1. Unit 1
1.1. Module 1
1.1.1. Lesson 1
1.1.1.1. Terms
1.1.1.1.1. Matter
1.1.1.1.2. Solid State
1.1.1.1.3. Liquid State
1.1.1.1.4. Gas State
1.1.1.1.5. Kinetic Energy
1.1.1.1.6. Temperature
1.1.1.1.7. Thermometer
1.1.1.1.8. Kelvin Scale
1.1.1.1.9. Potential Energy
1.1.1.1.10. Thermal Energy
1.1.1.1.11. Atoms
1.1.1.1.12. Substances
1.1.1.1.13. Elements
1.1.1.1.14. Compound
1.1.1.1.15. Molecule
1.1.1.1.16. Periodic Table of Elements
1.1.1.1.17. Element Symbols
1.1.1.1.18. Chemical Formula
1.1.2. Lesson 2
1.1.2.1. Jacques Charles
1.1.2.1.1. Jacques Alexandre César Charles was a French inventor, scientist, mathematician, and balloonist. Charles wrote almost nothing about mathematics, and most of what has been credited to him was due to mistaking him with another Jacques Charles, also a member of the Paris Academy of Sciences, entering on 12 May 1785.
1.1.2.2. Volume Temperature Law
1.1.2.2.1. the volume of a given amount of gas is directly proportional to its temperature on the kelvin scale when the pressure is held constant.
1.1.2.3. Thermal Contraction
1.1.2.3.1. occurs when materials are subjected to a decrease in temperature.
1.1.2.4. Thermal expansion
1.1.2.4.1. the tendency of matter to change in shape, volume, and area in response to a change in temperature.
1.1.2.5. Systems
1.1.2.5.1. a set of things working together as parts of a mechanism or an interconnecting network.
1.1.2.6. Heating
1.1.2.6.1. Think about a warm cup of hot cocca on a cold day. Thermal energy moves from the warm cup to your hands. The transfer of thermal energy from a region of higher temperature to a region of lower temperature is called heat. Just as temperature and thermal energy are not the same thing, neither are heat and thermal energy.
1.1.2.7. Pressure
1.1.2.7.1. continuous physical force exerted on or against an object by something in contact with it.
1.1.2.8. Phase Change
1.1.2.8.1. The conversion of matter from one state to another is called a phase change. This process occurs when a large amount of energy is gained or lost. Phase change also depends on factors like pressure and temperature.
1.1.2.9. Melting
1.1.2.9.1. Matter can change state when it gains or loses enough thermal energy. When the temperature of a substance increases, the particles speed up. As you have learned, when particles speed up, they start to move farther away from each other.
1.1.2.10. Freezing
1.1.2.10.1. The opposite of melting is freezing, the change of state from a liquid to a solid. The freezing point, which is the same as the melting point, is the temperature at which a liquid changes to a solid. Freezing requires the removal of thermal energy.
1.1.2.11. Condensation
1.1.2.11.1. the process where water vapor becomes liquid.
1.1.2.12. Vaporization
1.1.2.12.1. When you heat water, do you ever notice how bubbles begin to form at the bottom and rise to the surface? The bubbles contain water vapor, a gas. The change in state from a liquid into a gas is vaporization.
1.1.2.13. Boiling vs. Evaporation
1.1.2.13.1. Evaporation is a normal process that occurs when the liquid form changes into the gaseous form; while causing an increase in the pressure or temperature.
1.2. Lesson 3
1.2.1. Robert Boyle
1.2.1.1. British Scientist who discovered that the volume of a gas decreases with increasing pressure
1.2.2. Boyles Law - Pressure and Volume
1.2.2.1. a gas's pressure and volume are inversely proportional.
1.2.3. Boyles Law - Number of particles
1.2.3.1. holds true only if the number of molecules (n) and the temperature (T) are both constant.
