Key Terms:
 Group:
 Period:
 Orbital:
 Energy level:
 Quantized:
 Quantum numbers:
o Principle energy level:
 Discrete:
 Photon:
 Wavelength:
 Valence electron:
 Ionization energy:
 Electronegativity:
 Atomic radius:
 Shielding:
 Effective nuclear charge:
Key Principles/Laws
 Aufbau principle:
 Pauli Exclusion principle:
 Hund’s rule:
 Periodic Law:
Key Experiments/Scientists
 JJ Thompson:
o Experiment:
o What did it find:
 Rutherford
o Experiment:
o What did it find:
 Bohr
o Atomic Model:
o What did he find:
 Plank
o What did he find:
 Newlands:
 Mendeleev:
 Meyer:
 Mosely:
Electron Configuration Worksheet
PART A – ORBITAL NOTATION & ELECTRON CONFIGURATION
Use the patterns within the periodic table to draw orbital diagrams and write longhand electron
configurations for the following atoms.
Dot Diagram
Symbol
1.
Mg
2.
P
3.
V
4.
Ge
5.
Kr
# of e-
Orbital notation and Electron Configuration
Label the blank periodic table with the following terms:
Alkali Metals, Halogens, Metalloids, Transition Metals, Nobel gases, Lanthanide, Actinide
Periodic Trends
Use a periodic table to help you answer the following questions.
1. Which element in the second period has the greatest atomic radius?
2. Which of the group IIIA (13) elements is the largest?
3. Of the halogens, which has the smallest radius?
4. Which of the alkaline earth metals is the largest?
5. Which of the transition metals has the smallest atomic radius?
Which element in each pair has a larger ionization energy?
a) Na or O
b) Be or Ba
c) Ar or F
d) Cu or Ra
f) K or V
g) Ca or Fr
h) W or Se
Which particle has the larger radius in each atom/ion pair?
a) Na, Na+
b) S, S2c) I, Id) Al, Al3+
What is first ionization energy?
e) I or Ne
Arrange the following groups of elements in order of increasing ionization energy.
a) Be, Mg, Sr
b) Bi, Cs, Ba
c) Na, Al, S
Which element in each pair has a higher electronegativity value?
a) Cl, F
b) C, N
c) Mg, Ne d) As, Ca
Circle the best choice in each list:
a.
highest ionization energy:
C, N, Si
b.
largest ionic radius:
P-3, S-2, Cl-1
c.
highest electronegativity:
As, Sn, S
d.
smallest atomic radius
Na, Li, Be
e.
least reactive
Rb, K, Be
6. Indicate whether the following properties increase or decrease from left to right across the
periodic table. Account for the trend using the atomic model.
Trend
Atomic radius
Ionization energy
Electronegativity
Increasing or Decreasing
Explanation