Chemistry
Group 5A
Group 5A refers to the nitrogen group of elements in the periodic table, which includes nitrogen (N), phosphorus (P), arsenic (As), antimony (Sb), and bismuth (Bi). These elements share similar chemical properties, such as forming compounds with a -3 oxidation state and often acting as nonmetals. They are important in various industrial and biological processes, including the nitrogen cycle and the production of fertilizers.
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eBook - ePubEssentials of Inorganic Chemistry
For Students of Pharmacy, Pharmaceutical Sciences and Medicinal Chemistry
- Katja A. Strohfeldt(Author)
- 2015(Publication Date)
- Wiley(Publisher)
Chapter 6 Group 15 ElementsMembers of group 15 of the periodic table (15th vertical column) are summarised as group 15 elements (or the nitrogen group) consisting of nitrogen (N), phosphorus (P), arsenic (As), antimony (Sb) and bismuth (Bi) (Figure 6.1 ).Periodic table of elements. Group 15 elements are highlightedFigure 6.1The appearance of group 15 elements varies widely, reflecting the changing nature of the elements when descending within the group from nonmetal to metal. This trend can be seen both in their structures as well as in their chemical and physical properties. Nitrogen is a colourless and odourless gas. Phosphorous exists as white, red and black solids, whereas arsenic is found as yellow and grey solids. Antimony presents itself in a metallic grey form, and bismuth is a white crystalline metal.Nitrogen atoms are included in a variety of organic drugs, and their application will not further be discussed in this book. Phosphorus is also an essential element for human life, and some of its biochemical uses as well as clinical applications will be discussed in Section 6.2. The clinical use of arsenic is known as thestart of chemotherapy. Arsenic, despite its known toxicity, is still clinically used to combat a variety of diseases including cancer (see Section 6.3).6.1 Chemistry of group 15 elements
6.1.1 Occurrence and extraction
Nitrogen makes up 78% (by volume) of air, whereas phosphorus can be found in several minerals and ores. Phosphorus is an essential constituent of plants and animals, being present in deoxyribonucleic acid (DNA), bones, teeth and other components of high biological importance. Phosphorus does not occur in its elemental state in nature, as it readily oxidises and therefore is deposited as phosphate rock. The remaining elements of group 15 are mostly obtained from minerals, but can also be found in their elemental form in the earth's crust. Arsenic is mostly presented in nature as mispickel (FeAsS), realgar (As4 S4 ) and orpiment (As2 S3 ). Bismuth occurs as bismuthinite (Bi2 S3
eBook - PDFEssentials of Inorganic Chemistry
For Students of Pharmacy, Pharmaceutical Sciences and Medicinal Chemistry
- Katja A. Strohfeldt(Author)
- 2014(Publication Date)
- Wiley(Publisher)
6 Group 15 Elements Members of group 15 of the periodic table (15th vertical column) are summarised as group 15 elements (or the nitrogen group) consisting of nitrogen (N), phosphorus (P), arsenic (As), antimony (Sb) and bismuth (Bi) (Figure 6.1). The appearance of group 15 elements varies widely, reflecting the changing nature of the elements when descending within the group from nonmetal to metal. This trend can be seen both in their structures as well as in their chemical and physical properties. Nitrogen is a colourless and odourless gas. Phosphorous exists as white, red and black solids, whereas arsenic is found as yellow and grey solids. Antimony presents itself in a metallic grey form, and bismuth is a white crystalline metal. Nitrogen atoms are included in a variety of organic drugs, and their application will not further be discussed in this book. Phosphorus is also an essential element for human life, and some of its biochemical uses as well as clinical applications will be discussed in Section 6.2. The clinical use of arsenic is known as the start of chemotherapy. Arsenic, despite its known toxicity, is still clinically used to combat a variety of diseases including cancer (see Section 6.3). 6.1 Chemistry of group 15 elements 6.1.1 Occurrence and extraction Nitrogen makes up 78% (by volume) of air, whereas phosphorus can be found in several minerals and ores. Phosphorus is an essential constituent of plants and animals, being present in deoxyribonucleic acid (DNA), bones, teeth and other components of high biological importance. Phosphorus does not occur in its elemental state in nature, as it readily oxidises and therefore is deposited as phosphate rock. The remaining elements of group 15 are mostly obtained from minerals, but can also be found in their elemental form in the earth’s crust. Arsenic is mostly presented in nature as mispickel (FeAsS), realgar (As 4 S 4 ) and orpiment (As 2 S 3 ).
