Pearson eText Organic Chemistry -- Instant Access (Pearson+)
8th Edition
ISBN: 9780135213711
Author: Paula Bruice
Publisher: PEARSON+
expand_more
expand_more
format_list_bulleted
Concept explainers
Videos
Textbook Question
Chapter 1.9, Problem 32P
For each of the given species:
- a. Draw its Lewis structure.
- b. Describe the orbitals used by each carbon atom in bonding and indicate tbe approximate bond angles.
- 1. H2CO2
- 2. HCN
- 3. CCl4
- 4. H2CO3
Expert Solution & Answer
Want to see the full answer?
Check out a sample textbook solution
Students have asked these similar questions
1) What is the type of molecule? a. AX2E3 b. AX3E2 c. AX5 d. AX2E2
2) What is the molecular geometry of GL2-? a. Linear b. Trigonal Bypyramidal c. Bent or v-shaped d. Seesaw
3) What is the approx bond angle formed by L-G-L bond if the correct molecular geometry is followed? a. 180° b. 120° c. 109.5° d. 90°
4) Considering that L is more electronegative than G, and the en difference is 0.2, is the molecular polar?
5) What is the formal charge of G?
6) What is the formal charge of the labeled atom? (refer to the blue arrow)
For each of the given species:a. Draw its Lewis structure.b. Describe the orbitals used by each carbon atom in bonding and indicate the approximate bond angles.1. H2CO2 2. HCN 3. CC14 4. H2CO3
For each of the following,
a. Draw the lewis structure
b. Indicate the molecular geometry
c. Indicate the bond angles
1. PCI3
2. IBr4-
3. SeF4
4. NH2-
5. SCN-
6. SnCl5-
Chapter 1 Solutions
Pearson eText Organic Chemistry -- Instant Access (Pearson+)
Ch. 1.1 - Oxygen has three isotopes, 16O, 17O, and 18O. The...Ch. 1.1 - a. How many protons do the following species...Ch. 1.1 - Chlorine has two isotopes, 35Cl and 37Cl; 75.77%...Ch. 1.2 - Prob. 4PCh. 1.2 - a. Write the ground-state electronic configuration...Ch. 1.2 - Look at the relative positions of each pair of...Ch. 1.3 - a. Find potassium (K) in the periodic table and...Ch. 1.3 - Which bond is more polar? a. b. c. d.Ch. 1.3 - Which of the following has a. the most polar bond?...Ch. 1.3 - Use the symbols + and to show the direction of...
Ch. 1.3 - Explain why HCL has a smaller dipole moment than...Ch. 1.3 - After examining the potential maps for LiH, HF,...Ch. 1.4 - An atom with a formal charge does not necessarily...Ch. 1.4 - Prob. 16PCh. 1.4 - a. Draw two Lewis structure for C2H6O. b. Draw...Ch. 1.4 - Draw the lone-pair electrons that are not shown in...Ch. 1.4 - Prob. 20PCh. 1.4 - Which of the atoms in the molecular models in...Ch. 1.4 - Prob. 22PCh. 1.4 - Prob. 23PCh. 1.5 - Draw the following orbitals: a. 3s orbital b. 4s...Ch. 1.6 - Prob. 25PCh. 1.6 - Indicate the kind of molecular orbital (, , , or )...Ch. 1.7 - What orbitals are used to form the 10 sigma bonds...Ch. 1.7 - Explain why a bond formed by overlap of s orbital...Ch. 1.9 - Put n number in each of the blanks: a. __ s...Ch. 1.9 - For each of the given species: a. Draw its Lewis...Ch. 1.11 - Predict the approximate bond angles in a. the...Ch. 1.11 - According to the potential map for the ammonium...Ch. 1.12 - Prob. 35PCh. 1.13 - a. What are the relative lengths and strengths of...Ch. 1.13 - Prob. 38PCh. 1.14 - Describe the orbitals used in bonding and the bond...Ch. 1.15 - Which of the bond in a carbon-oxygen double bond...Ch. 1.15 - Would you expect a CC bond formed by sp2sp2...Ch. 1.15 - Caffeine is a natural insecticide found in the...Ch. 1.15 - a. What is the hybridization of each of the carbon...Ch. 1.15 - Predict the approximate bond angles for a. the CNC...Ch. 1.16 - What of the following molecules would you expect...Ch. 1.16 - Account for the difference in the shape and color...Ch. 1.16 - If the dipole moment of