1. Chemical Nomenclature
1. Binary Ionic Compounds - Type I
2. Binary Ionic Compounds - Type II
3. Ionic Compounds & Polyatomic (Complex) Ions
4. Hydrated Ionic Compounds
5. Binary Covalent Compounds
6. Binary Acids
7. Oxy-Acids

2. Definitions
An IONIC COMPOUND consists of a metal cation bonded to a nonmetal anion. Electrostatic attraction holds them together.
A COVALENT COMPOUND consists of two nonmetal atoms sharing valence electrons.
A BINARY compound is one that is made of just two elements. There can be one of each element such as in NaCl or KF. There can also be several of each element such as Na2O or AlBr3.

3. Type I Binary Ionic Compounds
The metal cations in these compounds have only ONE possible charge.
Na+ Zn2+ Al3+ Ca2+
sodium zinc aluminum calcium
The charges are memorized or predicted using a periodic table!
The cations are bonded to nonmetal anions:
O2- N3- F- Br -
oxide nitride fluoride bromide
Notice that simple anions are always named with the suffix “ide”

4. Predicting Charges on Monatomic Ions
KNOW THESE !!!!
Cd+2

5. COMPOUNDS FORMED FROM IONS
CATION +
ANION --->
COMPOUND
Na+ + Cl- --> NaCl
A neutral compound
requires
equal number of +
and - charges.

6. CaCl2 = calcium chloride
Naming Compounds
Binary Ionic Compounds:
1. Cation first, then anion
2. Monatomic cation = name of the element
Ca2+ = calcium ion
3. Monatomic anion = root + -ide
Cl- = chloride
CaCl2 = calcium chloride

7. Naming Binary Ionic Compounds
Examples:
NaCl
ZnI2
Al2O3

8. Learning Check Complete the names of the following binary compounds:
Na3N sodium ________________
KBr potassium ________________
Al2O3 aluminum ________________
MgS _________________________

9. Formulas for Binary Ionic Compounds
A binary compound is one made of two different elements. There can be one of each element such as in sodium bromide or potassium iodide. There can also be several of each element such as lithium oxide or aluminum bromide.

10. Writing Formulas Formula Unit – lowest whole number ratio of ions in an ionic compound
Points to remember about writing the formula from the name
The order in a formula is first the cation, then the anion.
You must know the charges associated with each cation and anion.
The sum of the positive charge and the sum of the negative charges MUST add up to zero.
You MAY NOT adjust the charges of the cations or anions to get a total charge of zero.
You MAY adjust the subscripts to get a total charge of zero.

11. Example #1 Suppose you must write the formula for sodium chloride.
             
Write down the Na+ and Cl¯ right next to each other, as in this image:
Move the positive charge (dropping the sign) to the subscript position of the anion:
Move the negative charge (dropping the sign) to the subscript position of the cation:
The result of all this moving is:
Since subscripts of one are not written, but understood to be present, the final answer is:

12. Example #2 Write the formula for aluminum oxide.
Write down the Al3+ and O2¯ right next to each other :
Move the positive charge (dropping the sign) to the subscript position of the anion:
Move the negative charge (dropping the sign) to the subscript position of the cation:
The result of all this moving is:

15. Learning Check
Write the correct formula for the compounds containing the following ions:
1. Sodium sulfide
a) NaS b) Na2S c) NaS2
2. Aluminum chloride
a) AlCl3 b) AlCl c) Al3Cl
3. Magnesium nitride
a) MgN b) Mg2N3 c) Mg3N2

16. Solution
1. Na+ S2-
b) Na2S
2. Al3+ Cl-
a) AlCl3
3. Mg2+ N3-
c) Mg3N2

17. Examples: Type I Binary Ionic Compounds
Write the formulas:
potassium oxide
zinc chloride
silver sulfide
aluminum nitride
gallium oxide
calcium iodide
Write the names:
K3N
AgI
ZnBr2
Al2O3
Ba3P2
LiH

18. Transition Metals
Elements that can have more than one possible charge MUST have a Roman Numeral to indicate the charge on the individual ion.
1+ or or 3+
Cu+, Cu Fe2+, Fe3+
copper(I) ion iron(II) ion
copper (II) ion iron(III) ion

