1. Post Lab Discussion
(Exp. 2A)

2. Heating Curve of Water
gas
boiling point
liquid
melting point
solid

3. Heating Curve of Mixture of Water and Alcohol

4. Conclusion Pure substances change phases at constant temperature.
Melting points and boiling points can be used to determine the identity of a substance and whether or not a substance is pure.

5. Periodic Table: NEED TO KNOW: Symbols & names 1-36
State of elements at room temps.
Periods vs. groups (rows) (columns)
Metals vs. non-Metals (lose e-) (gain e-)
Atomic Number = # of protons
Atomic Mass (Mass #) = # of protons + # of neutrons
Atomic Radius (page 319 in textbook)
Characteristic charges of groups (alkali metals = 1+)
Groups: Alkali Metals, Alkaline Earth Metals, Transition Metals, Halogens, Noble Gases

6. Ionic Compounds
(metal + non-metal)
Chemistry 11 Unit 3

7. Lowest common multiple of 2 and 3 is 6
7. Writing Formulas - Ionic Compounds
In an ionic compound, positive charges must balance the negative charges.
e.g.: What is the formula for magnesium phosphide?
Magnesium is Mg2+
Phosphorous is P3-
Lowest common multiple of 2 and 3 is 6
3 Mg2+ ions and 2 P3– ions
Mg3P2

8. Mg3P2 CaO Mg2+ P3- Mg2+ P3- Mg2+ 6+ 6-
e.g.: What is the formula for calcium oxide?
Calcium is Ca2+
Oxygen is O2-
1 Ca2+ ion and 1 O2– ion
CaO
(remember, the subscript 1 is never written)

9. Only use if you understand that the + and - charges must balance!
Short-cut
Only use if you understand that the + and - charges must balance!
Magnesium oxide
1. Write both symbols (+ion first) with ion charge 2+ 2- Mg O
2. Criss-cross the charges and write them as subscripts
Mg O 2 2
MgO
3. Reduce if possible
(remember, the subscript 1 is never written)

10. Sometimes, metal ions have more than one combining capacity
e.g.
Cu2+
Cu1+
Fe3+
Fe2+
The name of the compound will include a roman numeral that tells you which combining capacity to use 1+ I 5+ V 2+ II 6+ VI 3+
III 7+
VII 4+ IV
e.g.
Iron II oxide
Iron III oxide 2+ 2- 3+ 2- Fe O Fe O
FeO
Fe2O3

11. 8. Naming Ionic Compounds
1. Write the name of the metal first.
2. Write the name of the non-metal second,
and change the ending to “-ide”
3. ONLY IF THE METAL HAS 2 OR MORE COMBINING CAPACITIES,
Include a roman numeral to indicate which one it is.
e.g.
NaCl
Sodium
chloride
MgF2
Magnesium
fluoride 1+ Cu
CuCl2
copper has 2 ions: 2+ Cu
which one is it?

12. 9. Predicting Ion Charges
from Formulas
To find out which copper ion it is, look at the charge on the anion and balance the charges in reverse.
CuCl2 2+ 1- Cu Cl
from periodic table 1- Cl 2-
Therefore it is copper II chloride
CuCl therefore must be copper I chloride

13. Practice: Name and write the formulas for: a) chlorine & aluminum
Aluminum chloride; AlCl3
b) bromine & sodium
Sodium bromide; NaBr
c) magnesium & sulphur
Magnesium sulphide; MgS
d) calcium & nitrogen
Calcium nitride; Ca3N2
e) fluorine & beryllium
Beryllium fluoride; BeF2

14. More Practice:
Name and determine the charge on each of the transition metals in the following compounds:
a) CuO
Copper II oxide; Cu2+
b) FeAs
Iron III arsenide; Fe3+
c) CrBr3
Chromium III bromide; Cr3+
d) Cu2O
Copper I oxide; Cu+
e) FeCl3
Iron III chloride; Fe3+
f) CrCl2
Chromium II chloride; Cr2+

15. 10. Writing Formulas: Polyatomic Ions
Some groups of atoms act as individual ions
Ion Charge
e.g.
SO4-2
Sulphate ion -2
OH-1
Hydroxide ion -1
PO4-3
Phosphate ion -3
When writing formulas and naming, pretend the polyatomic ion is just one atom and follow the rules as usual. +1 -3
e.g. K
PO4
Potassium phosphate
K3PO4
Don’t change the endings of polyatomic ions

16. More Examples! Al SO4 Al2(SO4)3 Cu SO4 CuSO4 Aluminum sulphate+3 -2 Al
SO4
Al2(SO4)3
Aluminum sulphate
Put brackets around the SO4 to indicate 3 sulphate ions, not 43 oxygen atoms +2 -2 Cu
SO4
CuSO4
Copper (II) sulphate
Don’t forget the roman numeral since copper has more than one combining capacity
See the back of your periodic table for the names and formulas of important polyatomic ions.

17. 11. Naming Hydrates CuSO4 • 5H2O FeSO4 • 6H2O
Hydrates are ionic compounds with water molecules attached
e.g.
CuSO4 • 5H2O
- each copper II sulphate is attached to 5 water molecules
Copper II sulphate pentahydrate
e.g.
Iron II sulphate hexahydrate
FeSO4 • 6H2O

18. 12. Names of Common Acids HCl Hydrochloric acid HF Hydrofluoric acid
HNO3
Nitric acid
HNO2
Nitrous acid
H2SO4
Sulphuric acid

19. Hydro, -IC or -OUS? If the anion name ends in ide:
the acid name starts with hydro and ends with ic acid.
eg: HCl:
Cl- is chloride. So HCl is hydrochloric acid.
If the anion name ends in ate:
the acid name ends with ic acid; no hydro prefix.
eg: HNO3:
NO3- is nitrate. So HNO3 is nitric acid.
If the anion name ends in ite:
the acid name ends with ous acid; no hydro prefix.
eg: HNO2:
NO2- is nitrite. So HNO2 is nitrous acid.

20. 13. Binary Compounds of Non-Metals
Compounds composed of two non-metal elements
More metallic name comes first,
then use a prefix to show the number of atoms of the less metallic element, followed by the –ide ending
Name the following compounds:
a) CO2
Carbon dioxide
b) CO
Carbon monoxide
c) PCl3
Phosphorous trichloride
d) CCl4
Carbon tetrachloride
e) PF5
Phosphorous pentafluoride
f) H2O
Dihydrogen monoxide
a) S2O4
Disulphur tetraoxide

21. Assignment Homework: “Naming & Formula I” Worksheet
Quiz on Periodic Table next class