MODULE 1 CHAPTER 2 LECTURE OUTLINE

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.

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

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.

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

PROTONS PROTONS – are defined as: positively charged subatomic particles with a charge of +1.602x10-19 coulombs 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

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.

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

ELECTRONS ELECTRONS – are defined as: negatively charged subatomic particle with a charge of -1.602x10-19 coulombs 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

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

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

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

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

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

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!

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.