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OVERALL REACTIVITY TRENDS IONIC & COVALENT COMPOUNDS Section 2.1 and 2.3

OVERALL REACTIVITY TRENDS IONIC & COVALENT COMPOUNDS Section 2.1 and 2.3. METAL REACTIVITY TREND. Right to left: Reactivity INCREASES Top to bottom: Reactivity INCREASES. METAL REACTIVITY TREND (Right to Left: INCREASE). Ex: Na vs Mg Na has one valence electron

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OVERALL REACTIVITY TRENDS IONIC & COVALENT COMPOUNDS Section 2.1 and 2.3

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  1. OVERALL REACTIVITY TRENDS IONIC & COVALENT COMPOUNDS Section 2.1 and 2.3

  2. METAL REACTIVITY TREND • Right to left: Reactivity INCREASES • Top to bottom: Reactivity INCREASES

  3. METAL REACTIVITY TREND(Right to Left: INCREASE) • Ex: Na vs Mg • Na has one valence electron • Mg has two valence electrons • It takes LESS ENERGY to remove one electron than 2 electrons • What does this LOOK like?

  4. Mg + water Na + water

  5. METAL REACTIVITY TREND(Top to Bottom: INCREASE) • Na vs K Na K Both have 1valence electron, but… K has 4 rings and Na has 3 rings K is MORE reactive; more likely to give up e-

  6. NON METAL REACTIVITY TREND • Left to right: Reactivity INCREASES • Bottom to top: Reactivity INCREASES

  7. NON METAL REACTIVITY TREND(Left to right: Increase) • Ex: O vs F • O has 6 valence electrons • F has 7 valence electrons • F needs only 1 electron; • Need less energy to gain 1 electron so F is MORE REACTIVE • NOBLE GASES do NOT follow trend

  8. NON METAL REACTIVITY TREND(Bottom to top: Increase) • Cl vs F • Both have 7 valence electrons • F is more reactive because the electrons are closer to the nucleus

  9. IONIC COMPOUNDSSECTION 2.1 • Contain a metal and non-metal • Lattice of ions (endless, repeating pattern) • Na+Cl-Na+Cl-Na+Cl-Na+Cl- Na+Cl-Na+Cl-Na+Cl-Na+Cl- • Extremely stable structures

  10. PROPERTIES of IONIC compounds • Melting and boiling point: extremely high • strong forces holding atoms together • Exist mostly as solids • Brittle • When the structure shifts, similar charges line up

  11. PROPERTIES of IONIC compounds • Soluble in water • Ex: water and salt • Conduct electricity when in solution • Form ions in solution • Ions have a charge and can move around (to conduct)

  12. MOLECULAR COMPOUNDS • Consist of only non-metals held together by COVALENT bonds • Can exist as a solid, liquid or gas • Flexible and softer because of weak forces holding the atoms together Ex: Carbon Dioxide  • Low Melting and boiling points • Do not conduct electricity

  13. COVALENT BONDS • One pair of electrons shared constitues a SINGLE BOND • Two pairs: DOUBLE BOND • Three pairs: TRIPLE BOND • Pair of Electrons involved in bond: BONDING PAIR • Pair of Electrons not involved: • LONE PAIR

  14. HOMEWORK: • Read Pages 52-59 • Read Pages 76-78, 80-81 • Page 59- LC: 1-5 • Page 63- 1-9

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