Physical Science Mid-Term Study Guide
Atomic Theory
Describe the atomic theory over time (Rutherford, Bohr, Thompson, Dalton)
Describe the subatomic particles in terms of mass, charge and location
Draw a current model of an atom with correct placement of sub-atomic particles
How is the relative scale of atomic masses determined
Why was Rutherford surprised by his initial results of his gold foil experiment
If you could examine a single atom of gold and a single atom of lead, what would be similar about the
atoms?
What would be different about the atoms?
Periodic Table
What are valence electrons?
How are valence electrons related to an elements chemical properties
Write electron configurations
Identify trends in the periodic table
What is the pattern for increasing reactivity among metals and why
What is the pattern for increasing reactivity among non-metals and why
How does the Bohr model relate to electron configuration
How do trends in the periodic table allow for an easy understanding of how each element will bond with another
What is the “magic” number of e-‘s atoms seek for their outer energy level? ______ (except H, which would be happy
with 2)
Which groups are highly reactive and why?
Bonding to form compounds
A normal atom has ____ charge. When an atom gains or loses an e-, an ____ is formed which is another name for an atom
with a charge.
Alkali and halogens form strong bonds together called ____________ bonds, and form salts, like NaCl, KCl, LiBr, etc.
Any metal bonding with a nonmetal is an ionic bond.
If an atom gains a negative e-, it becomes a ___________ ion. If it loses a negative e- it becomes a _____________ ion.
When metals bond with other metals they simply share e-‘s and a less strong type of bond is formed called a
____________________ bond. Most compounds are this type of bond.
Only ____________ e-‘s participate in bonding. Atom’s properties are a result of these e-‘s.
Interpreting Chemical Formulas
When a chemical reaction occurs, you must count the atoms on both sides of the reaction because of the
_______________________________________.
The chemicals on the left side of the equation are called the __________ and on the right are the _______________. The
arrow between them means __________.
To balance an equation we can only place a _____________ in front of a molecule, as needed. It then gets
________________ times each subscript in the molecule.
When two or more substances combine to form one new compound the type of
chemical reaction is called a ________________ reaction. (p. 192)
When a single compound breaks down to form two or more simpler substances a ___________________ reaction has
occurred.
When one element replaces another element that is part of a compound we call that ______________ displacement (or
replacement) and when all the ions in two compounds switch places that is ______________ displacement.
When carbon is ignited in the presence of O2, a ___________ reaction occurs.
When an element has a different than normal number of neutrons it is called an _______________. You will see it
written like this: C-14 (with a dash and the new mass written next to the element’s symbol).
How does the law of conservation of matter relate to balancing equations?
Find example chemical equations and explain how it is this type of chemical reaction….
synthesis __________________________________________________________________________________
__________________________________________________________________________________________
decomposition______________________________________________________________________________
__________________________________________________________________________________________
single displacement(replacement)_______________________________________________________________
__________________________________________________________________________________________
double displacement_________________________________________________________________________
__________________________________________________________________________________________
combustion. ________________________________________________________________________________
___________________________________________________________________________________________
Mixtures
What is a pure substance?
What is a mixture
What is an element
What is a compound
What is a solution
Differentiate between heterogeneous and homogeneous mixtures
How can you determine whether a mixture is heterogeneous or homogeneous
Describe simple laboratory techniques that can be used to separate homogeneous and heterogeneous mixtures
(filtration, magnetism, evaporation, distillation, chromatography)
Physical/Chemical Properties
What are physical properties
Know the following terms: volume, mass, compressibility, density, conductivity, malleability, reactivity, Molecular
composition, freezing, melting and boiling points
Describe tests you would perform to determine if a sample was a metal or non-metal
Calculate the density of a substance
You notice that some metals are light such as tin or aluminum, while others are heavy, such as silver, gold and
Platinum. What physical and chemical properties support why this occurs and what evidence do you have to support your
answer
Acids/Bases
What are the characteristics of an acid
What are the characteristics of a base
What is the pH scale
How does the pH scale work
What is the relationship between pH and the H+ (hydrogen ion) concentration
How are pH and pOH related
How can a substance that is an acid be diluted into a base
An acid is any substance that forms hydrogen _____ (H+) in H20. These H+ ions bond with H20 to form H3O ions, aka
hydronium.Strong acids form more H+ ions than weak ones. A base forms hydroxide_______ (OH-) when placed in H20.
Strong bases from more OH- ions than weak ones.
When pH is low, the concentration of H+ is high. A low pH = acids. The lower the pH the stronger the acid. 7 is neutral.
Above 7 is basic. A higher pH = a stronger base.
Putting an acid and a base together causes ______________________ to occur which always produces H20 and salt.
Reaction Rates
Define the following:
Temperature
Pressure
Concentration
surface area
catalysts
activation energy
enzyme
reaction rate
inhibitor
Explain why it takes longer for food to go “bad” in a refrigerator rather than on the counter.
Why do you think doctors keep operating suites at very cold temperatures?
Why does it take a shorter amount of time to cook dinner in a pressure cooker than in a normal pot? Explain your answer.