Term

Definition
the distance between identical points on successive waves. (units = m or nm) 


Term

Definition
the vertical distance from the midline of a wave to the peak or trough. (E = 1/λ) 


Term

Definition
the number of waves that pass through a particular point in 1 second (Hz = 1 cycle/s = s^{1})
(s^{1} = 1/s) 


Term
What is the speed of a wave (u)? 

Definition
the product of the wavelength and frequency of the wave. (u = λv) 


Term
What is the numeric value of the speed of light? 

Definition
C = 3.00 x10^{8}m/s
or
3.00 x10^{17}nm/s 


Term
In the electromagnetic spectrum what is the order of radiation types from highest to lowest energy order? 

Definition
Gamma rays, X rays, Ultraviolet, Infrared, Microwave, Radio waves 


Term
Calculate the wavelength (in nm) of the red light emitted by a barcode scanner that has a frequency of 4.62 x10^{14} Hz.
1Hz = 1s^{1} 

Definition
C = λv
λ = C/v
λ = (3.00 x10^{17} ^{nm}/_{s }/ 4.62 x10^{14 }s^{1})
λ = 649nm 


Term
What is Planck's quantum theory equation? 

Definition
E = hv
E = energy of radiation (J)
h = Plancks constant (6.63 x10^{34} J.s.)
v = frequency of radiation (s^{1}) 


Term
What is Plancks constant? 

Definition


Term
What is the equation for the photoelectric efffect? 

Definition


Term
The energy required to dislodge electrons from sodium metal via the photoelectric effect is 275kJ/mol. What wavelength in nm of light has sufficient energy per photon to dislodge an electron from the surface of sodium? 

Definition
The energy 275kJ/mol is for one mol of photons. To find the energy per photon, we must divide by avagadro's number
E = (275kJ/1mol) x (1mol/6.022 x10^{23}photon) x (1000J/1kJ)
E = 4.567 x10^{19 }J/photon
E = hc/λ
λ = hc/E
λ = [(6.63 x10^{34 }J.s.) x (3.00 x10^{17 nm}/_{s})] /
(4.567 x10^{19} J)
λ = 436nm 


Term
When copper is bombarded with highenergy electrons, X rays are elimited. Calculate the energy (in joules) associated with the photons if the wavelength of the X rays is 0.154nm. 

Definition
E = hc/λ
E = [(6.63 x10^{34 }J.s.) x (3.00 x10^{17 nm}/_{s})] / (.154nm)
E = 1.29 x10^{15} J 


Term

Definition
E_{(n)} = R_{H}(1/n^{2}) 


Term
The change in energy when an electron undergoes a transition from one energy level to another is given by what equation? 

Definition
ΔE = R_{H} [(1/n_{f}^{2})  (1/n_{i}^{2})]
(R_{H} = 2.18 x10^{18 }J) 


Term
Calculate the wavelength (in nm) of a photon emitted by a hydrogen atom when its electron drops from the
n = 5 state to the n = 3 state. 

Definition
ΔE = R_{H} [(1/n_{f}^{2})  (1/n_{i}^{2})]
ΔE = 2.18 x10^{18} J [(1/3^{2})  (1/5^{2})]
ΔE = 1.55 x10^{19} J
E = hc/λ
λ = hc/E
λ = [(6.63 x10^{34} J.s.) x (3.00 x10^{17 nm}/_{s})] /
(1.55 x10^{19} J)
λ = 1280nm 


Term
What is the de Broglie equation? 

Definition


Term
Calculate the wavelength of an electron traveling with a speed of 2.65 x10^{6 }m/s.
(mass of electron = 9.10939 x10^{28} g)
(1J = 1kg m^{2}/s^{2})
(h = 6.63 x10^{34} J.s.) 

Definition
λ = (6.63 x10^{34} kg m^{2}/s^{2 }s) / [(9.10939 x10^{31} kg) x (2.65 x10^{6} m/s)]
λ = 2.74 x10^{10} m 


Term
Calculate the wavelength (in nm) of a H atom (mass = 1.674 x10^{27} kg) moving at a speed of 7.00m/s
(1J = 1kg m^{2}/s^{2}) 

Definition
λ = h/mv
λ = (6.63 x10^{34} kg m^{2}/s^{2} s) / [(1.674 x10^{27} kg) x (7.00 m/s)]
λ = (5.66 x10^{8} m) x (1 x10^{9} nm/1m)
λ = 56.6nm 


Term
What is the Heinsberg Uncertainty Principle? 

Definition
it is impossible to know simultaneously both the position and momentum of a particle as small as an electron 


Term
If l = 0, what orbital is it in? 

Definition


Term
If l = 1, then what orbital is it in? 

Definition


Term
If l = 2, what orbital is it in? 

Definition


Term
if l = 3, what orbital is it in? 

Definition


Term
Which set of quantum numbers is permissible for an electron in an atom?
a) n =1, l = 1, m_{l} = 0, m_{s} = +1/2
b) n = 3, l = 1, m_{l} = 2, m_{s} = 1/2
c) n = 2, l = 1, m_{l} = 0, m_{s} = +1/2
d) n = 2, l = 0, m_{l} = 0, m_{s} = +1 

Definition
a) n =1, l = 1, m_{l} = 0, m_{s} = +1/2
b) n = 3, l = 1, m_{l} = 2, m_{s} = 1/2
c) n = 2, l = 1, m_{l} = 0, m_{s} = +1/2
d) n = 2, l = 0, m_{l} = 0, m_{s} = +1 


Term
What does paramagnetic mean? 

Definition
elements and compounds that have unpaired electrons and are attached to a magnet 


Term
What does diamagnetic mean? 

Definition
substances in which all electrons are paired and are slightly repelled by a magnet 


Term
What is the Pauli exclusion principle? 

Definition
no two electrons in an atom can have the same four quantum numbers. 

