Chemistry Chapter 7 Flashcards
Name the four quantum numbers
n, l, ml, ms
Explain n quantum number
- the shell
- determines the energy and size of the orbital
Explain l quantum number
Azimuthal q#
- sublevel or subshell
- = to n-1
- determines energy and shape of the orbital
Explain ml
- magnetic Q#
- determines the orientation of the orbital
- rule: l, 0, +l
Explain ms
- spin Q#
- determines spin of an electron and the orientation of the magnetic field produced by this spin
- either +1/2 or -1/2
How do electrons spin when they are in the same and different orbitals
- same: spin opposite
- different: same spin
Name the different subshells or l
-0, 1, 2, 3, 4, 5
Define the 0 subshell
- (s): sharp
- has 1 orbital
- 2 electrons
- starting shell= s=1
Define the 1 subshell
- p(principle)
- has 3 orbitals
- has 6 electrons
- starting shells is sp=2
- dumbbell shape
Define the 2 subshell
- diffuse (d)
- has 5 orbitals
- has 10 electrons
- spd=3
- has butterfly shape
Define the 3 subshell
- fundamental (f)
- has 7 orbitals
- has 14 electrons
- starting shell is spdf=4
- shape is complex
How do you write the electron configuration for ions that are transition metals
- transition metals lose valence s electrons first then d
How do you write electron configuration for metals in lower p block ions?
- lose valence p electrons then s electrons
What is important about d orbitals
completely filled and half filled d orbitals ate stable and prefer to stay that way so they will transfer electrons to get to this stability
State the equation for speed
c= frequency(new) times (wavelength) lambda
State the equation for energy
E= planks constant times frequency
E= planks constant times speed divided by wavelength
What are the units for equation c= frequency times wavelength
- c= m/s
- wavelength= m
- frequency= s-1 or Hz
What are the units for the equations E= hv and E= hc/ wavelength
- E= J
- h: 6.626*10^-34 Js
- c= 2.998*10^8 m/s
How to you find the wavelength of light when electrons change states
1/wavelength= 1.097*10^7 (1/n2^2- 1/n1^2)
What area of the electromagnetic spectrum can humans see
350-800
What state are atoms usually in
- ground state
What happens when electrons absorb energy
- go to excited state
Why do atoms have line spectrum and not continuum spectra
- b/c they have discreet energy levels
What is effective nuclear charge
- the amount of positive charge experienced by an electron in a polyelectronic atom
