1008.4 kJ mol-1
In their outer electron shell, halogens have 7 valence electrons, one less than the number needed for a full shell. Therefore, it is much, much easier for the halogen to gain an electron in bonding than for it to lose 7 - the ionization energy (energy required to remove an electron from an atom) is quite high.
In their outer electron shell, halogens have 7 valence electrons, one less than the number needed for a full shell. Therefore, it is much, much easier for the halogen to gain an electron in bonding than for it to lose 7 - the ionization energy (energy required to remove an electron from an atom) is quite high.
How much energy is required to move the electron of the hydrogen atom from the 1s to the 2s orbital
The first ionization energy is the energy that is required in order to remove the first electron from an atom in the GAS phase, the second ionization energy is the energy required to remove the second electron from an atom in the GAS phase. Ionization energy will generally increase for every electron that is removed and increases from left to right in the periodic table and moving up the periods.
It releases the same amount of energy that it absorbed when it was excited to a higher energy state.
In their outer electron shell, halogens have 7 valence electrons, one less than the number needed for a full shell. Therefore, it is much, much easier for the halogen to gain an electron in bonding than for it to lose 7 - the ionization energy (energy required to remove an electron from an atom) is quite high.
In their outer electron shell, halogens have 7 valence electrons, one less than the number needed for a full shell. Therefore, it is much, much easier for the halogen to gain an electron in bonding than for it to lose 7 - the ionization energy (energy required to remove an electron from an atom) is quite high.
The energy gaps between levels are not all the same.
How much energy is required to move the electron of the hydrogen atom from the 1s to the 2s orbital
The energy required to ionize a hydrogen atom with an electron in the n4 level is 0.85 electron volts.
The energy to remove 1 electron is the first ionization energy. To remove a second electron requires more energy. This is because the electron being removed now has to overcome the +1 positive charge introduced after the 1st electron was removed.
The best modern answer would involve quantum chemistry, but an easier to understand explanation is that the outermost electrons in fluorine are much closer to the nucleus that provides the attraction to hold the electrons and nucleus together as an atom than are the outermost electrons in iodine. This is sometimes called the "screening effect" of inner shell electrons that weakens the attraction between the nucleus and the outer shell electrons in large atoms such as iodine.
Elements on the right side of the periodic table require large amounts of energy to remove an electron from the outermost energy level of their atoms. It is much easier for them to gain rather than lose electrons.
ok, so electron affinity is the amount of energy given off when a particular atom excepts electrons. Essentially, it is the likelihood that an atom will accept an electron, while ionization energy is how much energy is needed to take an electron off of a particular atom
A calorie is a measure of energy. It doesn't make sense to ask how much energy you need to lose energy.
How much iodine...
The first ionization energy is the energy that is required in order to remove the first electron from an atom in the GAS phase, the second ionization energy is the energy required to remove the second electron from an atom in the GAS phase. Ionization energy will generally increase for every electron that is removed and increases from left to right in the periodic table and moving up the periods.