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Periodic Table Trends

Periodic Table Trends. What is it?. Arrangement of the elements in order of their atomic numbers so that elements with similar properties fall in the same column, or group. Important Terms. Group: vertical column of periodic table Period: horizontal row of periodic table

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Periodic Table Trends

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  1. Periodic Table Trends

  2. What is it? • Arrangement of the elements in order of their atomic numbers so that elements with similar properties fall in the same column, or group

  3. Important Terms • Group: vertical column of periodic table • Period: horizontal row of periodic table • Valence Electrons: electrons that occupy the highest energy level • Up to 8 • Atoms want to have full valence shell • Ion: atom that has gained or lost an electron • Cation: atom loses electron; has + charge • Anion: atom gains electron: has - charge

  4. Group 1 • Alkali metals • Silvery appearance • Can be cut by knife • Highly reactive with water • Usually not found in nature as a pure element • Always forms cations with +1 charge • NOTE: Hydrogen, even though it is listed in group one, is NOT an alkali metal

  5. Group 2 • Alkaline-earth metals • Similar to alkali metals, but harder, denser, and stronger • Also not usually found in nature as a pure element • Always forms cations with +2 charge

  6. Groups 3-12 • Transition metals • Good conductors of electricity • High luster • Less reactive than alkali and alkaline-earth metals • Some do not easily form compounds! • Forms cations with varying charges

  7. Group 17 • Halogens • Most reactive non-metals • React with metals to form salts • Always form anions with -1 Charge

  8. Group 18 • Noble Gases • All electron shells full • Little to no chemical reactivity • Always has neutral charge

  9. Lanthanides and Actinides • Do not easily fit in any particular group, so these elements are usually separated in it’s own area on the periodic table • All actinides are radioactive • Only 4 are found naturally

  10. Periodic Properties • Atomic radii • Distance from the nucleus to the outer edge of electron cloud • Increases as you go read down the group • Decreases as you read across the period • Why?

  11. Periodic Properties • Ionic radii • Distance from the nucleus to the outer edge of electron cloud after an atom has gained or lost an electron • Groups 1-13 form cations (+) • Groups 15-17 form anions (-) • Increase as you go read down the group • Cationic radii decrease as you read across the period • Anionic radii increase as you read across the period • Why?

  12. Periodic Properties • Ionization energy • The energy needed to remove an electron from an atom • Decreases as you read down a group • Increases as you read across a period • Why?

  13. Periodic Properties • Electron Affinity • Energy change that occurs when an electron is gained by a neutral atom • Represented as a negative number • Decreases slightly as you read down a group • Greatly increases as you read across a period • Why?

  14. Periodic Properties • Electronegativity • The ability of an atom to attract an electron • Decreases as you read down a group • Increases as you read across a period • Why?

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