1. Chemical Nomenclature
How to write and say chemical formulas
General Chemistry 10-11

2. Elements Elements are said with just their name
Mg = magnesium
Ca = calcium
Some elements never exist by themselves
These are called diatomic molecules
There are seven of them and they make a seven on the periodic table

3. The Diatomic Molecules
These would still be said by their elemental name but would be written with a subscript of 2 N2 O2 F2
Cl2
Br2 I2 H2

4. Compounds
Most elements are not found separately but combined in a compound with something else
The reason for this is the octet rule
We want 8…eight is great!

5. Octet Rule
Noble gases are what all elements aspire to be like electronically
These elements have 8 electrons in highest energy level

6. Ionic Bond
Atoms will either give up or take electrons to get to have eight in their highest energy level
Na Cl

7. Hey, can you help me out and gimme an electron?
Na Cl

8. Why certainly, I have one I don’t want anyway.
Na Cl

9. Give up/take away electrons
Na Cl

10. Charges
Sodium now has a +1 charge since it has lost an electron
Chlorine a minus charge since it gained an electron
Na Cl + -

11. Ionic Bond - NaCl 4Eva + Na Cl
Opposites attract, so a bond is formed between the two of them.
Na Cl + -
(or until water breaks us apart)
NaCl 4Eva

12. Ionic Compound The combination of Na+ and Cl- form the compound NaCl
An ionic compound will always consist of:
A metal ion (also called a cation, the + one)
A non-metal ion (also called an anion, the - one)
CATION ALWAYS COMES BEFORE THE ANION; both in the name and the formula

13. Naming Ionic Compounds
When naming ionic compounds
Just say the name of the metal
For the non-metal, drop the ending and add -ide to it.
NaCl = sodium chloride

14. Practice Problem #1 Name the following ionic compounds ZnO Zinc oxide
LiBr
Mg3N2
BaS
K3P
Zinc oxide
Lithium bromide
Magnesium nitride
Barium sulfide
Potassium phosphide

15. Determining metal and non-metal charge
Where are the metals on the periodic table?
Metals always have what charge?
Where are the nonmetals?
Nonmetals always have what charge?
We’ll see the charges of the different families on the following slide.

16. Using the periodic Table to find an ion’s charge+1 +2 -1 -2 -3 -4
We’re going to forget all about the middle of the table for now.

17. Combining metals and nonmetals
When combining a metal and a non-metal, the overall charge of the compound must be zero.
You must balance out the overall charge!

18. Combining metals and nonmetals
Take for instance calcium nitride.
What is the charge of the calcium ion?
What is the charge of the nitride ion?

19. Combining metals and nonmetals
Ca+2 means each calcium ion has 2 more electrons than it wants
N-3 means each nitride ion needs 3 more electrons. Ca N

20. Hey buddy, can you spare 3 electrons?

21. Sorry, I only have two. Ca N

22. Maybe I can help! N Ca

23. Ca N

24. HEY, What about me? Ca +2 N -3
YEAH!
YEAH!

25. Hang loose, man. I’ll get one of my buddies.Ca +2 N -3

26. YO, YO, YO. Your hero has arrived.N Ca +2 N -3

27. N -3 -1
YEAH! +2 Ca +2 Ca

28. I still need two more. N -3 -1 +2 Ca +2 Ca

29. I need to get rid of two more.Ca
I need to get rid of two more. N -3 -1 +2 Ca +2 Ca

30. Ca N -3 -1 +2 Ca +2 Ca

31. The ions found they were still attracted to one another due to their opposing charges. And they all lived happily ever after. Ca +2 N -3

32. Now is the time to learn “SWITCHY SWITCHY” and reduce!
Practice Problem #2
Give the formulas for the following compounds
Beryllium iodide
Potassium sulfide
Magnesium oxide
Strontium fluoride
BeI2
K2S
MgO
SrF2
Now is the time to learn “SWITCHY SWITCHY” and reduce!

