Post on 25-Dec-2015
NAMING COMPOUNDS
TYPES OF COMPOUNDS Molecular compound (covalent bonds)
Compound made of two nonmetals NBr5
Ionic compound Compound made of a metal and a
nonmetal NaCl
Acid (ionic bonds) Compound that can donate a hydrogen ion HCl
MOLECULAR COMPOUND (TWO NONMETALS)
To name a molecular compound, you have two parts: The first element in the compound and The second element in the compound
NBr5
The first element is called by its normal name: N – nitrogen
The second name is called by its name and ends in –ide: Br – bromine bromide
PREFIXESIn addition to naming the
elements, you have to name how many they are. To do this you need prefixes.
The prefix goes in the front of the name of the element
PREFIXES (CONT)One – monoTwo – diThree – triFour – tetraFive - penta
Six – hexaSeven – hepta
Eight – octaNine – nonaTen - deca
MOLECULAR COMPOUND (CONT)
Therefore if you start with NBr5:Mononitrogen pentabromide
BUT wait, if you only have one element in the beginning part of the compound, you don’t have to put the prefix:Nitrogen pentabromide
TRY THESE
1. SCl62. N2O4
3. P3F5
4. CCl45. XeO
1. Trinitrogen hexaoxide
2. Boron pentabromide
3. Tetrasulfur decafluoride
4. Phosphorus octaiodide
ANSWERS1. Sulfur
hexachloride2. Dinitrogen
tetraoxide3. Triphosphorus
pentafluoride4. Carbon
tetrachloride5. Xenon monoxide
1. N3O6
2. BBr5
3. S4F10
4. PI8
SPECIAL CASEWhen naming some compounds, it is implied
that the compound is a DIATOMIC GASThere are only 7 diatomic molecules
HydrogenNitrogenOxygenFluorineChlorine IodineBromine
DIATOMIC MOLECULES If you ever see any of those molecules, you
write them as a compound with two of the atoms
Hydrogen – H2 Nitrogen – N2 Oxygen – O2 Fluorine – F2 Chlorine – Cl2 Iodine – I2 Bromine – Br2
IONIC COMPOUNDS (METAL AND NONMETAL)
The two parts of naming an ionic compound: The first element is always the metal The second element is the nonmetal
CaBr2 The first element is called by its normal
name: Ca Calcium The second element is named like a
molecular compound: Br bromideThe only difference is that you do
not use a prefix ever
IONIC COMPOUNDSTherefore if you start with
CaBr2:
Calcium Bromide
There is no prefix for bromide even though there is a 2
IONIC COMPOUNDSBefore we begin practice naming
ionic compounds, look at your ion sheet
Remember: To put ionic compounds together, you need to BALANCE THE CHARGE
EXAMPLE How would you show the following ionic
compound: Strontium iodide Strontium Sr (has a +2 charge: alkali earth
metal) Iodide (has a -1 charge: halogen) Just like before, cancel swap the charges
Sr+2 + 2I - SrI2
Your ion sheet gives you the names of several ions with the many possible charges of the transition metals
TRY THESE
1. BaCl22. K2O
3. AlF3
4. CaO
1. Magnesium oxide
2. Potassium sulfide
3. Sodium chloride
4. Beryllium iodide
ANSWERS1. Barium
chloride2. Potassium
oxide3. Aluminum
fluoride4. Calcium oxide
1. MgO2. K2S
3. NaCl4. BeI2
POLYATOMIC IONSAn ion that is composed of several
atomsFORMAL DEFINITION
Polyatomic ion: an electrically charged group of two or more chemically bonded atoms that function as a SINGLE ION
POLYATOMIC IONSSince the polyatomic ions are made of
more than 1 atom, their names are complicated
Example of some polyatomic ions:OH - hydroxideClO4 - perchlorateCO3
-2 carbonateNH4 + ammonium
POLYATOMIC IONS IMPORTANT NOTE: When combining
polyatomic ions, you still balance out the NET CHARGE:
Example: If you have sodium hydroxideSodium: Na+
Hydroxide: OH –
Na+ + OH - NaOH
POLYATOMIC IONWhat do you do if you have more than 1
polyatomic ion to balance out a charge?Example: If you have Magnesium acetate
Magnesium: Mg+2
Acetate: C2H3O2 –
Mg+2 + 2C2H3O2- Mg(C2H3O2)2
You put the entire polyatomic ion in brackets with the number of ions as a subscript
TRY THESE1. Lithium
oxalate2. Barium
bromate3. Sodium
Phosphate4. Aluminum
sulfate
1. K3BO3
2. Sr(NO2)2
3. Mg3(PO4)2
4. CaSO4
ANSWERS
1. Li2C2O4
2. Ba(BrO3)2
3. Na3PO4
4. Al2(SO4)3
1. Potassium borate
2. Strontium nitrite
3. Magnesium phosphate
4. Calcium sulfate
IONIC COMPOUNDS (TRANSITION METALS)
What do you do when you do not know the exact charge of the ion?
In other words, some of the transition metals can have more than 1 ionFe+2
Fe+3
You distinguish with Roman numerals
IONIC COMPOUNDS (TRANSITION METALS)
Solution: The name of the compound tells you the charge.
