Station 1 – LT 1.1
Lesson
1.1 – Introduction to the Atom
Questions 1. Where can you find the protons,
neutrons, and electrons in the atom?
2. What are the mass and charge of
protons, neutrons, and electrons?
3. Draw a picture of the atom. Label
the proton, neutron, and electron in
this model.
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your understanding of the concept using our
mastery scale.
4. On your picture from question 3, label the areas
of high density and the areas of low density. What
determines the density of each of these areas?
a. The energy level that the electrons orbit in
b. The nuclear charge of the nucleus pulling on
electrons
c. The mass of the subatomic particles contained in
the area
d. The concentration of energy in the region
Station 2 – LT 1.2
Lesson
1.2 – Development of Atomic Theory
Questions 1. Describe the experiment that J. J.
Thomson performed. Explain what he
discovered and draw a diagram of the
cathode-ray tube experiment that
demonstrated evidence for the
conclusion he reached.
2. Describe the experiment Ernest
Rutherford performed. Explain what
he discovered and draw a diagram of
the gold foil experiment that
demonstrated evidence for the
conclusion he reached.
3. How did Bohr modify Rutherford’s
model of the atom?
4. Below is a picture of Thomson’s plum
pudding model of the atom:
Explain how Rutherford’s and Bohr’s
experiments modified Thomson’s
model so as to develop the modern
model shown below:
electron
neutron
proton
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5. Niels Bohr modified Rutherford and Thomson’s
model of the atom by stating that:
A. Electrons are free to roam anywhere in the
electron cloud
B. Electrons can only orbit at specific energy
levels
C. Protons and neutrons must exist within the
nucleus of the atom
D. Protons and neutrons are free to roam
anywhere in the atom
Station 3 – LT 1.3
Lesson
1.3 – Introduction to the Periodic
Table
Questions 1. What determines an element’s
atomic number? What determines an
element’s atomic mass?
2. How is the Periodic Table
organized?
3. What is a group and what is a
period?
4. Your friend argues that the Periodic
Table is organized by atomic mass. Use
evidence from the Periodic Table to
disprove your friend’s claim.
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4. As you go down a group does an atom, generally,
get bigger or smaller? As you go across (left to
right) does an atom, generally, get heavier or
lighter?
a. Bigger; Heavier
b. Bigger; Lighter
c. Smaller; Heavier
d. Smaller; Lighter
Station 4 – LT 1.4
Lesson
1.4 – Electron Configurations and the
Octet Rule
Questions Open up the “Build An Atom Simulator”
handout in your binder. Go through the
simulator to review the important
concepts. NOTE – You cannot spend more
than 10 minutes at this station!
You can find this simulator at the link
below:
http://astronautschemclass.wikispaces.co
m/file/view/1.5.Lab%205.Build%20an%20
Atom.docx/522919750/1.5.Lab%205.Buil
d%20an%20Atom.docx
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1. When there is a difference between the number of
protons and the number of electrons what happens to
the atom?
a. The atom becomes heavier
b. The atom becomes unstable
c. The atom becomes stable
d. The atom becomes charged.
Station 5 – LT 1.4
Lesson
1.4 – Electron Configurations and the
Octet Rule
Questions 1. How many electrons can go in the
first electron orbit? How many
electrons can go in every orbit after
the 1st?
2. How can groups on the Periodic
Table provide a shortcut when drawing
Bohr structures?
3. Draw the Bohr electron
configuration for fluorine.
4. Draw the Bohr electron
configuration for nitrogen after it
satisfies the Octet Rule. What is the
charge of its ion?
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5. Draw the Bohr electron configuration for
magnesium after it satisfies the Octet Rule. What
is the charge of its ion?
Station 6 – LT 1.5
Lesson
1.5 – Metals, Nonmetals, Semimetals, and
Periodic Table Groups
Questions 1. Label the alkali metals, alkaline earth
metals, transition metals, halogens, and
Noble Gases on the table shown below:
2. Give one common property for each
group: alkali metals, alkaline earth metals,
halogens, and Noble Gases
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1. Why do elements in the same group demonstrate
similar properties?
a. Elements in the same group all have the same
number of valence electrons
b. Elements in the same group all have mass
c. Elements in the same group all have the same
number of neutrons
d. Elements in the same group all bond together
Station 7 – LT 1.6
Lesson
1.5 – Metals, Nonmetals, Semimetals,
and Periodic Table Groups
Questions 1. Describe how you determine if an
element is a metal, non-metal, or
semimetal.
2. What are some common properties
of metals, nonmetals, and semimetals?
Make a Venn Diagram of the
properties of metals, non-metals, and
semimetals.
3. Label the following as metals,
nonmetals or semimetals:




Carbon
Selenium
Barium
Magnesium




Bromine
Polonium
Rubidium
Vanadium
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4. Identify the following as metals, nonmetals, or
semimetals:
 i. Flourine
 ii. Copper
 iii. Silicon
 iv. Hydrogen
Station 8 – LT 1.7 and 1.8
Lesson
1.7 – Electronegativity and Atomic
Radius
Questions 1. What does the electronegativity of
an element describe?
2. How does nuclear charge contribute
to an element’s electronegativity?
3. What is the trend in
electronegativity as you go across a
period? Down a group?
4. Why do these trends exist?
5. Sort the following elements from
highest to lowest electronegativity:
a. Ca, Se, Ni ______________
b. O, Po, S ________________
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6. Sort the following elements from highest to
lowest electronegativity:
Cs, F, Ga _______________
Station 9 – LT 1.7 and 1.8
Lesson
1.7 – Electronegativity and Atomic
Radius
Questions 1. What does the atomic radius of an
element describe?
2. What is the trend in atomic radius
as you go across a period? Down a
group?
3. Why do these trends exist?
4. Sort the following elements from
smallest to largest atomic radius:
a. Ca, Se, Ni ______________
b. O, Po, S ________________
5. Nuclear charge plays a major role in the
three periodic trends that we studied.
Write a short response describing to an AP
student about what nuclear charge is and
how it leads to the trends that we
observed for electronegativity, ionization
energy, and atomic radius that we
observed.
LetsGeddit.com Taste Test! 6. Sort the following elements from smallest to
largest atomic radius:
a. Cs, F, Ga _______________