Ionic Compounds
- Composed of 2 or more particles (ions) that are oppositely charged
- Held together by electrostatic forces
- Electrons are transferred from a metal → non-metal
Ex. Na+ + Cl-
= NaCl Sodium Chloride
Li+ + N3-
Lithium Nitrogen charges
↓ ↓
3 ( + 1 ) + 1 ( - 3 ) = 0
↑ ↑
Balanced to equal zero
= Li3N Lithium Nitride
- If an ion has more than one charge, we use Roman Numerals to express that charge in writing
I | - +/- 1 | V | - +/- 5 |
II | - +/- 2 | VI | - +/- 6 |
III | - +/- 3 | VII | - +/- 7 |
IV | - +/- 4 | VIII | - +/- 8 |
Ex. Palladium has either a +2 or a +4 charge
If: Pd2+ + F-
= PdF2 Palladium (II) Fluoride
If: Pd4+ + P3-
= Pd3P4 Palladium (IV) Phosphide
- Complex ions are a group of atoms that behave as one atom
Ex. Na2SO4 Sodium Sulphate
Cu(NO2)2 Copper (II) Nitrite
Covalent compounds
- Shares electrons
- Non-metal with non-metal
- Uses Greek prefixes
Mono* | - 1 | Hexa | - 6 |
Di | - 2 | Hepta | - 7 |
Tri | - 3 | Octa | - 8 |
Tetra | - 4 | Nona | - 9 |
penta | - 5 | Deca | - 10 |
*if there’s only one in the first ion, then you don’t have to write Mono
Ex. CO2 Carbon Dioxide
S3B2 Trisulphur Diboride
CCl4 Carbon Tetrachloride
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| Diatomic Compounds on the Periodic Table |
o There are 7 diatomic molecules, which are 2 atoms of the same element
o They make a “7” shape on the Periodic Table, with the exception of Hydrogen
H2 | Hydrogen |
Br2 | Bromine |
I2 | Iodine |
O2 | Oxygen |
N2 | Nitrogen |
F2 | Fluorine |
Cl2 | Chlorine |
An easy way of remembering the 7 diatomic molecules is by remembering this name:
Fun Fact of the Day
DID YOU KNOW... if an octopus is hungry enough, it will eat its own arms??
By: Jason Zhang
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