Chemistry: An Introduction to General, Organic, and Biological Chemistry, Books a la Carte Plus Mastering Chemistry with Pearson eText -- Access Card Package (13th Edition)
13th Edition
ISBN: 9780134557335
Author: Karen C Timberlake
Publisher: PEARSON
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Textbook Question
Chapter 6.7, Problem 6.63PP
Using the periodic table, arrange the atoms in each of the following sets in order of increasing electronegativity.
a. Li, Na, K
b. Na, CI, P
c. Se, Ca, O
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In a covalent bond between two atoms, the more electronegative atom will attract more electron density toward itself, causing a polar bond. The more electronegative element is the negative pole, whereas the less electronegative element is the positive pole. The direction of the dipole is always toward the more electronegative element. This is often inflicated by an arrow, as shown in the figure. (Figure 1) The magnitude of the bond polarity is the difference in electronegativity values of the atoms. For example, in the molecule Cl2, the CICI bond is nonpolar because there is no difference in electronegativity between two atoms of the same element. In the CIBr molecule, However, the C1 Br bond is polar because Cl and Br have different electroneaativitv values. A CI I bond would be more polar than a C1 Br bond because there is a greater electronegativity difference between Cland I than between CI and Br.
Based on Linus Pauling's electronegativity scale, would H2S be considered a polar molecule?
Pick the best answer.
(a) No. It would technically be considered a non-polar molecule.
(b) No. Even though it contains polar bonds they are symmetrical and therefore H2S is non-polar.
(c) No. The electronegativity difference between H and S is so great that it would be considered an ionic compound.
(d) H2S violates the octet rule and therefore would not even exist
An unknown element M forms a chloride with the formula MCl3. This chloride compound was examined and found to have a trigonal pyramidal shape. Draw a Lewis structure for MCl3 that is consistent with this molecular geometry. Use your structure to propose an identity for the element M and explain how you have made your choice.
Chapter 6 Solutions
Chemistry: An Introduction to General, Organic, and Biological Chemistry, Books a la Carte Plus Mastering Chemistry with Pearson eText -- Access Card Package (13th Edition)
Ch. 6.1 - State the number of electrons that be must be lost...Ch. 6.1 - State the number of electrons that must be gained...Ch. 6.1 - State the number of electrons lost or gained when...Ch. 6.1 - Prob. 6.4PPCh. 6.1 - Write the symbols for the ions with the following...Ch. 6.1 - Write the symbols for the ions with the following...Ch. 6.1 - Prob. 6.7PPCh. 6.1 - State the number of protons and electrons in each...Ch. 6.1 - Write the symbol for the ion of each of the...Ch. 6.1 - Write the symbol for the ion of each of the...
