic bonds
Atoms lose or gain electrons to satisfy ____________ (become more stable)
Form two kinds of ______—atom that has an electrical charge.
Cations—____________ charged atoms.
Anions—_____________ charged atoms

5. Periodic trends associated with ionic bonding
___________________—energy required to remove an electron from the outer shell of an atom.
___________________—the change in energy when an electron is added to the outer shell.
For bonding—High IE, high EA = less likely to give electrons = _________
Low IE, low EA = more likely to give electrons = _________
Need more convincing?
Draw orbital diagram for F.

6. Formation of Cations Atoms that __________ electrons:
Low IE—does not require a ton of energy to take an e- away
Low EA-does not readily accept other e- into outer shell.
Examples: ___________
Li, Na, K, Be, Mg, Ca, etc
Draw orbital diagrams for the following: Li

7. Transition Metals
Form __________ with different oxidation states (depends on what it’s bound to)
Titanium: [Ar]4s23d2
Can lose two electrons for Ti2+ or four electrons for Ti4+
Sometimes they will rearrange to have a pseudo-noble gas configuration (full outer shell, but not really)
Copper usually has its electrons fully rearrange to form [Cu]4s13d10 instead of [Cu]4s23d9

8. Formation of Anions Atoms that _________ electrons:
High IE—requires a ton of energy to take an e- away
High EA-readily accepts other e- into outer shell.
Examples: ___________ and ____________
F, N, O, Cl, etc.
Draw orbital diagrams of the valence shells of the following: S

9. EXIT SLIP - Write the oxidation states for the following elementsB Br N Be Na F Al Se As

10. Ionic Bonds Held together by ______________________
Electrostatic force—force of ___________ between positively and negatively charged particles

11. Crystal lattice What is it?
a __________________ geometric arrangement of particles where + and – ions surround each other
the ions are packed into a regular _____________ pattern that balances the forces of attraction and repulsion between the atoms

12. Crystal lattice Na Cl
- In a solid state, ionic compounds are non-conductors,
ions must be free to move for a current to pass
through it
- In a liquid state (molten) or when dissolved in water
they are good conductors (ions are free to move)

13. Lattice energy
The energy released when 1 mol of an ionic compound is formed from gaseous ions.
_______________—energy has to be absorbed for the reaction to happen
Surroundings are colder
_______________—energy is released (Ex: -436 kJ/mol)
Surroundings feel warmer since energy is given off
Which is more stable?

14. Formation of ionic compounds is almost ALWAYS ____________ Why
Formation of ionic compounds is almost ALWAYS ____________ Why??? More stable with lower potential energy

15. Formulas
__________________-represents the most simple ratio of the ions in an ionic compound
The total number of e-‘s gained by the nonmetal must equal the number lost by the metal atoms
__________________—give insight into how the atom will bond
Used to determine the formula for a compound

16. Nomenclature What is it?? Rules for ionic nomenclature
The naming and writing of formulas for chemical compounds.
Rules for ionic nomenclature
1.) Cation is ALWAYS written first.
2.) Anion is ALWAYS written second.
3.) Use subscripts to cancel out charges

17. Nomenclature Naming Cation ALWAYS goes first.
If transition metal—write roman numeral to specify oxidation state
Anion ALWAYS goes second.
Monoatomic—drop suffix and add –ide
Polyatomic—use name of polyatomic ion

18. Bellringer (nomenclature quiz TOMORROW)
Elements Bonding
Chemical Formula
Chemical Name
Mg + NO3
Al + Br
Ag2+ + CrO4
C2H3O2 + Ca
F + NH4
Be + IO3
PO4 + NH4

19. Hydrides
________________ can gain or lose one e- depending on what it binds with…
WHY?
When bonding with metals, H gains an e-
Since it is an anion, it gets the “-ide” suffix
Examples: LiH, MgH2, NaH, etc.

20. Hydrates Contain ____________in crystalline lattice
Can remove water without chemically altering substance
Nomenclature is the same as ionic compounds, except take water molecules into account.
How? Use prefixes to show number of water molecules

21. Nomenclature for Hydrates
Examples: CuSO4· 5H2O
1.) Use name of compound:
2.) Name hydrate with correct prefix:
Mono = 1
Hexa = 6
Di = 2
Hepta = 7
Tri = 3
Octa = 8
Tetra = 4
Nona = 9
Penta = 5
Deca = 10

22. Practice
Name the following compounds:
NaCl∙2H2O
MgSO4∙7H2O
Al2(SO4)3∙9H2O
CoCl2∙5H2O
NiCl4∙3H2O

23. Practice Write the names for the following compounds:
Iron (II) fluoride tetrahydrate
Barium hydroxide octahydrate
Lead (II) perchlorate pentahydrate
Copper (II) acetate monohydrate
Tin (II) chloride dihydrate