Consider the following energy levels of a hypothetical atom: e4 −1.21 × 10−19 j e3 −5.71 × 10−19 j e2 −1.05 × 10−18 j e1 −1.55 × 10−18 j (a) what is the wavelength of the photon needed to excite an electron from e1 to e4? (b) what is the energy (in joules) a photon must have in order to excite an electron from e2 to e3? (c) when an electron drops from the e3 level to the e1 level, the atom is said to undergo emission. calculate the wavelength of the photon emitted in this process.

Explanation:

Energy levels of a hypothetical atom:

a) Wavelength of the photon needed to excite an electron from to .

Energy difference  between forth and first energy level =

139.2 nm is the wavelength of the photon needed to excite an electron from to .

b) Energy of a photon in order to excite an electron from to .

Energy difference between third and second energy level =

is the energy a photon to excite an electron from to .

c) Electron drops from the level to the level

Energy difference between third and first energy level =

202.3 nm is the wavelength of the photon of emitted.

explanation:

crosscutting concepts have application across all domains of science. as such, they are a way of linking the different domains of science. they include patterns; cause and effect; scale, proportion, and quantity; systems and system models; energy and matter; structure and function; and stability and change.

the ideal gas law equation is as follows

pv = nrt

where p - pressure

v - volume

n - number of moles

r - universal gas constant

t - temperature

so if the pressure, volume and temperature are already known

we are left with n and r

since r is the universal gas constant that has a known fixed value then r too is known

so we are left with 'n'

once we know temperature volume and pressure

we can find the number of moles of gas present using the ideal gas law equation

this is not my own answer, this is an answer for the same question by the user blahblahmali. i do not claim ownership of this account.