SKILLS Project

SKILLS Project

Naming and Building Ionics (I)

What are ionic compounds?

• Remember, this unit only applies to the naming and construction of ionic compounds.

• Ionic compounds are almost always made of a METAL and a NON-METAL.

• Remember, you can determine whether something is a metal or non-metal based on their position on the periodic table.

Naming Ionic Compounds

• Ionic nomenclature is fairly simple and follows the following steps:– The positive ion or ions are always named first

(typically a metal or metals.)– The anion is named second, but drops its suffix

and typically ends in –ide. – Polyatomics (larger ions with specific names)

do not undergo a change to their names when used in compounds.• Refer to the next slide for a complete list of

useful polyatomics and associated charges.

Polyatomic Ions

• NO31- - Nitrate

• NO21- - Nitrite

• SO42- - Sulfate

• SO32- - Sulfite

• PO43- - Phosphate

• PO33- - Phosphite

• OH1- - Hydroxide• CO3

2- - Carbonate

• NH41+ - Ammonium

• C2H3O21- - Acetate

• CN1- - Cyanide• MnO4

1- - Permanganate

• ClO41- - Perchlorate

• ClO31- - Chlorate

• ClO21- - Chlorite

• C2O42- - Oxalate

• IO31- - Iodate

• BrO31- - Bromate

• CrO42- - Chromate

• Cr2O7-2 - Dichromate

• O22- - Peroxide

• N31- - Azide

• AsO43- - Arsenate

• S2O32- - Thiosulfate

Sulfur

Example 1: Li2S

Lithium

Name the metal or positive ion first. These are usually at the beginning of the compound as well.

Sulfide

Name the non-metal or anion second. Typically, this will be at the end of the compound.

Replace the last syllable of the anion with –ide. Remember, we don’t do this for polyatomic ions.

OxideOxygen

Example 2: MgO

Magnesium




PhosphorousPhosphide

Example 3: Na3P

Sodium




CarbonCarbide

Example 4: Ca2C

Calcium




NitrogenNitride

Example 5: Ba3N2

Barium




SulfurSulfide

Example 6: (NH4)2S

Ammonium




Note: Even though this compound is made up only of non-metals, the bond between the ammonium and sulfur is actually ionic due to the charges.

Carbonate

Example 7: MgCO3

Magnesium



We don’t need to replace the ending of the polyatomic “carbonate” with –ide. Remember, we don’t need to change polyatomics when writing ionic names.

Hint: the challenge with working with polyatomics is recognizing them. As a rule, look for polyatomics when a compound contains 3 or more different elements.

Acetate

Example 8: NH4C2H3O2

Ammonium



We don’t need to replace the ending of the polyatomic “acetate” with –ide. Remember, we don’t need to change polyatomics when writing ionic names.

Dichromate

Example 9: K2Cr2O7

Potassium



We don’t need to replace the ending of the polyatomic “dichromate” with –ide. Remember, we don’t need to change polyatomics when writing ionic names.

Perchlorate

Example 10: CsClO4

Cesium



We don’t need to replace the ending of the polyatomic “perchlorate” with –ide. Remember, we don’t need to change polyatomics when writing ionic names.

Practice on Your Own:

1. Na3PO4 -

2. BaCl2 -

3. NaI -

4. LiIO3 -

5. Sr(NO3)2 -

6. NaH -

7. (NH4)2Se -

8. MgSO4 -

9. CsCN -

10.H3AsO4 -

Sodium phosphateBarium chloride

Sodium iodide

Lithium iodate

Strontium nitrate

Sodium hydrideAmmonium selenide

Magnesium sulfate

Cesium cyanide

Hydrogen arsenate

Building Ionic Compounds

• To build your compound, you will need to do five things:– Place the metal or positive ion in front of the

non-metal or negative ion.– Use the periodic table or a chart to find the

charges of each element. Ionics are made of “ions” or charged particles.

– Swap the charges and drop them below the elements or ions they represent.

– Remove the plus and minus signs- these numbers are no longer being used as charges.

– Simplify, if needed.

Ex. 11: Oxygen and Magnesium

MgO

1. Place the metal or positive ion in front of the non-metal or negative ion.

2. Use the periodic table or a chart to find the charges of each element. Ionics are made of “ions” or charged particles.

3. Swap the charges and drop them below the elements or ions they represent.

4. Remove the plus and minus signs- these numbers are no longer being used as charges.

5. Simplify, if needed.

OMg2+ 2-

2 2Both subscripts may be divided by 2 to simplify.

1 1Note: We never write “1” as a subscript. The presence of the symbol indicates that at least one is present already.

