HONORS CHEMISTRY CH 3, 7 & 8 ASSESSMENT REVIEW
3.1.1
Summarize the steps in the historical development of the periodic table
Discuss works of Döbereiner & Mendeleev
Predict properties of unknown elements given specific data, i.e. MiniLab 3.1, p. 87 or #15, p. 113
3.1.2
Predict similarities in properties of the elements by using the periodic table
If you know the formula for one compound, determine several
others, #25, p. 113, #8, p. 809
If you know the product of a reaction between 2 elements or
compounds, predict products for another; Alkali Metal Demo
Group elements that have similar properties (same group means
same # valence electrons); Oxidation Number (how many electrons an
atom gains or loses to become stable, or have an octet), #1, p. 809
3.2.1
Relate an element’s valence electron structure to its position on the periodic
table.
Draw Lewis Dot Diagrams
If an element has 5 valence electrons in the 3rd energy level, what is
it? #6, P. 809
3.2.2
Use the periodic table to classify an element as metal, nonmetal or
metalloid. #s 3 and 7 p. 809
Know Family names of Groups 1, 2, 17 and 18.
3.2.3
Compare the properties of metals, nonmetals, and metalloids. Know at
least 4 properties of each.
Why are transition elements and inner transition elements less
predictable than the chemistry of the main group elements?
If an element has tightly held electrons, and is a nonconductor of
electricity, what is it? How is conductivity affected by the flow of electrons?
Demo~Predicting a Periodic Trend
7.1.1
Relate emission spectra to the electron configurations of atoms.
How are the multiple wavelengths of red light given off in the
emission spectra for neon evidence of the existence of sublevels?
How is light created?
#1, p. 817
7.1.2
Examine energy sublevels and orbitals within an atom.
What sublevels are “allowed” in the first 4 energy levels? How many
orbitals are there within each sublevel? What is the maximum number of
electrons in an orbital? In a sublevel? In an energy level?
#2, p. 817
7.2.1
Distinguish between the s, p, d and f blocks on the periodic table and relate
them to an element’s electron configuration.
Name the highest occupied sublevel for an element; ex. barium
would be 6s and sulfur would be 3p.
#8, p. 818
7.2.2
Predict the electron configurations of elements using the periodic table.
Write configurations in both long form, and noble gas inner core
abbreviated form. Make sure you know the order to fill the sublevels; ex. 4s
comes before 3d.
Write the electron configuration for scandium: 1s22s22p63s23p64s23d1
#6 p. 818
Identify an element if you are given its electron configuration.
#5, p. 818
Explain WHY the transition elements have multiple oxidation
numbers. Use an example of a transition element to explain your answer.
#10, p. 818
Draw Orbital Filling Diagrams for a variety of elements ~
REMEMBER~ ALL VALENCE ELECTRONS and any incomplete d or f
sublevels are included~
8.1.1
Relate the position of main group elements on the periodic table to their
electron configurations. Period = outer energy level; Group corresponds to
# of valence electrons
8.1.3
Relate chemical behavior to electron configuration and atomic size.
Predict patterns in atomic size as it relates to increasing nuclear
charge. Write electron configurations for ions.
#s 1, 2 3 p. 818