Chapter 6.5 Quantum Mechanics And Orbital Balls

Question 0

Quantum numbers used to describe the quantum mechanical model

Answer 0

n ( the principal quantum number)
l (the angular momentum quantum number
m ( the magnetic quantum number)

Question 1

ORBITALS

Answer 1

A set of waves functions.
. Each orbital has a characteristic shape and energy
. It is a quantum mechanical model which describes electrons in term of probabilities,visualized as electron clouds)

Question 2

n ( the principal quantum number)

Answer 2

. Describes the ENERGY LEVEL on which orbital resides
.Can have positive integral values (1,2,3….)
. As n increases the orbital becomes larger and the electron spends more time away from the nucleus.
. Increase n= the electron has a higher energy and therefore less tightly bound to the nucleus.
. Equals the number of SUBSHELLS

Question 3

l (the angular momentum quantum number)

Answer 3

Have integral values from 0 to (n-1) for each value of n
. Defines the SHAPE of the orbital
. The value of l for a particular orbital is designated by letters s, p, d, and f, corresponding to values of 0,1,2,3

Question 4

Letters and numbers that designate the SHAPE of an orbital (l)

Answer 4

S= 0
P=1
D=2
F= 3

Question 5

The magnetic quantum number ( m)

Answer 5

. Describes the ORIENTATION of the orbital
. Can have integral values between -1 and 1( including zero)
.(2l+ 1)

Question 6

The designation s for l (orbital shape)

Answer 6

The value of l for s orbitals is 0.
They are spherical in shape.
The radius of the sphere increases with the value of n.

Question 7

Electron shell

Answer 7

The energy level that contains the orbitals

. Collection of orbitals with same value of n

Question 8

Subshell

Answer 8

Different orbital types within a shell are subshells.
. The set of orbitals that have the same n and l values
. It is designated by a number ( the value of n) and a letter ( s,p,d,f- values of l)