Final answer:
Ionization energy (IE) increases across a period and decreases down a group on the periodic table. Reaction rate can be affected by reactant concentration, temperature, and the presence of a catalyst. As a reaction approaches equilibrium, the rates of forward and reverse reactions change until they are equal.
Step-by-step explanation:
The Ionization Energy (IE) refers to the amount of energy required to remove an electron from an atom or ion in its gaseous state. IE trends on the periodic table generally show that IE increases as you move from left to right across a period and decreases as you move down a group. This is shown in figures like 8.6.2 and 9.9.2, where IE values are plotted against positions on the periodic table. Although there are exceptions, the overall trend can be observed.
The reaction rate is influenced by various factors, including the nature of the reactants, the concentration of reactants, temperature, the presence of a catalyst, and the phase of reactants. When conditions such as temperature and concentration are increased, the reaction rate typically increases as well. A catalyst is known to increase the reaction rate by providing an alternative pathway with a lower activation energy as per section 17.2 in textbooks.
As a reaction approaches equilibrium, the rates of the forward and reverse reactions change. Initially, the forward reaction rate is higher because the concentrations of reactants are greater. As the reactants are consumed and products are formed, the forward reaction rate decreases while the reverse reaction rate increases until the two rates become equal at equilibrium.