MIDTERM STUDY GUIDE—CP CHEMISTRY 09/10
Topics are listed in the order that they appear in the sections of a chapter.
CHAPTER 1





What is Chemistry?
What are the parts of the Scientific Method?
How is data plotted? What goes where?
Use histograms to analyze a set of related data.
Describe how density can be measured. Explain the relationship density=mass/volume.
Given any two variables in this formula, calculate the third.
 Significant figures — definition & use in calculations
CHAPTER 2
What kinds of energy are there? Examples?
Law of Conservation of Energy; Law of Conservation of Matter
Celsius and Kelvin temperature scales & conversions
States of matter and their properties
Physical vs. chemical changes
Elements, compounds and mixtures
CHAPTER 3
 Law of conservation of matter
 Law of constant composition
 Dalton’s atomic theory of matter
 Complete and know the information in this table:
Scientist
Experiment
What it proved
Rutherford
Thompson
Milliken
 Know ALL vocabulary words for section 3-2
 Be able to compare the relative mass and charge of a proton, a neutron and an
electron
 Given an atom or ion, be able to tell how many protons, neutrons, electrons are
present
 Given a number of protons, neutrons, electrons, be able to write the element symbol
with the appropriate atomic number, mass number, and charge
 Atomic mass unit—what is it?
 Isotopes and their effect on the atomic masses listed in the periodic table
CHAPTER 4
 “Light energy is quantized.” — what does this mean?
 Photons—definition, and how they relate to line spectra and the photoelectric effect
 Why do different elements have different line spectra—what IS the line spectrum of
an element? How are they formed?
 Bohr’s model of the atom — what was it and what was wrong with it?
 Principle quantum number, n
 Ground state
 Excited state
 Transitions between energy levels—what kind of transition is caused by photon
absorption, and what kind leads to photon emission?
 Principle energy levels and what orbitals (sublevels) they contain—also be able to
relate this to the layout of the periodic table
 Orbital shapes and names (s, p, d, f)
 How many s, p, d and f orbitals are there for a given energy level?
 Electron spin
 Order that orbitals fill with electrons
 Orbital diagrams (p. 148)—be able to recognize correct and incorrect orbital diagrams
for different electron configurations
 How periodic table position shows you what orbitals to include in the electron
configuration for that element
 Given an element, recognize the correct electron configuration
 Given an electron configuration, figure out the name of the element
 Use an electron configuration to figure out what Group or Period of the Periodic
Table the element is located
CHAPTER 5
 Who is Mendeleev? What did he do?
Label (from Ch. 5 Section 2):
 s, p, d, f-blocks—you may only see these in sections, so be familiar with the height
and width of the blocks, as well as a few of the elements from the block
 Major Groups by name (alkali metals, etc.)—try to be familiar with at least a couple
elements in each group
 Metals, nonmetals, semimetals (metalloids)—try to be familiar with at least a couple
elements in each group
DEFINE:
 Ion size
 Electronegativity
 Electron affinity
 Ionization energy
 Atomic radius
 Be able to describe how the above change either going across a period or down a group
 Know the terms PERIOD and GROUP
 Be able to relate the number of elements in a period to what sublevels (orbitals) are
present for that period; Ex: period 2 has s (2 e-) and p orbitals (6 e-), so should have 8
elements in it
 Going down a group in each block, how do the atomic numbers change? (there’s a
pattern)
CHAPTER 7
 Name all cations on p. 231
 Name all anions on p. 232
 Write the number of valence electrons for any s- or p- block element—be able to do this
using the GROUP NUMBER or the group name
 Write the name and formula for any s-block or p-block ion, based on its location on the
periodic table.
 Given the name of any transition metal cation (with roman numeral) write the ion
formula. Given formula and periodic table, write the name with roman numeral.
 Draw the Lewis dot diagram for an element (given the periodic table)
 List characteristics of ionic compounds
 List characteristics of covalent compounds
 State the number of shared electrons that make up single, double, and triple bonds
 Given electronegativity values, be able to classify ANY bond as ionic, polar covalent, or
nonpolar covalent
 Know the acid names on p. 249
 Draw Lewis Dot Structures for covalent compounds
FOR BOTH IONIC AND COVALENT COMPOUNDS:
 Given the compound name, write its chemical formula
 Given a chemical formula, name the compound