Download November 18

Thurs 11/18
Review for Test
Chapter 4
Know your E/M spectrum, from long wavelength/low frequency to short
wavelength. High frequency
2 formulas
C(speed of light 3x 108 m/s)=(lambda[wavelength in meters])(frequency in Hertz)
Energy in Joules = h (plank’s constant 6.6 x 10-34) x frequency
Example problem:
Given that red light has a wavelength of 700 x 10-9 meters, what is the frequency
and how much energy does it have?
To find frequency, use first formula, c=lambda x frequency
Frequency = 3x 108 m/s / 700 x 10-9 meters = 4.29 x 1014 Hz
To find Energy, plug it into the second formula:
E = hf = (6.6 x 10-34) x (4.29 x 1014 Hz) = 2.82 x 10-19 Joules
What is Fire? Excited electrons when energy is added release light when they
return to their original state
Know your flame test colors
Bohr’s model of atom, Heisenberg uncertainty principle, Quantum, Schrodinger
Chapter 5
Mendeleev, Moseley
Know group names, especially alkali metals and Noble gases, since we covered
them in class
Periodic Trends:
a) atomic radius b) ionic radius (size of atom after losing/gaining electron)
c)Ionization Energy (price to get electron from element)
d) Electron Affinity (how much energy element is willing to give for electron)
e) Electronegativity (how close element holds on to electron)
Example Problem:
Which is the largest/smallest ionic radii:
C, C4 +, C 4 -, C2C 4 – is the largest because it gained 4 electrons, C4 + is the smallest because it lost 4
electrons
Compare the atomic radius, Ionization energy, Electron Affinity, and
Electronegetivity for the following 4 elements:
K,Ca, Rb, Sr
Answer is: