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9th_Ch_2_3_The Four Quantum Numbers, Bohr Model and Atomic Spectra
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Created on January 4, 2023
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Transcript
The Four Quantum Numbers, Bohr Model and Atomic Spectra
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QUESTION 1/10
1. Which quantum number indicates the position of the orbital?
Magnetic
Charge
Angular momentum
correct!
QUESTION 2/10
2. What is the principal quantum number for the last electron that is added to potassium?
correct!
QUESTION 3/10
3. Which letter orbital corresponds to l = 2?
correct!
QUESTION 4/10
4. What is the largest principal quantum number that a calcium electron can have?
n = 0
n = 4
n = 3
correct!
QUESTION 5/10
5. Which of the following sets of quantum numbers CAN exist?
n = 2, l = 2, ml = 0, s = +1/2
n = 1, l = 0, ml = 1, s = +1/2
n = 2, l = 0, ml = 0, s = +1/2
correct!
QUESTION 1/10
6.How does the Bohr Model differ from the Rutherford model?
Rutherford assumed that the position of electrons was random, while Bohr identified that they were located in very specific energy levels.
Rutherford assumed that the nucleus did not have any charge at all, while Bohr correctly identified that it was negatively charged.
Rutherford assumed that the nucleus was negatively charged, while Bohr correctly identified that it was positively charged.
correct!
QUESTION 1/10
7.When an electron moves from an excited state to a ground state, it will _____.
release energy
absorb a photon
maintain a constant energy
correct!
QUESTION 1/10
8.Why should you avoid looking directly at magnesium burning?
Because of the low yellow burn that can be annoying to look at.
Because there is no energy released, which can deplete the area of oxygen.
Because of the high energy released and the ultraviolet flame present.
correct!
QUESTION 1/10
9.Which of the following is an example of when an electron absorbs energy?
When it goes from the second energy level to the fourth.
Because there is no energy released, which can deplete the area of oxygen.
Because of the high energy released and the ultraviolet flame present.
correct!
QUESTION 1/10
10
10.When writing electron configurations, electrons are represented in their lowest possible energy state, called their _____.
excited state
lowest state
ground state