Unit 4 Test Part. 2 Flashcards
Quantum number 1
QN1: Principle Quantum Number - Describes energy level
Quantum Number 2
QN2: Angular Momentum Quantum Number - Describes the shape of the orbitals
Quantum Number 3
QN3: Magnetic Quantum Number - Each sphere can be oriented differently in space
Quantum number 4
QN4: Spin Number - Electrons in an orbit spin on an axis creating a magnetic field.
1st rule of filing up orbitals
Aufbau Principle: an electron occupies the lowest-energy orbital that can receive it.
2nd rule of filling up orbitals
Pauli exclusion principle: no two electrons in the same atom can have the same set of 4 quantum numbers.
3rd rule of filling up orbitals
Hund’s rule: Orbitals of equal energy are occupied by one electron before any orbital is occupied by a second electron, and all singly occupied orbitals will have the same spin.
How scientists went from thinking the energy of light was a continuous wave to the dual-wave particle nature of light we accept now.
Initially, scientists thought light was a continuous wave. However, the photoelectric effect created a mystery: when light struck certain metals, it ejected electrons, but only above a certain frequency, no matter the intensity. Albert Einstein resolved this issue by proposing that light consists of packets of energy called photons, introducing the concept of dual-wavelike particles. This explained why low-frequency light no matter the intensity couldn’t eject electrons, as each photon needs sufficient energy to do so.
According to Bohr’s model, how is hydrogen’s line emission spectra produced?
when an electron in a hydrogen atom jumps from a higher energy level (excited state) to a lower energy level (ground state)
What is the issue with Bohr’s model?
it fails to accurately explain the behavior of electrons in atoms with multiple electrons, violates the Heisenberg Uncertainty Principle by assuming precise electron positions and orbits
