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.
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.
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.
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.
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.
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%.
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.
O.O! That isn't even a REAL word!
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.
The ionisation enthalpy of potassium is lower than that of sodium.
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.
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
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.
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.
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
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.
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.
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