Download Name: Per: _____ Date: ______ Unit 5 Redemption Packet: The

Name: ___________________________
Per: _____
Date: ____________
Unit 5 Redemption Packet: The Periodic Table
Use the information in your notes and text book, pages 174 - 194 to answer the following
questions. If you missed any notes, you will find them at www.starkchemistry.weebly.com.
1. Mendeleev arranged the elements in his periodic table by increasing _______________
________________.
2. Why did Mendeleev leave spaces in his periodic table?
_________________________________________________________________________
3. The modern periodic table is arranged by increasing ________________
_________________.
4. Elements become more / less metallic as you go across a period on the periodic table.
5. Elements in the same group / period have similar chemical properties.
6. Which element listed below should have chemical properties similar to fluorine (F)?
A. Li
C. Br
B. Si
D. Ne
7. Identify each property below as more characteristic of a metal or a nonmetal.
a) A gas at room temperature
________________
b) Brittle
________________
c) Malleable
________________
d) Poor conductor of heat
________________
e) Shiny
________________
8. Identify each element as a metal, metalloid, or nonmetal.
a) Fluorine
___________________
b) Germanium
___________________
c) Zinc
___________________
d) Phosphorus
___________________
e) Lithium
___________________
9. Which of the following is NOT a transition metal?
a) Magnesium
b) Titanium
c) Chromium
d) Mercury
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10. Elements can be divided into metals, nonmetals, and metalloids. Distinguish between them.
Metals:
________________________________________________________________
Nonmetals: _______________________________________________________________
Metalloids: ________________________________________________________________
11. The following families are located in which group(s) on the periodic table?
a) Alkali metals
_____________
b) Alkaline Earth metals _____________
c) Halogens
_____________
d) Noble gases
_____________
e) Transition Metals
_____________
12. Label as alkali metal, alkaline earth metal, halogen, noble gas, or transition metal.
a) Ca
________________________________
b) Cu
________________________________
c) Br
________________________________
d) Na
________________________________
e) He
________________________________
f)
________________________________
Fe
13. How many valence electrons do the following elements contain?
a) K
________
b) Cl
________
c) Ar
________
d) Si
________
e) Ga
________
f)
________
Cr
14. Name the element that matches the following description.
a) Has 5 electrons in the 3rd energy level.
_____________________
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b) Has an electron configuration that ends with 4s 4p _____________________
c) Group 6A element in period 4.
_____________________
d) Alkaline earth metal in period 5
_____________________
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15. Which noble gas does not have 8 valence electrons? _______________
16. How is the atomic radius of an atom determined? _________________________________
________________________________________________________________________
17. a) How does atomic radius change across a period? ________________________
b) How does atomic radius change down a group? _______________________
18. Circle the element in each pair that has atoms with a larger atomic radius.
a) Sodium, lithium
b) Strontium, magnesium
c) Carbon, germanium
d) Selenium, oxygen
19. Order the elements S, Cl, and F in terms of increasing atomic radii.
______________
20. Define ionization energy. _____________________________________________________
_________________________________________________________________________
21. a) How does IE change across a period? _____________________
b) How does IE change down a group? _____________________
22. Circle the element in each pair that has the greater ionization energy.
a) Lithium, boron
b) Magnesium, strontium
c) Cesium, aluminum
23. Arrange the following groups of elements in order of increasing ionization energy.
a) Be, Mg, Sr
______________________
b) Bi, Cs, Ba
______________________
c) Na, Al, S
______________________
24. Metal atoms tend to lose / gain electrons and form positive / negative ions. (circle)
25. Nonmetal atoms tend to lose / gain electrons to form positive / negative ions.
26. What is a cation? ____________________________________
27. What is an anion? ____________________________________
28. Circle the particle that has the larger radius in each atom / ion pair.
a) Na, Na+
c) I, I
b) S, S2
d) Al, Al3+
29. What is electronegativity? ____________________________________________________
_________________________________________________________________________
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30. How does EN change across a period? __________________________________
31. How does EN change down a group? _________________________________
32. Circle the element in each pair that has a higher electronegativity value.
a) Cl, F
c) Mg, Ne
b) C, N
d) As, Ca
33. When the elements in each pair are chemically combined, which element in each pair has a
greater attraction for electrons?
a) Ca or O
c) H or O
b) O or F
d) K or S
34. For which of these properties does lithium have a larger value than potassium?
A. First ionization energy
B. Atomic radius
C. Electronegativity
D. Ionic radius
35. Which of the following properties generally increases as we go from the lower left to the
upper right of the periodic table?
A. Atomic number
B. Number of electron shells
C. Atomic size
D. Ionization energy
E. None of the above
36. a) The overall reactivity of metals increases / decreases down a group.
b) The most reactive metal is ___________________.
37. a) The overall reactivity of nonmetals increases / decreases down a group.
b) The most reactive nonmetal is __________________.
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