1.2.4. Boyles Law - Pressure and States of matter
1.2.4.1. the volume of a given amount of gas held at constant temperature varies inversely with the applied pressure when the temperature and mass are constant.
1.3. Lesson 4
1.3.1. Molecules
1.3.2. Nonmetal Gases
1.3.2.1. poor conductors of heat and electricity, and are not malleable or ductile
1.3.3. Nonmetal Solids
1.3.3.1. brittle, meaning that they will shatter if struck with a hammer.
1.3.4. Metals
1.3.4.1. a solid material that is typically hard, shiny, malleable, fusible, and ductile, with good electrical and thermal conductivity (e.g., iron, gold, silver, copper, and aluminum, and alloys such as brass and steel).
1.3.5. Ionic Compounds
1.3.5.1. compounds made up of ions that form charged particles when an atom (or group of atoms) gains or loses electrons.
1.3.6. Covalent Compounds
1.3.6.1. formed when two nonmetals react with one another.
1.3.7. Polar Covalent Compounds
1.3.7.1. two atoms share a pair of electrons unequally because of differences in their electro-negativities.
1.3.8. Nonpolar Covalent Compounds
1.3.8.1. a type of chemical bond that is formed when electrons are shared equally between two atoms.
1.3.9. Dissolving
2. Lesson 3
2.1. Chemical Potential Energy
2.1.1. Chemical potential energy is the energy stored in the chemical bonds of a substance. The various chemicals that make up gasoline contain a large amount of chemical potential energy that is released when the gasoline is burned in a controlled way in the engine of the car.
2.2. Endothermic Reaction
2.2.1. In thermochemistry, an endothermic process is any thermodynamic process with an increase in the enthalpy H of the system. In such a process, a closed system usually absorbs thermal energy from its surroundings, which is heat transfer into the system.
2.3. Exothermic Reaction
2.3.1. In thermochemistry, an exothermic reaction is a "reaction for which the overall standard enthalpy change ΔH⚬ is negative." Exothermic reactions usually release heat.
2.4. Concentration in reactions
2.4.1. One of the factors guiding the reaction is the concentration of reactants. It is expressed in terms of the amount of product received per unit time. It means the concentration of the reactant is consumed in a unit time. Rate of reaction = Change in concentration per unit time.
2.5. Law of conservation of energy
2.5.1. In physics and chemistry, the law of conservation of energy states that the total energy of an isolated system remains constant; it is said to be conserved over time. Energy can neither be created nor destroyed; rather, it can only be transformed or transferred from one form to another.
3. Unit 3
4. Unit 4
4.1. Module 1
4.1.1. Lesson 1
4.1.1.1. Photosynthesis
4.1.1.2. Epidermal leaf cells
4.1.1.3. Cuticle
4.1.1.4. Stomata
4.1.1.5. Mesophyll Cells
4.1.1.6. Chloroplasts
4.1.1.7. Chlorophyll A and B
4.1.1.8. Light Cycle
4.1.1.9. Night Cycle
4.1.1.10. Different sugars
4.1.1.11. Cellular Respiration
4.1.1.12. Glycolysis
4.1.1.13. Mitochondria
4.1.1.14. Lactic Acid Fermentation
4.1.1.15. Ethanol Alcohol Fermentation
4.1.2. Lesson 2
4.1.2.1. Producers
4.1.2.2. Consumers
4.1.2.3. Primary Consumer
4.1.2.4. Secondary Consumer
4.1.2.5. Tertiary Consumer
4.1.2.6. Detritivores
4.1.2.7. Food Chain
4.1.2.8. Food Web
4.1.2.9. Energy Pyramid / 10 % rule
4.1.3. Lesson 3
4.1.3.1. Carbon Cycle
4.1.3.2. - Cellular Respiration
4.1.3.3. - Photosynthesis
4.1.3.4. - Sedimentation
4.1.3.5. - Decomposition
4.1.3.6. - Fossil Fuels
4.1.3.7. - Combustion