Review Sheet

Review Sheet

Chemistry

Chapter Six

1. Give the group, period, block, and symbol for elements with the following electron configurations:

a. [Ar] 4s² Group 2, period 4, s block
b. [Ar]4s²3d¹⁰4p² Group 14, period 4, p block
c. [Kr]5s²4d¹ Group 3, Period 5, d block

2. Write the abbreviated electron configuration for the following elements:

a. second period, group 1 [He] 2s¹
b. third period, group 16 [Ne] 3s²3p⁴
c. fourth period, group 6 [Ar] 4s²3d⁴
e. fifth period, group 11 [Kr] 5s²4d⁹

3. What is the most likely oxidation number for each of the following?

a. F -1 e. P -3
b. Cl -1 f. Mg +2
c. As -3 g. Al +3
d. Rb +1

4. What does everything in the same period share in common?

• 
  Have valence electrons in the same energy level
  
• 
  Have the same shielding effect
  

5. What does it mean if an element has a negative oxidation #? Which elements are most likely to do this?

The atom wants to gain electrons to have a stable outer shell. A stable outer shell has 8 electrons (octet rule). Non-metals are most likely to gain electrons.

6. What does it mean if an element has a positive oxidation number? Which elements are most likely to do this?

The atom wants to lose electrons in order to have a stable outer shell. A stable outer shell has 8 electrons (octet rule). Metals are most likely to have a positive oxidation number.

7. Why are the noble gases so unreactive? Why are groups 1 and 17 so reactive?

Noble gases have 8 electrons in their outer shell. 8 electrons means there is a stable outer shell.

8. Name three things that are common within the elements of the same group.

• 
  Same number of valence electrons
  
• 
  Similar chemical properties
  
• 
  Same effective nuclear charge
  
• 
  Oxidation number
  
• 
  Electron configuration
  

9. Which element has a larger atomic radii, barium or magnesium? Why? Which has a smaller radii, magnesium or silicon? Why?

Barium has a larger atomic radius because it has more energy levels and a larger shielding effect.
Silicon has a smaller atomic radius because it has a stronger nuclear charge.

10. Compare and explain the differences between the ionization energy of rubidium and iodine. Repeat for aluminum and indium.

Ionization energy is the amount of energy necessary to remove an electron.

Rubidum has a lower ionization energy than iodine because it has a lower nuclear charge so it is easier to remove an electron

Aluminum has a higher ionization energy than indium because there are fewer energy levels so it is more challenging to remove an electron.

11. Compare and explain the differences in electronegativity for potassium and bromine.

Electronegativity is the ability of an atom to pull electrons away from another atom.
Bromine has a higher electronegativity because it is better at pulling electrons away from another atom because it has a higher nuclear charge.

12. Where are metals, nonmetals and metalloids located on the periodic table? Differentiate between metals and nonmetals in terms of electrons. List Properties of each.

Metalloids are found on the staircase on the periodic table. They have properties of both metals and non-metals. They can be electron acceptors or electron donors.
Metals are found to the left of the staircase on the periodic table. Metals are generally electron donors. Metals are generally good conductors of heat and electricity and solid at room temperature.
Non-metals are found to the right of the staircase on the periodic table. They are generally electron acceptors. Non-metals are generally not solid at room temperature and poor conductors of heat and electricity.

13. 
    Don't forget to study Mendeleev and history of periodic table!!
    

Mendeleev organized the periodic table by an increasing atomic mass.

13. 
    What are the 4 major blocks of the periodic table and where are they located.
    

s


d

p

f