TIME ALLOTTED : 60 minutes
For every correct answer, you will be awarded +4 marks.
For every wrong answer, -1 marks will be deducted.
For every unattempted question, you will be given 0 marks.
ALL THE BEST
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
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Atomic masses
Nuclear Masses
Atomic numbers
Nuclear neutron-proton number ratios
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Increased attraction of electron towards nucleus
Extra stability of half filled 'p' orbital
Small size of N2
None of the above
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Direct relation
Group relation
Diagonal relation
Linear relation
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I > Br > Cl > F
F > Cl > Br > I
Cl > F > Br > I
Br > Cl > F > I
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Fe3+, Co3+
Fe3+, Mn2+
Co3+, Sr3+
Sc3+, Ti3+
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Ca < S < Ba < Se < Ar
S < Se < Ca < Ba < Ar
Ba < Ca < Se < S < Ar
Ca < Ba < S < Se < Ar
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Li > Na > K > Rb
K > Rb > Li > Na
Li > Na > Rb > K
Rb > Li > K > Na
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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
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K+, Ca2+, Sc3+, Cl-
Na+, Ca2+, Sc3+, F-
K+, Cl-, Mg2+, Sc3+
Na+, Mg2+, Al3+, Cl-
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Electronegativity
Electron affinity
Ionisation energy
Excitation potential
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D and E
C and D
B and C
A and B
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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
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25
50
30
10
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1s2 2s2 2p3
1s2 2s2 2p6 3s1
1s2 2s2 2p6
1s2 2s2 2p5
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Cl- , Ca2+ , K+ , S2-
S2- , Cl- , Ca2+ , K+
Ca2+, K+, Cl- , S2-
K+, S2-, Ca2+, Cl-
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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
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Al3+ > Mg2+ > Na+ > F+ > O2-
Na+ > Mg2+ > Al3+ > O2- > F-
Na+ > F- > Mg2+ > O2- > Al3+
O2- > F- > Na+ > Mg2+ > Al3+
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It forms diatomic molecules
It is a non-metal element
Its valency is 1
It forms basic oxide
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A
B
C
D
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V
Cr
Mn
Fe
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2
1
3
0
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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
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Screening effect increases down the group
Zeff increases down the group
Zeff. increases in a period
All of the above
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Fe
Fe+2
Fe+3
Fe+4
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Atomic radii
Atomic as well as M3+ radii
Valence electron
Oxidation state
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A
B
C
D
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Group number
Electronic configuration
Number of electron present in their d subshells
Both are transition metals
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0
1
2
3
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