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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
(1) Quantum Mechanics (electron configurations):
Na 1s2 2s2 2p6 3s1
Cl 1s2 2s2 2p6 3s2 3p5
metals valencenonmetal
cationanion
Na… ___ 3s
↑
Cl… ___ ___ ___ ___ 3s 3p
↓↑ ↑ ↑↓ ↓ ↓
How to Represent an Ionic Bond
2) Bohr Model
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
Valence Electrons On The Periodic Table
12 3 4 5 6 7
8
Sucktastic!Assume 2
Charges On The Periodic Table
+1+2 +3 +/-4 -3 -2 -1
0
Sucktastic!
Sodium + Chloride
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]
Properties of Ionic Compounds and Covalent Molecules
Ionic:
•_______________ of electricity when dissolved water or melted.
•formed between __________ and _________________
•have _________ melting points
•usually ________ soluble in water
• form ___________________ solids
Conductors
metals nonmetals
high
very
crystalline
(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"
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
• 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
Demonstration
good conductor
poor conductor
nonconductor
PureH2O
great conductor
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)
Example: ________________
• name uses Roman numerals
Example: ________________
• name ends in “-ate” or “ite”.
Example: _________________
salts
metal
Ca(OH)2
FeCrO4
lead(II) chloride
barium sulfate
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
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 b) (NH4)2CO3 c) NaCl d) CaO
sodium acetateammonium carbonate
sodium chloride
calcium oxide