Organic Chemistry: A Guided Inquiry
2nd Edition
ISBN: 9780618974122
Author: Andrei Straumanis
Publisher: Cengage Learning
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Textbook Question
Chapter 1, Problem 5E
Consider the molecules
a. Draw the valence shell representation of each.
b. Predict the value of the XYX bond angle, and explain your reasoning.
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Fill in the table. Central atom is listed first. A. Write the number of valence electrons below the formulaB. Draw the Lewis structureC & D. Write the Electron Group Geometry and Molecular Shape NamesE. Write the bond angleF. Write the molecular polarity. "P" for polar and "NP" for nonpolar.
SpeciesValenceElectrons(1 pt.)
LewisStructure(2 pt.)
Electron PairGeometryName(1 pt.)
Molecular ShapeName (1 pts.)
BondAngle (1 pt.)
Molecular Polarity(1 pt.)
PO43-
NOBr
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What is the nature of the bonding in C3H₂F2, Is it polar?
A. Submit your drawing with dipole moments
B. Identify the molecules polarity
C. Identify the molecules geometries
Predicting deviations from ideal bond angles
Consider the nitrogen trifluoride (NF3) molecule.
What is the central atom? Enter its chemical symbol.
How many lone pairs are around the central atom?
What is the ideal angle between the nitrogen-fluorine
bonds?
Compared to the ideal angle, you would expect the
actual angle between the nitrogen-fluorine bonds to
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Chapter 1 Solutions
Organic Chemistry: A Guided Inquiry
Ch. 1 - (E) What does the number (+Z) at the center of...Ch. 1 - Prob. 2CTQCh. 1 - Prob. 3CTQCh. 1 - Prob. 4CTQCh. 1 - Prob. 5CTQCh. 1 - Prob. 6CTQCh. 1 - Prob. 7CTQCh. 1 - You hear a student from a nearby group say that...Ch. 1 - Use VSEPR to explain why the HBH bond angle of BH3...Ch. 1 - Both the HCH and HCO bond angles of H2CO...
Ch. 1 - Prob. 11CTQCh. 1 - Consider the following flat drawing of methane...Ch. 1 - Use VSEPR to assign a value of (close to) 109.5,...Ch. 1 - A student draws the picture of ammonia (NH3) in...Ch. 1 - Prob. 15CTQCh. 1 - How many central atoms does the molecule H2NCH3...Ch. 1 - Indicate the bond angle and shape about each...Ch. 1 - Explain how there can be two kinds of bent:...Ch. 1 - A student makes the following statement: “The...Ch. 1 - A student who missed this class needs to know how...Ch. 1 - Prob. 1ECh. 1 - Prob. 2ECh. 1 - Consider the incomplete valence shell...Ch. 1 - How many valence electrons does a neutral a. K...Ch. 1 - Consider the molecules AlCl3 (aluminum chloride)...Ch. 1 - Draw an example of a bent molecule with a bond...Ch. 1 - Label each atom marked with an arrow with the...Ch. 1 - a model of each of the following molecules: a....
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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
- Best Lewis Formula and Molecular Geometry A student writes the Lewis electron-dot formula for the carbonate anion, CO32, as a Does this Lewis formula obey the octet rule? Explain. What are the formal charges on the atoms? Try describing the bonding for this formula in valence bond terms. Do you have any difficulty doing this? b Does this Lewis formula give a reasonable description of the electron structure, or is there a better one? If there is a better Lewis formula, write it down and explain why it is better. c The same student writes the following resonance description for CO2: Is there something wrong with this description? (What would you predict as the geometries of these formulas?) d Is one or the other formula a better description? Could a value for the dipole moment help you decide? e Can you write a Lewis formula that gives an even better description of CO2? Explain your answer.arrow_forwardIn addition to CO, CO2, and C3O2, there is another molecular oxide of carbon, pentacarbon dioxide, C5O2, a yellow solid. (a) What is the approximate C-to-C-to-O bond angle in pentacarbon dioxide? (b) What is the approximate C-to-C-to-C bond angle in this compound?arrow_forwardConsider the following molecules: SiH4, PH3, H2S. In each case, a central atom is surrounded by four electron pairs. In which of these molecules would you expect the bond angle to be less than 109.5? Explain your reasoning.arrow_forward
- For the following molecules: A. XeO₂F2 (neutron diffraction experiment by Peterson, Willett and Huston.[¹] showed that F-Xe-F bond angle is 180°) B. CIF 3 (1) Draw the valid Lewis structure, identify the (2) molecular group geometry, (3) electron group geometry, (4) polarity of the bonds, (5) over-all polarity, (6) number of lone pairs, and (7) number of bonding pairs.arrow_forwardWhat are valid uses of dummy atoms? A. They are needed to define dihedral angles when three or more bonded atoms are in a straight line B. They are needed to define bond angles in linear distributions of atoms in a molecule C. They can help build highly symmetrical structures D. They are used when a molecule has very heavy atoms O a. A, D b. C, D О с. A, C O d. B, Darrow_forwardWhat are the angles a and b in the actual molecule of which this is a Lewis structure? H H C H a H C ^ b C a = 11° b=0° H -H Note for advanced students: give the ideal angles, and don't worry about small differences from the ideal that might be caused by the fact that different electron groups may have slightly different sizes. X 3arrow_forward
- 1. Consider the diatomic molecules ( molecules with 2 atoms ) in this exercise : O2, N2, Cl2, and HCl . Do you think a diatomic molecule can be any shape other than linear ? Explain . because They are only two alems 2. Look at the Lewis structure you drew for SCl2 and CS2 Both of these molecules are made up of three atoms but have different molecular geometries . a . How is the arrangement of electrons around the central atoms different ? Give the number of lone pairs and bonding groups around each central atom Based on your previous answer , explain why SCl2 can't be linear . c . Explain why one molecule is polar and the other is nonpolararrow_forwardThe caffeine molecule is shown below. Indicate the electron geometry AND the molecular shape around each of the indicated atoms (six answers in total). Be aware that the angles may not be drawn correctly in this Lewis structure.arrow_forward10. Each ball-and-stick model below shows the electron-pair and molecular geometry of a generic molecule. Explain what is wrong with each molecular geometry and provide the correct molecular geometry based on the number of lone and bonding pairs around the central atom. (a) (b) (c) 11. Draw the Lewis structure for acetamide (CH3CONH2) and determine the geometry about each interior atom. Experiments show that the geometry about the N atom in acetamide is nearly planar. Draw a resonance structure that can account for the planar geometry about the N atom.arrow_forward
- Give the correct electron and molecular geometries that correspond to each set of electron groups around the central atom of a molecule.a. four electron groups overall; three bonding groups and one lone pairb. four electron groups overall; two bonding groups and two lone pairsc. five electron groups overall; four bonding groups and one lone paird. five electron groups overall; three bonding groups and two lone pairse. five electron groups overall; two bonding groups and three lone pairsf. six electron groups overall; five bonding groups and one lone pairg. six electron groups overall; four bonding groups and two lone pairsarrow_forwardWhat are the angles a and b in the actual molecule of which this is a Lewis structure? H H H C H a a = C b = ⁰ C H Note for advanced students: give the ideal angles, and don't worry about small differences from the ideal that might be caused by the fact that different electron groups may have slightly different sizes. H Xarrow_forward1) Use the 3D structure below to determine whether BH2CI is polar. To do this, you must use arrows to indicate polar bonds, and either use an arrow to indicate the net dipole moment or state that the molecule is non-polar. Cl B H.arrow_forward
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