Write answers to the following questions for these compounds: SO2 (sulfur in the middle with the two oxygens attached to it) C2H2 (carbons attached to each other with one hydrogen attached to each carbon CO2 (carbon in the middle with two oxygens attached to it). 1. determine the number of valence electrons for each compound 2. draw a Lewis structure and include non-bonding electrons if necessary 3. write the electron group geometry and molecular geometry terms

Write answers to the following questions for these compounds: SO2 (sulfur in the middle with the two oxygens attached to it) C2H2 (carbons attached to each other with one hydrogen attached to each carbon CO2 (carbon in the middle with two oxygens attached to it). 1. determine the number of valence electrons for each compound 2. draw a Lewis structure and include non-bonding electrons if necessary 3. write the electron group geometry and molecular geometry terms

Introductory Chemistry: An Active Learning Approach

6th Edition

ISBN:9781305079250

Author:Mark S. Cracolice, Ed Peters

Publisher:Mark S. Cracolice, Ed Peters

Chapter13: Structure And Shape

Section: Chapter Questions

Problem 68E: Classify each of the following statements as true or false: a Molecular geometry around an atom may...

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Classify each of the following statements as true or false: a Molecular geometry around an atom may or may not be the same as electron-pair geometry around the atom. b Electron pair geometry is the direct effect of molecular geometry. c If the geometry of a molecule is linear, the molecule must have at least one double bond. d A molecule with a double bond cannot have trigonal pyramidal geometry around the double bonded atom. e A CO2 molecule is linear, but an SO2 molecule is bent. f A molecule is polar if it contains polar bonds. g A molecule with a central atom that has one lone pair of electrons is always polar. h A molecule with a central atom that has two lone pairs and two bonded pairs of electrons is always polar. i Carbon atoms normally form four bonds. j Hydrogen atoms never form double bonds.
a) Draw a VSEPR diagram using the information below including all bond dipoles, the overall dipole, and any bond angles. b) What is the name of the molecular shape/molecular geometry for your molecule? c) Explain if your molecule is polar or non-polar. Information: Number of central atoms = 1 Number of other atoms surrounding the central atom = 4 Number of lone pairs surrounding the central atom = 1 The central atom is less electronegative than the surrounding atoms.
1. For each molecule and ion below, indicate the total number of valence electrons. Based on that number of electrons, draw a valid Lewis structure.2. Use VSEPR theory to determine the electron arrangement and the geometry of the molecule around the central atom(s). A table of geometries is attached.3. Build the molecule using the molecular models provided in the lab. Sketch your model well enough to show the geometry. Include bond angles.4. Using your understanding of electronegativity and its trends in the Periodic Table, determine if polar bonds exist in the molecule.5. Using bond polarity and molecular shape, determine if the molecule has an overall dipole. If all the bonds are nonpolar, the molecule is nonpolar. If polar bonds are present, then consider the shape to determine if the molecule has an overall dipole.
Answer each of the following questions for ClF3. (a) total valence electron count. (b) the Lewis structure. (c) the arrangement (or shape) of the electron grouping (includes lone pairs). (d) ideal bond angle. (e) actual molecular geometry (may be the same or different than answer (c). (f) actual bond angles (may use > or< symbols where appropriate).
Which statement about VSEPR theory is not correct? Select one: a. The molecular shape or geometry is determined by the positions of the lone pairs in the molecule. b. The steric number has five values from 2 to 6. c. The steric number of a central atom is the sum of the number of bonds around the atom plus the number of electrons in lone pairs pairs d. The electron-pair geometry is determined by the positions of the bonds and lone pairs in a molecule. e. In VSEPR theory, the shape or geometry of a molecule is determined by electron-electron repulsion.
Please draw the following Lewis structures (there are three). For each structure please identify the following. The total number of valence electrons (show work) A drawing of the correct Lewis structure The geometry of the molecule (required: give a one sentence justification of the geometry) The shape of the molecule (required: give a one sentence justification of the shape) Determine if the overall molecule is polar (required: give a one sentence justification of this answer) draw a Lewis structure and identify valence electrons, geometry, and shape. the three molecules are: TeI2Please enter in the total number of valence electrons for TeI2: A molecule composed of atom A with 5 valence electrons, and atom B with 7 valence electrons, and a formula of AB3. The AB bond is a polar bond.Please enter in the geometry of AB3: PF4+ (notice the positive charge)Please enter in the shape of PF4+:
Draw the Lewis structure for SeCI2 (selenium dichloride), then answer all of the following questions. For those questions in which a numerical response is required, express your answer with an integer (0, 1, 2, 3 etc.). a) Provide the symbol for the central element. This answer is case-sensitive. b) How many lone pair of electrons are surrounding the central element? c) How many lone pair of electrons in total are present in this molecule? d) How many non-bonding electrons are there in total in this molecule? e) How many electrons are being shared in total? f) How many single bonds are present in this molecule? g) How many double bonds are present in this molecule? h) How many triple bonds are present in this molecule?
Draw the Lewis structure for PBrI2, then answer all of the following questions. For those questions in which a numerical response is required, express your answer with an integer (0, 1, 2, 3 etc.). a) Provide the symbol for the central element. This answer is case-sensitive. b) How many lone pair of electrons are surrounding the central element? c) How many electrons are being shared in total? d) How many lone pair of electrons in total are present in this molecule? e) How many non-bonding electrons are there in total in this molecule? f) How many single bonds are present in this molecule? g) How many double bonds are present in this molecule? h) How many triple bonds are present in this molecule?
For each of the following molecules Determine the Steric Number around the central atom = number of atoms + lone pairs Determine the geometry of these electron pairs (including the lone pairs) Determine the molecular geometry by ignoring the lone pairs. Draw a 3D sketch of the molecule and make a model. O3 CH3OH ClO2- ICl4- COCl2 PCl6- GaCl3 HCCH ClF5
1. Draw the Lewis dot structure for HCOOH. (Hint: make the atom atom connectivity H-C-O-H, put in extra O on C) Based on your structure answer the following questions around the C. what is the electronic geometry? what is the molecular geometry? 2. Draw the Lewis dot structure for CH3NH2. (Hint: make the atom atom connectivity C-N-H) Based on your structure answer the following questions around the N. what is the electronic geometry? what is the molecular geometry?
Draw the Lewis structure for BrF4- in the window below and then answer the questions that follow. What is the electron-pair geometry for Br in BrF4- ? What is the the shape (molecular geometry) of BrF4-? fill in the blank aaf78d029036f9f_1
1. Briefly explain in your own words why the bond angle increases as the number of electron groups decrease? 2. How does electron domain geometry differ from molecular geometry? Briefly explain in your own words. 3. Write a complete list of steps you will utilize to predict the electron-domain geometry for a given species using only the Lewis structure. The only information you are provided with is the molecular formula and the net charge.