Darien High School
Chemistry 400 Honors – Mr. Heberton
Unit 6C
The PERIODIC TABLE
Dmitri Mendeleev is the father of the modern Periodic Table
The Periodic Table
CHEM WKST
p. 2
THE PERIODIC TABLE
DIRECTIONS: Answer correctly the following questions.
1. Who is considered to be the ‘father’ of the periodic table? __________________________________
2. How were the elements arranged? _____________________________________________________
3. What does periodic mean? ___________________________________________________________
4. How did Mendeleev predict in his Periodic Table the future discovery of then unknown elements?
_______________________________________________________________________________
5. Mendeleev noticed that properties of elements appeared at regular intervals when the elements were
arranged in order of increasing:
A. density
B. reactivity
C. atomic number
D. atomic mass
6. What was Henry Moseley’s contribution to the periodic table?_______________________________
7. The modern periodic law states that:
A. no two electrons with the same spin can be found in the same place in an atom
B. when elements are arranged according to increasing atomic number, there is a periodic repetition
of their chemical and physical properties
C. electrons exhibit properties of both particles and waves
D. the chemical properties of elements can be grouped according to periodicity, but physical
properties cannot
8. In a modern periodic table, every element is a member of both a vertical column and an horizontal
row. Which one is the group, which one is the period and which one is also called the family?
________________________________________________________________________________
9. On the periodic table, where are the:
A. main-group elements? ___________________________________________________________
B. transition elements? _____________________________________________________________
10. True or false:
A. ____All elements are either metals, non-metals or metalloids.
B. ____Most elements are non-metals
C. ____Group 1 elements (except for hydrogen) are known as the alkali metals
D. ____The transition elements include iron, copper, gold, nickel and zinc.
E. ____Group 13 elements are known as the alkaline earth metals
F. ____Inner transition metals are also called the f block elements
p. 3
The Periodic Table
DIRECTIONS: Use only the below periodic table to answer correctly the following questions.
11. What is the purpose of the dark ‘stairs’ on the right side of the periodic table?
________________________________________________________________________________
12. Name the group identified by each of the following letters:
A.
B.
C.
D.
E.
F.
G.
H.
I.
J.
13. Provide two properties for each of the following groups (from notes, book or online):
E.
F.
G.
H.
p. 4
The Periodic Table
14. What are five major properties of metals?
1)
____________________________
4) ____________________________________
2)
____________________________
5) ____________________________________
3)
____________________________
15. Which tends to be more reactive: alkali metals or alkaline earth metals? _______________________
16. An ionic compound that is brightly colored generally contains which type of metal? _____________
17. True or false:
A. ____Group 18 elements are very unreactive
B. ____Fluorine has a higher electrical conductivity than Chromium
C. ____Sulfur is an element that is brittle and does not conduct hear or electricity well
D. ____Out of Se, Si, P and Mg, only Mg is soft and malleable in its solid state
E. ____Most Halogens are solid at room temperature
18. Transition Metals - d-Block Elements
Transition metals generally have _____ valence electrons.
Define Ferromagnetism-
19. Inner transition Metals - f-Block Elements
Lanthanide Series = Elements # _____ to _____
Lanthanides are sometimes called “trace” elements. What does this mean?
Actinide Series = Elements # _____ to _____
Actinides are all ________________ elements and those with a higher atomic number than
Uranium are also called _______________________.
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The Periodic Table
CHEM WKST
PERIODIC TRENDS
DIRECTIONS: Answer the following questions correctly.
