Drawing Bohr Model

How do you set a pattern Bohr model showing the energy levels of spectroscopic transitions visible.

Read this before starting. Otherwise, you might be able to start again after something that is not clear, then it is too frustrating.

You draw seven (7) short horizontal lines (each about 5 cm should be allowed). The lines are drawn directly below one another so that they form a kind of block of the tower (without sides). The bottom line will be marked by one (1), the second line with (2), the second line with (3) .... up to the number (6), then the top line is marked (to infinity - make the next 8 Symbol if known). The spacing between the lines - they are not accurate (to scale) spacing, but give the right idea. Between line1 (the bottom line and line 2, a vacuum of about 4 cm, between 2 and 3, a difference of 3 cm, 3-4, 2 cm, 4-5, 1 cm, 5-6; 1cm (you have to be a bit less but it does not make much difference here), and 6-7, about 2 cm. Remember the line 6 is the 6 to 7 line number is infinite. All lines you do not have to worry about are packed into the space between these two. You're not going to bother with them because no transitions from or between one of these lines emit photons with frequency (ie energy) that we perceive as visible.

Now I cm along the line 3, draw a line 3 cm at right angles to the line 3, down to answer line 2.

You just draw a representation of the hydrogen alpha line, using the Bohr model of the atom. Line 3 is the third energy level has one electron in a hydrogen atom may live. The electron is said to be happy - it has potential energy that can lose. And he does it "fall" back to level 2 and in the process of getting rid of some of them giving the excitation energy to a photon - photon that appears red to us, the line alpha hydrogen for astronomers, the first line of Balmer rest of us. The electron can fall all the way back to a line, but then the photon would have more energy, have a higher frequency, we could not see it because of the photon and its ultra-violet.

Return to your diagram. half a cm to the right of the vertical line you have drawn, put a second vertical line of the line 4 to line 2. This is the second line Balmer (its green). Line 3 is derived from level 5 to level 2 (its blue) and line 4 is level 6 to level 2 (its purple)
She did. There are only 4 transitions in the Bohr model of the hydrogen atom to radiate visible photons. Each pass of all levels up to 1 (also called the state of the soil ") will radiate UV. Any transition leading to a higher level 6 to level 2 will also emit UV. Any transition leading to a low level 3 will radiate in the infrared.

When Balmer came with his remarkable formula linking the wavelengths of visible four lines he used the formula to predict the wavelengths of UV photons invisible. Nobody had realized that they were present, but photographic evidence was found soon. Using Science for prediction. When it works its great.