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Chemical Bonding

Chemical Bonding. Chapter 6. A Chemical Bond. A mutual attraction between the nuclei and valence electrons of different atoms that bind them together

charleen-nigel
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Chemical Bonding

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  1. Chemical Bonding Chapter 6

  2. A Chemical Bond • A mutual attraction between the nuclei and valence electrons of different atoms that bind them together • By itself, an atom has a high potential energy. Nature actually favors low energy (stability). Thus, atoms bonding increases stability by lowering potential energy

  3. Types of Chemical Bonds • Ionic Bonding • A chemical bond that results from the electrical attraction between large numbers of positive ions (cations) and negative ions (anions) • For example: Salt (NaCl)

  4. Ionic Bonding and Electronegativity • When the difference in electronegativity (∆EN) is greater that 1.8, the bond is ionic. • Remember that electronegativity is the ability of an atom to attract an electron from another atom. • Lets go back to NaCl… .93 3.16

  5. Ionic Bonding and Electronegativity • Chlorine has the greater electronegativity, so it will attract the lone valence electron more strongly to gain a full Octet of valence electrons .93 3.16

  6. Lets Review the Octet Rule • The octet rule: • states that atoms lose, gain or share electrons in order to acquire a full set of 8 valence electrons (the stable electron configuration of a noble gas)

  7. Ionic Bonding and Electronegativity • Difference in electronegativity is calculated by subtracting the two values. • ∆EN=0-0.3 non-polar covalent • ∆EN=0.4-1.7polar covalent • ∆EN≤ 1.8 Ionic .93 3.16 3.16-.93=2.23

  8. Lets Try Some Examples • HCl • KCl • BeO • H2O • SiH₄ • HBr • CH₄ • NH₃

  9. Examples • HCl (Hydrogen Chloride) • KCl (Potassium Chloride) .82 K Cl 3.16 2.20 3.16

  10. Examples • BeO (Beryllium Oxide) • This compound has a double bond. Each line represents a bonding electron pair. How many bonded electron pairs are there in this molecule? 1.57 3.44

  11. Examples • H2O(Water) 3.44 2.20 2.20

  12. Dipole Moments • Dipole-equal but opposite charges separated by a short distance • Dipole Moment-unequal and opposite charges separated by a short distance. Leads to one end of the molecule being more negative or more positive than the other. Represented with a δ+ or a δ-. This is called polarity.

  13. So lets revisit… • NaCl, Which direction is the dipole moment? .93 3.16

  14. So lets revisit… • BeO (Beryllium Oxide), which direction is the dipole moment? 1.57 3.44

  15. So lets revisit… • H2O, which direction is the dipole moment?

  16. Homework… • Pg195, 1-5 • Calculating Electronegativity worksheet

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