Atomic Theory and Electron Configuration Quiz

A fundamental concept suggesting that matter is composed of tiny, indivisible particles called atoms, meaning "indivisible". This theory was first proposed by Democritus in ancient Greece.

A theory that postulates that matter is composed of tiny indestructible particles called atoms. It suggests that atoms of a given element are identical in mass and properties. This theory was proposed by John Dalton in 1808.

A theory about the nature of matter based on the idea that matter is ultimately composed of indivisible particles called atoms. This theory is continuously evolving with the discovery of new evidences and advancements in technology.

The progression of ideas and concepts related to the structure of matter. This progression begins with ancient philosophers and continues to the present day.

The ability to perceive objects with the naked eye. It is limited by the resolution of our visual system, meaning we cannot see objects smaller than a certain size.

The fundamental building blocks of all matter. They are extremely small and cannot be seen with the naked eye.

Differences in the properties of materials are attributed to the differences in their atoms and how they are arranged. This means that the type of atoms and their arrangement in a material contribute to its unique characteristics.

The study of the composition, structure, properties, and reactions of matter. It explores the fundamentals of the universe and investigates the building blocks and interactions of matter.

The number of protons in the nucleus of an atom, defining its atomic identity.

The arrangement of electrons within the energy levels and sublevels of an atom in its ground state, indicating the distribution of electrons in orbitals.

A set of four quantum numbers (n, l, ml, and ms) that describes the state of an electron within an atom, specifying its energy, shape, spatial orientation, and spin.

The specific arrangement of orbitals within a subshell, indicated by letters (s, p, d, f), each representing a distinct shape and orbital behavior.

Filling atomic orbitals following the Aufbau principle, Hund's rule, and the Pauli exclusion principle, resulting in the most stable electron configuration for an atom.

Elements are grouped based on their similar chemical properties, which are determined by their outer-shell electron configurations. This helps us understand and predict their behavior.

The basis for classifying elements is their electron configurations, specifically the number of valence electrons. Elements with similar valence electron configurations exhibit similar chemical properties.

The two numbering systems for groups are the traditional system using Roman numerals and letters (IA, IIA, etc.) and the modern system using Arabic numerals (1, 2, etc.). The modern system reflects the number of valence electrons.

The first period fills the 1s subshell, which holds a maximum of two electrons. This results in the presence of only two elements in the first period: hydrogen and helium.

Elements are classified into representative, transition, and inner transition elements based on the type of subshell being filled. Representative elements fill the s and p subshells, transition elements fill the d subshells, and inner transition elements fill the f subshells.

Atomic size generally decreases across a period due to increasing nuclear charge pulling the electrons closer. This means elements on the right side of a period are smaller than those on the left.

Elements in Groups 1 and 2 (IA and IIA) are metals because they have low ionization energies, readily losing their valence electrons to form positive ions. Group 17 (VIIA) elements are non-metals because they have high electron affinities and easily gain electrons to become negatively charged.

Group 18 (VIIIA) elements are least reactive because they have a full valence shell, meaning they are stable and do not need to gain or lose electrons to achieve a stable octet.