STUDY GUIDE FOR THE SEMESTER FINAL
The exam covers the first six chapters of our textbook
This study guide is not comprehensive
The exam includes multiple-choice questions, short-response questions, and a15-line essay.
The periodic table will be provided
For the exam, bring only your calculator, no2 pencils, and pens (scantrons will be collected in class)
Areas of emphasis



The metric system
Prefixes and their symbols
Units for mass, volume and length; their symbols
2)Significant figures; rules for:
 Counting significant figures\
 Rounding up/down
 +, -, X, and dividing with significant figures
3)Definitions
Isotope
Atomic number
Mass number
Mole
Molar mass
Avogadro’s constant
Average atomic mass
4)From the atomic and mass numbers, and also from the “hyphen notation”, find the number of protons, neutrons, and
electrons
5) From the number of moles, find the mass of an element sample and vice versa p. 82
6) From the number of atoms, find the mass of an element sample and vice versa p. 82
Connection between electron
configuration and the periodic
table
Trends
Pages 128 to 139
P. 156/157, # 27 to 31
Pages 140 to 153
P. 157#32, 34, 35
Chapter 1
Distinguish between physical changes and chemical changes
Distinguish between elements, compounds, pure substances, and mixtures
Define volume, weight, mass, density
Explain, with diagrams representing the particles, the difference between
 Gases
 Liquids
 Solids
State the law of conservation of energy as applied to chemical reactions
Define chemical reaction
Chapter 2
Given a measurement, determine the number of significant figures
Round off data to a preset number of significant figures
Add, subtract, multiply, and divide data, and express the result with the right number of significant figures
Given sets of data, compare them as to accuracy and precision
Chapter 3
Dalton’s atomic theory
Define atom
Draw a diagram of the atom showing the nucleus, the protons, the neutrons, the electrons, and the valence
electrons
Determine the number of electrons, neutrons, and protons from the mass number and atomic number
Determine the atomic number and mass number from the number of neutrons and protons
State and apply three laws:
 Definite proportion
 Multiple proportions
 Mass conservation
Convert back and forth between mass and number (or fractions) of moles
Chapter 4
Principal quantum number
Angular quantum number
Magnetic quantum number
Spin quantum number
Main energy level
Subshell
Orbital
Spin
Define
 quantum numbers
 orbitals (p. 100)
Distinguish between subshells
Distinguish between orbitals in a subshell
Given an element, write the electron configuration by placing the correct number of electrons in each:
 Energy level
 Subshell
 Orbital
What is meant by quantized energy? (Think of the example of the ATM machine, and apply this to the position
of the electrons in an atom as it depends on their energy)
State and apply:
 Hund’s rule
 The Pauli exclusion principle
 The Aufbau principle
Given an element, write its orbital notation by applying the three aforesaid rules, and, as well, the electron
configuration and the noble-gas notation
Chapter 5
Describe the basic arrangement of the periodic table
In the periodic table:
a) How are columns called?
b) What does it mean for elements to belong to the same column?
c) How are rows called?
d) What does it mean for elements to belong to the same row?
e) How do you determine the number of valence electrons?
f) Where are the most reactive elements? The least reactive? Can they form compounds?
Compare and contrast the properties of metals, metalloids, and non-metals; locate them in the periodic table
State the periodic law
Define:
 Electronegativity
 Ionization energy
 Electron affinity
What happens to energy when:
 An electron changes levels within an atom?
 An electron is added to (or: removed from) an atom?
Chapter 6
What are covalent bonds?
They result from the attraction between _________ and protons.
Distinguish between polar and nonpolar covalent bonds
Use electronegativity to distinguish between types of bonds
Given the formula of a covalent compound, draw the electron-dot Lewis structure
How are valence electrons shared in metals?
Malleable means ___________ .
Why are metals malleable?
The topic of the essays may be like these:
a) Discuss the structure of the atom, based on the 3D model you constructed as a class project
b) Discuss three reasons why the periodic table is such a precious tool in chemistry.