33. Transition Metals The middle block of elements All cations
Most can take on multiple charges
Some Exceptions
Zn = +2
Ag = +1

34. Transition metal compounds
In order to tell what charge a transition metal has, put its charge in parenthesis
For instance Copper (II) Oxide means…
the copper ion here has a +2 charge
For instance Copper (I) Oxide means…
the copper ion here has a +1 charge
What are the formulas of these two ionic compounds?

35. Practice Problem #3 Give the formula of the following compounds:
Tungsten (IV) Chloride
Gold (III) phosphide
Tin (II) fluoride
Zinc sulfide
WCl4
AuP
SnF2
ZnS

36. Polyatomic Ions
Sometimes, atoms get together but can’t quite get to an overall zero charge.
This is where they become a polyatomic ion
They’re still a charged particle (mostly anions) so they can combine with an opposing charged ion to produce a compound
Naming is easy, we just say the name of the polyatomic ion
With
polyatomic ions
we don’t have to
change the
ending

37. Ionic Compounds involving a polyatomic ionH [
1N = -5
4H = -4
Total -9
One extra electon

38. Ionic Compounds involving a polyatomic ionH [ Cl

39. Ionic Compounds involving a polyatomic ionH [ +1 Cl [ -1
Opposites attract

40. NH Cl = Ammonium Chloride 4 Another happy compound formed![ +1 Cl [ -1
NH Cl = Ammonium Chloride 4
Another happy compound formed!

41. Practice Problem #4 Name the following compounds Ammonium sulfide
Calcium sulfate
Barium nitrate
Potassium carbonate
Magnesium phosphate
Name the following compounds
(NH4)2S
CaSO4
Ba(NO3)2
K2CO3
Mg3(PO4)2

42. Practice Problem #5 Write formulas for the following compounds
Aluminum nitrate
Beryllium sulfate
Calcium phosphite
Ammonium sulfite
Strontium nitrite
Al(NO3)3
BeSO4
Ca3(PO3)2
(NH4)2SO3
Sr(NO2)2

43. Covalent Bonds Cl Cl Compounds formed by two non-metals
More of a sharing of electrons rather than a give-take relationship Cl Cl

44. Can you spare an electron?Cl Cl

45. JINX! Cl Cl

46. Why don’t you share an electron? You know sharing is caring!Cl Cl

47. Valent=valence electrons… therefore, covalent is sharing electrons!
Co=together
Valent=valence electrons… therefore, covalent is sharing electrons!
Shared pair
of electrons =
Covalent Bond Cl Cl

48. Naming Covalent Bonds Prefixes on back of periodic table
If there is only one of the first element, no prefix. Otherwise attach prefix
Second always gets prefix and -ide ending (just like ionic anion)
Name these
ICl5
N2O

49. Practice Problem #7 Name the following covalent compounds
Carbon dioxide
Phosphorous pentachloride
Carbon monoxide
Triphosphorous hexaflouride
Name the following covalent compounds
CO2
PCl5 CO
P3F6

50. Practice Problem #8 Give the formula for the following compounds
Sodium acetate
Nickel (II) chloride
Carbon dioxide
Sulfur trioxide
Triphosphorous tetrachloride
NaC2H3O2
NiCl2
CO2
SO3
P3Cl4

51. One more thing…
If the ionic compound begins with a hydrogen ion, it’s an acid
We name binary acids by adding hydro as a prefix to the root of the anion and add ic, then add the word acid
Name these:
HCl HI HF
HBr

52. Acids involving polyatomic anions
These are even easier,
They’ll always involve oxygen
If an -ate ion, use root of polyatomic and add -ic
If an -ite ion, use root of polyatomic and add -ous
Then just add the word acid
If I ATE it I would say IC!

53. Practice Problem #6 Write the formulas for these acids H2SO4
H2CO3
HNO3
HNO2
H3PO4
H3PO3
Write the formulas for these acids
Sulfuric acid
Sulfurous acid
Carbonic acid
Nitric acid
Nitrous acid
Phosphoric acid
Phosphorous acid

54. THAT’S
ALL
FOLKS!