# JEE Main & Advanced Chemistry Classification of Elements and Periodicity in Properties Question Bank

### done Ionisation Energy

• A) The first ionisation potential of $Al$ is less than the first ionisation potential of $Mg$

B) The second ionisation potential of $Mg$ is greater than the second ionisation potential of $Na$

C) The first ionisation potential of $Na$ is less than the first ionisation potential of $Mg$

D) The third ionisation potential of $Mg$ is greater than the third ionisation potential of $Al$

• A) Remove one mole of electron from one mole of gaseous anion

B) Remove one mole of electron from one mole of gaseous cation of the element

C) Remove one mole of electron from one mole of monovalent gaseous cation of the element

D) Remove 2 moles of electrons from one mole of gaseous atoms

• A) The same as the electron affinity of the element

B) Equal in magnitude but of opposite sign to the electron affinity of the element

C) The energy released when an electron is added to an atom of the element

D) The energy required to remove the outermost electron of an atom of the element

• A) There is increase in the nuclear charge of the alkaline earth metals

B) There is a decrease in the nuclear charge of the alkaline earth metals

C) There is no change in the nuclear charge

D) None of the above

• A) The properties of elements are the periodic functions of their atomic numbers

B) Non-metallic elements are lesser in number than metallic elements

C) The first ionisation energies along a period do not vary in a regular manner with increase in atomic number

D) For transition elements the $d$-sub-shells are filled with electrons monotonically with increase in atomic number

• A) Ionization energy and electron affinity increases across a period

B) Ionization energy increases but electron affinity decreases along a period

C) Ionization energy decreases but electron affinity increases

D) Both decreases along a period

• A) Habit to loose electrons decreases

C) Ionization potential decreases

D) In $M{{X}_{2}}\,(M=$ metal and $X=$ halogen), covalent properties decreases

• A) Halogens

B) Inert gases

C) Alkaline earth metals

D) Alkali metals

• A) The ionization energy of hydrogen is to high for group of alkali metals, but too low of halogen group

