ORGANIC CHEMISTRY-W/ACCESS >CUSTOM<
5th Edition
ISBN: 9781260014112
Author: SMITH
Publisher: MCG CUSTOM
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Textbook Question
Chapter 1, Problem 1.28P
What orbitals are used to form each bond in the following molecules?
a.
b.
c.
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Students have asked these similar questions
Determine the electron geometry, molecular geometry, and idealized bond angles for each molecule. In which cases do you expect deviations from the idealized bond angle?a. CF4 b. NF3 c. OF2 d. H2S
Which bonds allow for a large, bonded network to be more directional and why?
1. Sigma bonds
2. Pi bonds
Because
1. The orbitals overlap side-to-side to hold the bond in place.
2. The orbitals overlap end-to-end in several different directions.
3. Multiple of these bonds result in delocalized electrons.
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O 2,1
O2,2
O 1,3
O 1,2
O2,3
O 1,1
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For which of the following molecules will the electron-pair geometry be different than the molecular geometry?
Draw Lewis structure for each molecule and write the electron pair and molecular geometries for each one in a separate sheet.
a.
BH3
b.
H2O
c.
CH4
d.
CO
e.
NH4+
Chapter 1 Solutions
ORGANIC CHEMISTRY-W/ACCESS >CUSTOM<
Ch. 1 - While the most common isotope of nitrogen has a...Ch. 1 - Label each bond in the following compounds as...Ch. 1 - How many covalent bonds are predicted for each...Ch. 1 - Draw a valid Lewis structure for each species. a....Ch. 1 - Draw an acceptable Lewis structure for each...Ch. 1 - Prob. 1.6PCh. 1 - Draw a Lewis structure for each ion. a. CH3Ob....Ch. 1 - Prob. 1.8PCh. 1 - Draw Lewis structures for each molecular formula....Ch. 1 - Classify each pair of compounds as isomers or...
Ch. 1 - Prob. 1.11PCh. 1 - Prob. 1.12PCh. 1 - Prob. 1.13PCh. 1 - Draw a second resonance structure for each species...Ch. 1 - Prob. 1.15PCh. 1 - Prob. 1.16PCh. 1 - Prob. 1.17PCh. 1 - Prob. 1.18PCh. 1 - Using the principles of VSEPR theory, you can...Ch. 1 - Convert each condensed formula to a Lewis...Ch. 1 - Prob. 1.21PCh. 1 - Prob. 1.22PCh. 1 - Convert each skeletal structure to a complete...Ch. 1 - What is the molecular formula of quinine, the...Ch. 1 - Draw in all hydrogens and lone pairs on the...Ch. 1 - Prob. 1.26PCh. 1 - What orbitals are used to form each of the CC, and...Ch. 1 - What orbitals are used to form each bond in the...Ch. 1 - Determine the hybridization around the highlighted...Ch. 1 - The unmistakable odor of a freshly cut cucumber is...Ch. 1 - Prob. 1.31PCh. 1 - Rank the following atoms in order of increasing...Ch. 1 - Prob. 1.33PCh. 1 - Prob. 1.34PCh. 1 - Provide the following information about...Ch. 1 - Use the ball-and-stick model to answer each...Ch. 1 - Citric acid is responsible for the tartness of...Ch. 1 - Zingerone gives ginger its pungent taste. a.What...Ch. 1 - Assign formal charges to each carbon atom in the...Ch. 1 - Assign formal charges to each and atom in the...Ch. 1 - Prob. 1.41PCh. 1 - Prob. 1.42PCh. 1 - Prob. 1.43PCh. 1 - Draw all possible isomers for each molecular...Ch. 1 - 1.45 Draw Lewis structures for the nine isomers...Ch. 1 - Prob. 1.46PCh. 1 - Prob. 1.47PCh. 1 - Prob. 1.48PCh. 1 - Prob. 1.49PCh. 1 - Prob. 1.50PCh. 1 - Prob. 1.51PCh. 1 - Prob. 1.52PCh. 1 - Consider compounds A-D, which contain both a...Ch. 1 - Prob. 1.54PCh. 1 - Prob. 1.55PCh. 1 - 1.56 Consider the compounds and ions with curved...Ch. 1 - 1.57 Predict all bond angles in each...Ch. 1 - 1.58 Predict the