Helium has 2 electrons in the 1s orbital, meaning that these electrons are as close to the nucleus as possible. The nucleus has a positive charge, pulling these negative electrons very tightly. It takes a lot of energy to break this attraction. Having 2 electrons in the 1s orbital also means that it is very stable. Other elements with full outer shells or with electrons in other orbitals having a smaller first ionisation energy than Helium. This is because the electrons in previous orbitals shield the valence (outer) electrons, so the charge of the nucleus isn't felt as much, and is therefore easier to break the attraction.
Helium has 2 electrons in the 1s orbital, meaning that these electrons are as close to the nucleus as possible. The nucleus has a positive charge, pulling these negative electrons very tightly. It takes a lot of energy to break this attraction. Having 2 electrons in the 1s orbital also means that it is very stable. Other elements with full outer shells or with electrons in other orbitals having a smaller first ionisation energy than Helium. This is because the electrons in previous orbitals shield the valence (outer) electrons, so the charge of the nucleus isn't felt as much, and is therefore easier to break the attraction.
He = 1s2, so all its electrons are in the 1s orbital. This means they are all very close to the positively charged nucleus and will be highly attracted to it. This also means that there isn't any shielding from other orbitals, so it willtake a huge amount of energy to pull an electron from it
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Helium has 2 electrons in the 1s orbital, meaning that these electrons are as close to the nucleus as possible. The nucleus has a positive charge, pulling these negative electrons very tightly. It takes a lot of energy to break this attraction. Having 2 electrons in the 1s orbital also means that it is very stable. Other elements with full outer shells or with electrons in other orbitals having a smaller first ionisation energy than Helium. This is because the electrons in previous orbitals shield the valence (outer) electrons, so the charge of the nucleus isn't felt as much, and is therefore easier to break the attraction.
Helium has a structure of 1s2 therefore has a completely filled outermost shell making it very stable. the electron that needs to be remove is very close to the nucleus and does not feel any shielding effect. there are also 2 protons attracting the negative electrons. this makes helium has the largest ionisation energy of all the atoms.
Helium has completely filled valence electrons and has stable electronic configuration. So it will not lose electrons and will have high ionisation energy.
noble gases have the maximum ionisation energy. helium has the highest ionisation energy
Helium
it would have to lose an electron to become an ion as it allredy has a full outershell, for every electron lost the He will gain a charge of +1, but this would be very difficult to obtain as its ionisation energy is very high, in the periodic table ionisation enerygy goes up as you go across the period (from left to right the amount of nuclear charge increases) and it also goes up as you go up a group (as you go up a group the amount of inner sheilding ans distance between outer electron and nucleus decreses, increasing nuclear charge and decreasing shielding and distance all increase ionisation energy) and He is right in the top right corner, Helium has the highest first ionisation energy (ionisation energy is the amount of energy needed to remove one electron from each atom in 1 mole of an element in an gaseous state). the charge of its ion will completely depend on how many electrons it has lost.
ionisation energy order for gr 14 is c>si>ge>sn<pb
Helium has the highest ionization energy.
noble gases have the maximum ionisation energy. helium has the highest ionisation energy
Helium
Helium has the greatest ionization energy. Its electron is being removed from the principal shell closest to the nucleus. It has a greater I.E. than hydrogen does because the electron is being pulled away from a greater nuclear charge.
Helium has the highest ionisation energy of all the elements. It takes 23779kJ to remove only one electron from 1 mol or 4.003g of helium. Trying to ionise 1 gram or 6.193L of Helium is the same as boiling around 75 850L of water Helium has a very high ionisation energy because its atomic radius is very small which causes the force of attractiion between the nucleus and the electrons to be very strong.
Nitrogen has the highest first Ionization potential.
The ionisation energy depends on the orbital from which the electron is removed and also the distance of the orbital from the nucleus. In the case of Helium, the electron is removed from 1s orbital whereas in the case of argon it is from 3p orbital. As 1s is closer to the nucleus, the force of attraction experience by these electrons is higher and hence helium will have higher 1st ionisation energy.
Helium has the highest ionization energy.
Helium (He) has the highest first ionization energy. Ionization energy increase as you go across the periodic table from left to right
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ionisation energy order for gr 14 is c>si>ge>sn<pb
it would have to lose an electron to become an ion as it allredy has a full outershell, for every electron lost the He will gain a charge of +1, but this would be very difficult to obtain as its ionisation energy is very high, in the periodic table ionisation enerygy goes up as you go across the period (from left to right the amount of nuclear charge increases) and it also goes up as you go up a group (as you go up a group the amount of inner sheilding ans distance between outer electron and nucleus decreses, increasing nuclear charge and decreasing shielding and distance all increase ionisation energy) and He is right in the top right corner, Helium has the highest first ionisation energy (ionisation energy is the amount of energy needed to remove one electron from each atom in 1 mole of an element in an gaseous state). the charge of its ion will completely depend on how many electrons it has lost.
Helium (He) has the highest ionization energy.