1. Nomenclature Ionic, Covalent, Acid
Unit 5: Formulas, Part 2
Nomenclature Ionic, Covalent, Acid
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2. Unit 5: Formulas, Part 2 Nomenclature!
(Is a fancy word for naming things)
There are 3 types of compounds you need to know how to name & write formulas for:
Ionic (we already learned that!)
Molecular (aka Covalent)
Acid (a special type of covalent)

3. A. Ionic FORMULAS Review
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 polyatomic ion.
Roman numerals indicate the ion’s CHARGE

4. A. Ionic NOMENCLATURE Write the names of both ions, cation first.
Change ending of monatomic ions to -ide.
Polyatomic ions have special names. Don’t change polyatomic endings!
Use Roman numerals to show the metal’s positive charge (except s-block, Ag, Zn, Al).
Overall charge must equal zero.
Charge balance!

5. A. Ionic Nomenclature Consider the following:
Does it contain a polyatomic ion?
-ide, 2 elements  no
-ate, -ite, 3+ elements  yes
Does it contain a Roman numeral?
Check its location on the periodic table– Roman #’s are required for metals not in Groups 1 or 2 (s-block) or Ag, Zn, Al.
No numerical prefixes!

6. Valence Electrons & Stability
Main Group Ion Charges 1+ 2+ 3+ 4± 3- 2- 1-

7. A. Ionic Formula Review potassium chloride magnesium nitrate
copper(II) chloride K+
Cl-
 KCl
Mg2+
NO3-
 Mg(NO3)2
Cu2+
Cl-
 CuCl2

8. A. Ionic Nomenclature Review
Name each compound:
NaBr
Na2CO3
FeCl3
sodium
bromide
sodium
carbonate
iron
(III)
chloride

9. B. Molecular Nomenclature
Prefix System (binary compounds)
Name first element. Name second element.
2. Add prefixes to indicate # of atoms. Omit mono- prefix on first element.
3. Change the ending of the final element to -ide.

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

11. B. Molecular Nomenclature
CCl4
N2O
SF6
carbon
tetrachloride
dinitrogen
monoxide
sulfur
hexafluoride

12. B. Practice! Give the subscripts
arsenic trichloride
dinitrogen pentoxide
tetraphosphorus decoxide
As1Cl3
N2O5
P4O10

13. B. Molecular Nomenclature
Remember the Seven Diatomic Elements!
Br2 I2 N2 Cl2 H2 O2 F2 H N O F Cl Br I

14. C. ACIDS! Acids Compounds that release H+ in water.
Formulas generally begin with ‘H’.
Examples:
HCl – hydrochloric acid
HNO3 – nitric acid
H2SO4 – sulfuric acid

15. We are learning two types of acid:
C. Acid Nomenclature
We are learning two types of acid:
Binary acids (only two elements)
HBr
Ternary acids (three or more elements)
H2SO4

16. Binary acids (only two elements)
C. Acid Nomenclature
Binary acids (only two elements)
hydro____ic acid
HBr
 hydrobromic acid
H2Se
 hydroselenic acid

17. C. Acid Nomenclature Ternary acids or oxoacids (three elements)
Are formed from polyatomic ions.
“ate” ions make “ic” acids
“ite” ions make “ous” acids
H2CO3
CO32- =
carbonate ion
 carbonic acid
H2SO3
SO32- =
sulfite ion
 sulfurous acid

18. C. Acid Nomenclature
(based on a
polyatomic ion)

19. C. Acid Nomenclature (monatomic ion ending) (binary acid)
(polyatomic ion ending)
(ternary acid)
(polyatomic ion ending)
(ternary acid)

20. C. Acid Nomenclature Practice
Name the following acids:
H3PO4
(a) hydrophosphic acid (b) hydrophosphorous acid
(c) phosphoric acid (d) phosphorous acid
HNO2
(a) hydronitric acid (b) hydronitrous acid (c) nitric acid (d) nitrous acid HF
(a) hydrofluoric acid (b) hydrofluorous acid
(c) fluoric acid (d) fluorous acid
H3PO4
(a) hydrophosphic acid (b) hydrophosphorous acid
(c) phosphoric acid (d) phosphorous acid
HNO2
(a) hydronitric acid (b) hydronitrous acid (c) nitric acid (d) nitrous acid HF
(a) hydrofluoric acid (b) hydrofluorous acid
(c) fluoric acid (d) fluorous acid

21. C. Writing Acid FORMULAS
The two kinds of acids have different rules for writing formulas.
Binary
Identify them:
The name begins with “hydro”

22. C. Acid FORMULAS Ternary
The two kinds of acids have different rules for their formulas.
Ternary
Identify them:
The name does not begin with “hydro”

23. We call this “charge balancing” the compound.
C. Acid FORMULAS
Two rules are true for both types of acid:
The formula begins with the element H.
You need to add subscripts to make the overall charge of the compound = 0
We call this “charge balancing” the compound.

24. C. Acid FORMULAS hydrofluoric acid H & F H1+ F1- H1F1
Must be binary because its name begins with “hydro”
Two elements:
Find their ion charges from periodic table:
Add subscripts to charge balance the compound.
H & F
H1+ F1-
H1F1
(Balance by finding the LCM, just like with ionic compounds.)

25. C. Acid FORMULA practice
Write a formula for:
hydronitric acid
How many elements?
What are they?
What are the subscripts on the formula?
2 elements (binary)
hydrogen & nitrogen
H1+ N3-
 H3N1

26. C. Acid FORMULAS nitric acid Nitric acid is ternary. NO3- HNO3
Must NOT be binary because its name does not begin with “hydro.”
Nitric acid is ternary.
Ternary acids are based on polyatomic ions:
NO3-
HNO3
(Remember, these are listed on the back of your periodic table.)

27. C. Acid FORMULAS
To write a ternary acid, you must identify the polyatomic ion it contains.
Ternary Acids have two possible endings:
“-ic acid”
Is based on an “-ate” polyatomic ion.
(sulfate, nitrate, carbonate, etc)

28. C. Acid FORMULAS
To write a ternary acid, you must identify the polyatomic ion it contains.
Ternary Acids have two possible endings:
“-ic acid”
Is based on an “-ate” polyatomic ion.
(sulfate, nitrate, carbonate, etc)
“-ous acid”
Is based on an “-ite” polyatomic ion.
(sulfite, hypochlorite, nitrite, etc.)

29. C. Acid FORMULA practice
sulfuric acid
How many elements?
Which polyatomic ion?
From the chart:
Add H1+ to the front, then charge balance:
ternary = 3 elements
The acid contains a polyatomic ion!
An “-ic acid”
comes from “-ate” ion
sulfur + “-ate”  sulfate ion
sulfate ion = SO42-
H1+ SO42-
 H2SO4

30. C. Acid FORMULA practice
Oxalic Acid
(a) binary or (b) ternary
How many hydrogens does it contain?
Hypochlorous acid
How many hydrogens
does it contain?
(b) ternary (no hydro)
oxalate = C2O42- 2
 H2C2O4
(b) ternary (no hydro)
hypochlorite = ClO-
 HClO 1