0
Why does first ionisation enthalpy would have higher electron gain enthalpy?
Wiki User
∙ 6y agoWant this question answered?
Be notified when an answer is posted
Add your answer:
Earn +20 pts
Would you expect the first ionisation enthalpy for two isotopes of the same element to be same or different?
This value is identical for isotopes.
Would you expect the second electron gain enthalpy of O as positive more negative or less negative than the first Justify your answer?
The second electron gain of an oxygen atom would be expected to be less negative. The reason for this outcome is that the oxygen atom gaining a second electron already has one electron and thus a negative charge. This negative charge repels the second electron to some extent, making the enthalpy of this process less negative than when the first electron was added to the neutral oxygen atom.
Why are the ionisation energy of isotopes the same?
no the same,first ionisation contains a slightly differences in isotopes
What is the ionic charge of 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.
Why is the first ionisation energy of hydrogen and oxygen the same?
The outer valence electron lies in a 1s orbital in Hydrogen. The effective nuclear charge of hydrogen can be taken as Z = 1. The electron that is being ionised in Oxygen lies in a 2p orbital which has an effective nuclear charge of Z = 8-(3.4 or 4.5 or something). The point is, this nuclear charge at a greater distance from the nucleus means the energies of the electrons are similar and so ionisation energis required are too similar.
Would you expect the first ionisation enthalpy for two isotopes of the same element to be same or different?
This value is identical for isotopes.
Why does helium has a higher first ionization energy than argon?
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.
What is ionisation energy What is first ionisation energy?
The first ionization energy of an atom or molecule describes the amount of energy required to remove an electron from the atom or molecule in the gaseous state.
First ionisation energies of alkaline earth metals are higher than those of alkali metals?
Yes, they are.
Why the first ionisation energy of O is less than that of N?
oxygen is more electronegative and so it wants the electron more than N
Would you expect the second electron gain enthalpy of O as positive more negative or less negative than the first Justify your answer?
The second electron gain of an oxygen atom would be expected to be less negative. The reason for this outcome is that the oxygen atom gaining a second electron already has one electron and thus a negative charge. This negative charge repels the second electron to some extent, making the enthalpy of this process less negative than when the first electron was added to the neutral oxygen atom.
Why second ionisation energy is larger than the first ionisation energy?
The reason the second ionization energy is higher than the first relates to the attraction between the electrons and the nucleus. When one electron is removed from an atom, the neutral atom becomes positive. When one attempts to remove a second electron from a positive ion, there is more attraction between the electrons and the nucleus due to the extra proton. Thus, the second electron is harder to remove and the ionization requires more energy.
Why the first ionisation energy of potassium is only a little less than the ionisation energy of sodium?
both are in the same period which accounts for closeness. they are nonetheless different because there are more protons in the nucleus which means electrons are brought closer to it so there is a higher ionisation energy or potential
What is meant by the first ionisation energy of nitrogen?
THis is the energy required to remove(ionise) one (the first) outer most electron. For nitrogen this would be quite a large figure, because nitrogen, wants to accept electrons ,rather than remove electrons. As a general rule as you go along any given period, the ionisation energies increase. There are two 'humps', with a slight fall in ionisation energiers in this general increase.
How would you explain the fact that the first ionization enthalpy of sodium is lower than that of magnesium but its second ionization enthalpy is higher than that of magnesium?
Sodium has only one valence electron, and when that is donated to some other atom, the remaining ion has a noble gas configuration that is highly stable. Disrupting that by another ionization requires much energy. Magnesium has two valence electrons; therefore the second is almost as easy to donate as the first. The third ionization enthalpy of magnesium would be very high.
Why are the ionisation energy of isotopes the same?
no the same,first ionisation contains a slightly differences in isotopes
Why is the first ionisation energy of strontium larger than the first ionisation energy of rubidium?
Because, as we know that when we go across the period of the periodic table, the number of shells remain the same but the number of electrons and protons increases. So, Rb having its atomic number as 37 and Sr as 38, Strontium has got more nuclear charge as well as more electrons. As a result the first ionisation energy required to remove one electron is more in Strontium than Rubidium.
