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Aug 13, 2022 · One scientific law that provides the foundation for understanding in chemistry is the law of conservation of matter. It states that in any given system that is closed to the transfer of matter (in and out), the amount of matter in the system stays constant.
- History
- Octet Rule Examples
- Why The Octet Rule Works
- Exceptions to The Octet Rule
- Uses of The Octet Rule
- Alternatives to The Octet Rule
- References
American chemist Gilbert N. Lewis proposed the octet rule in 1916. Lewis observed that noble gases, with their full valence shells of eight electrons, were especially stable and unreactive. He hypothesized that other elements achieve similar stability by sharing, gaining, or losing electrons to reach a filled shell. This led to his formulation of t...
Atoms follow the octet rule by either donating/accepting electrons or by sharing electrons. 1. Donating/Accepting Electrons: Sodium, a member of the alkali metals, has one electron in its outermost shell and eight electrons in the next shell. To achieve a noble gas configuration, it donates the one electron, resulting in a positive sodium ion (Na+)...
The octet rule works because of the nature of electron configuration in atoms, specifically in relation to the stability provided by a full valence shell. Electrons in atoms are organized into energy levels, or shells, and each shell has a maximum capacity of electrons it holds. The first energy level holds up to 2 electrons, the second holds up to...
There are exceptions to the octet rule, particularly for elements in the third period and beyond on the periodic table. These elements accommodate more than eight electrons because they have d and f orbitals in their valence shells. Here are a few examples of elements that do not strictly follow the octet rule: 1. Hydrogen: It only accommodates 2 e...
The primary benefit of the octet rule is its simplicity and broad applicability. It allows for a straightforward understanding of molecular structures and chemical reactions, making it a powerful tool in the early stages of chemical education.
However, the rule is not all-encompassing. The octet rule doesn’t apply well to many molecules, including those with an odd number of electrons like nitric oxide (NO), and compounds of transition metals. Furthermore, it does not account for the relative strengths of covalent bonds and the variation in bond lengths. So, there are alternatives to the...
Abegg, R. (1904). “Die Valenz und das periodische System. Versuch einer Theorie der Molekularverbindungen (Valency and the periodic system – Attempt at a theory of molecular compounds)”. Zeitschrif...Frenking, Gernot; Fröhlich, Nikolaus (2000). “The Nature of the Bonding in Transition-Metal Compounds”. Chem. Rev. 100 (2): 717–774. doi:10.1021/cr980401lHousecroft, Catherine E.; Sharpe, Alan G. (2005). Inorganic Chemistry(2nd ed.). Pearson Education Limited. ISBN 0130-39913-2.Langmuir, Irving (1919). “The Arrangement of Electrons in Atoms and Molecules”. Journal of the American Chemical Society. 41 (6): 868–934. doi:10.1021/ja02227a002Learn about the conservation of mass in physical and chemical reactions in this guide for students aged 11 to 14 from BBC Bitesize.
Solutions are mixtures made when a solute dissolves into a solvent. Learn about solutions in this Key Stage 3 chemistry guide aged from BBC Bitesize.
Jun 4, 2024 · The oxidation number (also known as oxidation state) is a number given to each atom or ion in a compound to keep track of how many electrons they have. In a single ion or molecular ion, the oxidation number tells us how many electrons have been lost or gained. Positive oxidation number = loss of electrons.
Nov 7, 2019 · Here are brief summaries of the most important laws, the foundational concepts, and principles of chemistry: Avogadro's Law. Equal volumes of gases under identical temperature and pressure will contain equal numbers of particles (atoms, ions, molecules, electrons, etc.). Boyle's Law.
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A slightly soluble electrolyte begins to precipitate when the magnitude of the reaction quotient for the dissolution reaction exceeds the magnitude of the solubility product. Precipitation continues until the reaction quotient equals the solubility product.
