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Understanding Matter: Atoms, Compounds, and Building Blocks

Explore the fundamentals of matter, including atoms, compounds, quarks, leptons, protons, and electrons. Learn about isotopes, atomic weight, moles, molar mass, and unit conversions. Dive into the periodic table to expand your knowledge of the elements.

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Understanding Matter: Atoms, Compounds, and Building Blocks

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  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.

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