Ch. 12.1 Notes---Ionic Bonding & Ionic Compounds
Ionic Bonds
•
•
metals transfer their _____________
valence
Form when ___________
electrons
to a _______________.
nonmetal
cation
The forces of attraction between the ____________
(+) and the
_____________
anion
(-) bind the compound together.
How to Represent an Ionic Bond
(1) Quantum Mechanics (electron configurations):
Na 1s2 2s2 2p6 3s1
Na… ___
↑
3s
Cl 1s2 2s2 2p6 3s2 3p5
↑ ↓ ___
↑ ↓ ___
Cl… ___
↑ ↓ ___
↓
3s
3p
How to Represent an Ionic Bond
2) Bohr Model
How to Represent an Ionic Bond
3) Electron Dot Notations:
Na +
Cl
 [ Na+1] [ Cl -1]
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.
Sodium + Chloride
Practice Problems:
3)
a) Draw the electron dot notation for a potassium atom.
K
b) Draw the electron dot notation for a potassium ion.
[K+1]
(4)
a) Draw the electron dot notation for a sulfur atom.
S
b) Draw the electron dot notation for a sulfur ion.
[S
-2]
Properties of Ionic Compounds and Covalent Molecules
Ionic:
•
•
•
•
•
Conductors
_______________
of electricity when dissolved water or melted.
formed between __________
metals and _________________
nonmetals
high melting points
have _________
usually ________
very soluble in water
crystalline
form ___________________
solids
(dissolved salt)
Crystalline Patterns
Quartz
• Quartz is the common mineral form of
silicon dioxide (SiO2). It is the dominant
mineral in most sands and sandstones.
Pyrite
• mineral form of the iron disulfide (FeS2)
with a gold-like appearance, making it
also known as "fool's gold"
Calcite
• Calcite is a carbonate mineral and the most
stable polymorph of calcium carbonate
(CaCO3). The shape is Rhombohedron.
Galena
• Galena is the natural mineral form of
lead sulfide. (PbS) It is the most
important lead ore mineral.
Gypsum
• Gypsum is a very soft mineral
composed of calcium sulfate dihydrate,
with the chemical formula
CaSO4·2H2O.
Properties of Ionic Compounds and Covalent Molecules
Molecular:
• ________________
of electricity always
Insulators
nonmetals
• formed between two _______________
low melting points
• usually have ________
• solubility in water _______:
(polar =dissolve; nonpolar = insoluble)
varies
For a compound to to conduct electricity it must have:
ions
(1) Charged Particles (_________)
liquid
aqueous phase)
(2) Particles Free to Move (___________
or __________
Demonstration
great
conductor
poor
conductor
good
conductor
Pure
H2O
nonconductor
Ch. 6 Notes---Chemical Names & Formulas
•
Ionic Compounds (“________”):
salts
metal
– Name or formula starts with a _________
(or NH4 +,
ammonium).
– Other quick ways to tell if the compound is ionic:
• formula uses parentheses
Ca(OH)2
Example: ________________
• formula contains more than 2 elements (capital letters)
FeCrO4
Example: ________________
• name uses Roman numerals
lead(II) chloride
Example: ________________
• name ends in “-ate” or “ite”.
barium sulfate
Example: _________________
1
Valence Electrons On The Periodic
Table
2
3 4 5 6 7
Sucktastic!
Assume 2
8
Charges On The Periodic Table
+1
+2
0
+3 +/-4 -3 -2 -1
Sucktastic!
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
+2 Br -1 CuBr …(don’t show 1’s)
Cu
=
2
____________________
aluminum nitrite
+3 NO -1
Al
= Al(NO2)3
2
_________________________
Ba+2 HCO3-1 = Ba(HCO3)2
barium hydrogen carbonate ___________________________
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.
a)
NaC2H3O2
sodium acetate
b) (NH4)2CO3
ammonium
carbonate
c) NaCl
sodium
chloride
d) CaO
calcium
oxide