1. Naming Inorganic Compounds Lesson 1
UNIT IV
Naming Inorganic Compounds
Lesson 1

2. INORGANIC NOMENCLATURE
Nomenclature refers to ‘naming’
Inorganic = Non Carbon compounds & Elements.
Organic chemistry= study of carbon compounds.
The periodic table organizes the elements by vertical columns (___________) and horizontal rows (______________).
The elements are arranged depending on the chemical and physical properties of elements in repeated patterns and increasing atomic masses.
Groups/familes- they tell you about charges
Horizontal= periods.

3. IV.1 THE CHEMICAL ELEMENTS
Element symbol: The first letter is always in upper case and the second letter (if present) is always lower case.
Ex: Sodium (Na), Nitrogen (N)
3 Major classifications: pg. 67
Non-Metals
Metals
Metalloids or Semi Metals
Clustered elements around the “staircase” between metals and non-metals.

4. Periodic table
.pdf

5. IV.2 NAMING INORGANIC COMPOUNDS
METALS:
Found on left side in periodic table
Form _________ ions
Cation: an ion with a positive charge
NON-METALS:
Found on right side in periodic table
form __________ ions
(H is generally an exception)
Anion: an ion with a negative charge

6. Naming inorganic compounds
Some other definitions
Monoatomic
Diatomic
Triatomic
Polyatomic

7. NAMING MONATOMIC METAL IONS Simply use the name of the metal and add the word “ion” Element Name Ion Name Sodium Metal(Na) Aluminum (Al) Write the names of the following ions: Ca+2 Ag+

8. NAMING MONATOMIC METAL IONS
If a metal has more than one possible charge, the charge has to be indicated by a Roman numeral, in parenthesis, immediately following the name. Ex: Fe+3 Fe+2 Roman numerals are: I 1 V 5 IX 9 II 2 VI 6 X 10 III 3 VII 7 IV 4 VIII 8

9. NAMING MONATOMIC METAL IONS
Write the formula of the following ions to show their charges:
Uranium (VI) ion = __________
Iron (II) ion = __________
Nickel (II) ion = __________

10. NAMING MONATOMIC NON-METAL IONS
Take off the original ending and add an “ide” ending.
Element Name Ion Name
Florine (F) 
  Sulphur (S) 
Write the names of the following ions:
a) Br- = __________________________
b) Cl- = __________________________
c) I- = __________________________
d) O-2 = __________________________
e) N-3 = __________________________

11. Naming Polyatomic Ions:
Rules for naming are more complicated (we won’t learn them). But we will need to KNOW some common polyatomic ions (names, formula, charge).
* Know table on page 69.

12. How to write the formula and how to write the name of Ionic Compounds

13. How to write the formula of ionic compounds
An ionic compound
A compound made up of ions ( usually a metal + non-metal )
The ions have charges but the compound is a neutral molecule.
remember in ionic compounds , one ion loses and one ion gains electrons).
The chemical name of an ionic compound always gives the positive ion (cation) first and the negative ion (anion) second.
Ex: Sodium Chloride

14. 3 simple rules

15. Calcium Chloride & Magnesium Oxide

16. Writing formula of Ionic compounds

17. More examples Potassium oxide: Tin (IV) oxide: Calcium phosphide
Iron (II) sulphate:
We do not change the endings of polyatomic ions because they already have special endings that end in “ate” or “ite”

18. How to Write the Name of an IONIC COMPOUND Check your periodic table to see if the positive ion has more than one ion charge.

