Most molecules are at peace with themselves. Bottles of sulfuric acid, sodium hydroxide, water, or acetone can be safely stored in a laboratory cupboard for years without any change in the chemical composition of the molecules inside. Yet if these compounds are mixed, chemical reactions, in some cases vigorous ones, will occur. This chapter is an introduction to the behavior of organic molecules: why some react together and some don’t, and how to understand reactivity in terms of charges, orbitals, and the movement of electrons. We shall also be introducing a device for representing the detailed movement of electrons—the mechanism of the reaction—called the curly arrow. To understand organic chemistry, you need to be fluent in two languages. The fi rst is the language of structure: of atoms, bonds, and orbitals. This language was the concern of the last three chapters: in Chapter 2 we looked at how to draw structures, in Chapter 3 how to f i nd out what those structures are, and in Chapter 4 how to explain structure using electrons in orbitals. But now we need to take up a second language: that of reactivity. Chemistry is fi rst and foremost about the dynamic features of molecules—how to create new molecules from old ones, for example. To understand this, we need new terminology and tools for explaining, predicting, and talking about reactions. Molecules react because they move. Atoms have (limited) movement within molecules— you saw in Chapter 3 how the stretching and bending of bonds can be detected by infrared spectroscopy, and we explained in Chapter 4 how the σ bonds of alkanes (but not the π bonds of alkenes) rotate freely. On top of that, in a liquid or a gas whole molecules move around continuously. They bump into each other, into the walls of the container, maybe into solvent in a solution. It is all this incessant motion which drives reactions, and we fi rst need to look at what happens when molecules collide.

مواضيع ذات صلة

Rotation and rigidity

The carbonyl group

We can hybridize any atoms

Hybridization of atomic orbitals

Molecular orbitals of molecules with more than two atoms

Other factors affecting degree of orbital interaction

Bonds between different atoms

Forming bonds using 2s and 2p atomic orbitals: σ and π orbitals

Bond order

Why hydrogen is diatomic but helium is not

Breaking bonds

Molecular orbitals—diatomic molecules