Organic Chemistry (8th Edition)
8th Edition
ISBN: 9780134042282
Author: Paula Yurkanis Bruice
Publisher: PEARSON
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Textbook Question
Chapter 1.9, Problem 30P
Put n number in each of the blanks:
- a. __ s orbital and __ p orbitals form __ sp3 orbitals.
- b. __ s orbital and __ p orbitals form __ sp2 orbitals.
- c. __ s orbital and __ p orbitals form __ sp orbitals.
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Chapter 1 Solutions
Organic Chemistry (8th Edition)
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...
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- Compare the configurations below with two electrons located in p orbitals. Which would be the most stable (have the lowest energy)? Which would be the least stable? Explain your answers.arrow_forwardGive electron configurations according to the Bohr model for each of the following elements. Try to not use Figure 3.11, but instead determine the configuration based on your knowledge of the number of electrons in each atom and the maximum number of electrons in each Bohr orbit. Indicate which of these elements you expect to be the most reactive and the least reactive. a. B b. Si c. Ca d. F e. Ararrow_forwardWhich of the following statements is(are) true? a. The 2s orbital in the hydrogen atom is larger than the 3s orbital also in the hydrogen atom. b. The Bohr model of the hydrogen atom has been found to be incorrect. c. The hydrogen atom has quantized energy levels. d. An orbital is the same as a Bohr orbit. e. The third energy level has three sublevels, the s, p, and d sublevels.arrow_forward
- Your text describes the probability map for an s orbital using an analogy to the earth’s atmosphere. Explain this analogy.arrow_forwardHow many valence electrons do each of the following elements have, and what are the specific valence electrons for each element? a. Ca b.O c. element 117 d. In e. Ar f. Biarrow_forwardThe following are orbital diagrams for presumed ground-state atoms. Several, though, violate Paulis principle or Hunds rule Which of the these follow both Paulis principle and Hunds rule, and which violate one or the other (state whether Paulis principle or Hunds rule is violated)? a b c d earrow_forward
- The spectra of hydrogen and of calcium are shown in Figure 6.13. What causes the lines in these spectra? Why are the colors of the lines different? Suggest a reason for the observation that the spectrum of calcium is more complicated than the spectrum of hydrogen.arrow_forward• sketch the shapes of s and p orbitals and recognize orbitals by their shapes.arrow_forwardWhich of the following electron configurations correspond to an excited state? Identify the atoms and write the ground-state electron configuration where appropriate. a. 1s22s23p1 b. 1s22s22p6 c. 1s22s22p43s1 d. [Ar]4s23d54p1 How many unpaired electrons are present in each of these species?arrow_forward
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