Which statement is always true according to VSEPR theory? O The shape of a molecule is determined only by repulsions among nonbonding electron groups. O The shape of a molecule is determined by the polarity of its bonds. The shape of a molecule is determined only by repulsions among bonding electron groups. O The shape of a molecule is determined by repulsions among all electron groups on the central atom (or interior atoms, if there is more than one). 5¹300 Aa -

Which statement is always true according to VSEPR theory? O The shape of a molecule is determined only by repulsions among nonbonding electron groups. O The shape of a molecule is determined by the polarity of its bonds. The shape of a molecule is determined only by repulsions among bonding electron groups. O The shape of a molecule is determined by repulsions among all electron groups on the central atom (or interior atoms, if there is more than one). 5¹300 Aa -

Living by Chemistry

2nd Edition

ISBN:9781464142314

Author:Angelica M. Stacy

Publisher:Angelica M. Stacy

ChapterU2: Smells: Molecular Structure And Properties

Section: Chapter Questions

Problem 12STP

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7.30 The bond in HF is said to be polar, with the hydrogen carrying a partial positive charge. For this to be true, the hydrogen atom must have less than one electron around it. Yet the Lewis dot structure of HF attributes two electrons to hydrogen. Draw a picture of the electron density distribution for HF and use it to describe how the hydrogen atom can carry a partial positive charge. How can these two models of the HF bond (the electron density and the Lewis structure) seem so different and yet describe the same thing?
Acrolein is the starting material for certain plastics. (a) Which bonds in the molecule are polar and which are nonpolar? (b) Which is the most polar bond in the molecule? Which atom is the partial negative end of this bond?
Fill in the blanks in each line of the following table that involves characteristics of various bonds between nonmetals. The first line is already completed as an example.
Successive substitution of F atoms for H atoms in the molecule CH4 produces the molecules CH3F, CH2F2, CHF3, and CF4. a. Draw Lewis structures for each of the five molecules. b. Using VSEPR theory, predict the geometry of each of the five molecules. c. Specify the polarity (polar or nonpolar) for each of the five molecules.
hat does it mean to say that a bond is polar? Give two examples of molecules with polar bonds. Indicate in your examples the direction of the polarity.
Consider the following compounds: CO2, SO2, KrF2, SO3, NF3, IF3, CF4, SF4, XeF4, PF5, IF5, and SCl6. These 12 compounds arc all examples of different molecular structures. Draw the Lewis structures for each and predict the molecular structure. Predict the bond angles and the polarity of each. (A polar molecule has a net dipole moment, while a nonpolar molecule docs not.) See Exercises 115 and 116 for the molecular structures based on the trigonal bipyramid and the octahedral geometries.
Distinguish between the terms electronegativity versus electron affinity, covalent bond versus ionic bond, and pure covalent bond versus polar covalent bond. Characterize the types of bonds in terms of electronegativity difference. Energetically, why do ionic and covalcnt bonds form?
The molecules BF3, CF4, CO2, PF5, and SF6 are all nonpolar, even though they all contain polar bonds. Why?