Ahydrogen atom requires a minimum energy of 2.18×10^-18 j atom to remove an electron from its ground state level. determine whether a blueviolet light with a wavelength of 434.0 nm can affect this process.

Just find the energy of the blueviolet light with a wavelength of 434.0 nm using the formula:

E  = hc / lambda

E = energy
c= speed of light =  3 x 10^8 m/s
h = planck's constant =  6.6 x 10^{-34}  m^2 kg / s
lambda =  434 nm =  434 x 10^{-9} m

Putting these values (with appropriate units) in the above formula :

we get:  Energy, E = 4.5 x 10^{-19} J

E = 0.45 x 10^{-18} J

Now, the minimum energy is 2.18×10^-{18} J but our energy is 0.45 x 10^{-18} J which is less.
Means the electron will not be removed

☆ionisation energy increases across a period from na -> ar☆ionisation energy decreases down a group from li -> fr☆ionic radius decreases across a period from na -> cl☆ionic radius increases down a groupfrom f -> ii hope it clarifies your doubts