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Chapter 10: Problem 148

Construct a concept map illustrating the connections between Lewis dot structures, the shapes of molecules, and polarity.

Short Answer

Expert verified
A concept map that connects Lewis dot structures, molecule shapes, and polarity would show that Lewis dot structure representation facilitates the understanding of molecular shapes via the VSEPR theory, and that the molecular geometry along with electronegativity differences helps in determining whether a molecule is polar or not.

Step by step solution

01

Connecting Lewis Dot Structures to Molecule Shapes

The shape of a molecule plays an important role in its reactivity. The shapes of molecules are primarily determined by the number of regions of electron density (which can be deduced from Lewis Structures) around the central atom. This is often explained using the VSEPR theory (Valence Shell Electron Pair Repulsion), which states that the electron groups around a central atom will adopt a geometry that minimizes the electron-electron repulsion.
02

Understanding the Concept of Polarity

Polarity in a molecule occurs as a result of an uneven distribution of charge. This uneven distribution could be due to difference in electronegativity of atoms and can also be influenced by the shape of the molecule. If the molecule is symmetrical, the charge may be evenly distributed and would hence be non-polar. If it's asymmetrical, then it would be polar. Polar molecules have a positive and a negative end, or poles.
03

Connecting Molecular Shapes to Polarity

The shape of a molecule can either stabilize or destabilize the uneven distribution of charge, leading to a polar or non-polar molecule. Molecules with symmetrical shapes, even with polar bonds, often become non-polar because the bond polarities cancel each other out. Conversely, molecules with asymmetrical shapes, even with non-polar bonds, may become polar if the distribution of atoms is uneven.

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Most popular questions from this chapter

One possibility for the electron-group geometry for seven electron groups is pentagonal-bipyramidal, as found in the IF \(_{7}\) molecule. Write the VSEPR notation for this molecule. Sketch the structure of the molecule, labeling all the bond angles.

Of the following species, the one with a triple covalent bond is (a) \(\mathrm{NO}_{3}^{-} ;\) (b) \(\mathrm{CN}^{-} ;\) (c) \(\mathrm{CO}_{2} ;\) (d) \(\mathrm{AlCl}_{3}\).

Use the VSEPR theory to predict the shape of (a) the molecule OSF \(_{2} ;\) (b) the molecule \(\mathrm{O}_{2} \mathrm{SF}_{2} ;\) (c) the ion \(\mathrm{SF}_{5}^{-} ;\) (d) the ion \(\mathrm{ClO}_{4}^{-} ;\) (e) the ion \(\mathrm{ClO}_{3}^{-}\).

Write Lewis structures for the following ionic compounds: (a) calcium chloride; (b) barium sulfide; (c) lithium oxide; (d) sodium fluoride.

Each of the following is either linear, angular (bent), planar, tetrahedral, or octahedral. Indicate the correct shape of (a) \(\mathrm{H}_{2} \mathrm{S} ;\) (b) \(\mathrm{N}_{2} \mathrm{O}_{4} ;\) (c) \(\mathrm{HCN} ;\) (d) \(\mathrm{SbCl}_{6}^{-}\); (e) \(\mathrm{BF}_{4}^{-}\)
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