B) Hydrogen can form compounds with all other elements

C) Hydrogen is much lighter element than the alkali metals or the halogens

D) None of the above

• A) Nitrogen has half filled p-orbitals

B) Nitrogen is left to the oxygen in the same period of the periodic table

C) Nitrogen contains less number of electrons

D) Nitrogen is less electronegative

• A) Potential energy

B) Ionization energy

C) Electrode potential

D) Activation energy

• A) Boron has higher nuclear charge

B) Atomic size of boron is more than that of beryllium

C) Boron has only one electron in p-sub-shell

D) Atomic size of boron is less than that of beryllium

• A) ${{E}_{1}}<\,{{E}_{2}}$

B) ${{E}_{1}}={{E}_{2}}$

C) ${{E}_{1}}>{{E}_{2}}$

D) ${{E}_{1}}\ne {{E}_{2}}$

• A) V

B) Ti

C) Cr

D) Mn

• A) $1{{s}^{2}}2{{s}^{2}}2{{p}^{1}}$

B) $1{{s}^{2}}2{{s}^{2}}2{{p}^{3}}$

C) $1{{s}^{2}}2{{s}^{2}}2{{p}^{2}}$

D) $1{{s}^{2}}2{{s}^{2}}2{{p}^{4}}$

• A) $Cu\to C{{u}^{+}}$

B) $Br\to B{{r}^{-}}$

C) $I\to {{I}^{-}}$

D) $Li\to L{{i}^{+}}$

• A) Na < Mg > Al < Si

B) Na > Mg > Al > Si

C) Na < Mg < Al > Si

D) Na > Mg > Al < Si

• A) 1

B) 2

C) 4

D) 6

• A) $P$

B) $Si$

C) $Mg$

D) $Al$

• A) Large size

B) Small size

C) Ionic bond

D) Covalent bond

• A) $8.29eV$, $9.32eV$

B) $9.32eV$, $9.32eV$

C) $8.29eV$, $8.29eV$

D) $9.32eV$, $8.29eV$

• A) $Na\to N{{a}^{+}}+{{e}^{-}}$

B) ${{K}^{+}}\to {{K}^{2+}}+{{e}^{-}}$

C) ${{C}^{2+}}\to {{C}^{3+}}+{{e}^{-}}$

D) $C{{a}^{+}}\to C{{a}^{2+}}+{{e}^{-}}$

• A) K

B) Na

C) Al

D) Mg

• A) 1

B) 2

C) 3

D) 4

• A) Li

B) Cs

C) Cl

D) I

• A) Fe

B) H

C) Li

D) He

• A) Remains same

B) Increases from left to right

C) First increases, then decreases

D) Decreases from left to right

• A) Noble gases

B) Platinum metals

C) Transition elements

D) Inner-transition elements

• A) $[Ne]\,3{{s}^{2}}\,3{{p}^{1}}$

B) $[Ne]\,3{{s}^{2}}\,3{{p}^{2}}$

C) $[Ne]\,3{{s}^{2}}\,3{{p}^{3}}$

D) $[Ar]\,3{{d}^{10}}\,4{{s}^{2}}\,4{{p}^{2}}$

• A) N

B) O

C) F

D) Ne

• A) B

B) C

C) N

D) O

• A) - 54.4 eV

B) - 13.6 eV

C) - 27.2 eV

D) + 27.2 eV

• A) A decrease in the ionisation potential

B) An increase in the ionisation potential

C) No effect on the ionisation potential

D) An increase in the attraction of the nucleus to the electrons

• A) Sulphur

B) Oxygen

C) Nitrogen

D) Phosphorus

• A) Less than the first ionization potential

B) Equal to the first ionization potential

C) Greater than the first ionization potential

D) None of these

• A) Alkali metals

B) Halogens

C) Rare gases

D) Transition elements

• A) $K$

B) $Na$

C) $B$

D) $Kr$

• A) Lithium

B) Hydrogen

C) Uranium

D) Iron

• A) $S<P<As$

B) $P<S<As$

C) $As<S<P$

D) $As<P<S$

• A) $U>K>Cs$

B) $B>U>K$

C) $Cs>U>B$

D) $Cs<U<K$

• A) B

B) Li

C) Ne

D) F

• A) $K>Na>Li$

B) $Be>Mg>Ca$

C) $B>C>N$

D) $Ge>Si>C$

• A) $B<C<N$

B) $B>C>N$

C) $C<B<N$

D) $N>C>B$

• A) $Ne>Cl>P>S>Al>Mg$

B) $Ne>Cl>P>S>Mg>Al$

C) $Ne>Cl>S>P>Mg>Al$

D) $Ne>Cl>S>P>Al>Mg$

• A) $C>N>O$

B) $C<N>O$

C) $O>N>O$

D) $C>N$~$O$

• A) $N{{H}_{3}}<P{{H}_{3}}<As{{H}_{3}}$-acidic nature

B) $L{{i}^{+}}<N{{a}^{+}}<{{K}^{+}}<C{{s}^{+}}$-ionic radius

C) $A{{l}_{2}}{{O}_{3}}<MgO<N{{a}_{2}}O<{{K}_{2}}O$-basic

D) $Li<Be<B<C$-1st ionisation potential

• A) Lithium (Li)

B) Helium (He)

C) Nitrogen (N)

D) Zinc (Zn)

