Download Periodic Table Packet

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Name
Teacher
Regents Chemistry
Periodic Table
What will students know and be able to do by the end of this instructional unit?
1. Define and describe:
a. Period
k. Alkali Metals
b. Group
1. Transition Metals
c. Family
m. Conductivity
d. lonization Energy
n. Ductile
e. Atomic Radii
o. Lustrous
f. Ionic Radii
p. Malleable
g. Electronegativity
q. Metalloids
h. Reactivity
'
r. Norrmetals
i. Metals
.
s. Halogens
j. Alkaline Earth Metals
t. Noble Gases
2. Be able to distinguish between metals and nonmetals based on their properties and
location on the periodic table.
3. Label the periodic table with solid, liquid and gas.
4. Locate where the most reactive and least reactive metals and nonmetals exist on the
periodic table.
5. Recognize the symbol of any element and be able to locate the element on the periodic
table.
6. Explain the placement of an unknown element on the periodic table based on its
properties.
7. Write the electron configuration of any atom in the ground state or excited state.
8. Read and interpret electron configurations.
9. Determine the number of occupied energy levels based on the atoms electron
configuration.
10. Determine the number of valence electrons in an atom.
11. Classify elements as metals, nonmetals, metalloids, noble gases, by their properties.
12. Compare the properties of elements within a group or period for Groups 1,2,13-18
Key Subject Competencies
• Understand the arrangement of the periodic table
• Identify the different groups in the periodic table
• Understand the arrangement of the periodic table
• Identify the different groups in the periodic table
• Identify the properties of metals, nonmetals, and semimetals
• Classify and organize elements according to atomic #, groups, and periods
• Identify the properties of the different groups in the periodic table
• Understand the arrangement of the periodic table
• Identify the different groups in the periodic table
• Identify the properties of metals, nonmetals, and seniimetals
• Identify and describe allotropes
• Define ionization energy
• Use Table S to find the first ionization energies of the elements
• Explain the trend in ionization energy across the periodic table and within a group
• Define electronegativity
Periodic Table
Use Table S to find the electro negativity of the elements
Explain the trend in electro negativity across the periodic table and within a group
Determine the natural states of the elements
Determine the state of the elements at different temperatures
Use Table S to find the melting and boiling points of the elements
Define electronegativity
Use Table S to find the atomic radius of the elements
Describe the change in atomic size as it becomes an ion
Explain the trend in atomic radius and ionic radius across the periodic table and within a
group.
Vocabulary
Alkali Metals
Conductivity
Halogen
lonization Energy
Noble Gas
Periodic Law
Alkaline Earth
Ductile
Metals
Lustrous
Transition Metals
Reactivity
Metalloids
Electronegativity
Nonrnetal
Malleable
Atomic Radius
Transition Metal
Ionic Radius
Family Metal
Period
Group Metalloid
Name
Period
Date
Activity: To make a colorful, educational periodic table.
Materials: Colored pencils and a fluorescent highlighter, a periodic table,
Directions: Read through all the steps before you start, then begin your
work. If you borrow the colored pencils, sharpen them before you return
them.
1. Color a box around each of the alkali metals, atomic numbers 3, 11,
19, 37,55, and 87 red, because they are wildly reactive. Color lightest
at the top through darkest at the bottom to indicate the increasing
reactivity of the group members.
2. Color a box around each of the alkaline earth metals, atomic, numbers
4, 12, 20, 38, 56, and 88 orange, because they are mildly reactive.
Shade in the color from lightest at the top to darkest at the bottom to
indicate the increasing reactivity of the group members.
3. Color a box around each of the transition elements in Groups 3-11
pale yellow, because they are only slightly reactive, compared to the
other groups of metals.
4. Color a box around the semi-metals, atomic numbers 5, 14, 32, 33, 51,
and 52 green; they are somewhat like the yellow transition metals,
and somewhat like the blue halogens.
5. Color a box around the halogens, numbers 9, 17, 35, and 53 blue,
because they are very reactive and at the other end of the spectrum of
chemical behavior of the alkali metals Color fluorine the darkest
because it has the greatest reactivity and lighten to astatine because it
is least chemically reactive in the group
6. Color a box around each of the noble gases, numbers 2, 10, 18, 36, 54,
and 86 lightly in black, because they are so chemically non-reactive
7. Use a fluorescent highlighter on elements 84-118 to indicate their
strictly radioactive state. Also highlight atomic number 43 to indicate
its radioactivity. Remember that all the elements have at least one
radioactive isotope, but these elements are strictly radioactive, with no
stable isotopes.
