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Student Packet for 12/7/15 – 12/11/15
Midterm set up:
40 Definitions
1. Hypothesis
2. Independent variable
3. Dependent variable
4. Observation
5. Constants
6. Control
7. Conclusion
8. Qualitative and quantitative
9. Accuracy and precision
10. Endothermic and exothermic
11. Matter, mass, volume, density
12. Solution, heterogeneous and homogeneous mixtures, colloids, suspensions
13. Solute and solvent
14. Protons, neutrons, electrons, ions, isotopes
Topics to be covered : 60 Questions
1. Be able to list and explain the steps in the Scientific method
2. Matter and its states, heterogeneous and homogeneous mixtures and their properties; compounds and elements
3. Chemical and physical properties and changes
4. Calculation of density, mass, volume
5. Charles and Boyles gas law
6. Endothermic and exothermic reactions
7. Atomic theories and models (Democritus, Dalton, Rutherford, Bohr)
8. Periodic table and its trends
9. Calculating subatomic particles
10. Ions and isotopes
11. Bohr Model
12. Electron Configuration, Energy Levels and orbitals
13. Valence Electrons
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List and describe the six steps to the scientific method in order.
1. ____________________________________________________________________________
2. ____________________________________________________________________________
3. ____________________________________________________________________________
4. ____________________________________________________________________________
5. ____________________________________________________________________________
6. ____________________________________________________________________________
7. ________ A student decided to set up an experiment to see if cats preferred skim milk or 2% milk. She put
out a cup of milk for 5 kittens and then measured how much the kittens drank over the course of a day. The
same kittens were used and the milk was served at the same temperature. The student discovered that the cats
liked the 2% milk more than the skim milk. What is wrong with the above experiment?
A. There is no independent variable.
B. The milk should be served at different temperatures
C. There are no constants present.
D. Repeated experimentation is needed
Raising the average temperature of the earth’s atmosphere will cause the polar ice caps to reduce in size.
8. ______________________________ is the independent variable
9. ______________________________ is the dependent variable
10. What is the control group?_________________________________
11. What is the independent variable?_____________________________________
12. What should Smither’s conclusion be?____________________________________
__________________________________________________________________________
__________________________________________________________________________
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1. Define Each of the following:
matter
volume
weight
gravity
mass
physical property
conductivity
malleability
ductility
solubility
density
boiling point
melting point
solute
solvent
atom
element
molecule
compound
heterogeneous mixture
homogeneous mixture
chemical property
flammability
reactivity
precipitate
viscosity
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2. Identify the following changes as either physical or chemical. Be able to explain your answer.
a. Burning coal
b. Baking brownies
c. Dissolving sugar in tea
d. Melting butter
e. Exploding fireworks
3. What are the signs of a chemical change?
4 What are the two types of pure substances? How are they alike? How are they different?
5 What are the three types of mixtures? How are they alike? How are they different?
6. draw a flow chart showing the classification of matter
DENSITY
1. What is the density of CO gas if 0.196 g occupies a volume of 100 ml?
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2. A block of wood 3 cm on each side has a mass of 27 g. What is the density of the
block? (Hint, don’t forget to find the volume of the wood.)
3. A block of lead has dimensions of 4.50 cm by 5.20 cm by 6.00 cm. The block
weighs 1587 g. From this information, calculate the density of lead.
4. What is the density of a board whose dimensions are 5.54 cm x 10.6 cm x 199 cm and
whose mass is 28.6 g?
5. Calculate the mass of a liquid with a density of 3.2 g/mL and a volume of 25mL.
6. Calculate the density of a 500 g rectangular block with the following dimensions:
length=8 cm, width=6 cm, height=5 cm
7. An irregular object with a mass of 18 g displaces 2.5mL of water when placed in a
large cylinder. Calculate the density of the object.
8. A graduated cylinder has a mass of 80g when empty. When 20 mL of water is added,
the graduated cylinder has a mass of 100 g. If a stone is added to the graduated
cylinder, the water level rises to 45 mL and the total mass is now 156 g. What is the
density of the stone?
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9. Draw the graphs for and explain Endothermic and Exothermic Reactions.
On the periodic table, these symbols refer to what elements?
1. Ar- ______________________ 2. Be _______________________
3. B ________________________
4. P - __________________________
5. Si- ___________________
6. Na ________________________
7. He- ________________________ 8. Mg- _________________________
9. N - ________________________ 10. Cl- ___________________________
11. Li _________________________ 12. F - ___________________________
13. Hydrogen ___________
14. Neon __________
1. The order of elements in the periodic table is based on
_________________________________________________________________________________
_________________________________________________________________________________
2.
