Chemistry Chapter 6 Review
6.1
1. How do chemists sort elements into groups?
Chemists used the properties of elements to sort them into groups.
2. How did Mendeleev arrange his periodic table?
In order of increasing atomic mass.
3. What two elements did Mendeleev predict would exist, but had not been discovered yet?
Gallium (Ga) and Germanium (Ge)
4. How are elements arranged in modern periodic tables?
In order of increasing atomic number
5. “Each period corresponds to a principle energy level.
6. What does the periodic law state: When elements are arranged in order of increasing atomic
number, there is a periodic repetition of their physical and chemical properties.
7. Place the following elements into three groups based on similar properties:
Li, As, Rb, P, F, Na, Cl, I, N
Class 
Property

1. Li, Rb, Na 2. N, P, As
3. F, Cl, I
8. What are the three classes elements can be grouped into, and what are their properties?
Metal
Metalloids
Nonmetal
-Good conductors of heat and
electricity
-High luster (shiny)
-Solid mostly
-Ductile (drawn into wire)
-Malleable (hammered into
sheets)
-Properties similar to both
metals and nonmetals
-Depends on conditions
-Variety of properties
-Gases mostly
-Poor conductors of heat and
electricity
-Brittle
-Opposite properties of metals
6.2
9. What type of information does the periodic table display?
Displays symbols and names of elements along with structure of their atoms.
10. What are the four groups elements can be sorted into based on their electron configuration?
Noble gases, representative elements, transition metals, and inner transition metals.
11. A. Color code the periodic table based on: 1. noble gases, 2. representative elements,
3. transition metals, and 4. inner transition metals. Make sure to create a key.
B. Circle each of the following: metal, nonmetal, metalloid
C. Above each group on the periodic table is a number-letter combo. Write this combo above
each group below.
6.3
12. Draw arrows representing increasing atomic size.
13. Draw arrows representing increasing ionization energy.
14. Draw arrows representing increasing electronegativity.
15. Define ionization energy:
Energy needed to remove an electron
16. Define electronegativity:
Ability of an atom to attract electrons when the atom is in a compound.