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because it has many number of shells.
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.
There are 12 such elements and they are hydrogen, helium, lithium, beryllium, boron, carbon, nitrogen, oxygen, fluorine, neon, sodium and magnesium.
The atomic no of Boron is 5 , so two electrons in ist shell the last three electrons are divided in two sub energy levels two in lower level 's' and one in higher level 'p'
The maximum capacity of electron accommodation in aluminium is 18 electrons( M shell) on contraty it has only 3 valence electrons whereas boron has maximum capacity of 8 electrons(L shell) and it has 3 valence electrons so electron population of Aluminium is less than that of boron.
Because in Boron there is a complete 2s orbital and the increased shielding of the 2s orbital reduces the ionisation energy compared to that seen in Beryllium.
The rise in ionisation energy is not regular. To explain this we must remember that the second shell of electrons is actually subdivided into 2s and 2p. The most easily removed electron in Boron is that in the 2p orbital, higher in energy than the 2s electrons in Beryllium. It therefore needs less energy for total removal than does the 2s electron of Boron. This outweighs the effect of the increased nuclear charge of Boron, which tends to make its outer electron harder to remove.
because it has many number of shells.
Lithium is wayy more reactive... like, duh? An elements reactivity depends on its ionisation energy (the amount of energy required to remove one electron from the atom) and if you look at a periodic table the ionisation energy is known to increase across the table and decrease down it. Berylium is further across the table than lithium so you'd expect it to have a lower ionisation energy and be less reactive. This is because beryllium (atomic number 4) has 4 protons, which cause a positive charge and subsequent attraction of electrons, while lithium has the atomic number 3 and therefore only has 3 protons to attract its electrons. Lithium is a Group I alkali metal, while Beryllium is a Group II alkaline earth metal. Group I Alkali metals are generally more reactive as they only need to lose one electron to have a complete outer shell.
Barium has more energy levels. So it has lesser ionization energy.
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 ionisation enthalpy of potassium is lower than that of sodium.
There are 12 such elements and they are hydrogen, helium, lithium, beryllium, boron, carbon, nitrogen, oxygen, fluorine, neon, sodium and magnesium.
The atomic no of Boron is 5 , so two electrons in ist shell the last three electrons are divided in two sub energy levels two in lower level 's' and one in higher level 'p'
It is about first ionization energy. It is less than alkaline earth metals.
Ionization energy generally increases across a period as a result of a higher nuclear charge, however there are some exceptions such as Boron which has a lower ionization energy than Beryllium (because it is in a P orbital), and Oxygen which has a lower ionization energy than nitrogen (Because ionization decreases the electron electron repulsion in its orbitals).
Because with the 2nd ionisation of K, you are trying to take an electron from a fully filled orbital (octet rule) whereas with calcium it is getting down to a fully filled orbital