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Understanding Chemical Bonding: Types, Examples, and Electronegativity

Explore the concept of chemical bonding, including types such as ionic bonding, examples like NaCl and H2O, and how electronegativity influences bond formation. Dive into dipole moments and polarity to deepen your understanding of this fundamental chemistry topic.

charleen-nigel
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Understanding Chemical Bonding: Types, Examples, and Electronegativity

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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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