Periodic Table of Elements with a Key
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The Development of the Periodic Table and Its Consequences Citation: J
Firenze University Press www.fupress.com/substantia The Development of the Periodic Table and its Consequences Citation: J. Emsley (2019) The Devel- opment of the Periodic Table and its Consequences. Substantia 3(2) Suppl. 5: 15-27. doi: 10.13128/Substantia-297 John Emsley Copyright: © 2019 J. Emsley. This is Alameda Lodge, 23a Alameda Road, Ampthill, MK45 2LA, UK an open access, peer-reviewed article E-mail: [email protected] published by Firenze University Press (http://www.fupress.com/substantia) and distributed under the terms of the Abstract. Chemistry is fortunate among the sciences in having an icon that is instant- Creative Commons Attribution License, ly recognisable around the world: the periodic table. The United Nations has deemed which permits unrestricted use, distri- 2019 to be the International Year of the Periodic Table, in commemoration of the 150th bution, and reproduction in any medi- anniversary of the first paper in which it appeared. That had been written by a Russian um, provided the original author and chemist, Dmitri Mendeleev, and was published in May 1869. Since then, there have source are credited. been many versions of the table, but one format has come to be the most widely used Data Availability Statement: All rel- and is to be seen everywhere. The route to this preferred form of the table makes an evant data are within the paper and its interesting story. Supporting Information files. Keywords. Periodic table, Mendeleev, Newlands, Deming, Seaborg. Competing Interests: The Author(s) declare(s) no conflict of interest. INTRODUCTION There are hundreds of periodic tables but the one that is widely repro- duced has the approval of the International Union of Pure and Applied Chemistry (IUPAC) and is shown in Fig.1. -
Dmitri Mendeleev
DOWNLOADABLE EXTRAS Atomic Structure: Part 1 1 Dmitri Mendeleev Dmitri Mendeleev was born on the 8th of February 1834 in Siberia, Russia. His father who was a teacher of the arts and politics, died when he was only thirteen. He was one of a large family and is thought to possibly have had 17 brothers and sisters. Due to his father’s death and a failed family business (a glass factory that burnt down) the family were very poor. Despite this, his mother wanted him to be educated at a higher level so she moved the family to St Petersburg in order for Dmitri to attend school. After graduating he became a teacher in the area of science. His passion was chemistry and he studied the capillarity of liquids (ability of a liquid to fl ow in a narrow space without any suction or pumping, like when water moves against gravity up a straw placed in a glass of water), the components of petrol and the spectroscope (a device that uses light to identify unknown materials). Because chemistry at the time was so disorganised, Mendeleev saw a need to establish a set of rules and guidelines that would be universal (able to be used across the world). He started by writing two very successful text books that included all of his chemistry knowledge. However he felt that this wasn’t enough and that the concepts of chemistry were too broad and unlinked. In 1869 he started to write a system that ordered the elements as these were the main concept behind a lot of other chemistry. -
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 -
Chemistry – Inorganic Chemistry
Answer on Question #53306 – Chemistry – Inorganic Chemistry Question What is oxidation state? How can find out the oxidation state of particular element? Explain its trend in the group and period, give reasons Answer The oxidation state is an indicator of the degree of oxidation (loss of electrons) of an atom in a chemical compound. The oxidation state, which may be positive, negative or equal to zero, is the hypothetical charge that an atom would have if all bonds to atoms of different elements were completely ionic, with no covalent component. To find out the oxidation state of particular element one should use some simple rules: 1. The oxidation state of an element in a simple substance (for example, He or Cl2, or Fe, or C, or whatever containing one type of atoms) is equal to zero. 2. The sum of the oxidation states of all the atoms or ions in a neutral compound is zero. 3. The sum of the oxidation states of all the atoms in an ion is equal to the charge on the ion. 4. The more electronegative element in a substance is given a negative oxidation state. The less electronegative one is given a positive oxidation state. 5. Some elements almost always have the same oxidation states in their compounds: Element Oxidation state Group 1 metals (Li, Na, K, Rb, Cs, Fr) always +1 Group 2 metals (Be, Mg, Ca, Sr, Ba, Ra) always +2 Fluorine (F) always -1 Oxygen (O) usually -2 (except in peroxides (-1) and F2O (+2)) Hydrogen (H) usually +1 (except in metal hydrides (-1)) Having known the oxidation states of these elements in the compound and having known the rule 3, the oxidation state of particular element can be found. -
Electron Configuration Example Script
