Test: Atomic Structure - SSC CGL MCQ

The fundamental unit of an element that participates in a chemical reaction is an atom. Atoms consist of electrons, protons, and neutrons. Each element is made up of unique atoms that determine its properties and behavior in chemical reactions.

The neutron was discovered by James Chadwick. Neutrons are neutral particles found in the nucleus of an atom alongside protons. Their discovery contributed significantly to our understanding of atomic structure and nuclear interactions.

The atomic number of an element is equal to the number of protons present inside the nucleus of its atom. It defines the element's identity and determines its placement on the periodic table based on the number of protons in its nucleus.

Dalton's Atomic Theory proposed that all matter is made up of indivisible and indestructible atoms, and all atoms of a given element have identical properties, including identical mass. This theory laid the foundation for modern atomic theory by emphasizing the concept of elements being composed of identical atoms.

Thomson's Atomic Model couldn't explain the origin of the spectral series of hydrogen and other atoms. This limitation led to the need for further developments in atomic theory, eventually leading to the Rutherford and Bohr models, which provided more accurate descriptions of atomic structure.

The Infrared Region of the electromagnetic spectrum is mainly associated with heat radiation. This region includes frequencies beyond the visible light spectrum, and objects emit infrared radiation as heat. Infrared radiation is commonly used in various applications, including thermal imaging and heat detection.

As per the distribution rules suggested by Bohr and Burry, the maximum number of electrons that can be accommodated in the outermost orbit of an atom is 8. This principle is crucial in understanding the electron configuration of atoms and how electrons are distributed across different energy levels.

The Azimuthal Quantum Number (l) determines the subshell (s, p, d, f) in a given principal energy level of an atom. It helps in specifying the shape and type of the orbital within a particular energy level, providing important information about the distribution of electrons in an atom.

The Aufbau Principle states that electrons enter the orbital of lowest energy first, followed by subsequent electrons in increasing energy order. This principle guides the arrangement of electrons in atoms based on their energy levels, helping to understand the stability and structure of atomic configurations.

Some heavy elements exhibit the property of radioactivity, where they disintegrate into lighter elements by emitting radiation. This process was discovered by Henri Becquerel in 1896. Radioactivity is a crucial concept in nuclear physics and has various applications in different fields, including medicine, archaeology, and industry.

β-rays consist of fast-moving electrons. These electrons are emitted during the process of beta decay, which is a type of radioactive decay. Understanding the properties and behaviors of β-rays is essential in the study of nuclear physics and radiation.

Soddy Fajan's Group Displacement Law states that when an α-particle is emitted, a new element is formed two places to the left of the parent element in the periodic table. This law helps in understanding the relationship between radioactive decay and the formation of new elements in the decay series.

The positron is a positively charged counterpart of the electron, discovered by Anderson in 1932. It plays a crucial role in particle physics and is involved in various interactions within the atomic and subatomic realms.

Planck's Quantum Theory states that the energy of a quantum of radiation is directly proportional to its frequency. This relationship is expressed by the equation E = hν, where E is energy, ν is frequency, and h is Planck's constant. This theory revolutionized the understanding of energy at the atomic and subatomic levels.

Pauli's Exclusion Principle, proposed by Wolfgang Pauli, establishes that no two electrons in an atom can have the same set of four quantum numbers. This principle is fundamental in understanding the behavior of electrons in atoms and plays a crucial role in determining the electron configurations of elements.