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  4. Classification of Elements and Periodicity in Properties Chapter-Wise Test 3

Classification of Elements and Periodicity in Properties Chapter-Wise Test 3

Correct answer Carries: 4.

Wrong Answer Carries: -1.

What is the general outer electronic configuration of d-block elements?

d-block elements (groups 3–12) have electrons filling \((n-1)d\) orbitals, with outer configuration \((n-1)d^{1-10} ns^{0-2}\).

\(ns^{1-2}\)
\(ns^2 np^{1-6}\)
\(ns^2 np^6\)
\((n-1)d^{1-10} ns^{0-2}\)
4

Which group 2 element forms a hydroxide with the lowest solubility in water?

Solubility of group 2 hydroxides increases down the group due to decreasing lattice energy. \(\ce{Be(OH)2}\) has the lowest solubility due to Be’s small size and high charge density.

Mg
Ca
Sr
Be
4

Which of the following fluorides has the highest ionic character?

Ionic character increases with larger cation size and lower polarizing power in group 2. \(\ce{BaF2}\) (Ba²⁺, largest) has the highest ionic character among BeF₂, MgF₂, CaF₂, and BaF₂.

\(\ce{BeF2}\)
\(\ce{BaF2}\)
\(\ce{MgF2}\)
\(\ce{CaF2}\)
2

Arrange the following elements in order of increasing metallic character: Si, P, S, Cl.

Metallic character decreases across period 3 due to increasing nuclear charge. Order: Cl < S < P < Si.

Si < P < S < Cl
Cl < S < P < Si
S < Cl < P < Si
P < Si < Cl < S
2

Which group 17 element has the highest electron affinity despite not having the most negative electron gain enthalpy?

Electron affinity is the energy change for \(\ce{X + e^- -> X^-}\). Cl has the highest electron affinity due to its balance of size and nuclear charge, though F’s electron gain enthalpy is less negative due to repulsion.

F
Br
Cl
I
3

Which of the following has the highest lattice energy among group 2 fluorides?

Lattice energy increases with smaller ionic radii (higher charge density). BeF₂ has the highest lattice energy in group 2 due to Be²⁺’s small size, compared to MgF₂, CaF₂, or SrF₂.

\(\ce{MgF2}\)
\(\ce{BeF2}\)
\(\ce{CaF2}\)
\(\ce{SrF2}\)
2

Which element has the electronic configuration \(1s^2 2s^2 2p^6 3s^1\)?

Total electrons = 11, corresponding to Na (period 3, group 1). Others: Mg (12 electrons), Al (13 electrons), Ne (10 electrons).

Mg
Na
Al
Ne
2

Which element in the fourth period has the highest electronegativity?

Electronegativity increases across a period. In period 4 (K to Kr), Br (group 17) has the highest electronegativity among K, Ca, and Br.

K
Ca
Br
Kr
3

Which element in group 16 has the most negative electron gain enthalpy?

Electron gain enthalpy becomes more negative across a period and less negative down a group. In group 16, O (period 2) has the most negative value compared to S, Se, and Te.

O
S
Se
Te
1

Which element in group 15 has the highest tendency to form stable compounds in the +3 oxidation state?

The +3 oxidation state becomes more stable down group 15 due to the inert pair effect. Bi forms stable \(\ce{BiCl3}\) (+3), more so than N, P, or As, where +5 is also common.

Bi
N
P
As
1

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