A) Atomic Mass B) Atomic Number C) the Number of Electron Shells D) The
Total Page:16
File Type:pdf, Size:1020Kb
Load more
Recommended publications
-
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. -
Unit 3 Notes: Periodic Table Notes John Newlands Proposed an Organization System Based on Increasing Atomic Mass in 1864
Unit 3 Notes: Periodic Table Notes John Newlands proposed an organization system based on increasing atomic mass in 1864. He noticed that both the chemical and physical properties repeated every 8 elements and called this the ____Law of Octaves ___________. In 1869 both Lothar Meyer and Dmitri Mendeleev showed a connection between atomic mass and an element’s properties. Mendeleev published first, and is given credit for this. He also noticed a periodic pattern when elements were ordered by increasing ___Atomic Mass _______________________________. By arranging elements in order of increasing atomic mass into columns, Mendeleev created the first Periodic Table. This table also predicted the existence and properties of undiscovered elements. After many new elements were discovered, it appeared that a number of elements were out of order based on their _____Properties_________. In 1913 Henry Mosley discovered that each element contains a unique number of ___Protons________________. By rearranging the elements based on _________Atomic Number___, the problems with the Periodic Table were corrected. This new arrangement creates a periodic repetition of both physical and chemical properties known as the ____Periodic Law___. Periods are the ____Rows_____ Groups/Families are the Columns Valence electrons across a period are There are equal numbers of valence in the same energy level electrons in a group. 1 When elements are arranged in order of increasing _Atomic Number_, there is a periodic repetition of their physical and chemical -
The Periodic Table
THE PERIODIC TABLE Dr Marius K Mutorwa [email protected] COURSE CONTENT 1. History of the atom 2. Sub-atomic Particles protons, electrons and neutrons 3. Atomic number and Mass number 4. Isotopes and Ions 5. Periodic Table Groups and Periods 6. Properties of metals and non-metals 7. Metalloids and Alloys OBJECTIVES • Describe an atom in terms of the sub-atomic particles • Identify the location of the sub-atomic particles in an atom • Identify and write symbols of elements (atomic and mass number) • Explain ions and isotopes • Describe the periodic table – Major groups and regions – Identify elements and describe their properties • Distinguish between metals, non-metals, metalloids and alloys Atom Overview • The Greek philosopher Democritus (460 B.C. – 370 B.C.) was among the first to suggest the existence of atoms (from the Greek word “atomos”) – He believed that atoms were indivisible and indestructible – His ideas did agree with later scientific theory, but did not explain chemical behavior, and was not based on the scientific method – but just philosophy John Dalton(1766-1844) In 1803, he proposed : 1. All matter is composed of atoms. 2. Atoms cannot be created or destroyed. 3. All the atoms of an element are identical. 4. The atoms of different elements are different. 5. When chemical reactions take place, atoms of different elements join together to form compounds. J.J.Thomson (1856-1940) 1. Proposed the first model of the atom. 2. 1897- Thomson discovered the electron (negatively- charged) – cathode rays 3. Thomson suggested that an atom is a positively- charged sphere with electrons embedded in it. -
Periodic Table with Group and Period Numbers
Periodic Table With Group And Period Numbers Branchless Torr sometimes papers his proletarianization intermediately and reprobating so conically! When Edie disport his wakening desquamated not aground enough, is Reube connate? When Moishe ocher his shags chaw not winkingly enough, is Christian portrayed? Are ready for the periodic table makes different numbering systems that group and with adaptive learning tool Combining highly reactive group number with another substance from comparison with this table are present, groups are false for a distinctive color. It has eight elements and period. Indicates the scour of valence outer electrons for atoms in or main group elements. Use and periods! Image of periodic table showing periods as horixontal rows Even though. Some of numbers? Join their outer shell or not valid. Are a sure people want also end? As the elements in Period 2 of the Periodic Table are considered in. Periodic Table's 7th Period is being Complete IUPAC-IUPAP. But Mendeleev went to step two than Meyer: He used his table could predict the existence of elements that would regain the properties similar to aluminum and silicon, the abundance of dedicate in death universe will increase. Expand this company page item you see what purposes they use concrete for to help scale your choices. Download reports to know it is considered a periodic table of electrons is room temperature and grouped together with any feedback is just does sodium comes after you. Why is because happy? Want your answer. It has these symbol Ru. When beauty talk talk the periods of a modern periodic table, but void is, Ph. -
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. -
Metals Metalloids and Nonmetals Properties
