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Model 2 — Average Bond Energy Bond H—CI c—cl Energy (kJ/mol) 432 411 386 431 346 358 305 327 602 745 494 Bond 0—0 Enerw (kJ/mol) 160 631 941 201 243 158 269 204 552 259 7. Look at the bond energies in Model 2. a. Are the bond energi ositive r negative? b. Do the bond energies refer t ond-breaki 8. Look at the energy values in Model 2. a ...

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CHAPTER 6 REVIEW Chemical Bonding

second, show a metallic bond that would be stronger. Be sure to include nuclear charge and number of electrons in your illustrations. a. b. weak bond strong bond . Note: In the strong bond, the charge on the nucleus and the number of electrons must be greater than in the weak bond. 11. Complete the following table: Metals Ionic Compounds ...

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financial engineers are creating new fixed-income securities almost continuously. In this chapter, we will introduce a wide variety of bond types used in international bond markets. Then, we will describe how bond markets are organized around the world. Finally, we will show how tools and concepts used in international bond markets.

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Short Manual to

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Chapter 13 – Chemical Bonding

Covalent bond –bond formed when atoms share one or more pairs of electrons Molecule –smallest unit of a substance that keeps all physical and chemical properties Metallic Bond –bond formed by attraction between positively charged metal ions and the electrons around them

C HAPTE R SE CTION 3 Covalent and Met allic Bonds

8.3.a, 8.3.b W hat Are Covalent Bonds? Another type of bond is a covalent bond. A covalent bond forms when atoms share electrons. Covalent bonds most often form between atoms of nonmetals. Remember that most nonmetals can fill the outermost energy level by gaining an electron. When a covalent bond forms, both

(Chapter 7)

When we are looking at a chemical bond to determine whether its actual bond type is pure covalent, polar covalent, or ionic, we must compare the electronegativities of the atoms in the bond. Simply subtract the EN values of the two elements in the bond and compare to the chart below: 0 - 0.3 ----> pure covalent 0.4 - 1.7 ----> polar covalent

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4 Bond Lengths of Ethyne, Ethene and Ethane The carbon-carbon bond length is shorter as more bonds hold the carbons together With more electron density between the carbons, there is more “glue” to hold the nuclei of the carbons together The carbon-hydrogen bond lengths also get shorter with more s character of the bond 2s orbitals are held more closely to the nucleus than 2p orbitals

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