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Matter, Atomic Structure-Periodic Table

Matter, Atomic Structure-Periodic Table. ISCI 2002 Spring 2009. Matter. Anything that has mass and occupies space Matter is what substances are made of Properties of matter 1. macroscopic – properties you can see 2. microscopic – atoms arranged in a solid, liquid, gas.

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Matter, Atomic Structure-Periodic Table

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  1. Matter, Atomic Structure-Periodic Table ISCI 2002 Spring 2009

  2. Matter • Anything that has massand occupies space • Matter is what substancesare made of • Propertiesof matter • 1. macroscopic– properties you can see • 2. microscopic– atoms arranged in a solid, liquid, gas

  3. Classification of Matter

  4. Atomic Structure • 1. Sizeand generalstructure • Small; cannot be seen with visible light • 2. Parts - atom • Nucleus • Protons and neutrons • Energylevels/ electron clouds • Electrons • 3. Atoms are mostly emptyspace • Nucleus determines the mass of the atom

  5. Subatomic Particles • Atomic mass unit (amu) – hydrogen atom (1 amu) • Electron mass = 1/2000 amu

  6. Nucleus of the Atom • 1. Proton+ Neutron • Mass of the atom • 2. Electrons • 1/2000 of one amu • Not included in the mass

  7. Atomic Number • Atomic Number – Periodic Table • Number of protons in an atom • Protons always equal electrons! • Using your periodic table determine the number of protons and electrons in the following atoms • Sodium • Chlorine • Nitrogen • Lithium

  8. Mass Number • Number of neutronsand protons • AverageAtomicMass • Average of all the isotopes in an element.

  9. Isotopes • 1. Elementsare composed of several different types of the same atom • Same type of atoms with differing number of neutrons • 2. Carbon • 3 isotopes • Carbon 12, 13, and 14 • Calculating neutrons

  10. Using the mass number and atomic number to determine the subatomic particles The atomic number equals the number of protons. Protons always equal the number of electrons!

  11. Drawing Planetary Models of Atoms

  12. Drawing Planetary Models • 1. Look at the atomicnumber • 2. Determine the number of electrons • 3. Draw each energylevelwith correct number of electrons • Draw only the ‘valence’ electrons • S and P orbitals only

  13. Periodic Table • 1. Symbol • 2. AtomicNumber • Number of protons • 3. AtomicMass-(Average Atomic Mass) • Mass of neutrons and protons • 4. Group • Vertical • 5. Period • Horizontal

  14. Periodic Table

  15. Periodic Table

  16. Groups and Periods

  17. Chemical and Physical Properties • PhysicalProperties • Appearance – hard or soft; dull or shiny; color • Density; melting point and boiling point • ChemicalProperties-describes changes of composition the substance undergo’s during a chemical change • What is required to bring about the change • Temperature, heat, number of electrons, etc.

  18. Chemical and Physical Properties • ExtensiveProperty • Depends on the ‘quantity’ of matter in a sample • Cannot be used to characterize a type of matter • Mass of water is 2.0 kg? Another sample may be 4.0 kg • Volume, mass • IntensiveProperty (distinguishes one substance from another) • Property shared by all examples of a specific type of matter • Density (m/v); color; melting point; solubility; acidic or alkaline • The density of water is 1.0 g/cm3

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