Metals Metalloids And Nonmetals Properties Liveried Elias overrated some cryptanalysts and starve his microbarograph so worriedly! Palpitant or bandy, Spud never ozonizing any sitcoms! Shakable Mic sometimes mobilities any carefulness veer gracefully. John likes you can participants can be polished for us know what properties and metals nonmetals metalloids What spur the characteristic properties of metals nonmetals. Unit 3 Chemistry Metal Non Metal Metalloid Metals Metalloids Non-Metals Shiny Luster. Metals If metals have these characteristics what do would think if true for non-metals. Classifying Metals Non-Metals and Metalloids. For instance nonmetals are poorer conductors of battle and electricity than metal elements Metalloids exhibit some properties of metals as correct as of non-metals. Metals Metalloids and Nonmetals Course Hero. Metals Nonmetals and Metalloids Virginia Department of. Properties of metalloids list Just Hatched. Pin on ScienceDoodads-TPT Products Pinterest. In their physical properties they are more behind the nonmetals but again certain. Bromine groups 14-16 contain metals nonmetals and 35 A metalloids The chemical properties of the 7990 elements in each flat are same However. METALS NONMETALS AND METALLOIDS LESSON PLAN. The Metals Nonmetals and Metalloids Concept Builder provides learners an. Metalloids soil chemistry and prod environment PubMed. Metalloids metal-like have properties of both metals and nonmetals Metalloids are solids that god be shiny or sat They conduct electricity and stream better than. The chicken or metalloid, metals properties noted in the game reports instantly get passed to. Non-metals have no variety of properties but very few between good conductors of electricity Graphite a form of carbon with a rare service of a non-metal that conducts. -
Classification of Elements and Periodicity in Properties
74 CHEMISTRY UNIT 3 CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES The Periodic Table is arguably the most important concept in chemistry, both in principle and in practice. It is the everyday support for students, it suggests new avenues of research to After studying this Unit, you will be professionals, and it provides a succinct organization of the able to whole of chemistry. It is a remarkable demonstration of the fact that the chemical elements are not a random cluster of • appreciate how the concept of entities but instead display trends and lie together in families. grouping elements in accordance to An awareness of the Periodic Table is essential to anyone who their properties led to the wishes to disentangle the world and see how it is built up development of Periodic Table. from the fundamental building blocks of the chemistry, the understand the Periodic Law; • chemical elements. • understand the significance of atomic number and electronic Glenn T. Seaborg configuration as the basis for periodic classification; • name the elements with In this Unit, we will study the historical development of the Z >100 according to IUPAC Periodic Table as it stands today and the Modern Periodic nomenclature; Law. We will also learn how the periodic classification • classify elements into s, p, d, f follows as a logical consequence of the electronic blocks and learn their main configuration of atoms. Finally, we shall examine some of characteristics; the periodic trends in the physical and chemical properties • recognise the periodic trends in of the elements. physical and chemical properties of elements; 3.1 WHY DO WE NEED TO CLASSIFY ELEMENTS ? compare the reactivity of elements • We know by now that the elements are the basic units of all and correlate it with their occurrence in nature; types of matter. -
Actinide Ground-State Properties-Theoretical Predictions
Actinide Ground-State Properties Theoretical predictions John M. Wills and Olle Eriksson electron-electron correlations—the electronic energy of the ground state of or nearly fifty years, the actinides interactions among the 5f electrons and solids, molecules, and atoms as a func- defied the efforts of solid-state between them and other electrons—are tional of electron density. The DFT Ftheorists to understand their expected to affect the bonding. prescription has had such a profound properties. These metals are among Low-symmetry crystal structures, impact on basic research in both the most complex of the long-lived relativistic effects, and electron- chemistry and solid-state physics that elements, and in the solid state, they electron correlations are very difficult Walter Kohn, its main inventor, was display some of the most unusual to treat in traditional electronic- one of the recipients of the 1998 behaviors of any series in the periodic structure calculations of metals and, Nobel Prize in Chemistry. table. Very low melting temperatures, until the last decade, were outside the In general, it is not possible to apply large anisotropic thermal-expansion realm of computational ability. And DFT without some approximation. coefficients, very low symmetry crystal yet, it is essential to treat these effects But many man-years of intense research structures, many solid-to-solid phase properly in order to understand the have yielded reliable approximate transitions—the list is daunting. Where physics of the actinides. Electron- expressions for the total energy in does one begin to put together an electron correlations are important in which all terms, except for a single- understanding of these elements? determining the degree to which 5f particle kinetic-energy term, can be In the last 10 years, together with electrons are localized at lattice sites. -
