Question

Below is the energy level diagram (not drawn to scale) representing the transitions made by an electron in a hydrogen atom that result in the observed lines of both the absorption and emission spectra. Some are in the visible region, and some are not.

4 different energy photons are represented (approximate wavelengths are given in parentheses):

infrared (~ 10e-4 m)

red (~ 10e-6 m)

blue (~ 10e-7 m)

ultraviolet (~ 10e-8 m)


Match the transition (a - h) with the photon described (approximate wavelengths are given in parentheses.) Your answer input should be a single, lower case letter.

(Please note: This is not a problem for which a calculator is required. Your knowledge of the Bohr model of the atom and the relative energies of transitions is all that is needed.)

Smallest energy emission

Answer 1

Answer:

x² + 7x + 10 is the required polynomial.

Explanation :

According to the Question

It is given that α and β are the zeroes of a polynomial .

Sum of zeros (α+β) = -7

Product of Zeros (αβ) = 10

we need to calculate the polynomial.

As we know that if the sum of zeros and product of zeros are given we can easily calculate the polynomial .

Let the Polynomial be P(x)

• P(x) = x²-(sum of zeros)x + (product of

Answer 2

Answer:

na wnskshs suskcvksoq w