Nomenclature of Elements with Atomic Numbers > 100 - Free MCQ Practice

The element of Copernicium’s atomic number is 112. it is otherwise called as Ununbium as per the IUPAC nomenclature. The name Copernicium is given after the astronomer Nicolaus Copernicus. It’s a d-block transactinide element that belongs to Group-12.

The correct answer to this question is option B, the 14 elements after actinium are called Actinides. Let us see what each of the options stands for to understand the answer in a better way.
First, let us see the series of elements lanthanides includes. Lanthanides are those elements which are in between atomic number 57 and 71. All the elements between atomic number 57 and 71 come under lanthanide series.
The series of lanthanides starts from element lanthanum which has the atomic number 57 and ends at the element lutetium which has the atomic number 71.
Second, actinides are those elements which are in between 89 and 103, starting from the element actinide which has the atomic number 89 and ending with the element lawrencium which has the atomic number 103.
Groups that come under atomic number 3 to 12 of the periodic table are called d-block elements. They are called d-block elements because d subshells are filled in the elements that come under d-block.
Groups that come under atomic number 13 to 18 of the periodic table are called p-block elements. They are called p-block elements because p subshells are filled in the elements that come under p-block.

Option D is correct.

The element with atomic number 11 is sodium (Na), which is a metal in Group 1.

Metals generally form basic oxides because they give ionic oxides that produce hydroxide ions on reaction with water.

Na forms the oxide Na₂O.

Na₂O + H₂O → 2 NaOH

In ionic terms, sodium atoms form Na⁺ ions and oxygen forms the oxide ion O^2-; the oxide reacts with water to produce OH^- (as part of NaOH), so the oxide is basic.

By contrast, the other choices give non-metal or metalloid oxides: atomic number 7 (nitrogen) and 17 (chlorine) form mainly acidic oxides, and atomic number 14 (silicon) forms SiO₂, which is an acidic oxide. Therefore only atomic number 11 yields a basic oxide.

Mendeleev placed elements like iodine and tellurium based on similar properties rather than atomic weight. This confirms that similarity in properties was given priority.

Newlands → Octaves
Moseley → Modern periodic law (atomic number)
Mendeleev → Atomic weight-based law
Dobereiner → Triads

Answer: A

Statement 1 is correct. The Modern Periodic Law states that the chemical and physical properties of elements are a periodic function of their atomic number.

Statement 2 is correct. The atomic number (the number of protons and, in neutral atoms, electrons) determines chemical behaviour and is therefore more fundamental than atomic mass. Ordering by atomic number resolves anomalies that appeared when elements were arranged strictly by mass.

Statement 3 is correct. Moseley's measurements of X-ray frequencies showed a systematic relation with atomic number, providing the experimental basis for the modern law.

Statement 4 is not correct. Mendeleev formulated the earlier periodic law based on atomic mass, not the atomic-number-based modern law.

Therefore the correct choice is A: 1, 2 and 3 only.

Across a period, nuclear charge increases while shielding remains nearly constant, leading to stronger attraction and higher ionization enthalpy.