geometry around each highlighted...Ch. 1 - Prob. 1.59PCh. 1 - Draw in all the carbon and hydrogen atoms in each...Ch. 1 - 1.61 Convert each molecule into a skeletal...Ch. 1 - Prob. 1.62PCh. 1 - Prob. 1.63PCh. 1 - Predict the hybridization and geometry around each...Ch. 1 - Prob. 1.65PCh. 1 - Ketene, , is an unusual organic molecule that has...Ch. 1 - Rank the following bonds in order of increasing...Ch. 1 - Prob. 1.68PCh. 1 - Two useful organic compounds that contain Cl atoms...Ch. 1 - Use the symbols + and to indicate the polarity of...Ch. 1 - Prob. 1.71PCh. 1 - Anacin is an over-the-counter pain reliever that...Ch. 1 - Answer the following questions about acetonitrile...Ch. 1 - Prob. 1.74PCh. 1 - 1.75 The principles of this chapter can be...Ch. 1 -
a. What is the hybridization of each N atom in...Ch. 1 - 1.77 Stalevo is the trade name for a medication...Ch. 1 - 1.78 and are two highly reactive carbon...Ch. 1 - 1.79 The N atom in (acetamide) is hybridized,...Ch. 1 - Prob. 1.80PCh. 1 - Prob. 1.81PCh. 1 - Prob. 1.82PCh. 1 - Prob. 1.83PCh. 1 - Prob. 1.84PCh. 1 - Prob. 1.85P
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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
- Among the following, which has the shortest bond and which has the longest: Li2, B2, C2, N2, O2?arrow_forwardIdentify the molecules with a dipole moment: (a) SF4 (b) CF4 (c) Cl2CCBr2 (d) CH3Cl (e) H2COarrow_forward7.85 Consider the molecule whose structure is shown below. (a) How many carbon atoms are sp3 hybridized? (b) What is the shape of the molecule around the carbon atom marked A? (c) What is the shape of the molecule around the carbon atom marked B?arrow_forward
- Which atomic orbitals overlap to form the C−O bond of dimethyl ether, (CH3)2O? A. C 2sp3 + O 2sp2 B. C 2sp2 + O 2p C. C 2sp2 + O 2sp2 D. C 2sp3 + O 2sp3arrow_forward4. Consider the structural changes that occur in the following molecules. According to Lewis and VSEPR theory, why do these changes occur? What are the ideal bond angles for each structure, and which are expected to be а. b. distorted? BH3 CH4 NH3 H20 HFarrow_forward3. In a pi bond, A. electron density lies along the internuclear axis. B. electron density lies above and below the internuclear axis. C. electrons are more dense than they are in sigma bonds. D. more than two electrons are involved in the bond. 4. The hybridization of the central atom in CIF3 is A. sp? B. sp C. sp'd D. sp?d? 5. Determine the formal charge on the nitrogen in the Lewis structure shown below. A. +1 В. -2 C.0 D. +2 : s=C-N:arrow_forward
- Which of the following compund has same molecular geometry and electron group geometry? A. H2O B. BrF3 C. NH3 D. SO2 E. NH4+arrow_forward4. Draw Lewis structures for the following molecules. Describe how the bond angles would bealtered based on the Lewis structure.a. CH2Sb. SCl2arrow_forwardWhich of the following is polar (possesses a dipole moment)? A. C6H6 B. CH4 C. H2S D. I2arrow_forward
- 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)arrow_forwarda. One of the two known binary compounds of xenon and oxygen is XeO3. A Lewis structure is shown here, which may or may not be complete. How many lone pairs should be present on the central Xe atom? b. What is the electron pair geometry around the Xe? c. What is the molecular geometry of XeO3? d. What hybrid orbitals does the Xe atom use?arrow_forward9. Show the dipole moment of each bond and then predict the overall molecule as either being polar or nonpolar? a. CH4 b. H2S c. PH3 d. SO3arrow_forward
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