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The Periodic Electronegativity Table
The Periodic Electronegativity Table Jan C. A. Boeyens Unit for Advanced Study, University of Pretoria, South Africa Reprint requests to J. C. A. Boeyens. E-mail: [email protected] Z. Naturforsch. 2008, 63b, 199 – 209; received October 16, 2007 The origins and development of the electronegativity concept as an empirical construct are briefly examined, emphasizing the confusion that exists over the appropriate units in which to express this quantity. It is shown how to relate the most reliable of the empirical scales to the theoretical definition of electronegativity in terms of the quantum potential and ionization radius of the atomic valence state. The theory reflects not only the periodicity of the empirical scales, but also accounts for the related thermochemical data and serves as a basis for the calculation of interatomic interaction within molecules. The intuitive theory that relates electronegativity to the average of ionization energy and electron affinity is elucidated for the first time and used to estimate the electron affinities of those elements for which no experimental measurement is possible. Key words: Valence State, Quantum Potential, Ionization Radius Introduction electronegative elements used to be distinguished tra- ditionally [1]. Electronegativity, apart from being the most useful This theoretical notion, in one form or the other, has theoretical concept that guides the practising chemist, survived into the present, where, as will be shown, it is also the most bothersome to quantify from first prin- provides a precise definition of electronegativity. Elec- ciples. In historical context the concept developed in a tronegativity scales that fail to reflect the periodicity of natural way from the early distinction between antag- the L-M curve will be considered inappropriate. -
Removal of Heavy Metals from Aqueous Solution by Zeolite in Competitive Sorption System
International Journal of Environmental Science and Development, Vol. 3, No. 4, August 2012 Removal of Heavy Metals from Aqueous Solution by Zeolite in Competitive Sorption System Sabry M. Shaheen, Aly S. Derbalah, and Farahat S. Moghanm rich volcanic rocks (tuff) with fresh water in playa lakes or Abstract—In this study, the sorption behaviour of natural by seawater [5]. (clinoptilolite) zeolites with respect to cadmium (Cd), copper The structures of zeolites consist of three-dimensional (Cu), nickel (Ni), lead (Pb) and zinc (Zn) has been studied in frameworks of SiO and AlO tetrahedra. The aluminum ion order to consider its application to purity metal finishing 4 4 wastewaters. The batch method has been employed, using is small enough to occupy the position in the center of the competitive sorption system with metal concentrations in tetrahedron of four oxygen atoms, and the isomorphous 4+ 3+ solution ranging from 50 to 300 mg/l. The percentage sorption replacement of Si by Al produces a negative charge in and distribution coefficients (Kd) were determined for the the lattice. The net negative charge is balanced by the sorption system as a function of metal concentration. In exchangeable cation (sodium, potassium, or calcium). These addition lability of the sorbed metals was estimated by DTPA cations are exchangeable with certain cations in solutions extraction following their sorption. The results showed that Freundlich model described satisfactorily sorption of all such as lead, cadmium, zinc, and manganese [6]. The fact metals. Zeolite sorbed around 32, 75, 28, 99, and 59 % of the that zeolite exchangeable ions are relatively innocuous added Cd, Cu, Ni, Pb and Zn metal concentrations (sodium, calcium, and potassium ions) makes them respectively. -
Most Atoms Form Chemical Bonds to Obtain a Lower Potential Energy