Now you have a colorful study aid to use to improve your understanding of
chemistry!
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Where Does This Element Live?????
Directions: Fill in the following blanks regarding the listed elements.
1. Carbon
Symbol
7. Neon
Symbol
Group
Group
Period
Period
2. Oxygen
Symbol
8. Argon
Symbol
Group
Group
Period
Period
3. Phosphorus
Symbol
9. Lithium
Symbol
Group
Group
Period
Period
4. Sodium
Symbol
10. Nitrogen
Symbol
Group
Group
Period
Period
5. Magnesium
Symbol
Group
Period
6. Calcium
Symbol
Group
Period
Properties of...
NONMETALS
METALS
METALLOIDS
Name:
.
1)
An atom of an element contains 20 protons, 20 neutrons, and 20 electrons. This
element is
a. an alkaline earth metal
b. a halogen
c. an alkali metal
d. a noble gas
2)
The chemical properties of elements are periodic functions of their
a. oxidation states
b. mass numbers
c. ionic charges
d. atomic numbers
3)
Who was credited with creating the first Periodic Table that organized the
elements according to atomic mass?
a. Dmitn Mendeleev •
b. John Dalton
c. Flenry Moseley
d. Ernest Rutherford
4)
On the Periodic Table, an element classified as a semimetal (metalloid) can be
found in
a. Period 3, Group 16
b. Period 2, Group 14
c. Period 4, Group 15
d. Period 6, Group 15
5)
Which element is in Group 2 and Period 7 of the Periodic Table?
a. Radium
b. Radon
c. Manganese
d. Magnesium
6)
In
a.
b.
c.
d.
the modem Periodic Table, the elements are arranged according to
mass number
atomic number
atomic mass
oxidation number
Periodic Table Homework
1.
List the symbol of each of the following elements:
a.
Fluorine:
b.
Chlorine:
c.
Magnesium:_
d.
Lithium:_
e.
Neon:
2.
Draw the Bohr diagram for each of the above 5 elements.
3.
Hdw" can you determine how many electrons a neutral element has?
4.
Write but electron configurations for these 5 elements.
a.
F luorine:
b.
Chlorine:
c.
Magnesium:
d.
Lithium: __
e.
Neon:
10
5.
List the different element groups (families) wtiiclvare represented by ouiv5
"
."
f*
4~* j
elements. Which elements are in the.same group?
• *:
a.
Fluorine
b.
Chlorine'
c.
Magnesium
d.
. Lithium
e.
Neon
6.
How can you tell, looking at the periodic table, if elements a*re m*the*same group
(family)?
.
\
~ ' ,
7.
Compare information concerning any of the 5 elements which are in the same
group. What is one similarity of elements in the same group?
„ ' , t.
11
lonization Energy
Definition:
A. Find the ionization energy for the following elements:
1. Li
2. B
3. O
4. Ne.
B. What is the trend when going across a period?
c. Find the ionization energy for the following elements
1. C
2. Si
3. Ge
4. Pb
D. What is the trend when going down a group?
12
Electronegativity
Definition:
A. Find the electronegativities for the following elements:
1. Li
2. B _
3. 0
4. Ne
B, What is the trend when going across a period?
C. Find the electronegativities for these elements:
1. C
2. Si
3. Ge_
4. Pb
D. What is the trend when going down a group?
Atomic Radii Worksheet
Definition:
