Chemistry In Focus
6th Edition
ISBN: 9781305084476
Author: Tro, Nivaldo J., Neu, Don.
Publisher: Cengage Learning
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Textbook Question
Chapter 5, Problem 30E
Draw a Lewis structure and use VSEPR theory to determine the geometry of each molecule. If the molecule has more than one central atom, indicate the geometry about each of these and draw the three-dimensional structure.
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The compound XeCl2F2 can exist in two different forms. One form is polar and the other form is non-polar. Draw a valid Lewis structure of XeCl2F2. Then, draw two 3-dimensional representations of this molecule (including all lone pairs); one that shows the polar form with a correct dipole arrow and the other that shows the non-polar form of the molecule.
Chapter 5 Solutions
Chemistry In Focus
Ch. 5 - Drawing Lewis Structures for Ionic Compounds Draw...Ch. 5 - Using Lewis Structures to Determine the Correct...Ch. 5 - Prob. 5.3YTCh. 5 - Prob. 5.4YTCh. 5 - Drawing Lewis Structures for Covalent Compounds...Ch. 5 - Prob. 5.6YTCh. 5 - Prob. 5.7YTCh. 5 - Prob. 5.8YTCh. 5 - Prob. 5.9YTCh. 5 - Determining if a Molecule Is Polar Is SCl2 a polar...
Ch. 5 - Based on the Lewis structures for hydrogen and...Ch. 5 - Prob. 2SCCh. 5 - Prob. 3SCCh. 5 - Prob. 4SCCh. 5 - Prob. 5SCCh. 5 - Prob. 6SCCh. 5 - Prob. 7SCCh. 5 - Why is salt, NaCl, relatively harmless even though...Ch. 5 - If sodium is dropped into water, a loud fizzing...Ch. 5 - Explain ionic bonding according to Lewis theory.Ch. 5 - Prob. 4ECh. 5 - Prob. 5ECh. 5 - Prob. 6ECh. 5 - Draw electron dot structures for the following...Ch. 5 - Explain VSEPR theory. According to this theory,...Ch. 5 - Prob. 9ECh. 5 - Prob. 10ECh. 5 - In what ways is water unique? What about the water...Ch. 5 - What is the difference between a polar and a...Ch. 5 - Why do polar molecules have a greater tendency to...Ch. 5 - Prob. 14ECh. 5 - Lewis Structures for Atoms Draw Lewis structures...Ch. 5 - Draw Lewis structures for each of the following...Ch. 5 - Ionic Lewis Structures Draw a Lewis structure for...Ch. 5 - Draw a Lewis structure for each of the following...Ch. 5 - Draw a Lewis structure for each of the following...Ch. 5 - Draw a Lewis structure for each of the following...Ch. 5 - Covalent Lewis Structures Draw a Lewis structure...Ch. 5 - Draw a Lewis structure for each molecular...Ch. 5 - General Lewis Structures Determine whether each...Ch. 5 - Determine whether each compound is ionic or...Ch. 5 - What is wrong with each Lewis structure? Fix the...Ch. 5 - What is wrong with each Lewis structure? Fix the...Ch. 5 - Predicting the Shapes of Molecules Use VSEPR...Ch. 5 - Use VSEPR theory to determine the geometry of the...Ch. 5 - Draw a Lewis structure and use VSEPR theory to...Ch. 5 - Draw a Lewis structure and use VSEPR theory to...Ch. 5 - CF2Cl2 is a chlorofluorocarbon implicated in ozone...Ch. 5 - Chlorofluorocarbons have been banned because they...Ch. 5 - Determining Molecular Polarity Determine whether...Ch. 5 - Determine whether each molecule is polar:...Ch. 5 - Determine whether each molecule is polar:...Ch. 5 - Determine whether each molecule is polar:...Ch. 5 - Explain why water would be a gas at room...Ch. 5 - Prob. 38ECh. 5 - Prob. 39ECh. 5 - One of the observations that led G. N. Lewis to...Ch. 5 - G. N. Lewis developed a model for chemical bonding...Ch. 5 - The opening quote of this chapter states that Man...Ch. 5 - Draw a Lewis structure of the H2 molecule. If you...Ch. 5 - Prob. 44ECh. 5 - The Lewis structures for CH4,N2,andCO2, along with...Ch. 5 - CH3COCH3 (acetone) is a common laboratory solvent...
