Ionization Energy Ie

Which one of the following orders is not in accordance with the property stated against?

1. $F_2>C{l}_2>B{r}_2>I_2$ $:$ $Oxidi\sin g$ $power$

2. $Hl>HBr>HCl>HF$ $:$ $Acidic$ $property$ $in$ $water$

3. $F_2>C{l}_2>B{r}_2>I_2$ $:$ $Electronegativity$

4. $F_2>C{l}_2>B{r}_2>I_2$ $:$ $Bond$ $dissociation$ $energy$

A configuration with the lowest ionization enthalpy among the following is:
1. $\mathrm{}$
2.
3.
4.

Amongst the elements with the following electronic configurations, which one of them may have the highest ionisation energy?

1. $\left[Ne\right]$ $3s^2$ $3p^2$

2. $\left[Ne\right]$ $3s^2$ $3p^3$

3. $\left[Ar\right]$ $3d^{10}$ $4s^2$ $4p^3$

4. $\left[Ne\right]$ $3s^2$ $3p^1$

For the second-period elements, the correct increasing order of first ionisation enthalpy is:

1.	Li < Be < B < C < O < N < F < Ne
2.	Li < Be < B < C < N < O < F < Ne
3.	Li < B < Be < C < O < N < F < Ne
4.	Li < B < Be < C < N < O < F < Ne

Arrange the elements Li, Be, B, C, and N in increasing order of their first ionization enthalpies:

1.	Li < B < Be < C < N	2.	Li < Be < C < B < N
3.	Li < Be < N < B < C	4.	Li < Be < B < C < N

Which of the following statements are true?

A.	Unlike Ga that has a very high melting point, Cs has a very low melting point.
B.	On Pauling scale, the electronegativity values of N and Cl are not the same.
C.	and are all isoelectronic species.
D.	The correct order of the first ionization enthalpies of Na, Mg, Al, and Si is Si > Al > Mg > Na
E.	The atomic radius of Cs is greater than that of Li and Rb.

Choose the correct answer from the options given below:

1.	C and D only
2.	A, C and E only
3.	A, B and E only
4.	C and E only