Physical Science: Quarter 1 Exam Study Guide
Nature of Science
1.
2.
3.
Phases of Matter
1.
Explain the difference between the normal and
scientific uses of the words “theory” and “law”.
Explain the difference between an observation and
an inference.
What are the various aspects of the nature of
science? Provide an example for each
Accuracy, Precision, Sci. Notation, & Significant Figures
1.
2.
3.
4.
Explain the difference between accuracy and
precision. (Make sure to know what each look like
visually)
What are the 3 main rules when counting significant
figures?
When doing calculations, what rules do you use
when rounding your final answer?
What steps are necessary when converting numbers
from standard notation to scientific notation?
Intro To Chem
1.
2.
What are the 5 fields of chemistry we covered in
class and what does each study?
What two things are studied in chemistry?
Properties & Changes
1.
2.
3.
4.
5.
6.
Atoms & The Periodic Table
1.
2.
3.
4.
5.
6.
7.
8.
9.
How are groups arranged on the Periodic Table?
What do these elements have in common?
How are Periods arranged on the Periodic Table?
What information can you gather from an element
square? What does it tell you about the number of
certain subatomic particles?
If you had an atom of an unknown element, which
subatomic particle could you use to identify it?
What are valence electrons? Why is it useful to know
how many an atom has?
How are isotopes of the same element different
from each other?
Define and explain:
a. Isotope
b. Atomic Mass
c. Atomic Number
d. Atom
How do you calculate average atomic mass?
What are the different groups found on the periodic
table? For each, give the name, group number,
characteristics, and at least 2 elements found in it.
10. What are the three types of elements found on the
periodic table? What are the characteristics of each?
For EACH of the 3 phases of matter covered in class,
list:
a. What do the particles look like? (draw it!)
b. How the particles are in relation to each
other
c. Whether it has definite volume & shape
d. The amount of energy its particles have
compared to other phases
e. 1 example
What is a property?
What’s the difference between a physical & a
chemical property? Give 2 example for each type of
property.
What’s the difference between a physical & a
chemical change? Give 2 examples of each type of
change.
a. What’s another name for a chemical
change?
What happens to the way atoms are bonded during
a chemical change?
What are some observable signs that a chemical
change has occurred?
Look at the picture below. Which is a chemical
change AND WHY:
Elements & Compounds
1.
2.
3.
Compare & Contrast elements & compounds
How are the properties of compounds different from
the elements that it is composed of?
Know how to read and write chemical/elemental
formulas (see back for practice problems)
Chemical Nomenclature
1.
2.
3.
4.
Know how to name binary molecular compounds
given a chemical formula (practice on the back)
Know how to come up with chemical formula for
binary molecular compounds given standardized
names (practice on the back)
What are the prefixes for # of atoms
What are the proper names for nonmetals when
adding -ide?
Unit Test 1 Math Practice Problems
Name: _________________________________ Block: _____
Directions: Fill in the missing information in the following table. Assume all atoms are neutral.
Element Name
Atomic Symbol
Atomic #
Atomic Mass
# of protons
# of neutrons
# of electrons
As
24.305
Bromine
Directions: Find the number of neutrons and protons for the isotopes listed below.
Isotope
# of Protons
# of Neutrons
Silver-109
Directions: Solve the following math problems on a separate piece of paper. Remember to SHOW YOUR WORK, BOX
your answers, and include the proper UNITS and CORRECT SIG FIGS.
1. Find the number of significant figures in the following numbers:
a. 34.550
b. 0.059100
c. 103.22
d. 0.000100
e.
40.0021
2. Convert the numbers from Questions 1 into scientific notation. Round to 2 decimal places.
3. Potassium has 3 naturally occurring isotopes. Potassium-39 has an isotopic mass of 38.963707amu and makes
up 93.2581% of all potassium atoms. Potassium-40 has a mass of 39.963999amu and makes up 0.0117% of all
potassium atoms. Potassium-41 has a mass of 40.961826amu and makes up 6.7302% of all iron atoms. Using
these measurements, what should the calculated average atomic mass of an iron atom be?
Directions: Fill out the information missing in the table below.
Standardized Name
Chemical Formula
S3N7
C6N
SeF2
Dinitrogen pentabromide
Trioxygen tetraiodide
Monophosphorus octachloride
Directions: Answer the questions on a separate piece of paper.
1. Which elements and how many atoms of each are in the following compounds: (NH4)2CrO4,Ce(SO4)2, NaBrO3
2. Pretend Bromine exists in nature as 3 bromine atoms bonded together. What is its elemental formula?