Classification of Elements and Periodicity in Properties Set-1

Q1: What physical property did Henry Moseley, in 1913, correlate with the characteristic X-ray spectra of elements to prove that atomic number ($Z$) is a more fundamental property than atomic mass?

Q2: Which chemist noted a similarity among the physical and chemical properties of groups of three elements, known as triads, in the early 1800s?

Q3: Mendeleev's Periodic Law stated that the properties of the elements are a periodic function of their:

Q4: John Alexander Newlands profounded the Law of Octaves in 1865. This law suggested that every eighth element had properties similar to the first element when arranged by increasing order of:

Q5: Which elements, in addition to actinium and protoactinium, were found in pitchblende, an ore of uranium, stimulating renewed interest in Inorganic Chemistry?

Q6: The Modern Periodic Law, which modified Mendeleev’s law, states that the physical and chemical properties of the elements are periodic functions of their:

Q7: The horizontal rows in the Modern Periodic Table are known as:

Q8: According to the recommendation of the International Union of Pure and Applied Chemistry (IUPAC), how are the vertical columns (groups) in the Modern Periodic Table numbered?

Q9: The element Iodine ($\text{I}$) has a lower atomic weight than Tellurium ($\text{Te}$). Mendeleev ignored the order of atomic weights and placed Iodine in Group VII along with Fluorine and Chlorine. This decision was based on:

Q10: What property did Mendeleev predict for Eka-silicon (later Germanium) regarding the formula of its oxide?

Q11: What would be the IUPAC name and symbol for the element with atomic number $Z=120$?

Q12: Using IUPAC nomenclature, the roots for the digits 1, 1, and 4 in the atomic number $Z=114$ are:

Q13: The element with the IUPAC temporary name Unnilhexium has the atomic number:

Q14: What is the permanent official name for the element with the temporary IUPAC name Ununbium ($Z=112$)?

Q15: Elements belonging to Group 1 and Group 2, having outermost electronic configurations $ns^1$ and $ns^2$ respectively, are collectively known as:

Q16: What is the general outer electronic configuration for the $d$-block elements (Transition Elements)?

Q17: The elements characterized by the filling of $f$-orbitals and positioned separately at the bottom of the Periodic Table are the:

Q18: The elements of Groups 13 to 18, along with the $s$-block elements, are collectively referred to as the:

Q19: An element has the electronic configuration $[\text{Rn}]5f^{14}6d^{10}7s^27p^5$. To which family/group would this element ($Z=117$) belong?

Q20: The principal quantum number ($n$) of the seventh period corresponds to the successive filling up of which set of orbitals?

Q21: The lanthanoid series (4$f$-inner transition series) begins with Cerium ($Z=58$) and ends at:

Q22: The period number in the Periodic Table corresponds to which quantum number for the elements in that period?

Q23: The fourth period ($n=4$) contains 18 elements. This is due to the filling of which orbitals in sequential order?

Q24: Based on the configuration $[\text{Ar}]3d^14s^2$, the element Scandium ($Z=21$) is the first element of the:

Q25: The positioning of Helium in the $p$-block along with Group 18 elements is justified because:

Q26: An element has the outer electronic configuration $\text{3s}^2\text{3p}^4$. Where is this element located in the Periodic Table?

Q27: The element with the outer electronic configuration $(n-1)d^2ns^2$ for $n=4$ belongs to which block and group?

Q28: Zinc ($\text{Zn}, Z=30$), Cadmium ($\text{Cd}$), and Mercury ($\text{Hg}$) do not show most properties of transition elements. This is explained by their electronic configuration:

Q29: The elements in the same vertical column (group) of the Periodic Table exhibit similar chemical behavior primarily because they have:

Q30: The maximum theoretical number of elements in the sixth period ($n=6$) is 32. This is because the successive electrons enter which combination of orbitals?