CH3F is 1.847 D and the...Ch. 1 - Draw a Lewis structure for each of the following:...Ch. 1 - Prob. 50PCh. 1 - What is the hybridization of all the atoms (other...Ch. 1 - Draw the condensed structure of a compound that...Ch. 1 - Predict the approximate bond angles: a. the CNH...Ch. 1 - Prob. 54PCh. 1 - Draw a Lewis structure for each of the following:...Ch. 1 - What is the hybridization of each of the carbon...Ch. 1 - Rank the bonds from most polar. a. CO, CF, CN b....Ch. 1 - Draw a Lewis structure for each of the following:...Ch. 1 - Prob. 59PCh. 1 - What is the hybridization of the indicated atom in...Ch. 1 - Predict the approximate bond angles for the...Ch. 1 - Prob. 62PCh. 1 - Draw the missing lone-pair electrons and assigns...Ch. 1 - a. Which of the indicated bonds in each molecule...Ch. 1 - For each of the following molecules, indicate the...Ch. 1 - Draw a Lewis structure for each of the following:...Ch. 1 - Prob. 67PCh. 1 - Rank the following compounds from highest dipole...Ch. 1 - In which orbitals are the lone pairs in nicotine?Ch. 1 - Prob. 70PCh. 1 - Prob. 71PCh. 1 - a. Which of the species have bond angles of 109.5?...Ch. 1 - Prob. 73PCh. 1 - Which compound has a larger dipole moment: CH3Cl...Ch. 1 - Prob. 75PCh. 1 - Explain why CH3Cl has a greater dipole moment than...Ch. 1 - a. Draw a Lewis structure for each of the...Ch. 1 - There are three isomers with molecular formula...
Knowledge Booster
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.Similar questions
- Why is the geometric structure of a molecule important, especially for biological molecules?arrow_forwardAtom A has 4 valence electrons. Atom Z has 6 valence electrons. For the AZ3-2 ion How many valence electrons are in the structure? b. How many single bonds are in the structure? c. How many double bonds are in the structure? d. How many triple bonds are in the structure? e. How many lone pairs are on the central atom in the structure? f. What is the shape of the structure? g. What are the bond angles of this ion?arrow_forward1. Draw the complete Lewis Structure for each. Then determine the electron pair geometry (EPG), make a 3-dimensional representation (drawing), and determine the molecular geometry (MG) for all of them. Determine whether each molecule is polar or non-polar. Formula Lewis structure EPG 3-D drawing MG polar? a. PF3 b. CH;F2 Cl3 d. SC4 e. XeF4arrow_forward
- A. CHF i. Best Lewis Structure B. HNO (H is connected to one of the O's) i. Best Lewis Structure ii. Electron geometry on the C atom ii. Electron geometry on the N atom iii. Approximate bond angles about the C atom iii. Approximate bond angles around the N atom v. Draw the shape with in and out wedges (as necessary) and dipole arrows around the C atom. v. Draw the shape with in and out wedges (as necessary) and dipole arrows around the N atom. vi. Is the molecule polar or nonpolar? vi. Is the molecule polar or nonpolar?arrow_forward8. For each molecular fomula, detem ine the electron pair geom etry (EPG), make a 3-dimensional representation, and determ ine the molecular geometry. Determine whether the molecule is polar or non- polar. All of these have central atoms surounded by term inal atom s/one pairs only. Formula A. CHF3 Lewis structure EPG 3-D drawing Mol Geom. Polar molecule? B. SF2arrow_forwardMolecular Formula SO₂ SiCl4 Total # of valence electrons CH₂Cl₂ Lewis Structure # of Electron Groups Bond Electron Geometry Angle Molecular Geometry QUESTION 1. Using the molecular model kit, make and compare the molecular models for CO₂, H₂O, and SO₂. Even though each molecule has 3 atoms, the molecular geometries (shapes) are very different. Explain why the shapes are different. on. -C Polar or Nonpolar Attractive Force O <arrow_forward
