Chemistry 10 Dr. Scholefield Chapter 10 Worksheet Homework is not collected or graded, but should be worked on seriously every week. Ions and Ionic Bonding 1. Why do all alkaline earth metals form cations with a +2 charge? Why not a –1 or a +3 charge? 2. Write complete electron configurations for the following ions: S-2 Rb+1 C-4 Al+3 Which noble gases have the same electron configurations as these ions? Which of these ions is larger than its parent atom? Which of these ions is smaller than its parent atom? 3. Write an equation using Lewis dot symbols showing the formation of sodium oxide from sodium and oxygen atoms. How many electrons are transferred? 4. Write an equation using Lewis dot symbols showing the formation of calcium phosphide from calcium and phosphorus atoms. How many electrons are transferred? Covalent Bonding 5. Consider the following Lewis structure for a molecule of formic acid: CO••••HO••••H a. How many valence electrons total are represented by this structure? b. How many valence electrons are being used for bonding? How many valence electrons are not involved in bonding? How many valence electrons are used in the double bond? c. Looking at this structure, can you identify any exceptions to the octet rule? If yes, describe the exception(s) and explain why it is an exception.6. Complete the following: A polar bond results when covalently bonded atoms share their valence electrons equally / unequally because the bonding atoms have the same / different electronegativities. A non-polar bond results when covalently bonded atoms share their valence electrons equally / unequally because the bonding atoms have the same / different electronegativities. 7. Determine whether the following molecules contain polar or non-polar bonds. If the bonds are polar, add δ- and δ+ symbols on the applicable atoms, as well as arrows on the bonds in the correct directions. S S C OO•••••••• SHH•••• 8. Which of the following bonds is the most polar? Explain your response. O–F N–F C–F H–F 9. Complete the following tables for each of the molecules provided. Lewis structures should clearly show bond electron pairs as lines and lone electron pairs as pairs of dots. Show resonance structures if appropriate. a. AsBr3 Resonance: Yes No Total # of Valence Electrons: Molecular Shape: Bond Angles: Lewis Structure Molecular Polarity: Polar Non-polar b. SO3 Resonance: Yes No Total # of Valence Electrons: Molecular Shape: Bond Angles: Lewis Structure Molecular Polarity: Polar Non-polar c. IO2-1 Resonance: Yes No Total # of Valence Electrons: Molecular Shape: Bond Angles: Lewis Structure Molecular Polarity: Polar Non-polard. SiHCl3 Resonance: Yes No Total # of Valence Electrons: Molecular Shape: Bond Angles: Lewis Structure Molecular Polarity: Polar Non-polar e. HOCN (connected in a line in the order given) Resonance: Yes No Total # of Valence Electrons: Molecular Shape: Bond Angles: Lewis Structure Molecular Polarity: Polar Non-polar f. OCS Resonance: Yes No Total # of Valence Electrons: Molecular Shape: Bond Angles: Lewis Structure Molecular Polarity: Polar Non-polar g. NO+1 Resonance: Yes No Total # of Valence Electrons: Molecular Shape: Bond Angles: Lewis Structure Molecular Polarity: Polar Non-polar h. OF2 Resonance: Yes No Total # of Valence Electrons: Molecular Shape: Bond Angles: Lewis Structure Molecular Polarity: Polar Non-polari. C2H4 Resonance: Yes No Total # of Valence Electrons: Molecular Shape: Bond Angles: Lewis Structure Molecular Polarity: Polar Non-polar j. PO3-3 Resonance: Yes No Total # of Valence Electrons: Molecular Shape: Bond Angles: Lewis Structure Molecular Polarity: Polar
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