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Unit 1 Test Study Guide
A. States of Matter
a. Matter is anything that has mass and takes up space.
b. Complete the table below on the States of Matter
Shape
Volume
Solid
Definite (Certain)
Definite
Liquid
Indefinite
(not fixed)
Definite
Gas
Indefinite
Indefinite
Picture of molecules
c. Give 3 examples of properties of matter.
i. Color- Physical property
ii. Melting and Boiling Point- physical property
iii.
Ability to have a chemical reaction- Chemical property
B. Mixtures vs. Pure Substances
a. Define Mixture: a substance made when mixing two or more substances together
b. What are the 2 types of mixtures?
i.
Homogenous
ii. Heterogenous
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c. Explain how each type of mixture is different.
Homogenous- mixture looks the same throughout the mixture. You cannot see the
individual components of the mixture.
Heterogenous- you can see the individual components of the mixture.
d. Give an example of each.
i. Homoegenous- Milk
ii.
Heterogenous- Salad
e. Define pure substance: substance made of one type of atom or molecule
f.
What are the 2 types of pure substances?
Elements are chemically the simplest substances and cannot be broken down
using chemical methods.
Compound- Made up of two or more elements chemically bonded together
g. Give an example of each.
i. Nitrogen- Element
ii.
Sugar- Compound
h. Identify the following as an element , compound, homogenous or heterogeneous
mixture
1. CO2- Compound
2. N - Element
3. Syrup- Homogenous Mixture
4. Ag - Element
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5. H2O - Compound
6. NaCl- Compound
7. Salt Water – Homogenous Mixture
8. Caesar Salad- Heterogenous Mixture
C. Atomic Theory
a. What is an atom?
An atom is the basic unit of an element, building blocks of all matter.
b. Summarize Dalton’s 5 postulates
i. All matter is made up of atoms
ii.
Atoms are indivisible and indestructible
iii.
Atoms of a given element are identical in size, mass, and other
properties; atoms of different elements differ in size, mass, and other
properties.
iv.
Atoms of different elements combine in simple whole-number ratio's
to form chemical compounds
v.
In chemical reactions, atoms are combined, separated, or rearranged
c. What is Conservation of Mass?
In chemical reactions, the mass will stay the same. Mass in neither created or
destroyed.
i. How does it relate to Dalton’s Atomic Theory?
The mass doesn’t change in chemical reactions because the atoms only
rearrange in the reaction, nothing is added or removed from the system.
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d. Draw a picture of Dalton’s Atom.
e. Was Dalton correct in his statement that Atoms cannot be further divided into smaller
pieces?
No
i. Explain. Atoms are made up into subatomic particles; protons, neutrons and
electrons.
f.
What did J.J. Thompson discover about the atom? Electrons (negatively charged
subatomic particles)
g. What did he call his model?
Plum Pudding Model
i. Draw a picture.
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h. Describe his experiment.
Experiment to show that cathode rays were electrically charged. The cathode ray tube
by which J.J. Thomson demonstrated that cathode rays could be deflected by a
magnetic field, and that their negative charge was not a separate phenomenon.
i.
What did Rutherford discover about the atom?
Atoms have a tiny heavy nucleus
j.
Describe his experiment.
Gold Foil Experiment- Rutherford designed an experiment to use the alpha particles
emitted by a radioactive element as probes to the unseen world of atomic structure.
They shot alpha particles at a sheet of gold foil, and noticed that most went
through, but some bounced back.
k. What was Rutherford’s original hypothesis for his experiment?
The particles would go through the foil.
i. What actually happened?
Some particles bounced backwards.
l.
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Draw Rutherford’s atom model.
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D. Periodic Table Nomenclature
a. Label each component on the periodic table for this element.
b. What does the Atomic Number tell you about the element? Number of protons and
electrons
c. What is the Element Symbol for this element? C
d. What is the Atomic Mass of this element? 12.01
e. What is the Mass Number? 12
f.
How would you determine how many neutrons are in this element? Subtract the atomic
number from the mass #
i. How many Neutrons are found in this element? (Show work)
12 – 6 = 6 neutrons
g. How many electrons are in this element? 6
h. How many protons are in this element? 6
i.
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What is the name of this element? Carbon
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Define isotope: Different versions of the same element. The have the same atomic
number, number of protons and electrons but a different mass number and number of
neutrons.
k. How can you tell isotopes of the same element apart?
They have a different number of neutrons
l.
Identify the missing components in the diagram below.
m. Write the number of proton, neutron and electrons for each isotope.
i.
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Nitrogen-15
Nitrogen- 20
# of Protons
7
7
# of neutrons
15-7= 8
20-7= 13
# of electrons
7
7
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