19. How to Write the Name of an IONIC COMPOUND
A) If the first ion has only one possible ion charge:
write the names of the ions(not elements) one after the other
omit the word “ion”
ZnCl2
Ag2SO4

20. B) If the first ion has more than one possible charge:

21. B) If the first ion has more than one possible charge:
“De-swap and de-drop” the subscripts (to find out the real charge)
check the charge on negative ion (if it is not as what it should be, you probably need to double or triple it)
write the charge of the positive ion with roman numerals
Write the charge of the negative ion with “ide”

22. Try these on your own
FeS
Fe2(SO4)3

23. Note: you must memorize the “common name” of 2 compounds:
H2O = water
NH3 = ammonia
be careful of Ammonium NH4+1

24. The # of water molecules is shown after a centered dot
Naming Hydrates
Hydrates are ionic compounds that include water molecules in their crystal structures.
Naming hydrates is pretty straightforward and relies on using prefixes to tell how many water molecules are attached.
The # of water molecules is shown after a centered dot
Example of a hydrate: CuSO4·5H2O
see table on page 72 for prefixes

25. Naming Hydrates
see table of page 72 for prefixes CuSO4.5H2O= copper (II) sulphate pentahydrate Ca(NO3)2·4H2O=

26. Practice Time! Self-test on page66 All of it Ex#1 on page 68
Page 73 Ex#6: a, c, d, f, g, I
Page 73 Ex#7: a, b, c, d, e, f

27. How to write the formula and how to write the name of
UNIT IV: LESSON 2
How to write the formula and how to write the name of
Covalent Compounds

28. Naming COVALENT COMPOUNDS Using the Prefix-Naming System
Remember covalent compounds SHARE their electrons ( usually two non-metals together).
Binary Compound: a compound made of two different types of atoms (usually two non-metals)
SO2, Na2S, NaCl
Tertiary Compound: a compound made of three different types of atoms.
H2SO4 KOH KMnO4

29. Naming COVALENT COMPOUNDS Using the Prefix-Naming System
We use the prefix-naming system
1- Each compound name is made of words, each with a suitable prefix
see p. 73

30. Naming COVALENT COMPOUNDS Using the Prefix-Naming System
Prefix-system naming continued
First word is the name of element(not ion) with a prefix to indicate the # of atoms
Second word is the name of the element with an “ide” ending and a prefix to indicate the # of atoms
P2S3 = diphosphorus trisulphide
Exception: if there is only ONE atom of the first element, don’t use the prefix mono.
Ex: CO2 =

31. Try on your own
Examples:
P2S3 =
CO =
BrCl3 =
S2Cl2 =

32. prefix naming system
Basically used when you have two different Non- Metals.
Non-metals are usually found on the right side of the periodic table.
Remember the prefixes.

33. Writing formulas for covalent compounds
Steps:
Write down the symbol for each element
Use the prefix to determine the number of atoms of each element.
Example: dinitrogen tetroxide carbon dioxide
Do NOT reduce !

34. A compound is called an acid when the chemical formula starts with ‘H’
Some Common Acids
A compound is called an acid when the chemical formula starts with ‘H’
ex: HCl, H2SO4
see common acids on p. 74 – KNOW THESE
Practice Questions
Naming - p. 75 # 15 – 65 (odds)
Formulas – p – 125 (odds)

35. Summary Naming First identify if it is ionic or covalent
Ionic compounds
Metal and non-metal
Positive ion first then negative ion
Use roman numerals to indicate the ions with more than one possible charge
For the negative ions(non-metals) change the ending to ide.
Covalent compounds
Non-metal and non-metal
For both, we use the prefix-naming system (mono, di, tri, tetra, etc)
First one, you just write the element’s original name with prefix
You change the second element’s name to “ide” with prefix.
Summary

36. Summary Writing Formulas First identify if it is ionic or covalent
Ionic compounds
Write formula for positive ion first then negative ion
Swap and drop charges as subscripts
Reduce if you need to.
Covalent compounds
Write down the symbol for each element
Use the prefix to determine the number of atoms of each element.
Do NOT reduce !

37. Practice time! Page 74 Ex8 and Ex9. Page 75 writing the names question
( only odd numbers )
15  ( only odds)
Page 76 writing the formulas question
( only even numbers)
90  162 (only evens)