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Why is the first ionisation energy of magnesium higher than that if sodium?
Wiki User
∙ 12y ago
It has to do with the VSEPR model for electron shell configurations. Zinc being the final transition metal in the 4th row of the Periodic Table has a full "D" shell of valance electrons. Gallium being the following element in the 4th row now has one valence electron in the "P" shell which is not full. An element with a full valence shell of whatever type will have a higher first ionization energy then an element with a shell that is not full.
Wiki User
∙ 15y ago
Wiki User
∙ 12y agobcz 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...
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Why is it easier to remove an electron from a sodium atom than from a magnesium atom?
Phosphorus has a higher energy level so it pulls harder on its electrons.
Why is the ionistaion energy of magnesium higher than that of sodium?
because ionization energy increases from left to right on the periodic table. Ionization energy is the amount of energy needed to take an electron away from the atom, or the energy needed to ionize it. Since Sodium is more likely to give up an ion to complete the octet rule, it has a higher ionization energy.
Why Magnesium metal is a better conductor than Sodium metal?
Because there are a higher amount of delocalised electrons.
What is the equation of magnesium nitrate with an excess of sodium phosphate to make sodium nitrate and magnesium phosphate.?
no reaction
Sodium is more or less active than magnesium?
Sodium is more reactive then Magnesium as it is a group 1 element and magnesium is a group 2 element
Is ionisation enthalpy of potassium higher than that of sodium?
The ionisation enthalpy of potassium is lower than that of sodium.
Is the ionisation energy of sodium same as chlorine?
No
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 are the ionisation enthalpies of potassium and sodium?
First ionization energy of sodium is 495,8 kJ/mol.First ionization energy of potassium is 418,8 kJ/mol.
Why is it easier to remove an electron from a sodium atom than from a magnesium atom?
Phosphorus has a higher energy level so it pulls harder on its electrons.
Which substance sodium oxide or magnesium oxide has higher melting point?
sodium oxide: 1132oC magnesium oxide: 2852oC
Which of the elements sodium calcium potassium and magnesium has the smallest first ionization energy?
Sodium
Why is the ionistaion energy of magnesium higher than that of sodium?
because ionization energy increases from left to right on the periodic table. Ionization energy is the amount of energy needed to take an electron away from the atom, or the energy needed to ionize it. Since Sodium is more likely to give up an ion to complete the octet rule, it has a higher ionization energy.
Why lithium has exothermic heat of solution whereas chlorides of sodium have endothermic heat of solution?
lithium have low ionisation energy.
Why Magnesium metal is a better conductor than Sodium metal?
Because there are a higher amount of delocalised electrons.
What is the first ionization energy for sodium?
Na(g) --> Na+(g) + e- First ionisation energy is always: X(g) --> X+(g) + e- with X being an element
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
