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| Concept/Formula | Definition/Equation | When to Use |
|---|---|---|
| Law of Definite Proportions | A given compound always contains exactly the same proportion of elements by mass. | Determining the composition of a pure compound. |
| Law of Multiple Proportions | If two elements form more than one compound, the ratios of the masses of the second element which combine with a fixed mass of the first element will be ratios of small whole numbers. | Comparing different compounds formed by the same two elements. |
| Avogadro's Law | Equal volumes of all gases, at the same temperature and pressure, contain the same number of molecules. | Relating gas volume to the number of molecules. |
| Ideal Gas Equation | Calculating gas properties under ideal conditions. |
Type A: Stoichiometric Calculations
Setup: "Given the mass of a reactant, calculate the mass of a product."
Method: Convert mass to moles, use the stoichiometric ratio from the balanced equation, and convert moles back to mass.
Example: If 4g of H2 reacts with excess O2, how much water is produced?
Type B: Gas Law Problems
Setup: "Given initial and final conditions of a gas, calculate the change in volume, pressure, or temperature."
Method: Use the appropriate gas law (Boyle's, Charles's, or Combined Gas Law) or the Ideal Gas Equation.
Example: A gas occupies 10L at 2 atm and 300K. What is the volume at 1 atm and 600K?
Problem: Calculate the number of moles in 22.4 L of a gas at STP. Steps:
"โAnswer: 1 mole
| Concept/Formula | Definition/Equation | When to Use |
|---|---|---|
| Atomic Number (Z) | Number of protons in the nucleus. | Identifying an element. |
| Mass Number (A) | Number of protons + number of neutrons. | Determining the composition of the nucleus. |
| Ionization Energy | Energy required to remove an electron from an atom. | Predicting the reactivity of an element. |
| Electronegativity | Measure of the ability of an atom to attract electrons in a chemical bond. | Predicting bond polarity. |
Type A: Electron Configuration
Setup: "Determine the electron configuration of an element or ion."
Method: Use the Aufbau principle, Hund's rule, and the Pauli exclusion principle.
Example: What is the electron configuration of oxygen (O)?
Type B: Periodic Trends
Setup: "Predict the trend in ionization energy, electronegativity, or atomic radius across a period or down a group."
Method: Consider the effective nuclear charge and shielding.
Example: How does ionization energy change down Group 1?
Problem: Determine the number of protons, neutrons, and electrons in . Steps:
"โAnswer: 11 protons, 12 neutrons, 11 electrons
| Concept/Formula | Definition/Equation | When to Use |
|---|---|---|
| Molarity (M) | Moles of solute per liter of solution. | Calculating solution concentration. |
| Solubility | The maximum amount of solute that can dissolve in a given amount of solvent at a specific temperature. | Determining the concentration of a saturated solution. |
| Saturated Solution | A solution that contains the maximum amount of solute that can dissolve at a given temperature. | Understanding solution equilibrium. |
| Unsaturated Solution | A solution that contains less solute than the maximum amount that can dissolve at a given temperature. | Describing solutions that can dissolve more solute. |
Type A: Solubility Calculations
Setup: "Given the solubility of a salt at a certain temperature, calculate the mass of salt that will dissolve in a given volume of water."
Method: Use the solubility value as a conversion factor.
Example: The solubility of NaCl is 36 g/100 mL at 25ยฐC. How much NaCl will dissolve in 500 mL of water?
Type B: Molarity Calculations
Setup: "Calculate the molarity of a solution given the mass of solute and volume of solution."
Method: Convert mass to moles, then divide by the volume in liters.
Example: What is the molarity of a solution containing 40 g of NaOH in 2 L of solution?
Problem: Calculate the molarity of a solution prepared by dissolving 5.85 g of NaCl in 500 mL of water. Steps:
"โAnswer: 0.2 M
| Concept/Formula | Definition/Equation | When to Use |
|---|---|---|
| Air Pollution | Contamination of the atmosphere by harmful substances. | Identifying environmental hazards. |
| Water Pollution | Contamination of water bodies by harmful substances. | Identifying sources of water contamination. |
| Soil Pollution | Contamination of soil by harmful substances. | Identifying sources of soil contamination. |
| Biodegradable Pollutants | Pollutants that can be broken down by natural processes. | Classifying pollutants. |
Type A: Identifying Pollutants
Setup: "Given a list of substances, identify which are pollutants."
Method: Consider the harmful effects of each substance on the environment.
Example: Which of the following are air pollutants: O2, CO2, SO2, N2?
Type B: Pollution Control
Setup: "Propose methods for controlling a specific type of pollution."
Method: Consider strategies for reducing the release of pollutants and cleaning up existing pollution.
Example: How can oil pollution in water be controlled?
Problem: Identify a source of air pollution and its effect. Steps:
"โAnswer: Burning fossil fuels leads to global warming.
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