naming chemical compounds. binary ionic compounds binary = 2 types of elements ionic = made of ions...
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Naming Chemical Compounds
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Binary Ionic Compounds
Binary = 2 types of elements Ionic = made of ions Compound = atoms bonded
together
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Ionic Compounds
Positive ions are attracted to Negative ions
FORMULA UNIT
Cation always comes first, then anion
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Elemental anions
When an element becomes an anion, it starts to end in –ide Fluoride Chloride Bromide Oxide Sulfide Nitride Phosphide
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Type I
The cation has a predictable charge Alkali Metals +1 Alkaline Earth Metals +2 Group 3A +3 Silver Ag+
Zinc Zn2+
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Type II
The cation has a variable charge All Transition metals except for Ag and Zn (for
our purposes) The name will have a roman numeral to
denote the CHARGE on the cation
Fe2+
Fe3+
Cu+
Cu2+
Iron(II)
Iron(III)
Copper(I)
Copper(II)
Ferrous
Ferric
Cuprous
Cupric
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Naming ionic compouds (Type I and II)
First name cation Just the name of element if Type I Name of element and roman numeral
with charge on cation if Type II Then name anion
Elemental anions end in “–ide”
When determining the formula, remember “swap ‘n’ drop”
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Name the following:
Na3N
MgCl2 Al2O3
CuCl CuCl2 PbBr4
Sodium nitride Magnesium chloride Aluminum oxide
Copper(I) chloride Copper(II) chloride Lead(IV) bromide
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Determine the formula of the following
Aluminum chloride Magnesium Oxide Sodium nitride Calcium chloride Copper(I) sulfide Lead (II) bromide Iron(III) oxide
AlCl3 MgO Na3N
CaCl2 Cu2S
PbBr2
Fe2O3
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Polyatomic Ions
Many anions are not just ions of elements.
Polyatomic Ions = many atomed particle with an overall charge
Mostly nonmetals bonded to Oxygens
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Polyatomic Ion Naming
Main polyatomic ion Ends in “–ate” Example: Chlorate ClO3
-
One fewer oxygens Ends in “-ite” Example: Chlorite ClO2
-
Even fewer oxygens Hypo = under Example: Hypochlorite ClO-
More oxygens than main ion Hyper = over, shortened to “per” Example: Perchlorate ClO4
-
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Common Polyatomic Ions
NO2- Nitrite
NO3- Nitrate
SO32- Sulfite
SO42- Sulfate
PO43- Phosphate
PO33- Phosphite
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Common Polyatomic Ions
Hydrogen can attach to the polyatomic ions as H+
This adds an H and reduces the overall charge by 1
PO43- Phosphate
HPO42- Hydrogen
Phosphate
H2PO41- Dihydrogen
Phosphate
CO32- Carbonate
HCO31-
Hydrogen carbonate
(bicarbonate)
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Name these compounds with PAIs
AlPO4
Cu(NO3)2
Na2SO4
NaHCO3
Mg3(PO4)2
Aluminum phosphate Copper(II) nitrate Sodium sulfate Sodium bicarbonate Magnesium Phosphate
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Molecular Compounds
Molecular compounds are not bonded by positive and negative ions
They SHARE electrons Made of two non-metals Cannot predict or explain charges
(no charges, because not LOSING or GAINING electrons – SHARING)
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Naming Molecular Compounds (Type III)
Because there is no way to neutralize the compounds (like for ions) we must determine how many there are another way:
Use PREFIXES
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How to tell if it’s Type III
Check the FIRST element – is it a non-metal?
If YES, it’s a Type III
Name the first element as the element
Name the second element ending in “-ide”
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Prefixes
1 2 3 4 5 6 7 8 9 10
Mono Di Tri Tetra Penta Hexa Hepta Octa Nona Deca
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Using prefixes
If there is only one of the first element, you may omit the “mono”
You may not omit any other prefixes
The more electronegative element goes last (upper right hand corner)
F, O, N, Cl,
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Name the following
PCl3 CO2
NO N2O4
N2F5
OF2
Phosphorus trichloride Carbon dioxide Nitrogen monoxide Dinitrogen tetroxide Dinitrogen pentafluoride Oxygen difluoride
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Naming Practice! For each of the following compounds, determine whether it is type I, II, or III.