A. Find tile Atomic Radii for the following elements;
•is
I . .Li
•
.-• 2.' B
.3. O
4. Ne
B. Whatsis "the. trend when going across a period?
C. Find the Atomic Radii for these elements:
.' T. G
" "'>"2. Si
.3. Ge
4. Pb
• -..«. .t-
D. What is^thte'trend when going do\vnjiaiigro'up?#*,«s*-
"• '•' ^^ :*'-ijfr^^P^^^to. Jr '-i"-J' T-"-
Element Group Properties
1. Alkali metals - Group 1
a. extremely reactive (not found free in nature) - form stable ionic compounds
b. react with water to form a base
c. • react with air to form oxides
d. react with acids to form salts
2. Alkaline earth metals - Group 2
a. reactive (not found free in nature) - form stable ionic compounds
b. react with water to form a base
c. react with air to form oxides
d. reactwith acids to form salts
3. Nitrogen family - Group 15
a. Members range from typical nonmetals (nitrogen and phosphorus) through
metalloids (arsenic and antimony) to metals (bismuth)
b. Nitrogen
i. Forms stable diatomic molecules with a triple bond
ii. Component of protein
iii. Forms some unstable compounds that are used as explosives
c. Phosphorus
i. Component of nucleic acids (DNA, RNA)
ii. More reactive than nitrogen at room temperature
4. Oxygen family - Group 16
a. Members range from typical nonmetals (oxygen and sulfur) through
metalloids (selenium and tellurium) to metals (polonium)
b. Solids except oxygen
5. Halogens
a.
b.
c.
d.
e.
f.
(salt formers) - Group 17
very reactive nonmetals - high electronegativity
not found free in nature
form diatomic molecules when free
react with metals to form salts
Tendency to form positive oxidation state increases with atomic number
Found in all three phases due to differences in Van der Waals forces
6. Noble gases
a. have complete outer shells
b. Almost inert (not reactive)
i. Krypton, xenon, and radon form compounds with oxygen and
fluorine
7. Transition elements
15
a. Positive oxidation state
b. Lose electrons from two outermost energy levels
c. Ions form colored solutions
Comparing Metals and Nonmetals
8. Metals
a. Chemical properties - tend to lose electrons easily " have low ionization
energy (energy needed to remove electrons)
i. have low electron affinity (attraction for electrons)
ii. form positive ions when combining with other atoms
b. Physical properties
i. good conductors of heat and electricity
ii. lustrous - reflect light, shine when they are polished
iii. flexible
1. malleable - can be rolled or hammered into sheets
2. ductile - can be drawn into wires " are solids at room
. temperature except for mercury
9. Nonmetals
a. Chemical properties - tend to gain electrons
i. have high electron affinities
ii. produce covalent bonds by sharing electrons with other nonmetals
b. Physical properties
i. exist as gases, molecular solids, or network solids at room
temperature except bromine
ii. solids are brittle - not ductile or malleable
iii. solids are dull - do not reflect light even when polished
iv. poor conductors of heat and electricity
10. Metalloids (semi-metals)
a. elements at the border between metals and nonmetals that have some
properties of both and have properties intermediate to metals and
nonmetals (special case of nonmetals)
16
The Periodic Table
Practice Questions
1 . Which trends are obsen'ed when the elements in
Period 3 on the Periodic Table are considered in
order of increasing atomic number?
A) The atomic radius decreases, and the first
ionization energy generally increases.
B) The atomic radius decreases, and the first
ionization energy generally decreases.
C) The atomic radius increases, and the first
ionization energy generally increases.
D) The atomic radius increases, and the first
ionization energy generally decreases,
2. Which element in Period 3 has the largest
atomic radius?
C) Na
A) Cl
D) P
B) Al
3. Which of the following particles has the
smallest radius?
A) Na°
B) K°
C) Na*
D) K*
4. Based on Reference Table S, atoms of which of
these elements have the strongest attraction for
the electrons in a chemical bond?
A) Al _
C) P
B) Si
D) S
7. Which trends appear as the elements in Period 3
are considered from left to right?
A) Metallic character decreases, and
electronegativity decreases.
B) Metallic character decreases, and
electronegativity increases.
C) Metallic character increases, and
electronegativity decreases.
D) Metallic character increases, and
. electronegativity increases.
8. Compared to atoms of metals, atoms of
nonmetals generally
A) have higher electro negativities
B) have lower first ionization energies
C) conduct electricity more readily
D) lose electrons more readily
9. In which reaction is the first ionization energy
greatest?
A) Na + energy -» Na+ + e~
B) K + energy ^ K"1" 4- e~
C) Mg + energy -». Mg+ + e~
D) Al + energy -» Al* + e~
10. Which type of energy is represented in the
equation
A)
B)
C)
D)
5. Which of the following elements has the highest
electronegativity?
A) H
C) Al
B) K
D) Ca
6. Which of the following atoms has the greatest
tendency to attract electrons?
