Chapter 4 Quarterly notes Flashcards
Heisenbergs proposal answers question of where electrons are
Located if they are both par files and wave s
(Heisenberg) electrons are detected by their
Interaction with photons
(Heisenberg) because photons have about the same energy as electrons any attempt to locate a specific electron with a
Photon knocks the electron off its course
Erwin schrodingers used the hypothesis that electrons have a dual wave particle nature and
Developed an equation that treated electrons in atoms as waves
Quantization of electron energies was a
Natural outcome of schrodingers equation
Only waves of specific energies, and thus frequencies provide
Solutions to the equation
Quantum theory describes mathematically the
Wave properties of electrons and other very small particles
Electrons do not travel around the nucleus in
Neat orbits
Electrons exist in certain regions called
Orbitals
An orbital is a three dimensional
Region around the nucleus that indicated the probable location of an electron
Electrons in atoms orbitals also have
Quantized energies
An electrons energy level is not the only characteristic of an orbital that is indicated by
Solving the schrodinger equation.
Quantum numbers specify the properties of
Atomic orbitals and the properties of electrons in orbitals
Principal quantum number symbolized by
N
Principal quantum number indicates the
Main energy level occupied by the electron
Total number of orbitals in a given shel is equal to
n^2
Angular momentum quantum number symbolized by
L
Angular momentum quantum number indicates the
Shape of the orbital
For specific main energy level number of orbital shapes possible is equal to
N
Values of n are
Positive integers only
Values of l are zero and all
Positive integers less than or equal to n - 1
When l equals 0 the shape is
S
L = 1 shape is
P
L = 2 shape is
D
L= 3 shape is
F
Magnetic quantum number symbolized by
M
Magnetic quantum number indicates the
Orientation of an orbital around the nucleus
Values of m are
Whole numbers including zero from -L to +L
Orientation of s corresponds to
M=0
3 p orbitals relate to m values of
-1 0 and +1
D orientations correspond to m values or
-2 -1 0 +1 +2
Number of electrons per main energy level
2n^2
Spin quantum number has only
Two possible values -1/2 or +1/2
Which indicate the two fundamental soon states of an electron in an orbital
Electron configuration is the
Arrangement of electrons in an atom
Ground state configuration. Is the lowest
Energy arrangement of the electrons for each element
Aufbau principle l, an electron occupies
The lowest energy orbital that can receive it
Pauli exclusion principle, no two electrons in the same atom can
Have the same set of four quantum numbers
Hund’s rule, orbitals of equal energy are each occupied by
One electron before any orbital is occupied by s second electron and all electrons in singly occupied orbitals must have the same spin state
Noble gases
The group 18 elements (helium neon argon krypton xenon and radon)
Noble gas notation
To simply writing an electron configuration symbol for the previous noble gas is enclosed in square brackets is used to represent part of the configuration
Heisenberg uncertainty principle states that it is
Impossible to determine simultaneously both the position and velocity of an electron or any other particle
