Honors Chemistry Review Sheet for Second Semester Final Exam

                                                                    (May 2008)

NOTE: Do not lose this, as you will not get another copy.

Chapter 5 - Gases

Terms:              elastic collision                          kinetic-molecular theory
                        gas constant = R                       STP
                        Pa, kPa, atm, mmHg                 Boyles’ Law
                        Charles’ Law                            Ideal Gas Law
                        degrees Kelvin              Partial Pressure

Concepts:

·          Able to solve problems using different gas laws, and knowing which law was used.

Example:

What will be the volume of a gas sample at 309 K if its volume at 215 K is 3.42 L?  Assume that pressure is constant.  Which gas law will you use to solve this.

 

 

A gas occupies a volume of 2.45 L at a pressure of 1.03 atm and a temperature of 293 K. What volume will the gas occupy if the pressure changes to 0.980 atm and the temperature remains unchanged?  Which gas law?

 

 

What volume will be occupied by 100. g of oxygen gas at a pressure of 1.50 atm and a temperature of 25°C?  (Which gas law?)

 

 

What volume will 45.0 g of chlorine gas fill at STP?

 

 

·          Any problem from the Chapter 5 test.

Chapter 6 - Thermochemistry

Terms:              endothermic                              exothermic
                        enthalpy                                    ΔH°
                        specific heat capacity                standard enthalpy change

Problems:

·          Calculating ΔH for a given equation

Example:

How much heat will be released when 1.48 g of chlorine reacts with excess phosphorus according to the following equation?

2P   + 5Cl₂   ®   2PCl₅              ΔH° = -886 kJ

 

·          Any terms or similar problems from the chapter 6 test, excluding Hess’ Law, and

calculation of specific heat capacity

 

Chapter 7 - Electron Structure

Terms:             wavelength                                           amplitude
                       speed of light                                        frequency

Concepts:

·          Properties of waves - frequency, wavelength, amplitude and speed

·          Conversion of wavelength to frequency, and reverse

·          Orbital diagrams and electron configurations, including rules for filing orbitals

NOTE: I will give you the following information, the order of the orbitals:

1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 5s, 4d, 5p, 6s

·          Any question from chapter 7 test

Example:

What is the wavelength for radiation that has a frequency of 2.5 x 10¹⁵ s^-1:

 

Write the electron configuration for Ca⁺²:

 

Chapter 8 : Chemical Bonding

Terms:              atomic radius                            ionization energy
                        electron affinity                         ionic radius
                        electronegativity                        ionic bond
                        polar covalent bond                  nonpolar covalent bond

 

Concepts:

·          trends on the periodic table, atomic radius

·          Lewis-dot structures of molecules

·          electron configurations for ions

·          difference between ionic and covalent bonding

·          any question from chapter 8/9 test

Draw the Lewis-dot diagram for CH₂Cl₂:

 

Chapter 9: Molecular Geometry

Terms:            
                       hybrid orbitals                           molecular polarity

Concepts:

·          Five major shapes, names, bond angles and hybrid orbitals

·          Molecular polarity

·          Any question from chapter 8/9 test

Examples: what is the shape of BF₃, its bond angle and the hybrid orbital.    Is it a dipole ?

 

Chapter 10: Liquids and Solids

Terms:              viscosity                                               intermolecular forces:
                        intramolecular forces                                         London dispersion
                        surface tension                                                 dipole-dipole
                        sublimation                                                       hydrogen bonding
                        vaporization (boiling)                                        
                        deposition                                             freezing
                        melting                                                  condensation

Concepts:

·          Similarities and differences between gases, liquids and solids

·          Differences between different types of solids

·          Anything from Chapter test 10/11

 

Chapter 11: Solutions:

Terms:              solute                           solvent
                        solution                         solvation
                        soluble                          colloids
                        supersaturated              saturated
                        molarity                        molality
                        Mole fraction

Concepts:

·          How solutions are formed, at the molecular level, using terms regarding intermolecular forces, polar/non-polar, etc

·          How to calculate problems dealing with molarity (M), molality (m) and mole fraction.

·          What factors affect both the solubility of a substance and the rate of solubility 

·          Anything from Chapter 10/11 Test

Chapter 12/13: Chemical Kinetics and Equilibrium

Terms:

reversible reaction                                 chemical equilibrium
            equilibrium constant                              equilibrium expression
            equilibrium position                               reaction quotient
            Le Chatelier’s principle             homogeneous/heterogenous equilibrium
            K_c                                                       

·          How to write a chemical reaction that is in equilibrium and its equilibrium expression

·          How to calculate the Q and determine if the reaction is in equilibrium

·          Predict the effects of increasing/decreasing factors based on Le Chatelier’s principle

·          Any question from Chapter 12/13 test

 

Chapter 14/15: Acids and Bases

Terms:

Arrhenius acid/base                              Brønsted-Lowry acid/base
            hydronium ion                                       indicators
            pH                                                       K_a
               K_b                                                                          titration

_·              Identify conjugate acid-base pairs and their relative strengths

·          Calculate acid/base dissociation constants and pH/pOH

·          Any problem from Test on Acids/Bases               

Constants: (you will be given the following numbers when taking the exam, as well as a periodic table if you do not have yours.  You must bring your own calculator.  If you return your old tests I will give you 4 extra credit points on your exam.)

 You must bring your textbook to the exam if you have not already turned it in.

Volume of gas at STP = 22.4 L/mol

Gas constant = R = 0.0821 atm × L
                                          mol × K

1 atm = 760 mmHg = 101,325 Pa = 101.325 kPa = 760 torr