Download Chapter 5 Section 1 - Ms. Halbohm`s Classroom

Chapter 6 Section 1
1. Who is credited with developing a method that led to the determination of standard relative atomic masses?
Who discovered the periodic law? Who established atomic numbers as the basis for organizing the periodic
table?
2. State the periodic law
3. Name three sets of elements added to the periodic table after Mendeleev’s time.
4. How do the atomic numbers of the elements within each of Groups 1, 2, and 13-18 of the periodic table vary?
5. How is the periodic law demonstrated within the groups of the periodic table?
Chapter 6 Section 2
1. Why are the noble gases relatively unreactive?
2. What determines the length of each period in the periodic table?
3. What is the relationship between the electron configuration of an element and the period in which that element
appears in the periodic table?
4. What information is provided by the specific block location of an element? Identify, by number, the groups
located within each of the four block areas.
5. Which elements are designated as the alkali metals? List four of the characteristic properties.
6. Which elements are designated as the alkaline-earth metals? How do their characteristics compare with those
of the alkali metals?
7. What name is sometimes used to refer to the entire set of d-block elements?
8. What types of elements make up the p-block? How do the properties of the p-block metals compare with those
of the s-block and the d-block?
9. Which elements are designated as halogens? List three of their characteristic properties.
10. Which elements are designated as metalloids? Describe their characteristic properties.
Chapter 6 Section 3
1. What is meant by atomic radius? What trend is observed among the atomic radii of main-group elements across
a period? How can this trend be explained?
2. Define the following terms:
a. Ion
b. Ionization
c. First ionization energy
d. Second ionization energy
3. How do first ionization energies of main-group elements vary across a period and down a group? Explain the
basis for each trend.
4. What is electron affinity? What signs are associated with electron affinity values, and what is the significance of
each sign?
5. Distinguish between a cation and an anion. How does the size of each compare with the size of a neutral atom
from which it is formed?
6. What are valence electrons? Where are the located?
7. For each of the following groups, indicate whether electrons are more likely to be lost or gained in compound
formation and give the number of such electrons involved:
a. Group 1
b. Group 2
c. Group 13
d. Group 16
e. Group 17
f. Group 18
8. What is electronegativity? Why is fluorine special in terms of electronegativity?
9. Identify the most and least electronegative groups of elements in the periodic table.