Question 1

Which electronic subshell is filled in the d block, period 4?&#10;A) 3d&#10;B) 4d&#10;C) 5d

Accepted Answer

The d block of period 4 corresponds to the filling of the 3d subshell, as the d subshell is always one principal quantum number less than the period number in which it is being filled.

Question 2

Find the element with the largest atomic radius:&#10;A) Ca&#10;B) Ba&#10;C) Cs

Accepted Answer

Cs (Cesium) has the largest atomic radius among the given options. This is because atomic size increases as you move down a group in the periodic table. Cs is located below both Ca (Calcium) and Ba (Barium) in Group 1 (the alkali metals), making it the largest in terms of atomic radius.

Question 3

Which combination of atomic properties would lead to a high first ionization potential:
(i) Small radius and high Z_eff
(ii) Large radius and high Z_eff
(iii) Small radius and low Z_eff

A) (i)
B) (ii)
C) (iii)

Accepted Answer

A high first ionization potential is typically associated with atoms that have a small radius and a high effective nuclear charge (Zeff), as this means the valence electron is closer to the nucleus and more strongly attracted to it, making it harder to remove.

Question 4

What can we say about an element's occurrence if we know it is a chalcophile element?&#10;A) The element occurs in silicate minerals.&#10;B) The element is found in sulfide minerals.&#10;C) The element is found in both oxides and sulfides.

Accepted Answer

Chalcophile elements have an affinity for sulfur and are typically found in sulfide minerals rather than in silicate minerals or oxides. This affinity is due to their chemical properties, which make them more likely to bond with sulfur.

Question 5

What can be said about the stability of high oxidation states within a group:&#10;A) The stability of high oxidation states increases down a group as the atomic radii increase.&#10;B) The stability of high oxidation states decreases down a group as the first ionization potential increases.&#10;C) The stability of high oxidation states remains more-or-less constant down a group.

Accepted Answer

The stability of high oxidation states increases down a group due to the increase in atomic radii. This is because larger atoms can distribute the charge over a larger volume, reducing the energy penalty associated with high oxidation states.

Question 6

Classify the following hydrides: (i) SiH₄, (ii) PH₃ and (iii) AsH₃ A) (i) is saline, (ii) and (iii) are metallic B) all are metallic C) all are molecular

Accepted Answer

The given hydrides are of silicon (SiH4), phosphorus (PH3), and arsenic (AsH3), which are all non-metals. Hydrides of non-metals are molecular (covalent) in nature, hence all are molecular.

Question 7

Which of the following oxides is basic? A) CaO B) CrO₃ C) P₄O₁₀

Accepted Answer

CaO (Calcium oxide) is a basic oxide because it reacts with water to form calcium hydroxide, which is a base.

Question 8

Zirconium forms two binary chlorides while molybdenum forms five. How can we explain this difference?&#10;A) Zirconium has a smaller radius and lower number of possible coordination numbers.&#10;B) Ionization energies of zirconium are higher than that for molybdenum.&#10;C) Zirconium has fewer accessible oxidation states than molybdenum.

Accepted Answer

Zirconium has fewer accessible oxidation states compared to molybdenum, which allows molybdenum to form a wider variety of binary chlorides by utilizing its multiple oxidation states.

Question 9

What is diagonal similarity?&#10;A) Similarity between the element at the head of a group and the element to its lower right&#10;B) Similarity between the element at the head of a group and the element to its lower left&#10;C) Similarity between the element in a group and the element to its lower right.

Accepted Answer

The answer of What is diagonal similarity?&#10;A) Similarity between the...

Question 10

Which pair of elements have similar properties according to the Z + 8 rule?&#10;A) Si and V&#10;B) S and Mn&#10;C) P and V

Accepted Answer

The Z + 8 rule suggests that elements with atomic numbers differing by 8 have similar properties. Phosphorus (P) has an atomic number of 15, and Vanadium (V) has an atomic number of 23. The difference in their atomic numbers is 8, making P and V a pair with similar properties according to this rule.

Deck 9: Periodic Trends