Periodic Table · JEE Main previous year questions

For the Balmer series in the spectrum of H atom, $\bar{\nu }=R_H\left\{\frac{1}{n_1^2}-\frac{1}{n_2^2}\right\}$, the correct statements among (I) to (IV) are : (I) As wavelength decreases, the lines in the series converge (II) The integer $n_1$ is equal to 2 (III) The line of longest wavelength corresponds to $n_2=3$ (IV) The ionization energy of hydrogen can be calculated from wave number of these lines

1. A.(II), (III), (IV)
2. B.(I), (II), (III)
3. C.(I), (III), (IV)
4. D.(I), (II), (IV)

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

1. A.496, 577, 786, 737
2. B.496, 737, 577, 786
3. C.786, 737, 577, 496
4. D.496, 577, 737, 786

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

1. A.(a) < (b) < (c) < (d) < (e)
2. B.(c) < (b) < (a) < (d) < (e)
3. C.(b) < (c) < (d) < (a) < (e)
4. D.(d) < (c) < (b) < (a) < (e)

For the following Assertion and Reason, the correct option is Assertion : For hydrogenation reactions, the catalytic activity increases from Group 5 to Group 11 metals with maximum activity shown by Group 7-9 elements. Reason : The reactants are most strongly adsorbed on group 7-9 elements.

1. A.Both assertion and reason are true and the reason is the correct explanation for the assertion.
2. B.The assertion is true, but the reason is false.
3. C.Both assertion and reason are true but the reason is not the correct explanation for the assertion.
4. D.Both assertion and reason are false.

The atomic radius of Ag is closed to :

1. A.Au
2. B.Cu
3. C.Hg
4. D.Ni

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

1. A.16, 6 and 3
2. B.15, 6 and 12
3. C.16, 5 and 2
4. D.15, 5 and 3

The pair that has similar atomic radii is :

1. A.Mo and W
2. B.Mn and Fe
3. C.Ti and Hf
4. D.Sc and Ni

The correct order of the first ionization enthalpies is :

1. A.Ti < Mn < Zn < Ni
2. B.Zn < Ni < Mn < Ti
3. C.Mn < Ti < Zn < Ni
4. D.Ti < Mn < Ni < Zn

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

1. A.Ba
2. B.Ca
3. C.Sc
4. D.K

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

1. A.Uun
2. B.Une
3. C.Uue
4. D.Unh

The correct order of atomic radii is :

1. A.Ho > N > Eu > Ce
2. B.Ce > Eu > Ho > N
3. C.N > Ce > Eu > Ho
4. D.Eu > Ce > Ho > N

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

1. A.Atomic Radius and Electronegativity
2. B.Electron Gain Enthalpy and Electronegativity.
3. C.Electronegativity and Atomic Radius.
4. D.Electronegativity and Electron Gain Enthalpy.

A group 13 element 'X' reacts with chlorine gas to produce a compound $\mathrm{XC}{\mathrm{l}}_3$. $\mathrm{XC}{\mathrm{l}}_3$ is electron deficient and easily reacts with $\mathrm{N}{\mathrm{H}}_3$ to form $\mathrm{C}{\mathrm{l}}_3\mathrm{X}\leftarrow \mathrm{N}{\mathrm{H}}_3$ adduct ; however, $\mathrm{XC}{\mathrm{l}}_3$ does not dimerize X is :

1. A.B
2. B.Al
3. C.Ga
4. D.In

For ${\text{Na}}^{+},{\text{Mg}}^{2+},{\text{F}}^{-}$ and ${\text{O}}^{2-}$; the correct order of increasing ionic radii is :

1. A.${\text{O}}^{2-}<{\text{F}}^{-}<{\text{Na}}^{+}<{\text{Mg}}^{2+}$
2. B.${\text{Na}}^{+}<{\text{Mg}}^{2+}<{\text{F}}^{-}<{\text{O}}^{2-}$
3. C.${\text{Mg}}^{2+}<{\text{Na}}^{+}<{\text{F}}^{-}<{\text{O}}^{2-}$
4. D.${\text{Mg}}^{2+}<{\text{O}}^{2-}<{\text{Na}}^{+}<{\text{F}}^{-}$

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

1. A.Na
2. B.K
3. C.Sc
4. D.Rb

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

1. A.1.36, 1.71 and 1.40
2. B.1.71, 1.40 and 1.36
3. C.1.71, 1.36 and 1.40
4. D.1.36, 1.40 and 1.71

Which of the following presents the correct order of second ionization enthalpies of C, N, O and F ?

