The question asks for the definition of a 'GROUP' in the modern periodic table. We need to recall the organization principles of the periodic table, specifically how elements are arranged in groups and periods, and what properties they share.
B) A vertical column; all elements in a group have the same number of valence electrons and same general electronic configuration of the outermost shell, hence similar chemical properties. This statement accurately describes a group in the modern periodic table and explains why elements within a group exhibit similar chemical behavior.
To locate an element in the periodic table given its atomic number (Z), we need to determine its period and group. The period is determined by the highest principal quantum number (n) of the valence electrons, and the group is determined by the number of valence electrons and the type of subshell being filled.
Correct Option: B) Period 7 and Group 14 (p-block) — element Flerovium (Fl); configuration [Rn] 5f¹⁴ 6d¹⁰ 7s² 7p²
The question asks about the placement of Hydrogen in the modern periodic table and why it is considered anomalous. To answer this, we need to recall the properties of Hydrogen and compare them with the properties of elements in Group 1 (alkali metals) and Group 17 (halogens).
C) Hydrogen is placed in Group 1 (with alkali metals) but is anomalous — it also resembles halogens (Group 17) as it can gain one electron to form H⁻ and is a non-metal. This option accurately describes Hydrogen's placement and its anomalous properties, highlighting its similarities to both Group 1 and Group 17 elements.
The question asks to identify the s-block elements in the modern periodic table. This requires knowledge of the classification of elements into blocks (s, p, d, f) based on the orbital in which the last electron enters, and their corresponding group numbers.
Correct Option: D) Groups 1 and 2 (alkali metals and alkaline earth metals) — their valence electrons are in the s-orbital; general configurations \(ns^1\) (Group 1) and \(ns^2\) (Group 2)
The question asks to identify the p-block elements in the modern periodic table. This requires knowledge of the classification of elements into s, p, d, and f blocks based on their electronic configurations and their corresponding group numbers.
Correct Option: D) Groups 13 to 18 — elements whose outermost electrons occupy the p-orbital; configurations ns²np¹ to ns²np¶. This accurately describes the p-block elements, their group numbers, and their characteristic valence electron configurations.
The question asks about the characteristics and placement of d-block elements (transition metals) in the modern periodic table. To answer this, we need to recall the definition of d-block elements, their group numbers, and their general electronic configuration.
A) Groups 3 to 12 in the modern periodic table — their last electron enters the d-orbital; general configuration \((n-1)\text{d}^{1-10} \text{ns}^{0-2}\). This option correctly identifies the groups (3 to 12), the characteristic filling of the d-orbital by the last electron, and provides the accurate general electronic configuration for d-block elements. For example, Scandium (Sc) in Group 3 has the configuration \([\text{Ar}]3\text{d}^1 4\text{s}^2\), and Zinc (Zn) in Group 12 has \([\text{Ar}]3\text{d}^{10} 4\text{s}^2\).