$ \text { Match the following } $

$ \begin{array}{cccc} \hline & \text { List-I (Elements) } & & \text { List-II (Group) } \\ \hline \text { A } & \mathrm{Mn}, \mathrm{Tc}, \mathrm{Re} & \text { I } & 12 \\ \hline \text { B } & \mathrm{Zn}, \mathrm{Cd}, \mathrm{Hg} & \text { II } & 4 \\ \hline \text { C } & \mathrm{Ti}, \mathrm{Zr}, \mathrm{Hf} & \text { III } & 17 \\ \hline \text { D } & \mathrm{Ga}, \mathrm{In}, \mathrm{Tl} & \text { IV } & 7 \\ \hline & & \text { V } & 13 \\ \hline \end{array} $

The correct answer is

Match the following

The correct answer is

In long form of periodic table an element ' $E$ ' has atomic number 78 . The period and group number of the element are $x$ and $y$ respectively. $(x+y)$ is equal to

In second period of the modern periodic table, two elements $X$ and $Y$ have higher first ionisation enthalpy values than the preceding and succeeding elements. $X$ and $Y$ are respectively

$ \text { Match the following. } $

The correct answer is

Observe the following data ( $\Delta_t H_1, \Delta_t H_2$ and $\Delta_{\mathrm{eg}} H$ represent the first, second ionisation enthalpies and electron gain enthalpy respectively)

Using the data identify the most reactive metal.

Atomic numbers of three elements $E_1, E_2$ and $E_3$ of periodic table are $Z_1, 50$ and $Z_2$ respectively. From the position of the elements shown in figure, the values of $\left(Z_2-Z_1\right)$ is

Electron gain enthalpy values $\left(\Delta_{\mathrm{cg}} H\right)$ (in $\mathrm{kJ} \mathrm{mol}^{-1}$ ) of elements $X, Y$ and $Z$ are $-349,-200$ and -295 respectively. $X, Y$ and $Z$ are respectively

In which of the following options, elements are correctly arranged in the increasing order of their atomic radius?

$A, B C, D$ and $E$ are elements with atomic numbers 13 , $11,9,7$ and 16 respectively. Among these elements, ion of an element $X$ has largest size and ion of an element $Y$ has smallest size. $X$ and $Y$ are respectively.(Assume that all ions have nearest inert gas configuration)

The correct order of atomic radii of group 13 elements is

Observe the following oxides. The number of amphoteric oxides from the given list is $\mathrm{CO}, \mathrm{B}_2 \mathrm{O}_3, \mathrm{SnO}_2, \mathrm{PbO}_2, \mathrm{Ga}_2 \mathrm{O}_3, \mathrm{SnO}, \mathrm{PbO}, \mathrm{CO}_2$

Assertion (A) : The ionic radii of $\mathrm{Na}^{+}$and $\mathrm{F}^{-}$are same.

Reason (R) : Both $\mathrm{Na}^{+}$and $\mathrm{F}^{-}$are isoelectronic species.

The correct answer is

Assertion (A) First ionisation enthalpy of oxygen is less than that of nitrogen.

Reason (R) Atoms with half-filled or completely filled orbitals are less stable.

The correct option among the following is

Tha atomic radius of gallium is less than that of aluminium. This is due to

$ \text { Match the following. } $

$ \begin{array}{cccc} \hline & \begin{array}{c} \text { List-I } \\ \text { (Atomic number) } \end{array} & & \begin{array}{c} \text { List-II } \\ \text { (Group number and } \\ \text { period number) } \end{array} \\ \hline \text { A. } & 56 & \text { I. } & 9,4 \\ \hline \text { B. } & 50 & \text { II. } & 3,6 \\ \hline \text { C. } & 27 & \text { III. } & 14,5 \\ \hline \text { D. } & 58 & \text { IV. } & 2,6 \\ \hline \end{array} $

The correct answer is

What is the correct order with respect to metallic property of Zr, Cd, Sn, Sr?

In which of the following options, the elements are correctly arranged with respect to their negative electron gain enthalpies?

