Classification of Elements and Periodicity in Properties
Test 14

Correct answer Carries: 4.

Wrong Answer Carries: -1.

Which of the following elements is a metalloid in group 15?

In group 15, As is a metalloid, while N (non-metal), P (non-metal), and Bi (metal) are not.

N
P
Bi
As
4

Which of the following elements is an alkaline earth metal?

Alkaline earth metals belong to group 2. Ca is in group 2, while B (group 13), N (group 15), and Cl (group 17) are not.

Ca
B
N
Cl
1

Which element in the fourth period has the highest fifth ionization enthalpy?

Fifth ionization enthalpy peaks when removing an electron from a stable \(\ce{X^4+}\) ion. P (after losing four electrons, becomes \(\ce{P^4+}\) with \(1s^2 2s^2 2p^6\)) has the highest value in period 4.

P
Si
S
Cl
1

Which element has the electronic configuration ending in \(4s^2 4p^3\) in its ground state?

The configuration \(4s^2 4p^3\) corresponds to As (Z=33, period 4, group 15), with full configuration \(1s^2 2s^2 2p^6 3s^2 3p^6 3d^{10} 4s^2 4p^3\).

Ge
As
Se
Br
2

Which group 15 element forms a hydride with the highest bond angle?

Bond angles in group 15 hydrides (\(\ce{NH3}\), \(\ce{PH3}\), \(\ce{AsH3}\), \(\ce{SbH3}\)) decrease down the group due to reduced hybridization. \(\ce{NH3}\) (107°) has the highest bond angle.

P
As
N
Sb
3

Arrange O, S, Se in order of decreasing electronegativity.

Electronegativity decreases down a group due to increasing size. For group 16: O > S > Se.

Se > S > O
O > S > Se
S > O > Se
O > Se > S
2

Which of the following ions has the smallest radius among isoelectronic species with 18 electrons?

For isoelectronic species (\(\ce{K+}\), \(\ce{Ca^2+}\), \(\ce{Sc^3+}\), all with 18 electrons), radius decreases with increasing nuclear charge. \(\ce{Sc^3+}\) (Z=21) has the smallest radius.

\(\ce{Sc^3+}\)
\(\ce{K+}\)
\(\ce{Ca^2+}\)
\(\ce{Cl^-}\)
1

Which of the following is a pnictogen?

Pnictogens are group 15 elements. Sb (group 15) is a pnictogen, while Te (group 16), I (group 17), and Sn (group 14) are not.

Te
I
Sb
Sn
3

Which group 14 element exhibits the maximum tendency to form \(\pi\)-bonds?

Smaller size and higher electronegativity favor \(\pi\)-bonding in group 14. C (period 2) forms \(\pi\)-bonds (e.g., in \(\ce{C2H4}\)) more readily than Si, Ge, or Sn due to effective 2p orbital overlap.

C
Si
Ge
Sn
1

Which pair of elements from different periods shows the least difference in electronegativity?

Diagonal relationships minimize electronegativity differences. Be (1.5, period 2) and Al (1.5, period 3) have nearly identical values, unlike other pairs with larger gaps.

Li, Na
Be, Al
C, Si
N, P
2

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