1. Chemical Names and Formula
Chemistry
Cook

2. Periodic Table
There are over 90 naturally occurring elements/atoms and about 25 elements made in the lab.
Various combinations of atoms can be formed, and which such diversity we need a way to name and communicate these variations

3. Periodic table
Elements are arranged in row and columns on the: Periodic table
Hydrogen, the smallest and lightest element in top right corner
Helium is atomic number 2

4. Atomic Numbers
Krypton

5. Calculate For any element: Number of Protons = Atomic Number
Number of Electrons = Number of Protons = Atomic Number
Number of Neutrons = Mass Number - Atomic Number
For krypton: Number of Protons = Atomic Number = 36
Number of Electrons = Number of Protons = Atomic Number = 36
Number of Neutrons = Mass Number - Atomic Number = = 48

6. Periodic Table
A column of elements in the periodic table is known as a group
There are 18 groups
Group 1A: H Li Na K RB Cs

7. Breakdown of each group
Group 1=Alkali Metals
Group 2= Alkaline Earth Metals
Group 3-12= Transition metals
Group 13,14 & 15= Other metals
Metalloids=Boron diagonal down over and down over( A big L)
Group =Non Metals
Group 17= Halogens (salt formers)
Group 18= Noble gases
Rare Earth Metals= Man made elements inserted in the transition metal at 56 and 88
Chemical Elements.com - Noble Gases

8. Alkali Metals/Representative metals (A)
The illustrate the entire range of chemical properties
Both metals and non metals
They do not include transition metals or inner transition metals (man made ones)

9. Metallic Metals A Groups (1, 2 13-18) Have high luster when cleaned
High electrical conductivity
Ductile
Can be drawn into wires
Malleable
Beaten into sheets (dyes at GM plants)

10. Groups 1A starts with H or Li 2A starts with Be 3A starts with B
Hydrogen is special It is a non metal in group 1A
2A starts with Be
3A starts with B
4A starts with C
5A starts with N
6A starts with O
7A starts with F

11. Transition Metals (B) B group elements
Inner transition metals (rare earth metals).

12. Non Metallic Elements that are: Non lustrous
Poor conductors of electricity
Some are gases
Others are brittle solids and some liquids at room temperature

13. Semi Metals or Metalloids
Elements with the properties of both metals and nonmetals
Silicon
Found in transistors
Good semi conductor
Conducts electricity in a special way
Breast implants (cheap ones)

14. Atoms and Ions All elements are composed of atoms of the same kind
Atomic Theory (review)
An atom is electrically neutral because it has an equal number of protons and electrons
Na atomic number is 11 and has 11 protons and is positively charged, has 12 neutrons
Because Neutrons have no charge the total charge of Na is (+11)+ (11)=0
When elements form compounds they can gain or lose electrons, and when the number of electrons is not equal to the number of protons then the atom becomes a
Ion

15. IOns
Are atoms or groups of atoms that have a positive or negative charge
Formed when atoms gain or lose electrons

16. Positive ions
Metals tend to form positive ions by losing one or more electrons
Cation
Any atom or group of atoms with a positive charge
Na ion is form by the loss of one electron from the Na atom
Sodium ion has 11 protons and 10 electrons it has a charge of 1+
Atomic charges are written with the number followed by a sign
Na1+ or Na+ (always write ions this way)
If the number is 1 it can be omitted

17. Ions
Mg ions are formed differently because they have different valence electrons (electrons in outer shell)
Mg has a charge of 2+ so it has 12 protons, and 10 electrons

18. Negative Ions Nonmetallic elements tend to gain one or more electrons
Anions
Atoms or groups of atoms with a negative charge
Anions have more electrons (unlike cations).
Cl ions has 17 protons and 18 electrons
It has a charge of -1
Oxide ion has a charge of -2

19. Compounds
Are pure substances the differ from elements because they contain more than one kind of atom.
Law Of Definite Proportions: In any chemical compound the elements are always combined in the same proportion by mass
A Molecule is a neutral group of atoms that act as a unit. All molecules of a given compound are neutral.
Compounds that are composed of molecules are molecular compounds.

20. Law of Definite Proportions
MgS is a compound. IF we have 100g of this compound
It will always contain:
43.13g of Mg
56.87g of S
This mass ratio will never change no matter how much you have

21. Chemical Formulas There are more than 4 million chemical compounds.
Some are molecular
Some are ionic
A chemical formula shows the number and kinds of atoms present in a molecule.
A molecular formula shows the number and kinds of atoms present in a molecule of a compound
Example = H2O CO2 C2H6 C2H6O

22. Formulas and Names of Common Metals Ions with more than 1 ionic charge
Formula Name Stock Name Classical Name
Cu Copper (I) Ion Cuprious ion
Cu Copper (II) Ion Cupric Ion
Fe Iron (II) Ion Ferrous Ion
Fe Iron (III) Ion Ferric Ion
Hg2 Mercury (I) Ion Mercurrous Ion
Hg Mercury (II) Ion Mercuric Ion
Review Table 5-3

23. Rules for naming Compounds that give OH- ions
Bases
Compounds that give H+ ions
Acids
ite ending
Will always indicate less oxygen
ate ending
Will always indicate more oxygens

24. Binary ionic compounds
Composed of two elements
Always cation and anion
They always have ide ending
Name metal first then put ide ending on nonmetal
Sodium chloride
Monoatomic always have ide ending

25. Binary Ionic compounds
Name by writing name of cation followed by name of anion (ide ending).

26. Ternary Ionic Compounds
Contain 3 different elements
They usually contain one or more polyatomic ions
First write down formulas of ions
Then balance charges
An ate or ite ending on polyatomic ion
Calcium nitrate

27. Acids
Are compounds that give off hydrogen ions when dissolved in water.
When anion ends in ide the acid name begins with prefix hydro. The stem (nonmetal in most cases ends with ic)
HCl= hydrochloric acid

28. rules Anion ending Example/Stem Acid Name Example ide Cl- Chloride
Hydro (stem) ic acid
Hydrochloric acid
ite
SO2-3
Sulfite
(stem) ous acid
Sulfurous acid
ate
NO-3
nitrate
(stem) ic acid
Nitric acid