All About Trends In Physical And Chemical Properties

The periodic table arranges the elements according to their increasing atomic number. All of these elements exhibit a variety of different trends, and we may utilize the periodic table and the periodic law to comprehend and anticipate the elements’ chemical, physical, and atomic properties.

To comprehend the trend, you must first evaluate the electron configuration of the element. All elements prefer an octet configuration and will add or lose electrons to achieve this stable structure. Now, let’s take a closer look at some of the periodic qualities of elements and the trends in these features as they relate to the periodic table.

Periodic trends are unique patterns in the properties of chemical elements that are seen in the periodic table of elements. Major periodic patterns include electronegativity, ionization energy, electron affinity, atomic radii, ionic radius, metallic character, and chemical reactivity. 

Period Trends 

1. Atomic radius 
2. Ionic radius 
3. Ionization energy 
4. Electron gain enthalpy 
5. Electronegativity 
6. Electron affinity

Atomic Radius 

atomic radius, half the distance between identical neighboring atoms’ nuclei in an element’s solid-state. Although an atom does not have a strict spherical shape, it can be conceived of as a small, compact positive nucleus surrounded by a diffuse negative cloud of electrons. The value of atomic radii varies according to the sort of chemical bond formed by the atoms (metallic, ionic, or covalent bond). When adjacent atoms are not identical, as in sodium chloride, a portion of the observed distance between atoms is attributed to one type of atom and the remainder to the other.

Ionic Radius 

The ionic radius (plural: ionic radii) is a unit of length used to describe the ion of an atom in a crystal lattice. It is the reciprocal of the distance between two ions that are barely touching. Because the boundary of an atom’s electron shell is somewhat hazy, ions are frequently represented as solid spheres fixed in a lattice.

The ionic radius may be more or lesser than the atomic radius (radius of an element’s neutral atom), depending on the ion’s electric charge. Cations are typically smaller than neutral atoms due to the removal of an electron and the remaining electrons being brought in closer to the nucleus. An anion contains one extra electron, which expands the electron cloud and may cause the ionic radius to exceed the atomic radius.

Ionization Energy 

In chemistry and physics, ionization energy is the amount of energy necessary to remove an electron from an isolated atom or molecule. Each consecutive electron withdrawn has corresponding ionization energy; nevertheless, the ionization energy associated with the removal of the first (most loosely held) electron is most frequently utilized.

The ionization energy of a chemical element, denoted in joules or electron volts, is often determined in an electric discharge tube by colliding a fast-moving electron created by an electric current with a gaseous atom of the element, ejecting one of its electrons. (Typically, chemists use joules, whereas physicists use electron volts.)

Electron Gain Enthalpy 

An element’s electron gain enthalpy is the energy produced when a neutral isolated gaseous atom accepts an additional electron to create a gaseous negative ion or anion. It is denoted by the symbol ∆egH. The more energy released in the preceding process the greater the element’s electron gain enthalpy. An element’s electron gain enthalpy is a measure of the firmness or strength with which an additional electron is bonded to it. It is expressed in terms of electron volts per atom or kilojoules per mole. When an electron is added to an atom, the reaction can be endothermic or exothermic.

Electronegativity 

Electronegativity, denoted by the symbol X, is the tendency of an atom of a certain chemical element to attract electrons from other atoms while forming a chemical bond with another atom. The electronegativity of an atom is influenced by two factors: the atomic number of the atom and the distance between its valence electrons and the positively charged nucleus.

Electron Affinity

In chemistry, the amount of energy released when an electron is added to a neutral atom to form a negatively charged ion is referred to as the affinity of the electron. It is difficult to measure the electron affinities of atoms; as a result, only a limited number of chemical elements, mostly halogens, have had their values determined. These values were derived through measurements of the temperatures of formation and lattice energies of ionic compounds of the elements’ constituent elements. Element electron affinity is a measure of an element’s tendency to act as an oxidizing agent (an electron acceptor), and it is often related to the type of chemical bonds that that element forms with other elements. 

Conclusion 

Periodic trends are unique patterns in the properties of chemical elements that are seen in the periodic table of elements. Major periodic patterns include electronegativity, ionization energy, electron affinity, atomic radii, ionic radius, metallic character, and chemical reactivity. Ionization energy is the amount of energy necessary to remove an electron from an isolated atom or molecule. It is often determined in an electric discharge tube by colliding a fast-moving electron created by an electric current with a gaseous atom of the element, ejecting one of its electrons.