A) barium
C) boron
B) beryllium
D) bromine
Na + energy _> Na+ + e~?
neutralization energy
ionization energy
nuclear energy
formation energy
1 1 . Which Period 4 element has the most metallic
properties?
A) As
C) Ge
B) Br
D) Sc
12. In Period 3, from left to right in order, each
successive element will
A) decrease in electronegativity
B) decrease in atomic mass
C) increase in number of protons
D) increase in metallic character
17
The Periodic Table
13. Most metals have the properties of
A) brittleness and high ionization energy
B) brittleness and low ionization energy
C) ductility and high ionization energy
v— •
D) ductility and low ionization energy
14. Compared to an atom of potassium, an atom of
calcium has a
A) larger radius and lower reactivity
B) larger radius and higher reactivity
C) smaller radius and lower reactivity
D) smaller radius and higher reactivity
15. The most active metals are in Group
A) 1
C) 13
B) 15
D) 17
16. Which element is malleable and can conduct
electricity in the solid phase?
A) iodine
C) sulfur
B) phosphorus
D) tin
(
17. Which substance can not be decomposed by
ordinary chemical means?
A) methane
C) ethanol
B) mercury
D) ammonia
18. At STP. an element that is a brittle solid and a
poor conductor of heat and electricity could
have an atomic number of
A) 12
C) 16
B) 13
D) 17
19. Which is a property of most nonmetallic solids?
A) high thermal conductivity
B) high electrical conductivity
C) brittleness
D) malleability
20. Which element is a noble gas?
A) krypton
C) antimony
B) chlorine
D) manganese
21. The element in Group 14, Period 3 on the
Periodic Table is classified as a
A) metal
•
C) metalloid
B) noble gas
D) nonmetal
22. Which list of elements contains two metalloids?
A) Si, Ge, Po, Pb
C) Si, P, S, Cl
B) As, Bi, Br; Kr
D) Po, Sb, 1, Xe
23. Pure silicon is chemically classified as a
metalloid because silicon
A) is malleable and ductile
B) is an excellent conductor of heat and
electricity
C) exhibits metallic and nonmetallic properties
D) none of the above
24. Which element has chemical properties that are
most similar to those of calcium?
A) Co
C) N
B) K
D) Sr
25. Which list consists of elements that have the
most similar chemical properties?
A) Mg; Al, and Si
C) K, Al, and Ni
B) Mg, Ca, and Ba
D) K, Ca, and Ga
18
Name
Ms, Tintella
Date
Regents Chemistry
Allotropes
Do Now:
Alexa
Brian
X12368713 folosearcfLnom
Fraternal Twins
Past Learning
Using the picture above and your knowledge of Biology, make observations and identify the similarities and
differences between Alexa and Briar.
Alexa
"^^
Brian
Applications to Chemistry
Using the mineral samples provided and your knowledge of Earth Science, make observations.and identify
the similarities and differences between Graphite and'Coal.- . . .
Slide 1:
What do all of these have in common?
Slide 2:
What is the atomic number and atomic mass?
Draw the Bohr Model.
Draw the Lewis Dot Diagram
Slide 3:
Can you identify some of these substances?
2.)
3.)
4.)
Slide 4:
What was the major similarity between the fraternal twins?_
What is the major similarity between graphite and charcoal?
20
Slides 5-7:
•
What is an allotrope?
Examples:
1.
All of these molecules contain
How do these molecule differ?
Slide 8:
You will watch an 8 minute video. Answer the questions below as you are watching the video.
• Why is graphite arranged in layers?
•
Describe the bonding between the layers? What is the result of this type of bonding?
•
Why is graphite used in pencils?
•
How are diamonds made?
•
What is the molecular arrangement of a diamond?
•
What is buckministerfullerene used for?
Slide 9:
Molecular Models of Carbon
Slide 10: Other Allotropes
1.
2.
These molecules contain
21
Name
.T
Explain how fraternal twins are like Allotropes?
Slide 11:
Slide 13;
Which statement explains why ozone gas, O3,
and oxygen gas, O2, have different properties?
1) They are formed from different elements.
2) They have different molecular structures.
3) They have different oxidation numbers.
4) They have different electraiiegaHvities.
