1 / 30

Chapter 6- The Periodic Table

Chapter 6- The Periodic Table.

timothy-beasley
Download Presentation

Chapter 6- The Periodic Table

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript

  1. Chapter 6- The Periodic Table • Vocabulary-Atomic Mass, Atomic number, macronutrient, trace element, trace amount, periodic table, periodic properties, electronegativity, ionization energy, orbital, transition metal, noble gas, alkali metal, alkali earth metal, atomic radius, valence, electron shell, electron configuration, bonding, Lewis dot diagrams

  2. The state says you need to • 3.01 Analyze periodic trends in chemical properties and use the periodic table to predict properties of elements. • Groups (families). • Periods. • Representative elements (main group) and transition elements.

  3. More • Electron configuration and energy levels. • Ionization energy. • Atomic and ionic radii. • Electronegativity.

  4. New way to examine • Chm.1.3 Understand the physical and • chemical properties of atoms • based on their position in the • Periodic Table.

  5. Chm.1.3.1 Classify the components of a periodic table (period, group, metal, metalloid, nonmetal, transition). Chm.1.3.2 Infer the physical properties (atomic radius, metallic and nonmetallic characteristics) of an element based on its position on the Periodic Table.

  6. Chm.1.3.3 Infer the atomic size, reactivity, electronegativity, and ionization energy of an element from its position in the Periodic Table.

  7. What is the universe made of? • The materials the universe first developed were few, mainly hydrogen and helium • Where did the rest come from? • (explain the process of fusion that happens in stars) • Pressure causes nuclei to fuse together

  8. The periodic table • Gregor Mendeleev notice patterns in the mass and reactions of elements • (Scientists notice patterns and anomolies) • Periodic means repeating

  9. Size of atoms

  10. The Strong nuclear force keeps the protons and neutrons together. • The more protons and more neutrons you have, the stronger the attraction between the nucleus and the electrons. • This is what makes the atom radius smaller as you cross the periodic table.

  11. Electronegativity • Electronegativity is the measure of how well an atom can attract electrons from another atom to which it is bonded. • They are already bonded...what does it do to the electrons. The more electronegative it is, the more likely it is to pull off electrons of its partner.

  12. Ionization energy • ionization energy - the energy required to remove an electron from its atom. • Almost, but not quite like electronegativity • Electronegativity is how well it takes someone else’s electron • Ionization energy is how well it holds on to its own electrons

  13. 6.2 Properties of groups • Columns on the periodic table are called groups or families. Each member of the group would have the same number of electrons in the outside orbital. Thus, they would be similar chemically

  14. Group I- Alkali Metals • (Hydrogen not actually considered a part of it) • Soft Metals. lose the one electron on its outer orbital easily. React explosively with water. • In your body used in nerve signaling. (electrolytes)

  15. Group II-Alkaline Earth metals • 2 outer electrons, they lose them easily (ions are B 2+ , Ca 2+ , etc) • CaO, CaCl2, etc

  16. Transition Metals • The low part of the periodic table • Outer electrons are in the d orbital • Can bond in different ways, both FeO and Fe2O3. • Traditional metals, good conductors of electricity

  17. Carbon, Nitrogen, Oxygen • Very flexible in bonding, especially carbon • 4, 5, and 6 electrons in their outer orbitals

  18. Halogens • Group 17 • 7 of 8 possible electrons in the outer orbital • Tend to pull an electron off another atom to form ionic bonds. • Form diatomic molecules (F2, Cl2, etc.) • Form acids with H (HCl, HBr, HF) • Form salts with metals (NaCl)

  19. Noble Gases • Don’t normally form bonds! • Outer orbitals are full!~

  20. Compounds • Compounds give each participating atom a full outer orbital. This makes it more stable. • CH4, H2O

  21. Section 6.3 Valence • Reactions only occur in the highest unfilled electron level. • Atoms react to have a full or empty outer level • The total possible valence electrons is 8 • Each group or family has the same number of electrons in every member’s outer shell.

  22. Lewis Dots • Lewis Dots represent the number of electrons in the outer orbits. These electrons are referred to as Valence electrons • Notice that each family looks the same in Lewis Dots • You need to be able to make Lewis dots for each group or family

  23. Notes • Make sure you read 189 to 191

  24. Faculty Periodic Table • Arrange at least 30 of the staff at Paisley into a periodic table. • Remember that “Periodic” means having patterns. • Explain your reasoning for your arrangement (75%) • Creativity with symbols and appearance is appreciated (25%)

  25. Included • Reason for groups (10 pt) • Reason for families (10) • At least two other “periodic” traits (10) • Creativity and appropriateness (10)

  26. To help you with patterns and the periodic table: • 6A • 6B

  27. Feb 9 • How are the projects coming? • 6C • Collect work • Lewis Dots

More Related