1. Ch. 12.1 Notes---Ionic Bonding & Ionic Compounds
Ionic Bonds
Form when ___________ transfer their _____________ electrons to a _______________.
The forces of attraction between the ____________ (+) and the _____________ (-) bind the compound together.
How to Represent an Ionic Bond
Quantum Mechanics (electron configurations):
Na 1s2 2s2 2p6 3s1
Cl 1s2 2s2 2p6 3s2 3p5
metals
valence
nonmetal
cation
anion
Na… ___ 3s ↑
Cl… ___ ___ ___ ___
3s p ↑ ↓ ↑ ↓ ↑ ↓ ↓

2. How to Represent an Ionic Bond
2) Bohr Model

3. How to Represent an Ionic Bond
3) Electron Dot Notations:
Na Cl  [ ] [ ]
Practice Problems: (1) Draw the electron dot notation for the formation of an ionic compound between sodium and oxygen.
(2) Draw the electron configuration notation for the formation of an ionic compound between magnesium and fluorine.
Na+1
Cl -1

4. Valence Electrons On The Periodic Table1 8 2 3 4 5 6 7
Sucktastic!
Assume 2

5. Charges On The Periodic Table+1 +2 +3
+/-4 -3 -2 -1
Sucktastic!

7. Sodium + Chloride

8. S [ S -2] K [K+1] Practice Problems:
3) a) Draw the electron dot notation for a potassium atom.
b) Draw the electron dot notation for a potassium ion.
(4) a) Draw the electron dot notation for a sulfur atom.
b) Draw the electron dot notation for a sulfur ion. K
[K+1] S
[ S -2]

9. Properties of Ionic Compounds and Covalent Molecules
_______________ of electricity when dissolved water or melted.
formed between __________ and _________________
have _________ melting points
usually ________ soluble in water
form ___________________ solids
Conductors
metals
nonmetals
high
(dissolved salt)
very
crystalline

10. Crystalline Patterns

11. Quartz
Quartz is the common mineral form of silicon dioxide (SiO2). It is the dominant mineral in most sands and sandstones.

13. Pyrite
mineral form of the iron disulfide (FeS2) with a gold-like appearance, making it also known as "fool's gold"

14. Gypsum
Gypsum is a very soft mineral composed of calcium sulfate dihydrate, with the chemical formula CaSO4·2H2O.

16. Properties of Ionic Compounds and Covalent Molecules
Molecular:
________________ of electricity always
formed between two _______________
usually have ________ melting points
solubility in water _______: (polar =dissolve; nonpolar = insoluble)
For a compound to to conduct electricity it must have:
(1) Charged Particles (_________)
(2) Particles Free to Move (___________ or __________ phase)
Insulators
nonmetals
low
varies
ions
liquid
aqueous

17. Demonstration PureH2O great conductor good conductor poor conductor
nonconductor

18. Ch. 6 Notes---Chemical Names & Formulas
Ionic Compounds (“________”):
Name or formula starts with a _________ (or NH4 +, ammonium).
Other quick ways to tell if the compound is ionic:
formula uses parentheses
Example: ________________
formula contains more than 2 elements (capital letters)‏
name uses Roman numerals
name ends in “-ate” or “ite”.
Example: _________________
salts
metal
Ca(OH)2
FeCrO4
lead(II) chloride
barium sulfate

19. Writing Formulas for Ionic Compounds
Step 1-- use your ion sheet and find the ions and their charges.
Step 2-- “Cross the charges” if they don’t balance out.
Step 3-- Use parentheses around polyatomic ion “chunks”.
Practice Problems: Write the formula for each ionic compound.
copper(II) bromide ____________________
aluminum nitrite _________________________
barium hydrogen carbonate ___________________________
Cu+2
Br -1
CuBr2
…(don’t show 1’s)‏ =
Al+3
NO2 -1
Al(NO2)3 =
Ba+2
HCO3-1
Ba(HCO3)2 =

20. Naming Ionic Compounds
Just use your ion sheet and find the names of the ions.
cation name anion name
Practice Problems: Name the following ionic compounds.
NaC2H3O b) (NH4)2CO c) NaCl d) CaO
ammonium carbonate
sodium chloride
calcium oxide
sodium acetate