1. Writing and Naming Ionic Formulas
U7D2
Writing and Naming Ionic Formulas

2. U7D2: Writing and Naming Ionic Formula
HW: WS: Formula Writing and Naming Practice
Do Now: 1.HW out for check
2. Is [Cd]-2 the correct ion dot diagram for a
Cadmium ion? Explain.
Today:
Review
Naming Ionic Compounds
Practice!!!
TTL

3. The three steps in forming an ionic bond are:
Metal loses e- to nonmetal becoming a cation.
____________________________________________
Nonmetal gains e- from metal to become an anion.
Cation and anion attract to form an ionic compound.
Period 1

4. Let’s practice

5. More???? Show me where you stand So.. Fist to Five
Fist (not understanding need help)
Five (feel I can teach it)
Show me where you stand

6. Ionic Formula Writing
The number of each type of ion that will form the new compound will depend on the size or magnitude of the charges (oxidation states).
The charges must add up to zero.
Ex. sodium reacts with chlorine,
sodium forms a Na+1 ion & chlorine forms a Cl-1 ion.
Only one of each ion is necessary ->
the charges add up to zero: (+1) + (-1) =0
the formula of the new compound, sodium chloride, is simply NaCl.

7. but what if the charges aren’t equal and opposite?
If sodium reacts with oxygen,
sodium still forms a Na+1 ion but oxygen forms a O-2 ion.
The new compound, sodium oxide, will require 2 Na+1 for every O-2: (+1) + (-2) =0 .
The formula for sodium oxide is Na2O.

8. Remember:
the charges are written as superscripts (Na+1) and the counters in formulas are written as subscripts (Na2O).
Positive ions are written first and negative ions are written second in a formula.
Lazy chemists do not bother to write 1 as counter in a formula. The element's symbol stands for the 1.
Ionic formulas are always written in lowest terms. => an empirical formula.
NaCl and Na2O are binary (2 element) ionic cds.

9. VI. DETERMINING CHARGES:
The oxidation state or number is the charge or apparent charge an atom has in a compound.
To determine the charge, simply look at the Periodic Table for the oxidation states of the element.
For nonmetals it is the FIRST (top) oxidation state ONLY.
For many metals, there is only one possibility for the charge.
Transition metals and those metals close to the “crack”, there are more than one charge.

10. Look up the charges on the following:
Remember to write the charges as superscript +2 +1 -1 -3 +1 -2 +2 +3 +1 +2 +3 -1
Draw a Lewis Dot structure for (p. 3 margin)
FeO and Fe2O3

11. WRITING BINARY FORMULAS
The ions of the elements combine in such a way that the charges have to add up to zero.
Metal or positive ion (cation) is written FIRST
Nonmetal or negative ion(anion)is written SECOND.
The number one,1, is not written in the formula
ex. NaCl.

12. Only the number in the charge for each ion is criss-crossed down and turned into subscripts.
Always check that the formula is in LOWEST terms.
K+1 O-2  K O  K2O1 or K2O
Pb+4 O-2 -> Pb O -> Pb2O4 simplifies to ______
PbO2

13. So… Let’s look at the different combinations we can have…XY XY XY
XY2
XY3

14. X2Y
X3Y
X3Y2
X2Y3
XY2

15. VII. NAMING
The name of the positive ion is followed by the name of the negative ion.
Group 1 & 2 Metals, Metals with ONE charge LISTED: name of the metal ONLY
For nonmetals, the ending of the nonmetal’s name with the ending changed to IDE.

16. Let’s try! Name ionic compounds: NaF: AlN: AgBr: sodium fluoride Na3P:
Li2O:
PbCl2 :
sodium fluoride
Aluminum nitride
Silver bromide
sodium phosphide
Lithium oxide
Lead (II) chloride

17. Practice LiF Lithium fluoride AlCl3 Aluminum chloride SrS
Strontium sulfide
K3N
Potassium nitride
Mg3P2
Magnesium phosphide

18. How about backwards? Name -> formula
Determine the elements involved, their charges & then write the formulas. Look up charges on the PT for the ions.
Na+1
Br-1
NaBr
Ca+2
O-2
CaO
Zn+2
ZnCl2
Cl-1
F-1
Be+2
BeF2
K+1
I-1 KI

19. VIII. DETERMINING CHARGES AND NAMING of TRANSITION ELEMENTS
Transition elements (metals) and some other metals located near the “crack”, can have more than one charge.
Either you will be told which one to use or the charge can be determined from the formula.
To distinguish between the different oxidation states or charges, a roman numeral equal to the charge on the ion is used to name the ion.

