and endings of these prefixes are dropped when they are attached to oxygen. The ending of “a” the last element is changed to The elements are written in the formula from least “-ide.” electronegative to most. Basically, elements are placed in the formula according to their left to right location in the periodic table. The one exception is to place hydrogen between nitrogen and oxygen, because its electronegativity falls between these two elements. Number of atoms of that element in the Prefix formula mono 1 (most electronegative only) 2 di 3 tri 4 tetra 5 penta 6 hexa Here are a few examples: PH3 is named phosphorus trihydride; N2O3 is named dinitrogen trioxide; NO is named nitrogen monoxide. Catalysis One of the requirements for a chemical reaction to is that the reacting molecules or atoms must collide with one another with enough kinetic energy so that products can form. This minimum energy needed to get the reaction started is called the activation energy. We can use the Maxwell-Boltzmann Distribution curve (below) to relate the activation energy of a reaction to the energy distribution of the reactant particles. The distribution curve shows the energy dynamics of the particles at a particular temperature. Keep in mind that the particles are moving around and colliding with each other and energy is being transferred among particles. The kinetic energy of each particle can change over time and not all particles have the same amount of energy. At any given time, most of the particles will have kinetic energies that are close to the average kinetic energy of the sample, while few particles will have very low energies or very high energies. Now suppose a particular reaction has a high activation energy. Since at any given time very few of the particles have high kinetic energy, the reaction will occur at a very slow rate. Maxwell-Boltzmann Distribution Curve () Catalysts speed up chemical reactions by providing a new pathway with a lower activation energy (Ea) for the reaction than is possible without them. While a catalyst is part of a chemical reaction and plays a crucial role therein, it is not one of the end products, nor is it a reactant, per se. That is, the catalyst is not consumed in a chemical reaction. The diagram at right compares the activation energy of an uncatalyzed reaction with that of a catalyzed reaction.
and “a” endings of these prefixes are dropped when they are attached to oxygen. The ending of the last element is changed to “-ide.” The elements are written in the formula from least electronegative to most. Basically, elements are placed in the formula according to their left to right location in the periodic table. The one exception is to place hydrogen between nitrogen and oxygen, because its electronegativity falls between these two elements. Number of atoms of that element in the formula Prefix 1 mono (most electronegative only) 2 di 3 tri 4 tetra 5 penta 6 hexa Here are a few examples: PH3 is named phosphorus trihydride; N2O3 is named dinitrogen trioxide; NO is named nitrogen monoxide. Catalysis One of the requirements for a chemical reaction to is that the reacting molecules or atoms must collide with one another with enough kinetic energy so that products can form. This minimum energy needed to get the reaction started is called the activation energy. We can use the Maxwell-Boltzmann Distribution curve (below) to relate the activation energy of a reaction to the energy distribution of the reactant particles. The distribution curve shows the energy dynamics of the particles at a particular temperature. Keep in mind that the particles are moving around and colliding with each other and energy is being transferred among particles. The kinetic energy of each particle can change over time and not all particles have the same amount of energy. At any given time, most of the particles will have kinetic energies that are close to the average kinetic energy of the sample, while few particles will have very low energies or very high energies. Now suppose a particular reaction has a high activation energy. Since at any given time very few of the particles have high kinetic energy, the reaction will occur at a very slow rate. Maxwell-Boltzmann Distribution Curve () Catalysts speed up chemical reactions by providing a new pathway with a lower activation energy (Ea) for the reaction than is possible without them. While a catalyst is part of a chemical reaction and plays a crucial role therein, it is not one of the end products, nor is it a reactant, per se. That is, the catalyst is not consumed in a chemical reaction. The diagram at right compares the activation energy of an uncatalyzed reaction with that of a catalyzed reaction.