Lesson 3: Quantum Numbers Flashcards
(32 cards)
Why doesn’t Hydrogen produce a continuous spectrum of light?
Because its orbitals have specific energy differences between them, resulting in light waves with specific energy levels and thus specific wavelengths. It cannot produce every different wavelength level.
What is the Rydberg equation for hydrogen, which relates wavelength of light emitted to the orbital level change of an electron?
(1/λ) = R((1/nf^2) - (1/ni^2)) λ = Wavelength R = Rydberg’s Constant (1.097 ⋅ 10^7) nf = Final Orbital Level ni = Initial Orbital Level
An electron within Hydrogen jumps from the second orbital to the first orbital. What wavelength of light is emitted considering that Rydberg’s constant is 1.097 ⋅ 10^7? (A) 6.78 ⋅ 10^-4 (B) 1.22 ⋅ 10^-7 (C) 1.81 ⋅ 10^-9 (D) 8.43 ⋅ 10^-15
(B) 1.22 ⋅ 10^-7 (1/λ) = R((1/nf^2) - (1/ni^2)) (1/λ) = (1.097 ⋅ 10^7)((1/1^2) - (1/2^2)) (1/λ) = approx. (.75 ⋅ 10^7) 1/(.75 ⋅ 10^7) = λ 1.34 ⋅ 10^-7 = λ, which is closest to (B) 1.22 ⋅ 10^-7
According to the Heisenberg uncertainty principle, it is impossible to know what two things about a moving particle at the same time? (A) Position and momentum (B) Direction and position (C) Momentum and acceleration (D) Acceleration and direction
(A) Position and momentum According to the Heisenberg uncertainty principle, it is impossible to know the position and momentum of a moving particle at the same time.
True or false? The ability to know the position, and the ability to know the momentum of a moving particle are inversely related.
True. The ability to know the position, and the ability to know the momentum of a moving particle are inversely related. As the knowledge of one increases, knowledge of the other decreases.
How does the Heisenberg uncertainty principle apply to the Bohr model of the electron?
It is impossible to know the location and momentum of an electron at the same time, which proves the Bohr model to be an inaccurate representation of the atom.
Which is the symbol for the principal quantum number? (A) l (B) n (C) m(l) (D) m(s)
(B) n n is the symbol for the principal quantum number.
Which is the symbol for the angular momentum quantum number? (A) l (B) n (C) m(l) (D) m(s)
(A) l l is the symbol for the angular momentum quantum number.
According to spectroscopic notation, which of the following angular momentum quantum numbers is improperly matched with its corresponding letter? (A) l = 0 , s (B) l = 3 , f (C) l = 2 , d (D) l = 4, h
(D) l = 4, h According to spectroscopic notation, the angular momentum quantum numbers’ corresponding letters are: l = 0 (s), 1 (p), 2 (d), 3 (f), 4 (g), 5 (h), etc. (alphabetical order).
Which is the symbol for the magnetic quantum number? (A) l (B) n (C) m(l) (D) m(s)
(C) m(l) m(l) is the symbol for the magnetic quantum number.
Which is the symbol for the spin number? (A) l (B) n (C) m(l) (D) m(s)
(D) m(s) m(s) is the symbol for the spin number.
Which quantum number is also called the azimuthal quantum number, and includes integer values up to n-1? (A) l (B) n (C) m(l) (D) m(s)
(A) l The angular momentum quantum number, or azimuthal quantum number, may have integer values as large as n-1.
Which of the following terms refers to an atom that has all of its electrons spin-paired, and will be slightly repulsed by an external magnetic field? (A) Magnetic (B) Paramagnetic (C) Ferromagnetic (D) Diamagnetic
(D) Diamagnetic A diamagnetic atom has all of its electrons spin-paired, and will be slightly repulsed by a magnetic field. Noble gases are diamagnetic.
Which of the following terms refers to an atom that does not have all of its electrons spin-paired, and will be slightly attracted by an external magnetic field? (A) Magnetic (B) Paramagnetic (C) Ferromagnetic (D) Diamagnetic
(B) Paramagnetic A paramagnetic atom has some electrons that are not spin-paired, and will be slightly attracted by an external magnetic field.
What are the possible values of n, l, m(l), and m(s) for when n = 1? How many electrons are in this shell?
n = 1 l = 0 (s) m(l) = 0 m(s) = +1/2 (up) or -1/2 (down) # of electrons = 2
What are the possible values of n, l, m(l), and m(s) for when n = 2? How many electrons are in this shell?
n = 2 l = 0 or 1 (s or p) m(l) = -1, 0, or +1 m(s) = +1/2 (up) or -1/2 (down) # of electrons = 8
What are the possible values of n, l, m(l), and m(s) for when n= 3? How many electrons are in this shell?
n = 3 l = 0, 1, or 2 (s, p, or d) m(l) = -2, -1, 0, or +1, +2 m(s) = +1/2 (up) or -1/2 (down) # of electrons = 18
What are the possible values of n, l, m(l), and m(s) for when n= 4? How many electrons are in this shell?
n = 4 l = 0, 1, 2, 3 (s, p, d, or f) m(l) = -3, -2, -1, 0, or +1, +2, or +3 m(s) = +1/2 (up) or -1/2 (down) # of electrons = 32
Draw the shape of the s orbital(s).
1 orientation
Draw the shape of the p orbital(s).
3 orientations
Draw the shape of the d orbital(s) and f orbital(s).
d has 5 orientations f has 7 orientations
Match the following orbitals with how many electrons can coexist in each. I. f II. s III. p IV. d (A) 10 (B) 6 (C) 14 (D) 2
I. (C) an f orbital can house 14 electrons. II. (D) an s orbital can house 2 electrons. III. (B) a p orbital can house 6 electrons. IV. (A) a d orbital can house 10 electrons.
Compare the Aufbau principle, the Pauli exclusion principle, and Hund’s rule.
The Aufbau principle is the “building up” principle, which states that electrons will fill in lower energy orbitals first. The Pauli exclusion principle is the “unique address” principle, which states that no two electrons can have the same four quantum numbers. Hund’s rule is the “empty bus seat” rule, which states that electrons will fill in orbitals one at a time before pairing up.
Which of these principles requires that an electron in the same orbital as another electron must spin in the opposite orientation? (A) Aufbau principle (B) Pauli exclusion principle (C) Hund’s rule (D) Electron configuration principle
(B) Pauli exclusion principle
