What is the minimum frequency of light needed to emit electron from titanium?

Answer 1

I think you need to know the binding energy of the valence electron that is being removed. Looking it up, I find it to be 8.1 electron volts for the 3 d electron (the easiest to remove). Converting this to joules, we have

8.1 eV x 1.60218x10^-19 J/eV = 1.298x10^-18 J

Now, to find the minimum frequency of light needed to remove this electron, it will be equal to the binding energy. E = hν where E = energy = 1.298x10^-18J, h = Plancks Constant = 6.626x10^-32 Js and ν = frequency

Solving for frequency we have....

ν = E/h = 1.298x10^-18 J/6.626x10^-32 Js = 1.959x10¹⁴ s-1 = 1.96x10¹⁴ Hz