Chem IH Atom Worksheet – Block ____ Teacher _________ Name _______________
As you saw in the video “The Hydrogen Atom”, the hydrogen atom’s electron has an
energy of –313.6 Kcal/mole/n2 where n is the shell or energy level the electron is in,
equal to the value of the principal quantum number for the electron.
In an H atom, the electron jumps from the energy level 6 to energy level 2. It
loses its energy by emitting a photo.
CALCULATE: The energy the electron has before the jump:
__-8.711__ ____ Kcal/mol = ____-36.45_____ KJ/mol = _-6.053 x 10-20 Joules.
The energy the electron has after the jump:
___-78.40______ Kcal/mol = __-328.0_____ _ KJ/mol = _-5.447 x 10-19_ Joules.
The energy the photon carries away:
____69.69__ ___ Kcal/mol = ____291.6_____ KJ/mol = __4.842 x 10-19_ Joules.
The frequency, υ, of the photon. __7.308 x 1014___/sec.
The wavelength, λ, of the photon; 4.105 x 10-7_ = _410.5__nm = _4105_ Ǻngstroms.
Color of this photon. ____violet_____. Show all work on the back of this sheet.
In an H atom, the electron jumps from the energy level 5 to energy level 2. It
loses its energy by emitting a photo.
CALCULATE: The energy the electron has before the jump:
__-12.54______ Kcal/mol = ___-52.48_____ KJ/mol = _-8.715 x 10-20_ Joules.
The energy the electron has after the jump:
___-78.40______ Kcal/mol = __-328.0_____ _ KJ/mol = _-5.447 x 10-19_ Joules.
The energy the photon carries away:
___65.86______ Kcal/mol = ___275.2______ KJ/mol = _4.576 x 10-19_ Joules.
The frequency, υ, of the photon. _6.906 x 1014_/sec.
The wavelength, λ, of the photon; 4.344 x 10-7 m = _434.4__nm = _4344_ Ǻngstroms.
Color of this photon. _violet / indigo . Show all work on the back of this sheet.
Constants:
4.184 Joules = 1 calorie. Visible light = 400-700nm. 6.022 x 1023 = 1 mol. h=6.626 x 10-34 J-sec.
C = 2.998 x 108 m/sec. 1012 pm - 1010Ǻ = 109nm = 106μm = 103 mm = 1 m = 10-3 Km = 10-6 Mm = 10-9 Gm
= 10-12 Tm.
In an H atom, the electron jumps from the energy level 3 to energy level 2. It
loses its energy by emitting a photo.
CALCULATE: The energy the electron has before the jump:
___-34.84_____ Kcal/mol = ___-145.8_____ KJ/mol = _-2.421 x 10-19_ Joules.
The energy the electron has after the jump:
___-78.40______ Kcal/mol = __-328.0_____ _ KJ/mol = _-5.447 x 10-19_ Joules.
The energy the photon carries away:
__43.56_______ Kcal/mol = _182.2________ KJ/mol = _3.026 x 10-19_ Joules.
The frequency, υ, of the photon. _4.567 x 1014_/sec.
The wavelength, λ, of the photon; 6.569 x 10-7 m __656.9_nm = __6569_ Ǻngstroms.
Color of this photon. __red / orange___. Show all work on the back of this sheet.
In an H atom, the electron jumps from the energy level 4 to energy level 2. It
loses its energy by emitting a photo.
CALCULATE: The energy the electron has before the jump:
___-19.60_____ Kcal/mol = ___-82.01_____ KJ/mol = -1.362 x 10-19_ Joules.
The energy the electron has after the jump:
___-78.40______ Kcal/mol = __-328.0_____ _ KJ/mol = _-5.447 x 10-19_ Joules.
The energy the photon carries away:
__58.80_______ Kcal/mol = __246.0_______ KJ/mol = _4.085 x 10-19_Joules.
The frequency, υ, of the photon. _6.165 x 1014__/sec.
The wavelength, λ, of the photon; 4.866 x 10-7m = _486.6__nm = __4866__ Ǻngstroms.
Color of this photon. ___indigo_____. Show all work on the back of this sheet.
Constants:
4.184 Joules = 1 calorie. Visible light = 400-700nm. 6.022 x 1023 = 1 mol. h=6.626 x 10-34 J-sec.
C = 2.998 x 108 m/sec. 1012 pm - 1010Ǻ = 109nm = 106μm = 103 mm = 1 m = 10-3 Km = 10-6 Mm = 10-9 Gm
= 10-12 Tm.