At STP. the clement oxygen can exist as either O
-, or O3 gas molecules. These two forms of the
element have
1) the same chemical and physical properties
2) the same chemical properties and different
physical properties
3) different chemical properties and the same
physical properties
4) different chemical and physical properties
Slide 14:
At STP, solid carbon can exist as graphite or as
diamond. Those two forms of carbon have
1) the same properties mid the same crystal
structures
2) the same properties and different crystal
structures
3) different properties and the same crystal
structures
4) different properties and different crystal
structures
Slide 12:
Which statement correctly describes two forms
of oxygen, O2 and O3V
1) They huve identical molecular structures <iml
identical properties.
2) They have identical molecular structures and
different properties.
3) They have different molecular structures and
identical properties.
4j They have different molecular structures ;md
dif'terem properties.
Slide 15:
At 298 K, oxygen (O?) and ozone (O3) have
different properties because their
I.) atoms have different atomic numbers
2} atoms have different atomic masses
3) molecules have different molecular structures
4) molecules have different average kinetic
enemies
22
Name
: Form W S 3 . 3 . 1 A
Date
PERIODIC TABLE
Period
iri: the Pcn®<gLie Tafefe?
What are the
Below is a portion of the periodic table. In the answer spaces provided in the table, fill in the [1] atomic number,
[2] atomic radius, [3] number of shells, and [4] number of outer shell electrons as indicated in the key below. Then,
answer the questions that follow.
KEY
Symbol
[1] Atomic Number
[2] Atomic Radius
[3] Number of Shells
[4] Number of Outer Electrons
rn
H
He
[11
m
[21
[3]
[31
[41
[4]
Li
m
Be
8
C
N
O
F
[21
[2]
rn
PI
T3]
[31
[31
[3]
m
[31
[31
[31
[4]
Kl
[4]
f4]
m
[41
[41
[41
rn
rn
Na
rn
m.
m
[21
m
[21
[21
A)
Mg
[11
[11
Si
m
[21
[2]
[21
[21
[21.
[31
rsi
[3]
[3]
[31
[4],
[4]
[4]
[4]
[41
m
Ca
K
[1]
m
[2]
[31
[31
m
[4]
m
HI
/
23
[11
p
.
,
[11
m
Pi
[41
s
[1]
Cl
[11
[11
[21
[21
[31.
[31
[41
[41
Ne
Ar
How is the Periodic Table Arranged?
: Form WS3 . 3 . 1A
Page 2
PERIODIC TABLE
Answer the questions below by referring to the data on the table you filled in on the first page.
1. As you go from left to right across a row of the Periodic Table:
a. What happens to the atomic number and the number of protons?
b. As a result, what happens to the pull on the electrons?
c. Therefore what happens to the atomic radius?
d. Finally, what does this mean about the likelihood of losing electrons? Do the elements become more or less
metallic?
2. As you go from top to bottom down a column of the Periodic Table:
a. What happens to the number of shells?
__
_____
b. As a result, what happens to the atomic radius?
c. Therefore, what happens to the pull on the electrons?
d. Finally, what does this mean about the likelihood of losing electrons? Do the elements become more or less
metallic?
3. Based on the analysis above, where do metals tend to be located on the Periodic Table1?
4. Based on the analysis above, where do nonmetals tend to be located on the Periodic Table1?
5. What do the elements at the extreme right of the Periodic Table have in common? What affect does this have
on the chemical properties?
.
6. Where on the Periodic Table, approximately, is the border between the metals and nonmetals (the metalloids)?
©Evan P. Silberstein, 2002
24
Name
: Form WS3.3.2B
Period
PERIODIC TABLE
©ri:
Date
ars
Below is a list of the 30 elements found on Mars. Place them in their proper place in the Martian Periodic Table using the information below. Martian elements
follow the same natural laws as the elements on Earth. (Note: The symbols and the elements described below are fictitious.)
ELEMENT LIST
P
A
B
Q
R
C
S
D
T
E
F
U
V
G
H
W
I
X
J
tc
L
M
N
O
Y
Z
6. Element W has 14 protons.
•H
7. B has 7 electrons.
1
+2
+3
+4
-3
-2
-1
8. Q has an atomic weight of 5 and a +1 oxidation state.
2
9. Y has only 1 electron in its outermost shell, but has 4 shells.
3
10. The N family is made up of the elements N, J, P, and X in
order of increasing weight.
