A model for H,O is shown in the chem3D window. H2O has bent geometry. This geometry is sometimes called angular or V-shaped geometry.ball & stick+| labels-Rotate the molecule until you have a feeling for its three-dimensional shape. How many atoms are bonded to the central atom?Consider the bond angle at the central atom. What is the approximate numerical value of this angle?degrees.You could view this geometry as being derived from a trigonal planar molecule by removing one atom, or as being derived from a tetrahedral moleculeby removing two atoms. Which does the bond angle suggest?For practice, type in the name of the geometry of the molecule:

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Answered: A model for H2O is shown in the chem3D…

Organic Chemistry: A Guided Inquiry

2nd Edition

ISBN:9780618974122

Author:Andrei Straumanis

Publisher:Andrei Straumanis

Chapter2: Lewis Structures

Section: Chapter Questions

Problem 3E

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A model for SiH4 is shown in the chem3D window. SiH4 has tetrahedral geometry. ball & stick |+ labels Rotate the molecule until you have a feeling for its three-dimensional shape. How many atoms are bonded to the central atom? If you take any three of the outer atoms, what shape do they define? | Consider the bond angles at the central atom. Do they all have the approximately the same numerical value? What is the approximate numerical value of this angle? | degrees. Are all four positions about the central atom equivalent, or is one of them different from the other three. For practice, type in the name of the geometry of the molecule: Previous Next
A model for SCI2 is shown in the chem3D window. SCI₂ has bent geometry. This geometry is sometimes called angular or V-shaped geometry. ball & stick V + labels Rotate the molecule until you have a feeling for its three-dimensional shape. How many atoms are bonded to the central atom? Consider the bond angle at the central atom. What is the approximate numerical value of this angle? degrees. You could view this geometry as being derived from a trigonal planar molecule by removing one atom, or as being derived from a tetrahedral molecule by removing two atoms. Which does the bond angle suggest? For practice, type in the name of the geometry of the molecule:
A model for BClz is shown in the chem3D window. BC13 has trigonal planar geometry. This is sometimes called triangular planar geometry. ball & stick + labels Rotate the molecule until you have a feeling for its three-dimensional shape. How many atoms are bonded to the central atom? | Rotate the molecule and look at it edge on. Does the central atom lie in the plane defined by the other three atoms?| Consider the bond angles at the central atom. Do they all have approximately the same numerical value? [ What is the approximate numerical value of this angle? [ | degrees. For practice, type in the name of the geometry of the molecule: Previous Next
||| Predicting deviations from ideal bond angles Consider the perbromate (BrO4) : anion. What is the central atom? Enter its chemical symbol. How many lone pairs are around the central atom? What is the ideal angle between the bromine-oxygen bonds? Compared to the ideal angle, you would expect the actual angle between the bromine-oxygen bonds to be ... 0 口。 (choose one) (choose one) about the same bigger smaller
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Consider the molecule of furan. Its Lewis structure is shown. H X Is furan polar? If yes, consider which side of the molecule has partial negative charge and which - partial positive. Then, indicate the direction of the dipole moment relative to the molecule as shown. Non-polar, zero dipole moment. Polar, the dipole vector points along one of the C-O bonds. Polar, the dipole vector points along one of the C-H bonds. Polar, the dipole vector points along the vertical axis. Polar, the dipole vector points along the horizontal axis.
Draw the 2D and the 3D Lewis structure for each molecule. You do not need to show resonance structures here. Determine the electron pair geometry (EPG), the molecular geometry (MG), the bond angle (BA) around the central atom, and the hybridization of the central or bold atom. Circle the formula of any polar molecule. For molecules with more than one central atom (e.g. CH,CH,0H) give the structure around the bold atom. Molecule ЕPG Hyb (circle if polar) 2D Lewis Structure 3D Lewis Structure MG ВА CH,S GeO2 CF4
Draw the 2D and the 3D Lewis structure for each molecule. You do not need to show resonance structures here. Determine the electron pair geometry (EPG), the molecular geometry (MG), the bond angle (BA) around the central atom, and the hybridization of the central or bold atom. Circle the formula of any polar molecule. For molecules with more than one central atom (e.g. CH,CH,0H) give the structure around the bold atom. Molecule ЕPG Hyb (circle if 2D Lewis Structure 3D Lewis Structure MG polar) ВА CH2S GeO2 CF,
A model for BF3 is shown in the chem3D window. BF3 has trigonal planar geometry. This is sometimes called triangular planar geometry. ball & stick + labels Rotate the molecule until you have a feeling for its three-dimensional shape. How many atoms are bonded to the central atom? Rotate the molecule and look at it edge on. Does the central atom lie in the plane defined by the other three atoms? Consider the bond angles at the central atom. Do they all have approximately the same numerical value? What is the approximate numerical value of this angle? v degrees. For practice, type in the name of the geometry of the molecule:
Determine the Lewis structures of the following compounds, and determine which ones have dipole moments. For each molecule that has a dipole moment, draw a ball-and-stick model and include an arrow to indicate the direction of the dipole moment. * Your answer is incorrect. Write the Lewis structure of the CH ✔Draw Your Solution eTextbook and Medial Hint Your answer is incorrect. Write the Lewis structure of the CHCl3. Hint Draw Your Solution * Your answer is incorrect. Write the Lewis structure of the CH₂Cl₂. ✔Draw Your Solution Hint
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Consider the nitrogen trifluoride (NF3) molecule. What is the central atom? Enter its chemical symbol. How many lone pairs are around the central atom? What is the ideal angle between the nitrogen-fluorine bonds? Compared to the ideal angle, you would expect the actual angle between the nitrogen-fluorine bonds to be ... 0° (choose one) X

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