1. Fancy word for naming and writing formulas
Nomenclature
Fancy word for naming and writing formulas

2. Video

3. Video

4. Where do the element symbols come from?
Most come from the first letter or the first two letters of their full name
C, O, Al, Ar, Be, Ba etc etc
Some from the first letter and another letter in their name
Cd, Cr, Cl, Mg
Some from their Latin names
Sb, Au, Fe, Pb
But for all of them, the first letter is always capitalized and the second is always lower case.

5. Ionic Compounds Formed by metals and non-metals put together
Metals are found on the left of the staircase
They all have a positive charge when they are ionized
Row 1 = +1, Row 2 = +2, Row 13 = +3
Non-metals are found to the right of the staircase
They all have a negative charge when they are ionized
Row , Row , Row
The semi-metals or metalloids are found beside the staircase and can act as metals or non-metals
Great for semi-conductors (microchips)

6. Some terms to know Cation Anion Monatomic – Made up of one atom
Positively charged ion (metals when they lose electrons)
Anion
Negatively charged ion (non-metals when they gain electrons)
Monatomic – Made up of one atom
Ne, H, O, Cl-, H+
Diatomic – Made up of two atoms
O2, NO, CO
Triatomic – Made up of three atoms
NO2, CO2, H2O
Polyatomic – Made up of many atoms
O2, NO, NO2, H3PO4

7. Rules for writing chemical formulas of non-multivalent ionic compounds
Metals are always written first, non-metals second
Write the charge of each ion as superscripts found from the periodic table
Balance the charges by finding the LCM of the charges
Use subscripts to show how many of each ion you need to make it balance
Reduce if you can
The final product should be neutral. Positive charge should equal negative charge. You can remove the superscripts.
Remove any 1’s as it is assumed in the final formula

8. Example - 1 Sodium chloride Potassium oxide Calcium phosphide
Hydrogen carbide
Silver sulphide

9. Rules for writing chemical formulas of multivalent ionic compounds
Same as writing for non-multivalents.
Only difference is the metal which can have multiple charges will have a roman numeral beside the name to show its charge.
+1 = I
+2 = II
+3 = III
+4 = IV
+5 = V
…..

10. Example - 2 Tin (IV) sulphide Iron (II) phosphide Copper (I) nitride
Iron (III) oxide
Chromium (III) chloride

11. Rules for writing chemical formulas of polyatomic ionic compounds
Write as you would naming non-polyatomic ionics
Polyatomic ions are groups of atoms that stay together and carry a charge. They act like a single ion. Treat them like a single ion
NH4+
SO43-
When you write the formula for polyatomics, they are written as one unit. If there are more than one of the polyatomic ion, you put parentheses around it and state how many.
(NH4)3 means there are 3 NH4‘s

12. Example - 3 Lithium phosphate Calcium sulphate Iron (II) nitrate
Ammonium oxide
Mercury (I) chloride

13. Note! Ammonium which is NH4+ is different from ammonia which is NH3.
One is an ion, the other is a molecule.
Mercury (I) is Hg22+ because it acts as one single unit like a polyatomic. It is mercury (I) because there are two mercury atoms and the total charge is 2+ so each one is 1+.

14. Rules for naming chemicals of non-multivalent ionic compounds
Use the periodic table to find the element symbol
Metal first, non-metal second
The non-metal (anion) drops all its syllables except for the first and ends in IDE
Chloride -> chloride
Oxygen -> oxide
Hydrogen -> hydride
Only the metalloids keep the first two syllables and then ends in IDE
The metal (cation) stays the same in terms of name
DO NOT CAPITALLIZE THE NAME! Only at the start of sentences!

