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