Nomenclature!!! - What’s in a name?
REMEMBER!!!
1. When naming compounds ALWAYS, ALWAYS have a periodic table in front of you!
2. Ions – positively or negatively charged atom due to an decrease or increase of electrons
– __________ – positively charged ( metals that loose electrons) ex. Na+
– __________ – negatively charged (non-metal that gains electrons) ex. ClNaming Binary Ionic Compounds
• Binary Ionic Compound
– A compound that has 2 atoms, __________ and __________
– Cation is always __________
– Type I and Type II
• Type I
– The metal only forms __________ type of cation, ex. Li → Li+
• Type 2
– The metal can form _________________ cations, ex. Cu → Cu+ or Cu2+
• How can you tell if it is a Type I or Type II?
– Type I: ________________, Al, Zn, Cd, and Ag,
– _________________ are almost always Type II
Rules for Naming Type I Ionic Compounds
1. Cation ( __________ ) is named before the anion (non-metal).
2. Cation (metal) is the name of the __________ .
3. Anion (non-metal) is the “ __________ ” of the element + ide
4. Combine the Cation and Anion
Ex. NaCl
1. Cation is named before the anion.
– we know that Na is first because it’s a cation
2. Cation is the name of the element.
– Na is __________
3. Anion is the “root” of the element + __________
– Cl is Chlorine, root is __________ = Chloride
4. Combine the Cation and Anion
– ________________ is the name!!
****Notice: The formula doesn’t show the __________ of the individual ions.
****Ex. NaCl means Na+ is present with Cl****Ex. CaS means __________ is present with __________
• Let’s try some!!
• CsF • CaBr2 • AlCl3 • ZnS • MgI2 • BaH2• KCl • Al2S3Binary Ionic Compounds Type II
• Some metals can form more than __________.
• This is what makes them Type II
– Ex. Lead(Pb) => Pb2+ or __________
– Ex. Iron(Fe) => Fe2+ or __________
– ____________________ are almost always Type II
• To name these we use the same naming method except we add a _______________ to the cation name.
• The anion stays the same as before.
EXTEMELY IMPORTANT!!!
• The Roman numeral tells the __________ , not the # of ions present.
• Ex. Fe3+ => iron(III) and Fe2+ => iron(II)
• Ex. Pb2+ => lead(II) and Pb4+ => lead(IV)
• The anion will be named the __________ as with Type I (using ide for the ending)
• Anion is the “root” of the element + ide
• Ex. O is Oxygen, root is Ox + ide = Oxide
• Ex. Cl is Chlorine, root is Chlor + ide = Chloride
• All together:
• FeCl2 => __________
• PbO2 => __________
Lets take a closer look.
• We are given FeCl2
• We know the overall charge has to be __________
• We know:
• Cl is going to have a ____ charge.
• there are 2 Cl
• Cl2 has an overall charge of ______
• There is only one Fe atom
• Therefore the one Fe has to have a charge of _____
Let’s try some!!!
1. CuCl
3. Fe2O
2. HgO
Rules for naming Binary Covalent Compound: Prefix System
1. The first atom is the __________ .
2. The second atom is named like an __________ .
3. Add __________ to indicate # of atoms. Omit mono- prefix on the __________ element.
Ex. PCl3 => phosphorus trichloride
• These are the prefixes that are used to indicate the number of atoms in a compound.
•
__________ is never used for the first atom.
• Binary Covalent Compound:
• Example: __________
1. The first atom is the element name.
– I becomes iodine
2. The second atom is named like an anion.
– O is Oxygen, root is __________ = oxide
3. Prefixes are given to each atom to tell the number of atoms present.
– di = 2, hepta = 7
– so… di + iodine = diiodine
– and… hepta + oxide = heptoxide
– Answer: __________
• Let’s try some!!!
1. BF3 –
5. Al2S3 2. NO 6. SnBr4 3. N2O5 7. CS2 4. AsF3 8. CdS -
Polyatomic Ions
– Charged entities composed of ______ ____ bound together
– Assigned __________ names
– No system, must be __________
– (don’t worry you don’t have to, just know how to use it)
– Ex. CN-, NH4+, NO3- , See pg 109
• Oxyanions
– Some of these polyatomic ions are called __________
– They contain an atom and different #’s of oxygen atoms.
– Ex. NO3-, ClO2-, PO43– These oxyanions, form in a __________.
• The smaller # O, ends with _____.
• The larger # O, ends with ____.
• The smallest # O, begins with _____, meaning less than
• The largest # O, begins with _____, meaning more than
– All combined
•
__________ = hypo => ClO- = hypochlorite
• Small = ite => ClO2- = ________
• Large = ate => ClO3- = __________
•
_________ = per => ClO4- = perchlorate
Now back to the naming complex compounds
• Need to _________ common polyatomic ions
• Now when you see NH4C2H3O2 you can break it down.
– __________=> ammonium and C2H3O2+ => __________
– It’s name is ammonium acetate
****Notice that it’s separate parts have a __________ but together they are neutral.
• Also like Type II, Binary Compounds, you may need ______________
• Ex. FeSO4 => iron(II) sulfate
• Ex. Mn(OH)2 => manganese(II) hydroxide
Lets practice some!!
• Na2(SO)4• KH2PO4• Fe(NO3)3-
Naming Acids!!
Acids
• Is a molecule with one or more ______ ions attached to an anion.
• Translation: A molecule with _______ and non-metals
• Ex. HCl, HCN, H2S
Naming Acids
• Two types:
1. Ones that __________ oxygen
2. Ones __________ oxygen
Those __________ oxygen
1. Start with the _________of the anion.
2. Add the prefix __________
3. Add the suffix __________
o Ex. hydrochloric acid
o Ex. hydrofluoric acid
Example: HCl
1. Start with the root of the anion. Cl is chlorine, root => __________
2. Add the prefix ________ , hydro + chlore = hydrochlore
3. Add the suffix ______ . hydrochlore + ic = hydrochloreic
4. Answer: hydrochloreic acid
A few exceptions
•
__________ => hydrocyanic acid
•
__________ => hydrosulfuric acid
Those
1.
2.
3.
•
•
•
____________ oxygen
Start with the __________ of the anion.
If the anion ends with an _______, Drop the ate and add ic
If the anion ends with _______, Drop the ite and add ous
Example: HC2H3O2
1. Start with the __________ of the anion. C2H3O2 is Acetate = > root is acet
2. If the anion ends with an ate, Drop the ate and add _________
3. Answer: Acet + ic => __________
Example: HNO2
1. Start with the root of the __________. NO2 is nitrite = > root is nitr
2. If the anion ends with _______, Drop the ite and add ous
3. Answer: Nitr + ous => ________
A few exceptions
Sulfur, H2SO4 => __________ acid
and
________ => phosphoric acid
Naming acids flow chart