Integrated Chemistry <Kovscek> 6-1-2 Explain why most atoms form chemical bonds. Most atoms form chemical bonds to obtain a lower potential energy. Many share or transfer electrons to get a noble gas configuration. 6-1-3 Describe ionic and covalent bonding. Ions form to lower the reactivity of an atom. Ionic bonding is when the attraction between many cations and anions hold atoms together. Covalent bonding results from the sharing of electron pairs between two atoms. That is, when atoms share electrons, the mutual attraction between the electrons (electron clouds) and protons (the nucleus) hold the atoms together. 6-1-4 Explain why most chemical bonding is neither purely ionic nor purely covalent. In order for a bond to be totally ionic one atom would have to have an electronegativity of zero. (there aren’t any). To have a purely covalent bond the electronegativity must be equal. (Only the electronegativity of atoms of the same element are identical, diatomic elements are purely covalent) 6-1-5 Classify bonding type according to electronegativity differences. Differences in electronegativities reflect the character of bonding between elements. The electronegativity of the less- electronegative element is subtracted from that of the more- electronegative element. The greater the electronegativity difference, the more ionic is the bonding. Covalent Bonding happens between atoms with an electronegativity difference of 1.7 or less. That is the bond has an ionic character of 50% or less. Electronegativity % Ionic Character Covalent Differences Bond Type 0 to 0.3 0% to 5% Non - Polar Over 0.3 up to 1.7 5% to 50% Polar Over 1.7 Greater than 50 % Ionic Ionic Bonding occurs between atoms with an electronegativity difference of greater than 1.7. -
ELECTRONEGATIVITY D Qkq F=
ELECTRONEGATIVITY The electronegativity of an atom is the attracting power that the nucleus has for it’s own outer electrons and those of it’s neighbours i.e. how badly it wants electrons. An atom’s electronegativity is determined by Coulomb’s Law, which states, “ the size of the force is proportional to the size of the charges and inversely proportional to the square of the distance between them”. In symbols it is represented as: kq q F = 1 2 d 2 where: F = force (N) k = constant (dependent on the medium through which the force is acting) e.g. air q1 = charge on an electron (C) q2 = core charge (C) = no. of protons an outer electron sees = no. of protons – no. of inner shell electrons = main Group Number d = distance of electron from the nucleus (m) Examples of how to calculate the core charge: Sodium – Atomic number 11 Electron configuration 2.8.1 Core charge = 11 (no. of p+s) – 10 (no. of inner e-s) +1 (Group i) Chlorine – Atomic number 17 Electron configuration 2.8.7 Core charge = 17 (no. of p+s) – 10 (no. of inner e-s) +7 (Group vii) J:\Sciclunm\Resources\Year 11 Chemistry\Semester1\Notes\Atoms & The Periodic Table\Electronegativity.doc Neon holds onto its own electrons with a core charge of +8, but it can’t hold any more electrons in that shell. If it was to form bonds, the electron must go into the next shell where the core charge is zero. Group viii elements do not form any compounds under normal conditions and are therefore given no electronegativity values. -
Is Selenium a Metal, Non-Metal Or Metalloid?
Is Selenium a metal, non-metal or metalloid? Abstract Is selenium(Se) a metal, non-metal, or a metalloid? There are various public opinions circulating around it. Since a long time from now, there are a lot of voices discussing this. Even until now, there is still no consensus about it. So, in this project, we are trying to find out whether selenium is a non-metal, metal or metalloids base on its physical and chemical properties which could be studied in the secondary school combining with the other information from the internet. Principles and hypothesis Studied from the secondary school chemistry, the general properties of metals include being good conductors of heat and electricity, having high melting and boiling points. Non-metals generally have a lower melting point and boiling point than metals and they being poor conductors of heat and electricity, etc. And the physical properties of metalloids are having extremely high melting/ boiling point, and having fair electrical conductivity. On the other hand, the oxides of metal are generally basic whereas the oxide of non-metals and metalloids are generally acidic. We will define selenium’s chemical category based on the above properties. Besides, we would like to introduce the concept of displacement reaction in studying the chemical properties of the chalcogens(e.g. sulphur(S) and selenium(Se)), especially selenium such rarely mentioned element. We can assume selenium is a metal if selenium could displace a metal oxide or a metal could displace selenium (IV) oxide. If selenium is a non-metal, its oxide could be displaced by sulphur which is supposed to be more reactive than selenium in the chalcogen group. -