1. The energy required to remove an electron from an atom is the atom’s ________________________
A. electron affinity
B. electron energy
C. electronegativity
D. ionization energy
2. Moving from left to right across a period on the periodic table,
A. electronegativity values tend to become (larger or smaller)
B. ionization energy values tend to become (larger or smaller).
C. atomic radii tend to become (larger or smaller).
____________
____________
____________
3. Name:
A. the halogen with the lowest electronegativity value:
____________
B. the alkali metal with the highest ionization energy:
____________
C. the element in Period 3 with the smallest atomic radius:
____________
D. the Group 14 element with the largest electronegativity:
____________
4. Define the following terms:
A. atomic radius: __________________________________________________________________
B. ionization energy:_______________________________________________________________
C. ionic radius: ___________________________________________________________________
D. valence electrons: _______________________________________________________________
E. electronegativity: _______________________________________________________________
F. anion: ________________________________________________________________________
G. cation:________________________________________________________________________
H. nuclear charge: ________________________________________________________________
5. Explain the shielding effect and its importance in ionization periodic trends down groups.
6. The size of the atom gets bigger as one goes down the column of a group on the Periodic Table is due
to two factors: ________________________________________________________________.
7. As one goes from left to right across a period, the atomic radius decreases because of the increased
attraction of the electrons by an increased number of _____________________________________.
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The Periodic Table
8. Explain the trend for ionization energy going across the periods.
9. As one moves down a group, the reason that the ionization energy decreases, making it easier to
remove an electron is that the electrons are farther from the:________________________.
10. Rank in order of decreasing electronegativity: F, B, C.
11. Explain the trend for electronegativity going across the periods.
12. How does an atom turn into:
A. an anion? _____________________________________
give an example: ______________
B. a cation? ______________________________________
give an example: ______________
13. What is the octet rule? _____________________________________________________________
14. Use arrows on the following periodic tables to indicate increasing trends, by period and group, for the
following properties:
A. Atomic Radii
B. Ionization Energy
C. Electronegativity
\
D. Ionic Radius
The Periodic Table
p. 7
15. Use the periodic table to write the symbol, the most likely oxidation state (ion charge) and to describe
the key chemical properties of the following elements:
A. fluorine: ______________________________________________________________________
B. xenon:________________________________________________________________________
C. magnesium: ____________________________________________________________________
D. sodium:_______________________________________________________________________
E. oxygen: _______________________________________________________________________
F. gold: _________________________________________________________________________
16. Where are the most active metals located and why are they so reactive?
________________________________________________________________________________
17. Where are the most active nonmetals located and why are they so reactive?
________________________________________________________________________________
18. As you go from left to right across a period, the atomic size ( decreases / increases). Why?
________________________________________________________________________________
________________________________________________________________________________
19. As you go down a group/family, the atomic size ( decreases / increases ). Why?
________________________________________________________________________________
________________________________________________________________________________
20. As you go down a group/family, the first ionization energy generally: ( decreases / increases ).
21. The tendency of an atom to attract other electrons to itself is referred to as its: ___________________
22. Where is the atom with the following characteristic found on the periodic table?
A. highest electronegativity: _________________________________________________________
B. lowest electronegativity: _________________________________________________________
The Periodic Table
p. 8
23. Respond to the following questions:
A. Rank the following elements by increasing atomic radius: carbon, aluminum, oxygen, potassium.
B. Rank the following elements by increasing electronegativity: sulfur, oxygen, neon, aluminum.
C. Why does fluorine have a higher ionization energy than iodine?
D. Why do elements in the same group tend to behave similarly in chemical reactions?
E. Rank in order of increasing atomic radius: K, Na, Rb.
F. Rank in order of increasing atomic radius: N, O, F.
G. Rank in order of increasing ionization energy: Ca, Mg, Ra.
H. Rank in order of increasing ionization energy: Xe, Te, Sn.
I.
Rank in order of decreasing electronegativity: Li, Na, Cs.
J. Rank in order of decreasing electronegativity: Si, Cl, P.
K. Rank in order of decreasing ionic radius: Be, Sr, Mg.
24. A negative ion is ( smaller / larger ) than its parent ion. Why?
25. A positive ion is ( smaller / larger ) than its parent ion. Why?
26. Why is the electronegativity of an element such an important factor in determining its chemical
properties?