20. (Draw the Ion dot diagram for Iron (II) oxide)
Ex, tin comes in two charges, +2 and +4.
Sn+2 is called tin (II) and Sn+4 is called tin (IV).
The formula of tin (II) oxide is SnO and
the formula of tin (IV) oxide is SnO2.
The charge on the tin makes a difference!
If Fe2O3 is iron (III) oxide, what would be the formula for iron (II) oxide? _____
(Draw the Ion dot diagram for
Iron (II) oxide)
FeO

21. ROMAN NUMERALS: +1 ___, +2 ____, +3 ____, +4 ____, +5 ____, +6 _____I II
III IV V VI
Cu2O
Copper (I) oxide
Ni2O3
Nickel (III) sulfide
FeI2
Iron (II) iodide
Au3N
Gold (I) nitride
PbO2
Lead (IV) oxide

22. Going Backwards! Cu+1 F-1 CuF Cu+2 Cl-1 CuCl2 Au+3 O-2 Au2O3 Sn+4 O-2
Pb+2
P-3
Pb3P2

23. Naming the Ionic Compounds from JUST the Formula
Determine if it has a metal with more than 1 charge or not
If yes, then look up the nonmetal’s charge and write the formula with each of the charges.
Ex . FeO Fe+2 O  FeO
Fe+3 O  Fe2O3
a) Since the formula with Fe+2 matches, FeO, then Fe+2 was used.
Use the Roman numeral equal to this charge in the middle of the
compound’s name. Iron (II)
b) Change the name of the non-metal to the ending “ide”. Oxide
Iron (II) Oxide
If no, then just use the metal’s name and change the name of the non-metal to the ending “ide”.
Ex AgCl Ag is the only charge
Silver Chloride
Remember any element in Groups 1 & 2 have ONLY one Charge!! No Roman Numeral ever!!!

24. Silver chloride Iron (III) oxide Lead (IV) oxide Gold(III) iodide
Tin (II) oxide
Chromium(III) Nitride
Sodium phosphide
Copper(II) oxide
Zinc bromide
Calcium nitride

25. IX. POLYATOMIC IONS (PAI)
A. Reference Table E
Groups of atoms bond together by sharing electrons to form ions.
one of the atoms in the group brings along a charge and group of atoms is not neutral
“many atom” ion.

26. Complete this chart using reference table E.
carbonate
NO3 -
acetate
ClO2 -
CrO4 -2
sulfate
SO3 -2
chlorate
PO4 -3
hydroxide

27. What type of charge do most of the PAI have? __________________
Most of these PAI end in _________ or __________
Two important exceptions are the positive ion _________ (ammonium) and the negative ion _________ (hydroxide).
negative
-ate
-ite
NH4 +
OH-

28. B. Writing and Naming Compounds with Polyatomic Ions
Rules:
The formula must be in lowest terms
the charges must add up to zero.
Parenthesis are used around the polyatomic ion when more than one of these ions is necessary in a formula: (NH4)2O.
To name compounds with polyatomic ions, use the name of the polyatomic ion listed on the reference table.
Ex: (NH4)2O is ammonium oxide;
K2CO3 is potassium carbonate.
ternary ionic compounds: K2CO3 and NaClO4
binary ionic compounds: K2O and NaCl

29. Try your hand at these! KNO3 Potassium nitrate Al(ClO3)3
Aluminum chlorate
SrSO4
Strontium sulfate
KNO2
Potassium nitrite
Mg3(PO4)2
Magnesium phosphate

30. Going Backwards! ternary compounds
OH -
NaOH
Ca +1
SO2 -2
CaSO4
K +1
CrO4 -2
K2CrO4
Au +3
CO3 -2
Au2(CO3)3
NH3 +
ClO4 -
NH3ClO4

31. Ok…so how’d we do today Cation:__Ag+1__ Anion:___ (OH)-1____1.
Cation:__Ag+1__ Anion:___ (OH)-1____
Formula:___________________
Name:_____________________ 2.
Cation:____ Fe+3__ Anion:___ (PO4)-3___