Overview of Periodic Trends in Properties of Elements

Periodic trends are distinct patterns in the behaviour of chemical elements that can be found in the periodic table. Electronegativity, ionisation energy, electron affinity, atomic radii, ionic radius, metallic character, and chemical reactivity are all major periodic patterns.

Variations in the atomic structure of chemical elements within their respective periods (horizontal rows) and groups (vertical columns) in the periodic table give birth to periodic trends. Depending on their atomic structures and properties, these principles allow the chemical elements to be grouped in the periodic table. The unknown characteristics of every element can be extrapolated in part because of periodic trends.

Periodic Trends In Properties Of Elements

Periodic trends are the explanations for certain characteristics of elements in the periodic table. Electronegativity, ionic radius, atomic radius, electron affinity, ionisation energy, chemical reactions of elements, and metallic properties are some of the periodic trends.

Period and Group

• Periods are items that are organised horizontally (from left to right).
• A group is made up of pieces that are arranged vertically (from top to bottom).

Factors Influencing Periodic Trends

The periodic patterns are influenced by the overall amount of protons in the nucleus, the overall amount of energy levels, and the shielding effects.

Electronegativity

Electronegativity is the ability of an atom to attract a shared pair of electrons towards itself. The electronegativity of elements is affected by the size of an atom and its nuclear charge. It rises as we move from the left to the right side of the periodic table and falls as we move from the top to the bottom.

The electronegative value of fluorine is higher, while the electronegative value of caesium is lower. It also differs between metals and nonmetals. Non-metals have a higher electronegative potential than metals. It also aids in the identification of the different sorts of bonds that exist between the components.

Ionic Radius

Ionic radius is described as the radius of the ions of the components present in the periodic table. Ions are produced either by gaining or losing electrons of an atom.The ionic radius is the distance between the nucleus’s centre and the ion’s greatest end. The ionic radius of anions is greater than that of cations. When the atomic number is raised, the ionic radius rises with it. Because of the greater atomic number, potassium ions have a larger ionic radius than lithium ions.

Atomic Radius

The size of an atom is evaluated by observing the distance between the nucleus and the atom’s outermost electron.

As we move from the left to the right side of the periodic table, it reduces, and as we keep moving from the top to the bottom, it increases. The concept of atomic radius can be used to ascertain covalent radius (for non-metals) and metallic radius (for metals). The number of protons and the attraction between electrons and protons are also factors.

Electron Affinity

When electrons are added to a neutral gaseous atom, a certain quantity of energy is released. Electron affinity is the term for this. Electron affinity causes a negative ion or anion to form. The periodic table shows that it climbs from left to right and declines from top to bottom. Electron affinity reduces as atomic size increases, and vice versa. The electron affinity is further affected by the screening effect and the reactivity of non-metals.

Ionisation Energy

Because it is difficult to eliminate one electron from an atom, ionisation energy is defined as the greatest energy necessary to do it. This ionisation energy determines the chemical bonding and molecular shape. From top to bottom of the periodic table, it climbs from left to right and declines.

Metallic Character 

The characters linked with the metals seen on the periodic table are referred to as metallic characters. Metallic lustre, hardness, malleability, thermal conductivity, and other characteristics are among them.

The elements that are found on the periodic table’s left side have a higher metallic quality. The addition of electrons causes it to drop from left to right, while the removal of electrons causes it to grow from top to bottom. The skill to lose electrons increases as the atomic number increases.

Melting Point

The melting point is the total energy necessary to transform a solid substance into a liquid. When the link in between atoms of elements is strong, it takes a lot of energy to break it.

As we proceed from top to bottom, it gets smaller. For non-metals, however, it rises from the top to the bottom of the periodic table.

Amongst metals, carbon does have a high melting point. Boron is a semimetal with a high melting point. Tungsten is a metal with a high melting point.

Chemical Element

A chemical element, often known as an element, is a substance that cannot be broken down or converted into another substance through chemical processes. Elements can be regarded as the fundamental chemical components of matter. There are a total of 118 elements that have been identified. The number of protons in each element’s atomic nucleus is used to identify it. By adding extra protons to an atom, a new element can be generated. The atomic number, or Z, of atoms in the same element is the same.

• A chemical element is a material that contains only one atom type. To put it another way, every atom in an element has the same number of protons.
• A chemical element’s identity cannot be altered by any chemical process. A nuclear reaction, on the other hand, can change one element into another.
• The building units of matter are known as elements. True, but it’s worth remembering that an element’s atoms are made up of subatomic particles.
• There are a total of 118 elements that have been identified. It is still possible to synthesise new elements.

Ionic Radius

The electrons in an ion’s many shells and the nucleus make up the ion. The ionic radius of an ion is the distance between both the nucleus and also the electron in the ion’s last outermost shell. There is a tendency that may be seen in the periodic table based on the ionic radius of different elements. This pattern can be summarised as follows

• The ionic radius of the elements increases in value as we proceed down the periodic table from top to bottom. This occurs because the number of layers or shells of electrons increases as we proceed down the periodic table.
• The ionic radius tends to shrink as we move sideways from left to right on the periodic table. Even though it appears strange that as additional protons, electrons, and neutrons are added, the ionic size decreases. Unfortunately, this occurs since metals shed their outer electron layers as we move sideways on the periodic table in order to generate cations.

Conclusion

The periodic table is a table that displays chemical elements in order of their electronic configuration, atomic number, and common chemical characteristics. There are some trends that may be found in all populations and time periods.Periods are the rows, and the periodic table has seven of them. Metals may be found on the left rows, whereas nonmetals can be found on the right. The columns, on the other hand, are referred to as groups. Elements in groups exhibit a variety of chemical properties. There are 18 groups, with halogens being found in group 17 and noble gases being found in group 18.