Ch. 6.1 - Write the names for each of the following ions:...Ch. 6.1 - Write the names for each of the following ions:...Ch. 6.1 - State the number of protons and electrons in each...Ch. 6.1 - State the number of protons and electrons in each...Ch. 6.2 - Which of the following pairs of elements are...Ch. 6.2 - Which of the following pairs of elements are...Ch. 6.2 - Write the correct ionic formula for the compound...Ch. 6.2 - Write the correct ionic formula for the compound...Ch. 6.2 - Write the symbols for the ions, and the correct...Ch. 6.2 - Write the symbols for the ions, and the correct...Ch. 6.3 - Write the name for each of the following ionic...Ch. 6.3 - Prob. 6.22PPCh. 6.3 - Write the name for each of the following ions...Ch. 6.3 - Prob. 6.24PPCh. 6.3 - Write the name for each of the following ionic...Ch. 6.3 - Prob. 6.26PPCh. 6.3 - Prob. 6.27PPCh. 6.3 - Prob. 6.28PPCh. 6.3 - Prob. 6.29PPCh. 6.3 - Write the formula for each of the following ionic...Ch. 6.3 - Prob. 6.31PPCh. 6.3 - Prob. 6.32PPCh. 6.3 - The following compounds contain ions that are...Ch. 6.3 - Prob. 6.34PPCh. 6.4 - Write the formula including the charge for each of...Ch. 6.4 - Prob. 6.36PPCh. 6.4 - Prob. 6.37PPCh. 6.4 - Prob. 6.38PPCh. 6.4 - Prob. 6.39PPCh. 6.4 - Prob. 6.40PPCh. 6.4 - Write the correct formula for the following ionic...Ch. 6.4 - Write the correct formula for the following ionic...Ch. 6.4 - Prob. 6.43PPCh. 6.4 - Write the formula for the polyatomic ion and name...Ch. 6.4 - Name each of the following ionic compounds:...Ch. 6.4 - Name each of the following ionic compounds:...Ch. 6.5 - Name each of the following molecular compounds:...Ch. 6.5 - Prob. 6.48PPCh. 6.5 - Prob. 6.49PPCh. 6.5 - Name each of the following molecular compounds: a....Ch. 6.5 - Write the formula for each of the following...Ch. 6.5 - Write the formula for each of the following...Ch. 6.5 - Write the formula for each of the following...Ch. 6.5 - Write the formula for each of the following...Ch. 6.5 - Name each of the following ionic or molecular...Ch. 6.5 - Name each of the following ionic or molecular...Ch. 6.6 - Determine the total number of valence electrons...Ch. 6.6 - Determine the total number of valence electrons...Ch. 6.6 - Draw the Lewis structure for each of the following...Ch. 6.6 - Draw the Lewis structure for each of the following...Ch. 6.7 - Describe the trend in electronegativity as...Ch. 6.7 - Prob. 6.62PPCh. 6.7 - Using the periodic table, arrange the atoms in...Ch. 6.7 - Using the periodic table, arrange the atoms in...Ch. 6.7 - Prob. 6.65PPCh. 6.7 - Prob. 6.66PPCh. 6.7 - Predict whether each of the following bonds is...Ch. 6.7 - Predict whether each of the following bonds is...Ch. 6.7 - For each of the following bonds, indicate the...Ch. 6.7 - For each of the following bonds, indicate the...Ch. 6.8 - Choose the shape (1 to 6) that matches each of the...Ch. 6.8 - Prob. 6.72PPCh. 6.8 - Prob. 6.73PPCh. 6.8 - Complete each of the following statements for a...Ch. 6.8 - Prob. 6.75PPCh. 6.8 - Prob. 6.76PPCh. 6.8 - 6.77 Use VSEPR theory to predict the shape of each...Ch. 6.8 - Use VSEPR theory to predict the shape of each of...Ch. 6.9 - Prob. 6.79PPCh. 6.9 - Prob. 6.80PPCh. 6.9 - Prob. 6.81PPCh. 6.9 - Identify each of the following molecules as polar...Ch. 6.9 - Prob. 6.83PPCh. 6.9 - Prob. 6.84PPCh. 6.9 - Prob. 6.85PPCh. 6.9 - Prob. 6.86PPCh. 6.9 - Prob. 6.87PPCh. 6.9 - Prob. 6.88PPCh. 6.9 - Prob. 6.89PPCh. 6.9 - Prob. 6.90PPCh. 6.9 - Prob. 6.91PPCh. 6.9 - Prob. 6.92PPCh. 6 - Prob. 6.93UTCCh. 6 - a. How does the octet rule explain the formation...Ch. 6 - Prob. 6.95UTCCh. 