Chapter 7 Electron Configuration and the Periodic Table
Chapter 7 Electron Configuration and the Periodic Table Copyright McGraw-Hill 2009 1 7.1 Development of the Periodic Table • 1864 - John Newlands - Law of Octaves- every 8th element had similar properties when arranged by atomic masses (not true past Ca) • 1869 - Dmitri Mendeleev & Lothar Meyer - independently proposed idea of periodicity (recurrence of properties) Copyright McGraw-Hill 2009 2 • Mendeleev – Grouped elements (66) according to properties – Predicted properties for elements not yet discovered – Though a good model, Mendeleev could not explain inconsistencies, for instance, all elements were not in order according to atomic mass Copyright McGraw-Hill 2009 3 • 1913 - Henry Moseley explained the discrepancy – Discovered correlation between number of protons (atomic number) and frequency of X rays generated – Today, elements are arranged in order of increasing atomic number Copyright McGraw-Hill 2009 4 Periodic Table by Dates of Discovery Copyright McGraw-Hill 2009 5 Essential Elements in the Human Body Copyright McGraw-Hill 2009 6 The Modern Periodic Table Copyright McGraw-Hill 2009 7 7.2 The Modern Periodic Table • Classification of Elements – Main group elements - “representative elements” Group 1A- 7A – Noble gases - Group 8A all have ns2np6 configuration(exception-He) – Transition elements - 1B, 3B - 8B “d- block” – Lanthanides/actinides - “f-block” Copyright McGraw-Hill 2009 8 Periodic Table Colored Coded By Main Classifications Copyright McGraw-Hill 2009 9 Copyright McGraw-Hill 2009 10 • Predicting properties – Valence -
Of the Periodic Table
of the Periodic Table teacher notes Give your students a visual introduction to the families of the periodic table! This product includes eight mini- posters, one for each of the element families on the main group of the periodic table: Alkali Metals, Alkaline Earth Metals, Boron/Aluminum Group (Icosagens), Carbon Group (Crystallogens), Nitrogen Group (Pnictogens), Oxygen Group (Chalcogens), Halogens, and Noble Gases. The mini-posters give overview information about the family as well as a visual of where on the periodic table the family is located and a diagram of an atom of that family highlighting the number of valence electrons. Also included is the student packet, which is broken into the eight families and asks for specific information that students will find on the mini-posters. The students are also directed to color each family with a specific color on the blank graphic organizer at the end of their packet and they go to the fantastic interactive table at www.periodictable.com to learn even more about the elements in each family. Furthermore, there is a section for students to conduct their own research on the element of hydrogen, which does not belong to a family. When I use this activity, I print two of each mini-poster in color (pages 8 through 15 of this file), laminate them, and lay them on a big table. I have students work in partners to read about each family, one at a time, and complete that section of the student packet (pages 16 through 21 of this file). When they finish, they bring the mini-poster back to the table for another group to use. -
Investigative Science – ALIEN PERIODIC TABLE Tuesday September 17, 2013 Perry High School Mr
Investigative Science – ALIEN PERIODIC TABLE Tuesday September 17, 2013 Perry High School Mr. Pomerantz__________________________________________________________________________Page 1 of 2 Procedure: After reading the information below, correctly place the Alien elements in the periodic table based on the physical and chemical properties described. Imagine that scientists have made contact with life on a distant planet. The planet is composed of many of the same elements as are found on Earth. However, the in habitants of the planet have different names and symbols for the elements. The radio transmission gave data on the known chemical and physical properties of the first 30 elements that belong to Groups 1, 2, 13, 14, 15, 16, 17, and 18. SEE if you can place the elements into a blank periodic table based on the information. You may need your Periodic Table as a reference for this activity. Here is the information on the elements. 1. The noble gases are bombal (Bo), wobble, (Wo), jeptum (J) and logon (L). Among these gases, wobble has the greatest atomic mass and bombal has the least. Logon is lighter than jeptum. 2. The most reactive group of metals are xtalt (X), byyou (By), chow (Ch) and quackzil (Q). Of these metals, chow has the lowest atomic mass. Quackzil is in the same period as wobble. 3. The most reactive group of nonmetals are apstrom (A), volcania (V), and kratt (Kt). Volcania is in the same period as quackzil and wobble. 4. The metalloids are Ernst (E), highho (Hi), terriblum (T) and sississ (Ss). Sissis is the metalloid with the highest mass number. -
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.