4
11. J is'the heaviest of all atoms and is radioactive.
5
12. M is in period 5 and has an oxidation state of +2.
Use the descriptions below to put the elements in the proper
place on the Martian Periodic Table.
1. The most metallic element is R.
13. <*• is in period 2 and group 2
14. U is like our element carbon and is in the same family as W,
Z., and J.
2. The most nonmetallic element is O.
15. Their solvent, like our most important liquid has the formula
E2F.
3. The inert gases are L, ¥, G, and V. Us the lightest, G is the
heaviest and ? is in period 2.
16. The oxidation states of the following elements are: a =-1;
4. Their lightest element of all Is E,
5. All of the following elements have three shells and the
number of outermost electrons for each is as follows: K = 1;
H = 2;J =3; W = 4; I-5; D-6; and C-7
Evan P. Silberstein, 2002
17. Now every space should be filled. Can you give each element
its proper atomic number?
f: Form WS3 . 2 . 2A
Name
Period
Date
PERIODIC TABLE
Each element has its own box on the Periodic Table with a lot of
information in it. There is a key to tell you what information in each box
means. Although Periodic Tables differ, most have the same basic
information. Starting from the top of the box, the information on the key to
the right is as follows: [1] atomic mass - weighted average of the mass of the
common isotopes of the element; [2] common oxidation states - tells number
of electrons lost, gained or shared during bonding; [3] symbol - one, two, or
three letters related to the name with the first letter
NumbDr Prefix
capitalized and other letters lower case. The three letter
symbols are systematic names that represent the atomic 0
nil
1
un
numbers of unnamed elements (currently, elements beyond
2
bi
109); [4] atomic number - number of protons; and 3
tri
[5] electron configuration - arrangement of electrons in 4
quad
energy levels.
Atomic
12.0111
Symbol.
Atomic Number
Electron Configuration
6
c
2-4
Symbol
Number
Prefix
Symbol
n
u
b
t
5
pent
hex
sept
oct
enn
P
h
s
q
6
7
8
9
0
e
Answer the questions below by referring to the Periodic Table of the Elements and to the explanation of the
key above.
("
1. How many protons do each of the following elements have?
a. calcium
___^__
b. sodium
c. iodine
e. nitrogen
d. sulfur
f. mercury
J
g. ununoctium
h. silver
2. What is the mass of the most common isotope of each of the following elements?
a. phosphorus_
c. barium
e. lead
g. chlorine
b. potassium
d. oxygen
f. uranium
h. sold
3. How many occupied principal energy levels do elements in period 4 have?
4. How many valence electrons do the elements in group 17 have?
5. What are the oxidation states for:
a. elements in group 1 ?
b. elements in group 2?
6. Which groups have elements with more than one positive oxidation state?
7. Which groups have elements with both positive and negative oxidation states?
EvanP.SiIberstein,2002
26
: Form WS3.2.1A
Name
PERIODIC TABLE
Date
is
Period
Tafefe
Below is a portion of the periodic table. In the answer spaces provided in the table, fill in the [1] atomic number,
[2] electron configuration, [3] number of shells, and [4] number of outer shell electrons as indicated in the key below.
Then, answer the questions that follow.
KEY
Symbol
[1] Atomic Number
[2] Electron Configuration
[3] Number of Shells
[4] Number of Outer Electrons
Jyloseley
m
(
H
m
[21
T21
[31
m
[41
[41
Be
Li
B
C
N
O
F
Ne
[1]
[1]
[11
[11
[11
[11
m
[21
[2.1
[21
[21
[21
[21
[21
[21
[31
[3]
PI
[31
[31
[31
[31
[31
'[41
T41,
[4]
[4]
[41
[41
m
T4J.
Na
[H
m
[21
PI
[31
[41
m
Si
Al
P
S
[11
Cl
Ar
[1]
[11
ri]
[21
[21
[21
[21
[21
PI
[31
PI
m
[31
[31
[31
[31
[4]
J4]
[41
[41
[41
[41,
K
Mg
Ca
[11
[11
m
m
[31
[31
HI
[41
27
[11
He
[11
..
f4]
: Form W S 3 . 2 . 1 A
How is the Periodic Table Arranged?
PERIODIC TABLE
Page 2
Answer the questions below by referring to the data on the table you filled in on the first page.