Electron Configuration Example Script This video demonstrates how to write electron configurations and draw orbital diagrams for main group elements. To write an electron configuration you could memorize the order in which orbitals are filled according to their energy level, but a more convenient method is to use the periodic table. The periodic table is arranged in blocks, each block represents an orbital, and each space in the block counts as one electron. The s block is the first two left-hand columns of the periodic table and includes helium. The p block is the last six columns on the right hand side stating at boron. The d block is the transition metals in the middle of the periodic table, and the f block is the lanthanide and actinide series. To begin start at the top left hand corner of the periodic table and work your way down by reading across a row from left to right and filling in the proper amount of electrons for each orbital until you reach your element. Use the number assigned to each row, 1 thru 7, as the value of the principle quantum number n, when you arrive at the d and f blocks; subtract one from the n value for the d orbitals, and two from the n value for the f orbitals. This periodic table has the electron configuration for each row written along the left hand side using the method just outlined. Let’s use it to write the electron configuration of a neutral bromine atom, a bromine atom has 35 electrons. -
Electron Configurations, Orbital Notation and Quantum Numbers
5 Electron Configurations, Orbital Notation and Quantum Numbers Electron Configurations, Orbital Notation and Quantum Numbers Understanding Electron Arrangement and Oxidation States Chemical properties depend on the number and arrangement of electrons in an atom. Usually, only the valence or outermost electrons are involved in chemical reactions. The electron cloud is compartmentalized. We model this compartmentalization through the use of electron configurations and orbital notations. The compartmentalization is as follows, energy levels have sublevels which have orbitals within them. We can use an apartment building as an analogy. The atom is the building, the floors of the apartment building are the energy levels, the apartments on a given floor are the orbitals and electrons reside inside the orbitals. There are two governing rules to consider when assigning electron configurations and orbital notations. Along with these rules, you must remember electrons are lazy and they hate each other, they will fill the lowest energy states first AND electrons repel each other since like charges repel. Rule 1: The Pauli Exclusion Principle In 1925, Wolfgang Pauli stated: No two electrons in an atom can have the same set of four quantum numbers. This means no atomic orbital can contain more than TWO electrons and the electrons must be of opposite spin if they are to form a pair within an orbital. Rule 2: Hunds Rule The most stable arrangement of electrons is one with the maximum number of unpaired electrons. It minimizes electron-electron repulsions and stabilizes the atom. Here is an analogy. In large families with several children, it is a luxury for each child to have their own room. -
Unit 5.1 Periodic Table: Its Structure and Function
Unit 5.1 Periodic Table: Its Structure and Function Teacher: Dr. Van Der Sluys Objectives • Mendeleev • Information in the Periodic Table – Metals, nonmetals and metalloids – Main Group, Transition Metals, Rare Earth and Actinide Dmitri Mendeleev (1869) In 1869 Mendeleev and Lothar Meyer (Germany) published nearly identical classification schemes for elements known to date. The periodic table is base on the similarity of properties and reactivities exhibited by certain elements. Later, Henri Moseley ( England,1887-1915) established that each elements has a unique atomic number, which is how the current periodic table is organized. http://www.chem.msu.su/eng/misc/mendeleev/welcome.html 1 Information About Each Element Atomic Number 1 H Atomic Symbol Average Atomic 1.00794 Mass Periodic Table Expanded View •The way the periodic table usually seen is a compress view, placing the Lanthanides and actinides at the bottom of the stable. •The Periodic Table can be arrange by subshells. The s-block is Group IA and & IIA, the p-block is Group IIIA - VIIIA. The d-block is the transition metals, and the f-block are the Lanthanides and Actinide metals 2 Periodic Table: Metals and Nonmetals 1 18 IA VIIIA 2 13 14 15 16 17 1 IIA IIIA IVA VA VIA VIIA • Layout of the Periodic Table: Metals vs. nonmetals 2 3 4 5 6 7 8 9 10 11 12 3 IIIB IVB VB VIB VIIB VIIIB IB IIB 4 Nonmetals 5 Metals 6 7 Periodic Table: Classification • Metals - Solids, luster, conduct heat and electricity, malleable and ductile • Nonmetals - Gases, liquids or low melting solids that are sometimes brittle and nonconducting • Metalloids - Have properties of both metals and nonmetals. -
Dmitry I. Mendeleev and His Time
Firenze University Press www.fupress.com/substantia Historical Article Dmitry I. Mendeleev and his time Citation: D. Pushcharovsky (2019) Dmitry I. Mendeleev and his time. Sub- Dmitry Pushcharovsky stantia 3(1): 119-129. doi: 10.13128/ Substantia-173 Lomonosov Moscow State University, Department of Geology, Vorob’evy gori, 1, 119899 Moscow, Russia Copyright: © 2019 D. Pushcharovsky. E-mail: [email protected] This is an open access, peer-reviewed article published by Firenze University Press (http://www.fupress.com/substan- Abstract. The history of the creation of Periodic table and of the Mendeleev’s discovery tia) and distribuited under the terms of Periodic Law is considered. The different approaches used by Mendeleev’s colleagues of the Creative Commons Attribution are discussed. The contribution of the Periodic system to the extension of the scientific License, which permits unrestricted ideas in geology and best of all in geochemistry and mineralogy is illustrated by the use, distribution, and reproduction discovery of new chemical elements and by the isomorphic replacements in minerals. in any medium, provided the original author and source are credited. The details of uneasy history of Mendeleev’s nomination to the St. Petersburg Academy and for the Nobel Prize are given. Data Availability Statement: All rel- evant data are within the paper and its Keywords. Periodic table, isomorphism, Nobel Prize, electronic structure of atom. Supporting Information files. Competing Interests: The Author(s) declare(s) no conflict of interest. Periodic table of chemical elements on the front of the main building of the Central Board of Weights and Measures in St. Petersburg; height – 9 m, area – 69 m2; red colour - ele- ments, known in the Mendeleev lifetime, blue colour – elements discovered after 1907 (Pub- lic domain) Substantia. -