Periodic Table 1 Periodic Table
Periodic table 1 Periodic table This article is about the table used in chemistry. For other uses, see Periodic table (disambiguation). The periodic table is a tabular arrangement of the chemical elements, organized on the basis of their atomic numbers (numbers of protons in the nucleus), electron configurations , and recurring chemical properties. Elements are presented in order of increasing atomic number, which is typically listed with the chemical symbol in each box. The standard form of the table consists of a grid of elements laid out in 18 columns and 7 Standard 18-column form of the periodic table. For the color legend, see section Layout, rows, with a double row of elements under the larger table. below that. The table can also be deconstructed into four rectangular blocks: the s-block to the left, the p-block to the right, the d-block in the middle, and the f-block below that. The rows of the table are called periods; the columns are called groups, with some of these having names such as halogens or noble gases. Since, by definition, a periodic table incorporates recurring trends, any such table can be used to derive relationships between the properties of the elements and predict the properties of new, yet to be discovered or synthesized, elements. As a result, a periodic table—whether in the standard form or some other variant—provides a useful framework for analyzing chemical behavior, and such tables are widely used in chemistry and other sciences. Although precursors exist, Dmitri Mendeleev is generally credited with the publication, in 1869, of the first widely recognized periodic table. -
Mendeleev's Periodic Table of the Elements the Periodic Table Is Thus
An Introduction to General / Inorganic Chemistry Mendeleev’s Periodic Table of the Elements Dmitri Mendeleev born 1834 in the Soviet Union. In 1869 he organised the 63 known elements into a periodic table based on atomic masses. He predicted the existence and properties of unknown elements and pointed out accepted atomic weights that were in error. The periodic table is thus an arrangement of the elements in order of increasing atomic number. Elements are arranged in rows called periods. Elements with similar properties are placed in the same column. These columns are called groups. An Introduction to General / Inorganic Chemistry The modern day periodic table can be further divided into blocks. http://www.chemsoc.org/viselements/pages/periodic_table.html The s, p, d and f blocks This course only deals with the s and p blocks. The s block is concerned only with the filling of s orbitals and contains groups I and II which have recently been named 1 and 2. The p block is concerned only with the filling of p orbitals and contains groups III to VIII which have recently been named 13 to 18. An Introduction to General / Inorganic Chemistry Groups exist because the electronic configurations of the elements within each group are the same. Group Valence Electronic configuration 1 s1 2 s2 13 s2p1 14 s2p2 15 s2p3 16 s2p4 17 s2p5 18 s2p6 The type of chemistry exhibited by an element is reliant on the number of valence electrons, thus the chemistry displayed by elements within a given group is similar. Physical properties Elemental physical properties can also be related to electronic configuration as illustrated in the following four examples: An Introduction to General / Inorganic Chemistry 1. -
Recent Developments in Chalcogen Chemistry