Atoms of elements that are in the same group have the same number of
______________________________________________________________________________
3. List alkali metals and give 2 characteristics
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4. List Alkaline earth metals and give 2 characteristics
5. List the halogens – and give 2 characteristics
6. List the noble gasses – and give 2 characteristics
7. What groups form anions? What groups form cations?
8. Group 1 is called _____________________________
9. Group 2 is called ___________________________
10. Groups 3-12 are called _________________________________________
11. Group 17 is called ___________________________________
12. Group 18 is called __________________________________
13. What are metalloids
__________________________________________________________________________
__________________________________________________________________________
Development of Atomic Theory: Part 1 (Democritus to Thomson)
Do ideas or theories in
Science stay the same? What
causes this?

Who was Democritus?
What does the Greek word
atomos” mean?

________________________________
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What is our modern definition
of the atom?
In the late 1700’s a British
chemist and schoolteacher,
John Dalton, brought back
Democritus’s idea of the atom.
What 3 ideas did his new
theory of the atom propose?
In 1897 a British scientist
named Thomson discovered
that atoms were not indivisible
but were made up of smaller
particles. What particle did
Thomson discover and what
electrical charge does it
have?
Thomson showed that
electrons were part of atoms.
 Where did he think
they were?
 What was the funny
name for this
model?
 Draw a model of
the atom proposed
by Thomson Label
electrons.
1. _________________________________
_________________________________
_________________________________
_________________________________
2. _________________________________
_________________________________
_________________________________
3. _________________________________
_________________________________
The particle Thomson discovered was the
____________. It has a ___________charge.
On the back of this sheet draw a diagram
(Fig. 3) that shows the Cathode Ray
Experiment” that Thomson used to prove
that atoms included smaller particles.
(.Include all text boxes a-e)
 Thomson believed the electrons were
______________________________________
 Thomson’s model was called the
________________________________ but
today we might call it the _________________
_____________________________________.
In 1909 a former student
of Thomson’s, Ernest
Rutherford decided to
test the idea that
electrons are evenly
distributed throughout the
atom. Draw a diagram
that shows Rutherford’s
Gold Foil Experiment.
Label
What did Rutherford
discover about the
 Most of the particles ____________________
_______________________________________
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movement of the particles
that he shot at the gold
foil?
Due to the results of his
experiment Rutherford
revised the atomic
theory in 1911. Using
Fig. 6 and page 168
complete the
statements that
describe Rutherford’s
revised atomic theory.
 But surprisingly a few particles ____________
___________________________ and some
even ________________________________
Result: Most of the positively charged particles went
straight through the gold foil.
Atomic Theory: Most of the matter of the atom is
found in a _________________part of the atom.
This is called the ___________ of the atom. It is very
tiny and extremely __________.
Result: Some of the positively charged particles
were deflected or even bounced back.
Atomic Theory: Like charges repel so the nucleus
must have a _____________________. If electrons
have a negative charge they could not be in a
positively charged nucleus. Electrons must
______________________________________.
Result: The diameter of the nucleus is 100,000
times smaller than the diameter of the entire gold
atom.
Atomic Theory: Atoms are mostly ______________
with a tiny, massive _________________________.
In 1913, Niels Bohr
studied the way that
atoms react to light.
 What did he learn
about electron
movement?
 Can they change
paths?
The Modern Theory of
the atom states that
electrons do not travel in
specific paths or orbits.
 Describe the
region where
electrons travel.
 Can we predict
where an electron
may be found?
Electron clouds exist at a
certain Energy Level.
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Therefore the energy
that an electron has is
based on what?
1. Draw representatives of the atomic model and explain them for each of the following
Dalton
Thompson
Rutherford
Bohr
Worksheet: Boyle’s Law and Charles’s Law
CHEMISTRY: A Study of Matter
1. Boyle’s Law: When
_ proportional.
_ is held constant, the pressure and volume of a gas are
2. Mathematically, Boyle’s law is stated PV =
_ or P1V1 =
.
3. At a pressure of 405 kPa, the volume of a gas is 6.00 cm3. Assuming the temperature remains
constant, at what pressure will the new volume be 4.00
cm3?
4. A volume of gas at 1.10 atm was measured at 326 cm3. What will be the volume
if the pressure is adjusted to 1.90 atm?
