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  • First and second ionization energy (video) | Khan Academy
    An element's second ionization energy is the energy required to remove the outermost, or least bound, electron from a 1+ ion of the element Because positive charge binds electrons more strongly, the second ionization energy of an element is always higher than the first
  • Khan Academy
    Learn about first and second ionization energy in this Khan Academy video tutorial
  • Ionization energy: group trend (video) | Khan Academy
    An element's first ionization energy is the energy required to remove the outermost, or least bound, electron from a neutral atom of the element On the periodic table, first ionization energy generally decreases as you move down a group This is because the outermost electron is, on average, farther from the nucleus, meaning it is held less tightly and requires less energy to remove
  • Ionization energy: period trend (video) | Khan Academy
    An element's first ionization energy is the energy required to remove the outermost, or least bound, electron from a neutral atom of the element On the periodic table, first ionization energy generally increases as you move left to right across a period This is due to increasing nuclear charge, which results in the outermost electron being more strongly bound to the nucleus
  • Ionization energy trends | Periodic table (video) | Khan Academy
    Definition of ion and ionization energy, and trends in ionization energy across a period and down a group
  • Ionization energy trends (video) | Khan Academy
    Ionization is the process of removing an electron from a neutral atom (or compound) The energy required to remove an electron is the ionization energy The ionization energy differs for each atom There are trends that match the structure of the periodic table Across a period, ionization energy tends to increase Down a group, the ionization energy tends to decrease
  • Ionisation enthalpies of transition elements - Khan Academy
    The oxidation state of an element is closely related to its ionization enthalpy Ionization enthalpy, also known as ionization energy, is the energy required to remove an electron from an atom or ion in its gaseous state
  • Identifying an element from successive ionization energies (worked . . .
    Since ionization energy is the amount of energy required to remove an electron, a high ionization indicates a difficult to remove electron This tells us the atom resisted losing that fourth electron more so than the first three
  • Identifying an element from successive ionization energies (worked . . .
    When electrons are removed in succession from an element, the transition from removing valence electrons to removing core electrons results in a large jump in ionization energy By looking for this large jump in energy, we can determine how many valence electrons an element has, which in turn can help us identify the element
  • Periodic trends and Coulombs law (video) | Khan Academy
    Periodic trends (such as electronegativity, electron affinity, atomic and ionic radii, and ionization energy) can be understood in terms of Coulomb's law, which is Fₑ = (q₁q₂) r² For example, consider first ionization energy: Coulomb's law tells us that the greater the nuclear charge (q₁) and the shorter the distance between the nucleus and the outermost electron (r), the stronger





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