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Name _____________________________
Mrs. Murray
HONORS
Chemistry, period____
Date ______________
UNIT4: Periodic Table
Text Book
 Chapter 6 - The Periodic Table and Periodic Law, pages 174-194
A. ELEMENT PROJECT
Instructions:
This project is worth 1 test grade and
divided into three parts.
ELEMENT:
DUE DATE:
1. Research 20 facts about your element. Information to include:
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The element name and symbol
The origin of the name of the element
The date the element was discovered
The name of the discoverer of the element
The atomic mass and atomic number of the element
Chemical/physical properties of the element
Interesting uses of the element/ compounds of the element
A picture / pictures of the element
Each fact must be submitted as a list (TYPED) on a sheet of paper.
EACH fact gets neatly and creatively displayed on a circle ( 4 circle pages needed)
Each circle can have a maximum of 5 words!!!
2. Write an info-mercial about the element. The ad may be a want ad, personal ad, sales ad
etc...Be creative! In the ad, display some of the information about your element. The ad
must be computer generated on a poster, pamphlet, moviemaker, animoto etc.
3. Create a new element square. The square must be done on paper provided. The
square must contain:
ON FRONT:
 Chemical Symbol
 Atomic Number
 Interesting Picture of something you learned about the element
ON THE BACK:
 Explanation of the picture on front
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HONORS
B: Activity of the Elements
Referring to a periodic table, circle the member of each pair of elements which is most
chemically active.
1 . Li and Na
16. CI2 and Br2
2. CI2 and F2
17. Xe and I2
3. N2 and Ne
18. Fe and Ra
4. Rb and Ca
19. Sr and Mn
5. Ti and Ca
20. K and Na
6. K and Mg
21. Au and Mg
7. O2 and S
22. S and Rn
8. I2 and Br2
23. Li and Be
9. Na and Zn
24. Se and Br2
10. P and S
25. I2 and F2
11. N2 and O2
26. Rb and Sr
12. CI2 and Ar
27. Ba and Ra
13. Ba and Fr
28. Na and Mg
14. Rb and Cu
29. Te and I2
15. Be and Cr
30. Ca and Rn
31. What is the strongest metal on the periodic table? Strongest non-metal?
32. A characteristic of most nonmetallic solids is that they are
1. brittle
3. malleable
2. ductile
4. conductors of electricity
33. Which of the following period 3 elements has the least metallic character?
1. Na
3. Al
2. Mg
4. Si
34. The chemical properties of the elements are periodic functions of their atomic
1. masses
3. numbers
2. weights
4. radii
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HONORS
C: Periodic Table
Place the letter of each of the above elements next to its description below.
1 . An alkali metal ______________
2. An alkaline earth metal ______________
3. An inactive gas _______________
4. An active nonmetal ______________
5. A metalloid (semimetal) _____________
6. An transition element _________________
7. Its most common oxidation state is -2 _________________
8. A metal with more than one oxidation state ________________
9. Metal with an oxidation number of +3 _________________
10. Has oxidation numbers of + 1 and -1 _________________
11. Which element is so active chemically that it occurs naturally only in compounds?
1. potassium
3. copper
2. silver
4. sulfur
12. Which element is not a semimetal?
1. arsenic
2. boron
3. silicon
4. sulfur
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D: Ions:
1. What is an ion?
2. How does an atom become a positive ion?
3. How does an atom become a negative ion?
4. Complete the table.
Element
Name
Ion
Formed
and Name
Loss/ Gain
how many
electrons
Ion Bigger
or Smaller
than Atom
Protons,
Neutrons
and
Electrons
Lewis Dot
Structure of
the Atom
Lewis Dot
Structure
of the ION
Aluminum
Bromine
Sulfur
Sodium
Neon
Nitrogen
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HONORS
E: Element Characteristics
Use a periodic table to help you answer the following questions.
1. a. How many protons does an atom of bromine (Br) have? ____________
b. In which group is bromine found? ______________
c. What is the name of its chemical family? _________________
d. How many valence electrons does it have? _____________________
e. Draw the Lewis Dot structure for the atom_____________________
f. Is it a metal, a nonmetal, or a semimetal? _____________________
g. What ion is it most likely to form in compounds? __________________
h. Draw the Lewis Dot structure for the ion._____________________
2. a. How many protons does an atom of magnesium (Mg) have? _______________________
