Chemistry Lab Methods: Review for Test 1
Name: _________________ Period: ____ Date: _____
Sample Questions
Labs
1. Rutherford’s gold foil experiment resulted in a change in the atomic structure model of the time
– from the “Plum Pudding” model to the “Rutherford” model. What were the two main changes
to the model?
2. Which of the sub-atomic particles were transferred when the rulers in the Electrical Charge lab
were rubbed with wool or plastic?
3. What would you predict would happen if both rulers were rubbed with wool – and then held
close together?
4. Which of the two particles – iodine or starch – moved through the dialysis tubing in the Another
Look at Size lab?
5. What evidence did you have that the substance really did move through the tubing?
6. Other than being small enough to fit through the “holes” in the tubing, what else was happening
to allow the particles to move from one side to the other?
Atomic Structure
1. Atoms are made up of what three sub-atomic particles?
2. In a neutral atom, there are the same number of which two sub-atomic particles?
3. The nucleus of an atom contains which two sub-atomic particles?
4. Which of the sub-atomic particles travel in orbits? What is the charge of these particles?
5. The mass number of an isotope equals the total number of which two sub-atomic particles?
6. If an atom gains an electron, what charge does it become?
7. What is a negatively-charged ion called? What is a positively-charged ion called?
Periodic Table
1. What element characteristics were used to arrange the table?
2. An element is defined by which of the three subatomic particles?
3. What are the columns called and how are the elements in each column similar to each other?
4. What are the horizontal rows called and how many are there in the Periodic Table?
5. To which family does each of the following columns of elements belong? (Give the family name)
a. Farthest column to the right _____________
b. Column with Fluorine at the top ____________
Chemistry Lab Methods: Review for Test 1
Name: _________________ Period: ____ Date: _____
6. Fill in the following table for a NEUTRAL atom:
Element
Symbol
# protons
# electrons
Atomic Mass
Gold
Ga
17
7. Fill in the following table:
Mass Number: most common
Element
isotope
Carbon
Bromine
Potassium
8.
#
protons
#
neutrons
Isotope Name
Fill in the following table:
Element
# Valence
Electrons
# Electrons atom
will gain or lose
Charge of ion likely
to form
Symbol for
ion
9. How many electrons do elements in column 1 tend to lose to form an ion?
10. Which element has fewer protons than helium?
11. What element would you get if you added 6 protons to a neutral carbon atom?
12. What element would you get if you added 3 electrons to a nitrogen atom?
Other topics to review
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Scientific Law & Theory – definitions and key similarities and differences
Observations & Interpretations – definitions and differences
Measurements – how to measure with a meter stick and with a graduated cylinder
Graphing – critical components of a good graph
Definitions - on the Vocabulary Wall
Unit Conversions – VERY comfortable with “level 1” problems. Ok with “level 2”.
Density – equation and calculations
Atomic Structure – be able to draw a model of an atom or ion
Labs – overview of procedure and results
Star Stuff video – all elements come from stars; Big Bang created cloud of hydrogen
Chemistry Lab Methods: Review for Test 1
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Name: _________________ Period: ____ Date: _____
This is the ion that is named first when naming ionic compounds.
This is the name for SO4
This is the chemical formula for sodium hydroxide
This is the chemical formula for beryllium nitride
This is the name for Li2SO4
This is the chemical formula for silver nitrate
This is what we call a bond that shares electrons
This is how an ionic bond is formed
This is the kind of bond likely to form between two non metals
The type of bond formed by Na and Cl
This is the type of bond that forms KNO3
The type of bond that c and o are likely to form with each other
Compounds containing this type of bond are likely to conduct electricity
C11H22011 in solution is likely to conduct electricity (true/false)
This is the name for the negatively charged ion in an ionic bond
This is the reason dry ionically bonded substances do not conduct electricity
This is why the iodine entered only one side of the dialysis tubing in the charged particles lab
Chemistry Lab Methods: Review for Test 1
Name: _________________ Period: ____ Date: _____
Things to study for chemistry test #1
Rutherford’s experiment
Structure of atoms (be able
to draw/calculate the
number of protons, neutrons,
electrons)
Protons, neutrons, electrons
(know where they are
located/their charge/how
many each atom has)
Metals, nonmetals,
metalloids, noble gases, ect.
Labs- electrical charge lab,
Rutherford, grouping by
chemical behavior,
Another look at size,
conductivity, know what
conducts and why (must be
ionic, must be in solution,
must contain mobile ions),
charged particles in solution
Ionic and covalent bonds (how
they’re formed, their properties,
what elements are likely to form
which)
Ionic compounds versus
molecules (formed with covalent
bonds) Naming ionic compounds
Writing compounds using names
Atoms or elements versus
compound
Valence electrons
Organization of the periodic table
Families and groups
Charges of atoms
Ch 17 and 23 in your textbook
Metric conversion
Metric system
Scientific method
Parts of a graph
Graphing
Length
Volume
Elements
Compounds
Density calculations
Mass
Temperature
Labs- mass and volume of
water, Measurement review
Density of water
3 step method
Measurement