1. The Language of Chemistry
Mr. Kinton
Honors Chemistry
Enloe High School

2. Classification of Matter
Matter is anything that occupies space (volume) and has mass
At this point we are only going to focus on pure substances:
Elements
Compounds

4. Elements
A substance that cannot be broken down into simpler substances by chemical means
At the atomic level, only one type of atom is present
Can be found directly on the periodic table
Allotropes: different physical forms of an element
Charcoal, diamond, and graphite are all allotropes of carbon

5. Compounds
A substance composed of 2 or more elements, united chemically in definite proportions
At the atomic level, 2 or more different atoms are present in a compound
Each compound has a fixed chemical ratio
Water- H2O
Hydrogen peroxide- H2O2
Can be either ionic or covalent

6. Compounds Be familiar with the names and formulas of the following:
Methane: CH4
Ammonia: NH3
Isopropyl Alcohol: C3H7OH
Acetone: C3H6O
Sugar: C6H12O6

7. Ions
We have seen in the past how we can have positively and negatively charged ions
An ion is either positive or negative based on whether or not the atom lost or gained an electron (monatomic)
In electron configuration we discussed how to assign the most likely oxidation state
Additionally some ions are formed when a group of atoms has a positive or negative charge (polyatomic)

8. Monatomic Ions
Cations are positively charged ions due to the loss of an electron
All metals will form cations
There are 2 different types of metal cations:
Metals that form only one charge
Metals that form multiple charges

9. Cations with Only 1 Charge
Alkali metals will always form a 1+ cation
Alkaline earth metals will always form a 2+ cation
Silver will always form a 1+ cation
Zinc will always form a 1+ cation
Aluminum will always form a 3+ cation

10. Cations with Only 1 Charge
Potassium ion- K+
Calcium ion- Ca2+
Silver ion- Ag+
Notice in the name the word ion always precedes the name
All of the symbols have a number and a + to indicate the number of electrons lost

11. Cations with Multiple Charges
The transition metals and the remaining representative metals can form cations with different charges
This is because of the presence of the d orbitals
To distinguish between 2 different cations of the same element the charge will be indicated with a Roman numeral in the name

12. Cations with Multiple Charges
Manganese (II) ion- Mn2+
Manganese (V) ion- Mn5+
Titanium (II) ion- Ti2+
Titanium (IV) ion- Ti4+
Again the word ion has to come after the name and the number represents the number of electrons lost

13. Roman Numerals
Number
Roman Numeral 1 I 2 II 3
III 4 IV 5 V 6 VI 7
VII

14. Monatomic Anions
Anions are formed when nonmetals gain additional electrons to fill their octet
All nonmetals will form anions. Hydrogen can form a cation
All anions will form only one charge

15. Monatomic Anions When writing the name change the ending to –ide
Group 7A elements will form 1- charge
Group 6A nonmetals will form a 2- charge
Group 5A nonmetals will form a 3- charge

16. Monatomic Anions Chloride- Cl1- Oxide- O2- Sulfide- S2- Nitride- N3-
Phosphide- P3-

17. Polyatomic Ions
Group of atoms that have an overall positive or negative charge
Oxyanions: polyatomic ions that contain oxygen

18. Oxyanions
Based on the prefixes and suffixes in the name that will help you determine how many oxygens are present
The most common oxyanion will have an –ate ending
The oxyanion with 1 less oxygen than the –ate ending will have an –ite ending
The oxyanion with 1 less oxygen than the –ite ending is given the prefix hypo-
The ion with 1 more oxygen than the –ate ending is given the prefix per-

19. Oxyanions Hypobromite: BrO1- Bromite: BrO21- Bromate: BrO31-
Perbromate: BrO41-

20. Other Polyatomic Ions All other polyatomic ions need to be memorized
Start by memorizing the polyatomic ions that end in – ate first

21. Ionic Compound Nomenclature
Formula Unit: the smallest unit of an ionic compound which is composed of a cation and an anion
When writing the chemical formula for an ionic compound it is always the same as the empirical formula
Empirical formula: shows the atoms in the simplest whole number ratio
The formula of an ionic compound must be electrically neutral
The charges must add up to equal 0

22. Writing Formulas for Ionic Compounds
Write the chemical formula for the cation
Write the chemical formulas for the anion
Find the least common multiple between the 2 charges on the cation and anion
The subscript for each ion will be the factor needed to reach the LCM
Use parentheses with a subscript on the outside for polyatomic ions only
Reduce the subscripts to the smallest ratio

23. Writing Chemical Formulas
Lithium fluoride:
Calcium oxide:
Aluminum nitride:
Magnesium phosphate:

24. Naming Ionic Compounds
Divide the formula into the positive half and the negative half (cation and anion)
Write the name for the positive ion
Write the name for the negative ion
Use the charge for the negative ion to determine the oxidation state for the positive ion when a Roman numeral is needed
If the positive ion is monatomic and NOT in column IA, IIA and is not silver, zinc, or aluminum you must use a Roman numeral to name it
Write the name of the cation and then the name of the anion

25. Molecules and Molecular Compounds
Molecule: Smallest unit of a covalent compound (2 nonmetals)
Binary molecule: molecule that is composed of only 2 elements
Greek prefixes are used when naming covalent compounds

26. Greek Prefixes Greek Prefix Number of Atoms Mono 1 Di 2 Tri 3 Tetra 4
Penta 5
Hexa 6
Hepta 7
Octa 8
Nona 9
Deca 10

27. Naming and Formula Writing for Covalent Compounds
When the prefix ends in a or o, and the name of the second elements begins with a vowel (such as oxide), the a or o is often dropped
The first word of the name is made up of a prefix and the first element in the compound
The prefix is only used when more than 1 atom is present
The second word of the name always has a prefix and ends in - ide

28. Covalent Naming and Formula Writing
Carbon monoxide
SO2
Dinitrogen pentoxide
P4O10

29. Naming Acids
A substance that produces hydrogen ions when dissolved in water
Acids will always have hydrogen written as the 1st element in the chemical formula
We will derive the name of the acid from the name of the anion

30. Naming Acids Anion Acid -ate -ic acid -ite -ous acid -ide
Hydro________ic acid

31. Naming Acids HC2H3O2 HF HClO2 Carbonic acid Phosphorus acid
Hydroiodic acid

32. Naming Bases
Any substance that produces hydroxide ions when dissolved in water
Common bases include metal hydroxides, group 1A and 2A metal oxides (MO) and ammonia (NH3)
In order to name bases use the rules for ionic nomenclature

33. Naming Bases
LiOH
SrO
NH3
Sodium oxide
Magnesium hydroxide

34. Naming Hydrates
An ionic compound that has a specific number of water molecules attached to the structute
Writing formulas and naming takes rules from both ionic and covalent nomenclature
For the ionic component use the ionic nomenclature rules
For the water portion to indicate the number of waters use the Greek prefixes

35. Naming Hydrates Barium chloride dehydrate
Magnesium sulfate heptahydrate
Sr(NO3)2 ● 4H2O
CuSO4 ● 5H2O