Chapter 2: Atomic Structure Flashcards
How many electrons can each orbital hold?
2 electrons each
How many orbitals in each sublevel?
The s sublevel has one orbital
The p sublevel has 3 orbitals
The d sublevel has 5 orbitals
How many sublevels in the nth main energy level?
n sublevels
What is the Pauli Exclusion Principle?
No more than 2 electrons can occupy any one orbital and if 2 electrons occupy the same orbital, they must spin in opposite directions.
What is the Aufbau Principle?
Electrons fill orbitals/sublevels of lowest energy first.
What is Hund’s 3rd Rule?
If more than one orbital in a sublevel is available, electrons occupy different orbitals with parallel spins in order to minimize mutual repulsion.
What are the two elements in which the 4s orbital is filled after the 3d orbital?
Copper and Chromium
Do radio waves or gamma waves have shorter wavelengths and higher frequencies?
Radio waves have greater wavelengths and thus lower frequencies than gamma waves.
This means that gamma waves are higher in energy .
What is the difference between a continuous spectrum, emission spectrum and absorption spectrum?
The continuous spectrum shows all wavelengths of visible light however the absorption spectra has missing wavelengths whereas the emission spectra has only certain wavelengths visible.
How can electrons transition between main energy levels?
By emitting or absorbing radiation.
To fall to lower energy levels, an electron must emit radiation and absorb it to transition to higher energy levels.(excited state)
How do you calculate the Energy of the photon emitted by each electron transition?
(Planck’s constant x speed of light)/wavelength
Why do certain metal ions give off colors when placed in a flame?
As when the sample containing the ions are heated, electrons absorb energy and transition to higher energy levels (excited state).
This electrons then emit energy in the form of certain wavelengths of visible light and return to lower energy levels.
The exact wavelength depend on the energy difference between the energy levels, therefore each element has a different energy difference between the energy levels and produces a different color.
What does a large increase in successive ionization energies indicate?
A jump from the outermost main energy level to the next one below as a greater proportion of energy is required.
Why is there an increase in successive ionization energies between sub-levels?
As lower sublevels experience stronger electrostatic forces of attraction from the nucleus.
