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Answered 2011-04-17 03:41:19

About twice as large, which is not that much at the first ionization level. Still, Magnesium has a slightly larger, one proton nucleus and one more electron in that valence level to add to the energy needed to pill the first electron out of it's orbital. Electron shielding may have something to do with this also as the other valance electron of this 2+ element may shield the pulled electron.

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a magnesium atom is smaller because it has a higher first ionisation energy and therefor holds its electrons more tightly .


bcz as we move frm left to ryt in a period ionisatn enrgy increase n moreovr charge on magnesium is higer thn thaat of sodium so its ionisatn enrgy is higher...


Ionisation energy of elements increases across periods.The ionisation energy of metals is the lowest as metal elements has a low electronegativity which means it tend to lose it's electrons easily.Ionisation energy increases in such a trend :Metals Therefore comparing sodium ( Na ) and copper (Cu), Cu is more on the right side of the periodic table, causing it to have a high ionisation energy.


The ionisation enthalpy of potassium is lower than that 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


First ionization energy of sodium is 495,8 kJ/mol.First ionization energy of potassium is 418,8 kJ/mol.



Take Sodium for an example: The first ionisation energy for sodium is small, while the second is very large. The electron arrangement for Sodium is 2)8)1) so the first ionisation energy removes the first outer electron leaving a stable electron arrangement of 2)8). The electrons are now closer to the nucleus so the attraction is larger, increasing the energy needed to take another electron away. Because there is one less electron, this will mean an increase in nuclear attraction for the remaining electrons.


Sodium has a lower ionization energy, meaning it takes less energy to remove the valence electrons. Magnesium has higher electronegativity, which is a relative scale for the attraction of electrons, meaning sodium is less likely to gain them. Sodium also has a greater atomic radius, so the negative electrons being removed are farther from the positively charged nucleus than those of magnesium.


The second ionization energy of sodium is so much greater than the first because the first electron is removed from the valence shell, while the second electron is removed from the core orbitals. Additionally, the sodium atom has a positive charge after the first ionization, which thus attracts the remaining electrons more strongly. Both of these factors lead to a much higher second ionization energy compared to the first.


Because with increase in number of electrons the attraction of electrons towards nucleus increases hence the size of magnesium is less than that of sodium.



Down a group, the ionisation energy decreases, electropositivity increases. Hence potassium is more reactive than sodium.


A magnesium ion will be smaller because there will be a greater Zeff on the electrons in the magnesium ion due to a greater number of protons in the nucleus.


Magnesium chloride(MgCl2 ) is a salt of magnesium. Sodium chloride(NaCl) is a salt of sodium.


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.


The ionization energy of lithium is a bit greater than the ionization energy of sodium. Sodium is more reactive.


The ionization energy of sodium is greater than the ionization energy of potassium.


The ionization energy of lithium is a bit greater than the ionization energy of sodium.


When sodium undergoes a reaction it loses one electron to form the Na+ ion. When magnesium reacts it forms the Mg2+ ion. It takes more energy to remove two electrons that it does to removed one. Additionally, there is a greater positive charge on magnesium's nucleus than in sodium, and since the two elements have the same degree of electron shielding, there is a greater degree of attraction between the valence electrons and the nucleus.


Mixture of sodium carbonate and magnesium


Sodium is more reactive than magnesium.


Na(g) --> Na+(g) + e- First ionisation energy is always: X(g) --> X+(g) + e- with X being an element


MgCI+ NaC ------> MgC + NaCI Magnesium chloride + Sodium carbinate ------> Magnesium carbonate + Sodium chloride.


nothing because magnesium is not as reactive as sodium



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