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Ch.9 - Molecular Geometry and Bonding Theories
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All textbooksBrown 14th EditionCh.9 - Molecular Geometry and Bonding TheoriesProblem 16

Chapter 9, Problem 16

Describe the bond angles to be found in each of the following molecular structures: (a) trigonal planar, (b) tetrahedral, (c) octahedral, (d) linear.

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Hi everyone here we have a question asking us for the following molecular geometries give the possible bond angles in each a linear b Trigano by pyramidal, C, square pyramidal and deep in so for linear, It has to have a bond angle of 180° for Trigana by Pierre middle. It can have angles of 90° 120° And 180° For square pyramidal. It can have bond angles of 90° Or 180°, and lastly for Ben, It has an angle of 0.5 degrees. And these are our answers. Thank you for watching. Bye.
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Textbook Question

(a) Boron trichloride 1BCl32 and the carbonate ion 1CO3 2- 2 are both described as trigonal. What does this indicate about their bond angles?

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(b) The PCl3 molecule is trigonal pyramidal, while ICl3 is T-shaped. Which of these molecules is flat?

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How does a trigonal pyramid differ from a tetrahedron so far as molecular geometry is concerned?
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(b) An AB4 molecule has two lone pairs of electrons on the A atom (in addition to the four B atoms). What is the electron-domain geometry around the A atom?

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Would you expect the nonbonding electron-pair domain in NCl3 to be greater or smaller in size than the corresponding one in PCl3?

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In which of the following molecules can you confidently predict the bond angles about the central atom, and for which would you be a bit uncertain? Explain in each case. (a) H2S, (b) BCl3, (c) CH3I, (d) CBr4, (e) TeBr4.

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