1. In what order are the elements of the Periodic Table arranged?
2. What do all the elements in a vertical column of the Periodic Table have in common?
3. What do all the elements in a horizontal row of the Periodic Table have in common?
4, By what tvvo characteristics are all the elements of the Periodic Table placed in a particular row and column?
5. Imagine element number 15 had never been discovered. What
characteristics would you predict it to have based on its location
on the periodic table?
H
Li
Be
B
C
O
F
Ne
Na
Mg
Al
Si
s
a
Ar
K
Ca \
6. Which element has 3 outer electrons and 2 shells?
7. How is helium different from neon and areon? How is it similar?
Evan P. Silberstein, 2002
28
He
: Form
S4.1A
Name
PERIODICITY
Date
Period
by Evan P. Silbersteln
"How are the elements arranged?" you ask.
Mendeleev said they're arranged by mass,
'Cause when they're arranged by mass, you will see,
The properties repeat so periodically.
My dear Mr. Mendeleev, I think you've erred.
There's another order that is much preferred.
When elements're arranged by mass, unfortunately.
Some of them end up in the wrong family.
Chorus:
Periodicity is really cool.
Periodicity really rules.
It's one of chemistry's finest tools The Periodic Table, is oh so cool!
My name is Mosely, and I've found out,
Atomic number is the key, and there's no doubt.
Since protons are known to cause the properties,
Atomic number causes periodicity.
\Vhy should all the elements have to fit?
Some of them are measured wrong, I'm sure of it.
I'm sure that when the mass is measured properly
All of them will fit in perfect harmony.
When elements are ordered by atomic number
No disorder shows up to disturb our slumber.
The elements all fall in the right family,
And the properties repeat so periodically.
c
Voice
"How are the el-e-ments ar - ranged?" you ask.
Men - dele-ev said they're ar-ranged
F
-If—
i
\
-^-*
1
4
by mass
~T£
—'
-*^J
J
J
'Cause when they're
"""
91— *— *_Jr-j
"-•
I
,
J
m
m
ar-ranged by mass
.
—A
J1
G7
I
_J
-L-*
you will
see
Am
Dm
|
I
^
j ^=r^
•^-J-i
j
T
j
J•—J1—«
=•
The pro-per-ties
G
I
J j
U
i
*
1
J
1
J
^—*
*
\t so p e r - i
Per - i-o-di-ci-
Am
C
ty
i
rea]-]y rules.
Dm
It's one of chem - i - sty's
fin-est
E7
tools,
Am
oh
so
cool!
Evan P. Silberstein, 2003
29
The
Per-i - o-dic Ta-ble is
Name
Lab#
Mini Mendeleev Lab
Goal; To simulate a Periodic Table with known element values.
Background:
Dmitri Mendeleev is credited with developing the first Periodic Table in 1869.
Based on the physical and chemical properties of known element at the time, Mendeleev
looked for a logical way to organize the elements. Mendeleev arranged the elements in
order of increasing atomic mass. The element were placed in horizontal rows in such a
way that element with similar properties fell into the same vertical columns. He left
blank spaces on the table if no known element had the expected properties and atomic
masses to fill that particular spot. Although the elements are now arranged by atomic
number, not atomic mass, Mendeleev's work was a major achievement. In this lab you
will follow a path similar to that of Mendeleev. You will be provided with 12 elements
along with a list of some of their'physical and chemical properties. It is your goal to
arrange these elements into a table and explain your organizational scheme to the class.
Procedure:
•
•
•
•
•
•
Read and study all of the properties of the elements.
Look for similarities between elements.
Record all of the properties you observe.
Arrange the cards based on these similarities.
Try to create groups with the greatest number of similarities.
Once you have regrouped your elements, look at each group
INDIVIDUALLY.
• Try to arrange the members of each group in a logical way.
• Then, determine a logical way to arrange each group relative to the others.
• Tape or glue the element cards to a piece of paper using your organizational
scheme.
• Be prepared to explain your organizational scheme to the class.
Vocabulary:
Period Group Electro negativity lonization Energy Questions:
1. What criteria did you first use to organize your elements?
2. What was the next property used?
3. Can elements be organized in more than one way? If yes, how
30
1. On the Periodic Table of the Elements, all the
elements within Group 16 have the same
number of
6. An unknown element Xcan form a compound
with the formuIa^Br3. In which group on the
Periodic Table would element^Tbe found?
