Found 12 Articles for Classification of Elements and Periodicity in Properties

Introduction Atoms are the tiniest building pieces of elements or the simplest material that can be subsequently chemically degraded. The periodic table of elements is a depiction of atoms as well as elements in a certain order. Atoms are made up of protons (p), neutrons (n), and electrons (𝑒−) . Atomic mass (A) is extremely important in establishing the element's composition as well as relevance. What is Atomic Mass? The mass of protons (p) plus neutrons (n) in an atom is defined as the atomic mass. The atomic mass (A) of an element is described as its entire mass. The ... Read More

Introduction An atom's electrical configuration shows how many electrons are in each subshell that surrounds its nucleus. The greatest number of electrons that can be found in the orbitals, which are represented by the symbols s, p, d, and f, are 2, 6, 10, and 14. The notation is used to describe the subshell's number of electrons. The shell number, the identity of the subshell, and the overall number of electrons in the subshell are all written in superscript. Electronic configuration, often called electronic structure, is the configuration of electrons in different energy levels surrounding an atomic nucleus. What is ... Read More

Introduction The quantity of energy released or absorbed when a neutral isolated gaseous atom absorbs an $\mathrm{e^{-}}$ to create a negatively charged anion is described as electron gain enthalpy. When the $\mathrm{e^{-}}$ joins with the isolated gaseous atom, energy can be produced or absorbed, depending on whether the process is exothermic or endothermic. The greater the energy released during the mixing process, the greater the electron gain enthalpy, indicated as 𝛥𝐻𝑒𝑔. $$\mathrm{X(g)\:+\:e^{-}\rightarrow\:X^{-}(g)}$$ Normally, exothermic processes occur, resulting in a negative electron gain enthalpy. Because halogens only require one atom to achieve the noble gas configuration, they have a substantially negative ... Read More

Introduction Jöns Jacob Berzelius proposed the word "electronegativity" in 1811. The propensity of an atom of a particular chemical element to draw the shared pair of electrons when a chemical connection is formed is called electronegativity. The symbol for it is X. The bond energy, the direction and strength of a bond's chemical polarity, and other bond properties can all be quantitatively estimated using electronegativity. It is unusual for the more electronegative atom to fully dominate the bond pair of electrons in covalent bonds where there is a significant difference in the electronegativities of the bound atoms, leading to ... Read More

Introduction Ionization energy (I.E.) is described as the minimum (min) required energy (e) to remove (throw out) the most loosely (weakly) bounded electron (e) of an isolated gaseous (g) atom, +ve ion, or molecule. Ionization energy (I.E) follows periodicity in the modern periodic table. The normal or general trend is that the ionization energy (I.E) increases on moving from left (l) to right (r ) across the period (p). And, on moving from the top (t) to bottom (b) across a group (g), ionization energy decreases or reduces. There are also certain exemptions to (I.E.) ionization energy. What ... Read More

Introduction All known living or non-living things are classified and arranged based on their characteristics. Like different plants and animals are classified and organised into groups and species likewise many scientists tried to set the bases of the elements on their atomic number or atomic mass. Many scientists fail to arrange the elements properly. The elements are arranged according to periodic properties and atomic numbers in that table. Several scientists worked to arrange elements, but Mendeleev’s Table worked well. Mendeleev’s periodic table was later modified by atomic numbers by the scientist Henry Moseley. Brief History of Periodic Table ... Read More

Introduction An atom's electrical configuration is determined by how its electrons are arranged in orbitals and shells. The energy required to remove an e^- from an atom is what determines whether an orbital is stable. An orbital is more stable the higher its energy level. The quantity of protons there in the nucleus determines the electronic structure of an atom. The atomic no. of an atom is based on how many protons are present in its nucleus. The no. of electrons in an atom is also based on how many protons are present in its nucleus. Standard Notation of Electron ... Read More

Introduction Electronegativity is the ability of an atom or any individual atom to attract(force) shared electrons (e-) or electron density while forming a bond(chemical). The electronegativity of any individual atom can be affected by two factors, and they are- its atomic number (Z) and the distance(separation) at which its valence (complete octet) electrons stay from (away) the charged nucleus. We can also determine the electronegativity of an atom with the help of some factors like nuclear charge, the number of electrons in the atomic shell, etc. Generally, electronegativity increases when we move or go from left (l) to right ... Read More

Introduction Electronegativity can be described as the capability of an atom (inside a molecule) to attract (force) the electrons (shared ones) towards itself at the time of bond formation. The electronegativity of an atom can be affected (varies) by its atomic number (Z) and, also the distance from where the valence electrons stay or are found to be present in the charged nucleus. Electronegativity is useful in the estimation of the bond energy. Electronegativity for an element can be determined with the help of some scales like the Mulliken scale, polling scale, and Allred Roschow’s scale. A polling scale ... Read More

Introduction Electron gain enthalpy is the energy change process during the addition of an electron to an isolated atom. The ability to add an electron and form an anion refers to electron affinity. The elements undergoing this energy change or addition of electrons are due to acquiring stable electronic configuration. Here, Chlorine undergoes the addition of an electron for a stable octet. The electron affinities and negative ions or anions mainly belong to groups 6th and 7th of the periodic table. It has either negative or positive values depending on the size and nuclear charge of the elements. For ... Read More