Chemistry for Today: General, Organic, and Biochemistry
9th Edition
ISBN: 9781305960060
Author: Spencer L. Seager, Michael R. Slabaugh, Maren S. Hansen
Publisher: Cengage Learning
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Textbook Question
Chapter 4, Problem 4.104E
Which molecule below has a nonpolar bond in which the electrons are being shared equally?
a.
b.
c.
d.
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Propylene, 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?
Nitrogen trifluoride (NF3) is used in the electronics industry to clean surfaces. NF3 is also a potent greenhouse gas.
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Propylene, C3H6, is a gas that is used to form the importantpolymer called polypropylene. Its Lewis structure is
(a) What is the total number of valence electrons in the propylenemolecule? (b) How many valence electrons are usedto make s bonds in the molecule? (c) How many valenceelectrons are used to make p bonds in the molecule? (d) Howmany valence electrons remain in nonbonding pairs in themolecule? (e) What is the hybridization at each carbon atomin the molecule?
Chapter 4 Solutions
Chemistry for Today: General, Organic, and Biochemistry
Ch. 4 - Refer to the group numbers of the periodic table...Ch. 4 - Prob. 4.2ECh. 4 - Write abbreviated electronic configurations for...Ch. 4 - Write abbreviated electronic configurations for...Ch. 4 - Draw Lewis structure for the elements given in...Ch. 4 - Draw Lewis structures for the elements given in...Ch. 4 - Prob. 4.7ECh. 4 - Prob. 4.8ECh. 4 - Prob. 4.9ECh. 4 - Prob. 4.10E
Ch. 4 - Use the periodic table and predict the number of...Ch. 4 - Prob. 4.12ECh. 4 - Write a symbol for each of the following ions: a.A...Ch. 4 - Write a symbol for each of the following ions: a.A...Ch. 4 - Prob. 4.15ECh. 4 - Identify the element in period 3 that would form...Ch. 4 - Identify the noble gas that is isoelectronic with...Ch. 4 - Identify the noble gas that is isoelectronic with...Ch. 4 - Write equations to represent positive and negative...Ch. 4 - Prob. 4.20ECh. 4 - Write the formula for the ionic compound formed...Ch. 4 - Prob. 4.22ECh. 4 - Classify each of the following as a binary...Ch. 4 - Prob. 4.24ECh. 4 - Prob. 4.25ECh. 4 - Prob. 4.26ECh. 4 - Prob. 4.27ECh. 4 - Prob. 4.28ECh. 4 - Prob. 4.29ECh. 4 - Name the following binary ionic compounds: a. SrS...Ch. 4 - Name the following binary ionic compounds, using a...Ch. 4 - Name the following binary ionic compounds, using a...Ch. 4 - Prob. 4.33ECh. 4 - Prob. 4.34ECh. 4 - Prob. 4.35ECh. 4 - Write formulas for the following binary ionic...Ch. 4 - Prob. 4.37ECh. 4 - Prob. 4.38ECh. 4 - Identify the ions that would occupy lattice sites...Ch. 4 - Identify the ions that would occupy lattice sites...Ch. 4 - Calculate the mass in grams of positive ions and...Ch. 4 - Calculate the mass in grams of positive ions and...Ch. 4 - Prob. 4.43ECh. 4 - Prob. 4.44ECh. 4 - Represent the following reaction using Lewis...Ch. 4 - Prob. 4.46ECh. 4 - Prob. 4.47ECh. 4 - Represent the following molecules by Lewis...Ch. 4 - Draw Lewis structures for the following polyatomic...Ch. 4 - Prob. 4.50ECh. 4 - Prob. 4.51ECh. 4 - Prob. 4.52ECh. 4 - Predict the shape of each of the following...Ch. 4 - Prob. 4.54ECh. 4 - Prob. 4.55ECh. 4 - Prob. 4.56ECh. 4 - Use the periodic table and Table 4.4 to determine...Ch. 4 - Use Table 4.4 and classify the bonds in the...Ch. 4 - Use Table 4.4 and classify the bonds in the...Ch. 4 - Prob. 4.60ECh. 4 - On the basis of the charge distributions you drew...Ch. 4 - Prob. 4.62ECh. 4 - Prob. 4.63ECh. 4 - Prob. 4.64ECh. 4 - Show the charge distribution in the following...Ch. 4 - Prob. 4.66ECh. 4 - Prob. 4.67ECh. 4 - Prob. 4.68ECh. 4 - Prob. 4.69ECh. 4 - Prob. 4.70ECh. 4 - Prob. 4.71ECh. 4 - Prob. 4.72ECh. 4 - Prob. 4.73ECh. 4 - Prob. 4.74ECh. 4 - Prob. 4.75ECh. 4 - The covalent compounds ethyl alcohol and dimethyl...Ch. 4 - Prob. 4.77ECh. 4 - Prob. 