Chapter 8 (Quantum) Flashcards
Define wavelength (λ)
Midpoint of two peaks or two troughs (usually measured in meters)
Define frequency (ν)
The number of oscillations per second (usually measured in 1/s or Hz)
Define amplitude
Half peak to trough
Speed of light (c)
3x10^8 m/s
What power of 10 is meters to nanometers?
10^-9
In the visible light spectrum, which has more energy: Blue or red light?
Shorter wavelengths have more energy and a higher frequency. Blue light has more energy compared to red light.
Define spectral lines
When a substance is heated, it emits energy in the form of light. The different wavelengths that are emitted are atom specific, so we can tell what element it is by these spectral lines.
What is an energy level?
A defined distance from the nucleus, where n can go to infinity.
What is ground state?
The lowest energy electron configuration of an element
What is excited state?
Any electron configuration arrangement that has higher energy than the ground state (promoting electrons from n=1 to n=2)
What’s the difference between absorption and emission
Absorption is when an electron absorbs energy to jump energy levels, and emission is the wavelength of light that is emitted when the electron returns to its ground state.
What are quantum numbers and why are they important?
They are “coordinates” of each electron in space. This helps us understand many things including the characteristics of elements.
Heisenberg uncertainty principle
There’s a limit to knowing the precise location of a particle (electron)
State what each quantum number means (n, l, ml, ms)
Apartment building analogy
n = energy level = 1, 2, 3… = (Floor)
l = orbital = n-1 = (Type of apt: 1BR, 2BR..etc)
ml = orientation = - l to l = (Apt number)
ms = spin up/spin down = 1/2 / -1/2 = (Your room)
What are the letters of the orbitals in order of increasing energy?
s, p, d, f
