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Why are the first ionisation energies of sulfur and aluminium lower than those of phosphorus and magnesium?
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
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What else can I help you with?
Is magnesium's ionization energy higher or lower than chlorine?
ionization energies of mg is less than chlorine because chlorine requires only one electron to complete its octet so it will not prefer to loose its electron morover its electronegativity is also higher and it is of smaller size than mg so electtron removal is difficult
Why are sodium and magnesium highly reactive?
Sodium and magnesium are highly reactive because they both have low ionization energies, meaning they can easily lose outer shell electrons to form stable cations. This makes them readily combine with other elements to form compounds. Additionally, the resulting compounds are energetically more stable, driving the reaction forward.
What is meant by the first ionisation energy of nitrogen?
The first ionization energy of nitrogen is the energy required to remove one electron from a neutral nitrogen atom to form a positively charged nitrogen ion. It represents the strength of the bond between the electron and the nitrogen atom.
How do the lattice energies of different ionic compounds compare in terms of their stability and bonding strength?
The lattice energies of different ionic compounds vary in terms of their stability and bonding strength. Compounds with higher lattice energies are more stable and have stronger bonding compared to compounds with lower lattice energies.
Is it going to be easier for a magnesium atom to gain or lose electrons?
It is easier for a magnesium atom to lose electrons because it has two electrons in its outer shell, making it more stable to achieve a full outer shell with eight electrons through loss rather than gain.
First ionisation energies of alkaline earth metals are higher than those of alkali metals?
Yes, they are.
Who ionisation energy differs?
Ionisation energy differs between elements due to variations in the number of protons in their nucleus, which affects the strength of the attraction between the electrons and the nucleus. Elements with higher atomic numbers typically have higher ionisation energies due to increased nuclear charge. Additionally, ionisation energy generally increases across a period and decreases down a group on the periodic table.
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.
Has largerst ionization energy in its period?
The element with the largest ionization energy in its period is typically found in the top right corner of the periodic table. This is because elements in this region have the highest effective nuclear charge, making it harder to remove an electron. In general, elements like helium, neon, and fluorine tend to have the highest ionization energies in their respective periods.
Ionisation energy of noble gases?
Noble gases have high ionization energies due to their stable electron configurations and full outer electron shells. This makes it difficult to remove an electron from them compared to other elements. The ionization energy generally increases from helium to radon within the noble gas group due to increasing nuclear charge.
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 atoms have the smallest values for the first ionisation energies?
Helium and hydrogen have the smallest values for the first ionization energies. Helium has the lowest first ionization energy due to its stable electron configuration with a full outer shell, while hydrogen has a low ionization energy because it has only one electron in its outer shell.
What are the two energies?
There are no known "infinite energies" in our real Universe.