5. If 36.5 m3 of a gas are collected at a pressure of 755 mm Hg, what volume will
the gas occupy if the pressure is changed to 632 mm Hg?
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7. Mathematically, Charles’s Law is stated: V/T = ________or V1/T1 = ____________________
8. The ___________________ temperature scale must be used in all gas law problems.
9. At 189 K, a sample of gas has a volume of 32.0 cm3. What volume does the gas
occupy at 242 K?
10. 10. The gas in a balloon occupies 2.25 L at 298 K. At what temperature will theballoon
expand to 3.50 L?
11. A sample of gas has a volume of 852 mL at 25°C. What Celsius temperature is
necessary for the gas to have a volume of 945 mL?
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History of the Atom Worksheet
John Dalton (1766 – 1844):
John Dalton was an English chemist. His ideas form the atomic theory of matter.
Here are his ideas.




All elements are composed (made up) of atoms. It is impossible to
divide or destroy an atom.
All atoms of the same elements are alike. (One atom of oxygen is like
another atom of oxygen.)
Atoms of different elements are different. (An atom of oxygen is
different from an atom of hydrogen.)
Atoms of different elements combine to form a compound. These
atoms have to be in definite whole number ratios. For example, water
is a compound made up of 2 atoms of hydrogen and 1 atom of oxygen
(a ratio of 2:1). Three atoms of hydrogen and 2 atoms of oxygen
cannot combine to make water.
1. What is the name of John Dalton’s theory?
_____________________________________
2. What are elements made of?
________________________________________________
3. An atom of hydrogen and an atom of carbon are
_________________________________.
4. What are compounds made of?
_______________________________________________
5. The ratio of atoms in HCl is:
a) 1:3
b) 2:1
c) 1:1
J. J. Thompson (Late 1800s):
J. J. Thompson was an English scientist. He discovered the electron when he
was experimenting with gas discharge tubes. He noticed a movement in a tube.
He called the movement cathode rays. The rays moved from the negative end
of the tube to the positive end. He realized that the rays were made of
negatively charged particles – electrons.
1. What did J.J. Thompson discover?
_____________________________________________
2. What is the charge of an electron?
____________________________________________
3. What are cathode rays made of?
______________________________________________
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4. Why do electrons move from the negative end of the tube to the positive
end?
________________________________________________________________
__________
5. What was Thompson working with when he discovered the cathode rays?
________________________________________________________________
__________
Lord Ernest Rutherford (1871 – 1937):
Ernest Rutherford conducted a famous experiment called the gold foil
experiment. He used a thin sheet of gold foil. He also used special equipment to
shoot alpha particles (positively charged particles) at the gold foil. Most
particles passed straight through the foil like the foil was not there. Some
particles went straight back or were deflected (went in another direction) as if
they had hit something. The experiment shows:


Atoms are made of a small positive nucleus; positive nucleus repels
(pushes away) positive alpha particles
Atoms are mostly empty space
1. What is the charge of an alpha particle?
_______________________________________
2. Why is Rutherford’s experiment called the gold foil experiment?
_____________________
________________________________________________________________
__________
3. How did he know that an atom was mostly empty space?
__________________________
________________________________________________________________
__________
4. What happened to the alpha particles as they hit the gold foil?
_____________________
________________________________________________________________
__________
5. How did he know that the nucleus was positively charged?
_________________________
________________________________________________________________
__________
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Niels Bohr (Early 1900s):
Niels Bohr was a Danish physicist. He proposed a model of the atom that is
similar to the model of the solar system. The electrons go around the nucleus
like planets orbit around the sun. All electrons have their energy levels – a
certain distance from the nucleus. Each energy level can hold a certain number
of electrons. Level 1 can hold 2 electrons, Level 2 - 8 electrons, Level 3 - 18
electrons, and level 4 – 32 electrons. The energy of electrons goes up from level
1 to other levels. When electrons release (lose) energy they go down a level.
When electrons absorb (gain) energy, they go to a higher level.
1. Why could Bohr’s model be called a planetary model of the atom?
__________________
________________________________________________________________
__________
2. How do electrons in the same atom differ?
_____________________________________
________________________________________________________________
__________
3. How many electrons can the fourth energy level hold?
____________________________
4. Would an electron have to absorb or release energy to jump from the second
energy level to the third energy level?
_____________________________________________________
5. For an electron to fall from the third energy level to the second energy level,
it must ___________________________________ energy.
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