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Create a Table
Chem catalyst:
We have spent several
days talking about atoms. Explain 5
patterns we have found in the periodic table so far.
Procedure 1:
1. Work in groups of 4 with one set of periodic table
cards.
2. Find Be, Mg, Ca, and Sr from Mendeleev's table and
arrange them in a column.
3. With your group, decide how you can use the
remainder of the cards to reconstruct Mendeleev's table.
4. Arrange the cards.
Answer
the following questions:
1. What characteristics did you use for sorting?
2. Describe as many patterns or trends as you can find in the table
you created.
3. Where did you put H and He? What was your reasoning for this
placement?
4. What exceptions or irregularities did you notice
while you were making the table?
Physical description
5. Where are
most of the gases located on the periodic table?
6. Where are
the nonmetals located?
7. Where are
the shiny elements located?
8. Most
periodic tables have a dividing line between the metals and the nonmetals.
Where would you place this line?
9. Is Tl
(thalium) a metal, metalloid or nonmetal?
Reactivity
10. In what
areas of the periodic table do you find the most highly reactive elements?
11. How would
you expect Cs (cesium) to react with water? Explain your reasoning.
12. Find the
element with the atomic number 89. If there were a card for this element, what
would it probably say in the lower left comer?
Compound
formation
13. What do you
notice about the chemical formulas for the compounds that form for elements
that are in the same column? (Chemical formula is the symbol and
subscript. For example CaCl2.)
14. What
compound will form between the elements Ba and Cl?
Periodic
properties
15. What
properties do the elements in Group VIIIA in common?
16. What
properties do the elements in Group IA have in common?
17. When something is
periodic, it means that there are repeating patterns. Explain, using examples,
why the table of elements is called a periodic table of the elements.
Procedure 2:
1.Get a blank periodic
table from Mr. De Santo.
2. The halogens are a group
of elements that form 1 ions. The halogens are fluorine, chlorine, bromine,
iodine, and astatine. Find them on your table.
Label the top of the column with the word halogens and a 1. Color these boxes light violet.
3. The alkalai metals are a
group of elements that form +1 ions.
The alkalai metals are H, Li, Na, K, Cs, Rb and Fr. Label this group with the word alkalai and
a +1. Color this group light red.
4. The alkalai earth metals
are a group of elements that form +2 ions.
The alkalai earth metals are all in group IIA. Label these elements with a group name and charge then color the
boxes light orange.
5. The noble gases are yet
another group of elements with similar properties. All of these elements are
highly NON-reactive. The noble gases are helium, neon, argon, krypton, xenon,
and radon. Write noble gases above this column and leave them white.
6. The lanthanides and
actinides are the two rows of elements at the very bottom of the
periodic table. They are below the table for simplicity's sake. If they were
included in the table the table would be too long for most pieces of paper.
Each row of elements has similar properties and thus is given a name. The
lanthanides are the uppermost row and the actinides are the bottom row. Outline
the squares of the lanthanides with dark green and the actinides with brown.
Label each row, too.
7. The B group elements,
which stretch from Group IIIB to Group IIB in the middle of the line along the
left side of scandium, yttrium, lanthanum and actinium (between group 2 and
group 3) to show where the transition metals begin. Draw a dark vertical line
along the right side of zinc, cadmium and mercury (between group 12 and group
13) to show where the transition metals end.
8. Look at the elements in
group VIA. These elements are most
likely to form 2 ions. Write the
charge above the column and color these with dark blue (be able to separate these
from the group V.)
9. Group V tends form 3
ions. Label this column with the charge
and color these boxes light light blue.
10. Group IV is an unusual
group of elements. These elements from
+4 ions if they are attached to halogens and 4 ions if they are attached to
metals. Label this column with +
4 and color it green.
11. Mercury and bromine are
the only two elements in the periodic table that are liquids in their state.
Outline these two boxes with a dark red pencil.
12. Quite a few of the
nonmetal elements are gases in their natural state. They are oxygen, nitrogen,
helium, hydrogen, argon, neon, krypton, xenon, chlorine, fluorine, and radon.
Outline these elements with a dark purple pencil.
13. All of the elements
higher than element #92 (93 and greater) are man-made. Mark these elements with
dark yellow dots.
14. Seven elements are
diatomic in nature. This means that if the atom is in its elemental form, not
combined with other elements, it will co-exist with an atom of the same
element. For example, oxygen occurs as 02 in nature, not as plain 0.
With a dark black pen, write a small 2 in the lower right corner of each symbol
of each of the seven diatomic elements: hydrogen, nitrogen, oxygen, fluorine,
chlorine, bromine, iodine.
15. Columns 1A and 2A are
called S-Block elements. Put a letter S
below these columns. Columns 3A 8A
are called P block elements. Put a
letter P under these columns. Columns
3B-2B are called transition metals and D-Block elements. Please label these columns with both
names. The separated group at the
bottom of the table are F-block elements.
Please label this group with an F.
16. Make a key in the back
of your periodic table so you will know what each mark means.
Answer the following
questions:
16. How many groups are
there in the periodic table? ___
17. How many periods are
there in the periodic table?___
18. Most of the elements in
the periodic table are (circle one): metals nonmetals metalloid
19. Where are the nonmetals
located on the periodic table?
20. How many elements are
gases in their natural state? _____
21. How many elements are
solids in their natural state? ____
22. Name the four main
families:
a. group 1, IA:
b. group 2, IIA:
c. group 17, VIIA:
d. group 18, VIIIA:
23. Most elements found in nature are (solids, liquids,
gases). (Circle one.)
scan and insert periodic table here.
Draw spaces on back of the table for tool kit. Key to front, key equations, unit factors,
etc.
Periodic Table Notes
PERIODIC LAW WHEN ATOMS ARE ARRANGED IN ORDER OF
INCREASING ATOMIC NUMBER, THEIR PHYSICAL AND CHEMICAL PROPERTIES SHOW A
REPEATING PATTERN.
MENDELEEV SONG A musical interlude to celebrate the
chemist who was brilliant enough to find patterns in the elements.
PERIODIC TRENDS
Atomic
Radius actual size of the atom.
- larger as you go down a column each new row adds a
new shell of electrons.
-
smaller from left to right each new column adds protons and attracts
electrons
more tightly.
Ionization energy How strongly atoms hold on to
their outermost electrons
-
weaker as you move down a column
- stronger from left to right
Electronegativity the ability to attract electrons
in a chemical bond (Know this well!!!!!!!)
-
relative term, cannot be measured, relates to size and ionization energy
-
weaker as you move down a column
-
stronger as you move left to right.
GENERAL RULE MORE PROTONS = STRONGER ATTRACTION.
SMALLER
SIZE = STRONGER ATTRACTION
Think
about the relationship attraction in chemistry analogy.