MODULE 1

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 +1.602x10-19coulombs • found inside the nucleus • composed of 2 up quarks and 1down quark • mass = 1.672622x10-24 g or 1.007276 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 = 1.674927x10-24 g or 1.008665 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 -1.602x10-19coulombs • leptons • found outside of the core of the atom • mass = 9.1x10-28 g or 0.00055 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 = 6.022 x 10 23 particles - Just like 1 dozen eggs = 12 eggs - 1 mole eggs = 6.022 x 10 23 eggs

14. MOLAR MASS • MOLAR MASS – the mass in grams of one mole of atoms of any element which is 6.022 x 10 23 atoms of that element Ex. 1 mole of Na = 22.9898 grams of Na 1 mole of Na = 6.022 x 10 23 atoms of Na 22.9898g of Na = 6.022 x 10 23 atoms of Na

15. Conversion of Units • Review Example 2.4 - Mass, Moles, and Atoms pg. 60-61 • Review Example 2.5 - 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.