19. Names of Variable Ions FeCl3 (Fe3+) iron (III) chloride
These elements REQUIRE Roman Numerals because they can have more than one possible charge:
anything except Group 1A, 2A, Ag, Zn, Cd, and Al
(You should already know the charges on these!)
Or another way to say it is: Transition metals and the metals in groups 4A and 5A (except Ag, Zn, Cd, and Al) require a Roman Numeral.
FeCl3 (Fe3+) iron (III) chloride
CuCl (Cu+ ) copper (I) chloride
SnF (Sn4+) tin (IV) fluoride
PbCl (Pb2+) lead (II) chloride
Fe2S (Fe3+) iron (III) sulfide

20. Learning Check
Complete the names of the following binary compounds with variable metal ions:
FeBr2 iron (_____) bromide
CuCl copper (_____) chloride
SnO2 ___(_____ ) ______________
Fe2O3 ________________________
Hg2S ________________________

21. Examples: Type II Binary Ionic Compounds
Write the formulas:
iron (II) oxide
copper (II) chloride
tin (IV) sulfide
cupric nitride
nickel (III) oxide
ferrous iodide
cobalt (III) selenide
Write the names:
Fe2O3
SnS
NiBr2
CuS
Pb3P2
CuBr
FeCl3

22. Formulas of Ionic Compounds
Formulas of ionic compounds are determined from the charges on the ions
atoms ions
    –
Na  +  F :  Na : F :  NaF
   
sodium + fluorine sodium fluoride formula
Charge balance: = 0

23. Polyatomic Ions
NO3-
nitrate ion
NO2-
nitrite ion

24. Polyatomic (Complex) Ions
All of the cations and anions so far have been simple ions - single atoms that have lost or gained electrons.
Complex polyatomic ions may be cations or anions.
examples:
nitrate: NO3- sulfate: SO42- hydroxide: OH-

25. 4/21/2017
IONIC COMPOUNDS
NH4+
Cl-
ammonium chloride, NH4Cl

26. Things to Notice
Most complex ions are anions. Ammonium, NH4+, is the most common complex cation.
Several complex ions form a short series of ions. The ions differ only in the number of oxygen atoms:
perchorate ClO4- sulfate SO42-
chlorate ClO3- sulfite SO32-
chlorite ClO2-
hypochlorite ClO- nitrate NO3-
nitrite NO2-

27. If an ion carries a charge like “-2” or “-3”, a series of related ions can be formed by adding hydrogen cations (H+) while still leaving a net charge:
examples:
Sulfide: S2- hydrogen sulfide: HS-
(bisulfide)
Sulfate: SO42- hydrogen sulfate: HSO4-
(bisulfate)
Carbonate: CO32- hydrogen carbonate: HCO3-
(bicarbonate)
Phosphate: PO43- hydrogen phosphate: HPO42-
dihydrogen phosphate: H2PO4-

28. Ionic Compounds containing Polyatomic Ions
Writing Formulas
Write each ion, cation first. Don’t show charges in the final formula.
Overall charge must equal zero.
If charges cancel, just write symbols.
If not, use subscripts to balance charges.
Use parentheses to show more than one of a particular polyatomic ion.
Use Roman numerals to indicate the ion’s charge when needed (stock system)

30. Learning Check 1. aluminum nitrate a) AlNO3 b) Al(NO)3 c) Al(NO3)3
2. copper(II) nitrate
a) CuNO3 b) Cu(NO3)2 c) Cu2(NO3)
3. Iron (III) hydroxide
a) FeOH b) Fe3OH c) Fe(OH)3
4. Tin(IV) hydroxide
a) Sn(OH)4 b) Sn(OH) c) Sn4(OH)

31. Writing formulas with Complex Ions
a) Ammonium chloride
b) Silver sulfate
c) Aluminum hydroxide
d) Calcium phosphate
e) Iron (III) nitrite
f) Copper(II) permanganate
g) Ammonium dichromate
h) Zinc acetate