In group 13 of the long form of periodic table an element $X$ has a boiling point of $T_2(\mathrm{~K})$ and melting point of $T_1(\mathrm{~K})$. Identify the element $X$ for which $T_2-T_1(\mathrm{~K})$ is maximum

Consider the following.

(I) The order of first ionisation enthalpy of first three elements of 3rd period is $\mathrm{Mg}>\mathrm{Al}>\mathrm{Na}$.

(II) The element with electronegativity of 3.5 is chlorine.

(III) The order of sizes of ions $\mathrm{Mg}^{2+}, \mathrm{Na}^{+}, \mathrm{F}^{-}$and $\mathrm{O}^{2-}$ is $\mathrm{Mg}^{2+}<\mathrm{Na}^{+}<\mathrm{F}^{-}<\mathrm{O}^{2-}$.

(IV) The IUPAC name of the element with atomic number 106 is bohrium.

The correct statements are

Identify the correct statements from the following.

(I) Au is soluble in aqua regia but not Pt .

(II) Among the oxoacids of chlorine highest oxidation state possible for chlorine is +7 .

(III) Among the hydrogen halides lowest boiling point is for HCl .

(IV) The order of stability of oxides of halogens is $\mathrm{Cl}>\mathrm{Br}>\mathrm{I}$.

Which of the following sequence is correct for decreasing order of ionic radius?

The successive ionisation energies (starting from the 1 st ) of an element are $801,2430,3660,25,000$ and $32,800 \mathrm{~kJ} \mathrm{~mol}^{-1}$, respectively. The element is

Assertion (A) The ionic radii of the alkaline earth metals are smaller than those of alkali metals in the same period.

Reason (R) Alkali metals have higher nuclear charge than that of the alkaline earth metals.

The correct option among the following is

Which of the following species are isoelectronic species?

(A) $\mathrm{O}^{2-}$

(B) $\mathrm{F}^{-}$

(C) $\mathrm{Na}^{+}$

(D) $\mathrm{Mg}^{2+}$

Arrange the following in increasing order of ionic radii

$ \mathrm{O}^{2-}, \mathrm{Na}^{+}, \mathrm{F}^{-}, \mathrm{Mg}^{2+} $

The correct order of ionic radii for the given species is

Which of the following set of properties generally decreases along a period?

The correct order of the electron gain enthalpy of the given elements is

How many of the following statements are correct?

(A) ' $\mathrm{He}^{\prime}$ ' is the second most abundant element in the universe.

(B) The symbol for the element with atomic number 110 is Ds.

(C) Osmium has the highest density among all elements.

(D) Francium is the most electropositive element in the periodic table.

The correct order of the first ionisation enthalpies of the following elements is

The basic difference in approach between Mendeleev's periodic law and modern periodic law is the change on the basis of classification of elements from

Which of the following pairs shows diagonal relationship?

Arrange the following ions in the correct order with respect to their ionic radii.

Based on the quantum numbers, what will be the maximum number of element for sixth period of the periodic table?

Assertion (A) $\mathrm{Mg}^{2+}$ and $\mathrm{Al}^{3+}$ are isoelectronic but the magnitude of ionic radius of $\mathrm{Al}^{3+}$ is less than that in $\mathrm{Mg}^{2+}$.

Reason (R) The effective nuclear charge on the outermost electrons in $\mathrm{Al}^{3+}$ is greater than that in $\mathrm{Mg}^{2+}$.The correct option among the following is

The successive ionisation energy values for an element ' $X$ ' are given below :

(i) 1st ionisation energy $=410 \mathrm{~kJ} \mathrm{~mol}^{-1}$

(ii) 2nd ionisation energy $=820 \mathrm{~kJ} \mathrm{~mol}^{-1}$

(iii) 3rd ionisation energy $=1100 \mathrm{~kJ} \mathrm{~mol}^{-1}$

(iv) 4th ionisation energy $=1500 \mathrm{~kJ} \mathrm{~mol}^{-1}$

(v) 5th ionisation energy $=3200 \mathrm{~kJ} \mathrm{~mol}^{-1}$