MgO Done! You’ve just built magnesium oxide.

Note: We never write “1” as a subscript. The presence of the symbol indicates that at least one is present already.

NaNa3P

Ex. 12: Sodium and Phosphorous

PNa






P1+ 3-

3 1The subscripts cannot be simplified any further (divided by a common number).

Done! You’ve just built sodium phosphide.

Fe2S3S

Ex. 13: Iron (III) and Sulfur

SFe






Fe3+ 2-

2 3Neither subscript may be divided by a common factor.Done! You’ve just built Iron (III) sulfide


FBaF2

Ex. 14: Barium and Fluorine

FBa






Ba2+ 1-

1 2Neither subscript may be simplified any further.Done! You’ve just built barium fluoride.

4


2VVSe2

Ex. 15: Vandium (IV) and Selenium

SeV






Se4+ 2-

2

Both subscripts may be divided by 2 to simplify.

1

Done! You’ve just built vanadium (IV) selenide.


1. Iridium (III) Iodide –

2. Sodium Silicide –

3. Calcium Nitride –

4. Lithium Oxide –

5. Zinc (II) Phosphide –

6. Iron (II) Oxide –

7. Calcium Carbide –

8. Manganese (VII) Nitride –

9. Cesium Selenide –

10.Strontium Bromide –

IrI3

Ca2C

Ca3N2

Li2O

Zn3P2

FeO

Na4Si

Mn3N7

Cs2Se

SrBr2

Working with Polyatomics

• Remember, polyatomics are a series of charged particles (ions) made up of more than one atom. Hence poly- (many), -atomic (atoms) means “many atoms.”

For Example, Carbonate Ion:

CO32-(CO3)2-

The (2-) charge applies to the ENTIRE polyatomic. So, when you “swap and drop,” you will be doing so to the entire thing all at once.

=

(NH4)2CO3(NH4)

Ex. 16: Ammonium and Carbonate

CO32-NH4

1+






(CO3)1+ 2-

2Neither subscript may be simplified any further.

1

Note: We never write “1” as a subscript. The presence of the symbol indicates that at least one is present already. Also, you can remove the parenthesis in this case.

Done! You’ve just built ammonium carbonate

PbPb2(Cr2O7)3

Ex. 17 : Lead (III) and Dichromate

Cr2O72-Pb3+






(Cr2O7)3+ 2-

2Neither subscript may be simplified any further.3

Done! You’ve just built ammonium carbonate

Na2C2O4Na

Ex. 18 : Sodium and Oxalate

C2O42-Na


2. Use the periodic table or a chart to find the charges of each particle. Ionics are made of “ions” or charged particles.




(C2O4)1+ 2-

2Neither subscript may be simplified any further.1

Done! You’ve just built sodium oxalate.



(SO4)Pb(SO4)2Pb

Ex. 19 : Lead (IV) and Sulfate

SO42-Pb4+






4+ 2-

2Both subscripts may be divided by 2.4

Done! You’ve just built lead (IV) sulfate.

1 2

311Fe


(AsO4)FeAsO4

Ex. 20 : Iron (III) and Arsenate

AsO43-Fe3+






3+ 3-

3Both subscripts may be divided by 3.

Done! You’ve just built iron (III) arsenate.

A quick note:

• Going from names to formulas follows a fairly easy and consistent pattern.

• However, going from formulas to names can prove tricky if transition metals are involved.

• REMEMBER: always find the charge of a transition metal (virtually any metal that is NOT in the “s” block (groups 1 and 2) and place it as a roman numeral in your compound’s name.)

• Watch out for simplification! You may have to reverse this to find the actual charge of a transition metal.

You can prevent these mistakes quite easily by putting your polyatomics in parentheses when you see them and before you do any “swapping and dropping” - like this:

Quick tip!

• When reversing a “swap and drop,” be careful not to accidentally use a subscript that is part of a polyatomic.

• For example:

FeNO3

Fe (NO)3+ 1-

Fe (NO3)1+ 1-

FeNO3 Fe1(NO3)1


1. Lead (IV) chlorite -

2. Cesium phosphate -

3. Ammonium sulfate -

4. Ammonium sulfide -

5. Ammonium sulfite -

6. La(ClO4)3 -

7. Fe3PO4 -

8. Ag2CO3 -

9. V(C2H3O2)5 -

10.CuSO3 -

Pb(ClO2)4

Cs3PO4

(NH4)2SO4

(NH4)2S

(NH4)2SO3

Lanthanum (III) perchlorateIron (I) phosphate

Silver (I) carbonate

Vanadium (V) acetate

Copper (II) sulfite

Advanced Practice

• The slides that follow deal with naming and determining formulas under a variety of conditions. Remember:– Transition metals are given their charges

with a roman numeral. This must be shown in naming them.