6 - Prob. 6.96UTCCh. 6 - Prob. 6.97UTCCh. 6 - Prob. 6.98UTCCh. 6 - Prob. 6.99UTCCh. 6 - Prob. 6.100UTCCh. 6 - Prob. 6.101UTCCh. 6 - 6.102 State the number of valence electrons,...Ch. 6 - Prob. 6.103UTCCh. 6 - Prob. 6.104UTCCh. 6 - Prob. 6.105UTCCh. 6 - Prob. 6.106UTCCh. 6 - Prob. 6.107UTCCh. 6 - Prob. 6.108UTCCh. 6 - Prob. 6.109APPCh. 6 - Prob. 6.110APPCh. 6 - Prob. 6.111APPCh. 6 - Prob. 6.112APPCh. 6 - Prob. 6.113APPCh. 6 - Prob. 6.114APPCh. 6 - Prob. 6.115APPCh. 6 - Prob. 6.116APPCh. 6 - Prob. 6.117APPCh. 6 - Prob. 6.118APPCh. 6 - Prob. 6.119APPCh. 6 - 6.120 Write the formula for each of the following...Ch. 6 - Prob. 6.121APPCh. 6 - Prob. 6.122APPCh. 6 - Prob. 6.123APPCh. 6 - Prob. 6.124APPCh. 6 - Prob. 6.125APPCh. 6 - Prob. 6.126APPCh. 6 - 6.127 Draw the Lewis structure for each of the...Ch. 6 - 6.128 Draw the Lewis structure for each of the...Ch. 6 - Prob. 6.129APPCh. 6 - 6.130 Use the periodic table to arrange the...Ch. 6 - Prob. 6.131APPCh. 6 - Prob. 6.132APPCh. 6 - Show the dipole arrow for each of the following...Ch. 6 - Show the dipole arrow for each of the following...Ch. 6 - Prob. 6.135APPCh. 6 - Prob. 6.136APPCh. 6 - Prob. 6.137APPCh. 6 - Prob. 6.138APPCh. 6 - Prob. 6.139APPCh. 6 - Prob. 6.140APPCh. 6 - Prob. 6.141APPCh. 6 - Prob. 6.142APPCh. 6 - Prob. 6.143APPCh. 6 - 6.144 Classify each of the following molecules as...Ch. 6 - Indicate the major type of intermolecular...Ch. 6 - Indicate the major type of intermolecular...Ch. 6 - Prob. 6.147CPCh. 6 - Prob. 6.148CPCh. 6 - Prob. 6.149CPCh. 6 - Prob. 6.150CPCh. 6 - Prob. 6.151CPCh. 6 - Prob. 6.152CPCh. 6 - Prob. 6.153CPCh. 6 - Prob. 6.154CPCh. 6 - Prob. 6.155CPCh. 6 - Prob. 6.156CPCh. 6 - Prob. 7CICh. 6 - Prob. 8CICh. 6 - Prob. 9CICh. 6 - Prob. 10CICh. 6 - Prob. 11CICh. 6 - Of much concern to environmentalists is radon-222,...
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- The “Chemistry in Focus“ segment Broccoli—Miracle Food? discusses the health benefits of eating broccoli and gives a Lewis structure for sulforaphane, a chemical in broccoli. Draw possible resonance structures for sulforaphane.arrow_forwardOn the basis of the electronegativity values given in Fig. 12.3, indicate whether each of the following bonds would be expected to be ionic, covalent, or polar covalent. msp;a.HOc.HHb.OOd.HClarrow_forwardCH3COCH3 (acetone) is a common laboratory solvent that is often used in nail polish remover. Its Lewis structure and space-filling molecular image are shown here: Acetone is a polar molecule; the oxygen end has a slightly negative charge (oxygen is more electronegative), whereas the carbon and hydrogen end has a slightly positive charge. In liquid acetone, the molecules are attracted to each other via these polar ends-the positive end of one molecule is attracted to the negative end of its neighbor-and therefore align as shown here: Draw a Lewis structure and space-filling molecular image for CH2Cl2 (dichloromethane), another common laboratory solvent. Is the molecule polar? Which end of the molecule has a slightly negative charge? Which end has a slightly positive charge? Draw several space-filling molecular images of CH2Cl2 showing how they align in liquid dichloromethane.arrow_forward
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