Download Atoms and the Periodic Table

ATOMS AND THE PERIODIC TABLE
Physical Science 2nd Semester
NAME: ____________________________
CLASS PERIOD: ______
TEACHER: __________________
ASSIGNMENT
Blank Periodic Table of Elements
Learning Targets: Atomic Structure
Scientific Contributions
PAGE
NUMBERS
DUE DATE
1
2-3
4
Build an Atom: Phet
5-6
Atomic Structure WS
7
Bohr Models
8
Periodic Practice
9
Periodic Family Notes
10-11
Atoms and the Periodic Table Review
12-13
TOTALS
HW POINTS
EARNED
LAB POINTS
EARNED
1
Learning Targets:
A: I can describe the
relative charges, masses,
and locations of the protons,
neutrons, and electrons in
an atom.
1 – Below Standard
What are the relative charges
of protons, neutrons, and
electrons?
2 – Approaching Standard
What are the relative masses of
protons, neutrons, and
electrons? What units are used
for these masses?
3 – At Standard
Draw a Bohr model of Boron,
labeling where electrons,
neutrons, and protons are
found.
4 – Above Standard
Describe how electrons move
around the nucleus of an atom.
If a neutral atom has 5
protons, how many electrons
will it have?
How are atomic number, mass
number, and atomic mass
different?
What is the atomic number of
Carbon? What is the mass
number of carbon if it has 7
neutrons?
Using the atomic mass, what is
the most common isotope of
Oxygen? How many neutrons
and protons are present in this
isotope?
Growth Chart:
1st
2nd
3rd
Lvl 4
Lvl 3
Lvl 2
Lvl 1
B: I can explain what
happens to an atom when
you change the number of
protons, neutrons, and
electrons.
Growth Chart:
1st
2nd
3rd
Lvl 4
Lvl 3
Lvl 2
Lvl 1
2
C: I can identify the mass
Fill out the following table.
number, number of protons,
number of neutrons, and
identity of an atom using the
periodic table.
Growth Chart:
Element
# Protons
1st
2nd
3rd
Lvl 4
Copper (Cu)
Mass #
# p+
12
6
19
Lvl 3
Gold (Au)
Lvl 2
13
35
3
Barium (Ba)
Lvl 1
D: I can predict the
chemical properties of an
element based on its valence
electrons.
Growth Chart:
1st
Fill out the following table.
2nd
14
18
15
1
#n0
20
1
Fill out the following table
Element
# p+
When do isotopes become
unstable? Is it the same
throughout the whole periodic
table?
#n0
C-13
F-18
Ta-182
H-2
How many valence electrons
do most atoms want?
Which of the following atoms
have the same number of
valence electrons: calcium,
sodium, fluorine, chlorine,
sulfur.
How does reactivity change as
you move across the periodic
table?
Why are alkali metals so
reactive? Which is the most
reactive?
Elements in the periodic table
are arranged based on
increasing ___________.
What are the columns called?
Rows?
What do each of the periods in
a periodic table represent?
What subatomic particle do
they correspond to?
How does atomic radii change
across a period? How does
reactivity change down a
group?
Why are halogens so reactive?
Why are noble gases inert? (Be
sure to mention electrons)
3rd
Lvl 4
Lvl 3
Lvl 2
Lvl 1
E: I can explain the
arrangement of the periodic
table, including significant
relationship among
elements in a given column
or row.
Growth Chart:
1st
2nd
3rd
Lvl 4
Lvl 3
Lvl 2
Lvl 1
3
Scientific Contributions
Cartoon
Hmmm… I wonder if I could
keep cutting this in half
forever?... Probably not, before
long it would be too small to see.
It would become invisible…. Ah
Ha! Invisible, indivisible… The
Atom
Scientists and their contributions:
Date:
2 important contributions to the Atomic Theory:
Date:
An Atom must be much like
a miniature solar system with
electons in orbit about the
nucleus, much like our
planets orbit our sun.
Scientist:
Scientist:
3 important contributions to the Atomic Theory:
Date:
Scientist:
2 important contributions to the Atomic Theory:
To my great astonishment I have discovered that
the atom is mostly empty space. It seems to be
occupied by a small dense positive force
surrounded by negatively charged particles.
…And so… all elements are made of atoms.
1. Atoms are invisible, indivisible particles
2. Atoms of the same element are identical
3. Atoms of different elements are
dissimilar
4. When two or more elements chemically
combine they form a compound
Date:
Scientist:
4 important contributions to the Atomic Theory:
These are the critical parts of MY “Atomic
Theory”!