1. FeCl32. NaCl3. Cu(OH)2
4. N2O
5. BaSO4
6. PO5
7. (NH4)CO3
8. SnBr2
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Naming Practice! For each of the following compounds, determine the CHARGE on the cation (+1, +2, +3, or +4)
1. FeCl32. Cu(OH)2
3. Cr2S3
4. NiS5. Pb(NO3)2
6. SnCl4
1. 3
2. 2
3. 3
4. 2
5. 2
6. 4
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Acids
All acids have the H+ ion in them as the cation.
All acids have “acid” in their name
Consider Hydrochloric Acid HCl
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Naming Acids
If the anion DOES NOT CONTAIN OXYGEN: Prefix hydro- Root name of anion element Suffix –ic
Examples HF H2S
Hydrofluoric Acid
Hydrosulfuric Acid
Hydrooxygenic acid
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Naming Acids
If the anion CONTAINS OXYGEN (ie: is a polyatomic ion) Root name of the PAI If anion ends in -ate,
acid ends in –ic If anion ends in –ite,
acid ends in –ous
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Naming Acids Examples
H2SO4
H2SO3
HNO3
HNO2
HC2H3O2
Phosphoric Acid Carbonic Acid
Sulfuric Acid Sulfurous Acid Nitric Acid Nitrous Acid Acetic Acid
H3PO4
H2CO3
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Organic Molecules
Carbon based Naming is based on number of
carbons Functional groups
Sets of molecules attached to the carbons
Naming is also based on what functional groups are where
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Alkanes
The simplest organic molecules are Alkanes.
Carbons are all single bonded to each other
When not bonded to another carbon, bonded to a Hydrogen
All alkanes end in -ane
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Prefixes
Note that the prefixes pertain to all types of carbon based molecules with any types of functional groups or chains
•Meth•Eth•Prop•But
•Pent•Hex•Hept•Oct
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Alkenes and Alkynes
A functional group can be a set of atoms, or the way they are bonded.
Alkenes Carbons have double bonds between
them Alkynes
Carbons have triple bonds between them
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Alkenes and Alkynes
To Name All alkenes end with –ene. All alkynes end with –yne Number the carbons in the longest
chain. Carbon 1 is at the end of the chain
closest to the first functional group Put the number that the bond is on,
then the chain length (some name by putting the number
BEFORE the functional group ending)
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Isomer = molecule with SAME formula but DIFFERENT structure
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Alcohols
Have an –OH group attached Name the carbon chain (prefix and
bond) End in –ol Indicate which carbon the –OH is on
2-propanol 1-Butanol 3-Octenol
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What are the formulas for these alcohols?
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Alcohols
Some alcohols have common names like glycerol
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Branched Hydrocarbons
The longest continuous chain of carbon atoms gives the root name/prefix.
Substituent is named by the number of carbons.
Specify location of substituent by numbering carbon atoms in longest chain.
Substituent often referred to as R or R’ (for second substituent)
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Substituent often referred to as R or R’ (for second substituent)
If more than one alkyl group, use prefix di, tri, etc. to alkyl name
Substituents listed in alphabetical order (disregarding prefix)
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Branched Hydrocarbon SubstituentAlkyl groups
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What is the name of the compound?
Hints
•Number Carbon chain from on side closest to first alkyl group
•Single carbon branch called methyl, triple carbon group called propyl
•More than one branch, use prefixes di-, tri-, etc.
2,4 dimethyl hexane 4 ethyl,5 methyl heptane
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Tricky ones!!!
Each END of a line is a Carbon atom. No H’s are indicated, but they are assumed
See if you can name these.
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Halohydrocarbons
Functional group is a halogen (X = F, Cl, Br, I)
General Formula R – X
Naming Select longest chain containing halogen Number so that C with halogen gets
lowest number
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Ethers
Functional group - O –
General Formula R – O – R’
Naming Name the R group as an alkyl Name the R’ group as an alkyl End in ether
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Aldehydes
Functional group - C – H
General Formula R – C – H
Naming Name the R group Change the ending to -al
||O
||O