CMY 385: Atom Theory Revision
What does it mean if said that energy is quantized? and what confirms this? - correct answer
only certain energy states are allowed in an atom, Line spectra of elements
Describe the Bohr model of atom theory - correct answer 1. e-'s are limited to
certain energy states
2. Energy levels: 𝑛 = 1, 2, 3, 4,. . ∞ n is a Unitless integer and called the principal quantum number
3. e-'s are limited to these levels
4. Absorption of energy (photon) takes place where e- "jumps" to a higher level
5. e- then "jumps" back to lower level and energy is released as a photon with 𝜈 (frequency) ∝ Δ𝐸 where
∆𝐸 is the difference in energy of the two levels
6. This released energy is the lines shown in spectra
Describe Schrödinger's quantum mechanical take on atom theory (Quantum mechanical model of the
atom) - correct answer 1. Electron described as a wave function 𝜳
2. Only some functions are allowed (again energy is quantized)
3. The solution to Shrödinger's equation predicts 3D-space in which e- with specific E can be found
4. 3 quantum numbers:
- n: describes size of orbital
- ℓ: shape of orbital
- mℓ: orientation of orbital
5. 𝜳^𝟐: probability of finding an e- in a small space
Comparison of allowed energies in the Bohr model and Quantum mechanical model of the atom (slide 5)
- correct answer 1. Quantum mechanical model: Orbitals of different principal
energy levels become mixed up (4s is lower than 3d)
2. Bohr's rule that electrons must have as low an energy as possible still applies
3. The crossing of energies of orbitals means that the 4s orbital will be filled before the 3d orbital
, Energy sublevels - correct answer slide 6
Draw s, p and d orbitals - correct answer slides 7-11
Each 𝒑-orbital is characterized by ______ nodal plane and d-orbitals and f- orbitals? - correct answer
1, 2, 3 nodal planes
What are quantum numbers? - correct answer 1. Terms that result from the math
of the Schrödinger equation
2. Describe specific orbital where electron can be found
3. "Address" of electron
Information needed for each electron (from quantum numbers) - correct answer 1.
Energy level (n)
2. Type of orbital (l)
3. Spatial orientation of orbital (ml)
4. Spin of the electron (ms)
Describe the Principal quantum number, n - correct answer 1. n = 1, 2, 3, ...
2. indicates energy level and size of orbital
3. The larger n, the larger the orbital
4. Electrons with the same n-value are in the same energy level (electron shell)
Describe the Angular momentum quantum number, ℓ - correct answer 1. = 0, 1, 2,
3, ..., 𝒏-1
2. Describe orbital type/shape
3. - ℓ =0= s
= 1= p
= 2= d
What does it mean if said that energy is quantized? and what confirms this? - correct answer
only certain energy states are allowed in an atom, Line spectra of elements
Describe the Bohr model of atom theory - correct answer 1. e-'s are limited to
certain energy states
2. Energy levels: 𝑛 = 1, 2, 3, 4,. . ∞ n is a Unitless integer and called the principal quantum number
3. e-'s are limited to these levels
4. Absorption of energy (photon) takes place where e- "jumps" to a higher level
5. e- then "jumps" back to lower level and energy is released as a photon with 𝜈 (frequency) ∝ Δ𝐸 where
∆𝐸 is the difference in energy of the two levels
6. This released energy is the lines shown in spectra
Describe Schrödinger's quantum mechanical take on atom theory (Quantum mechanical model of the
atom) - correct answer 1. Electron described as a wave function 𝜳
2. Only some functions are allowed (again energy is quantized)
3. The solution to Shrödinger's equation predicts 3D-space in which e- with specific E can be found
4. 3 quantum numbers:
- n: describes size of orbital
- ℓ: shape of orbital
- mℓ: orientation of orbital
5. 𝜳^𝟐: probability of finding an e- in a small space
Comparison of allowed energies in the Bohr model and Quantum mechanical model of the atom (slide 5)
- correct answer 1. Quantum mechanical model: Orbitals of different principal
energy levels become mixed up (4s is lower than 3d)
2. Bohr's rule that electrons must have as low an energy as possible still applies
3. The crossing of energies of orbitals means that the 4s orbital will be filled before the 3d orbital
, Energy sublevels - correct answer slide 6
Draw s, p and d orbitals - correct answer slides 7-11
Each 𝒑-orbital is characterized by ______ nodal plane and d-orbitals and f- orbitals? - correct answer
1, 2, 3 nodal planes
What are quantum numbers? - correct answer 1. Terms that result from the math
of the Schrödinger equation
2. Describe specific orbital where electron can be found
3. "Address" of electron
Information needed for each electron (from quantum numbers) - correct answer 1.
Energy level (n)
2. Type of orbital (l)
3. Spatial orientation of orbital (ml)
4. Spin of the electron (ms)
Describe the Principal quantum number, n - correct answer 1. n = 1, 2, 3, ...
2. indicates energy level and size of orbital
3. The larger n, the larger the orbital
4. Electrons with the same n-value are in the same energy level (electron shell)
Describe the Angular momentum quantum number, ℓ - correct answer 1. = 0, 1, 2,
3, ..., 𝒏-1
2. Describe orbital type/shape
3. - ℓ =0= s
= 1= p
= 2= d