RECENT DEVELOPMENTS IN CHALCOGEN CHEMISTRY Tristram Chivers Department of Chemistry, University of Calgary, Calgary, Alberta, Canada WHERE IS CALGARY? Lecture 1: Background / Introduction Outline • Chalcogens (O, S, Se, Te, Po) • Elemental Forms: Allotropes • Uses • Trends in Atomic Properties • Spin-active Nuclei; NMR Spectra • Halides as Reagents • Cation Formation and Stabilisation • Anions: Structures • Solutions of Chalcogens in Ionic Liquids • Oxides and Imides: Multiple Bonding 3 Elemental Forms: Sulfur Allotropes Sulfur S6 S7 S8 S10 S12 S20 4 Elemental Forms: Selenium and Tellurium Allotropes Selenium • Grey form - thermodynamically stable: helical structure cf. plastic sulfur. R. Keller, et al., Phys. Rev. B. 1977, 4404. • Red form - cyclic Cyclo-Se8 (cyclo-Se7 and -Se6 also known). Tellurium • Silvery-white, metallic lustre; helical structure, cf. grey Se. • Cyclic allotropes only known entrapped in solid-state structures e.g. Ru(Ten)Cl3 (n = 6, 8, 9) M. Ruck, Chem. Eur. J. 2011, 17, 6382 5 Uses – Sulfur Sulfur : Occurs naturally in underground deposits. • Recovered by Frasch process (superheated water). • H2S in sour gas (> 70%): Recovered by Klaus process: Klaus Process: 2 H S + SO 3/8 S + 2 H O 2 2 8 2 • Primary industrial use (70 %): H2SO4 in phosphate fertilizers 6 Uses – Selenium and Tellurium Selenium and Tellurium : Recovered during the refining of copper sulfide ores Selenium: • Photoreceptive properties – used in photocopiers (As2Se3) • Imparts red color in glasses Tellurium: • As an alloy with Cu, Fe, Pb and to harden -
Immobilization of Heavy Metals in Contaminated Soils—Performance Assessment in Conditions Similar to a Real Scenario
applied sciences Article Immobilization of Heavy Metals in Contaminated Soils—Performance Assessment in Conditions Similar to a Real Scenario Antonio A. S. Correia 1,* , Martim P. S. R. Matos 2, Ana R. Gomes 3 and Maria G. Rasteiro 4 1 Chemical Process Engineering and Forest Products Research Centre, Department of Civil Engineering, University of Coimbra, Rua Luís Reis Santos, 3030-788 Coimbra, Portugal 2 Department of Civil Engineering, University of Coimbra, Rua Luís Reis Santos, 3030-788 Coimbra, Portugal; [email protected] 3 Department of Chemical Engineering, University of Coimbra, Rua Sílvio Lima, 3030-790 Coimbra, Portugal; [email protected] 4 Chemical Process Engineering and Forest Products Research Centre, Department of Chemical Engineering, University of Coimbra, Rua Sílvio Lima, 3030-790 Coimbra, Portugal; [email protected] * Correspondence: [email protected] Received: 28 September 2020; Accepted: 7 November 2020; Published: 10 November 2020 Abstract: Soil “health” is becoming an increasing concern of modern societies, namely, at the European level, considering its importance to the fields of food, clean water, biodiversity, and even climate change control. On the other hand, human activities are contributing more and more to induce contamination in soils, especially in industrialized societies. This experimental work studies different additives (carbon nanotubes, clay, and Portland cement) with the aim to evaluate their effect on heavy metals, HMs (lead, cooper, nickel, and zinc) immobilization in a contaminated soil in conditions similar to a real scenario. Suspension adsorption tests (fluid-like condition) were performed aiming to supply preliminary information about the adsorption capacity of the soil towards the different HMs tested, while percolation tests (solid-like conditions) were performed aiming to evaluate the HMs immobilization by different additives in conditions similar to a real situation of soil contamination. -
Periodic Table Trends Periodic Trends
Periodic Table Trends Periodic Trends • Atomic Radius • Ionization Energy • Electron Affinity The Trends in Picture Atomic Radius • Unlike a ball, an atom has fuzzy edges. • The radius of an atom can only be found by measuring the distance between the nuclei of two touching atoms, and then dividing that distance by two. Atomic Radius • Atomic radius is determined by how much the electrons are attracted to the positive nucleus. • The fewer the electrons in each period, the lesser the attraction. • Lesser attraction = • larger nucleus Atomic Radius Trend • Period: in general, as we go across a period from left to right, the atomic radius decreases – Effective nuclear charge increases, therefore the valence electrons are drawn closer to the nucleus, decreasing the size of the atom • Family: in general, as we down a group from top to bottom, the atomic radius increases – Orbital sizes increase in successive principal quantum levels Concept Check • Which should be the larger atom? Why? • O or N N • K or Ca K • Cl or F Cl • Be or Na Na • Li or Mg Mg Ionization Energy • Energy required to remove an electron from an atom • Which atom would be harder to remove an electron from? • Na Cl Ionization Energy • X + energy → X+ + e– X(g) → X+ (g) + e– • First electron removed is IE1 • Can remove more than one electron (IE2 , IE3 ,…) Ex. Magnesium Mg → Mg+ + e– IE1 = 735 kJ/mol Mg+ → Mg2+ + e– IE2 = 1445 kJ/mol Mg2+ → Mg3+ + e– IE3 = 7730 kJ/mol* *Core electrons are bound much more tightly than valence electrons Periodic Ionization Trend • Trend: • Period: -
