All categories

2 years ago

If an electron falls from the n = 2 to the n = 1 energy levels in a Hydrogen atom what wavelength of light is emitted?

Chemistry

1 answer:

telo118 [61]2 years ago

6 0

The wavelength is obtained as 122 nm. Option A

<h3>What is the wavelength?</h3>

We know that from the Bohr model of the atom, an electron can move from a higher energy level to a lower energy level or from a lower energy level to a higher energy level. This is the idea of energy quantization as put forward by Neill Bohr.

The wavelength can be obtained by the use of the formula;

1/λ = RH(1/n^2initial - 1/n^2 final)

λ = wavelength of the emitted light

RH = Rydberg's constant

n intial = initial energy level

nfinal = final energy level

Thus;

1/λ = 1.09 * 10^7(1/1^2 - 1/2^2)

1/λ = 1.09 * 10^7( 1 - 0.25)

λ = 122 nm

Learn more about the wavelength:brainly.com/question/13533093

#SPJ1

You might be interested in

Consider the following reversible reaction.

andriy [413]

Answer:

No one is correct. The correct expression is:

Keq = [H₂]² . [O₂]² / [H₂O]²

Explanation:

To build the Keq expression in a chemical equilibrium you must consider the molar concentrations of reactants / products, and they must be elevated to the stoichiometric coefficient.

The balance reaction is:

2 H₂O (g) ⇄ 2 H₂ (g) + O₂ (g)

Keq = [H₂]² . [O₂] / [H₂O]²

In opposite side: 2 H₂ (g) + O₂ (g) ⇄ 2 H₂O (g)

Keq = [H₂O]² / [H₂]² . [O₂]

6 0

4 years ago

When Mendel crossed a plant with green peas and a plant with yellow peas, what color peas did the offspring have?

Alexxandr [17]

Answer:

B. All offspring had yellow peas.

Explanation:

7 0

3 years ago

Part A. At present, automobile batteries are sealed. When lead storage batteries discharge, they produce hydrogen. Suppose the v

kondaur [170]

Answer:

Part A. 10 atm

Part B. C₆H₆

Explanation:

Part A. At present, automobile batteries are sealed. When lead storage batteries discharge, they produce hydrogen. Suppose the void volume in the battery is 100 mL at 1 atm of pressure and 25°C. What would be the pressure increase if 8 × 10⁻² g H₂ were produced by the discharge of the battery?

We can find the pressure for this amount of Hydrogen using the ideal gas equation.

$P.V=n.R.T\\P.V=\frac{m}{M} .R.T\\P=\frac{m.R.T}{M.V} =\frac{8 \times 10^{-2}g \times (0.082atm.L/mol.K) \times 298K }{(2g/mol) \times 0.1L} =10atm$

Part B. A certain compound containing only carbon and hydrogen was found to have a vapor density of 2.550 g/L at 100°C and 760 mmHg. If the empirical formula of this compound is CH, what is the molecular formula of this compound?

First, we have to look for the molar mass of the compound through the following expression:

$P.M=\rho .R.T\\M = \frac{\rho .R.T}{P} =\frac{2.550g/L \times (0.08206atm.l/mol.K) \times 373.15K }{760mmHg} .\frac{760mmHg}{1atm} =78.1g/mol$

Now, we need the relation between the molar mass of the molecular formula and the molar mass of the empirical formula.

$\frac{78.1g/mol}{13.0g/mol} =6.01 \approx 6$

Finnally, we multiply the empirical formula by this coefficient to get the molecular formula.

(CH) × 6 = C₆H₆

5 0

4 years ago

Leona [35]

Explanation:

element symbol is Na

total electrons is 11

valences electron is 1

4 0

4 years ago

Four moles of Argon gas are at a pressure of 1.90 atm, and the temperature is 50 degrees C. What is the volume of the gas?

soldier1979 [14.2K]

N = 4 moles of Ar2, P = 1.90 atm, V = ?
T = 50C = 273 + 50K = 323K
PV = nRT --> V = nRT/P
V = (4)(.0821)(323)/1.90
V = 106.07/ 1.9
V = 55.8 L

4 0

3 years ago