Download Explain what he discovered and draw a diagram of the cathode

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.
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?
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
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. 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?
5. Your friend argues that the Periodic
Table is organized by atomic mass. Use
evidence from the Periodic Table to
disprove your friend’s claim.
Station 4 – LT 1.4
Lesson
1.4 – Electron Configurations and the
Octet Rule
Questions Take out your “Build An Atom
Simulator” handout in your binder. Go
through the simulator to review the
important concepts. NOTE – You
cannot spend more than 15 minutes at
this station!
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?
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
Question 1. Why do elements in the same group
s
demonstrate similar properties?
2. Label the alkali metals, alkaline earth
metals, transition metals, halogens, and
Noble Gases on the table shown below:
3. Give one common property of alkali
metals, alkaline earth metals, halogens,
and Noble Gases
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 Ven Diagram of the properties
of metals, non-metals, and semimetals.
3. Label the following as metals,
nonmetals or semimetals:






Carbon
Selenium
Copper
Barium
Silicon
Magnesium






Bromine
Hydrogen
Polonium
Rubidium
Fluorine
Vanadium
Station 8 – LT 1.7
Lesson
1.6 – Ionization Energy
Questions 1. What does the ionization energy of
an element describe?
2. How does nuclear charge contribute
to an element’s ionization energy?
3. What is the trend in ionization
energy as you go across a period?
Down a group?
4. Why do these trends exist?
5. Sort the following elements from
lowest to highest ionization energy:
a. O, S, Po _______________
b. F, O, N _______________
c. Na, Li, K _______________
Station 9 – LT 1.8
Lesson
Questions
1.7 – Electronegativity and Atomic
Radius
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 ________________
c. Cs, F, Ga _______________
Station 10 – LT 1.7, 1.8, and 1.9
Lesson
1.6 – Ionization Energy
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 ________________
c. Cs, F, Ga _______________
5. Nuclear charge plays a major role in the
three periodic trends that we studied.
Write a short response describing to
someone what nuclear charge is and how it
leads to the trends that we observed for
electronegativity, ionization energy, and
atomic radius that we observed.