Physicsiscool said:Can someone please help me understand the following question?
The ionization energy of the outermost electron in Li is 5.390 eV. What is the effective charge seen by the outermost electron? (Li has 2 energy levels)
Li's outermost electron ionization energy refers to the amount of energy required to remove the outermost electron from a Li atom in its ground state. This energy is measured in units of kilojoules per mole (kJ/mol) and is an important factor in determining the atom's reactivity and chemical properties.
The outermost electron ionization energy of Li is determined experimentally through a process called ionization energy spectroscopy. In this process, a beam of electrons is directed at a sample of Li atoms and the energy required to remove an electron is measured. This process is repeated multiple times to get an average value for Li's outermost electron ionization energy.
Li's outermost electron ionization energy is important because it affects the atom's reactivity and chemical properties. A lower ionization energy means that it is easier for Li to lose an electron and form positive ions, making it more reactive. On the other hand, a higher ionization energy indicates a more stable atom with less tendency to react.
Li's outermost electron ionization energy is relatively low compared to other elements in the periodic table. This is because Li has a larger atomic radius and a lower nuclear charge, making it easier for the outermost electron to be removed. However, Li's ionization energy is higher than that of elements in the same group, such as Na and K, due to the increased shielding effect in larger atoms.
Li's outermost electron ionization energy generally increases with increasing atomic number. This is because as the atomic number increases, the number of protons in the nucleus also increases, resulting in a stronger attraction between the nucleus and the outermost electron. This makes it more difficult to remove the electron, thus increasing the ionization energy.