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Chemistry 121 Review
Chemistry 121 review for chemistry 122
| Question | Answer |
|---|---|
| Alkali Metals | Group 1A; Li, Na, K, Rb, Cs, Fr |
| Alkaline Earth Metals | Group 2A; Be, Mg, Ca, Sr, Ba, Ra |
| Chalcogens | Group 6A; O, S, Se, Te, Po |
| Halogens | Group 7A; F, Cl, Br, I, At |
| Noble Gases (or rare gases) | Group 8A; He, Ne, Ar, Kr, Xe, Rn |
| Molecular Formulas | Chemical formulas that indicate the actual numbers and types of atoms in a molecule |
| Empirical Formulas | Chemical formulas that give only the relative number of atoms of each type in a molecule |
| Ion | A charged particle |
| An ion with a positive charge | Cation |
| An ion with a negative charge | Anion |
| Ionic compound | A compound that contains both positively and negatively charged ions. |
| Procedure for calculating an empirical formula from percentage composition | Mass % elements>Assume 100 g sample>Grams of each element>Use molar mass>Moles of each element>Calculate mole ratio>find empirical formula |
| Whole-number multiple | Molecular weight/Empirical weight |
| Solvent | The substance present in the greatest quantity |
| Solute | The other substances in the solution |
| Electrolyte | A substance whose aqueous solutions contain ions |
| Nonelectrolyte | A substance that does not form ions in solution |
| Strong electrolytes | Those solutes that exist in solution completely or nearly completely as ioiins |
| Weak electrolytes | Those solutes that exist in solution mostly in the form of molecules with only a small fraction in the form of ions |
| Soluble Ionic Compounds | NO3, CH3COO, Cl, Br, I, SO4 |
| Insoluble Ionic Compounds | S, CO3, PO4, OH |
| Acids | Substances that ionize in aqueous solutions to form hydrogen ions |
| Bases | Substances that accept H+ ions |
| Strong Acids | Hydrochloric, Hydrobromic, Hydroiodic, Chloric, Perchloric, Nitric, Sulfuric |
| Strong Bases | Group 1A metal hydroxides (LiOH, NaOH, KOH, RbOH, CsOH), Heavy group 2A metal hydroxides [Ca(OH)2, Sr(OH)2, Ba(OH)2] |
| Salt | Any ionic compound whose cation comes from a base and whose anion comes from an acid |
| Oxidation | Loss of electrons by a substance |
| Reduction | The gain of electrons by a substance |
| Oxidation number | The actual charge for a monatomic ion |
| Concentration | The amount of solute dissolved in a given quantity of solvent or quantity of solution |
| Molarity | Moles Solute/Volume of solution in liters |
| energy | The capacity to do work or to transfer heat |
| Work | The energy used to cause an object with mass to move against a force |
| Heat | The energy used to cause the temperature of an object to increase |
| Kinetic energy | The energy of motion [(1/2)mv^2] |
| Potential energy | The energy stored in chemical bonds (mass*force of gravity*height) |
| Force of gravity | 9.8 m/s^2 |
| Electrostatic potential energy | The interactions between charged particles (KQ1Q2/d) K=Constant of porportionality Q=Electrical charges |
| Joule | SI unit for energy 1J=1 kg-m2/s2 |
| calorie | The amount of energy to raise the temperature of 1g of water from 14.5 C to 15.5 C. 1 cal = 4.184 J |
| Equation for work | W = F x d |
| First law of thermodynamics | Energy is conserved |
| Internal energy | The sum o fall the kinetic and potential energies of all its components. |
| Change in internal energy equation | E(final)-E(initial) |
| Explanation of change in internal energy | A positive value indicates a gain in energy from the surroundings. A negative value indicates a losing energy to the surroundings. |
| Equation for first law of thermodynamics | Change in energy= q + w (q is given by the heat added to or liberated from the system), w is work done on the system |
| Endothermic | When a system absorbs heat |
| Exothermic | When a system releases heat |
| Enthalpy | Accounts for heat flow in processes occurring at constant pressure when no forms of work are performed. |
| Calorimetry | The measurement of heat flow |
| Heat capacity | The temperature change experienced by an object when it absorbs a certain amount of heat |
| Molar heat capacity | The heat capacity of one mole of a substance |
| Specific heat | The heat capacity of one gram of a substance |
| Specific heat equation | Specific heat= (quantity of heat transferred)/(grams of substance)*(temperature change) |
| Hess's Law |
Created by:
calebmo
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