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because it has many number of shells.
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∙ 12y ago
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How does low ionisation energy favor the formation of ionic bond?
Ionisation energy is defined as the amount of energy required to remove the most loosley bound or valence electron from an atom. The lower the ionisation energy, the easier it is to remove the electron. Once the electron has been removed, electroneutrality is lost and the atom develops a positive charge and is known as a positively charged ion. Now, an ionic bond is the bond formed between two oppositely charged species. For example, a bond between a positively charges sodium ion and a negatively charged chloride ion. The lower the ionisation energy, the easier it will be for the atom to lose an electron, thereby forming a positively charged species which will be capable of forming an ionic bond with a negatively charged species. Or lower the ionisation energy, the greater is the tendency to form an ionic bond.
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 :)
What is the relationship between ionization energy and the halogens?
The further you are down the halogen group (group 7) the lower the 1st ionisation energy (amount of energy required to remove 1 electron from the atom) is. This is because the electron in question becomes further from the positive charge of the nucleus the more electron shells there are, and electron shielding (the blocking of the effect of the positive charge's attraction) is increased.
What generally happens to the first ionization energy of the element's within a period as the atomic number of the element's increases?
Ar P Al Na K In general the ionisation energy (this answer refers to first ionisation energy, although most of the principles mentioned here apply to all ionisation energies) increases as one moves across the period, this is due to an increasing nuclear charge and decreasing atomic radius (recall that F=(kq1q2)/r2 ). However there are exceptions to this, notably, on moving from group II to group III we see that ionisation energy decreases, like wise on moving from group V to group VI. The first of these decreases is a result of the additional electron occupying the p orbital (and therefore experiencing a lesser effective nuclear charge). The second decrease (which is less marked) is due to the additional electron being "placed" into an orbital already occupied by another electron (an electron pair is formed), these electrons have the same charge and therefore repel each other, as they are in the same orbital the repulsion is particularly strong, therefore the effective nuclear charge is less and first ionisation energy is lower. I hope this answer is acceptable, for more information see the Wikipedia article on electronic configuration.
Explain the increase in pH on progressing from magnesium oxide to barium oxide?
On progression from magnesium oxide to barium oxide, the metal ion has an increasing atom size, with a decreasing ionisation energy and can easily lose one electron to form more the hydroxide ions (or in another point of view leads to lower activation energy and hence faster reaction) this is why there is an increase in pH.
Does Sulfur has a lower ionization energy than chlorine?
no sulfur is practically a gas
How does low ionisation energy favor the formation of ionic bond?
Ionisation energy is defined as the amount of energy required to remove the most loosley bound or valence electron from an atom. The lower the ionisation energy, the easier it is to remove the electron. Once the electron has been removed, electroneutrality is lost and the atom develops a positive charge and is known as a positively charged ion. Now, an ionic bond is the bond formed between two oppositely charged species. For example, a bond between a positively charges sodium ion and a negatively charged chloride ion. The lower the ionisation energy, the easier it will be for the atom to lose an electron, thereby forming a positively charged species which will be capable of forming an ionic bond with a negatively charged species. Or lower the ionisation energy, the greater is the tendency to form an ionic bond.
Is ionisation enthalpy of potassium higher than that of sodium?
The ionisation enthalpy of potassium is lower than that of sodium.
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 :)
Why boron has a lower first-ionization energy than beryllium?
Because in Boron there is a complete 2s orbital and the increased shielding of the 2s orbital reduces the ionisation energy compared to that seen in Beryllium.
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.
Why the second ionization energy of Ca is lower than the second ionization energy of k?
Because with the 2nd ionisation of K, you are trying to take an electron from a fully filled orbital (octet rule) whereas with calcium it is getting down to a fully filled orbital
Why does Ca have a higher ionization energy than Ga?
because it lower than Ba as you go down ionization energy increases
Why metal has lower ionisation energy?
Because the force of attraction between the nucleus and the outer most electron is less. In addition, most metals (but not all) will gain the stable electronic configuration of the nearest noble gas if they lose electron.
Why oxygen have less ionisation enthalpy than fluorine?
Oxygen has a lower electronegativity than fluorine (3.5 as compared to 4).
What is the relationship between ionization energy and the halogens?
The further you are down the halogen group (group 7) the lower the 1st ionisation energy (amount of energy required to remove 1 electron from the atom) is. This is because the electron in question becomes further from the positive charge of the nucleus the more electron shells there are, and electron shielding (the blocking of the effect of the positive charge's attraction) is increased.
What happens to a lant when it doesn't get enough phosphorus?
The production per hectare is lower.
