Semester 1 Chemistry Final Study Guide
Chapter 1

Be able to distinguish between the chemical and physical properties of
matter

Classify changes in matter as chemical or physical

Explain the gas, liquid and solid phase of matter

Distinguish between a mixture and a pure substance
Chapter 2

Be able to convert between SI prefixes.
For example 2.8 cm= 2.8x10-3km

Be familiar with the tables on pg 34, 35, 36

Be able to calculate Mass, density or volume from the equation D=M/V

Refresh yourself about the Density of Pennies Lab and its objectives/
procedures
Chapter 3
SECTION 3.1

Be able to explain the Law of Conservation of Mass, the Law of Definite
Proportions, and the Law of Multiple Proportions

Be able to summarize Dalton’s Atomic Theory ( understand which parts
of his theory have changed and why)

Be able to explain the purpose of the Law of Conservation Lab,
observations, discrepancies in data, etc.
SECTION 3.2

Be able to summarize the cathode ray experiment and how it led to
knowledge that the electron has both mass and charge.

Be able to summarize Rutherford’s work the led to current understanding of
the nucleus

List properties of the protons, neutrons, electrons, and the nucleus. (Table
3-1 on pg 74 would be helpful)

Be able to explain why the nucleus is so small and dense (high mass and low
volume) it’s due to nuclear forces…see page 74.

Define and describe an atom
SECTION 3-3

Know how to write both hyphen notation and nuclear symbol for isotopes

Be able to calculate mass number, protons, neutrons, and electron for a given
isotope. (Ex Sample problem 3-1 pg77)

Know the difference between average atomic mass, relative atomic mass, and
molar mass. Remember they are all the same number, but have a different
use/ meaning.

Be able to solve for mass/ moles/ atoms. I will copy the chart on page 82 so
make sure that you can use it. Sample problems 3-2 through 3-5 are good
practice problems. Remember the best way to prepare for a test is to
practice the skill that you will be using on the test… practice problem
solving!!!
Chapter 22
From 22-1 be able to…

Define and relate the terms mass defect and nuclear binding energy

Know how to balance a nuclear equation (pg 704 sample and practice
problems)
Chapter 4 Section 1

Be able to explain the mathematical relationship between the speed,
wavelength and frequency of EMR. Be able to solve problems for either
frequency of wavelength.

Understand that light (EMR) behaves as both a wave and a particle. Know
what research that helped support this theory.

Understand and be able to explain the significance of the photoelectric
effect and the line emission spectrum of hydrogen to the development of
the atomic model.

Describe the Bohr model of the hydrogen atom and be able to explain why
the model was eventually discarded.
Chapter 4 Section 2

Be able to describe how the work of DeBroglie helped develop the idea of
the quantum model of the atom.

Be able to compare and contrast the Bohr model and the quantum model of
the atom.

Explain how the Heisenberg Uncertainty Principle and the Schrodinger Wave
Equation led to the idea of atomic orbitals.

List the four quantum numbers and describe what each represents.

Relate the number of sub-levels corresponding to each of an atom’s main
energy levels, the number of orbitals per sub-level, and the number of
orbitals per main energy level. (Table 4-2 pg 104)
Chapter 4 Section 3

Be able to list the total number of electrons needed to fully occupy each
main energy level.

State the Aufbau Principle, the Pauli Exclusion Principle and Hund’s Rule.
Understand how each rule governs the configuration of electrons.

Describe the electron configuration for the atoms of any element using
orbital notation, electron configuration, or noble gas configuration.

Be able to determine the number of valence electrons for an element from
the electron configuration.
Understand that only the highest s and p orbital electrons are valence
electrons. So d and f do not have valence electrons.

Understand that elements gain or lose electrons in order to become stable
like a noble gas. Be able to write the electron for an ion that has lost or
gained electrons.
Chapter 5-1

Describe the modern periodic table
Chapter 5-2

Describe the relationship of electrons in sublevels and the length of each
period of the periodic table (table 5-1 pg 128)

Locate and name the four blocks of the periodic table.

Understand the relationship between group configuration and group number.
(table 5-2 pg 137)

Describe general properties of elements on the periodic table based on their
location (alkali, alkaline-earth, transition metals, non-metals, halogens, noblegases.)
Chapter 5-3

Know group and period trends of ionization energy, atomic radii, reactivity,
electron affinity, ionic radii, and electronegativity.
Chapter 6-1

Define a chemical bond and explain why most atoms form chemical bonds.

Describe ionic and covalent bonding

Be able to determine if a bond is ionic, polar-covalent, or nonpolar-covalent
based on electronegativity differences.
Chapter 6-2

State the octet rule

Be able to draw Lewis structures for covalently bonded molecules, resonance
structures, and polyatomic ions. (Sample problems 6-2 6-4 pgs 170-174
would be good practice
Chapter 7-1

Use prefixes to name a binary molecular compound from its formula.Ex., CO2
is carbon dioxide

Write the formula of a binary molecular compound given its name
Ex., zinc iodide is ZnI2

Determine the formula of an ionic compound formed between two given.
Ex., Cobalt (IV) oxide is CoO2

Know common monatomic and polyatomic ions and their charges. (table 7-1 pg
205 and Table 7-2 pg 210)

Know the names and formulas of common binary acids and oxyacids (table 75 pg 214) Also covered in chapters 15-16
Chapter 7-2

Assign oxidation numbers of each element in the formula of a chemical
compound. (Rules for assigning oxidation numbers are on pg 216 and sample
problems on pg 217)
Chapter 7-3

Be able to calculate the number of molecules, formula units or ions in a given
molar amount of a chemical compound and be able to calculate the percent
composition of a given chemical compound (sample problems 7-9 to 7-11 pgs
225- 228 should be good practice.)
Chapter 7-4

Determine and empirical formula from either a percentage or a mass
composition. (Sample problems 7-12 and 7-13 pgs 230-231)

Determine a molecular formula from an empirical formula (Sample problem
7-14 pg 232)