ionization potential energy.
but remember the atom must be neutral .
The energy required to remove an electron from an atom is called ionization energy.
The ionization energy, expressed in kJ/mol.
first ionization energy
Ionisation energy
Ionization energy.
second ionization energy
This is called ionization energy.
magnesium has a 2 valence electrons. because the third electron is not a valence electron, or in the outer shell, much more energy would be needed to remove it
Ionization energy is the energy needed to remove 1 mole of loosely bonded electrons from one mole of atoms or ions.
as you go down a group the elements become more metallic. why? ionization energy decreases. ionization energy is the amount of energy needed to remove the most loosely held electrons. when electrons are lost, a metal is formed. so as you go down a group, the electrons are futher away from the nuclear pull (because the period increases). therefore, not much energy is needed to remove the electrons making it easier to loose them
Briefly, it is the energy required to completely remove a valence (outer shell) electron from its atom when forming an ionic bond.See related links below for more info
This is called the ionization energy and an is different for each electron in the atom. Electrons in the outer shell (furthest from the nucleus) have the lowest ionization energy, electrons in the innermost shell (closest to the nucleus) have the highest ionization energy.
the bottom of the Periodic Table. why? a metal looses electrons and at the bottom of the periodic table is the lowest amount of ionization energy (the energy needed to remove electrons) with low ionization energy, not much energy is needed to remove those electrons making it faster and easier to do so.
There is an attraction of the nucleus for electrons. This attractive force must be overcome to remove an electron. The energy to overcome this attraction and remove an electron from the atom is 'ionization energy'.
Ionization energy
magnesium has a 2 valence electrons. because the third electron is not a valence electron, or in the outer shell, much more energy would be needed to remove it
The energy needed to remove an electron from an atom (in the gaseous state) is called the IONIZATION ENERGY.
Ionization energy is the energy needed to remove 1 mole of loosely bonded electrons from one mole of atoms or ions.
bond energy
as you go down a group the elements become more metallic. why? ionization energy decreases. ionization energy is the amount of energy needed to remove the most loosely held electrons. when electrons are lost, a metal is formed. so as you go down a group, the electrons are futher away from the nuclear pull (because the period increases). therefore, not much energy is needed to remove the electrons making it easier to loose them
the nucleous is positively charged , the electron is negatively charged..the closer to the nucleous an electron is the strongest is the force that attracts it (the force of the nucleous) so more energy is needed to remove it
Briefly, it is the energy required to completely remove a valence (outer shell) electron from its atom when forming an ionic bond.See related links below for more info
This is the second ionization energy.
This is called the ionization energy and an is different for each electron in the atom. Electrons in the outer shell (furthest from the nucleus) have the lowest ionization energy, electrons in the innermost shell (closest to the nucleus) have the highest ionization energy.