Now, endothermic reactions involve absorbing thermal energy by the system from the surroundings. As a result of absorbing this thermal energy, the molecules will start to speed up, and if they are given enough energy, they can use it to break their bonds. So, endothermic reactions are heat-absorbing, bond-breaking reactions. If we look at it in terms of phase changes, when heat is absorbed, it helps to spread molecules apart. Imagine having a solid, for instance, an ice cube; the solid absorbs enough heat, or thermal energy, and what happens over time? It melts. Now it's a liquid. Let's continue adding a little more heat to that liquid water. What happens to it eventually? It vaporizes into a gas, breaking the connections between water molecules as it transitions from solid to liquid to gas. Going from a solid to a liquid is called melting, or fusion in terms of thermochemistry. If you're going from a liquid to a gas, that's vaporization, and if you're going from a solid directly to a gas, that's called sublimation.
In real-world applications, if you are observing an endothermic reaction that's absorbing heat from the surroundings, and if you were to touch a container containing an endothermic reaction, it would absorb heat from your hand. Consequently, the substance absorbs heat from your hand, making it feel cold to you because you're losing heat to the container.
Finally, energy diagrams are a way of showing how a reaction progresses in terms of energy. You start off with reactants and proceed to your final product. In an endothermic reaction, your enthalpy value, which is Δh, is positive. At the beginning of this energy diagram, our reactants are represented, and here is where you end, which represents our products. Here, our y-axis is energy. In an endothermic reaction, our reactants start off at a lower energy level, and our products end at a higher energy level. This results in a positive enthalpy or Δh.