Download Study Guide Chapter 6

Study Guide Chapter 6 - Key
1. (a) How did Mendeleev organize the periodic table?
Mendeleev’s periodic table organized the periodic table in order of increasing
atomic mass and put elements with similar properties in the same column.
(b) How did Moseley update the periodic tables?
Moseley organized the periodic table in order of increasing atomic number.
2. Define: (a) group (b) period (c) octet (d) octet rule (e) duet rule (f) semiconductor
(a) group: one of the 18 columns of elements in the periodic table.
(b) period: one of the 7 rows of elements in the periodic table.
(c) octet: 8 electrons in the outer level of an atom.
(d) octet rule: 8 electrons in the outer level of an atom makes it very stable.
(e) duet rule: 2 electrons will stabilize an atom with only one energy level.
(f) semiconductor: An element which is neither a good conductor or a good
insulator, but rather lies somewhere between the two.
3. What is similar about elements in the same
(a) group?
Elements in the same group have similar electron configurations and similar
properties.
(b) period?
Elements in the same period have the same number of energy levels (same outer
energy level).
4. State the four sublevel blocks of the periodic table and describe their basic location in
the periodic table.
5. Use the periodic table to predict the abbreviated electron configurations, starting with
the correct noble gas, for:
(a) As = [Ar]4s23d104p3
(b) Ir = [Xe]6s24f145d7
(c) Np = [Rn]7s25f5
6. (a) What is electron promotion?
Electron promotion is the process where an electron or two is moved from the
last “s” sublevel into the last “d” or “f” sublevel in order to either fill or half-fill the
“d” or “f” sublevel. This makes the atom more stable
(b) The predicted electron configuration for copper is slightly different than its’
actual electron configuration. Write the actual electron configuration
and explain why it is more stable than the predicted configuration.
The predicted electron configuration of copper is [Ar]4s23d9. Electron promotion
occurs and an electron is moved from the “s” sublevel to the “d” sublevel in order to
fill the “d” sublevel. The actual electron configuration is [Ar]4s13d10 which is more
stable with its full d sublevel.
7. List the various levels of stability from most stable to least stable (see Zones of
Stability chart in the notebook).
The Zones of Stability (see Zones of Stability chart in the notebook) shows that some
electron configurations are more stable than others. The most stable electron
configuration is a full outer level of electrons which is an octet for all levels except
the first level which only requires two electrons to fill it. The next most stable
electron configuration is a full last sublevel followed by a half full last sublevel. All
other electron configurations have no special stability.
8. (a) Where in the periodic table do we find metals, nonmetals, and metalloids.
Metals are to the left of the staircase line in the periodic table (except for
hydrogen which is a nonmetal). Nonmetals are to the right of the staircase line
in the periodic table. Metalloids are along the staircase line.
(b) State 6 differences in the properties between metals and nonmetals.
A table is given to you at the end of the second page of the chapter 6 notes that lists
these properties of metals and nonmetals.
(c) List the metalloids and explain their properties.
The metalloids include boron, silicon, germanium, arsenic, antimony, tellurium.
Metalloids have properties somewhere between metals and nonmetals.
9. List the families of the periodic table and the major properties associated with those
families.

Alkali Metals:
Group 1.

Alkaline Earth Metals: Highly reactive metals found in compound form in
the earth’s crust. Group 2. Important minerals.

Transition Metals: Less reactive harder metals found in groups 3 – 12.

Chalcogens: Nonmetals. Group 16. Many sulfur compounds stink.

Halogens: Most reactive nonmetals. Group 17. Have strong unpleasant
odors and are poisonous.

Noble Gases:
electrons.

Rare Earth Elements: Metals in the “f” block. Very uncommon. Many are
man made.
Most reactive metals. Low density, soft metals found in
Stable nonmetals. Group 18. Contain full outer level of