Question

Write the electron configurations for the following atoms. Enter full electron configuration in order electrons fill the subshells. Enter subshells in parentheses followed by numbers of electrons in the exponent. For example you should enter "(1s)²(2s)²(2p)⁵" for atom of fluorine. The answer is case sensitive.

As, Cl, Ni, Si

Calculate the energy in joules of a photon of green light having a wavelength of 537 nm. Report your result to three significant figures.

What is the letter code for a subshell with (a) ℓ = 1 (b) ℓ = 3?

In New York City, radio station WCBS broadcasts its FM signal at a frequency of 101.1 megahertz (MHz). What is the wavelength of this signal in meters?

In the spectrum of a specific element, there is a line with a wavelength of 434 nm. Use the Rydberg equation to calculate the value of n for the higher energy Bohr orbit involved in the emission of this light. Assume the value for the lower energy orbit equals 2.

Answer 1

1) As --->1s² < 2s² < 2p⁶ < 3s² < 3p⁶ < 4s² < 3d¹⁰ < 4p³

Cl --> 1s² < 2s² < 2p⁶ < 3s² < 3p⁵

Ni ---> 1s² < 2s² < 2p⁶ < 3s² < 3p⁶ < 4s² < 3d⁸

Si ---> 1s² < 2s² < 2p⁶ < 3s² < 3p²

2) Energy = Planck's constant*velocity of light/wavelength = (6.63*10^-34)*(3*10⁸)/(537*10^-9) = 3.704*10^-19 J

3) l=1 is p-subshell and l=3 is f-sbhell

4) wavelength = velocity of light/frequency = (3*10⁸)/(101.1*10⁶) = 2.967m