If you have a compound of iron and oxygen, an example would be: Iron (III) oxide
This means that iron has a +3 charge2Fe+3 + 3O-2 Fe2O3
IONIC COMPOUNDS (TRANSITION METALS)
This means that if you’re given the formula, you have to figure out the charge of the metal ion:
Example: MnO2
What you know: O has a -2 chargeTherefore the total negative is -4This means that you need a +4 to
balanceYou get Manganese (IV) oxide
TRY THESE1. Nickel (III)
iodate2. Lead (II)
chloride3. Gold (I)
Sulfate4. Vanadium (III)
chlorate
1. W(PO4)2
2. AuBO3
3. Tl3PO4
4. Sn(NO3)4
ANSWERS
1. Ni(IO3)3
2. PbCl23. Au2SO4
4. V(ClO3)3
1. Tungsten (VI) phosphate
2. Gold (III) borate
3. Thallium (I) phosphate
4. Tin (IV) nitrite
ACIDS What is an acid?
For now: An acid is a compound that will donate a proton (H+)
How do you recognize an acid Any compound that begins with H+
There are two basic types of acids for naming Binary acid Polyatomic acid
BINARY ACID A binary acid has a hydrogen ion and a single
halide Examples: HCl, HF, HBr, HI
Naming these acids takes the following format: Hydro-(root of the name of the halide)-ic acid
Therefore HCl becomes Hydrochloric acid
BINARY ACID What would be the names of the
following:1. HF2. HBr3. HI
ANSWERS
1. Hydrofluoric acid2. Hydrobromic acid3. Hydroiodic acid
POLYATOMIC ACIDSSimilar convention to binary acids
(Base name of the polyatomic ion)-ic acid
HC2H3O3
This is an H+ with a C2H3O3-
The name of the polyatomic ion is acetate
The name is Acetic acid
POLYATOMIC ACIDSThe differencesWhat if you have H2SO4 and
H2SO3
What’s the difference in these two names?: only one can be sulfuric acid
POLYATOMIC ACIDS If the ion ends in the name “-ate”
Sulfate, nitrate, chlorate The name of the acid is (root of ion)-ic acid Sufuric acid, nitric acid, chloric acid
If the ion ends in the name “-ite” Sulfite, nitrite, chlorite The name of the acid is (root of ion)-ous acid Sulfurous acid, nitrous acid, chlorous acid
TRY THESE
1. H2CO3
2. HNO2
3. HIO3
4. H3PO4
1. Oxalic acid2. Sulfurous
acid3. Sulfuric
acid4. Bromic acid
ANSWERS1. Carbonic
acid2. Nitrous acid3. Iodic acid4. Phosphoric
acid
1. H2C2O4
2. H2SO3
3. H2SO4
4. HBrO3
SUMMARYBefore you start naming,
determine the type of compound Molecular, ionic or acid
Naming molecular compounds (nonmetal and nonmetal) Name of the first element Base name of the second element + ide Make sure you use the prefix indicating
number of atoms
SUMMARY (CONT) Naming ionic compounds (metal and
nonmetal) Name of the first element
Name of the second element + ide or
Name of the second polyatomic ion
Make sure you balance the charges of each ion
If the metal has more than 1 possible charge, indicate the charge with a Roman numeral
SUMMARY (CONT)Acids (the compound has a
hydrogen ion H+) Binary acids Hydro (base name of the halogen)-ic acid
Polyatomic acids (Base name of the polyatomic ion w/
“-ate”) – ic acid (Base name of the polyatomic ion w/
“-ite”) – ous acid
WRITE THE SYMBOL OR NAME
1. Calcium chloride2. Lead (IV) sulfate3. Carbon
tetrachloride4. Hydroiodic acid5. Sulfuric acid6. Dinitrogen
hexachloride
7. HBr8. NH4NO3
9. S3Br8
10. NO11. HNO2
12. Mn(C2H3O2)3
13. Pb(SO3)2
ANWERS
1. CaCl22. Pb(SO4)2
3. CCl44. HI5. H2SO4
6. N2Cl6
7. Hydrobromic acid8. Ammonium nitrate9. Trisulfur
octabromide10. Nitrogen monoxide11. Nitrous acid12. Manganese (III)
acetate13. Lead (IV) sulfite
PUTTING THIS IN A CHEMICAL REACTION
General Format: Reactants Products
Steps Translate the chemical into its symbol and
then put the state of matter AFTER the chemical symbol
Put a “+” between each set of reactants and products
STATES OF MATTER Symbols for states of matter:
Solid (s) Liquid (l) Gas (g) Aqueous (aq)
EXAMPLE Solid sodium is mixed with chlorine gas
to form aqueous sodium chloride Solid sodium = ? is mixed with = ? chlorine gas = ? to form = ? aqueous sodium chloride = ?
FINAL ANSWER
Na(s) + Cl2(g) NaCl(aq)
TRY THESE1. Solid iron is combined with oxygen gas
to produce solid iron(III) oxide.2. Aqueous magnesium nitrate is
combined with solid zinc to form aqueous zinc nitrate and solid magnesium.
ANSWERS
1. Fe(s) +O2(g) Fe2O3(s)
2. Mg(NO3)2(aq) + Zn(s) Zn(NO3)2(aq) + Mg(s)