– If you are using names to find formulas, be careful. You may have to reverse simplifications to find the true charges of transition metals.

– Polyatomics are given specific names that should not be altered.

– These problems are excellent practice and should be worked through carefully.

First, name the cation and anion, in order. Note that iron, Fe, is a transition metal. We will have to find the original charge of the iron to finish this name.

Finally, ask yourself if these numbers have been simplified. The oxygen is “-2” as we expect. This means that no simplification has occurred and that we can assume iron has a 3+ charge.

Iron (III) Oxide

Oxide

Example 21: Name Fe2O3

Iron (?)

To find the charge of the iron we will have to reverse the “swap and drop” we normally do when creating formulas.

Fe O 3 2

2-3+

Now that the charges are back, they can be made + and – again.

After checking our work, we can conclude that the charge on iron is +3 this time, so we use iron (III) in the name.

Finally, ask yourself if these numbers have been simplified. The oxygen is “-1” while we know it should be “-2”. This means that both charges were divided by 2 to simplify at some point.

Iron (II) Oxide

Oxide

Example 22: Name FeO

Iron (?)

First, name the cation and anion, in order. Note that iron, Fe, is a transition metal. We will have to find the original charge of the iron to finish this name.

To find the charge of the iron we will have to reverse the “swap and drop” we normally do when creating formulas.

Fe O 1 1

1-1+

Now that the charges are back, they can be made + and – again.After checking our work, we can conclude that the charge on iron is +2 this time, so we use iron (II) in the name.

Multiply by 2 to reverse the simplification and find the original charges that were given to iron and oxygen.

2-2+

Multiply by 2 to reverse the simplification and find the original charges that were given to manganese and chromate.

First, name the cation and anion, in order. Note that manganese, Mn, is a transition metal. We will have to find the original charge of the Mn to finish this name.

To find the charge of the manganese we will have to reverse the “swap and drop” we normally do when creating formulas.


Finally, ask yourself if these numbers have been simplified. The chromate is “-1” while we know it should be “-2”. This means that both charges were divided by 2 to simplify at some point.

After checking our work, we can conclude that the charge on Mn is +4 this time, so we use manganese (IV) in the name.

4+

Manganese (IV) Chromate

Chromate

Example 23: Name Mn(CrO4)2

Manganese (?)

Mn (CrO4) 2 1

1-2+ 2-

Finally, ask yourself if these numbers have been simplified. The sulfite is “-2” while we know it should be “-2”. This means that simplification has not occurred.

First, name the cation and anion, in order. Note that copper, Cu, is a transition metal. We will have to find the original charge of the Cu to finish this name.

To find the charge of the copper we will have to reverse the “swap and drop” we normally do when creating formulas.


Cu (SO3) 1+

After checking our work, we can conclude that the charge on Cu is +1 this time, so we use copper (I) in the name.

Copper (I) Sulfite

Sulfite

Example 24: Name Cu2SO3

Copper (?)

1 2

2-

Finally, ask yourself if these numbers have been simplified. The phosphate is “-1” while we know it should be “-3”. This means that both charges were divided by 3 to simplify at some point.

First, name the cation and anion, in order. Note that vanadium, V, is a transition metal. We will have to find the original charge of the vandadium to finish this name.

To find the charge of the vanadium we will have to reverse the “swap and drop” we normally do when creating formulas.

Now that the charges are back, they can be made + and – again.After checking our work, we can conclude that the charge on vanadium is +3 this time, so we use vanadium (III) in the name.

Multiply by 3 to reverse the simplification and find the original charges that were given to vanadium and phosphate.

Vanadium (III) Phosphate3+

V (PO4)

Phosphate

Example 25: Name VPO4

Vanadium (?)

1 1

1-1+ 3-

Practice on Your Own

• Fe3AsO4 -

• CuF -• Pb(NO3)2 -

• Ir(Cr2O7)3 -

• Zr(S2O3)2 -

• Ag2C2O4 -

• Ti(CN)4 -

• Ga2(SO4)3 -

• WCrO4 -

• (NH4)3PO3 -

Iron (I) arsenateCopper (I) fluoride

Lead (II) nitrate

Iridium (VI) dichromate

Zirconium (IV) thiosulfate

Silver (I) oxalateTitanium (IV) cyanide

Gallium (III) sulfate

Tungsten (II) chromate

Ammonium phosphite

Excellent!

• If you’ve made it this far, you should have virtually complete mastery of chemical nomenclature.

• Congratulations!

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