By Harold D. Nathan Charles Henrickson
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A. b. c. 2 3 4 3. When calcium (Ca) and chlorine (Cl) react they each form an ion, what are the charges on the calcium ion and chloride ion, respectively? a. +2 and –2 b. +1 and –2 c. +2 and –1 4. What is the formula of the compound formed between calcium and chlorine? a. CaCl2 b. Ca2Cl c. CaCl 5. What is the expected formula for the compound formed when one sulfur atom reacts with hydrogen? a. HS b. H2S c. H6S Answers: 1. c 2. c 3. c 4. a 5. b Chapter 6 ORGANIC COMPOUNDS Chapter Check-In ❑ Learning why the chemistry of carbon is so extensive ❑ Understanding the importance of structure ❑ Seeing how carbon forms single, double, and triple bonds between atoms ❑ Forming derivatives of organic compounds rganic chemistry is the chemistry of carbon, an element that forms strong chemical bonds to other carbon atoms as well as to many other O elements like hydrogen, oxygen, nitrogen and the halogens.
Figure 4-2 Filling of the s subshells. 1 2 H He 1s 1 1s 2 3 4 Li Be 2s 1 2s 2 11 12 Na Mg 3s 1 3s 2 19 20 K Ca 4s 1 4s 2 The loss of these s-subshell valence electrons explains the common +1 and +2 charges on ions of these elements, except for helium, which is chemically inert. 35 Chapter 4: Electron Configurations The six elements from boron through neon show the insertion of electrons into the lowest-energy p-type subshell. ) Figure 4-3 Filling of the 2p subshell. 5 6 7 8 9 10 B C N O F Ne 2p 1 2p 2 2p 3 2p 4 2p 5 2p 6 The same type of subshell is used to describe the electron configurations of elements in the underlying rows.
The relatively weak attraction for electrons by the alkali metals and alkaline earths is responsible for the loss of electrons by those elements. Two atoms of the same electronegativity will share electrons equally in a pure covalent bond; therefore, any molecule that contains atoms of only one element, like H2 or Cl2, has pure covalent bonding. Two atoms of different electronegativities, however, will have either the distorted electron distribution of a polar bond or the complete electron transfer of an ionic bond.