Download Student midterm review sheet

General Chemistry
Review plan for Midterm/Week of January 16, 2012
Please note that all page references refer to the course textbook.
Dr. L. O’Reilly

The midterm exam will consist of multiple choice questions, numeric responses, short
answer questions and problems.
 The format will be the same as all of the in-class chapter tests given to date.
 The questions will include some chapter test questions already given and new questions.
 The material that will be tested includes information contained in the textbook and given
in class from chapters 1 and 2, & 4 through and including any material covered in chapter
9.
 Please bring a #2 pencil to the test.
To study for the midterm, YOU SHOULD:
Review all past assignments, including in-class worksheets.
Review your notes.
Review past quizzes and chapter tests.
Review all class handouts (Vocabulary; how-to guidelines; Aufbau principle & energy levels)
Review the vocabulary (highlighted words) in each chapter.
Review the concepts and questions noted below.
Do the suggested practice problems (if noted below).
Chapter 1
Topics by section
Section 1.1
 What are the traditional areas of study
in chemistry?
 Why is the area of chemistry important
to study?
Section 1.2
 What are some of the technologies that
have resulted from the study of
chemistry?
Section 1.3
 What are the steps involved in the
scientific method?
Section 1.4
 What is an effective approach to
solving a problem?
Suggested Problems: pg #/Q#
Pg. 5: Q6
Pg. 28: Q46, 47, & 48
Pg. 26: Q29; Pg. 28: Q51
Chapter 2
Vocabulary words (in bold throughout chapter) and:
Topics by section
2.1
 Identification of Extensive vs. Intensive
Properties
 The three different states of matter
 Characteristics of each state of matter
2.2
 Mixtures & the two types of mixtures
2.3
 Distinction between an element and a
compound
 Distinction between a substance and a
mixture
2.4
 Distinction between a chemical
property and a physical property
 Distinction between a chemical change
and a physical change
 Law of conservation of mass
Suggested Problems: pg #/Q#
Pg. 55/Q39
Pg. 55/Q43, 44
Pg. 37/Q6
Pg. 55/Q50; Pg. 56/Q72
Pg. 56/Q75
Pg. 56/Q73
Pg. 56/Q73; pg. 57/Q76,77,78
Pg. 57/Q80
Chapter 4
Vocabulary Words (in bold throughout chapter) and:
Topics by section
Suggested Problems: pg #/Q#
4.1
 Contributions of Democritus & Dalton Pg. 104/Q1, Q2; Pg. 122/Q37
toward the model of the atom
Pg. 104/Q6
 Relative size of an atom
 Instrument used to observe an atom
4.2
Pg. 109/Q11; Pg. 122/Q41
 What are the three types of subatomic
particles? What are their properties?
Pg. 109/Q12;Pg. 122/Q43
 Roles that Thompson, Millikan,
Goldstein, & Chadwick played in
identifying the three types of subatomic
particles
Pg. 109/Q13 to 15
 Rutherford Atomic Model
Topics by section
4.3
 What does the atomic number of an
element represent?
 What subatomic particles are taken into
account in an element’s atomic mass?
 What is an isotope?
 Calculate the atomic mass of an
element using a weighted average
Suggested Problems: pg #/Q#
Pg. 113/Q16 & 17; Pg. 122/Q49
Pg. 114/Q18 & 19; Pg. 122/Q50
Pg. 122/Q52
Pg. 122/Q53; Pg. 119/Q25
Chapter 5
Vocabulary words (in bold throughout chapter) and:
Topics by section
5.1
 Bohr’s model of the atom; how it
compares to Rutherford’s Model
 Principle energy levels and sublevels;
shapes of sublevels
 Quantum mechanical Model
5.2
 Rules for writing electron
configurations (Aufbau Principle, Pauli
Exclusion, Hund’s rule)
 Elements that are the exception to the
rules when filling sublevels
5.3
 Characteristics of Light as a wave
(amplitude, wavelength, frequency)
 Electromagnetic Spectrum &
relationship between wavelengths and
energy, frequency
 Energy associated with light (Planck’s
constant problems)
 Photons & the photoelectric effect
(light as a particle)
Suggested Problems: pg #/Q#
Pg. 132/Q1
Pg. 132/Q4; Pg. 155/Q34
Pg. 152/Q36-38; 40; Pg. 153/Q56
Pg. 152/Q45; Pg. 154/Q68
Pg. 152//Q47
Pg. 153/Q64; 66
Pg. 154/Q70
Chapter 6
Vocabulary Words (handout & Word activity);
Periodic Table Activities done in class;
Name Origins of Elements (by people, place, Latin/Greek origin) and:
Topics by section
6.1
 Organizing principles of the periodic
table: past and present
 Three classes of elements; location on
periodic table; properties of each type
6.2
 Groups/Family names
 Horizontal rows = periods
 Representative elements 1A -8A
 Why members of a family are
chemically the same
 S, p, d & f blocks in periodic table
6.3
 Trends in atomic size
 Trends in ionization energy
 Trends in ionic size
 Trends in Electronegativity
 Formation of ions
Suggested Problems: pg #/Q#
Pg. 166/Q2, 3
Pg. 166/Q4,5,6,7
Pg. 173/Q14,15,16,17
Pg. 182/Q18
Pg. 182/Q20
Pg. 182/Q21
Pg. 182//Q22; Pg. 186/Q45
Chapter 7
Vocabulary Words (Handout & Word Activity);
How to Write a Winning Ionic Formula and:
Topics by section
7.1
 How to determine the number of
valence electrons: Representative
elements
 Electron Dot (Lewis)Structures
 Octet Rule & Ion Formation: Loss or
Gain of Electrons (or How do I become
Noble?Let me count the ways!)
Suggested Problems: pg #/Q#
Pg. 214/Q27, 28
Pg. 214/Q29
Pg. 214/Q32, 33, 34, 36
Topics by section
7.2
 Ionic Compounds are Electrically
Neutral: Writing Formula Units
 Properties of Ionic Compounds: high
melting point, good conductor of
electricity, held together by ionic
bonds, metal & nonmetal components
Suggested Problems: pg #/Q#
Pg. 214/Q35, 43, 44
LAB (Covalent vs. Ionic); Pg. 214/Q46
7.3


Crystalline Structure of Metals
Alloys you may be familiar with
Pg. 216/Q73
Pg. 216/Q75
Chapter 8
Vocabulary; How to write Electron Dot (Lewis) Structures for Compounds; and
Topics by section
8.1
 Molecules & Molecular Formulas
 Nobility now means sharing electrons
(covalent bonds)
Suggested Problems: pg #/Q#
Pg. 256/Q40,41
Pg. 256/Q45
8.2







Once again, the Octet Rule rules!
Different representations of molecules
& the information they tell you
Electron Dot Structures (Lewis
Structures)
Single to triple covalent bonds
Polyatomic atoms
Coordinate covalent bonds
Bond dissociation energy
Pg. 173/Q14,15,16,17; Pg. 256/Q57
Pg. 256/Q49,58
Pg. 256/Q47
Pg. 256/Q56
Topics by section
8.3
 VSEPR Theory
 Shapes of molecules/bond
angles/example molecules
Suggested Problems: pg #/Q#
8.4



Electronegativity & types of bonding
Intermolecular forces: Hydrogen bond,
van der Waals Forces
Properties of a Molecular Compound:
low melting point, sharing of electrons,
poor conductor of electricity, weak
intermolecular forces
Pg. 257/Q64, 65
Pg. 257/Q66,67,68
LAB (Covalent vs. Ionic)