1) valence electrons
1) 1
2) energy levels
2) 2
3) protons
3) 13
4) neutrons
4) 14
2. After a neutral sulfur atom gains two electrons,
what is the resulting charge of the ion?
7. Which atom forms an ion with the largest radius?
1) I
2) Br
3. A chloride dissolves in water to form a colored
solution. The chloride could be
3) CI
4) F
1) HC1
2) KC1
3) CaCl2
8. What is the total number of valence electrons in
an atom of sulfur in the ground state?
1) 6
4) CuCl2
2) 8
4. In which section of the Periodic Table are the
most active metals located?
3) 3
4) 4
1) upper right corner
2) lower right comer .
3) upper left corner
9. In comparison to an atom of ^F in the ground
state, an atom of ^C in the ground state has
4) lower left corner
1) three fewer neutrons
2) three fewer valence electrons
5. On the present Periodic Table of the Elements,
the elements are arranged according to increasing
3) three more neutrons
4) three more valence electrons
1) number of oxidation states
2) number of neutrons
3) atomic mass
4) atomic number
31
Element 1
Element 2
Appearance: Colorless, odorless,
gas
Appearance: Colorless, odorless,
gas
Appearance: Colorless, odorless,
gas
Density: 0.0018 g/ml
Melting Point-189°C
Boiling point: -186°C
Electrical Behavior: Nonconductor
Density: 0.00018 g/ml
Melting Point -272°C
Bofling point: -269°C
Electrical Behavior Nonconductor
Density: 0.0038 g/ml
Melting Point -157°C
Boiling point -153°C
Electrical Behavior Nonconductor
Behavior with water: Unreactive
Behavior with water: Unreactive
Behavior with water Unreactive
Element 4
Elements
Element 6
Appearance: Soft,.silvery solid.
Tarnishes in air.
Appearance: Shiny violet-black
solid. Sublimes to form a violet
vapor with an irritating odor.
Appearance: Soft, silvery-white
solid. Tarnishes in air.
Density: 0.70 g/ml
Melting Point: 98°C
Boiling point: 892°C
Electrical Behavior: Conductor
__
Density: 4.9 g/ml
Melting Point: 113°C
Boiling point: 184°C
Electrical Behavior: Non-conductor
Elements
Density: 0.86 g/ml
Melting Point: 63 °C
Boiling point 774°C
Electrical Behavior: Conductor
Behavior with water: Reacts .
vigorously to produce hydrogen gas
and fprrnajjasic solution.
Element 7
Behavior with water Reacts very
slightly to form an jddic solution.
Element 8
Behavior with water Reacts
violently to produce hydrogen gas
andj.jjaacjsolution.
Element 9
Appearance: Pale yellow gas with
an irritating odor.
Appearance: Soft, silvery-white
solid. Tarnishes in air.
Appearance: Colorless, odorless,
gas
Density: 0.001
Melting Point: -220°C
Boiling point-118°C
Electrical Behavior Non-conductor
/ml
Melting Point: 179°C
Boiling point 1372°C
Electrical Behavior: Conductor
Behavior with water: Reacts
violently to release oxygen and form
an acidic solution.
Behavior with water Reacts
moderately to produce hydrogen gas
and form a basic solution.
Element 10
Element 11
Element 12
Appearance: Greenish-yellow gas
with an irritating odor.
Appearance: Soft, silvery-white
solid. Tarnishes in air.
Density: 0.0032 g/ml
Me!tingPoint:-101°C
Boiling point: -34 C
Electrical Behavior: Non-conductor
Density: 1.53 g/ml
Melting Point 3 9°C
Boiling point 679°C
Electrical Behavior: Conductor
Appearance: Reddish brown liquid.
Vaporizes readily to form a red
vapor with an irritating odor.
Behavior with water: Reacts
moderately to form an acidic
solution.
Behavior with water Reacts very
violently to produce hydrogen gas
and form a basic solution.
32
Density: -Q.Q0090 g/ml
Melting Point: -249°C
Boiling point -246°C
Electrical Behavior Nonconductor
Behavior with water Unreactive
Density: 3.1 g/ml
Melting Point-73°C
Boiling point 59°C
Electrical Behavior Non-conductor
Behavior with water Reacts
slightly to form an acidic solution.