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polet [3.4K]
3 years ago
7

Calculate the energy difference for a transition in the paschen series for a transition from the higher energy shell n=4. expres

s your answer to four significant figures and include the appropriate units.
Chemistry
1 answer:
Troyanec [42]3 years ago
5 0
Electrons are orbiting around the nucleus in a specific energy level as described in Bohr's atomic model. There are 7 energy levels all in all; 1 being the strongest and nearest to the nucleus, and 7 being the weakest and farthest away from the nucleus. Electron can transfer from one energy level to another. If it increases energy, it absorbs energy. If it goes down an energy level, it emits energy in the form of light. This light can be measure in wavelength through the Rydberg equation:

1/λ =R(1/n₁² -1/n₂²), where
λ is the wavelength
R is the Rydberg constant equal to 1.097 × 10⁻7<span> per meter
n</span>₁ and n₂ are the energy levels such that n₂>n₁

In the Paschen series is an emission spectrum of hydrogen when the energy level is at least n=4. So, this covers n=4 to n=7.

1/λ =(1.097 × 10⁻7)(1/4² -1/7²)
λ  = 216.57 ×10⁻⁶ m or 216.57 μm
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Step 1 : convert given masses into moles.

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Moles of B =\frac{\text{ given mass of B}}{\text{ molar mass of B}}= \frac{16.4g}{11g/mole}=1.5moles

Moles of O =\frac{\text{ given mass of O}}{\text{ molar mass of O}}= \frac{48.6g}{16g/mole}=3moles

Step 2 : For the mole ratio, divide each value of moles by the smallest number of moles calculated.

For Na = \frac{1.5}{1.5}=1

For B = \frac{1.5}{1.5}=1

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