• A) Greater than $Be$

B) Less than $Be$

C) Equal to that of $Na$

D) Equal to that of $F$

• A) H

B) He

C) Be

D) Ne

• A) He

B) C

C) N

D) H

• A) s

B) p

C) d

D) f

• A) $Na>Mg>Al$

B) $Mg>Na>Al$

C) $Al>Mg>Na$

D) $Mg>Al>Na$

• A) $C{{s}^{+}}<{{K}^{+}}<M{{g}^{2+}}<A{{l}^{3+}}$

B) ${{K}^{+}}<C{{s}^{+}}<M{{g}^{2+}}<A{{l}^{3+}}$

C) $C{{s}^{+}}<{{K}^{+}}<A{{l}^{3+}}<M{{g}^{2+}}$

D) ${{K}^{+}}<C{{s}^{+}}<A{{l}^{3+}}<M{{g}^{2+}}$

• A) $Na<Mg>Al<Si$

B) $Na<Mg<Al<Si$

C) $Na>Mg>Al>Si$

D) $Na<Mg<Al>Si$

• A) $-13.6\,\,eV$

B) $13.6\,\,eV$

C) $-3.4\,eV$

D) $3.4\,\,eV$

• A) Weak oxidising agents

B) Strong reducing agents

C) Strong oxidising agents

D) Weak reducing agents

• A) $N{{a}^{+}}$

B) $M{{g}^{++}}$

C) ${{F}^{-}}$

D) ${{O}^{--}}$

• A) $Li>Na>K>Cs$

B) $Na>Li>K>Cs$

C) $Li>Cs>K>Na$

D) $K>Cs>Na>Li$

• A) ${{I}_{Mg}}=I{{I}_{Na}}$

B) ${{I}_{Na}}>{{I}_{Mg}}$

C) $I{{I}_{Mg}}>I{{I}_{Na}}$

D) $I{{I}_{Na}}>I{{I}_{Mg}}$

• A) $N>O>Be>B$

B) $N>Be>O>B$

C) $Be>B>N>O$

D) $B>Be>O>N$

• A) ${{M}^{-}}(g)\to M(g)$

B) $M(g)\to {{M}^{+}}(g)$

C) ${{M}^{+}}(g)\to {{M}^{2+}}(g)$

D) ${{M}^{2+}}(g)\to {{M}^{3+}}(g)$

• A) $O$

B) ${{O}_{2}}$

C) $O_{2}^{+}$

D) $O_{2}^{-}$

• A) Ge

B) Se

C) As

D) Br

• A) Less

B) More

C) Equal

D) None of these

• A) Potassium

B) Helium

C) Hydrogen

D) Xenon

• A) Nitrogen

B) Carbon

C) Oxygen

D) Fluorine

• A) $13.6eV$

B) $>13.6eV$

C) $<13.6eV$

D) $1.5eV$

• A) $Mg$

B) $Rb$

C) $Li$

D) $Ca$

• A) I group

B) IV group

C) VII group

D) Zero group

• A) $F\to {{F}^{-}}$

B) $Cl\to C{{l}^{-}}$

C) $O\to {{O}^{2-}}$

D) $H\to {{H}^{-}}$

• A) Increases

B) Decreases

C) Remains same

D) None of the above

• A) $Be,\,B,\,C,\,N$

B) $B,\,Be,\,C,\,N$

C) $C,\,N,\,Be,\,B$

D) $N,\,C,\,Be,\,B$

• A) $1{{s}^{1}}$

B) $1{{s}^{2}},\,2{{s}^{2}}{{p}^{6}}$

C) $1{{s}^{2}},\,2{{s}^{2}}{{p}^{2}}$

D) $1{{s}^{2}},\,2{{s}^{2}}{{p}^{6}},\,3{{s}^{1}}$

• A) C

B) N

C) B

D) O

• A) Na

B) Mg

C) C

D) F

• A) Li > Be >B > Na

B) Be >B > Li > Na

C) Na > Li > B > Be

D) Be > Li > B > Na

E) B > Be > Li > Na

• A) Greater attraction of electrons by the nucleus

B) The size of nitrogen atom being smaller

C) The half-filled $p$-orbitals possess extra stability

D) Greater penetration effect

• A) Same as that of $Na$

B) 5.68 eV

C) 4.34 eV

D) 10.88 eV

• A) Same e/m ratio

B) Same electron affinity

C) Same group

D) Same ionic potential

• A) ${{O}^{-}}$ ion will tend to resist the addition of another electron

B) Oxygen has high electron affinity

C) Oxygen is more electronegative

D) ${{O}^{-}}$ion has comparatively larger size than oxygen atom

• A) It is independent of atomic radii

B) It increases with increase in atomic radii

C) It remains constant with increase in atomic radii

D) It decreases with increase in atomic radii

• A) Highest electron affinity

B) Highest $E_{\text{red}}^{\text{0}}$

C) Highest $E_{\text{oxid}}^{\text{0}}$

D) Lowest electron affinity

• A) Pb

B) Sn

C) Si

D) C

• A) $s>p>d>f$

B) $f>d>p>s$

C) $p<d<s<f$

D) $d>f<s>p$

E) $f>p>s>d$

• A) Li

B) Be

C) B

D) C

• A) ${{K}^{+}},C{{l}^{-}},M{{g}^{2+}},S{{c}^{3+}}$

B) $N{{a}^{+}},C{{a}^{2+}},S{{c}^{3+}},{{F}^{-}}$

C) ${{K}^{+}},C{{a}^{2+}},S{{c}^{3+}},C{{l}^{-}}$

D) $N{{a}^{+}},M{{g}^{2+}},A{{l}^{3+}},Cl$

• A) $F>Cl>Br>I$

B) $F<Cl>Br<I$

C) $F<Cl<Br<I$

D) $F<Cl<Br>I$

• A) B

B) N

C) O

D) Be

• A) $C>N>O$

B) $C>N<O$

C) $C<N>O$

D) $C<N<O$