Periodic Table And Structure Of Atom- Combined Test

N=3, l=1, m=1, s=+1/2

N=3, l=2, m=1, s=+1/2

N=4, l=0, m=0, s=+1/2

N=3, l=0, m=0, s=+1/2

D and E

C and D

B and C

A and B

N=4, l=3, m=+4, s=+1/2

N=4, l=4, m=-4, s=-1/2

N=4, l=3, m=+1, s=+1/2

N=3, l=2, m=-2, s=+1/2

K⁺, Ca²⁺, Sc³⁺, Cl^-

Na⁺, Ca²⁺, Sc³⁺, F^-

K⁺, Cl^-, Mg²⁺, Sc³⁺

Na⁺, Mg²⁺, Al³⁺, Cl^-

Ca < S < Ba < Se < Ar

S < Se < Ca < Ba < Ar

Ba < Ca < Se < S < Ar

Ca < Ba < S < Se < Ar

Cl^- , Ca²⁺ , K⁺ , S^2-

S^2- , Cl^- , Ca²⁺ , K⁺

Ca²⁺, K⁺, Cl^- , S^2-

K⁺, S^2-, Ca²⁺, Cl^-

I > Br > Cl > F

F > Cl > Br > I

Cl > F > Br > I

Br > Cl > F > I

Al³⁺ > Mg²⁺ > Na⁺ > F⁺ > O^2-

Na⁺ > Mg²⁺ > Al³⁺ > O^2- > F^-

Na⁺ > F^- > Mg²⁺ > O^2- > Al³⁺

O^2- > F^- > Na⁺ > Mg²⁺ > Al³⁺

Reactivity decreases in the alkali metals but increases in the halogens with increase in atomic number down the group

In both the alkali metals and the halogens the chemical reactivity decreases with increase in atomic number down the group

Chemical reactivity increases with increase in atomic number down the group in both alkali metals and halogens

In alkali metals, the reactivity increases but in the halogens it decreases with increase in atomic number down the group

Atomic masses

Nuclear Masses

Atomic numbers

Nuclear neutron-proton number ratios

V

Cr

Mn

Fe

It forms diatomic molecules

It is a non-metal element

Its valency is 1

It forms basic oxide

1s² 2s² 2p³

1s² 2s² 2p⁶ 3s¹

1s² 2s² 2p⁶

1s² 2s² 2p⁵

Atomic radii

Atomic as well as M³⁺ radii

Valence electron

Oxidation state

Electronegativity

Electron affinity

Ionisation energy

Excitation potential

Increased attraction of electron towards nucleus

Extra stability of half filled 'p' orbital

Small size of N₂

None of the above

Al³⁺ < Mg²⁺ < Na⁺ < F^- : Increasing ionic size

B < C < N < O : increasing first ionization energy

I < Br < F < Cl - increasing electron gain enthalpy (With negative sign)

Li < Na < K < Rb - increasing metallic radius

Fe³⁺, Co³⁺

Fe³⁺, Mn²⁺

Co³⁺, Sr³⁺

Sc³⁺, Ti³⁺

Direct relation

Group relation

Diagonal relation

Linear relation

Li > Na > K > Rb

K > Rb > Li > Na

Li > Na > Rb > K

Rb > Li > K > Na

Occur only within the same period

Have identical atomic mass(weight)

Have identical number of neutrons

Have the same number of electrons in the outer shell

Group number

Electronic configuration

Number of electron present in their d subshells

Both are transition metals

Screening effect increases down the group

Zeff increases down the group

Zeff. increases in a period

All of the above

+1/2, +1/2

-1/2 , +1/2

-1/2 , -1/2

0,1

0

1

2

3