& BE 4 ) 6. 8 Q { Recitation Problem Set 9 Ch 8/9 Name: 1. Predict the type of bond (ionic, purely covalent, nonpolar covalent or polar covalent) one would expect to form between the following pairs of elements. Use the table of electronegativity values. Use the arrow notation to indicate which element is the positive end option and which is the negative end of the dipole in the bonds that are polar (length of arrow tells how polar bond is). Indicate the positive and negative ions in ionic compounds. option A. Rb and Cl B. S and S C. C and F D. Ba and S E. N and P F. B and H

& BE 4 ) 6. 8 Q { Recitation Problem Set 9 Ch 8/9 Name: 1. Predict the type of bond (ionic, purely covalent, nonpolar covalent or polar covalent) one would expect to form between the following pairs of elements. Use the table of electronegativity values. Use the arrow notation to indicate which element is the positive end option and which is the negative end of the dipole in the bonds that are polar (length of arrow tells how polar bond is). Indicate the positive and negative ions in ionic compounds. option A. Rb and Cl B. S and S C. C and F D. Ba and S E. N and P F. B and H

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Circle the more electronegative in each pair. (a) F vs. N (b) Si vs. C (c) O vs. Cl (d) Cu vs. C
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Select all of the statements that are supported by the diagram shown below: H CI &+ 8- H-CI | The electrons in the covalent bond are shared equally by both atoms | This is a polar bond | There is a greater chance of find the shared electrons closer to the chlorine atom than the hydrogen atom | There is no chance of finding the electrons along the internuclear axis | The hydrogen atom has a partial positive charge This is a covalent bond
Please categorize the following bond based on its bond polarity Si-P? A)Pure covalent bond B)Polar covalent bond C)Ionic Bond
Re-order each list of elements in the table below, if necessary, so that the elements are listed in order of decreasing electronegativity. elements P, C1, S As, S, Se elements in order of decreasing electronegativity 0 0,0,... × Ś
Provide the following information for each of the following chemical formulas. (NO2)-1 : (H3O)+1 : CHF3 : BF3 a) Needed electrons= H. Draw the Lewis Structure b) available electrons= c) shared electrons= d) number of bonds= e) what is the central atom? f) How many unshared (lone) pairs of electrons on the central atom? g) Does the central atom obey the octet rule or is it an exception the octet rule?
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Use the figure to find the electronegativity difference between each of the following pairs of elements, then use the table below to classify the bonds that occur between them as pure covalent, polar covalent, or ionic. (Electronegativity of CrCr is 1.6) Electronegativity Difference (ΔENΔEN) Bond Type Example zero (0−0.40−0.4) pure covalent Cl2Cl2 intermediate (0.4−2.00.4−2.0) polar covalent HFHF large (2.0+2.0+) ionic NaClNaCl Find the electronegativity difference between Br and Br. Express your answer using two significant figures.
electrostatic potential map -ol possible chemical formula (check all that apply) □NO ₂ O CICN CO₂ H₂CO HCN
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.
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