Please answer all of the questions. Questions are in the image. 2. If the molecule has only one bond, determine polarity of the bond. Nonpolar bond, willgive nonpolar molecule and polar bond will give polar molecule.Examples:а. Н2b. HCI13. Molecules with more than one bondA. The molecule is symmetrical: If there are no lone pairs on the central atom, and if all thebonds to the central atom are the same, the molecule is nonpolar.Examples:1. СО22. BF33. CCI4 Steps to determine polarity of a molecule1- Draw the correct Lewis structure2- Determine shape of the molecule and the angle3- Determine polarity of different bonds in the molecule4- Look at overall molecular geometry to determine polarity of the moleculeRules for determining polarity of a molecule:

The Lewis structure of a molecule describes the bonding between the atoms in a molecule. The symbols…

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Chemistry

Please answer all of the questions. Questions are in the image

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 46E

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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.
Which molecule is nonpolar and contains a nonpolar covalent bond? a.F2 b.HI c.KCl d.NH3
Indicate whether each of the following molecules is polar or nonpolar. The molecular geometry is given in parentheses. a. PH2Cl (trigonal pyramidal with P at the apex) b. SO3 (trigonal planar with S in the center position) c. CH2Cl2 (tetrahedral with C in the center position) d. CCl4 (tetrahedral with C in the center position)
a model of each of the following molecules: a. Based on your model, draw a bond-line representation with as many atoms as possible in the plane of the paper. Use wedge and dash bonds to represent any atoms that do not lie in the plane of the paper. b. Indicate each unique bond angle and the shape of each unique central atom.
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.
Determine the molecular geometry and polarity (polar or nonpolar) for carbon tetrafluoride. Fill in the boxes below.Molecular geometry: polarity:
1. Describe the difference between bond polarity and molecular polarity.
Define the difference between a polar and non-polar covalent bond. How do you determine if a molecule is polar or non-polar? Explain how a lone pair affects the bond angles of a substance
Which one of the following statements is false? a. ionic bonding results from the trnasfer of electrons from one atoms to another b. dipole moments result from the unequal distribution of electrons in a molecule c. the electrons in a polar bond are found nearer to the more electronegative element d. a molecule with very polar bonds can be nonpolar e. linear molecules cannot have a net dipole moment
A. Fluoromethane B. Methanol C. Chloromethane D. Water 1. Which molecule has the highest dipole moment? 2. Which molecule has the greatest bond angle relative to the electronegative atom? 3. Which molecule has the most optimal bond angle? 4. Which molecule is the most polar? 5. Which molecule contains the most electronegative atom?
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).
'Geometry and Polarity of Molecules'