1. Write the electron configuration for K and Br.
Circle the Valence Electrons

2. A John Modica Production
NOMENCLATURE
OF IONIC
COMPOUNDS
A John Modica Production

3. Ionic Compounds Mg O Because electrons are negatively charged…
an atom becomes positively or negatively charged as it loses or gains an electron, respectively.
Any atom or group of atoms with a net charge (whether positive or negative) is called an ion.
A positively charged ion is a cation
A negatively charged ion is an anion. +2
positively t Mg
negatively n n O -2

4. IONIC COMPOUNDS Metal Non-metal Oxygen-8 Magnesium-12
Compounds are two or more elements that are held together by opposite charge attraction.
IONIC COMPOUNDS
Oxygen-8
8 (+) 10 (-) -2 Charge
12 (+) 10 (-) +2 Charge
Magnesium-12
Metal
Non-metal

5. Ionic Formulas
Ions combine in small, whole number proportions so that the sum of oxidation numbers will be zero!
Electrons are transferred from the metal to the non-metal
The metal become a cation (+ charge)
Why?
The non-metal becomes an anion (- charge)

6. Metals Non-metals Metals combine with non-metals
Metals loose electrons to non-metals
They attract because their charges are opposite.
Metals
Non-metals

7. Ionic Formulas These are called Binary Compounds
The prefix “bi” meaning two
Two elements bonding to form a compound
The metal ion ALWAYS goes first, followed by the non-metal ion

8. So what does this look like?Mg +2 O -2
Magnesium Oxide

9. So what does this look like?Al +3 S -2 2 3
Aluminum Sulfide

10. So what does this look like?Na +1 Cl -1
A.k.a. Table Salt
Sodium Chloride

11. Your Turn! Na +1 F -1 Ba +2 Cl -1 Al +3 Br -1 K +1 O -2 +1 -2 Li S

12. Your Turn! Na F Ba Cl 2 Al Br 3 K O Li S 2 2

13. Now let’s Kick it up a notch!

14. Polyatomic Ions A group of 2 or more atoms that act as a single unit
When a metal and a polyatomic ion bond this forms a tertiary compound
3 or more elements reacting to form a compound

15. POLYATOMIC IONS Polyatomic ions are mostly made of two non-metals.
Ions with -1 charge
perbromate BrO4-1
bromate BrO3-1
bromite BrO2-1
hypobromite BrO-1
perchlorate ClO4-1
chlorate ClO3-1
chlorite ClO2-1
hypochlorite ClO-1
periodate IO4-1
iodate IO3-1
iodite IO2-1
hypoiodite IO-1
nitrate NO3-1
nitrite NO2-1
hydroxide OH-1
cyanide CN-1
acetate C2H3O2-1
Permanganate MnO4-1
bicarbonate HCO3-1
Ions with a -2 Charge
carbonate CO3-2
sulfate SO4-2
sulfite SO3-2
chromate CrO4-2
dichromate Cr2O7-2
oxalate C2O4-2
Ions with a -3 Charge
phosphate PO4-3
phosphite PO3-3
arsenate AsO4-3
Ions with +1 charge
ammonium ion NH4+1
Yes, I can read your minds…

16. No you do not have to memorize these polyatomic ions
No you do not have to memorize these polyatomic ions. You will receive a chart with these
Obviously!!!

17. Na PO Tertiary Compounds
Polyatomics ions react as one unit, so you treat them the same when writing formulas
Use the criss-cross method Na PO +1 -3 4 3
Sodium Phosphate

18. Tertiary Compounds Mg
( ) SO +2 -2 4
Magnesium Sulfate

19. Al NO ( ) Yeah, I’ve got nothing. Tertiary Compounds Aluminum Nitrite+3
( ) -2 2 2 3
Aluminum Nitrite
Yeah, I’ve got nothing.

20. Na SO Ba ClO Al PO K NO Li SO Your Turn! +1 -2 +2 -1 4 2 +3 -3 4 +1 -1

21. Your Turn! Na
( ) SO Ba
ClO 2 4 2 2 Al
( ) PO 4 K NO Li SO 2 2 3

22. How do we know the charge of the elements?
Glad you asked!

23. Click on element to see its oxidation number(s)
Oxidation Numbers (most common) -3 -2 +2 +1 -1 +3 -4 +1 +2 +2 +3 +2 +4 1A 7A 8A H H He 2A 3A 4A 5A 6A Li Be B C N O F Ne
Click on element to see its oxidation number(s) Na Mg Al Si P S Cl Ar K Ca Sc Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br Kr Rb Sr Y Zr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te I Xe Ce Ba La Hf Ta W Re Os Ir Pt Au Hg Tl Pb Bi Po At Rn Fr Ra Ac Rf Db Sg Rh Hs Mt Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb Lu
return Th Pa U Np Pu Am Cm Bk Cf Es Fm Md No Lr