[...]... PROBLEM 5 N Which of the following has a the most polar bond? NaI b the least polar bond? LiBr KCl Cl 2 Understanding bond polarity is critical to understanding how organic reactions occur, because a central rule that governs the reactivity of organic compounds is that electron-rich atoms or molecules are attracted to electron-deficient atoms or molecules Electrostatic potential maps (often simply called... promotion is 114 kcal>mol Linus Carl Pauling (1901–1994) was born in Portland, Oregon A friend’s home chemistry laboratory sparked Pauling’s early interest in science He received a Ph.D from the California Institute of Technology and remained there for most of his academic career He received the Nobel Prize in chemistry in 1954 for his work on molecular structure Like Einstein, Pauling was a pacifist, winning... Double Bond All the bonds in methane and ethane are sigma (s) bonds because they are all formed by the end-on overlap of atomic orbitals All single bonds found in organic compounds are sigma bonds PROBLEM 15 N 29 All single bonds found in organic compounds are sigma bonds 3-D Molecule: Ethane What orbitals are used to form the 10 covalent bonds in propane (CH 3CH 2CH 3)? The MO diagram illustrating... Système International unit Those who opt to adhere strictly to SI units can convert it into picometers: 1 picometer 1pm2 = 10-12 m; 1 Å = 10-10 m = 100 pm Because the angstrom continues to be used by many organic chemists, we will use angstroms in this book American chemist Gilbert Newton Lewis (1875–1946) was born in Weymouth, Massachusetts, and received a Ph.D from Harvard in 1899 He was the first person... or fewer bonds than the number required for a neutral atom will have either a formal charge or an unpaired electron These numbers are very important to remember when you are first drawing structures of organic compounds because they provide a quick way to recognize when you have made a mistake F one bond Cl I H Br O one bond N three bonds two bonds C four bonds In the Lewis structures for CH 2O2 , HNO3... two identical atoms using their three degenerate atomic orbitals to form three bonds—one s bond and two p bonds Side-to-side overlap of two p atomic orbitals forms a P bond All other covalent bonds in organic molecules are S bonds A S bond is stronger than a P bond > Figure 1.6 nodal plane Side-to-side overlap of two parallel p orbitals to form a p bonding molecular orbital and a p* antibonding molecular... theory tell us that the electrons shared by carbon and oxygen are not shared equally—the oxygen atom of a carbon–oxygen bond has a partial negative charge and the carbon atom has a partial positive charge Organic chemists find that the information obtained from MO theory, where valence electrons occupy bonding and antibonding molecular orbitals, does not always yield the needed information about the bonds... and Ethane: Single Bonds their atomic orbitals, and because electron pairs repel each other, the bonding electrons and lone-pair electrons around an atom are positioned as far apart as possible Because organic chemists generally think of chemical reactions in terms of the changes that occur in the bonds of the reacting molecules, the VSEPR model often provides the easiest way to visualize chemical change... molecular orbital 1s, s*, p, or p*2 that results when the orbitals are combined as indicated: a c + d + + + b 1.7 Bonding in Methane and Ethane: Single Bonds We will begin the discussion of bonding in organic compounds by looking at the bonding in methane, a compound with only one carbon atom Then we will examine the bonding in ethane (a compound with two carbons and a carbon–carbon single bond), in... carbons and a carbon–carbon double bond), and in ethyne (a compound with two carbons and a carbon–carbon triple bond) Next, we will look at bonds formed by atoms other than carbon that are commonly found in organic compounds—bonds formed by oxygen, nitrogen, and the halogens Because the orbitals used in bond formation determine the bond angles in a molecule, you will see that if we know the bond angles in . need to get started with your study of organic chemistry. Chapter 1 reviews the topics from general chemistry that will be important to your study of organic chemistry. The chapter starts with a. for organic compounds.” Organic compounds are now defined as compounds that contain carbon. Why is an entire branch of chemistry devoted to the study of carbon-containing compounds? We study organic. chemical properties simply by sharing electrons. When we study organic chemistry, we study how organic compounds react. When an organic compound reacts, some old bonds break and some new bonds