Honors Chemistry ___/___/___
Name ____________________ Honors Chemistry ___/___/___ Chapter 3 Practice Test Part I: For each of the following, write the symbol of the element that best fits the description given. You may use an element more than once; you may even use it more than twice. (2 point each) 1. Li The alkali metal with the greatest ionization energy. 2. F The halogen with the greatest electronegativity. 3. Rn The noble gas with the greatest atomic radius. 4. Br The fourth period element with the highest electron affinity. 5. Pm The synthetic rare-earth element with the smallest atomic number. 6. Be The alkaline-earth element with the greatest second ionization energy. 7. Sb The fifth period metalloid with the largest atomic radius. 8. He The element on the periodic table with the smallest atomic radius. 9. Ar The third period non-metal with the highest ionization energy. 10. C The second period non-metal with the fewest valence electrons. 11. U The naturally occurring element with the greatest atomic mass. 12. Ne The second period element with the greatest ionization energy. 13. He The element with the greatest ionization energy. 14. Se The chalcogen non-metal with the greatest number of protons. 15. Al The third period metal with a 3+ oxidation number. 16. Fr The element with the lowest ionization energy. 17. Be The alkaline-earth element with the smallest atomic radius. 18. F The element with the greatest electronegativity. 19. At The sixth period element with the greatest electronegativity. 20. B The metalloid with the fewest valence electrons. -
Conceptual Progress for Explaining and Predicting Self-Organization on Anodized Aluminum Surfaces
nanomaterials Review Conceptual Progress for Explaining and Predicting Self-Organization on Anodized Aluminum Surfaces Mikhail Pashchanka Department of Chemistry, Eduard-Zintl-Institute, Technical University of Darmstadt, Alarich-Weiss-Straße 12, 64287 Darmstadt, Germany; [email protected] Abstract: Over the past few years, researchers have made numerous breakthroughs in the field of aluminum anodizing and faced the problem of the lack of adequate theoretical models for the interpretation of some new experimental findings. For instance, spontaneously formed anodic alumina nanofibers and petal-like patterns, flower-like structures observed under AC anodizing conditions, and hierarchical pores whose diameters range from several nanometers to sub-millimeters could be explained neither by the classical field-assisted dissolution theory nor by the plastic flow model. In addition, difficulties arose in explaining the basic indicators of porous film growth, such as the nonlinear current–voltage characteristics of electrochemical cells or the evolution of hexagonal pore patterns at the early stages of anodizing experiments. Such a conceptual crisis resulted in new multidisciplinary investigations and the development of novel theoretical models, whose evolution is discussed at length in this review work. The particular focus of this paper is on the recently developed electroconvection-based theories that allowed making truly remarkable advances in understanding the porous anodic alumina formation process in the last 15 years. Some explanation of the synergy between electrode reactions and transport processes leading to self-organization is provided. Finally, future prospects for the synthesis of novel anodic architectures are discussed. Citation: Pashchanka, M. Conceptual Progress for Explaining Keywords: porous anodic alumina (PAA); chaos and self-organization theory; electroconvection; and Predicting Self-Organization on colloidal gel model; anion exchange; DLVO theory; fluid mechanics; surface chemistry; surface Anodized Aluminum Surfaces.