32. More Formulas with Complex Ions
a) NaHCO3
b) Ni(HS)2
c) Al(ClO4)3
d) Ba(H2PO4)2
e) Fe2(SO2)3
f) CuHSO4
g) Zn(IO4)2

33. Mixed Practice!
Name the following:
Na2O
CaCO3
PbS2
Sn3N2
Cu3PO4
HgF2

34. Mixed Up… The Other Way Write the formula: Copper (II) chlorate
Calcium nitride
Aluminum carbonate
Potassium bromide
Barium fluoride
Cesium hydroxide

35. Naming Molecular Compounds
4/21/2017
Naming Molecular Compounds
All are formed from two or more nonmetals.
CO2 Carbon dioxide
Ionic compounds generally involve a metal and nonmetal
(NaCl)
BCl3 boron trichloride
CH4 methane

36. Binary Covalent Compounds
Covalent compounds are made of two NONMETAL elements sharing valence electrons.
There are no ions involved!!
Because there are no charges to help us write the formulas of covalent compounds, prefixes are used to indicate the number of each atom present in the formula.
The first element receives a prefix if the subscript is greater than one. The second element ALWAYS gets a prefix.Change the ending of the second element to -ide.
The prefix, “mono”
is never used for
the first element
in the formula!

37. Molecular (Covalent) Nomenclature for two nonmetals
Prefix System (binary compounds)
CO2 is named “carbon dioxide”
CO is named “carbon monoxide”
N2O is named “dinitrogen monoxide”
SO3 is named “sulfur trioxide” .

38. Molecular Nomenclature Prefixes
mono-
di-
tri-
tetra-
penta-
hexa-
hepta-
octa-
nona-
deca-
NUMBER 1 2 3 4 5 6 7 8 9 10

39. Molecular Nomenclature: Examples
CCl4
N2O
SF6

40. More Molecular Examples
arsenic trichloride
dinitrogen pentoxide
tetraphosphorus decoxide

41. Learning Check
Fill in the blanks to complete the following names of covalent compounds.
CO carbon ______oxide
CO2 carbon _______________
PCl3 phosphorus _______chloride
CCl4 carbon ________chloride
N2O _____nitrogen _____oxide

42. Learning Check 1. P2O5 a) phosphorus oxide b) phosphorus pentoxide
c) diphosphorus pentoxide
2. Cl2O7 a) dichlorine heptoxide
b) dichlorine oxide
c) chlorine heptoxide
Cl2 a) chlorine
b) dichlorine
c) dichloride

43. Binary Acids
A simple definition of an “acid” is a substance which produces H+ ions in water.
Most acids have hydrogen ions in their formulas.
A binary acid composed of a hydrogen cation bonded to one other element:
HCl HBr H2S
hydrochloric acid hydrobromic acid hydrosulfuric acid
Binary acids are always named: hydro____ic acid

44. Oxy-Acids
An acid can also be made of a hydrogen ion bonded to a complex ion.
Complex ions whose names end in “ate”:
NO SO42- CO32- PO43-
nitric acid: HNO3
sulfuric acid: H2SO4
carbonic acid: H2CO3
phosphoric acid: H3PO4
Can you propose a rule for naming oxy-acids with complex ions ending in “ate”?

45. More Oxy-Acids Complex ions ending in “ite”: NO2- SO32- ClO- ClO2-
nitrous acid: HNO2
sulfurous acid: H2SO3
hypochlorous acid: HClO
chlorous acid HClO2
Can you propose a rule for naming oxy-acids with complex ions ending in “ite”?

46. Hydrated Ionic Compounds
A HYDRATE is an salt that has water molecules trapped within its crystals.
Every hydrate has a certain number of water molecules associated with each formula unit of the ionic compound. The number of water molecules is indicated by using prefixes.
mono hexa
di hepta
tri octa
tetra nona
penta deca
CuSO4 · 5 H2O
copper (II) sulfate pentahydrate
MgCO3 ·10 H2O
magnesium carbonate decahydrate

47. Examples of hydrates: Write the formulas:
copper(II) fluoride tetrahydrate CuF2 ·4 H2O
calcium nitrate trihydrate Ca(NO3)2 ·3 H2O
Write the names:
MgSO4 · 7 H2O magnesium sulfate heptahydrate
FeCl2 · H2O iron (II) chloride monohydrate