Photo by Ra’ike

Remember…

Rules for Naming Ions

Examples of naming ions:

sulfidenitride

potassium

oxide

lithiumbromide

chloridehydrogen (+), hydride (-)

sulfate

permanganate

hydroxide

carbonatesulfite

nitrate

CaBr2

Step 1: Write the name of the metal ion.Step 2: Write the name of the nonmetal ion.

calcium bromide

1. NaFsodium fluoride

2. MgOmagnesium oxide

3. SrCl2strontium chloride

4. Li2Slithium sulfide

5. CaOcalcium oxide

6. KIpotassium iodide

1. NH4Fammonium fluoride

2. CaSO4calcium sulfate

3. Mg(NO3)2magnesium nitrate

4. NaOHsodium hydroxide

When polyatomic ions are used, simply use the name of the polyatomic ion in the compound.

You can also determine the formula of an ionic compound from its name. To do this, you will need to use what you already know about the Periodic Table.

magnesium iodide

Step 1: Write the symbol and charge of the metal ion using the Periodic Table.Step 2: Write the symbol and charge of the nonmetal ion using the Periodic Table.Step 3: Determine the formula from the ions.

Mg I+2 -

MgI2

This is just as easy to do with polyatomic ions. You just need to use the table of polyatomic ions found on the naming compounds reference sheet.

strontium nitrate

Step 1: Write the symbol and charge of the metal ion.Step 2: Write the formula and charge of the polyatomic ion using your STAAR Reference Sheet.

Step 4: Determine the formula from the ions.

Sr NO3+2 -

Sr(NO3)2

Be very careful that you do not mix up the names of ions. This is very common for beginners to naming.

Helpful Hint: If the ion ends in –ide, it is probably from the periodic table. If the ion ends in –ate or –ite, it is a polyatomic ion. If you’re not sure, just check the list to see if it is there!

Remember that the names of transition metals includes their charge because their charges are less predictable.

What are the charges of the transition metals below:

We know they are positive because metals are always positive.

The charges of the transition metals are important when you are determining the formula of an ionic compound.

iron (III) oxide

Step 1: Write the symbol and charge of the metal ion using the ROMAN NUMERAL given.Step 2: Write the symbol and charge of the anion.Step 4: Determine the formula from the ions.

Fe O+3 -2

Fe2O3

KISnCl4

BaSO4

NaClSrSCuCO3

AlBr3

Li3N

So why do atoms share electrons?Atoms share electrons so that they can both

be in the most stable configuration!

So when are atoms the most stable?Atoms are the most stable when they have 8 valence electrons in their outer energy level.

(Hydrogen and Helium only need 2 valence electrons.)

Chemical reactions occur when atoms gain, lose, or share electrons.

Sharing electrons creates a covalent bondNonmetals can _______ electrons to

form a covalent bond.This creates a ___________.

share

molecule

Nonmetals

There are 7 elements that exist in nature as diatomic molecules.

What elements exist as diatomic molecules?

H2, N2, O2, F2, Cl2, Br2, I2

There are millions of covalent compounds. These can be classified into many different types of compounds. Each type of compound has a different set of rules for naming. You will be learning about the easiest type of covalent compound to name:

Nonmetals can share electrons in many different ways. This means that two nonmetals can create multiple compounds together.

Each of these contains a different ratio of elements. Because of this, we have to make sure that the name of the compound explains the correct ratio.

To show the correct ratio of elements, we use prefixes.

Steps for Naming Binary Covalent Compounds

N2O4

Step 1: Write the name of the first nonmetal.Step 2: Write the name of the second nonmetal changing its ending to -ide.

Step 3: Add prefixes to specify how many of each element are present.

nitrogen oxidedinitrogen tetroxide

Rules for Using PrefixesRule 1: Prefixes are only for COVALENT compounds.Rule 2: The prefix mono- is never used on the first element of a binary covalent compound. Without a prefix it is assumed that there is only 1.

Rule 3: Remove the -o or -a from a prefix before adding it to oxide.

Example: CO2 is carbon dioxide, not monocarbon dioxide.

Example: CO is carbon monoxide, and not carbon monooxide.

How would you write each of the prefixes in front of oxide?

mono- ____________ di- ____________tri- ____________ tetra- ____________penta- ____________ hexa- ____________hepta- ____________ octa- ____________nona- ____________ deca- ____________

monoxide dioxidetrioxide tetroxide

pentoxide hexoxideheptoxide octoxidenonoxide decoxide

Remember: Remove the -o or -a from a prefix before adding it to oxide. Leave -i alone.

Name the binary covalent compounds that are found on your notes.

carbon dioxidecarbon disulfidephosphorous tribromidephosphorous pentabromidediphosphorous pentasulfidedinitrogen monosulfidesilicon disulfidenitrogen tribromidedinitrogen tetrachloride

Because of the prefixes, it is very easy to go from the name of a binary

covalent compound to its formula.dinitrogen tetrafluoride

Step 1: Write the symbol of the first nonmetal and the subscript that matches the prefix.Step 2: Write the symbol of the second nonmetal and the subscript that matches the prefix.

N2 F4

Write the formulas of the binary covalent compounds in your notes.

CCl4PCl5N2O

CSBH3S2Br6SiS2 PI3

NCl3

IF7N2O4

PCl3COICl

S4N4H2OClF5

NO2