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Write these questions in your NB

Write these questions in your NB. Compare/Contrast an Element vs. Compound Who is attributed with developing the Periodic Table? How was the 1 st Periodic Table Arranged? How is that different from now? What is periodicity?. Periodic Patterns. Unit 4 – Periodic Table. METALLIC TREND.

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Write these questions in your NB

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  1. Write these questions in your NB • Compare/Contrast an Element vs. Compound • Who is attributed with developing the Periodic Table? • How was the 1st Periodic Table Arranged? How is that different from now? • What is periodicity?

  2. Periodic Patterns Unit 4 – Periodic Table

  3. METALLIC TREND INCREASES INCREASES

  4. ATOMIC RADIUS • Radius is the distance from the center of the nucleus to the “edge” of the electron cloud. • Atomic radii are usually measured in picometers (pm) or angstroms (Å). An angstrom is 1 x 10-10m.

  5. ATOMIC RADII TRENDS DOWN A FAMILY OR GROUP WHY? • As you go down a family thenvalue increases making the radius larger. INCREASES

  6. ATOMIC RADII TRENDS ACROSS A PERIOD WHY? • As you go across a period the number of protons increases, (nuclear charge) pulling the electrons in tighter making the radius smaller. DECREASES

  7. IONS- Has a charge Metals • Lose electrons becoming positive. Calcium – Ca Loses 2 e-s becoming Ca+2 Nonmetals • Gain electrons becoming negative. Chlorine – Cl Gains one e- becoming Cl-1

  8. IONS – How can I remember? Metals Nonmetals This is Cat-ion - CATION This is Ann ion - ANION He is a “plussy” cat! She is unhappy and negative.

  9. IONIC RADII TRENDS DOWN A FAMILY OR GROUP WHY? • As you go down a family thenvalue increases making the radius larger. INCREASES

  10. IONIC RADII TRENDS ACROSS A PERIOD WHY? • For the metals thenuclear chargeis greater than then number of electronspulling them in tighter making the radius smaller. • At the nonmetals the radius gets larger because the ion has gained electrons. DECREASES then INCREASE

  11. METALLIC ATOM AND ION COMPARISON

  12. Shielding Effect As more electrons are added to atoms, the inner layers of electrons shield the outer electrons from the nucleus. The effective nuclear charge on those outer electrons is less, and so the outer electrons are less tightly held

  13. Example of Shielding Effect

  14. Ionization Energy The energy required to remove an electron from an atom is ionization energy. (measured in kilojoules, kJ)

  15. IONIZATION ENERGY The larger the atom is, the easier its electrons are to remove. Ionization energy and atomic radius are inversely proportional. Ionization energy is always endothermic, that is energy is added to the atom to remove the electron.

  16. IONIZATION TREND INCREASES INCREASES

  17. Electron Affinity is a measure of the energy change when an electron is added to a neutral atom to form a negative ion

  18. ELECTRON AFFINITY Why do the Alkaline Earth Metals and Noble Gases not have measurable Electron Affinities?

  19. Electronegativity is a measure of the tendency of an atom to attract a bonding pair of electrons.

  20. ELECTRONEGATIVITY

  21. In Summary…. Electronegativity Electronegativity

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