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Chapter 7: Q39 E (page 406)

The arrangement of atoms in several biologically important molecules is given here. Complete the Lewis structures of these molecules by adding multiple bonds and lone pairs. Do not add any more atoms.

Short Answer

Expert verified

The Lewis structure for the following are:

Step by step solution

01

Define Chemical Bonding

A chemical bond is a long-term attraction between atoms, ions, or molecules that allows chemical compounds to form.

02

Concept

The following are the steps to drawing a Lewis structure:

(1) First, determine the total number of valence electrons, then deduct one electron for each positive charge if it is a cation, or add one electron for each negative charge if it is an anion.

(2) Now, arrange the atoms around the core atom to form a skeletal structure for the molecule. The least electronegative atom is typically chosen as the center atom. Connect each atom to the core atom with a single bond now.

(3) Now, on all atoms save the center atom, distribute the remaining electrons as lone pairs to complete their octet. (With the exception of hydrogen, which only takes two electrons to complete its duplet.)

(4) Now, arrange the remaining electrons around the center atom.

(5) Now, if any atom's octet is not full, draw several bonds with the centre atom correspondingly.

03

Writing the Lewis structure

  1. The Lewis structure of Amino acid serine is:

04

Writing the Lewis structure

(b) The Lewis structure of urea is:


05

Writing the Lewis structure

(c) The Lewis structure of pyruvic acid is:


06

Writing the Lewis structure

(d) The Lewis structure of uracil is:


07

Writing the Lewis structure

(e) The Lewis structure of carbonic acid is:


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Most popular questions from this chapter

Write out the full electron configuration for each of the following atoms and for the monatomic ion found in binary ionic compounds containing the element: (a) \({\rm{Al}}\) (b) \({\rm{Br}}\) (c) \({\rm{Sr}}\) (d) \({\rm{Li}}\) (e) \({\rm{As}}\) (f) \({\rm{S}}\) .

Predict the electron pair geometry and the molecular structure of each of the following:

  1. \({\rm{IO}}{{\rm{F}}_{\rm{5}}}\)(I is the central atom)
  2. \({\rm{POC}}{{\rm{l}}_{\rm{3}}}\)(P is the central atom)
  3. \({\rm{C}}{{\rm{l}}_{\rm{2}}}{\rm{SeO}}\)(Se is the central atom)
  4. \({\rm{ClS}}{{\rm{O}}^{\rm{ + }}}\)(S is the central atom)
  5. \({{\rm{F}}_{\rm{2}}}{\rm{SO}}\)(S is the central atom)
  6. \({\rm{N}}{{\rm{O}}_{\rm{2}}}^{\rm{ - }}\)
  7. \({\rm{SiO}}_{\rm{4}}^{{\rm{4 - }}}\)

Which of the following atoms would be expected to form negative ions in binary ionic compounds and which would be expected to form positive ions:\({\rm{P, I, Mg, Cl, In, Cs, O, Pb, Co}}\)?

Methanol,\({{\text{H}}_{\text{3}}}{\text{COH}}\), is used as the fuel in some race cars. Ethanol,\({{\text{C}}_{\text{2}}}{{\text{H}}_{\text{5}}}{\text{OH}}\), is used extensively as motor fuel in Brazil. Both methanol and ethanol produce\({\text{C}}{{\text{O}}_{\text{2}}}\)and\({{\text{H}}_{\text{2}}}{\text{O}}\)when they burn. Write the chemical equations for these combustion reactions using Lewis structures instead of chemical formulas.

From their positions in the periodic table, arrange the atoms in each of the following series in order of increasing electronegativity: (a)\({\rm{As, H, N, P, Sb}}\)(b)\({\rm{Cl, H, P, S, Si}}\)(c)\({\rm{Br, Cl, Ge, H, Sr}}\)(d)\({\rm{Ca, H, K, N, Si}}\)(e)\({\rm{Cl, Cs, Ge, H, Sr}}\).
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