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Chapter 10: Q10.27P (page 406)

If you know the formula of a molecule or ion, what is the first step in predicting its shape?

Short Answer

Expert verified

The first step in predicting its shape is finding its outermost shell electron or valence shell.

Step by step solution

01

Lewis Structure

A Lewis structure can be defined as the basic structure of a molecule that used the valence electron of each atom involved.In Lewis鈥檚 structure, the smallest amountof electronegative atom is going to be the central atom. The Lewis structure is based on the valence shell electron of an atom. It can predict the number of bonds.

02

Shape prediction step

The shape predicting the first step of the molecule or ion is finding the outermost shell electron. If we know the valence shell electronthen we can find out how much electron molecule can donate or gain or can share with another molecule. On the behalf of the valence shell, we can find out with what number it can bond. The valence shell electron can find out by using electronic configurationbased on atomic number.

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Most popular questions from this chapter

Arrange the following ACln species in order of decreasing Cl-A-Cl bond angles:SCl2 ,data-custom-editor="chemistry" OCl2 ,role="math" localid="1656921147907" PCl3 ,SiCl4 ,data-custom-editor="chemistry" SiCl62-

Consider the following molecular shapes.

a.Which has the most electron pairs (both bonding and lone pairs) around the central atom?

b.Which has the most lone pairs around the central atom?

c.Do any have only bonding pairs around the central atom? A B C

Which of the following numbers of electron groups can give rise to a bent (V-shaped) molecule: two, three, four, five, six? Draw an example for each case, showing the shape classification (AXmEn) and the ideal bond angle.

Draw Lewis structures of all the important resonance forms of (a) HCO2- (H is attached to C); (b) HBrO4HOBrO3

Methane burns in oxygen to form carbon dioxide and water vapor. Hydrogen sulfide burns in oxygen to form sulfur dioxide and water vapor. Use bond energies (Table 9.2, p. 353) to determine the heat of each reaction per mole of O2 (assume Lewis structures with zero formal charges; BE ofS=O is 552 kJ/mol).
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