Electron Configuration, and Element No.155 of the Periodic Table of Elements
April, 2011 PROGRESS IN PHYSICS Volume 2 Electron Configuration, and Element No.155 of the Periodic Table of Elements Albert Khazan E-mail: [email protected] Blocks of the Electron Configuration in the atom are considered with taking into ac- count that the electron configuration should cover also element No.155. It is shown that the electron configuration formula of element No.155, in its graphical representation, completely satisfies Gaussian curve. 1 Introduction K L M N O Sum Content in the shells As is known, even the simpliests atoms are very complicate s 2 2 in each shell systems. In the centre of such a system, a massive nucleus p 2 6 8 in each, commencing is located. It consists of protons, the positively charged par- in the 2nd shell ticles, and neutrons, which are charge-free. Masses of pro- d 2 6 10 18 in each, commencing tons and neutrons are almost the same. Such a particle is in the 3rd shell almost two thousand times heavier than the electron. Charges f 2 6 10 14 32 in each, commencing of the proton and the electron are opposite, but the same in in the 4th shell the absolute value. The proton and the neutron differ from g 2 6 10 14 18 50 in each, commencing the viewpoint on electromagnetic interactions. However in in the 5th shell the scale of atomic nuclei they does not differ. The electron, the proton, and the neutron are subatomic articles. The theo- Table 1: Number of electrons in each level. retical physicists still cannot solve Schrodinger’s¨ equation for the atoms containing two and more electrons. -
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. -
Chapter 7 Periodic Properties of the Elements Learning Outcomes
Chapter 7 Periodic Properties of the Elements Learning Outcomes: Explain the meaning of effective nuclear charge, Zeff, and how Zeff depends on nuclear charge and electron configuration. Predict the trends in atomic radii, ionic radii, ionization energy, and electron affinity by using the periodic table. Explain how the radius of an atom changes upon losing electrons to form a cation or gaining electrons to form an anion. Write the electron configurations of ions. Explain how the ionization energy changes as we remove successive electrons, and the jump in ionization energy that occurs when the ionization corresponds to removing a core electron. Explain how irregularities in the periodic trends for electron affinity can be related to electron configuration. Explain the differences in chemical and physical properties of metals and nonmetals, including the basicity of metal oxides and the acidity of nonmetal oxides. Correlate atomic properties, such as ionization energy, with electron configuration, and explain how these relate to the chemical reactivity and physical properties of the alkali and alkaline earth metals (groups 1A and 2A). Write balanced equations for the reactions of the group 1A and 2A metals with water, oxygen, hydrogen, and the halogens. List and explain the unique characteristics of hydrogen. Correlate the atomic properties (such as ionization energy, electron configuration, and electron affinity) of group 6A, 7A, and 8A elements with their chemical reactivity and physical properties. Development of Periodic Table •Dmitri Mendeleev and Lothar Meyer (~1869) independently came to the same conclusion about how elements should be grouped in the periodic table. •Henry Moseley (1913) developed the concept of atomic numbers (the number of protons in the nucleus of an atom) 1 Predictions and the Periodic Table Mendeleev, for instance, predicted the discovery of germanium (which he called eka-silicon) as an element with an atomic weight between that of zinc and arsenic, but with chemical properties similar to those of silicon. -
Hobart Mendeleev 2-3-11.Pdf
Czar Nicholas II and Alexi at Tobolsk, Siberia in 1917 - Beinecke Library, Yale University Dr. David Hobart Los Alamos National Laboratory Academician Boris Myasoedov Secretary General Russian Academy of Sciences U N C L A S S I F I E D LA-UR-09-05702 U N C L A S S I F I E D National Laboratory From Modest Beginnings Dmitri Ivanovich Mendeleev was born on February 8th, 1834 in Verhnie Aremzyani near Tobolsk, Russian Empire From modest beginnings in a small village in Siberia an extraordinary Russian chemist conceived of a profound and revolutionary scientific contribution to modern science: the Periodic Table of the Elements. The Greek Periodic Table ~ 400 BC As with most profound discoveries a number of important developments and observations were made prior to that discovery Definition of an Element In 1661 Boyle criticized the experiments of “alchemists” - Chemistry is the science of the composition of substances - not merely an adjunct to the art of alchemy - Elements are the un-decomposable constituents of material bodies - Understanding the distinction between mixtures and compounds, he made progress in detecting their ingredients - which he termed analysis Robert Boyle 1627-1691 The Atomic Theory The Greek philosopher Democritus first proposed the atomic theory but centuries later John Dalton established the scientific foundation: - All atoms of a given element are identical - The atoms of different elements can be distinguished by their relative weights Democritus of Abdera John Dalton 460-370 BC 1766-1844 Early Knowledge and Discovery The elements gold, silver, copper, tin, Searching for the “Philosopher’s lead, mercury, and others were known Stone” German alchemist Henning from antiquity.