Classification of elements and periodicity in properties practice · Medium

Which of the following is not a member of actinoid series?

Assertion : ${Na}^{+}$ and ${Cl}^{-}$ have similar ionic radius.

Reason : ${Z}_{\text {eff}}$ in ${Na}^{+}$ and ${Cl}^{-}$ are same.

The value of $\mathrm{IE}_1, \mathrm{IE}_2, \mathrm{IE}_3$ and $\mathrm{IE}_4$ of an atom are $7.5 \mathrm{~eV}, 25.6 \mathrm{~eV}, 48.6 \mathrm{~eV}$ and $170.6 \mathrm{~eV}$ respectively.
The electronic configuration of the atom will be:-

Consider the following elements In, Tl, Al, Pb, Sn and Ge.

The most stable oxidation states of elements with highest and lowest first ionisation enthalpies, respectively, are

Which of the following elements are found in pitch blende?

Consider the following elements.
${\text{Group}} \downarrow \,_{C'\,D'}^{A'\,B' \to {\text{Period}}}$
Which of the following is/are true about $A^{\prime}, B^{\prime}, C^{\prime}$ and $D^{\prime}$ ?

A. Order of atomic radii: $\mathrm{B}^{\prime} < \mathrm{A}^{\prime} < \mathrm{D}^{\prime} < \mathrm{C}^{\prime}$

B. Order of metallic character: $B^{\prime} < A^{\prime} < D^{\prime} < C^{\prime}$

C. Size of the element: $D^{\prime} < C^{\prime} < B^{\prime} < A^{\prime}$

D. Order of ionic radii : $\mathrm{B}^{\prime+} < \mathrm{A}^{\prime+} < \mathrm{D}^{\prime+} < \mathrm{C}^{\prime+}$

Choose the correct answer from the option given below:

Which among the following elements has highest negative electron gain enthalpy?

The $\mathrm{I}{\mathrm{P}_1}$ is maximum for:

Maximum I.E is for

Which of the following option is the correct order for the basic strength of metallic hydroxides?

Assertion : IP of $F$ $>$ EA of $F.$

Reason : ${F}$ is a highly electronegative element.

Which of the following metal is expected to have the highest third ionisation energy ?

Which of the following has the smallest size?

Which of the following should be correct for ${Z_1}$ and ${Z_2}$ in the following two processes
${M^ + } + {Z_1}\xrightarrow{\,}{M^{2 + }} + {e^ - }$
${M^{2 + }} + {Z_2}\xrightarrow{\,}{M^{3 + }} + {e^ - }$

Assertion : Size of $\mathrm{Ca}^{2+}$ is larger than $\mathrm{K}^{+}$.

Reason : Number of electrons in $\mathrm{Ca}^{+2}$ is more than $\mathrm{K}^{+}$.

The first ionization enthalpy of $\mathrm{Na}, \mathrm{Mg}$ and $\mathrm{Si}$, respectively, are : 496,737 and $786 \mathrm{~kJ} \mathrm{~mol}^{-1}$. The first ionization enthalpy $\left(\mathrm{kJ} \mathrm{mol}^{-1}\right)$ of $\mathrm{Al}$ is:

An element having electronic configuration $1 s^2 2 s^2 2 p^6 3 s^2 3 p^6 4 s^1$ forms

The energy evolved is highest for which of the following reactions.

S-I: $\mathrm{Cu}^{+2}$ paramagnetic.

S-II: All the orbitals present in $\mathrm{Cu}^{+2}$ ion are doubly occupied.

The electronic configuration, $1{s^2},\;2{s^2}2{p^6},\;3{s^2}\;3{p^6}3{d^9}$ represents a

Four successive members of first row transition elements are listed below with their atomic numbers. Which one of them is expected to have the highest third ionization enthalpy

The ionic radius of ‘Cr’ is minimum in which of the following compounds?

Aqueous solutions of two compounds $M-{O}-{H}$ and $M^{\prime}-{O}-{H}$ have been prepared in two different beakers. If the electronegativity of $M=3.5, M^{\prime}=1.72$, ${O}=3.0$ and ${H}=2.1$, then the solutions respectively are

The first, second and third ionisation energies of ${Al}$ are 578,1817 and $2745 \mathrm{~kJ} \mathrm{~mol}^{-1}$ respectively. Calculate the energy required to convert all the atoms of ${Al}$ to ${Al}^{+3}$ present in $270{mg}$ of ${Al}$ vapours

Arrange the following elements in increasing order of electronegativity:

$\mathrm{N}, \mathrm{O}, \mathrm{F}, \mathrm{C}, \mathrm{Si}$

Choose the correct answer from the options given below:

Higher values of ionisation energies of the 5d-transition elements are consistent with the :

A large difference between the third and fourth ionization energies indicates the presence of :

Which of the following does not represent the correct order of the properties indicated?

The second ionization enthalpies of elements are always higher than their first ionization enthalpies because:

S-I: The second ionisation energy of '$O$' is greater than that of '$N$'.

S-II: The half filled p-orbitals cause greater stability.