Periodic Properties and Their Variation in Groups and Periods

The ions  ${\mathrm{O}}^{2-},{\mathrm{F}}^{-},{\mathrm{Na}}^{+},{\mathrm{Mg}}^{2+}\mathrm{and}{\mathrm{Al}}^{3+}$ are isoelectronic. Their ionic radii show:

The atomic number of Vanadium $\left(\mathrm{V}\right)$, Chromium $\left(\mathrm{Cr}\right)$, Manganese $\left(\mathrm{Mn}\right)$ and Iron $\left(\mathrm{Fe}\right)$ are, respectively, $23, 24, 25 \mathrm{and} 26$. Which one of these may be expected to have the highest second ionization enthalpy?

Which one of the following arrangements does not truly represent the property indicated against it?

(A)${\mathrm{Br}}_2 < {\mathrm{Cl}}_{2 }< {\mathrm{F}}_2$ : Oxidising power

(B) $\mathrm{Br}< \mathrm{Cl}<\mathrm{F}$          : Electronegativity

(C) $\mathrm{Br}< \mathrm{F} < \mathrm{CI}$        : Electron affinity

(D) ${\mathrm{Br}}_2 < {\mathrm{Cl}}_2 < {\mathrm{F}}_2$  : Bond energy

Which of the following statements are not correct?

A. The electron gain enthalpy of $\mathrm{F}$ is more negative than that of $\mathrm{Cl}.$

B. Ionization enthalpy decreases in a group of periodic table.

C. The electronegativity of an atom depends upon the atoms bonded to it.

D. ${\mathrm{Al}}_2{\mathrm{O}}_3$ and $\mathrm{NO}$ are examples of amphoteric oxides.

Choose the most appropriate answer from the options given below:

For elements $\mathrm{B}, \mathrm{C}, \mathrm{N} \mathrm{Li}, \mathrm{Be}, \mathrm{O} \mathrm{and} \mathrm{F}$, the correct order of first ionisation enthalpy is

The difference between electron gain enthalpies will be maximum between :

The correct order of electronegativity for given elements is

Correct order of first Ionisation energy for $\mathrm{Li},\mathrm{Be},\mathrm{C},\mathrm{B},\mathrm{N},\mathrm{O},\mathrm{F}$.

The correct order of electronegativity of $\mathrm{Br},\mathrm{P},\mathrm{C} \mathrm{and} \mathrm{As}$.

Select The Correct Order Of Ionic Radii For ${\mathrm{Na}}^{+},{\mathrm{Mg}}^{2+},{\mathrm{F}}^{-}\mathrm{and} {\mathrm{O}}^{2-}$?

When the added electron goes to smaller n=3 quantum level ( $\mathrm{S} \mathrm{or} \mathrm{Cl}$)electron repulsion is much less. This is because?

Triad-$\mathrm{I}$ $\left[{\mathrm{N}}^{3-},{\mathrm{O}}^{-,}{\mathrm{Na}}^{+}\right]$

Triad-$\mathrm{II}$$\left[{\mathrm{N}}^{+}, {\mathrm{C}}^{+}, {\mathrm{O}}^{+}\right]$

Choose the species with lowest IP form triad-I and highest IP form Triad-II.

The correct order of stability of ${\mathrm{Al}}^{+},{\mathrm{Al}}^{+2},{\mathrm{Al}}^{+3}$ is:

Which is not correct order for the stated property ?

For the process

$$\begin{gathered} {\mathrm{X}}_{\left(\mathrm{g}\right)}+{\mathrm{e}}^{-}\stackrel{}{\to }{\mathrm{X}}_{\left(\mathrm{g}\right)}^{-} ∆\mathrm{H}=-\mathrm{x} \\ {\mathrm{X}}_{\left(\mathrm{g}\right)}^{-}\stackrel{}{\to }{\mathrm{X}}_{\left(\mathrm{g}\right)}+{\mathrm{e}}^{-} ∆\mathrm{H}=\mathrm{y} \end{gathered}$$

Elements $\mathrm{X},\mathrm{Y}$ and $\mathrm{Z}$ have atomic numbers $19,37$ and $55$ respectively. Which of the following statements is true about them?