Classification of elements and periodicity in properties practice · Mixed difficulty

The first four ionisation energy values of an element are 191, 578, 872 and 5962 kcal. The number of valence electrons in the element is

Which of the following represents the correct order of increasing negative electron gain enthalpy of the elements?

Statement I: Ionisation potential of $Be$ is less than $B.$
Statement II: The first electron released from $Be$ is of s-orbital but that from $B$ is of p-orbital.

The process requiring the absorption of energy is

Number of elements presents in the fifth period of periodic table is

Although electron gain enthalpy of fluorine is less negative as compared to chlorine, fluorine is a stronger oxidising agent then chlorine. This is attributed to

Atomic radii of fluorine and neon in angstrom unit are respectively given by:

At present, how many elements are known

Among the elements Ca, Mg, P and Cl, the order of increasing atomic radii is

The incorrect order is

Which of the following should be the order of increasing values of second ionisation potential of C, N, O and F

Elements having similar outer shell electronic configuration in their atoms are arranged in

Which of the following has the largest size

${M^{ + 3}}$ ion has the electronic configuration as $\left[ {Xe} \right]\,\,5{d^{10}}4{f^{14}}6{s^2},$ hence the element $M$ belongs to

Which of the following statement(s) is/are true?

Electronegativity refers to the tendency of atom to

Assertion (A): $\mathrm{Na}^{+}$ and $\mathrm{Al}^{3+}$ are isoelectronic but the ionic radii of $\mathrm{Al}^{3+}$ is smaller than $\mathrm{Na}^{+}$
Reason (R): The nuclear attraction on the outermost shell electrons of $\mathrm{Al}^{3+}$ is greater than that of $\mathrm{Na}^{+}$.

Read the following three statements and choose the correct option. Here $\mathrm{T}$ stands for true and $\mathrm{F}$ stands for false statement.

(i) Boron has a smaller first ionization enthalpy than beryllium.

(ii) Nitrogen has smaller first ionization enthalpy than oxygen.

(iii) The first ionization enthalpy increases across a period.

The electron configuration of an element ‘M’ is $\left[ {Ar} \right]\,\,3{d^{10}}4{s^2}4{p^3}.$ Then ‘M’ belongs to

Statement I: Ionic radius of $\mathrm{O}^{2-}$ is greater than $\mathrm{F}^{-}.$

Statement II: $\mathrm{O}^{2-}$ and $\mathrm{F}^{-}$are isoelectronic species.

In light of the above statements, choose the correct answer from the options given below

Atomic number 116 is written in IUPAC as

The element with atomic number 36 belongs to …block in the Periodic Table.

The $\mathrm{I}{\mathrm{P}_1},\mathrm{I}{\mathrm{P}_2},\mathrm{I}{\mathrm{P}_3},\mathrm{I}{\mathrm{P}_4},\mathrm{ and } \, {\mathrm{IP}_5}$ of an element are $7.1,\mathrm{ }14.3,\mathrm{ }34.5$, $46.8$,$162.2 \, \, \text{eV}$ respectively. The element is likely to be:

In which of the following species ${2^{nd}}I.E\mathrm{ } < \mathrm{ }{1^{st}}I.E$

Statement I: $F$ is more electronegative than $Cl.$

Statement II: $F$ has high electron affinity than $Cl.$

Identify the correct order of solubility of $\mathrm{N}{\mathrm{a}_2}\mathrm{S},\mathrm{CuS}$ and $\mathrm{ZnS}$ in aqueous medium:

The ionisation energy and electron affinity of an element are 13.0 eV and 3.8 eV resp.
It’s electronegativity is

$X - O - H\xrightarrow[{{H_2}O}]{}$

$Y - O - H\xrightarrow[{{H_2}O}]{}$

E.N. - Electronegativity value

Incorrect option is:

The period containing max. number of element is:

The first ionisation enthalpy of $Na$ is 5.1 eV, the value of electron gain enthalpy of $N{a^ + }$ will be