Periodic Trends in Group 15 Elements

Nitrogen (N), phosphorus (P), arsenic (As), antimony (Sb), and bismuth are all members of the nitrogen family of chemicals (Bi). The electron configuration ns²np³ is found in the outer shells of all Group 15 elements, where n is the primary quantum number. As seen in the diagram, the nitrogen family is found in Group 15’s p-block.

Periodic Trends

The following general periodic trends apply to all Group 15 elements:

As the group progresses, electronegativity (the capacity of an atom to attract electrons) declines. The amount of energy required to remove an electron from an atom in its gas phase diminishes as you progress down the group. The size of atomic radii grows as the group progresses. Down the group, electron affinity (an atom’s capacity to take an electron) declines. Melting point (the amount of energy required to break bonds in order to convert a solid phase substance to a liquid phase substance) rises as you progress through the group.

The boiling point (the amount of energy required to break bonds and convert a liquid to a gas) rises as the group progresses. The group becomes more metallic as it progresses.

Electronic Configuration

The arrangement of electrons into energy levels surrounding an atomic nucleus is called electronic configuration or electronic structure. Electrons occupy various levels in the older shell atomic model, from the first shell, K, closest to the nucleus towards the seventh shell, Q, distant from the nucleus. The K–Q shells are subdivided into a set of orbitals (orbital) that can each hold no more than a pair of electrons in a more detailed quantum-mechanical model. The number of orbitals in each of the first four shells is listed in the table below.

The number of electrons for each shell, starting with the first, can be used to express an atom’s electrical configuration in the shell atomic model. The 11 electrons in sodium (atomic number 11) are divided as follows: the K and L shells are totally filled with 2 and 8 electrons, respectively, and the M shell is only half filled with one electron.

Atomic Radius

The atomic radius of a neutral atom is the distance between its nucleus and its outermost stable electron. In practice, the diameter of an atom is measured and divided in half to get the value. Neutral atoms have radii ranging from 30 to 300 pm (thousands of a metre).

The atomic radius is a measurement of an atom’s size. This value, however, has no universally accepted definition. The ionic radius, as well as the covalent, metallic, and van der Waals radius, are all examples of atomic radius.

Ionic Radius

The ionic radius is equal to half of the distance between the two gas atoms that are contacting. 30 p.m. to over 200 p.m. are typical values. The atomic and ionic radius are the same for a neutral atom, however many elements have anions or cations. The ionic radius is less than the atomic radius since the atom loses an electron energy shell when it loses its outermost electron (positively charged called cation). When an atom gets an electron (negatively charged called anion), the electron usually falls into an existing energy shell, so the ionic and atomic radius are similar in size.

Ionization Enthalpy

Ionization The amount of energy required for an isolated gaseous atom to lose one electron in its ground state is referred to as the enthalpy of elements. Cations develop when electrons are lost.

Conclusion 

The elements of the p-block are arranged in groups of 13 to 18 on the periodic table’s right side. The separating electron in the valence p subshell of p-block elements enters the iotas. The np subshell is gradually filled in these pieces in this fashion.

Group fifteen elements have a common valence shell electronic configuration ns², np^1-6. Helium has a 1s² electrical structure. There are no orbitals in this object. It is a p-block element, however, because its physical and chemical properties are similar to those of other p-block elements in the eighth group. Non-metals make up the majority of P-block elements, with metalloids and metals making up the remainder. Nitrogen, phosphorus, arsenic, antimony, and bismuth are all members of Group 15 of the periodic table. Nitrogen makes up 78 percent of the volume of air. It is the most common member of this family and exists as a diatomic gas in its free state, N₂.

Phosphorus is a key component of both animal and plant life. Nucleic acids, such as DNA and RNA, have phosphate groups as components. Phosphates make up over 60% of all bones and teeth. Egg yolks, milk, and bone marrow all contain phosphoproteins. Arsenic, antimony, and bismuth, for example, are mostly found as sulphides.