4.78ECh. 4 - Prob. 4.79ECh. 4 - Prob. 4.80ECh. 4 - Prob. 4.81ECh. 4 - Prob. 4.82ECh. 4 - Suppose an element from group II(A)(2) and period...Ch. 4 - What would be the mass in grams of 0.200moles of...Ch. 4 - The ampere unit is used to describe the flow of...Ch. 4 - Prob. 4.86ECh. 4 - Prob. 4.87ECh. 4 - Prob. 4.88ECh. 4 - Prob. 4.89ECh. 4 - Prob. 4.90ECh. 4 - Prob. 4.91ECh. 4 - Prob. 4.92ECh. 4 - Prob. 4.93ECh. 4 - Prob. 4.94ECh. 4 - Prob. 4.95ECh. 4 - Noble gases: a.have low boiling points. b.are all...Ch. 4 - Prob. 4.97ECh. 4 - Name the type of bond that is formed when...Ch. 4 - Prob. 4.99ECh. 4 - A atom becomes an ion that possesses a negative...Ch. 4 - When calcium reacts with chlorine to form calcium...Ch. 4 - Prob. 4.102ECh. 4 - Prob. 4.103ECh. 4 - Which molecule below has a nonpolar bond in which...Ch. 4 - What is the correct formula for bismuth (III)...Ch. 4 - Which of the following species will combine with a...Ch. 4 - What type of bond is created when bromine and...Ch. 4 - The parts of an atom directly involved in ionic...Ch. 4 - In forming an ionic bond with an atom of chlorine,...Ch. 4 - In bonding, what would happen between the...Ch. 4 - Which compound contains a bond with no ionic...Ch. 4 - Prob. 4.112ECh. 4 - Which molecule is nonpolar and contains a nonpolar...Ch. 4 - Which of the following is a nonpolar covalent...Ch. 4 - Prob. 4.115ECh. 4 - Prob. 4.116E
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- 1.1 Define electronegativity and explain why electronegativity increases with atomic number within a period of the Periodic Table. 1.2 Describe the type of bonding that exists in F2 (g) molecule. How does this type of bonding differ from that found in the HF (g) molecule? 1.3 Define hydrogen bonding using examples. 1.4 PH3 and NH3 moleculea are the same shape but the molecules are non-polar and polar respectively. Explain why this is so. 1.5 Give an example of molecule that has a coordinate covalent bond. 1.6 Draw a Lewis structure for each of the following molecules of ions: a) HF3 b) CIO3-arrow_forwardIdentify the molecules with a dipole moment: (a) SF4 (b) CF4 (c) Cl2CCBr2 (d) CH3Cl (e) H2COarrow_forwardWhy are all diatomic molecules linear, regardless of the number of valence electron pairs on the atoms involved?arrow_forward
- Chlorofluorocarbons have been banned because they cause ozone depletion. The main replacements are hydrofluorocarbons, such as CF3CFH2. Draw a Lewis structure for CF3CFH2, determine its geometry, make a sketch of the molecule, and determine whether it is polar. (The two carbons are bonded to each other in the middle of the molecule, and the other atoms are bound to the two central carbon atoms.)arrow_forwardIdentify the electron pair geometry and the molecular structure of each of the following molecules or ions: (a) IF6+ (b) CF4 (c) BF3 (d) SiF5 (e) BeCl2arrow_forward7.97 Consider the structure shown below for as well as any other important resonance structures. (a) What is the expected O—N—O bond angle in this structure? (b) The molecule contains N—O bonds of two different lengths. How many sborter N—O bonds would be present?arrow_forward
- a Carbonyl fluoride, COF2, is an extremely poisonous gas used in organofluorine synthesis. Give the valence bond description of the carbonyl fluoride molecule. (Both fluorine atoms are attached to the carbon atom.) b Nitrogen, N2, makes up about 80% of the earths atmosphere. Give the valence bond description of this molecule.arrow_forwardWhich of the following molecules and ions contain polar bonds? Which of these molecules and ions have dipole moments? (a) CIF5 (b) CIO2 (c) TeCI42 (d) PCl3 (e) SeF4 (f) PH2 (g) XeF2arrow_forwardTwo variations of the octahedral geometry (see Table 8.7) are illustrated below. Which of the compounds in Exercises 91 and 92 have these molecular structures? PF5, SF4, ClF3 and Br3 SF6, ClF5, and XeF4arrow_forward
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