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Why are the first ionisation energies of sulfur and aluminium lower than those of phosphorus and magnesium?
Wiki User
∙ 13y ago
Well between Magnesium and Aluminium there is a change in sub-shells as the outer most electron in Aluminium is within the p-shell, where as the Magnesium is within the s-shell . This means the electron within Aluminium is further away from the nucleus, in addition there is more shielding involved. Consequently the electron needs less energy to force it away
phosphorus and sulphur and are in the same shell , however sulphur contains a extra electron to phosphorus. This extra electron is paired with another electron which in turn as the both are negatively charge repel each other , making it easier to force the electron out
:)
Wiki User
∙ 13y ago
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What factors need to be considered when predicting the trend in ionisation energies across a period?
The charge on the nucleus.The distance of the electron from the nucleus.The number of electrons between the outer electrons and the nucleus.
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.
Is it going to be easier for a magnesium atom to gain or lose electrons?
Magnesium is a metal, and metals lose electrons to form positive ions. Magensium (Mg) will lose two electrons, which means its first and second ionization energies are relatively low compared to its third ionization energy.
What is concept of hybridization?
hybridization is defined as the intermixing of different orbitals with different energies to form a new set of orbitals with equivalent energies and shapes
The mixing of two or more atomic orbitals of similar energies on the same atom to produce new orbitals of equal energies is called?
hybridization
Has largerst ionization energy in its period?
Ionisation energies GENERALLY increase across a period. As a result, the noble elements (i.e. Group 0 elements) usually have the highest ionisation energies, as they are highly stable.
First ionisation energies of alkaline earth metals are higher than those of alkali metals?
Yes, they are.
Why are alkali metals highly responsive?
The have only one electron in the valency shell and low ionisation energies which allow them to become highly reactive cations.
What is the relationship between ionization energy and the alkali metals?
There is no relation ship. They have the lowest ionization energies.
What factors need to be considered when predicting the trend in ionisation energies across a period?
The charge on the nucleus.The distance of the electron from the nucleus.The number of electrons between the outer electrons and the nucleus.
What atoms have the smallest values for the first ionisation energies?
I do believe, if my memory serves me correctly, that it is the elements in the first column.... they have only one atom on the outer shell, so it is less full.
What are some properties of metalliods?
They are nonmetallic With intermediate ionisation energies EN values around 2 Form poly metric oxides that are mostly amphoteric Form covalent chlorides form covalent hydride's
When alkali metals lose electrons they achieve an inert gas configuration where all their shells are full. Why aren't their ionization energies zero?
Because they need the ionisation energy to lose the electron in the first place.
Is ionization energy generally uniform?
No, ionisation energies change depending on which element you look at and which ionisation (i.e. 1st, 2nd, 3rd...) you are taking about. For example, as you go across period 3, the 1st ionisation energy generally increases. - sodium (Na) has the lowest I.E.* as it has the lowest nuclear charge *[actual value is 494 KJ/mol ] - magnesium (Mg) has a higher I.E.* than sodium as it has a higher nuclear charge *[actual value 736KJ/mol] - Aluminium drops* below Mg but still higher than Na, this is because although the nuclear charge is greater the 1st electron is being taken from the 3P orbital as opposed to the 3S orbital. This means that the electrons distance from the nucleus is further (so lower attraction). *[actual value 577KJ/mol] The trend increases from there except from Si to Cl [1060 to 1000KJ/mol], but I think you get the idea. The I.E. is dependant on 1. Shielding 2. Distance from the nucleus 3. Nuclear charge
Is the ionization energy of alkali metals larger or smaller than the alkaline earth metals in the same period?
It is about first ionization energy. It is less than alkaline earth metals.
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.
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.