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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.arrow_forwarda. How many sticks did you need to make the skeleton structure?____________ b. How many sticks are left over? ____________ If your model is to obey the octet rule, each ball must have four sticks in it except for hydrogen atom balls, which need and can only have one. Each atom in an octet rule species is surrounded by four pairs of electrons. c. How many holes remain to be filled? ____________ Fill them with the remaining sticks, which represent nonbonding electron pairs. Draw the complete Lewis structure for NH2Cl using lines for bonds and pairs of dots for nonbonding electrons.arrow_forwardWithout actually drawing the Lewis structure, determine how many valence electrons are available for covalent bonding in each of the following molecules. a. SiH4 b. NCl3 c. H2S d. Cl2Oarrow_forward
- How many electron dots should appear in the Lewis structures for each of the following polyatomic ions? a. ClO b. ClO2 c. S22 d. NH4+arrow_forwardDraw Lewis structures to illustrate the bonding in the following molecules. In each case, there will be at least one multiple bond present in a molecule. a. COCl2: Both chlorine atoms and the oxygen atom are bonded to the carbon atom. b. C2H2Br2: The two carbon atoms are bonded to one another. Each carbon atom also has a bromine atom and a hydrogen atom bonded to it. c. C2N2: The two carbon atoms are bonded to one another, and each carbon atom also has a nitrogen bonded to it. d. CH2N2: A central carbon atom has both nitrogen atoms bonded to it. Both hydrogen atoms are bonded to one of the two nitrogen atoms.arrow_forwardTwo different molecules have the formula C2H2Cl2. Draw a Lewis structure for each molecule. (All the H and Cl atoms are bonded to carbon. The two carbon atoms are bonded to each other.)arrow_forward
- Draw Lewis structures to illustrate the bonding in the following molecules. In each case, there will be at least one multiple bond present in a molecule. a. C3H4: A central carbon atom has two other carbon atoms bonded to it. Each of the noncentral carbon atoms also has two hydrogen atoms bonded to it. b. N2F2: The two nitrogen atoms are bonded to one another, and each nitrogen atom also has a fluorine atom bonded to it. c. C2H3N: The two carbon atoms are bonded to each other. One of the carbon atoms has a nitrogen atom bonded to it, and the other carbon atom has three hydrogen atoms bonded to it. d. C3H4: A central carbon atom has two other carbon atoms bonded to it. One of the noncentral carbon atoms also has one hydrogen atom bonded to it, and the other one has three hydrogen atoms bonded to it.arrow_forwardWithout actually drawing the Lewis structure, determine how many valence electrons are available for covalent bonding in each of the following molecules. a. CBr4 b. SF2 c. PH3 d. OF2arrow_forwardClassify each bond as nonpolar covalent or polar covalent or state that ions are formed. (a) SH (b) PH (c) CF (d) CClarrow_forward
- A polyatomic ion is composed of C, N, and an unknown element X. The skeletal Lewis structure of this polyatomic ion is [XCN]. The ion X2 has an electron configuration of [Ar]4s23d104p6. What is element X? Knowing the identity of X, complete the Lewis structure of the polyatomic ion, including all important resonance structures.arrow_forwardCH4 Sketch the proper Lewis structure for this substance, according to the guidelines given in this class. Be sure to follow octet/duet rules for each atom and use the total number of valence electrons available. Calculate the difference in electronegativity (AEN) for the bonds, being sure to use our electronegativity values. The bonds in this molecule are polar Are all of the domains surrounding the central atom bonds? Yes Are the outer atoms the same? Yes Is the molecule symmetrical? Yes The molecule is polar because [Select ] <トarrow_forwardWrite the Lewis structure for the following molecule. State the electronic structure (shape based on electron pairs or bonds) AND the geometric structure (shape based on the atoms only). Include all valence electrons in your structure. State how many electrons are used to form covalent bonds in the molecule. Is the molecule polar? O2arrow_forward
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