Atomic Orbitals Flashcards
What is the acronym to remember the electromagnetic spectrum
red
martians
invade
venus
using
X-ray
guns
What increases across the electromagnetic spectrum
energy and frequency
What decreases along the EM spectrum
wavelength
Electromagnetic spectrum question equation
C=f(lamda)
Explain the lines on emission spectra
Electron absorbs energy from heat or flame and is promoted to a higher energy level (excited state)
When the electron falls, it releases energy in the form of a wave
How to identify elements
Use their own spectra
(each element has their own)
How to calculate energy associated with wavelength
E=LHF or E=LHC/1000(lamda)
What is the principal quantum number
main energy level (n)
- can have value from 1 onwards
What is the angular momentum quantum number
the number of the subshell (l)
-value from 0 to n-1
What is the magnetic quantum number
the number of orbitals in each sub-shell (m)
- can take values from -l to +l
What is the term used to describe orbitals with the same energy
degenerate
What is the spin quantum number
the direction the electron is spinning in (ms)
What is the Aufbau principal?
energy levels filled up by increeasing energy
What is the pauli exclusion principle
electrons must have opposite spins
What is Hunds rule
each orbital must be filled before electrons start pairing up
What is ionisation energy
the energy required to remove 1 mol of e from 1 mol of atoms in the gaseous state
What is the second ionisation energy
the energy required to remove 1 mole of e from 1 mol of the positive ion
Why is it easy to remove an electron from aluminium than it is magnesium?
magnesium has a full sub shell which is therefore more stable than 3p1 in aluminium
Why is the ionisation energy for nitrogen higher than oxygen?
all orbitals are half filled in nitrogen, making it more stable
