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Understanding Ionic and Covalent Bonds: Key Concepts in Molecular Chemistry

This text delves into the specifics of ionic and covalent bonding, discussing the transfer and sharing of electrons between atoms. It highlights the characteristics of resonance structures and the unique behavior of hydrogen in bond formation. The text compares the polarity and strength of CO and CF bonds, along with the properties of polar and nonpolar molecules. Additionally, it clarifies the shape of H2O and PH3, the distribution of valence electrons, and the energy dynamics when bonds form, providing a comprehensive overview of molecular chemistry.

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Understanding Ionic and Covalent Bonds: Key Concepts in Molecular Chemistry

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Presentation Transcript

  1. The Ionic bond exists between atoms that __________________ electrons.

  2. Donate and Accept

  3. The covalent bond is formed because of an attraction between __________________________.

  4. The negative valence electrons of one atom and the positive nucleus of another atom.

  5. A resonance structure is __________.

  6. Another possible Lewis Structure.

  7. ______________ can only form one bond EVER.

  8. Hydrogen

  9. Which bond is more polar, CO or CF? Explain how you know.

  10. CF, it has a higher electronegativity difference.

  11. Which bond is predicted to be stronger, CO or CF?Explain.

  12. CF, because of the higher electronegativity difference.

  13. Polar molecules can have nonpolar bonds. True or False?

  14. Usually false (as far as you’re concerned.)

  15. The shape of H2O is ________.

  16. Bent

  17. How many total valence electrons does CN- have?

  18. 4+5+1 = 10

  19. Label the partial positive and partial negative dipoles on the Si—S bond.

  20. Si-S

  21. What is the shape of PH3?

  22. Trigonal pyramidal

  23. Potential energy is the _________when a bond is formedand the atoms are stable.

  24. Potential energy is the LOWESTwhen a bond is formedand the atoms are stable.

  25. The bond energy is ______ when the bond length is ______.

  26. The bond energy is LARGER when the bond length is SMALLER.OR The bond energy is LESS when the bond length is GREATER.

  27. Explain why CO2 is either a polar or nonpolar molecule.

  28. Nonpolar.Even though the bondsare each polar covalent, the oxygen are equally spaced around carbon. This means the electrons are equally distributed throughout the molecule and there is no dipole.

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