Lewis Structure of Elements Draw the Lewis structure of elements and determine the number of electrons gained or lost by an element in an ion formation. Lewis Structure Element Compound Formula Compound Formation Potassium and Bromine r: [K] [:Br:] KBr K. + ·Br: K. Br: Potassium Bromide Calcium and Nitrogen Lithium and Oxygen Sodium and Phosphorous Aluminum and Sulfur

Lewis Structure of Elements Draw the Lewis structure of elements and determine the number of electrons gained or lost by an element in an ion formation. Lewis Structure Element Compound Formula Compound Formation Potassium and Bromine r: [K] [:Br:] KBr K. + ·Br: K. Br: Potassium Bromide Calcium and Nitrogen Lithium and Oxygen Sodium and Phosphorous Aluminum and Sulfur

Chemistry for Today: General, Organic, and Biochemistry

9th Edition

ISBN:9781305960060

Author:Spencer L. Seager, Michael R. Slabaugh, Maren S. Hansen

Publisher:Spencer L. Seager, Michael R. Slabaugh, Maren S. Hansen

Chapter4: Forces Between Particles

Section: Chapter Questions

Problem 4.2E

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The ionic compound AB is formed. The charges on the ions may be +1, 1; +2, 2; +3, 3; or even larger. What are the factors that determine the charge for an ion in an ionic compound?
Distinguish between the terms electronegativity versus electron affinity, covalent bond versus ionic bond, and pure covalent bond versus polar covalent bond. Characterize the types of bonds in terms of electronegativity difference. Energetically, why do ionic and covalcnt bonds form?
Using the standard enthalpy of formation data in Appendix G. determine which bond is stronger: the PCl bond in PCl3(g) or in PCl5(g)?
What is meant by a chemical bond? Why do atoms form bonds with each other? Why do some elements exist as molecules in nature instead of as free atoms?
Occasionally, we will see an ionic compound that has a 1 counterion. (Later we will find that 1 counterions are often more than spectators and take an active role in many reactions.) a. What elements (other than H) on the periodic table are most likely to form a 1 anion? b. Draw a Lewis structure for the ionic compound NH4Cl (Hint. One atom is a 1 counterion).
Using the standard enthalpy of formation data in Appendix G, determine which bond is stronger: the SF bond in SF4(g) or in SF6(g)?
rite the Lewis structure for each of the following atoms. msp;a.He(Z=2)d.Ne(Z=10)b.Br(Z=35)e.I(Z=53)c.Sr(Z=38)f.Ra(Z=88)
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For three simple molecules of your own choice, apply the rules for writing Lewis structures. Write your discussion as if you are explaining the method to someone who is not familiar with Lewis structures.
Think of forming an ionic compound as three steps (this is a simplification, as with all models): (I) removing an electron from the metal; (2) adding an electron to the nonmetal; and (3) allowing the metal cation and nonmetal anion to come together. a. What is the sign of the energy change for each of these three processes? b. In general, what is the sign of the sum of the first two processes? Use examples to support your answer. c. What must be the sign of the sum of the three process d. Given your answer to part c, why do ionic bonds occur? e. Given your above explanations, why is NaCl stable but not Na2Cl? NaCl2? What about MgO compared to MgO2? Mg2O?
rrange the atoms and/or ions in the following groups in order of decreasing size. msp;a.O,O,O2b.Fe2+,Ni2+,Zn2+c.Ca+,K+,Cl
The Lewis representation above depicts a reaction between a halogen (blue) and a main-group element from group (7A + (red). In this representation, each Y atom needs 1 electron(s) to complete its octet, and gains these electrons by forming bond(s) with atoms of X . There are unshared electron pair(s) and bonding electron pair(s) in the product molecule. The bonds in the product are Submit Answer Retry Entire Group 9 more group attempts remaining Previous Next Email Instructor Save and Exit Cengage Learning | Cengage Technical Support