The first ionisation enthalpy of Na, Mg and Si are 496, 737, 776 kJ/mol respectively. What will be the first ionisation enthalpy potential of AI in kJ/mol?

Question

The first ionisation enthalpy of Na, Mg and Si are 496, 737, 776 kJ/mol respectively. What will be the first ionisation enthalpy potential of AI in kJ/mol? (A) > 766 kJ/mol (B) > 496 and < 737 kJ (C) > 737 and < 766 kJ/mol (D) > 496 kJ/mol

Tardigrade Admin · Accepted Answer

Na , Mg , Al and Si are in period 3 and as we move across the period, the atomic size decreases and hence ionisation enthalpy increases. So, the order is Na < Mg < Al < Si Hence, IE of Al is greater than that of Mg (737 kJ / mol ) and lower than that of Si (776 kJ / mol )

Q. The first ionisation enthalpy of Na, Mg and Si are 496, 737, 776 kJ/mol respectively. What will be the first ionisation enthalpy potential of AI in kJ/mol?

> 766 kJ/mol

> 496 and < 737 kJ

> 737 and < 766 kJ/mol

> 496 kJ/mol

$N a, M g, A l$ and $S i$ are in period $3 an d a s$ we move across the period, the atomic size decreases and hence ionisation enthalpy increases. So, the order is $N a < M g < A l < S i$ Hence, IE of Al is greater than that of Mg $(737 k J / m o l)$ and lower than that of Si $(776 k J / m o l)$

Q. The first ionisation enthalpy of Na, Mg and Si are 496, 737, 776 kJ/mol respectively. What will be the first ionisation enthalpy potential of AI in kJ/mol?

> 766 kJ/mol

> 496 and < 737 kJ

> 737 and < 766 kJ/mol

> 496 kJ/mol

Na,Mg,Al and Si are in period 3andas we move across the period, the atomic size decreases and hence ionisation enthalpy increases. So, the order is Na<Mg<Al<Si Hence, IE of Al is greater than that of Mg (737kJ/mol) and lower than that of Si (776kJ/mol)

$N a, M g, A l$ and $S i$ are in period $3 an d a s$ we move across the period, the atomic size decreases and hence ionisation enthalpy increases. So, the order is $N a < M g < A l < S i$ Hence, IE of Al is greater than that of Mg $(737 k J / m o l)$ and lower than that of Si $(776 k J / m o l)$