Last Updated on July 11, 2020 By Mrs Shilpi Nagpal Leave a Comment. Diversity in chemistry is the hallmark of p–block elements manifested in their ability to react with the elements of s–, d– and f–blocks as well as with their own. It is additionally found as the fundamental constituent of proteins, nucleic acids, amino acids, and catalysts. Physical properties In fact, Bismuth hardly forms any compounds with -3 oxidation state. The p-Block Elements Class 12 Notes Chemistry Chapter 7. a) phosphorus exists as white, black or red phosphorus. Alongside, you will be shown the following properties as well: Electronic configuration. Electron Gain Enthalpy Your email address will not be published. The electronic configuration of atoms of group 15 are half filled, npx1, npy2 npz1 and are stable. (4) Nitrogen and phosphorus also show oxidation state of +4 because of the ability of one lone pair on NH3 and PH3 to form dative bonds with Lewis acids.However, nitrogen can exist in various oxidation states from -3 to +5 in its hydrides, oxides and oxo acids. Explanation: The elements of group 15 have smaller size and greater nuclear charge of atoms and therefore, they have higher electronegativity values. Group 15 elements have higher ionization energy than group 16 elements because they have stable electronic configuration i.e., half filled p-orbitals. The following element in the group is phosphorus. However, from As to Bi only a small increase in covalent radius is observed. Phosphorus is the eleventh element in order of abundance in crystal rocks of the earth. (5) Melting and boiling points: The melting points of group 15 elements first increase from nitrogen to arsenic and then decreases to antimony and bismuth. (1) Atomic and ionic radii : The atomic and ionic radii of group 15 elements are smaller than the atomic radii of the corresponding group 14 elements. Filed Under: Chemistry, Class 12, The p-Block Elements. Among the elements of group 15, phosphorus has the maximum tendency for catenation forming cyclic as well as open chain compounds consisting of many phosphorus atoms. 3M + 2E → M 3 E 2 Binary compound Download Files. Ionisation enthalpy. Group 15 elements of the periodic table constitute the elements nitrogen (N), phosphorus (P), arsenic (As), antimony (Sb) and bismuth (Bi). The first, Nitrogen is gas but as you move down there is a significant increase in the metallic character of the elements. The continuous interchange of nitrogen between the atmosphere and biosphere is called, Phosphorus is the eleventh element in order of abundance in crystal rocks of the earth. The elements of Group 15 have a general electronic configuration of “ns 2 np 3 ” that is, they have five electrons in their outermost shell with half-filled p orbitals. These elements are put together called p-block elements. All Group 15 elements tend to follow the general periodic trends: Electronegativity (the atom's ability of attracting electrons) decreases down the group. Nitrogen and phosphorus are non-metals, arsenic and antimony are metalloids and bismuth is a typical metal. The common oxidation states of these elements are -3, +3 and +5. For the main group elements (s and p blocks), valence electrons are the electrons in the outermost (highest energy) s and p sublevels. Phosphorus is also found in ATP (adenosine triphosphate and ADP (adenosine diphosphate). Like the group 14 elements, the lightest member of group 15, nitrogen, is found in nature as the free element, and the heaviest elements have been known for centuries because they are easily isolated from their ores. However, we see that from Arsenic to Bismuth only a small increase in ionic radius is observed. Author of this website, Mrs Shilpi Nagpal is MSc (Hons, Chemistry) and BSc (Hons, Chemistry) from Delhi University, B.Ed (I. P. University) and has many years of experience in teaching. This is due to the fact that group 15 element have extra stable half-filled p orbitals electronic configurations. 7.2 Dinitrogen. The next two, arsenic and antimony are metalloids whereas the last element, bismuth is a metal. It is used in the manufacture of HNO3, NH3, CACN2 (calcium cyanamide) and other nitrogenous compounds. 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The p-block elements (Group 15 to 18) Topics. All its known minerals are, Phosphorus is essential for life, both as a structural material in animals and plants. About 60% bones and teeth are Ca3(PO4)2  or [3{Ca3(PO4}2.CaF2]. So the elements here can either lose 5 electrons or gain 3. Atomic radii increase in size down the group. Nitrogen is the real constituent of the air and records for 78% of it by volume. For example: hydrazine (H2NNH2) has two N atoms bonded together, hydrazoic acid (N3H) has three N-atoms, azide ion, N3¯ has also three N atoms bonded together. Group 15 elements have higher ionisation energy than group 14 elements due to smaller size of group 15 elements. Explanation: The