1. 4.2 Names and Formulas of Compounds
Ionic ________________________are made up of _______________ and _____________ ions.
All of the positive and negative ions organize in a _________________.
Negative-positive _______________.
Negative-negative and positive-positive _________.
Ionic compounds form from the inside out as ___________________________.
A salt shaker contains thousands of small pieces of NaCl (each tiny grain of salt you see is made of many Na and Cl ions, NOT just one of each)
Salt, NaCl
See pages
Water, H2O
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2. Names and Formulas of Compounds
Covalent _____________________share electrons.
There is generally no order to the formation of covalent molecules.
These molecules ____________________________as solids, liquids or gases.
Covalent molecules are like a play-pit full of plastic balls.
Each plastic ball = 1 _______________________of H2O
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3. The Chemical Name and Formula of an Ionic Compound
The _______________ of an ionic compound = positive ion + negative ion-ide.
We can write the name if we know the two elements involved:
For example, an ________________________________forms between magnesium and oxygen.
The_____________________is the first part of the name, ______________________.
The __________________________forms part
of the ending of the name, __________________.
Add -ide to the end of the name to form
_________________________________.
Magnesium oxide is used as a drying agent.
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4. The Chemical Name and Formula of an Ionic Compound
We can also make a name from an ________________________________________
For example, what is the name of Ca3N2?
Ca, the __________________ ion, is ___________________.
N, the __________________ ion, is ____________________.
Drop the end of the anion and add ____________
____________________________
See pages
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5. Naming Ionic Compound Examples
Name the following:
1. NaBr
2. MgS
3. AlF3
4. Fe2O3
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6. The Chemical Name and Formula of an Ionic Compound (continued)
Writing ___________________ for ionic compounds:
In an ionic compound, the ____________________charges balance out the ______________________ charges.
To do this, we need to criss-cross the charges (see below)
The ratio is always written in the lowest possible form.
For example, what is the formula for magnesium phosphide?
Calcium oxide, also known as “quicklime” was once produced by cooking limestone in ancient kilns.
magnesium is ________ phosphorous is __________
Criss-cross to get:
See page 188
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7. Ionic Formula Examples
Write the formulas for the following compounds:
1. Magnesium Phosphide
2. Calcium Bromide
3. Aluminum Oxide
4. Lithium Nitride
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8. Formula of an Ionic Compound with a Multivalent Metal
Some transitional metals are _____________________meaning they have ___________________________ion form.
On the periodic table, the most common form of the ion is listed __________
In the name of the compound, ___________________________are used following the positive ion to indicate ________________________was used.
For example, what is the formula manganese (III) sulphide?
This manganese is ___________, sulfur is _________
____________________
For example, what is the name of TiF4
titanium is ____________ Roman numeral: __________
____________________________
See pages
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9. Polyatomic Ions
Some ions, called _________________________, are made up of ____________________joined together with covalent bonds.
The __________________________has a + or – charge, not the individual atoms.
When naming these compounds, DO NOT change the ending of the polyatomic ion!
See pages
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10. Polyatomic Examples Write the formula for the following:
1. Sodium sulphate
2. Potassium permanganate
Write the name for the following:
1. KClO
2. Fe(OH)3
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11. Names and Formulas of Covalent Compounds
Covalent compounds are also called__________________.
Covalent compounds are made up of two or more ____________.
Subscripts mean something different in covalent compounds
Ionic compounds subscripts show the smallest whole-number _________________between the ions in the compound.
Covalent molecules have subscripts that show the _____________________________ of atoms in the molecule.
See page 193
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12. Naming Covalent Compounds
Covalent compounds (two non-metal atoms) use a system of _____________ for naming.
Prefixes (mono, di, tri, etc) are often used
_________________ the atom name to indicate the
number of atoms in the molecule.
You must always use prefixes EXCEPT for the
first atom when there is only one of them, then you
may leave out the ‘mono’
CO2 = carbon dioxide, not monocarbon dioxide
Write the most ___________________ atom (farthest left) first
Add -ide to the end of the second atom’s name
See pages
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13. Covalent Compounds Examples
Write names for the following compounds: 1. Si3P6 2. N2O4 3. NI3
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14. Covalent Compound Examples
Write formulas for the following compounds:
1. Trinitrogen tetrachloride
Dichlorine monoxide
Carbon tetraiodide
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15. Comparing Ionic and Covalent Compounds
To determine whether a compound is ionic or covalent:
Examine the formula.
Ionic compounds start with a metal or the ammonium ion.
Covalent compounds start with a non-metal.
If the compound is covalent:
Use the prefix system of naming if the compound does not start with hydrogen. (If it does, then it is an acid. We will learn about those soon.)
If the compound is ionic:
Check the metal to see if it is multivalent (add a Roman numeral if it is multivalent). Naming starts with the name of the metal atom.
If it ends with a single non-metal, naming will just end in -ide.
If it ends in a polyatomic ion, look up the name/formula in the chart
See pages
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