
Interpretation:
The tetrahedron shape of CH4 molecule and the similarities with NH3 and H2O needs to be explained.
Concept introduction:
The Lewis structure of an organic compound represents the bonding of atoms with lone pairs (if any). It indicates the bonds with atoms and also the arrangement of atoms in a molecule.
Hybridization of an atom indicates the molecular geometry of a molecule. The formula to check the hybridization can be written as:
Hybridization = Number of sigma bonds + Number of lone pair
The molecular geometry of molecules with lone pair on central atom is given by the VSEPR theory.

Answer to Problem 9E
All these three molecules have the same type of hybridization and should have tetrahedral geometry but due to the presence of lone pairs on the central atom, the molecular geometry changes to a pyramidal and bent shape.
Explanation of Solution
For Lewis structure of CH4 molecule, calculate total number of valence electrons:
CH4 molecule = 4 electrons in C + 4 × 1 valence electrons in H = 8 electrons
Hybridization = Number of sigma bonds + Number of lone pair
Hybridization of C atom = 4 + 0 = 4 = sp3
Thus, with sp3 hybridization, the molecular shape must be tetrahedral and must be fit in a tetrahedron.
For Lewis structure of NH3 molecule, calculate total number of valence electrons:
NH3 molecule = 5 electrons in N + 3 × 1 valence electrons in H = 8 electrons
Hybridization = Number of sigma bonds + Number of lone pair
Hybridization of N atom = 3 + 1 = 4 = sp3
Thus, with sp3 hybridization, the molecular shape must be tetrahedral but due to the presence of lone pair on the central N atom, the geometry alters to trigonal pyramidal shape.
For Lewis structure of H2O molecule, calculate total number of valence electrons:
H2O molecule = 6 electrons in O + 1 × 2 valence electrons in H = 8 electrons
Hybridization = Number of sigma bonds + Number of lone pair
Hybridization of O atom = 2 + 2 = 4 = sp3
Thus, with sp3 hybridization, the molecular shape must be tetrahedral but due to the presence of two lone pairs on the central O atom, the geometry alters to a bent shape.
Although all these three molecules have same type of hybridization and should have tetrahedral geometry but due to presence of lone pairs on central atom, the molecular geometry changes to pyramidal and bent shape.
Chapter U2 Solutions
Living by Chemistry
Additional Science Textbook Solutions
Human Anatomy & Physiology (2nd Edition)
Human Physiology: An Integrated Approach (8th Edition)
Campbell Essential Biology with Physiology (5th Edition)
Campbell Biology: Concepts & Connections (9th Edition)
Microbiology with Diseases by Body System (5th Edition)
Chemistry: The Central Science (14th Edition)
- 4. Read paragraph 4.15 from your textbook, use your calculated lattice energy values for CuO, CuCO3 and Cu(OH)2 an explain thermal decomposition reaction of malachite: Cu2CO3(OH)2 →2CuO + H2O + CO2 (3 points)arrow_forwardPlease sirrr soollveee these parts pleaseeee and thank youuuuuarrow_forwardIII O Organic Chemistry Using wedges and dashes in skeletal structures Draw a skeletal ("line") structure for each of the molecules below. Be sure your structures show the important difference between the molecules. key O O O O O CHON Cl jiii iiiiiiii You can drag the slider to rotate the molecules. Explanation Check Click and drag to start drawing a structure. Q Search X G ©2025 McGraw Hill LLC. All Rights Reserved. Terms of Use F 3 W C 3/5arrow_forward
- 3. Use Kapustinskii's equation and data from Table 4.10 in your textbook to calculate lattice energies of Cu(OH)2 and CuCO3 (4 points)arrow_forward2. Copper (II) oxide crystalizes in monoclinic unit cell (included below; blue spheres 2+ represent Cu²+, red - O²-). Use Kapustinski's equation (4.5) to calculate lattice energy for CuO. You will need some data from Resource section of your textbook (p.901). (4 points) CuOarrow_forwardWhat is the IUPAC name of the following compound? OH (2S, 4R)-4-chloropentan-2-ol O (2R, 4R)-4-chloropentan-2-ol O (2R, 4S)-4-chloropentan-2-ol O(2S, 4S)-4-chloropentan-2-olarrow_forward
- ChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage LearningChemistryChemistryISBN:9781259911156Author:Raymond Chang Dr., Jason Overby ProfessorPublisher:McGraw-Hill EducationPrinciples of Instrumental AnalysisChemistryISBN:9781305577213Author:Douglas A. Skoog, F. James Holler, Stanley R. CrouchPublisher:Cengage Learning
- Organic ChemistryChemistryISBN:9780078021558Author:Janice Gorzynski Smith Dr.Publisher:McGraw-Hill EducationChemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage LearningElementary Principles of Chemical Processes, Bind...ChemistryISBN:9781118431221Author:Richard M. Felder, Ronald W. Rousseau, Lisa G. BullardPublisher:WILEY