- Carbon ring structures are common in organic chemistry. Draw a Lewis structure for each carbon ring structure, including any necessary resonance structures.a. C4H8 b. C4H4 c. C6H12 d. C6H6arrow_forwardHow many lone pairs and double bonds are present in the Lewis Structure of a.Chlorite ion B. SO2arrow_forwardConsider the generic polyatomic ion XY3". Element X is the least electronegative. For neutral atoms, element X has 7 valence electrons and element Y has 6. The highest occupied principal energy level of the central atom is greater than 2. A. How many total valence electrons are in the molecule. B. Draw a BEST Lewis structure (i.e. a major resonance contributor) for this molecule. Show all valence electrons on your structure. C. If you haven't already, add the formal charge of each atom to the structure. Show at least one sample calculation for formal charge. D. Outline 4 short bullet points (~several words each) that explain why your structure from part B is the best one. Hint: think about what makes a valid structure and what makes a best structure. E. Perform a calculation to determine the average bond order between the X and Y atoms in your structure from part B. No credit will be given for just a number. F. Draw one more valid resonance structure other than the one from part B.…arrow_forward
- The formula for nitryl chloride is CINO2 (in which N is the central atom). a.Draw the Lewis structure for the molecule, including all resonance structures. b.What is the N-O bond order? c.Describe the electron-pair and molecular geometries and give values for all bond angles. d.What is the most polar bond in the molecule? Is the molecule polar? e.The computer program used to calculate electrostatic potential surfaces gave the following charges on atoms in the molecule: A =-0.03, B = -0.26, and C = +0.56. Identify the atoms A, B, and C. Are these calculated charges in accord with your predictions?arrow_forward12. Acetamide is a colorless, crystalline (sand-like) material. It is used in lacquers, explosives, and soldering flux, and as a stabilizer, plasticizer and solvent. H. -N-H acetamide a. Identify all sigma bonds and pi bonds. What is the total number of each in this molecule? b. Identify the molecular geometry of each central atom c. Draw the 3D Lewis structure for this compoundarrow_forwardDetermine if the structural formula below are acceptable Lewis structures for organic compounds. Point out the problems in cases where structure is invalid. CH3 CH;-N-CH-CH3 ČH3 A. This structure is correct because the valance of Nitrogen is complete. B. This is not a correct Lewis structure because Nitrogen can accommodate more atoms. C. This is not a correct Lewis structure because Nitrogen has a charge if it does not have three bonds. D. This is a correct Lewis structure.arrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
Introductory Chemistry: A FoundationChemistryISBN:9781337399425Author:Steven S. Zumdahl, Donald J. DeCostePublisher:Cengage Learning
Introductory Chemistry: A Foundation
Chemistry
ISBN:9781337399425
Author:Steven S. Zumdahl, Donald J. DeCoste
Publisher:Cengage Learning
Stoichiometry - Chemistry for Massive Creatures: Crash Course Chemistry #6; Author: Crash Course;https://www.youtube.com/watch?v=UL1jmJaUkaQ;License: Standard YouTube License, CC-BY
Bonding (Ionic, Covalent & Metallic) - GCSE Chemistry; Author: Science Shorts;https://www.youtube.com/watch?v=p9MA6Od-zBA;License: Standard YouTube License, CC-BY
General Chemistry 1A. Lecture 12. Two Theories of Bonding.; Author: UCI Open;https://www.youtube.com/watch?v=dLTlL9Z1bh0;License: CC-BY