eBook - PDF- Bernard Moody(Author)
- 2013(Publication Date)
- Arnold(Publisher)
21 Group V: the nitrogen group Nitrogen, phosphorus, arsenic antimony and bismuth 7 The gradation of properties N shown by compounds of 2,5 Group V elements covers a 15 wide range. The elements P change in character from 2,8,5 non-metallic gaseous nitro-33 gen and solid phosphorus, As to arsenic, antimony and the 2,8,18,5 metallic bismuth, all solids. 51 The changeover from non-Sb metal to metal is seen in the 2,8,18,18,5 middle families of the Periodic Table. This was 83 Bi seen in Group IV but the 2,8,18,32,18,5 elements of Group V are more electronegative and the metallic state, when it appears is less pro-nounced. The borderline between non-metal and metal comes between arsenic and antimony, the latter forming positive ions and having the proper-ties of a weak metal. Nitrogen has the distinctly anomalous properties associated with the first members of Groups V, VI and VII, and also apparent with the metallic families. Nitrogen has a valency of three in simple compounds. Phosphorus, arsenic and antimony show valencies of three and five, the latter being the principal valency state of phosphorus. The valency of bismuth is three, although some poorly defined oxides of a higher valency state exist and Sodium bismuthate' is assigned the approximate formula NaBiC>3. The higher valency state used to be denoted by the suf-fixes -ic and -ate and the lower, by -ous and -ite. Oxidation numbers range from -3 to +5 for nitrogen (p. 124) while the others exhibit oxidation states of-3 (PH 3 ), +3(AsCl 3 )and +5(Sb 2 0 5 ), the illustrative examples applying generally. Many of the compounds formed by nitrogen are different enough from those of the other elements of Group V to warrant the consideration that nitrogen ought to be separately classified from the remaining elements, the Phosphorus Group. Nitrogen has a high electronegativity ( = 3.0) which makes it a very strong non-metal.
eBook - PDFInorganic Chemistry
Butterworths Intermediate Chemistry
- C. Chambers, A. K. Holliday(Authors)
- 2016(Publication Date)
- Butterworth-Heinemann(Publisher)
The other Group V elements can behave in a similar manner but their atoms have an increasing reluctance to accept electrons, and to donate the lone pair. These atoms can, however, increase their covalency to five, for example in the vapour of phosphorus pentachloride, or even to six, for example in the ions [PF 6 ] ~, [PC1 6 ] . Hence phosphorus, arsenic, antimony and bismuth are able to form both trivalent and quinquevalent compounds Chapter 9 Group V NLtrnn«n nhn.nhorus. arsenic antimonv. bismuth 187 Occurrence and extraction of the elements Table 9.1 Element N P As Sb Bi Selected properties of the elements Atomic number 1 15 33 51 83 Outer electrons 2s 2 2p 3 3s 2 3p 3 3d 10 4s 2 4p 3 4d 10 5s 2 5p 3 5d 10 6s 2 6p 3 Atomic radius nm 0.070* 0.110* 0.125 0.145 0.170 m.p./K 63 317f 1090Î 903 545 b.p./K 11 554t sublimes 1910 1832 First ionization energy k J m o l -1 1403 1012 947 834 703 Electro-negativity (Pauling) 3.0 2.1 2.0 1.9 1.9 *covalent radius, fwhite P. {under pressure. but as we go from phosphorus to bismuth it becomes increasingly more difficult to achieve a quinquevalent state —thus phosphorus(V) oxide, P 4 O 10 , is readily obtained by burning phosphorus in excess of air, but the» corresponding oxides of antimony and bismuth require the action of strong oxidizing agents for their preparation and bismuth(V) oxide is particularly unstable. 9.2 Occurrence and extraction of the elements 9.2.1 Nitrogen Nitrogen is an essential constituent of all living matter, being one of the elements present in proteins. Proteins are synthesized by plants from nitrogen compounds in the soil, usually with the help of bacteria although some plants can absorb and utilize free gaseous nitrogen. The replacement of nitrogen compounds in the soil is essential for continued growth of crops; hence the manufacture of fertilizers such as ammonium or nitrate salts is a major industry since, because they are water soluble, inorganic nitrogen compounds are only rarely found in nature.
