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Periodic trends
- 3. Atomic Radius (Covalent Radius) • Defined as ______ the distance half between the nuclei of identical atoms that are bonded together • Ex. Cl2 Cl Cl ½ distance
- 4. Atomic Radius Trend Increases down and to the left Francium • Largest : ____________ Helium • Smallest : __________
- 5. Atomic Radius Trend • REASON: increasing __________ nuclear charge (protons) – pulls the electrons _________ to the nucleus. closer • Example: Which element has a larger atomic radius – Silicon or Silicon Sulfur? __________ • Example: Which element has a larger atomic radius – Sodium or Potassium? _____________ Potassium
- 6. 2. IONIZATION ENERGY
- 7. IONIZATION ENERGY • Ion : an atom or group of bonded atoms that have a __________ or __________ negative positive charge. Ex. Na+ Cl- 11 protons = 11 + 17 protons = 17 + 10 electrons = 10 - 18 electrons = 18 - 1+ 1-
- 8. IONIZATION ENERGY • Ionization Energy : the energy required to remove ____ ________ from a neutral one electron atom. • Trend: Increases up and to the right
- 9. Ionization Energy • Lowest ionization energy : _____________ Francium Group : _____________ Alkali Metals • Highest ionization energy: _____________ Helium Group : _____________ Noble Gas Ex. What has the higher ionization energy – Aluminum or Phosphorus? _____________ Phosphorus Ex. What has the lower ionization energy – Calcium or Strontium? _____________ Strontium
- 11. Electronegativity • Definition: the measure of the ability of an atom in a chemical compound to _______ electrons closer to it. attract • _______ _______ don’t form Noble Gases compounds, so they are not included.
- 12. Electronegativity Periodic Trend • Trend : Increases up and to the right
- 13. Electronegativity • Highest Electronegativity : ________ Fluorine • Lowest Electronegativity : ________ Francium • Only element with 4.0 : __________ Fluorine • Only elements in the 3’s : Oxygen Chlorine Nitrogen _________, _________, __________.
- 15. METALLIC ACTIVITY TREND • Largest : ____________ Francium Helium • Smallest : __________
- 16. 5. IONIC RADII
- 17. Ionic Radii • Positive ion : ________ cation Na+ ex. ______ • Negative ion : _______ anion ex. ______ Cl- lose • Neutral atoms _____ an electron to become positive __________ ions. Ex. K (19 electrons) K+ (18 electrons) + 1e- gain • Neutral atoms _____ an electron to become negative __________ ions. Ex. Cl (17 electrons) + 1e- Cl- (18 electrons)
- 18. Ionic Radii • Positive ions, ex. ___, are ________ Na+ smaller than a neutral atom of that same element. (LOSE an electron) • Negative ions, ex. ____, are _______ Cl- larger than a neutral atom of the same element. (GAIN an electron)
- 19. REVIEW
- 20. Atomic Radius