Date:
My research has led me to
Scientist:
2 important contributions to the Atomic Theory:
believe that there are both
positive and negative forces
at work within the atom.
4
Build an Atom
Directions:
1. Go to http://phet.colorado.edu/en/simulation/build-an-atom and click the green “Run Now!” button.
2. Explore the Build an Atom simulation with all of the boxes open and checked to see all the info.
3. Using the simulation, talk with your group as you play with the parts of atoms to find:
A. What parts go in the center of the atom? _________________________________________
B. You can call the center of the atom, the nucleus. Most atoms in our environment have a stable nucleus.
Explore the simulation, and write down one example of an atom that has a stable nucleus and include a
drawing of your nucleus.
Number of particles in
Draw
What element
your nucleus:
your nucleus
is it?
Protons: __
Neutrons:__
1.
C. Which particle (or particles) determines the name of the element?___________________
Test your idea by identifying the element for the case below.
Particles
1.
What
Element?
Protons: 6
Neutrons: 7
Electrons: 5
What Determines
the Element?
Circle the Element
☐ Proton
☐ Neutron
☐ Electron
4. Explore until you discover what affects the charge of your atom or ion. What is a rule for making:
A. A neutral atom (one with 0 total charge)?
______________________________________________________________________________
B. A +ion (positive ion, one with extra positive charge)?
______________________________________________________________________________
C. A - ion (negative ion, one with extra negative charge)?
______________________________________________________________________________
5. Show a neutral atom, a positive ion, and a negative ion. (These examples should be consistent with the rules
you discovered.) All of your examples should also have a stable nucleus.
Number of Particles?
Neutral
Protons: __
Neutrons:__
Electrons:__
+ Ion
Protons: __
Neutrons:__
Electrons:__
- Ion
Protons: __
Neutrons:__
Electrons:__
Draw Your Atom or Ion
5
What is the Charge?
6. Explore what affects the mass of your atom or ion. Which particle(s) are heavy?______________ Which
particle(s) are light?_________ What is a rule for determining the mass?______________
7. Using all of your rules, figure out what changes for each of these actions to an atom or ion. You can test
your ideas with the simulation. If you have new ideas, rewrite your rules.
Action
What
Changes?
How Does it Change?
☐ Element
Add a
Proton
Action
☐ Charge
☐ Mass
What
Changes?
How Does it Change?
☐ Element
Remove a
Neutron
Action
☐ Charge
☐ Mass
What
Changes?
How Does it Change?
☐ Element
Remove an
Electron
☐ Charge
☐ Mass
8. What does the tool called Symbol tell you about what parts are in an atom or ion?
 What rules can you use to tell how many protons, neutrons and electrons make
atom or ion from the information in the symbol?
up an
 Check your ideas with the simulation and write down two examples that show your rules work and
include a drawing and the correct symbol for each.
9. Click the tab at the top that says “Game”.
a. Play each level until you score at least 9 out of 10, and have your teacher check it off once you are done.
Your quiz Friday will probably be very similar to this!
Level 1 _____
Level 2 _____
Level 3 _____
Level 4 _____
6
1. What are the three main particles that make up an atom? List their charges and masses.
Particle:
Charge:
Mass:
2. Which of those particles make up the nucleus?
3. In the neutral atom, the number of _____________ always equals the number of ______________.
4. The number of ____________ plus the number of ____________ always equals the mass number of
an element.
5. When the # of neutrons change within the same element, the end result is a(n) ________________.
6. A ______________ is a chemical combination of two or more elements.
7. Calculate how many protons and neutrons are in the following isotopes:
Isotope
Chlorine -35
Chlorine-37
Neon-20
Neon-22
Oxygen-16
Oxygen-17
Oxygen-18
Protons
Neutrons
8. Complete the following table:
Element
Symbol
Atomic #
Mass #
Protons
Neutrons
Mn-55
Tin
50
69
127
53
Pb-207
82
Sodium
12
98
197
7
Electrons
BOHR MODELS
8
Name
Sodium
Symbol
Lead
Manganese
Sr-88
Atomic #
Si-28
48
Mass #
88
Hg-201
29
112
58
64
36
207
201
209
Protons
Neutrons
Electrons
83
14
28
14
25
48
76
Group/
Family
Period
115
14
4
6
9
Alkali Metals
Alkaline Earth Metals
Physical characteristics:
Chemical
characteristics:
Location on the
periodic chart:
Number of valence
electrons:
Other important
characteristics or
information:
10
Transition Metals
Boron Family
Carbon Family
Nitrogen Family
Oxygen Family
Physical characteristics:
Chemical
characteristics:
Location on the
periodic chart:
Number of valence
electrons:
Other important
characteristics, or
information:
11
Halogens
Noble Gases
Matching:
Match the terms on the left with the proper definitions on the right.
