What are Group 15 Elements?
Group 15 elements are also called the Nitrogen family. It includes nitrogen, phosphorus, arsenic, antimony and bismuth elements. The p-block elements are also known as the Representative Elements which are placed on the right side of the main periodic table.
Table of Contents
The modern periodic table as conceived by Dimitri Mendeleev arranges all the elements known to man on the basis of its atomic number, which is unique to every element. The results of such an arrangement were the periodic table. The elements with similar properties were arranged into a column called a group.
Periodic Trends in Group 15 Elements
So in Group 15 elements as you would move down a group, starting with the lightest element and finishing with the heavy ones; you’d notice a general flow in properties as you move down the order. For eg, Nitrogen is a gas and non-metal but as you move down the group, we encounter metalloids and then at the bottom, metal i.e. Bismuth. These trends in the periodic table help us better understand the behaviour of atoms and also helps us predict new elements.
|Atomic mass (amu)||14.01||30.97||74.92||121.76||209.98|
|Valence electron configuration||[He]2s2 2p3||[Ne]3s2 3p3||[Ar]3d10 4s24p3||[Kr]4d10 5s25p3||[Xe]4f14 5d106s26p3|
Boiling point (°C)
|Density (g/cm3) at 25°C||1.15(g/L)||1.8||5.7||6.68||9.79|
|Atomic radius (pm)||56||98||114||133||143|
|First Ionization energy (kJ/mol)||1402||1012||947||834||703|
|Common Oxidation state(s)||-3 to +5||+5, +3, -3||+5, +3||+5, +3||+3|
|Ionic radius (pm)||146(-3)||212(-3)||58(+3)||76(+3)||103(+3)|
Some of the trends in the modern periodic table with respect to group 15 elements of the p-Block elements are discussed below.
1. Electronic Configuration
- The valence shell electronic configuration plays a major role in how an element behaves. The valence electron shell configuration of group 15 elements is ns2np3.
- All the group 15 elements have the same arrangement and this is why they’re similar.
- The s-orbital in this group is completely filled and the p-orbitals are half filled and this makes their configuration extra stable.
2. Atomic and Ionic Radii
- If you see the electronic configuration of elements in the table above, you will notice that with every step you move downwards, new orbitals are added to the atom.
- This addition of new orbitals increases both the Atomic and the Ionic radii of group 15 elements.
- However, we see that from Arsenic to Bismuth only a small increase in ionic radius is observed.
- This is due to the presence of completely filled d and/or f orbitals in heavier members.
3. Ionization Enthalpy
- Ionization Energy is the amount of energy required to remove an electron from the outermost orbit of the atom.
- This is basically a measure of how hard the nucleus is holding on to the electron.
- The closer the electron is to the nucleus the stronger its hold and thus the energy required is more.
- As we move down the group, the radius of the atom increases, and therefore the Ionization energy decreases due to the weaker hold of the nucleus.
- The electronegativity value decreases down the group with increasing atomic size.
- This again is due to the increasing distance between the nucleus and the valence shell as we move down the group.
5. Physical Properties
- All the elements of the group exist in a polyatomic state.
- First, Nitrogen is gas, but as you move down, there is a significant increase in the metallic character of the elements.
- Nitrogen and Phosphorus are non-metals, Arsenic and Antimony are metalloids and Bismuth is a metal.
- These changes can be attributed to the decrease in Ionization enthalpy and increase in atomic size.
- Boiling points also, in general, show an increasing trend as you move down.
- Except for Nitrogen, all the other elements have allotropes.
6. Chemical Properties
- The valence shells of the p-Block elements have a configuration of ns2 np3.
- So the elements here can either lose 5 electrons or gain 3.
- The common oxidation states of these elements are -3, +3 and +5.
- With a decrease in the Ionization enthalpy and electronegativity due to the increasing atomic radius, the tendency to gain three electrons to create a -3 oxidation state decreases down the group.
- In fact, Bismuth hardly forms any compounds with a -3 oxidation state.
- As we go down, the stability of the +5 state decreases and that of +3 increases due to the inert pair effect.
Apatite families can be described as a group of similar isomorphous hexagonal phosphate minerals. The main apatite group consists of Fluorapatite, Chlorapatite, and Hydroxylapatite. The teeth and bones of various animals, including humans, are composed of Calcium phosphate, which is also the same material as apatite.
The primary Apatite group includes Fluorapatite, Chlorapatite, and Hydroxylapatite. The extended Apatite supergroup describes additional minerals such as Pyromorphite, Mimetite, and Vanadinite. Apatite is the main source of phosphorous, an important nutrient required by plants. As such, apatite is the key ingredient in phosphate fertilizers. Most of the phosphorus used in fertilizer comes from phosphate rock, which is mined almost exclusively for this application.
Frequently Asked Questions – FAQs
Why is Group 15 called P block?
It is a p-block element since it takes the physical and chemical properties after that of other p-block elements of the eighteenth group. P-block elements are generally non-metals, while the remaining are metalloids and metals.
What is the other name of group 15 elements?
This group is also known as the nitrogen family. It consists of the elements nitrogen (N), phosphorus (P), arsenic (As), antimony (Sb), bismuth (Bi), and perhaps the chemically uncharacterized synthetic element moscovium (Mc). In modern IUPAC notation, it is called Group 15.
Why do all Group 15 elements have similar chemical properties?
Each element within a group has similar physical or chemical properties because of its atom’s outermost electron shell (most chemical properties are dominated by the orbital location of the outermost electron).
What element family does oxygen belong to?
Chalcogens. Group 6A (or VIA) of the periodic table are the chalcogens: the nonmetals oxygen (O), sulfur (S), and selenium (Se), the metalloid tellurium (Te), and the metal polonium (Po).
What do we use nitrogen for?
Nitrogen is important to the chemical industry. It is used to make fertilizers, nitric acid, nylon, dyes and explosives. To make these products, nitrogen must first be reacted with hydrogen to produce ammonia.
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