Molar Mass----> Mass of the Atom

• The mass in grams of 1 mole of a substance is called a “Molar Mass”
• It can be determined from the atomic mass on the periodic table.
• Measured in g/mol.
• Some common masses are:

1. Hydrogen =1.0079
2. Helium = 4.0
3. Nitrogen = 14.01
4. Zinc = 65.37
5. Iron = 55.845
6. Sodium = 22.9
7. Uranium = 238.03

1) Molar Mass

• The atomic mass----> Molar Mass
• The molar mass is the weight of one mole or 6.02 x 1023 molecules.
• The base SI Unit for mass is the Kilogram.
• To determine the molar mass of a compound, add the mass of all the atom together.
• Always have 2 or more significant digits.
• For example: Find the Molar Mass of the compound CO2 (Carbon Dioxide)

1. Atomic mass carbon = 12.01      
2. Atomic mass of oxygen = 16.00
3. Molecular Mass for Carbon monoxide = the atomic mass carbon + the atomic mass oxygen
4. 12.01 + 2(16.00) = 44.01 g/mole

2) Moles to Volume Conversion:
Mass<-(Molar Mass)->Moles<-(Molar Volume)->Volume

• Volume at STP (Standard Temperature and Pressure)
• The Volume is always the same as long as it is the same STP.
• The Volume only applies to gases.
• 1 mole of any gas occupies the same volume.
• At 0 degrees celsius and 101.3 kPa (1 mol=22.4L) 
• 22.4L/mol is the molar volume at STP

• KEY information to remember:

1 mol = 6.02 x 1023 particles
1 mol = g-formula-mass (periodic table)
1 mol = 22.4 L for a gas at STP
 Examples:
1. A certain gas is found to occupy 0.040 moles at STP. Find the volume in liters.
(0.040 mol) x(22.4 L/ 1 mol) = 0.896L

2. How many moles of Sulfur atoms are present in 11.2 L of Sulfur gas at STP?
(11.2L)x(1mol/ 22.4L) = 0.5 mol

Naming Compounds

This section will cover how to name  Ions, Binary Ions, Polyatomic ions, Molecular Compounds, Hydrates,  Bases and acids.

1) Chemical Nomenclature

• Today's most common system for chemicals is IUPAC 
• IUPAC stands for International Union of Pure and Applied Chemistry

2) Chemical Formulas

     This section will be easier if you know the differences between Ions and a compounds formulas

Ex. 

       

This is an Atom of Calcium

This is a Ion of Calcium
(Notice how the electrons from the valence shell are removed, This is why the 2+ is at the top corner)





(Cat-ions are positive)
(An-ions are negative)

3) Multivalent Ions:

• Some elements can form  more than one ion. For example:   Nickel (Ni2+) or (Ni3+)
• The top numbers on the periodic table are more common. For example (Ni2+) is more common than (Ni3+)
• IUPAC uses roman numerals in parenthesis to show the charge. For example: Nickel (II) or Nickel (III)

4) Classical

• IE (old) systems use Latin names of elements and the suffixes -ic (larger Charge) and - ous (smaller Charge)
• Some examples are:

1)Sodium ( Na) Natrium
2)Potassium (K) Kalium
3)Iron (Fe) Ferrum
4)Copper (Cu) Cuprum
5)Tungsten (W) Wolfram
6)Mercury (Hg) Hydragyrum 

7)Gold (Au) Aurum 

8)Lead (Pb) Plumbum 

9)Tin (Sn) Stannum 

10)Silver (Ag) Argentum 

11)Antimony (Sb) Stibium

5) Complex Ions

• Complex ions are larger groups of atoms that stay together during a chemical reaction
• Almost all are anions
• Write the metal name and then the polyatomic ions’ name.
• The numbers of ligands in a complex are specified using the Greek prefixes:

1. di for 2
2. tri for 3
3. tetra for 4
4. penta for 5
5. hexa for 6

Examples:

• [Cu(H2O)6]2+ is called the hexaaquacopper(II) ion.
• CuCl42-   is called tetrachlorocuprate (II) ion.


6) Hydrates

• Some compounds can form latticess that bond to water molecules.
• For example Cooper Sulphate or Sodium Sulphate.
• These crystals contain ater inside them which can be released by heating.
• “Anhydrates” is removing the water.
• So the compound is often preceded by “Anhydrates”
• To name Hydrates:

1. Write the name of chemical Formulas
2. Add a prefix indicating the number of water molecules (mono =1,di=2, tri=3)
3. Add hydrate after prefix 

7) Acids:

• Hydrogen compounds are acids
• For example: HCl (aq) = Hyrdochloric Acid
• Another example: H2SO4 (aq) = Sulphuric Acid
• Hydrogen appears first in the formula unless it is part of a polyatomic group.
• For example: CH3COOH = Acetic Acid

8) Bases:

• Corrosive ('burns' your skin)
• Has a pH more than 7
• Turns red litmus paper to a blue colour
• Many alkalis (soluble bases) contain hydroxyl ions (OH-)
• Reacts with acids to form salt and water