Essential Organic Chemistry, Global Edition
3rd Edition
ISBN: 9781292089034
Author: Paula Yurkanis Bruice
Publisher: PEARSON
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Chapter 1, Problem 46P
List the bonds in order from most polar to least polar.
- a. C 8 O, C 8 F, C 8 N
- b. C 8 Cl, C 8 I, C 8 Br
- c. H 8 O, H 8 N, H 8 C
- d. C 8 H, C 8 C, C 8 N
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Rank the bonds from most polar to least polar : a. C¬O, C¬F, C¬N b. C¬Cl, C¬I, C¬Br c. H¬O, H¬N, H¬C d. C¬H, C¬C, C¬N
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)
Consider the compound nitrogen triflouride, NF3
a. What is the electronic geometry of the molecule?
b. What is the molecular geometry of the molecule?
c. How many are bonding electrons?
Chapter 1 Solutions
Essential Organic Chemistry, Global Edition
Ch. 1.1 - Oxygen has three isotopes, 16O, 17O, and 18O. The...Ch. 1.2 - Prob. 2PCh. 1.2 - How many valence electrons do chlorine, bromine,...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?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 - After examining the potential maps for LiH, HF,...Ch. 1.4 - An atom with a formal charge does not necessarily...
Ch. 1.4 - Prob. 12PCh. 1.4 - a. Draw two Lewis structures for C2H6O. b. Draw...Ch. 1.4 - Draw the lone-pair electrons that are not shown in...Ch. 1.4 - Prob. 16PCh. 1.4 - Which of the atoms in the molecular models in...Ch. 1.4 - Prob. 18PCh. 1.7 - What orbitals are used to form the 10 sigma bonds...Ch. 1.9 - Put a number in each of the blanks: a. ___ s...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. 25PCh. 1.13 - a. Predict the relative lengths and strengths of...Ch. 1.13 - Prob. 28PCh. 1.14 - Which of the bonds in a carbonoxygen double bond...Ch. 1.14 - Caffeine is a natural insecticide, found in the...Ch. 1.14 - a. What is the hybridization of each of the carbon...Ch. 1.14 - Prob. 33PCh. 1.14 - Describe the orbitals used in bonding and the bond...Ch. 1.15 - Account for the difference in the shape and color...Ch. 1.15 - Which of the following molecules would you expect...Ch. 1 - Draw a Lewis structure for each of the following...Ch. 1 - Prob. 38PCh. 1 - What is the hybridization of all the atoms (other...Ch. 1 - Prob. 40PCh. 1 - Draw the condensed structure of a compound that...Ch. 1 - Prob. 42PCh. 1 - Prob. 43PCh. 1 - Draw a Lewis structure for each of the following...Ch. 1 - Prob. 45PCh. 1 - List the bonds in order from most polar to least...Ch. 1 - What is the hybridization of the indicated atom in...Ch. 1 - Write the Kekul structure for each of the...Ch. 1 - Assign the missing formal charges.Ch. 1 - Predict the approximate bond angles for the...Ch. 1 - Prob. 51PCh. 1 - a. Which of the indicated bonds in each compound...Ch. 1 - In which orbitals are the lone pairs in nicotine?...Ch. 1 - Draw the missing lone-pair electrons and assign...Ch. 1 - Rank the following compounds from highest dipole...Ch. 1 - Prob. 56PCh. 1 - a. Which of the species have bond angles of 109.5?...Ch. 1 - Prob. 58PCh. 1 - Sodium methoxide (CH3ONa) has both ionic and...Ch. 1 - a. Why is a H 8 H bond (0.74 ) shorter than a C 8...Ch. 1 - Which compound has a larger dipole moment, CHCl3...Ch. 1 - Which compound has a longer C 8 Cl bond?Ch. 1 - Prob. 63PCh. 1 - The following compound has two isomers. One isomer...
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- G. N. Lewis developed a model for chemical bonding that you have learned in this chapter. His theory was extremely successful and is used today at all levels of chemistry, from the introductory class to the research laboratory. Why was Lewis theory so successful?arrow_forwardWhich of the following has the bonds correctly arranged in order of increasing polarity? Be—F, Mg—F, N—F, O—F O—F, N—F, Be—F, Mg—F O—F, Be—F, Mg—F, N—F N—F, Be—F, Mg—F, O—F Mg—F, Be—F, N—F, O—Farrow_forward5)A) In which case is the bond polarity incorrect?a) δ+H–Fδ–b) δ+K–Oδ–c) δ+Mg–H δ–d) δ-Cl–Iδ+e) δ-Si–Sδ+ B) In the Lewis structure for SeF6, the central sulfur atom shares __________ electrons.a) 4b) 8c) 10d) 12e) None of the aboveC) Consider the following moleculesI. BF3II. CHBr3 (C is the central atom)III. Cl2IV. XeBr2V. PBr5VI. SCl4 Select the molecule(s) that fit the given statement. Which molecules violate the octet rule?A) I, II, IVB) I, II, III, IV, VIC) III, V, VID) I, IV, VIE) I, IV, V, VIarrow_forward
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