Electronic Configuration of Antimony Explained

Group 15 elements contain nitrogen (N), Phosphorus (P), Arsenic (As), Antimony (Sb), and Bismuth (Bi). All group 15 elements have the electron configuration ns²np³ in their outer shell, where n is the principal quantum number. The N family is found in the p-block in group 15.

Valence electrons are the electrons in an atom's outermost shell or energy level. In other words, a valence electron may be a negatively charged particle placed in the outermost shell of an atom that can be transferred to or shared with another atom.

Group 15 Elements in The Periodic Table

What is Electronic Configuration?

Electronic configuration, also referred to as electronic structure or electron configuration, is the arrangement of electrons in orbitals around an atomic nucleus. The symbols used for writing the electron configuration begin with the shell number (n) followed by the type of orbital. Eventually, the superscript indicates how many electrons are in the orbital.

Rules to Write the Electronic Configuration

Rules to determine the electronic configuration for any element are listed below:

• Aufbau Principle

• Pauli Exclusion Principle

• Hund’s Rule

The filling of electrons into the orbitals of different atoms takes place according to the Aufbau principle which is based on Pauli’s exclusion principle, Hund’s rule of maximum multiplicity, and the relative energies of the orbitals.

Electronic Configuration of Group 15 Elements

Nitrogen: (Atomic no. 7)

The electronic configuration of N is 1s²2s²2p³. It is a non-metallic component and has no taste and no colour. When compared with the rest of group fifteen, N has the highest electronegativity which makes it the most nonmetallic of the group. The common oxidation states of (atomic number 7) N are +5, +3, and -3.

Phosphorus : (Atomic no. 15)

The electron configuration of P is [Ne]3s²3p³. The most common oxidation state of phosphorus is -3. Phosphorus is the eleventh most abundant component, making up 0.11% of the Earth's crust. The main source of phosphorus compounds is phosphorus rocks.

Group 15 Element’s Electron Configuration

Arsenic : (Atomic no. 33)

The electron configuration of As is [Ar]3d¹⁰4s²4p³. Arsenic may be an extremely toxic metalloid. Because it's a nonmetal, arsenic contains a high density, moderate thermal conduction, and a restricted ability to conduct electricity. The oxidation states of arsenic are +5, +3, +2, +1, and -3. Compounds of arsenic are utilised in pesticides, weed killers, and alloys.

Antimony : (Atomic no. 51)

The electron configuration of Antimony (Sb) is [Kr]4d¹⁰5s²5p³.

Bismuth : (Atomic no. 83)

The electron configuration of Bi is [Xe]4f¹⁴5d¹⁰6s²6p³.

Valence Electrons in Antimony

Antimony (Sb) has an atomic number of 51. The valence electrons are referred to as the free electrons that are available at the last orbital. In Sb, the total electron shells are five. The electronic configuration of Sb is 2, 8, 18, 18, and 5. Thus, the Antimony valence electrons are five.

Electron configuration of Sb is 1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d¹⁰ 4p⁶ 4d¹⁰5s² 5p³. In the above configuration, the last orbital is five. Therefore, the valency of Sb or Antimony valency is 5. Antimony is a non-metal. The oxidation states of Sb are +3, -3, and +5. Sb exhibits allotropy; the most stable allotrope is the metallic form, which is analogous in properties to arsenic:

• High density.

• Moderate thermal conductivity.

• Limited ability to conduct electricity.

The oxide of Sb is Sb (III) oxide which is amphoteric, which means it will act as an acid and a base.

Noble Gas Electron Configuration for Nitrogen

The noble gas configuration of nitrogen is [He]2s²2p³_. Nitrogen has atomic number seven on the periodic table. This implies that every N atom has seven protons in its nucleus. A neutral N atom additionally has seven electrons. The noble gas electron configuration contains the symbol for the noble gas within the previous period and also the remaining configuration is written out. N is in the 2^nd period of the periodic table, therefore the previous noble gas is He.

Interesting Facts

• Antimony is obtained mainly from its sulphide ores, and it evapourates at low temperatures.

• Along with arsenic, Sb is often utilised in alloys.

• Arsenic and Sb are used to manufacture semiconductor materials like GaAs, GaSb, and InSb in electronic devices.

Important Questions

1. What are the atomic properties of group 15 elements?

Ans:

• Atomic and ionic radii: The atomic and ionic radii of group fifteen components are smaller than the atomic radii of the corresponding group fourteen components.

• Ionisation enthalpies: On going down the group, the ionisation enthalpies decrease.

• Electronegativity values: On going down the group, the electronegativity value decreases.

The elements of group fifteen are less metallic. However, on going down the group, the metallic character will increase from N to Bi. For example, the N and P are non-metallic, As and Sb are partially non-metallic whereas Bi is a metal.

Conclusion

The elements of group fifteen in the periodic table are called the nitrogen family. The atoms of group fifteen have 5 electrons within the outermost shell, two in s, and three in the p subshell. The final electronic configuration of this group could also be expressed as ns² np³. The valency of Sb and the noble gas configuration of N and another group fifteen components are often determined.