chapter 6 electronic structure of atoms
DESCRIPTION
CHAPTER 6 ELECTRONIC STRUCTURE OF ATOMS. Almost everything we now know about electrons came from the study of light. Light is a type of electromagnetic radiation. Types of Electromagnetic Radiation. Three complete cycles of wavelength (l ). - PowerPoint PPT PresentationTRANSCRIPT
CHAPTER 6
ELECTRONIC STRUCTURE OF ATOMS
Almost everything we now know about electrons came
from the study of light.
Light is a type of electromagnetic radiation.
Types of Electromagnetic Radiation
Three complete cycles of wavelength
The product of the frequency and its
wavelength equals the speed of light (c).
c =
C =
Since the speed of light is 3 x 108 m/s, there must be an inverse relationship between wavelength and frequency
The yellow light given off by a sodium vapor lamp
used for public lighting has a wavelength of 589 nm. What is the frequency of
this radiation?
The yellow light given off by a sodium vapor lamp
used for public lighting has a wavelength of 589 nm. What is the frequency of
this radiation? c = = 5.09 x 1014 s-1
Max Planck assumed that small quantities of energy (quantum) can be emitted or absorbed as
electromagnetic radiation.
E = hv Planck’s constant (h) = 6.63 x 10-34 joule-seconds (J-s)
Since yellow light has a wavelength of 589 nm, what is the smallest quantum of
energy that can be absorbed from yellow light?
Since yellow light has a wavelength of 589 nm, what is the smallest quantum of
energy that can be absorbed from yellow light?
E=hv E=(6.63 x 10-34)(5.09 x 1014)
E = 3.37 x 10-19 J
Johann Balmer observed the 4 lines of the hydrogen
spectrum to come up with a formula:
v=C(1/22-1/n2) n= 3,4,5,6
Niels Bohr assumed that electrons orbit in circular paths around the nucleus.
He also said that orbits of certain radii correspond to
certain energies.
En=(-RH)(1/n2)
n= 1, 2, 3, 4, …
n= the principal quantum number
RH = 2.18 x 10-18 J
Bohr assumed that electrons could “jump” from one
energy state to another by absorbing or emitting energy
of certain frequencies.
E= Ef - Ei = hv
By combining some equations:
v= E/h = (RH/h)(1/ni2-1/nf
2)Calculate the wavelength of light that
corresponds to the transition of the electron from the n=4 to n=2 state of the
H atom.
Heisenberg’s Uncertainty Principle:
It is impossible for us to know the exact velocity or
exact location of an electron
This is a probability
density of the location of the electron in a H atom.
This represents the shape of the s orbital.
The p Orbitals
The d Orbitals