1. Kinetic Molecular Theory of Gases
1.1. It explains how pressure and temperature are related to molecular behavior
1.2. The KMT for Gases assumes that a gas's kinetic energy is proportional to its Kelvin temperature.
1.3. The KMT of Gases assumes that particle collisions are elastic.
2. Hybridizations
2.1. Unique combinations of different orbitals
2.1.1. An example is the s1p3 orbital which is a combination between and s orbital and 3 p orbitals
2.1.2. ++ The sp orbital, which has one s and one p,
2.1.3. ++ a single p orbital The s1p2 orbital, which consists of one s and two p orbitals
2.2. In hybridization, the Aufbau Principle is used.
2.2.1. The Aufbau principle is used to figure out how certain molecules' electron configurations are formed.
3. Alcohols
3.1. hydroxyl (-OH) functional group and contains Hydrogen, Carbon, and Oxygen.
3.2. A volatile liquid at room temperature that is highly flammable.
3.3. Can form hydrogen bonds and undergo combustion reactions, just like water.
3.4. Pentanol is a type of alcohol that is commonly found in food. everyday life, such as alcoholic beverages
4. Aldehydes
4.1. The general formula for Aldehydes is R-Cho
4.1.1. R can be a hydrogen atom or any alkyl group
4.2. Their functional group consists of a carbonyl group and a hydrogen atom.
4.3. Its boiling point rises as molecular size increases.
4.4. Aldehydes are flammable and volatile, with a high chemical reactivity.
5. Volume of Gases
5.1. The volume of matter is the amount of space it takes up.
5.1.1. Because it is a state of matter, gas takes up space.
5.2. Real Gas
5.2.1. Real gases cannot be compressed indefinitely because their volumes are fixed.
5.3. Ideal Gas
5.3.1. Ideal Gases are those that can be compressed indefinitely.
5.4. Tend to expand to fill the entire container
5.4.1. When a gaseous substance is transferred from a smaller container to a larger one, it expands rapidly to fill the larger container.
5.5. The most common unit of measurement is the liter.
6. Ketones
6.1. They also have a functional group of carbonyl.
6.2. Have no more than two R groups attached to their carbon atom.
6.3. The general formula is R-CO-R
6.3.1. R can stand for an alkyl or aryl group.
6.4. Because its boiling point rises with molecular size, it's similar to aldehydes.
7. Esters
7.1. An example of an ester is methyl ethanoate
7.2. Used as solvents for perfume and cosmetics, since they are sweet scented
7.3. Flammable and Volatile
7.4. Have a higher boiling point that hydrocarbons
7.5. esterification
7.5.1. Groups of organic compounds produced from the reaction between an alcohol and a carboxylic acid
7.6. The general formula is R'-COOR
7.6.1. R can be an alkyl or an aryl group
7.6.2. R’ can represent hydrogen, an alkyl, or an aromatic hydrocarbon group.
8. Temperature of Gases
8.1. The absolute temperature of a gas is proportional to its kinetic energy, which in turn is proportional to its velocity.
8.1.1. The average kinetic energy of gas molecules is the sum of all their kinetic energies.
8.2. If the temperature rises, the velocity will rise as well.
8.2.1. This will cause the gas to expand and take up more space.
9. Carboxylic Acids
9.1. group of hydrocarbons that contain the carboxyl R'(-COOH) functional group
9.2. boiling point increases as more carbon atoms are added to its chain
9.3. general formula of carboxylic acids = CnH2n+1COOH (where n = 0, 1, 2, …)
9.4. have higher boiling point than alcohols
9.5. An example is Acetic Acid (ethanoic acid)
9.5.1. Main component of vinegar. Which give its pungent smell and sour taste
9.6. Can be classified into two types
9.6.1. Open-chain
9.6.2. Closed-chain
10. Gas Pressure
10.1. Molecules follow a straight path until they collide with another molecule or the container's wall.
10.2. Pressure is defined as force applied per unit area = FORMULA
10.2.1. Can be measured through pascals (Pa)
10.2.1.1. Named after the French scientist Blaise Pascal
10.2.1.2. Bar, millimeters mercury (mmHg), Torr, and atmospheres are examples of nonstandard units used to express pressure (atm)
10.3. There is no kinetic energy lost when gas molecules collide with each other and the container walls.
10.4. The standard temperature and pressure (STP) of an ideal gas are set at 0°C and 1 bar, respectively.
11. Boyle's and Charle's law
11.1. Boyle's Law
11.1.1. Robert Boyle, a British chemist, proved it.
11.1.2. Given that the temperature of the system is kept constant, the pressure and volume of a confined gas are inversely proportional to one another.
11.1.2.1. PV=K P=K (1/v)
11.1.2.2. P1V1=P2V2
11.2. Charles' Law
11.2.1. Proven by Jacques Charles
11.2.2. Deflated hot air balloons can be used to demonstrate this.
11.2.3. When the pressure in the system is kept constant, the temperature and volume of a confined gas are directly proportional.
11.2.3.1. V=T