important questions in the overall scheme of life (or what i learned in chemistry class yesterday!)

Important Questions In The Overall Scheme

of Life (or

what I learned in chemistry class

yesterday!)

Give one noteworthy piece

of information indicating an electron is a

particle and then do the same thing

from a wave perspective.

When Schroedinger treated the electron as a wave he came up with

his famous “wave equation”…what

information does psi, , stand for?....what about

2

When considering the size of an

electron, what makes us rationalize why it

makes sense for to have many solutions for the same energy

value?

Give one noteworthy piece of information

indicating an electron is a particle and then do the same thing from a wave

perspective.Particle: electrons have a massWave: electrons produce interference patterns in the double slit experiment.

A series of images taken in a double-slit experiment with electrons as the electron current density is increased. Since there is only oneelectron in the apparatus at a given time, this figure shows how aninterference pattern can be built up from single-electron events.

(Taken from physicsweb.org/box/world/15/9/1/bologna-image)

When Schroedinger treated the electron as a wave he came up with his famous “wave equation”…what

information does psi, , stand for?....what about 2

stands for location of the electron stands for the probability of finding the electron at a specific location

When considering the size of an electron, what makes us

rationalize why it makes sense for to have many solutions for the same energy value?

Heisenberg’s Uncertainty Principle tells us that we can’t predict where an electron will be, only where it will probably be!

The given can be characterized by certain

parameters called quantum numbers…

•n (the principle quantum #)

•l (the secondary quantum #)

•ml (magnetic quantum #)

n values could be: 1, 2, 3, 4…∞

l values could be: 0, 1, 2, 3…n-1

For a given electron:

ml values could be: -l…0…+l

ms values could be: +1/2 or -1/2(spin quantum #... describes the direction of electron spin)

(describes the principle energy level)

(describes the sublevel of energy)

(describes which orbital)

n (the principle quantum #)

l (the secondary quantum #)

ml (magnetic quantum #)

sizeshape

orientation

n value getting bigger…larger orbital

l value =

0 (for all)

ml value =

0 (for all)ms value =

+1/2 or -1/2

l value =

1 (for all)

ml value =-1 ml value =0 ml value =

+1

p orbitalsp orbitals

l value =

2 (for all)

ml value =-2 ml value =+2

d d orbitalsorbitals

l value =

3 (for all)

ml value =

-3

ml value =+3

f orbitalsf orbitals

Construct a 4p orbital (contour) and assign the electron a set of quantum numbers.

Dumbbell shaped orbital with two nodes per loben= 4, l= 1, ml= -1, ms=

+1/2

Describe an orbital with the quantum number values:

n = 3, l = 2, ml = 1

Clover shaped….no nodes

Describe and construct an orbital with the quantum number values:

n = 4, l = 0, ml = 0Spherically shaped….three nodes