b. In which group is magnesium found? ___________________
c. What is the name of its chemical family? _______________________
d. How many valence electrons does it have? __________________
e. Draw the Lewis Dot structure for the atom_____________________
f. Is it a metal, a nonmetal, or a semimetal? __________________
g. What ion is it most likely to form in compounds? _______________________
h. Draw the Lewis Dot structure for the ion._____________________
3. a. How many protons does an atom of potassium (K) have? ___________________
b. In which group is potassium found? ________________
c. What is the name of its chemical family? _______________________
d. How many valence electrons does it have? __________________
e. Draw the Lewis Dot structure for the atom_____________________
f. Is it a metal, a nonmetal, or a semimetal? __________________
g. What ion is it most likely to form in compounds? _______________________
h. Draw the Lewis Dot structure for the ion._____________________
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HONORS
F: Periodic Table Trends
1. Where are the most active metals located? __________________________
2. Where are the most active nonmetals located? ___________________________
3. As you go from left to right across a period, the atomic size ( decreases / increases).
Why? ___________________________________________________________
4. As you travel down a group, the atomic size (decreases /increases).
_________________________________________________________________
5. A negative ion is ( larger / smaller) than its parent atom.
6. A positive ion is ( larger / smaller) than its parent atom.
7. As you go from left to right across a period, the first ionization energy generally
( decreases / increases). ________________________________________
8. As you go down a group, the first ionization energy generally ( decreases / increases)
____________________________________________________________
9. Where is the highest electronegativity found? _____________________________
10. Where is the lowest electronegativity found? ______________________________
11. Elements of Group 1 are called ____________________________
12. Elements of Group 2 are called ____________________________
13. Elements of Group 3-11 are called __________________________________
14. As you go from left to right across the periodic table, the elements go from
( metals / nonmetals) to ( metals / nonmetals ).
15. Group 17 elements are called _________________________________
16. The most active element in Group 17 is _____________________________
17. Group 18 elements are called _____________________________________
18. Can lose electrons from valence and sub-valence electrons _______________________
19. Elements within a group have a similar number of _______________________
20. Elements across a period have the same number of ______________________
21. A colored ion generally indicates ____________________________________
22. As you go down a group, the elements generally become (more / less) metallic.
23. The majority of elements in the periodic table are (metals / nonmetals).
24. Elements in the periodic table are arranged according to their ___________________
25. An element with both metallic and nonmetallic properties is called a _________________
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HONORS
G: More Periodic Trends
Complete the following tables:
Periodic Trend Going Across the Periodic Table
Element
Atomic
Radius
(pm)
Electronegativity
First Ionization
Energy
(kJ/mole)
Electron Affinity*
Calcium
Selenium
Trend
Explanation
of Trend
Periodic Trend Going Down the Periodic Table
Element
Atomic
Radius
(pm)
Electronegativity
First Ionization
Energy
(kJ/mole)
Electron Affinity*
Fluorine
Iodine
Trend
Explanation
of Trend
* online information…not on Table S!
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HONORS
H: Multiple Choice
___1. The elements from which two groups of the periodic table are most similar in their chemical
properties?
(1) 1 and 2
(2) 1 and 17
(3) 2 and 17
(4) 17 and 18
___2. Elements in the modern periodic table are arranged according to their
(1) atomic number
(2) atomic mass
(3) relative activity
(4) relative size
___3. As elements of Group 15 of the periodic table are considered in order from top to bottom,
the metallic character of the atoms of each successive element generally
(1) decreases
(2) increases
(3) remains the same
___4. As the elements in Group 15 are considered in order of increasing atomic number, which
sequence in properties occurs?
(1) nonmetal  metalloid  metal
(2) metalloid  metal  nonmetal
(3) metal  metalloid  nonmetal
(4) metal  nonmetal  metalloid
___5. Which statement is true about the properties of the elements in anyone period of the periodic
table?
(1) They are determined by the number of neutrons.
(2) They are determined by the number of electrons in the first principal energy level.
(3) They change in a generally systematic manner.
(4) They change in a random, unpredictable manner.
___6. Which statement describes the elements in Period 3?
(1) Each successive element has a greater atomic radius.
(2) Each successive element has a lower electro negativity.
(3) All elements have similar chemical properties.
(4) All elements have valence electrons in the same principal energy level.
___7. Which noble gas has the highest first ionization energy?
(1) radon
(3)neon
(2) krypton
(4) helium
___8. Which of these metals loses electrons most readily?
(1) calcium
(2) magnesium
(3) potassium
(4) sodium
___9. In which area of the periodic table are the elements with the strongest nonmetallic properties located?
(1) lower left
(2) upper left
(3) lower right
(4) upper right
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HONORS
I: SAT II
Questions 1-4 refer to the following atoms in the ground state.
(A) Ar
(B) O
(C) S
(D) Ti
(E) U
1. Has the electron configuration 1s2 2s22p63s23p4 _______________
2. Has the same number of electrons as Ca2+ _______________
3. Has electrons in f orbitals _________________
4. Is the LEAST chemically reactive ________________
____5. For elements in the left-most column of the periodic table, properties that have
increasing values as the atomic number increases include which of the following?
