C/wavelength

c=3.00^8

C/frequency

c=3.00^8

Formula for Energy

HC/wavelength

h=6.626^-34

c=3.00^8

H/M*V=wavelength

H=6.626*10^-34

M=kg

V=m/s

Wavelength=pm

row or section

ex: 1=s 2=p 3=d 4=f

• Orientation in space of an orbital
• Slide 49
  Slide 49

  üEach sub shell is subdivided into “ORBITALS,” each capable of holding a pair of electrons.

  üml can have any integer value from -l  to +l.

  Each orbital within a given sub shell has the same energy.

• goes up to the second column
• charges +1, +2
• shape is circle
• l=0

• Column 13-18 on periodic Table
• only first two rows have P without D
• After row 3 all P orbitals have d^10
• Has 6 columns
• Shape is two clovers
• l=1

• Rows after 3 have D orbitals
• Last two rows of D have f^14
• full D is d^10
• l=2
• Shape is four clovers

• l=3
• Shape is crazy!
• Any element in Last two rows of D have f^14

• •Although we cannot precisely define an electron’s orbit, we can obtain the probability of finding an electron at a given point around the nucleus.
• Erwin Schrodinger defined this probability in a mathematical expression called a wave function, denoted y  (psi).
• ØThe probability of finding a particle in a region of space is defined by y2.

• The probability map for an electron 

• According to classical physics, particles move in a path determined by the particle’s velocity, position, and forces acting on it determinacy = definite, predictable future
  
• Because we cannot know both the position and velocity of an electron, we cannot predict the path it will follow indeterminacy = indefinite future, can only predict probability

• Increases to the left and down

Heisenburg

Uncertainty Principle

• Heisenberg stated that the product of the uncertainties in both the position and speed of a particle was inversely proportional to its mass
• This means that the more accurately you know the position of a small particle, like an electron, the less you know about its speed and visa-versa

• proposed electrons can only have specific amounts of energy
• fixed amounts=quantized
• electrons travel in a fixed distance from the nucleus=stationary states

• the atoms of a solid oscillate with a definite frequency
• E=nhv
• proposed that an atom could have only certain energies of vibration, E, those allowed by the formula
• h (Planck’s constant) is assigned a value of 6.63 x 10-34 J. s and  must be an integer.

• many metals emit electrons when a light shines on their surface
• if the wavelength of light is made shorter, or the light waves intensity made brighter, more electrons should be ejected

• violet to red (400-800)
• VIOLET,BLUE,GREEN,YELLOW,ORANGE,RED

• maximum wavelength for electrons to be emitted

• particles can have wave-like character
• the electron interferes with its own wave
• wavelength of a particle was inversely proportional to its momentum