# Electron Config Practice For Test

```Review for Electron Configuration Test
Principles/Rules of the following individuals?
Aufbau
Hund
Pauli Exclusion
Heisenberg Uncertainty
Quantum numbers – n,l,m,s.. mean?
What was learned from Bohr model?
How Quantum model DIFFERENT from Bohr model?
An atom has 30 protons:
How many electrons are in this atom?
How many energy levels (principal quantum number, n) does this atom have in the lowest
energy state?
How many electrons are in the last energy level of the element when it is in the lowest
energy state?
What is the total number of sublevels in this element?
The letter designations for the first four sublevels, with the number of electrons that can
be accommodated in each sublevel are
Which of the following sublevels is 2nd lowest in energy?
a. 3d
b. 4s
c. 4p
d. 4d
How many electrons are there in the partially filled sublevel of chlorine?
How many sublevels does Krypton (z = 36) have?
The maximum number of electrons that can be present in an orbital is ____.
Based on the Bohr atomic model, calculate the following. Identify each answer CLEARLY.
a. What is the energy (in eV) of an emitted photon when an electron jumps from n=4
orbit to n=2 orbit?
b. What is the frequency of the emitted photon?
c. What is the wavelength of the emitted photon in nm or m? (1 m = 109 nm)
d. What is the speed of the emitted photon?
En= -13.6 eV/n2
E= hν
Energy of photon = hv= hc/λ
v= c/λ
Record correct electron configuration and Lewis dot structure for the elements:
Sulfur
Silver
Iron
c=νλ
```