15. Example - 4
NaCl
CaCl2
CaO
MgCl2
Li2O

16. Rules for naming chemicals of multivalent ionic compounds
Similar to naming non-multivalents
Look at the charge of the non-metal from the periodic table. It never changes!
Multiply the charge with the number of anions.
This is the total negative charge!
Remember, an ionic compound is neutral so the positive charge must be the opposite positive charge.
Divide the positive charge by the number of cations. This is the charge of each cation.
This is your roman numeral
Write the full name with the roman numeral between the cation and anion in parentheses

17. Example - 5
Fe2S3
CuCl
VCl3
CrI3
SnO2

18. Rules for naming chemicals of polyatomic ionic compounds
Similar to the previous two
Just the polyatomic ion does not change ending. Keep it the same!
Sulphate (SO42-) is sulphate, not sulphide (S2-)

19. Example - 6
Ag3PO4
Al2 (SO4)3
(NH4)2 S
NH4HCO3
Mg(HSO3)2

20. Common names H2O = water NH3 = ammonia CH3COOH = vinegar CaO = lime
NaClO = bleach

21. Hydrates
Hydrates are ionic compounds that have water molecules attached to it
Even if it is dry!
It is attached as individual molecules after it is dried from an aqueous solution

22. Rules for writing chemical formulas of hydrates
Write the chemical formula of the ionic as the same as before.
To write the chemical formulas of hydrates, you have to know how many hydrates there are. This is represented by the prefix in front of the word “hydrate”
Mono – 1
Hexa – 6
Di – 2
Hepta – 7
Tri – 3
Octa – 8
Tetra – 4
Nona – 9
Penta - 5
Deca - 10

23. Rules for writing chemical formulas of hydrates
If the name is pentahydrate, you have to write it as 5H2O to state there are 5 water molecules attached.
Octahydrate = 8H2O
You separate the ionic compound from the hydrate with a dot ● (not so big though)

24. Example - 7 Sodium chloride pentahydrate
Iron (III) sulphide hexahydrate
Calcium oxide monohydrate
Zinc acetate dihydrate
Calcium nitrate tetrahydrate

25. Rules for naming chemicals of hydrates
Same as naming ionic compounds
The coefficient in front of the H2O is how many hydrates there are.
You name the ionic compound and then put the prefix for the number of water molecules and then “hydrate”

26. Example - 8 FeBr3 ● 6H2O CoF2 ● 4H2O Na2SO4 ● 10H2O Na2S ● 9H2O
Al2O3 ● 3H2O

27. Covalent Compounds
Two or more non-metals put together. No metals involved
Different naming scheme than ionic
Ionic means electrons is the transferring of electrons to the non-metal
Covalent is the sharing of electrons between the non-metals (not equal though)
We use prefixes to tell how many of each elements there are

28. Rules for writing chemical formulas of covalent compounds
The prefixes are the same as hydrates
So you will know how many of each element you have based on the prefix.
How many element you have will be turned into the subscript beside the element.
If an element has no prefix, it is assumed as 1.
Mono – 1
Hexa – 6
Di – 2
Hepta – 7
Tri – 3
Octa – 8
Tetra – 4
Nona – 9
Penta - 5
Deca - 10

29. Example - 9 Carbon dioxide Carbon monoxide Dinitrogen trioxide
Sulphur hexafluoride
Dihydrogen monoxide!!! (Very deadly)

30. Rules for naming of covalent compounds
You keep the first elements name the same, like you do in the metal of ionics
You change the 2nd element’s ending to IDE like non-metals
You use prefixes to tell how many of each element is present.
You do not need to write MONO if the first element is only 1 as it is assumed.

31. Example - 10 CO
CO2
P2O3
S4 N2
N2O3

32. Naming Acids All acids start with the element H (hydrogen).
That means even water is an “acid” (more of this in grade 12)
All acids are assumed dissolved in water so they are aqueous solutions
All are assumed to be ionic where the hydrogen acts as the metal
But change the hydrogen to “hydro” if the non-metal is not a polyatomic

33. Naming Acids The non-metal name changes If the non-metal name ends in
IDE turns into IC (hydrogen chloride -> hydrochloric acid)
ATE turns into IC but you drop the hydro (hydrogen sulphate -> sulphuric acid)
ITE turns into OUS and drop the hydro (hydrogen sulphite -> sulphurous acid)

34. Practice - 1 Page 71 - #4 Page 72 - #5 Page 73 - #6-7 Page 74 - #8-9