I. Ionization energy (potential)
II. Atomic radius
III. Atomic mass
(A) I only
(B) III only
(C) I and II only
(D) II and III only
(E) I, II, and III
____6. Compared to the atomic radius of a sodium atom, the atomic radius of a magnesium
atom is smaller. The smaller radius is primarily a result of the magnesium atom having
A. a greater charge on the nucleus.
B. a smaller charge on the nucleus.
C. more principal energy levels.
D. fewer principal energy levels.
____7. As the elements in Period 3 are considered from left to right, they tend to
A. lose electrons more readily and increase in metallic character.
B. lose electrons more readily and increase in nonmetallic character.
C. gain electrons more readily and increase in metallic character.
D. gain electrons more readily and increase in nonmetallic character.
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HONORS
____8. Which diagram correctly shows the relationship between electronegativity and atomic
number for the elements of Period 3?
___9. A sulfur ion is represented as S2-. How is the sulfide ion different from a sulfur atom?
A. The sulfide ion has gained two electrons.
B. The sulfide ion has gained two protons.
C. The sulfide ion has lost two electrons.
D. The sulfide ion has lost two protons.
___10. When an atom of aluminum forms an ion, the resulting ionic symbol is correctly written
as
A. Al3+
B. Al2+
C. Al2D. Al3___11. Which element has properties most like those of oxygen?
A. nitrogen
B. fluorine
C. sulfur
D. chlorine
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HONORS
J. DBQ
DRY ICE
Dry ice is frozen carbon dioxide. It has a
unique feature. Under normal atmospheric
conditions, it sublimes; changes from a solid to a
gas.
If you ever have to handle dry ice, you
want to be sure to wear heavy gloves, because a
block of dry ice has a surface temperature of 78.5 ° C. The super-cold surface temperature can easily damage your skin if you touch it directly.
While dry ice looks like it would be cold, it's extremely dangerous to the touch and can
cause severe burns. It's actually a lot like if you were to touch the handle of a hot pot or pan
without an oven mitt. If you did this for less than a second -- so that you simply felt the heat and
quickly pulled your hand away -- then at most your skin would be a little red. However, if you
were to grab a hold of the handle tightly for a couple of seconds or more, chances are you
would get a pretty nasty burn. The heat kills the skin cells. It's the same with dry ice. Dry ice
actually freezes your skin cells. The resulting injury is very similar to a burn and should be
treated with the same medical attention. For the same reason you never want to taste or
swallow dry ice. This would be like drinking something that was scalding hot and you would risk
damaging your mouth, throat and part of your esophagus.
1. What is sublimation?
2. What other chemical sublimes?
3. Is sublimation a chemical or physical change? Explain.
4. What is the surface temperature of dry ice? Convert this temperature to Kelvin.
5. What is the oxidation state of oxygen in carbon dioxide?
6. What happens when you touch dry ice?
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HONORS
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HONORS
UNIT 4 Periodic Table:
1. Periodic Table was originally developed by Dmitri Mendeleev.
2. It is arranged according to increased atomic number.
3. The Periodic Law states that the chemical properties of elements are periodic functions of
their atomic number.
4. Elements are classified as metals, non-metals and metalloids.
 Metals 
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make up more than 2/3 of the periodic table
found on the left side of the staircase on the periodic table
lose electrons to form positive ions which are smaller than the metal
atom
solids at room temperature except Mercury (Hg) which is a liquid
most active metals found on lower left of table (Francium)
good conductors of heat and electricity
malleable, ductile and have luster

Non-Metals  found on the right of the staircase on the periodic table
 gain electrons to form negative ions which are larger than the atom
 Bromine is the only liquid non-metal
 most active non-metal found upper right of table (Fluorine)
 brittle and dull
 poor conductors of electricity

Metalloids  found on the staircase on the periodic table
 have properties of both metals and non-metals
5. Vertical columns on the Periodic Table are called groups or families. Atoms in the same
group have the same number of valence electrons, therefore reacting very similarly.
Elements of the same group have the most in common.
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Group 1 = Alkali Metals. Very reactive metals-found in nature in compound form only
Group 2 = Alkaline Earth Metals. Reactive metals mostly found in nature in
compound form
Group 17 = Halogens (all diatomics) - this group contains all three phases of
matter at room temperature. F2, Cl2 - gases, Br2 - liquid, I2 - solid). These are
very reactive elements that are found in nature in compound form only.
Group 18 = Noble Gases (monatomics) have 8 valence electrons in the outer PEL,
except He which only has 2.
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HONORS
Group 3-11 – Transition Metals - found in the middle of the periodic table.
 can have electrons from two outermost shell involved in bonding
 they have multiple oxidation states
 form colored ions in compounds or in solution
6. Horizontal rows on the Periodic Table are called periods or rows. Atoms in the same row
have the same number of occupied principal energy levels.
7. General trends of the periodic table:
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Metallic character increases
Increasing PELs
Atomic radius increases
Ionization energy decreases
Electronegativity decreases
Electron Affinity decreases
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Metallic character decreases
Increased Effective nuclear charge
Atomic radius decreases
Ionization energy increases
Electronegativity increases
Electron Affinity increases
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