The first ionization enthalpy of carbon is 1086 KJ Mol would you expect the first ionization enthalpy of SI to Greater or lesser than this amount explain
Si is a larger atom, the outside electron is farther away from the nucleus so it should be easier to remove it.
Well, SI stands for Silicon, not Superman's secret identity, in case you were confused. Now, let's talk about ionization enthalpy. Silicon is below carbon in the periodic table, which means it has an extra electron shell. This additional shell shields the outermost electrons from the positive charge of the nucleus, making it easier to remove an electron from silicon. So, logically speaking, you would expect the first ionization enthalpy of silicon to be lesser than that of carbon. But hey, don't go around challenging silicon atoms to an arm-wrestling match just yet!
Silicon (Si) is located below carbon (C) on the periodic table. In general, as we move down a group in the periodic table, the atomic size increases due to the addition of more electron shells.
Since silicon is in the same group (group 14) as carbon, we can expect that silicon would have a larger atomic size compared to carbon. The larger atomic size in silicon means that the outermost electron in silicon is farther away from the positively charged nucleus, leading to less electrostatic attraction between the electron and the nucleus.
As a result, the first ionization enthalpy of silicon would be expected to be lower than that of carbon. This means that it would require less energy to remove the first electron from an atom of silicon compared to an atom of carbon. Therefore, the first ionization enthalpy of silicon would be lesser than 1086 kJ/mol.
To determine whether the first ionization enthalpy of Si (Silicon) would be greater or lesser than that of Carbon, we need to consider the periodic trends and the electronic configuration of both elements.
Periodic trends indicate that ionization enthalpy generally increases across a period from left to right. This is mainly due to the increasing effective nuclear charge, which results in a stronger attraction between the positively charged nucleus and the negatively charged electrons in the outermost shell.
Carbon (C) is located to the left of Silicon (Si) in the periodic table. Carbon has an atomic number of 6, and its electronic configuration is 1s^2 2s^2 2p^2. The first ionization enthalpy of carbon is 1086 kJ/mol, which means that it requires 1086 kJ of energy to remove one mole of electrons from a mole of carbon atoms.
Silicon (Si) has an atomic number of 14, and its electronic configuration is 1s^2 2s^2 2p^6 3s^2 3p^2. As we move across the periodic table from left to right, the effective nuclear charge increases. Therefore, the first ionization enthalpy of Silicon is expected to be greater than that of Carbon.
In conclusion, the first ionization enthalpy of Silicon (Si) is expected to be greater than 1086 kJ/mol, which is the first ionization enthalpy of Carbon (C).