ORGANIC CHEM ALC&STU S/G&S W/MASTER CHE
8th Edition
ISBN: 9780134581583
Author: Bruice
Publisher: PEARSON
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Textbook Question
Chapter 1.4, Problem 21P
Which of the atoms in the molecular models in Problem 20 have
- a. three lone pairs?
- b. two lone pairs?
- c. one lone pair?
- d. no lone pairs?
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In C=C, there are ____ atoms bonded to each other. The geometry is ______. In single bond will have_____ bonded atoms for each carbon. The geometry is now________
Atom 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?
a. How many shared and unshared electrons are there in the structure?
b. how many shared and unshared pairs of electrons are in the structure?
c. Determine the total number of valence electrons in the structure.
Chapter 1 Solutions
ORGANIC CHEM ALC&STU S/G&S W/MASTER CHE
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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- Why is the geometric structure of a molecule important, especially for biological molecules?arrow_forward1. For each molecule and ion below, indicate the total number of valence electrons. Based on that number of electrons, draw a valid Lewis structure.2. Use VSEPR theory to determine the electron arrangement and the geometry of the molecule around the central atom(s). A table of geometries is attached.3. Build the molecule using the molecular models provided in the lab. Sketch your model well enough to show the geometry. Include bond angles.4. Using your understanding of electronegativity and its trends in the Periodic Table, determine if polar bonds exist in the molecule.5. Using bond polarity and molecular shape, determine if the molecule has an overall dipole. If all the bonds are nonpolar, the molecule is nonpolar. If polar bonds are present, then consider the shape to determine if the molecule has an overall dipole.arrow_forwardPropylene, C3H6,C3H6, is a gas that is used to form the important polymer called polypropylene. Its Lewis structure is (a) What is the total number of valence electrons in the propylene molecule? (b) How many valence electrons are used to make σσ bonds in the molecule? (c) How many valence electrons are used to make ππ bonds in the molecule? (d) How many valence electrons remain in nonbonding pairs in the molecule? (e) What is the hybridization at each carbon atom in the molecule?arrow_forward
- How can you convert CsCl into NaCl like structure?arrow_forwarda) how many total pairs of electrons does CF4 have? b) How many bonded pairs and how many lone pairs does CF4 have? c) What is the molecular shape and angle of CF4? d) what is the lewis structure for CF4?arrow_forwardFunctional Groups List the functional groups, what is the chemical formula for each and what are the characteristics of each? Draw the molecular structure for eacharrow_forward
- Apply to each moluecla: 1.) Draw the complete 3-D structure with respect to the central atom (s).2.) Draw the Lewis structure for another molecule or species with a different atomic arrangement. (If applicable)arrow_forwardConsider the carbon-oxygen bond in formaldehyde (CH2O) and carbon monoxide (CO). In which molecule is the CO bond shorter? In which molecule is the CO bond stronger?arrow_forwardescribe the type of bonding that exists in the Cl2(g)molecule. How does this type of bonding differ from that found in the HCl(g)molecule? How is it similar?arrow_forward
- How are single, double, and triple bonds similar? How do they differ?arrow_forwardConsider the molecular structures illustrated in the previous exercise. For each structure, give an example compound that has that arrangement of atoms.arrow_forwardHow does adding an atom affect the position and angles of existing atoms or lone pairs? How does adding a lone pair affect the position and angles of existing atoms and lone pairs? Is the effect of adding bonded atoms and lone pairs to the central similar? Explain your answer. Describe what is meant by the "Steric #". Explain the difference between the terms "Electron Geometry" and "Molecule Geometry". How does changing a bond to a double or triple bond affect the shape of the molecules? List the molecules in Part III where the real bond angles differ from the theoretical model values. Why do you think the values differ?arrow_forward
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