what is the frequency of light emitted when the electron in a hydrogen atom undergoes a transition from energy level n

Answers

Answer 1

Answer:

Complete question is;

What is the frequency of light emitted when the electron in a hydrogen atom undergoes a transition from energy level n=6 to level n=3?

Answer:

Frequency = 2.742 × 10^(14) s^(-1)

Explanation:

First of all, the energy of hydrogen electron from online values is;

E_n = -2.18 × 10^(-18) × (1/n²) J

n is the principal quantum number

We are told that hydrogen atom undergoes a transition from energy levels n = 3 to n = 6.

Thus, it means we have to find the difference between the electrons energy in the energy levels n = 3 to n = 6.

Thus;

E_n = E_6 - E_3

Thus;

E_n = [-2.18 × 10^(-18) × (1/6²)] - [-2.18 × 10^(-18) × (1/3²)]

E_n = (2.18 × 10^(-18)) × [-1/36 + 1/9]

E_n = 0.1817 × 10^(-18) J

From Planck expression, we can find the frequency. Thus;

E = hf

Where h is Planck's constant = 6.626 × 10^(-34) m²kg/s

Thus;

0.1817 × 10^(-18) = 6.626 × 10^(-34) × f

f = (0.1817 × 10^(-18))/(6.626 × 10^(-34))

f = 2.742 × 10^(14) s^(-1)

Answer 2

Answer:

Final answer:

The frequency of light emitted during an electron transition in a hydrogen atom is determined by calculating the energy difference between the two energy levels and then using this to calculate the frequency using the equation for energy of a photon.

Explanation:

The frequency of light emitted during a transition of an electron in a hydrogen atom can be calculated using the formula for the energy difference (∆E) between two energy levels n1 and n2 in the hydrogen energy level diagram.

The formula to calculate energy difference is: ∆E = E(n2) - E(n1) where E(n) represents the energy of an energy level n. The energy difference ∆E is negative when an electron goes down an energy level (i.e., emits a photon), as the energy level n1 is greater than n2.

The frequency of the emitted photon (∆E) is then given by the formula ∆E = hf where h is Planck's constant (6.63 x 10^-34 Joule seconds) and f is the frequency. Therefore, you can rearrange the equation to find the frequency: f = ∆E / h.

Learn more about Electron Transitions here:

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Answers

Answer:

See the attached file for the structure

Explanation:

See the attached file

6. A sample of nitrogen gas weighs 130 g. Write the chemical formula for nitrogen gas. Howmany molecules of elemental nitrogen is this? How many atoms of nitrogen are in this sample?

Answers

Chemical formula for nitrogen gas is N₂.

To find the number of molecules in the given sample, we have to convert the mass of the sample to moles by using the molecular mass of elemental nitrogen (N₂).

$130gN_2\cdot(1molN_2)/(28gN_2)=4.64molN_2$

Now, we have to use Avogadro's number (6.022x10^23) that indicates the number of molecules in one mole of substance:

$4.64molN_2\cdot(6.022*10^(23)molecules)/(1molN_2)=2.79*10^(24)molecules$

It means that there are 2.79x10^24 molecules of elemental nitrogen.

To find the number of atoms we just have to multiply the number of molecules by 2, which is the number of atoms of nitrogen per molecule of elemental nitrogen:

$2.79*10^(24)molecules\cdot(2atoms)/(1molecule)=5.59*10^(24)atoms$

There are 5.59x10^24 atoms of nitrogen in the sample.

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