The amount of energy necessary to remove an electron from an atom is a quantity called the ionization energy, Ej. This energy can be measured by a technique called photoelectron spectroscopy, in which light of wavelength Iv is directed at an atom, causing an electron to be ejected. The kinetic energy of the ejected electron (Ek) is measured by determining its velocity, v (Ek= mv2/2), and Ei is calculated using the conservation of energy principle. That is, the energy of the incident light is equal to Ej plus Ek. What is the ionization energy of selenium atoms (in kilojoules per mole) if light with wavelength = 48.2 nm produces electrons with a velocity of 2.37l x 10e6 m/s? The mass, m, of an electron is 9.109 x 10e-31 kg. (Remember 1 Joule= 1 kgm2/s2)
- What is the overall trend that we observe in the graph for the ionization energy vs atomic number graph, in a sentence?
- Which subshell contains the electrons with the lowest ionization energy?
- How to guess ionization energy?
- Consider the isoelectronic series Sc^3+ , Ti^4+ , V^5+ , Cr^6+ In order of: a) incr. atomic or ionic radius b) incr. ionization energy?
- Which element (larger than atomic number 36) has the largest first ionization energy and what is the approximate value?