BeaulacHighlineCHEM& 1216)Double and triple bonds form becausea. the atoms involved have high electronegativities.b. single covalent bonds do not give all of the atoms in the molecule 8valence electrons.C. one of the atoms in the molecule has more than 8 valence electrons.d. the ions involved have charges larger than one.0) Group IIA metals form ions with acharge.8) Group VA nonmetals form ions with acharge.) Group VIIA nonmetals form ions with acharge.) List the metals not in group IA or IIA that only form one ion.) Fill in the blanks in the following table:Polyatomic IonChemical FormulaPolyatomic IonChemical FormulasulfatechlorateNO2ammoniumperbromatePO,3-CIO-nitratebicarbonatecyanideioditeOHcarbonate

6) Double and triple bonds form because a. the atoms involved have high electronegativities. b. single covalent bonds do not give all of the atoms in the molecule 8 valence electrons. C. one of the atoms in the molecule has more than 8 valence electrons. d. the ions involved have charges larger than one. Group IIA metals form ions with a charge. Group VA nonmetals form ions with a charge.

6) Double and triple bonds form because a. the atoms involved have high electronegativities. b. single covalent bonds do not give all of the atoms in the molecule 8 valence electrons. C. one of the atoms in the molecule has more than 8 valence electrons. d. the ions involved have charges larger than one. Group IIA metals form ions with a charge. Group VA nonmetals form ions with a charge.

Living by Chemistry

2nd Edition

ISBN:9781464142314

Author:Angelica M. Stacy

Publisher:Angelica M. Stacy

ChapterU2: Smells: Molecular Structure And Properties

Section: Chapter Questions

Problem 3STP

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In bonding, what would happen between the electrons of K and Br? a.They would be transferred. b.They would be shared. c.Neither of the above. d.They would be both transferred and shared.
Use the simulation (http://openstaxcollege.org/l/16MolecPolarity) to perform the following exercises for a two-atom molecule: (a) Adjust the electronegativity value so the bond dipole is pointing toward B. Then determine what the electronegativity values must be to switch the dipole so that it points toward A. (b) With a partial positive charge on A, turn on the electric field and describe what happens. (c) With a small partial negative charge on A, turn on the electric field and describe what happens. (d) Reset all, and then with a large partial negative charge on A, turn on the electric field and describe what happens.
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?
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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Using the bond energies in Table 7.2, determine the approximate enthalpy change for each of the following reactions: (a) H2(g)+Br2(g)2HBr(g) (b) CH4(g)+I2(g)CH3I(g)+HI(g) (c) C2H4(g)+3O2(g)2CO2(g)+2H2O(g)
What is a dipole moment? Give four examples of molecules that possess dipole moments, and draw the direction of the dipole as shown in Section 12.3.
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