1. A.$\mathrm{F}>\mathrm{O}>\mathrm{N}>\mathrm{C}$
2. B.$\mathrm{O}>\mathrm{N}>\mathrm{F}>\mathrm{C}$
3. C.$\mathrm{C}>\mathrm{N}>\mathrm{O}>\mathrm{F}$
4. D.$\mathrm{O}>\mathrm{F}>\mathrm{N}>\mathrm{C}$

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

1. A.$\mathrm{A}{\mathrm{l}}^{3+}>\mathrm{M}{\mathrm{g}}^{2+}>\mathrm{N}{\mathrm{a}}^{+}>{\mathrm{F}}^{-}>{\mathrm{O}}^{2-}$
2. B.$\mathrm{N}{\mathrm{a}}^{+}>\mathrm{M}{\mathrm{g}}^{2+}>\mathrm{A}{\mathrm{l}}^{3+}>{\mathrm{O}}^{2-}>{\mathrm{F}}^{-}$
3. C.$\mathrm{N}{\mathrm{a}}^{+}>{\mathrm{F}}^{-}>\mathrm{M}{\mathrm{g}}^{2+}>{\mathrm{O}}^{2-}>\mathrm{A}{\mathrm{l}}^{3+}$
4. D.${\mathrm{O}}^{2-}>{\mathrm{F}}^{-}>\mathrm{N}{\mathrm{a}}^{+}>\mathrm{M}{\mathrm{g}}^{2+}>\mathrm{A}{\mathrm{l}}^{3+}$

The set representing the correct order of ionic radius is :

1. A.$\mathrm{N}{\mathrm{a}}^{+}>\mathrm{L}{\mathrm{i}}^{+}>\mathrm{M}{\mathrm{g}}^{2+}>\mathrm{B}{\mathrm{e}}^{2+}$
2. B.$\mathrm{L}{\mathrm{i}}^{+}>\mathrm{N}{\mathrm{a}}^{+}>\mathrm{M}{\mathrm{g}}^{2+}>\mathrm{B}{\mathrm{e}}^{2+}$
3. C.$\mathrm{M}{\mathrm{g}}^{2+}>\mathrm{B}{\mathrm{e}}^{2+}>\mathrm{L}{\mathrm{i}}^{+}>\mathrm{N}{\mathrm{a}}^{+}$
4. D.$\mathrm{L}{\mathrm{i}}^{+}>\mathrm{B}{\mathrm{e}}^{2+}>\mathrm{N}{\mathrm{a}}^{+}>\mathrm{M}{\mathrm{g}}^{2+}$

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?

1. A.The reactivity decreases in the alkali metals but increases in the halogens with increase in atomic number down the group
2. B.In both the alkali metals and the halogens the chemical reactivity decreases with increase in atomic number down the group
3. C.Chemical reactivity increases with increase in atomic number down the group in both the alkali metals and halogens
4. D.In alkali metals the reactivity increases but in the halogens it decreases with increase in atomic number down the group

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

1. A.F < S < P < B
2. B.P < S < B < F
3. C.B < P < S < F
4. D.B < S < P < F

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

1. A.${\mathrm{O}}^{2-}$
2. B.${\mathrm{B}}^{3+}$
3. C.$\mathrm{L}{\mathrm{i}}^{+}$
4. D.${\mathrm{F}}^{-}$

The correct order of ionic radius is

1. A.$Ce>Sm>Tb>Lu$
2. B.$Lu>Tb>Sm>Ce$
3. C.$Tb>Lu>Sm>Ce$
4. D.$Sm>Tb>Lu>Ce$

$C{e}^{+3},L{a}^{+3},P{m}^{+3}$ and $Y{b}^{+3}$ have ionic radii in the increasing order as

1. A.$L{a}^{+3}<C{e}^{+3}<P{m}^{+3}<Y{b}^{+3}$
2. B.$Y{b}^{+3}<P{m}^{+3}<C{e}^{+3}<L{a}^{+3}$
3. C.$L{a}^{+3}=C{e}^{+3}<P{m}^{+3}<Y{b}^{+3}$
4. D.$Y{b}^{+3}<P{m}^{+3}<L{a}^{+3}<C{e}^{+3}$