Classification of Elements and Periodicity — JEE Main PYQs

The ionic radius of ${\mathrm{Na}}^{+}$ion is $1.02\stackrel{\circ }{A}$. The ionic radii (in $\stackrel{\circ }{\mathrm{A}}$ ) of ${\mathrm{Mg}}^{2+}$ and ${\mathrm{Al}}^{3+}$, respectively are:

The ionic radii of F⁻ and O²⁻ respectively are 1.33 Å and 1.4 Å, while the covalent radius of N is 0.74 Å. The correct statement for the ionic radius of N³⁻ from the following is:

The atomic radius of Ag is closest to

The order of electron gain enthalpy in $\mathrm{kJ}/\mathrm{mol}$ of fluorine, chlorine, bromine and iodine, respectively are

Within each pair of elements $\mathrm{F}\&\mathrm{Cl},\mathrm{S}\&\mathrm{Se}$ and $\mathrm{Li}\&\mathrm{Na}$, respectively, the elements that release more energy upon an electron gain are

The third ionization enthalpy is minimum for :

The first ionization energy (in $\mathrm{kJ}/\mathrm{mol}$ ) of $\mathrm{Na},\mathrm{Mg},\mathrm{Al}$ and Si respectively, are :

The increasing order of the atomic radii of the following elements is:
(a) C
(b) O
(c) F
(d) Cl
(e) Br

The first and second ionisation enthalpies of a metal are 496 and $4560\mathrm{kJ}{\mathrm{mol}}^{-1}$, respectively. How many moles of HCl and ${\mathrm{H}}_2{\mathrm{SO}}_4$, respectively, will be needed to react completely with 1 mole of the metal hydroxide ?

The acidic, basic and amphoteric oxides, respectively, are:

B has a smaller first ionization enthalpy than Be. Consider the following statements:
(i) it is easier to remove $2p$ electron than $2s$ electron.
(ii) $2p$ electron of $B$ is more shielded from the nucleus by the inner core of electrons than the $2s$ electrons of Be.
(iii) $2s$ …

The correct order of the ionic radii of ${\mathrm{O}}^{2-},{\mathrm{N}}^{3-},{\mathrm{F}}^{-},{\mathrm{Mg}}^{2+},{\mathrm{Na}}^{+}$ and ${\mathrm{Al}}^{3+}$ is:

The atomic number of the element unnilennium is

The five successive ionization enthalpies of an element are 800, 2427, 3658, 25024 and $32824\mathrm{kJ}{\mathrm{mol}}^{-1}$. The number of valence electrons in the element is:

Among the statements (I - IV), the correct ones are:
(I) Be has smaller atomic radius compared to Mg.
(II) Be has higher ionization enthalpy than AI.
(III) Charge/radius ratio of Be is greater than that of AI.
(IV) Both Be and AI form mainly covalent compounds.

The atomic number of Unnilunium is _____.

The ionic radii of ${\mathrm{O}}^{2-},{\mathrm{F}}^{-},{\mathrm{Na}}^{+}$ and ${\mathrm{Mg}}^{2+}$ are in the order:

The process that is NOT endothermic in nature is:

The size of the iso-electronic species ${\mathrm{Cl}}^{-}$, $\mathrm{Ar}$ and ${\mathrm{Ca}}^{2+}$ is affected by

The IUPAC symbols for the element with atomic number 119 would be:

The element having greatest difference between its first and second ionization energies, is

The electronegativity of aluminium is similar to

The correct option with respect to the Pauling electronegativity values of the elements is:

The group number, number of valence electrons and valency of an element with atomic number 15, respectively, are:

The correct order of the atomic radii of $\mathrm{C},\mathrm{Cs},\mathrm{Al}$ and S is:

The element with $Z=120$ (not yet discovered) will be an/a

The pair that has similar atomic radii is:

In comparison to boron, berylium has:

When the first electron gain enthalpy $({\Delta }_{\mathrm{eg}}\mathrm{H})$ of oxygen is $-141\mathrm{kJ}/\mathrm{mol}$, its second electron gain enthalpy is

In general, the properties that decrease and increase down a group in the periodic table respectively are

In the following reactions, ZnO is respectively acting as a/an :
(a) $\mathrm{ZnO}+{\mathrm{Na}}_2\mathrm{O}\to {\mathrm{Na}}_2{\mathrm{ZnO}}_2$
(b) $\mathrm{ZnO}+{\mathrm{CO}}_2\to {\mathrm{ZnCO}}_3$

Which of the following atoms has the highest first ionization energy?

The ionic radii (in $\mathring{A}$) of ${\mathrm{N}}^{3-}$, ${\mathrm{O}}^{2-}$ and ${\mathrm{F}}^{-}$ are respectively:

The first ionization potential of Na is 5.1 eV. The value of electron gain enthalpy of ${\mathrm{Na}}^{+}$ will be:

Which of the following represents the correct order of increasing first ionization enthalpy for $\mathrm{Ca},\mathrm{Ba},\mathrm{S},\mathrm{Se}$ and Ar?

The increasing order of the ionic radii of the given isoelectronic species is :

The correct sequence which shows decreasing order of the ionic radii of the elements is

In which of the following arrangements, the sequence is not strictly according to the property written against it ?

The set representing the correct order of ionic radius is :

The increasing order of the first ionization enthalpies of the elements $B,P,S$ and $F$ (lowest first) is

Following statements regarding the periodic trends of chemical reactivity of the alkali metals and the halogens are given. Which of these statements gives the correct picture?

In which of the following arrangements the order is NOT according to the property indicated against it?
(1) ${\mathrm{Al}}^{3+}<{\mathrm{Mg}}^{2+}<{\mathrm{Na}}^{+}<{\mathrm{F}}^{-}$ — Increasing ionic size
(2) $\mathrm{B}<\mathrm{C}<\mathrm{N}<\mathrm{O}$ — Increasing first ionization e …

Of the following sets which one does NOT contain isoelectronic species?

Which one the following ions has the highest value of ionic radius?

Among ${\mathrm{Al}}_2{\mathrm{O}}_3$, ${\mathrm{SiO}}_2$, ${\mathrm{P}}_2{\mathrm{O}}_3$ and ${\mathrm{SO}}_2$ the correct order of acid strength is

The formation of the oxide ion ${\mathrm{O}}^{2-}(\mathrm{g})$ requires first an exothermic and then an endothermic step as shown below
$\mathrm{O}(\mathrm{g})+{\mathrm{e}}^{-}\to {\mathrm{O}}^{-}(\mathrm{g})$ $\Delta {\mathrm{H}}^{\circ }=-142{\mathrm{kJmol}}^{-1}$ …

Which among the following factors is the most important in making fluorine the strongest oxidizing halogen?

Beryllium and aluminium exhibit many properties which are similar. But the two elements differ in