Chapter 2 Flashcards
Pauli Exclusion Principle
2 electrons per orbital
Hund’s rule
single electron occupy all empty orbitals within a sub-level before they start to form pairs in orbitals
State number of electrons in sub-levels s,d,p,f
s- 2, p-6, d-10, f-14
Aufbau Principle
electrons are placed into orbitals of lowest energy first
frequency(v) of waves
the number of waves which pass a particular point in 1 second
equation for measuring the speed of light (c) with wavelength λ and frequency v
c= vλ
continuous spectra
includes all of the frequencies and wavelengths of light
identify: rainbow
line spectra
includes selected frequencies
identify: lines
absorption spectrum
shows the radiation absorbed as atoms move from a lower to a higher energy level
emission spectrum
shows the radiation that is emitted when an atom moves from a higher to a lower energy level
What happens when an electron gains energy?
The atom becomes unstable and the electron falls to a lower energy level, thus emitting energy in the form of electromagnetic radiation.
What is planck’s constant? (h)
6.63x10 (to the)-34
What is c, the speed of light?
3 x 10 (to the) 8 m/s
What is Planck’s equation
energy = h x v
When an electron falls to the first energy level, what energy does it produce?
ultraviolet
When an electron falls to the 2nd energy level, what energy does it produce?
visible light
When an electron falls to the 3rd or higher energy level, what energy does it produce?
infrared radiation
True or false: Are energy levels closer together at higher energy?
True
Two isotopes of the same element have the same what?
- the same chemical properties
- the same atomic number