larger ionisation enthalpy is due to greater nuclear charge, small size and stable configuration of the atoms of group 15 elements. The stability of the highest oxidation state (+5) decreases down the group. View All Topics. Explanation: The nuclear charge in case of elements of group 15 is larger than in the case of elements of group 14. (4) Metallic character: The elements of group 15 are less metallic. All the elements of group 15 react with metals to form their binary compounds showing -3 oxidation state with the general formula M 3 E 2. CBSE Class 12 Chemistry Notes: The p Block Elements – Nitrogen Family. Here, M stands for metals while E stands for an element of group 15. (2) Nitrogen does not form compounds in +5 oxidation state such as NF5, NCl5, etc. Group 15th elements are nitrogen (N), phosphorus (P), arsenic (As), antimony (Sb) and bismuth (Bi). On going down the group, the atomic radii increase with increase in atomic number. • Group 14: Carbon Group • Group 15: Nitrogen Group • Group 16: Oxygen Group • Group 17: Halogens o The most highly reactive nonmetals. The results of such an arrangement were the periodic table. Except for Nitrogen, all the other elements have allotropes. Nitrogen is the real constituent of the world's air, and records for 78% of it by volume. Description. The lesser tendency of elements of group 15 to show catenation in comparison to carbon is their low (M-M) bond dissociation enthalpies. Chapter 15 Group 15 Elements Occurrence and extraction Physical Properties Metals Halides, oxides, hydroxides, salts of oxoacids Phosphoacids Sulfides and selenides Class 6. Explanation: The melting points increase down the group due to increase in atomic size However, the unexpected decrease in the melting points of Sb and Bi is because of their tendency to form three covalent bonds instead of five covalent bonds, due to inert pair effect. (1) All the elements of group 15 exhibit positive oxidation states of +3 and +5. o Strong oxidizers – they readily pull electrons from other atoms. In group 15 of the Periodic Table, the elements, nitrogen (7 N), phosphorus (15 P), arsenic (33 As), antimony (51 Sb) and bismuth (83 Bi) are present. Your email address will not be published. The first two elements N and P are non – metal. Atomic and ionic radii. 2. The p-block elements (Group 15 to 18) Previous . The elements belonging to groups 1 and 2 belong to s- block and have the general configuration ns1-2. All its known minerals are orthophosphates. Bismuth. Molecular nitrogen comprises about 78% by volume of the Earth’s atmosphere, it is not very abundant in the earth’s crust.Since nitrates are very soluble in water so these are not widespread in the earth’s crust. This document contains detailed info on fundamentals, concept and explanation of various terms and definitions required to perfect knowledge of Group elements The chapter starts with the nitrogen family. (7) Allotropy: Except nitrogen and bismuth, all other elements of this group show allotropy. As a result, the attraction among their atoms is weak and hence their melting points are low. Some Important Compounds of Nitrogen Ammonia Ammonia is covalent. because it does not have vacant d-orbitals in its valence shell which can enable it to extend its octet. The atoms of group 15 have five electrons in the outermost shell, two in s and three in p subshell. The higher temperature reaction has explosive power and that is the reason that NH 4 NO 3 is used as a component of dynamite Plants need nitrogen to grow but the N Classes. Group 15 elements have higher ionisation energy than group 14 elements due to smaller size of group 15 elements. It is present in bones as well as in living cells. The Elements of Group 15 (5A, V, VA) The Nitrogen Group (Pnictogens/Pnicogens ) N, P, As, Sb, Bi Valence electron configuration: ns 2np 3 Standard States Nitrogen is the most abundant element in our atmosphere (78%), found as a diatomic gas. (1) Nitrogen being the smallest and most electronegative element of the group forms  N3–(nitride) ion and shows an oxidation state of 3 in nitrides of some highly electropositive metals such as Mg3N2, Ca3N2, etc. (6) The maximum covalency of nitrogen is restricted to four because it does not have vacant d-orbitals in its outermost valence shell (n = 2). (3) Electronegativity: The electronegativity values of elements of group 15 are higher than the corresponding elements of group 14. They belong to groups 1, 2 and from 13 to 18. About 60% bones and teeth are Ca, The general electronic configuration of this group may be expressed as ns, The electronic configuration of atoms of group 15 are half filled, np. For example: calcium phosphide (Ca3P2), sodium arsenide (Na3As), zinc antimonide (Zn3Sb2), magnesium bismuthide (Mg3Bi2). P block elements are shiny and usually a good conductor of electricity and heat as they have a tendency to lose an electron. 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