Exam #4 Review
Electron Configuration and Periodic Table
1-
What do the following mean:
a. Group: column
b. Family: column
c. Period: row
d. Valence electrons: outermost energy level
electrons
2- How did Mendeleev contribute to the layout of the periodic table?
Organized the elements by increasing atomic mass – noticed a pattern in their properties
3- How did Mosley organize the periodic table? How was this organization a better improvement?
4-
5678-
Organized the elements by increasing atomic number; patterns became more regular with fewer
exceptions
Know the 5 major groups on the periodic table and their locations.
Group 1 – Alkali metals (except H), Group 2 – Alkaline Earth metals, Groups 3-12 – Transition metals,
Group 17 – Halogens, Group 18 – Noble gases
Give the difference between a neutral atom and an ion.
Neutral atom: P = E
Ion: P≠E
What is a cation and what is an anion?
Cation = + ion
Anion = - ion
How does the quantum model describe the structure of the atom (what are energy levels made up of)?
Energy levels are made up of sublevels, which are made up of orbitals, where the e- are found; more specific
Determine if the following are going to give or steal electrons and what their charge is going to be:
# of Valence Electrons
Element
Give Away or Steal
Charge of Ion
Ex: Phosphorus
5
Steal 3 or Give Away 5
-3
Sulfur
6
Steal 2 or give away 6
-2
Magnesium
2
Steal 6 or give away 2
+2
Aluminum
3
Steal 5 or give away 3
+3
Fluorine
7
Steal 1 or give away 7
-1
9Sublevel
Shape
# of Orbitals
Total # of electrons found
s
Spherical
1
2
p
Propeller
3
6
d
Double propeller
5
10
f
“flower”
7
14
10- How many total sublevels are found in the following:
a. 1st energy level: 1 (s)
b. 2nd energy level: 2 (s and p)
c. 3rd energy level: 3 (s, p and d)
11- Find the element that stops filling electrons at:
a. 6s2 Barium (Ba)
b. 4p5 Bromine (Br)
d. 4th energy level: 4 (s, p, d and f)
e. 5th energy level: 4 (s, p, d and f)
c. 3d3 1 Vanadium (V)
d. 5f8 Berkelium (Bk)
12- State the 3 Rules for doing electron configuration.
Aufbau principle – electrons fill lowest energy orbitals first (follow Aufbau sequence)
Hund’s Rule – p, d and f orbitals must each have 1 e- before any can have 2 ePauli Exclusion Principle – all orbitals can hold a maximum of 2 e- that move in opposite directions
13- Be able to do orbital diagramming for ANY element on the periodic table. Here are a few to practice.
a. Oxygen – 1s22s22p4
b. Nickel – 1s22s22p63s23p64s23d8
c. Selenium – 1s22s22p63s23p64s23d104p4