1. Review of Atomic Theory

2. What is matter?
Mather is anything that has mass and volume. What isn’t matter?

3. What isn’t matter? Energy is not matter as it has no mass or volume.
Eg. Light, heat, electricity
Forces: gravity, magnetism
All matter is composed of elements.

4. What is an element?
An element is any substance that cannot be broken down into simpler substances by ordinary chemical means.
Elements are made up of atoms.

5. What is an atom?
An atom is the smallest unit of an element that still retains the properties of an element.
Eg. Oxygen, Carbon, Gold, Silver, Mercury

6. What is a compound?
a pure substance made up of two or more types of atoms chemically joined in fixed proportions
Eg: water, sugar, salt
H2O, NaCl

7. Do you remember the parts of the atom?

8. Parts of the atom

9. Bohr Model
Indicates number of ELECTRONS in each of the ENERGY LEVEL / SHELL / ORBITAL.
Each energy level can only hold so many electrons:
1st shell: 2 electrons
2nd shell: 8 electrons
3rd shell: 8 electrons
4th shell: 18 electrons

11. Difference between atomic mass and atomic number
Atomic Number = protons
Atomic Mass = protons = neutrons

12. Fun Facts you should know about atoms:
Where each subatomic particle can be found.
What charge each subatomic particle has.
Why are atoms are neutral?
Atoms are mostly empty space – what subatomic particle accounts for most of the volume?
What subatomic particles account for most of an atom’s mass?
How to determine the number of protons, neutrons, electrons

13. Each atoms prefers to have a FULL valence shell
An atom will lose or gain electrons to achieve a Stable Octet (full valence shell).
When a neutral atom gains electrons  negative
When an atom loses electrons  positive

14. What is an ion? An ion is an atom that has gained a charge
Can be positive (cation)
or negative (anion)

16. Where can an atom get another electron?
From an atom wanting to get rid of one of course:

19. Naming Binary Ionic Compounds
First name unchanged, Second name add -ide
NaCl MgCl2
MgO
LiF

20. Naming Ionic Compounds with Polyatomic Ions
CaCO3 is calcium carbonate
Na0H
MgSO4
KNO3

21. Two types of Compounds
Ionic
Covalent

22. What are isotopes?
Isotopes are different forms of the same element (same number of protons) but with different number of neutrons.
Atomic number same (protons)
Atomic mass different (p + n)

23. Isotopes are identified by their Atomic Mass
Lithium lithium lithium 8

24. You try: Write the atomic number and mass of each carbon isotope
You try: Write the atomic number and mass of each carbon isotope. Normal Carbon has 6 protons.

25. You try: Write the atomic number and mass of each carbon isotope
You try: Write the atomic number and mass of each carbon isotope. Normal Carbon has 6 protons.
Mass
Protons
Neutrons

26. Why are isotopes important?

27. Why are isotopes important?
Isotopes are unstable and will decay at a reliable rate over long periods of time
Scientists compare original (parent) isotope to resulting (daughter) isotope to determine age of very old geological features.
Eg. Carbon dating.

28. Homework
Read pages of your text and answer Questions #1, 2, 5, 6, 7 on page 33.