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This explanation covers a lot of mid-level chemistry, for those who don't know a lot about it and may need some background.

  • The electrons in an atom are arranged into orbitals, then further divided into sublevels. The order of sublevels is 1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 5s, 4d... The cause of the discrepancy in 4s/3d being reversed is due to electrons in 4s having less energy than those in 3d; it is close, though, so they can easily flip back and forth when excited (the science word for 'given lots more energy').
  • Each type of sublevel holds a fixed maximum amount of electrons: s-levels hold 2, p-levels hold 6, d-levels hold 10 (and f-levels hold fourteen, but that's another unnecessary, unrelated story). The electrons in each sublevel are then "organised" into pairs; one "up" spin, one "down" spin - their spins then cancel (another related, but unnecessary story to that is how iron is magnetic).
  • Now, silicon has 14 electrons while aluminum has 13. Their arrangements are:(for silicon) 1s2, 2s2, 2p6, 3s2, 3p2 and (for aluminum) 1s2, 2s2, 2p6, 3s2, 3p1. Note that aluminum has only one electron in its 3p sublevel and that silicon has two. Because 3p has a maximum size of six, neither is full.
  • When talking about ionisation energies (IEs), we refer to the energy needed to remove an electron only. So for the first IE, we remove one electron from each.
  • The arrangements are now 1s2, 2s2, 2p6, 3s2, 3p1 for silicon and 1s2, 2s2, 2p6, 3s2 for aluminum. Again, note the number in the 3p sublevel: silicon has only one, but aluminum now has zero. Since that sublevel is empty, we go to the next one down, aluminum's 3s.
  • When we do the second IE, we remove a second electron. This is quite easy to do to silicon, because it has only one electron in its valence (outermost) sublevel and it is unpaired. But because aluminum's valence sublevel is now 3s, which is full and has both its electrons paired, we must break up the pair and break up a full sublevel. This takes more energy than just one electron from 3p; so aluminum's second IE is higher than silicon's.
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Does calcium oxide have a higher lattice energy than magnesium oxide?

Yes, calcium oxide has a higher lattice energy than magnesium oxide. This is due to the higher charge of the calcium ion compared to the magnesium ion, leading to stronger electrostatic attraction between the ions in the lattice structure.


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 is the first ionisation energy of magnesium higher than that if sodium?

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.


Which base is stronger Calcium or Aluminum or Magnesium or Sodium?

Calcium is a stronger base compared to Aluminum, Magnesium, and Sodium. This is because it has a higher affinity for accepting a proton (H+) and can release hydroxide ions more readily in solution, making it a stronger base.


What one has a higher mass percent of magnesium MgO or Mg3N2?

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%.

Related Questions

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.


What magnesium oxide has higher boiling point than aluminium oxide?

O.O! That isn't even a REAL word!


Does calcium oxide have a higher lattice energy than magnesium oxide?

Yes, calcium oxide has a higher lattice energy than magnesium oxide. This is due to the higher charge of the calcium ion compared to the magnesium ion, leading to stronger electrostatic attraction between the ions in the lattice structure.


Is ionisation enthalpy of potassium higher than that of sodium?

The ionisation enthalpy of potassium is lower than that of sodium.


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.


Elements with high ionisation energy have?

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


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.


Does aluminium have higher thermal capacity than water?

No, water has a higher specific heat capacity than aluminium. This means water can absorb and store more heat energy per unit mass compared to aluminium before its temperature increases.


Why is the first ionization energy of aluminium is less than the first ionisation energy of silicon?

Al has atomic number 13, and silicon has atomic number 14. The extra electron that silicon has is in a 3p orbital. In simple terms the extra charge on the silicon nucleus contracts the electron shell, this increases the energy to remove an electron and also decreases the atomic radius. Al, first ionization energy 577.5 kJ/mol, atomic radius 125pm Si, first ionization energy 786.3 kJ/mol, atomic radius 110pm


Suggest why aluminium is more expensive than iron?

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.


Why is the first ionisation energy of magnesium higher than that if sodium?

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.


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