Because aluminum has 3 electrons in its valence shell and when you get to the 3rd ionization energy it has an empty valence shell with a configuration as the noble gas Neon. Aluminum wants to stay at this state and will take a lot of energy to loose another electron from next energy level.
This explanation covers a lot of mid-level chemistry, for those who don't know a lot about it and may need some background.
Removing the third electron from magnesium, or the fourth electron from aluminium, means removing an electron from a filled shell. This is much more difficult than removing an electron from an unfilled shell.
The second ionization energy of calcium is higher than its first ionization energy. You are, after all, removing an electron from a positively charged ion; however, the Ca+ ion does not have a noble gas configuration, so it easily loses a second electron to achieve one. If you were to look up calcium's 3rd ionization energy, you would find it to be tremendously higher than the second, just as potassium's second ionization energy is much higher than its first.
As silicons electrons pair up in the 3s orbital hence there is mutual repulsion between electrons and the 2nd ionisation energy is lowered.
Magnesium has higher 3rd ionisation energy. It is difficult to remove 3rd electron from completely filled orbit.
Just for the lol's.
Cao or CaS have a higher lattice energy
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.
Magnesium nitride (Mg3N2) has a higher percentage composition of magnesium than magnesium oxide (MgO) does. The percentage composition of magnesium in magnesium nitride is 72.2% and the percentage composition of magnesium in magnesium oxide is 60.3%.
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.
Phosphorus has a higher energy level so it pulls harder on its electrons.
During a chemical reaction, Magnesium can replace Aluminum due to a higher activity level.
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
O.O! That isn't even a REAL word!
The ionisation energy depends on the orbital from which the electron is removed and also the distance of the orbital from the nucleus. In the case of Helium, the electron is removed from 1s orbital whereas in the case of argon it is from 3p orbital. As 1s is closer to the nucleus, the force of attraction experience by these electrons is higher and hence helium will have higher 1st ionisation energy.
Cao or CaS have a higher lattice energy
The ionisation enthalpy of potassium is lower than that of sodium.
1.A small atomic/ionic radius 2.therefore less number of protons 3. more net nuclear attraction between the positively charged nucleus 4. higher energy is needed to break those bonds. 5. therefore an element has high ionisation energy
Aluminium is more expensive than iron because of its lower abundance in the Earth's crust. It is also more costly to extract and refine aluminium due to the energy-intensive process of electrolysis. Additionally, aluminium has a higher demand and is used in a wide range of industries which further contributes to its higher price.
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
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.
Bromine has less valence shells than lead making the distance between its valence electron and its nucleus less than that of lead. This means that there is greater attraction between the nucleus and electron for bromine and it requires a higher ionisation energy to remove its electron.
Magnesium nitride (Mg3N2) has a higher percentage composition of magnesium than magnesium oxide (MgO) does. The percentage composition of magnesium in magnesium nitride is 72.2% and the percentage composition of magnesium in magnesium oxide is 60.3%.