1. Orbital_____
A. The electrons in an atom have the lowest possible energies
2. Nucleus_____
B. The sum of the protons and neutrons in an atom
3. Atomic Number_____
C. The center of an atom
4. Mass Number_____
D. Region of space around the nucleus where electrons are likely to be found
5. Isotope_____
E. The total number of protons in a nucleus
6. Electron_____
F. Particle with a positive charge
7. Neutron____ _
G. Particle with no charge
8. Proton_____
H. Particle with a negative charge
9. Energy levels_____
I. Possible energies of an electron
10. Ground State_____
J. Atoms with the same number of protons but different numbers of
neutrons
Fill in the Blank
Write the name of the scientist whose contribution to the atomic theory is described.
Bohr
Thomson
Democritus
Dalton
Rutherford
11. Scientist who discovered the electron. ___________________
12. Created an atomic model with a dense center called a nucleus. _________________
13. Developed the “plum pudding” model. ______________________
14. Proposed the idea that matter was made of indivisible particles called atoms._____________________
15. Discovered that the atom was mostly empty space. _________________
16. Proposed that electrons move in spherical orbits at fixed distances from the nucleus, much like planets orbit the sun.
________________________
17. Proposed a four-part atomic theory, and concluded that all compounds combine in fixed proportions.
_________________________
Periodic Table Relationships:
In each of the following sets of terms, three of the terms are related. One term does not belong. Read each group of terms, identify the
characteristic common to three of the terms, and then circle the term that does not belong.
18. Period 5, Group 5, Atomic number 41, Halogen
19. Sodium, Alkali metal, Unreactive, Group 1
20. Vertical column, group, period, family
21. Technetium, gas, 43, Metal
22. Sodium, Aluminum, Sulfur, Fluorine
Identifying Unknown Elements
23. This element is in the same family as lead, and it has fewer protons than sodium ___________________
24. This Element has an atomic number that is one greater than platinum ____________________
25. This element has the most protons of any element in Group 15 ____________________
26. This element has more than 50 but less than 75 protons in Group 17 _________________________
27. This element has more valence electrons than oxygen, fewer valence electrons than neon, more protons than sodium, but fewer
protons than argon _________________________
12
Multiple Choice
Identify the letter of the choice that best completes the statement or answers the question.
28. Which particle is the least massive?
a. Proton
c. Nucleus
b. Electron
d. Neutron
29. Which of the following identifies an element?
a. Mass number
c. Number of neutrons
b. Atomic number
d. Valence Number
30. The nucleus…
a. Is the center of the atom
c. Accounts for 99.9% of the mass of the atom
b. Contains proton and neutrons
d. All of the above
31. Which statement about subatomic particles is NOT true?
a. Protons and neutrons have almost the same mass.
b. Protons and electrons have opposite charges.
c. Unlike protons and electrons, neutrons have no charge.
d. Protons and neutrons have the same charge.
32. This Group 2 element has fewer protons than bromine, but no more protons than sulfur.
a. Potassium
c. Magnesium
b. Strontium
d. Calcium
33. Suppose an atom has a mass number of 23. Which statement is true beyond any doubt?
a. The atom has an odd number of neutrons.
b. The atomic number is less than 11.
c. The atom is not an isotope.
d. The number of protons in the nucleus does not equal the number of neutrons
34. Which statement is true about oxygen-17 and oxygen-18 isotopes?
a. They do not have the same number of neutrons.
b. They do not have the same number of electrons.
c. They do not have the same number of protons.
d. They have the same mass number
35. The _____________ family of elements contains all of the elements that are inert.
a. Halogens
c. Alkaline Earth Metals
b. Transition Metals
d. Noble Gases
36. Why are atoms neutral?
a. They have the same number of neutrons as electrons
b. They do not contain charged particles
c. They have the same number of protons as electrons
d. They have different isotopes
37. This contribution to the atomic theory is used to describe the possible locations of electrons around the nucleus. The cloud is
denser in places where the probability of finding an electron is high.
a. Electron cloud model
c. Planetary model
b. Plum pudding model
d. Gold foil model
Use your knowledge of the periodic table to fill in the missing information in the diagram below :
Element
Symbol
Atomic #
Mass #
Protons
Neutrons
Electrons
Ca-40
Zinc
65
146
2
4
47
Bromine
61
26
Draw Bohr Models for the following Elements:
Mg-26
F-20
Ne-20
13
92
Ne-20
14
15