eBook - PDFThe History and Use of Our Earth's Chemical Elements
A Reference Guide
- Robert E. Krebs(Author)
- 2006(Publication Date)
- Greenwood(Publisher)
These families of related elements are called groups. The next several sections of this book present elements from the boron group (group 13; IIIA) through the noble gas group (group 18; VIII). The similarities and differences between the elements in each of these groups are not uniform and require some study in order to be understood in relation to the periodic table. Please note that names given to these groups in this book are not necessarily the same as used by some other references. Rather, they are descriptive as to their properties and characteristics. Not all elements in these groups have the same properties and characteristics. For instance, in group15, nitrogen is a gas, whereas the element just below it in group 15 is phosphorous, a non- metallic solid (semimetal). Just below phosphorous is arsenic (semimetal), followed by antimony and then bismuth, which are more metal-like. These last two, antimony and bismuth, are metals that might be considered an extension of periods 5 and 6 of the transition elements. Even though the elements listed in groups 13 (IIIA) to 18 (VIIIA) may not have the same properties and characteristics, they do have a distinct number of electrons in their outer valence shells related to their specific group. For instance, group 13 elements have three electrons in their outer valence shell, and group 14 elements have four electrons. Group 15 elements have five electrons in their outer valence shell, and group 16 elements have six elec- trons. The halogens in group 17 have seven electrons, and the inert elements in group 18 have a completed outer valence shell with eight electrons. At the end of each periods of group 18 (whose elements each have eight electrons in their respective outer valence shells), the table starts over with elements containing one electron in their respective valence shells (the alkali earth metals in group 1 [IA]).
eBook - PDF- Alina Kabata-Pendias(Author)
- 2010(Publication Date)
- CRC Press(Publisher)
353 20 Elements of Group 15 (Previously Group Va) Trace elements of the Group 15 are arsenic (As), antimony (Sb), and bismuth (Bi). These elements have similar structure and some similar properties. However, their geochemical characteristics are widely diverging. The variations in electrical charges and in valence states are especially common features of these elements (Table 20.1). The metalloids As and Sb, and the metal Bi are highly chalcophilic. Often As follows P in biogeochemical behavior, especially in aerated systems. ARSENIC I I NTRODUCTION A The average content of As in the Earth’s crust is estimated as 1.8 mg/kg (Table 3.2). It is found abundantly in argillaceous sediments (up to 13 mg/kg) than in any other rocks (Table 20.2). Its oxidation states are variable, of which As 0 and As 3 + are characteristic of reducing environments. According to Welch and Lico (1998), As 5 + is adsorbed preferably by sediments than other As ions. There are many As minerals, of which about 60% are arsenates. As is highly associated with deposits of several metals and metalloids and therefore is known as a good indicator in geochemical prospecting surveys. Numerous oxide minerals of As are a result of the oxidation of sulfide deposits. These are arsenates and arsenites in which As is combined with some metal (e.g., Fe, Pb, and Cu). The most common As mineral, however, is a sulfide–arsenopyrite (FeAsS). As-rich pyrite is common in the sedimentary formations rich in OM, especially shale, coal, and peat deposits. Its other common minerals are orpiment As 2 S 3 ; realgar, AsS; arenolite, As 2 O 3 ; domeykite, Cu 3 As; nikieline, NiAs; and sperrylite PtAs 2 . Global production of As was estimated as 53.5 kt in 2008 (USDI, 2009). As is generally recovered from sludge and flue dust during smelting of Cu, Zn, Pb, Au, and Ag ores. Until the 1970s, about 80% of As was used in the manufacturing of pesticides.
- Hongzhe Sun(Author)
- 2010(Publication Date)
- Wiley(Publisher)
Chapter 1 The Chemistry of Arsenic, Antimony and Bismuth Neil Burford, Yuen-ying Carpenter, Eamonn Conrad and Cheryl D.L. Saunders Department of Chemistry, Dalhousie University, Halifax, Nova Scotia, B3H 4J3, CanadaArsenic, antimony and bismuth are the heavier pnictogen (Group 15) elements and consistent with their lighter congeners, nitrogen and phosphorus, they adopt the ground state electron configuration ns 2 np 3 . Arsenic and antimony are considered to be metalloids and bismuth is metallic, while nitrogen and phosphorus are non-metals. Arsenic and antimony are renowned for their toxicity or negative bioactivity [1, 2] but bismuth is well known to provide therapeutic responses or demonstrate a positive bioactivity [3]. As a background to the biological and medicinal chemistry of these elements, the fundamental chemical properties of arsenic, antimony and bismuth are presented in this introductory chapter.1.1 Properties of the ElementsSelected fundamental parameters that define the heavier pnictogen elements are summarized in Table 1.1 [4]. While arsenic and bismuth are monoisotopic, antimony exists as