Test #4 Review
Periodic Table Basics, Electron Configuration, and Periodic Trends
Periodic Table Basics:
1. How did Mendeleev arrange the elements?
How did Moseley organize the periodic table?
Which way is it organized today?
2. What is the difference between groups and periods on the periodic table?
3. Know the 6 major families on the periodic table and their locations:
4. What side of the stair-step
are the metals found on?
Nonmetals?
5. Where are the
metalloids located?
6. List 4 PROPERTIES of metals
7. List 4 PROPERTIES of nonmetals
8. If an element has properties of both metals and nonmetals, what is it?
9. Why do the elements potassium and sodium have similar physical and chemical properties?
10. How do you know the number of valence electrons an atom has by looking at the periodic
table?
Electron Configuration & Waves:
11. Know the 3 rules that electrons follow when filling up sublevels
Afbau Principle –
Hund’s Rule –
Pauli Exclusion Principle –
12. Label each of the energy levels and sublevels on the periodic table.
13. Fill in the following table with the information for each sublevel:
Sublevel
Shape
Maximum # of Electrons
# of Orbitals
s
p
d
f
14. What sublevels are found in the following?
a. 1st energy level:
b. 2nd energy level:
c. 3rd energy level:
d. 4th energy level:
15. The following elements are characterized by the filling of what sublevels?
a. Alkali Metals and Alkaline Earth Metals:
b. Transition Metals:
c. Rare Earth Metals:
d. Non-Metals:
16. Write the complete electron configuration and noble gas configuration for each atom:
a. Oxygen
b. Cobalt
c. Phosphorus
d. Radium
17. Draw the Lewis Dot Structure for each of the following elements:
Carbon
Bromine
Calcium
Sulfur
Nitrogen
18. Name the element with the following electron configuration:
a. 1s22s22p63s1 _______________________
b. 1s22s22p63s23p64s23d8 _________________________
c. 1s22s22p63s23p64s23d104p4 ___________________________
19. Draw the orbital diagram for the following elements:
a. Sulfur
b. Iron
c. Iodine
20. When an electron falls from a higher energy level to a lower energy level, how is the energy
released? (Think of the flame test lab)
21. Draw and label the parts of a wave
22. What is the relationship between frequency and wavelength? What does this mean?
23. What is the frequency of light with a wavelength of 5.62 x 10-7 meters?
c=f×λ
c = speed of light = 3.00 x 108 m/s
Periodic Trends
24. What does atomic radius measure?
25. Which atom has the largest atomic radius?
26. Going down a group, does atomic radius increase or decrease? WHY?
Moving across a period (left to right)? WHY?
27. Put the following in order of increasing atomic radius (smallest to biggest)
a. P, Na, Cl, Al _________________________________
b. Sr, Ra, Be, Mg ________________________________
28. Define ionization energy
29. Which family has the highest ionization energy?
30. Going down a group, does ionization energy increase or decrease? WHY?
Moving across a period (left to right)? WHY?
31. Put the following in order of increasing ionization energy
a. O, Ne, Li, C ______________________________
b. P, N, Bi, As ______________________________
32. Define electronegativity
33. What element has the highest electronegativity?
34. Going down a group, does electronegativity increase or decrease? WHY?
Moving across a period (left to right)? WHY?
35. Put the following in order of increasing electronegativity
a. Mg, S, Ar, Al ____________________________
b. F, I, Cl, Br _____________________________