Download CHEMISTRY 2nd Semester Review Chapter 3: Temperature

2nd
CHEMISTRY
Semester Review
Chapter 3: Temperature, Energy and Heat
3.1Temperature
 Brownian motion
 temp def
 temp scales
 Absolute zero
3.2 Heat and Thermal Energy
 definitions heat =
thermal energy =
 units – joule, calorie, BTU
 Thermodynamics
o 2nd Law
o system – open or closed
 1st Law
 thermal equilibrium
 specific heat – equation
 Heat transfer – conductor vs. insulator
3.3 Phase Changes
 def
 melting point, boiling point
 heat of fusion, heat of vaporization
 solving probs
 evaporation and condensation
Chapter 14 = Gases
14.1 Pressure & Kinetic Theory
-kinetic molecular theory =
-Brownian motion =
- pressure =
- standard pressure =
 measuring pressure
 Kinetic theory of pressure: molecular impacts; effect of temperature, effect of density
14.2 The Gas Laws
 Boyle's Law – volume vs. pressure: P1V1 = P2V2
 Charles's Law – volume vs. temperature: V1 = V2
T1 T2
 Kelvin temperature scale
 The Combined Gas Law: P1V1 = P2V2
T1
T2
 The Ideal Gas Law: PV = nRT
 Universal gas constant – choosing the correct value for "R"
 Molar volume = 22.4 L
14.3 Stoichiometry & Gases
 Gas – solid calculations
 Gas – solution calculations
 Gas – gas calculations
Review Problems - #s 18, 19, 21, 23, 24, 28
Chapter 9 = Water & Solutions Review Problems - #s 30, 32, 40, 41, 48, 54, 57, 60, 66, 71, 74
9.1 Solutes, Solvents & Water
- solution =
- solvent =
- solute =
- dissolved =
- polar =
- hydrogen bond =
 Water: properties, importance of hydrogen bonding
 Universal solvent: why?
- hydration =
 state of matter symbols: (s), (l), (g), (aq)
- aqueous =
 Why are aqueous solutions important?
 Other solvents: nonpolar
9.2 Concentration & Solubility
- concentration =
- dilute =
- concentrated =
- solubility =
 Ways to measure concentration: grams per liter , percent mass, molarity
 Molarity: why is it useful?
- molarity =
 Equilibrium
- saturated =
- aqueous equilibrium =
 Solubility & Temperature: effect of temperature on solubility
 Dissolving Rate: effect of changing particle size on dissolving rate, effect of temperature on
dissolving rate
 Solubility of Gases: effect of temperature on gas solubility, effect of pressure on gas solubility
9.3 Properties of Solutions
 reaction rate: effect of concentration & temperature
 Energy & solutions: exothermic, endothermic
- heat of solution =
- enthalpy =
- calorimetry =
 Solution calorimetry: heat lost must equal heat gained: net change is zero.
 Density, freezing & boiling: effect of solute on these properties of the solution vs. pure solvent
 Colligative Properties: freezing point depression formula
- colligative property =
- entropy =
- molality =
-electrolyte =
Chapter 13 = Acids & Bases
13.1 The Chemical Nature of Acids & Bases
- neutral =
- acid =
- base =
 The importance of the H+ ion
- Arrhenius theory =
- hydronium ion =
 Brønsted-Lowry definition
- acid =
- base =
-amphoteric =
 Brønsted-Lowry: acid-base pairs
 Identifying acids/bases: acids have leading "H", strong bases have "OH"
- strong =
- weak =
13.2 The pH Scale: acids-pH<7, neutral-pH = 7, bases-pH>7
-logarithm =
 Definition of pH
 Calculating pH for acids
 Calculating pH for bases
 pH indicators
- indicator =
13.4 Acid-Base Reactions: neutralization, corrosion & etching
 Neutralization
- neutralization =
 Titration
- titration =
- equivalence point =
 Salts
- salt =
 Salts of weak acids-raise pH; salts of strong bases do not affect pH
Review Problems - #s 21, 23, 24, 27, 29, 30, 31, 32, 35, 40, 44, 52, 58,60
Chapter 4: Physical and Chemical Change
4.1 Understanding Chemical Changes
 def
 irreversible
 interatomic forces vs intermolecular forces
 chemical bonds
o covalent bond – molecule
o ionic bonds
 enthalpy of formation
 reactivity
4.2 Chemical Reactions
 chemical reaction
 reactants & products
 balance equation
 coefficient
 endothermic vs. exothermic
o activation energy
4.3 Chemical Reactions in the Lab
 symbols for states of matter
 precipitate
 salt
 oxidation vs. reduction
 acid-base reaction
o pH scale
Chapter 10 = Chemical Reactions
10.1 Chemical Equations & 10.2 Methods for Balancing Chemical Equations
 Language of chemistry
- chemical reaction =
- chemical equation =
- reactants =
- products =
 Conservation of Mass
- law of conservation of mass =
- balanced chemical equation =
- coefficients vs. subscripts
10.3 Types of Chemical Reactions
 Synthesis: general formula, definition
 Decomposition: general formula, definition
 Single displacement: general formula, definition
 Double displacement: general formula, definition, precipitate reactions
 Precipitates & Solubility: solubility rules
 Polymerization reactions
10.4 Chemical Reactions & Energy
 exothermic (ΔH<0) vs. endothermic (ΔH>0)
 Thermochemical equations
- enthalpy of formation =
 exothermic & endothermic = reverse reactions
 Calculating enthalpy change: role of coefficients
 Energy profile: total bond energy vs. reaction progress
 Energy barrier
- energy barrier =
- spontaneous =
 Hess's Law
- Hess's Law =
 enthalpy = state function = depends only on final & initial states
Review Problems - #s 30, 32, 38, 39, 41, 43, 46