Draw Lewis structures for each of the following. Count valence electrons, then determine the number of REDS to select the molecular shape from the list. Use the AEN to determine the type of bonds, and to select the type of molecule from the list. v Do not put covalent bonds between metals and nonmetals. v Put brackets around anions to show both charge and quantity. v There are 3 pages. 1. Са(НСО»)2 calcium hydrogen carbonate Shape tetrahedral ругamidal bent trigonal planar linear diatomic monoatomic ions shape at the central 0 = type of molecule = Iype of Molecule nonpolar polar ionic 2. Co(HSO;)2 cobalt (II) hydrogen sulfite shape at the S = type of molecule = 3. (NH4)-CO3 ammonium carbonate shape at the C = type of molecule =

Draw Lewis structures for each of the following. Count valence electrons, then determine the number of REDS to select the molecular shape from the list. Use the AEN to determine the type of bonds, and to select the type of molecule from the list. v Do not put covalent bonds between metals and nonmetals. v Put brackets around anions to show both charge and quantity. v There are 3 pages. 1. Са(НСО»)2 calcium hydrogen carbonate Shape tetrahedral ругamidal bent trigonal planar linear diatomic monoatomic ions shape at the central 0 = type of molecule = Iype of Molecule nonpolar polar ionic 2. Co(HSO;)2 cobalt (II) hydrogen sulfite shape at the S = type of molecule = 3. (NH4)-CO3 ammonium carbonate shape at the C = type of molecule =

Living by Chemistry

2nd Edition

ISBN:9781464142314

Author:Angelica M. Stacy

Publisher:Angelica M. Stacy

ChapterU2: Smells: Molecular Structure And Properties

Section: Chapter Questions

Problem 3STP

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Use the Molecule Shape simulator (http://openstaxcollege.org/I/6MolecShape) to build a molecule. Starting with the central atom, click on the double bond to add one double bond. Then add one single bond and one lone pair. Rotate the molecule to observe the complete geometry. Name the electron group geometry and molecular structure and predict the bond angle. Then click the check boxes at the bottom and right of the simulator to check your answers.
Successive substitution of F atoms for H atoms in the molecule CH4 produces the molecules CH3F, CH2F2, CHF3, and CF4. a. Draw Lewis structures for each of the five molecules. b. Using VSEPR theory, predict the geometry of each of the five molecules. c. Specify the polarity (polar or nonpolar) for each of the five molecules.
The valence shell of an atom in a legitimate Lewis structure (see Figure 2.3) has what in commonwith the valence shell of a noble gas? (Noble gases are stable elements found in the last column ofthe periodic table, e.g., He, Ne, Ar, etc.)
Acrolein is the starting material for certain plastics. (a) Which bonds in the molecule are polar and which are nonpolar? (b) Which is the most polar bond in the molecule? Which atom is the partial negative end of this bond?
rite a Lewis structure for each of the following simple molecules. Show all bonding valence electron pairs as lines and all nonbonding valence electron pairs as dots. msp;a.GeH4c.NI3b.ICld.PF3
Complete a Lewis structure for the compound shown below, then answer the following questions. What are the predicted bond angles about the carbon and nitrogen atoms? How many lone pairs of electrons are present in the Lewis structure? How many double bonds are present?
Successive substitution of F atoms for H atoms in the molecule NH3 produces the molecules NH2F, NHF2, and NF3. a. Draw Lewis structures for each of the four molecules. b. Using VSEPR theory, predict the geometry of each of the four molecules. c. Specify the polarity (polar or nonpolar) for each of the four molecules.
For three simple molecules of your own choice, apply the rules for writing Lewis structures. Write your discussion as if you are explaining the method to someone who is not familiar with Lewis structures.
7.40 Why is it impossible for hydrogen to be the central atom in the Lewis structure of a polyatomic molecule?
Write Lewis structures that obey the octet rule (duet rule for H) for each of the following molecules. a. H2CO b. CO2 c. HCN Carbon is the central atom in all of these molecules.