1. MODULE 1
CHAPTER 2
LECTURE OUTLINE

2. Types of Matter (Chapter 1 Review):
ATOM - The smallest particle of an element that retains the chemical properties of that element.
COMPOUND - Matter that is composed of 2 or more elements combined in definite proportions.
ELEMENT - Matter that is composed of only one type of atom.
MOLECULE - A definite group of atoms that are chemically bonded, i.e. tightly connected by attractive forces.
MATTER - Anything that has mass and occupies space.
SUBSTANCE - Matter that can not be separated by physical techniques, and that has a unique set of properties.

3. Fundamental Building Blocks
All matter is composed of 12 fundamental building blocks
6 are called quarks and
6 are called leptons.

4. QUARKS
QUARKS - composite particles that protons, neutrons and other subatomic particles are made from.  There are 6 different types of quarks:
Up & down,
Charm & strange, and
Top & bottom.

5. LEPTONS LEPTONS – are independent particles of 6 different types:
Electrons & electron neutrino,
Muon & muon neutrino, and
Tau & tau neutrino.

6. PROTONS PROTONS – are defined as:
positively charged subatomic particles with a charge of x10-19 coulombs
found inside the nucleus
composed of 2 up quarks and 1down quark
mass = x10-24 g or AMU
* The elements atomic number ( Z#) = # protons

7. NEUTRON NEUTRONS – are defined as
electrically neutral subatomic particle
found inside the nucleus
composed of 2 down quarks and 1 up quark
mass = x10-24 g or AMU.

8. NUCLEUS NUCLEUS – is defined as: core of the atom centrally located
positively charged
contains most of the atom's mass
very dense
small relative to the overall size of the atom

9. ELECTRONS ELECTRONS – are defined as:
negatively charged subatomic particle with a charge of x10-19 coulombs
leptons
found outside of the core of the atom
mass = 9.1x10-28 g or AMU
travel in orbitals around the nucleus
mostly empty space
occupies most of the size of the atom

10. ATOMS ATOMS – are defined as:
smallest particle of an element that retains the chemical properties of that element
composed of the nucleus (core) surrounded by electrons

11. ISOTOPES ISOTOPES – are defined as:
Atoms of the same atomic number but different mass
B-10 = Boron has 10 mass units, 5 protons & 5 neutrons
B-11 = Boron also can have 11 mass units, 5p & 6n
Percent Abundance = # of atoms in an isotope x 100%
total # of all isotopes of that element

12. ATOMIC WEIGHT ATOMIC WEIGHT or ATOMIC MASS – are defined as:
Average mass of all naturally occurring isotopes of that element
See Table 2.2 on page 57
Review Exercise 2.4 – Calculating Atomic Wt., pg. 58
Review Screen 2.12 on the CD-ROM

13. CONCEPT OF A MOLE
MOLE – amount of substance that contains as many elementary particles as there are atoms in exactly 12 grams of the carbon-12 isotope
1 mole = x particles
- Just like 1 dozen eggs = 12 eggs
- 1 mole eggs = x eggs

14. MOLAR MASS
MOLAR MASS – the mass in grams of one mole of atoms of any element which is x atoms of that element
Ex. 1 mole of Na = grams of Na
1 mole of Na = x atoms of Na
g of Na = x atoms of Na

15. Conversion of Units
Review Example Mass, Moles, and Atoms pg
Review Example Mole Calculations pg. 61
** Use unit label to perform all conversions!

16. The Periodic Table View Screens 2.13 & 2.14 on the CD-ROM
Go into the Interactive Periodic Table on the CD-ROM and familiarize yourself with its features.
Read pages 62 – 72 in the text and pay particular attention to the display on page 63.