District 5 - Stoichiometry and Solutions
The Capitol is so infatuated with stoichiometry and solutions that they granted them two Districts (as opposed to one that all other Districts are allotted). Additionally, the Capitol showers them with praise throughout the year by providing them with more food and supplies then all the other Districts. This District is just as fierce and destructive as their sister District (District 4). Many Hunger Games have come down to a battle royale between District 4 and 5. You will need to have a profound understanding of stoichiometry and solutions in order to take this District down because they possess the power to perform the ultimate kill move: the grams to moles to moles to grams conversion.
Past District 5 Champions
- Johannes Diderik van der Waals was one of the first to ever come up with the idea of intermolecular forces. He knows exactly how things are attracted to each other. Just make sure he doesn't lure you to your doom!
Please take out your District 5 guided notes and watch the lesson below:
Atoms in a solid hold a very fixed position. They are said to be vibrating in place. There is a large amount of forces between the molecules.
Atoms in a liquid are further spread out from one another. They flow freely within the solution and are moving in a random motion. There are some forces between the molecules, but not as many as solids have.
Atoms in a gas are in constant random motion. There are very few forces between the molecules.
Intermolecular forces are forces that attract molecules to one another. All intermolecular forces are the result of the attraction between opposite charges. The three main types of intermolecular forces are:
- Hydrogen Bonding
- Dipole-Dipole Forces
- Dispersion Force (also known as Van der Waals Forces)
Solid, liquid, and gas phase and the amount of forces that exist in each phase.
Here we can see hydrogen (electronegativity = 2.1) and chlorine (electronegativity = 3.5) with a difference of 1.4 in electronegativity on the pauling scale. This induces a permanent dipole which will cause the hydrogen to be partially negative, and the chlorine to be partially positive.
A dipole is a separation of charge. Recall, electronegativity is how well an element pulls electrons towards itself. Molecules can have a separation of charge because a very electronegative element is bound to an element with a lower electronegativity. This causes the electrons to be held closer to the element with the higher electronegativity.
Dipole-dipole forces refer to the attraction between molecules that have a permanent dipole. The positive end of one molecule will be attracted to the negative end of the other molecule. Molecules that have permanent dipoles are known as polar compounds.
Hydrogen bonding refers to the attraction of one molecule that contains hydrogen to another molecule. When hydrogen is bound to N, O, or F, there is a large difference in electronegativity and this creates a partial positive charge and a partial negative charge (H has the partial positive charge because it has its electrons pulled away). The partial positive charge on hydrogen is attracted to N, O, or F of another molecule. This results in a hydrogen bond.
Van Der Waals
Because dispersion forces rely so much on the random motion of electrons dispersed throughout atoms, the amount of touching surface area is very important. This is how geckos can climb up walls!
Some molecules do not have dipoles within the molecule (e.g. O2), but they can have an induced dipole. Dispersion forces are the intermolecular forces resulting from the uneven distribution of electrons and the creation of temporary dipoles. This is the weakest intermolecular force.
When two molecules are brought close to one another, electrons rearrange themselves so that a temporary dipole results, this is dispersion forces. Molecules that only exhibit temporary dipoles are known as non-polar compounds.
Solubility and How to Impact It
Dissolving substances in various liquids can involve complex chemistry, having a solid understanding of what's going on at the particulate level is SUPER important if you want to have success in the hunger games.
In order to dissolve a solute in a solvent, the solvent must use intermolecular forces in order to break the solute apart and pull it into solution.
The most common example is NaCl dissolving in water. A water molecule has a dipole with a partial negative charge on the oxygen and a partial positive on the hydrogen. In addition to the hydrogen bonding that it can form with itself, it also can form dipole-dipole forces with NaCl. The negativly charged oxygen is attracted the positive Na ion and the positively charges hydrogen is attracted to the negative Cl. The water molecules form "water cages" around each Na and Cl ion in order to break the crystal apart and pull the solute into solution.
Water forming a cage around a positive Na ion
At high temperature, liquid molecules move quick which leads them to collide with the solute more, resulting in higher overall solubility.
The rate at which a solute dissolves in a solvent depends on numerous factors. We can alter the rate at which the solute dissolves by altering the temperature of the solution, the surface area of the solute, or the pressure of the solution.
As you increase the temperature, the rate at which the solute dissolves increases. As you increase the temperature, molecules start moving faster. By moving faster, the molecules are better able to grab the solute, form the cages around them and pull them into the solution. Therefore, the faster molecules are moving, the faster something dissolves.
As you increase the surface area, the rate at which the solute dissolves increases. As you increase the surface area of a substance, you are providing more sites for the solvent to interact with the solute. This allows for the solute to be pulled into solution at a much quicker rate when compared to those of a lower surface area.
As you increase the pressure, the rate at which the solute dissolves increases. The solubility and pressure relationship is clearly seen when a gas dissolves in a liquid. When a gas is above a liquid and the pressure is increased, the gas molecules collide more often with the wall of the liquid and this causes more gas to be pushed into the liquid.
Dissolving of a gas is directly dependent on pressure. A high pressure leads to more collisions, which leads to higher overall solubility. This is how soda bottles get their CO2!