Write Lewis structures for the following: (a) \(\mathrm{H}_{2} \mathrm{CO}\) (both \(\mathrm{H}\) atoms are bonded to \(\mathrm{C} ),(\mathbf{b}) \mathrm{H}_{2} \mathrm{O}_{2},(\mathbf{c}) \mathrm{C}_{2} \mathrm{F}_{6}\) (contains \(\mathrm{a} \mathrm{C}-\mathrm{C}\) bond), \((\mathbf{d}) \mathrm{AsO}_{3}^{3-},\) (e) \(\mathrm{H}_{2} \mathrm{SO}_{3}(\mathrm{H}\) is bonded to \(\mathrm{O})\) \((\mathbf{f}) \mathrm{NH}_{2} \mathrm{Cl}\)

Short Answer

Expert verified
The Lewis structures for the requested molecules are as follows: (a) H2CO: \(\mathrm{H-C=O}\) (b) H2O2: \(\mathrm{H-O-O-H}\) (c) C2F6: \(\mathrm{F^-\equiv F^-\equiv C-F^-\equiv F^-\equiv C-F^-\equiv F^-}\) (d) AsO3^3-: \(\mathrm{:O=As=O:}\) (e) H2SO3: \(\mathrm{O=C-OH}\) (f) NH2Cl: \(\mathrm{H-N-Cl}\)

Step by step solution

01

(Step 1: Total valence electrons)

For each molecule, find the total number of valence electrons. (a) H2CO: H has 1 valence electron; C has 4 valence electrons; O has 6 valence electrons. Total = (2x1) + 4 + 6 = 12 valence electrons. (b) H2O2: H has 1 valence electron; O has 6 valence electrons. Total = (2x1) + (2x6) = 14 valence electrons. (c) C2F6: C has 4 valence electrons; F has 7 valence electrons. Total = (2x4) + (6x7) = 46 valence electrons. (d) AsO3^3-: As has 5 valence electrons; O has 6 valence electrons; the 3- charge adds 3 more electrons. Total = 5 + (3x6) + 3 = 26 valence electrons. (e) H2SO3: H has 1 valence electron; S has 6 valence electrons; O has 6 valence electrons. Total = (2x1) + 6 + (3x6) = 26 valence electrons. (f) NH2Cl: N has 5 valence electrons; H has 1 valence electron; Cl has 7 valence electrons. Total = 5 + (2x1) + 7 = 14 valence electrons.
02

(Step 2: Draw skeleton structures)

Draw the skeleton structure for each molecule with a single bond between the atoms. (a) H2CO: `[H-C-H]` and place the O above the C atom. (b) H2O2: `[H-O-O-H]`. (c) C2F6: `[C-C]` with three F atoms around each C atom. (d) AsO3^3-: `[As]` with three O atoms around it. (e) H2SO3: `[S]` with three O atoms around it and one H atom attached to two of the O atoms. (f) NH2Cl: `[N]` with one H atom and one Cl atom placed around the N atom.
03

(Step 3: Distribute electrons)

Distribute the remaining valence electrons as lone pairs (LP) and complete the octets for each atom. (a) H2CO: `[H-C-H]` and place two LP on the O atom, and double bond between C and O. (b) H2O2: `[H-O-O-H]` and place two LP on each O atom. (c) C2F6: `[C-C]` with three F atoms around each C atom and add three LP to each F atom. (d) AsO3^3-: `[As]` with three O atoms around it, place three LP on each O atom and place a double bond between As and each O atom. (e) H2SO3: `[S]` with three O atoms around it, place three LP on each O atom, place two LP on the S atom, and place a double bond between S and one O atom. (f) NH2Cl: `[N]` with one H atom and one Cl atom placed around the N atom, add one LP to the N atom, and three LP to the Cl atom. These are the Lewis structures for the requested molecules.

Unlock Step-by-Step Solutions & Ace Your Exams!

  • Full Textbook Solutions

    Get detailed explanations and key concepts

  • Unlimited Al creation

    Al flashcards, explanations, exams and more...

  • Ads-free access

    To over 500 millions flashcards

  • Money-back guarantee

    We refund you if you fail your exam.

Over 30 million students worldwide already upgrade their learning with Vaia!

One App. One Place for Learning.

All the tools & learning materials you need for study success - in one app.

Get started for free

Most popular questions from this chapter

What is the Lewis symbol for each of the following atoms or ions? (a) \(\mathrm{K},\) (b) As, (c) \(\mathrm{Sn}^{2+},(\mathbf{d}) \mathrm{N}^{3-}\) .

Some chemists believe that satisfaction of the octet rule should be the top criterion for choosing the dominant Lewis structure of a molecule or ion. Other chemists believe that achieving the best formal charges should be the top criterion. Consider the dihydrogen phosphate ion, \(\mathrm{H}_{2} \mathrm{PO}_{4}^{-}\) , in which the \(\mathrm{H}\) atoms are bonded to \(\mathrm{O}\) atoms. (a) What is the predicted dominant Lewis structure if satisfying the octet rule is the top criterion? (b) What is the predicted dominant Lewis structure if achieving the best formal charges is the top criterion?

(a) Use Lewis symbols to represent the reaction that occurs between Ca and F atoms. (b) What is the chemical formula of the most likely product? (c) How many electrons are transferred? ( \(\mathbf{d} )\) Which atom loses electrons in the reaction?

(a) Using Lewis symbols, diagram the reaction between magnesium and oxygen atoms to give the ionic substance MgO. (b) How many electrons are transferred? (c) Which atom loses electrons in the reaction?

Consider the lattice energies of the following Group 2 \(\mathrm{A}\) compounds: \(\mathrm{Be} \mathrm{H}_{2}, 3205 \mathrm{kJ} / \mathrm{mol} ; \mathrm{MgH}_{2}, 2791 \mathrm{kJ} / \mathrm{mol}\) \(\mathrm{CaH}_{2}, 2410 \mathrm{kJ} / \mathrm{mol} ; \mathrm{SrH}_{2}, 2250 \mathrm{kJ} / \mathrm{mol} ; \mathrm{BaH}_{2}, 2121 \mathrm{kJ} / \mathrm{mol}\) (a) What is the oxidation number of \(\mathrm{H}\) in these compounds? (b) Assuming that all of these compounds have the same three-dimensional arrangement of ions in the solid, which of these compounds has the shortest cation-anion distance? (c) Consider BeH \(_{2} .\) Does it require 3205 kJ of energy to break one mole of the solid into its ions, or does breaking up one mole of solid into its ions release 3205 \(\mathrm{kJ}\) of energy? (d) The lattice energy of \(\mathrm{ZnH}_{2}\) is 2870 \(\mathrm{kJ} / \mathrm{mol}\) . Considering the trend in lattice enthalpies in the Group 2 \(\mathrm{A}\) compounds, predict which Group 2 \(\mathrm{A}\) element is most similar in ionic radius to the \(\mathrm{Zn}^{2+}\) ion.

See all solutions

Recommended explanations on Chemistry Textbooks

View all explanations

What do you think about this solution?

We value your feedback to improve our textbook solutions.

Study anywhere. Anytime. Across all devices.

Sign-up for free