two substantially abundant naturally occurring isotopes. All isotopes of the heavy pnictogens are NMR active nuclei, indicating that the nuclear spin will interact with an applied magnetic field. However, as the nuclear spins of these isotopes are all quadrupolar, NMR spectra generally consist of broad peaks and provide limited information. The atoms As, Sb and Bi all have the same effective nuclear charge (Zeff = 6.30, Slater), which estimates the charge experienced by a valence electron taking into account shielding by the other electrons. As a consequence, the ionization energies and electron affinities for As, Sb and Bi are very similar. The ionization energy is the energy required to remove a valence electron from an atom or an ion in the gas phase. The ionization energies are predictably greater for ions with higher positive charge and are typically lower for atoms or ions with higher principal quantum number (n). The electron affinity is the energy released when an atom gains an electron to form an anion in the gas phase. The electronegativity (χP
eBook - PDF- Leo J. Malone, Theodore O. Dolter(Authors)
- 2012(Publication Date)
- Wiley(Publisher)
Why did Mendeleev succeed where others had failed? For additional practice, work chapter problems 4-1 and 4-2. C C ASSESSING THE OBJECTIVE FOR SECTION 4-1 FIGURE 4-4 Nonmetals The bottle on the left contains liquid bromine and its vapor. The flask in the back contains pale-green chlorine gas. Solid iodine is in the flask on the right. Powdered red phosphorus is in the dish in the middle, and black powdered graphite (carbon) in the watch glass in front. Lumps of yellow sulfur are shown in the front. 4-2 Using the Periodic Table 121 and hydrogen—are in this category. One group of the representative elements includes the highly reactive metals that we discussed earlier. Notice that lithium, sodium, and potassium are found in Group IA. This family of elements (not including hydrogen) is known as the alkali metals. Another set of metals that are also somewhat chemically reactive is found in Group IIA and is known as the alkaline earth metals. Group VIIA elements are all nonmetals and are known as the halogens. The other representative element groups (IIIA, IVA, VA, and VIA) are not generally referred to by a family name but are instead identified by the element at the top of the column. Hence, any element in column VA is part of the nitrogen family. In Chapter 9, we will discuss in more detail some of the physical and chemical properties of the representative elements. 2. The Noble or Inert Gases (Group VIIIA) These elements form few chemical compounds. In fact, helium, neon, and argon do not form any compounds. The noble gases all exist as individual atoms in nature. 3. The Transition Metals (Group B Elements) Transition metals include many of the familiar structural metals, such as iron and chromium, as well as the noble metals—copper, silver, and gold (Group IB)—which we discussed earlier. 4. The Inner Transition Metals The 14 inner transition metals between lanthanum (number 57) and hafnium (number 72) are known as the lanthanides.
- Martha Mackin(Author)
- 2012(Publication Date)
- Academic Press(Publisher)
2. Nitrogen makes up 80% by volume of the air. a) Nitrogen-fixing bacteria convert the element nitrogen into nitrogen-containing compounds that are essential for all life. b) Liquid nitrogen is used as a coolant. c) Nitrogen is used to make ammonia. 3. Phosphorus exists as several allotropes; red phosphorus is used in safety matches and munitions. 4. Arsenic is a toxic element; it is used in gunshot and in semiconductors. 5. Bismuth, when combined with other metals, has a low melting point and is used in automatic fire sprinkler systems. I. Group 6A elements 1. Oxygen and sulfur are the most common elements in the group. 2. Oxygen is the most abundant element on Earth. a) Oxygen in elemental form is essential for life. b) Oxygen supports combustion. c) It is used in welding and in rocket propulsion. d) Ozone is an allotrope of oxygen. e) Ozone in the upper atmosphere prevents harmful ultraviolet radiation from reaching the surface of the Earth. 3. Sulfur is a basic raw material in industry. 4. Sulfur is used in treating rubber (vulcanization) to make it less brittle. 5. Selenium is used in photoelectric cells. J. Group 7A elements: the halogens 1. The elements of this group are strongly nonmetallic. 2. Fluorine is the most chemically active element known. 3. Chlorine is a greenish-yellow poisonous gas; it is used in chlorination of water. 4. Bromine is a red-brown liquid at room temperature; it has an irritating vapor. 5. Iodine is a shiny bluish-black solid. a) It has the ability to change directly from a solid to a gas (sublimation). b) It is used as a disinfectant. K. The noble gases 80 Fill-in 81 1. These elements make up about 1% of the atmosphere by volume? 90% of the total amount of the noble gases is argon. 2. They are exceptionally stable. 3. They were once called inert gases but a few compounds containing these elements have since been prepared. 4. Helium is the second most common element in the universe, but is found in only small amounts on Earth.
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