periodic table assignment quizlet

Periodic Table of Elements

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• Atomic number
• Property values
• Logarithmic
• Exponential
• 1 H Hydrogen 1.008
• 2 He Helium 4.0026
• 3 Li Lithium 6.94
• 4 Be Beryllium 9.0122
• 5 B Boron 10.81
• 6 C Carbon 12.011
• 7 N Nitrogen 14.007
• 8 O Oxygen 15.999
• 9 F Fluorine 18.998
• 10 Ne Neon 20.180
• 11 Na Sodium 22.990
• 12 Mg Magnesium 24.305
• 13 Al Aluminium 26.982
• 14 Si Silicon 28.085
• 15 P Phosphorus 30.974
• 16 S Sulfur 32.06
• 17 Cl Chlorine 35.45
• 18 Ar Argon 39.948
• 19 K Potassium 39.098
• 20 Ca Calcium 40.078
• 21 Sc Scandium 44.956
• 22 Ti Titanium 47.867
• 23 V Vanadium 50.942
• 24 Cr Chromium 51.996
• 25 Mn Manganese 54.938
• 26 Fe Iron 55.845
• 27 Co Cobalt 58.933
• 28 Ni Nickel 58.693
• 29 Cu Copper 63.546
• 30 Zn Zinc 65.38
• 31 Ga Gallium 69.723
• 32 Ge Germanium 72.630
• 33 As Arsenic 74.922
• 34 Se Selenium 78.971
• 35 Br Bromine 79.904
• 36 Kr Krypton 83.798
• 37 Rb Rubidium 85.468
• 38 Sr Strontium 87.62
• 39 Y Yttrium 88.906
• 40 Zr Zirconium 91.224
• 41 Nb Niobium 92.906
• 42 Mo Molybdenum 95.95
• 43 Tc Technetium (98)
• 44 Ru Ruthenium 101.07
• 45 Rh Rhodium 102.91
• 46 Pd Palladium 106.42
• 47 Ag Silver 107.87
• 48 Cd Cadmium 112.41
• 49 In Indium 114.82
• 50 Sn Tin 118.71
• 51 Sb Antimony 121.76
• 52 Te Tellurium 127.60
• 53 I Iodine 126.90
• 54 Xe Xenon 131.29
• 55 Cs Caesium 132.91
• 56 Ba Barium 137.33
• 57 La Lanthanum 138.91
• 58 Ce Cerium 140.12
• 59 Pr Praseodymium 140.91
• 60 Nd Neodymium 144.24
• 61 Pm Promethium (145)
• 62 Sm Samarium 150.36
• 63 Eu Europium 151.96
• 64 Gd Gadolinium 157.25
• 65 Tb Terbium 158.93
• 66 Dy Dysprosium 162.50
• 67 Ho Holmium 164.93
• 68 Er Erbium 167.26
• 69 Tm Thulium 168.93
• 70 Yb Ytterbium 173.05
• 71 Lu Lutetium 174.97
• 72 Hf Hafnium 178.49
• 73 Ta Tantalum 180.95
• 74 W Tungsten 183.84
• 75 Re Rhenium 186.21
• 76 Os Osmium 190.23
• 77 Ir Iridium 192.22
• 78 Pt Platinum 195.08
• 79 Au Gold 196.97
• 80 Hg Mercury 200.59
• 81 Tl Thallium 204.38
• 82 Pb Lead 207.2
• 83 Bi Bismuth 208.98
• 84 Po Polonium (209)
• 85 At Astatine (210)
• 86 Rn Radon (222)
• 87 Fr Francium (223)
• 88 Ra Radium (226)
• 89 Ac Actinium (227)
• 90 Th Thorium 232.04
• 91 Pa Protactinium 231.04
• 92 U Uranium 238.03
• 93 Np Neptunium (237)
• 94 Pu Plutonium (244)
• 95 Am Americium (243)
• 96 Cm Curium (247)
• 97 Bk Berkelium (247)
• 98 Cf Californium (251)
• 99 Es Einsteinium (252)
• 100 Fm Fermium (257)
• 101 Md Mendelevium (258)
• 102 No Nobelium (259)
• 103 Lr Lawrencium (266)
• 104 Rf Rutherfordium (267)
• 105 Db Dubnium (268)
• 106 Sg Seaborgium (269)
• 107 Bh Bohrium (270)
• 108 Hs Hassium (277)
• 109 Mt Meitnerium (278)
• 110 Ds Darmstadtium (281)
• 111 Rg Roentgenium (282)
• 112 Cn Copernicium (285)
• 113 Nh Nihonium (286)
• 114 Fl Flerovium (289)
• 115 Mc Moscovium (290)
• 116 Lv Livermorium (293)
• 117 Ts Tennessine (294)
• 118 Og Oganesson (294)

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• The first periodic table
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• Periodicity of properties of the elements
• Other chemical and physical classifications

What is the periodic table?

Where does the periodic table come from, why does the periodic table split.

• Is mathematics a physical science?
• How is the atomic number of an atom defined?

periodic table

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• UEN Digital Press with Pressbooks - Introductory Chemistry - The Periodic Table
• Chemistry LibreTexts - The Periodic Table
• Ohio State University - Origins - Mendeleev's Periodic Table
• National Center for Biotechnology Information - PubChem - Periodic Table of Elements
• NeoK12 - Educational Videos and Games for School Kids - Periodic Table
• LiveScience - Periodic Table of the Elements
• Khan Academy - The periodic table, electron shells, and orbitals
• Western Oregon University - A brief history of the development of Periodic Table
• Royal Society of Chemistry - Patterns in the Periodic Table
• periodic table - Children's Encyclopedia (Ages 8-11)
• periodic table - Student Encyclopedia (Ages 11 and up)
• Table Of Contents

The periodic table is a tabular array of the chemical elements organized by atomic number , from the element with the lowest atomic number, hydrogen , to the element with the highest atomic number, oganesson . The atomic number of an element is the number of protons in the nucleus of an atom of that element. Hydrogen has 1 proton, and oganesson has 118.

What do periodic table groups have in common?

The groups of the periodic table are displayed as vertical columns numbered from 1 to 18. The elements in a group have very similar chemical properties, which arise from the number of valence electrons present—that is, the number of electrons in the outermost shell of an atom .

The arrangement of the elements in the periodic table comes from the electronic configuration of the elements. Because of the Pauli exclusion principle , no more than two electrons can fill the same orbital. The first row of the periodic table consists of just two elements, hydrogen and helium . As atoms have more electrons, they have more orbits available to fill, and thus the rows contain more elements farther down in the table.

The periodic table has two rows at the bottom that are usually split out from the main body of the table. These rows contain elements in the lanthanoid and actinoid series, usually from 57 to 71 ( lanthanum to lutetium ) and 89 to 103 ( actinium to lawrencium ), respectively. There is no scientific reason for this. It is merely done to make the table more compact.

periodic table , in chemistry , the organized array of all the chemical elements in order of increasing atomic number —i.e., the total number of protons in the atomic nucleus. When the chemical elements are thus arranged, there is a recurring pattern called the “periodic law” in their properties, in which elements in the same column (group) have similar properties. The initial discovery, which was made by Dmitry I. Mendeleev in the mid-19th century, has been of inestimable value in the development of chemistry .

It was not actually recognized until the second decade of the 20th century that the order of elements in the periodic system is that of their atomic numbers, the integers of which are equal to the positive electrical charges of the atomic nuclei expressed in electronic units. In subsequent years great progress was made in explaining the periodic law in terms of the electronic structure of atoms and molecules. This clarification has increased the value of the law, which is used as much today as it was at the beginning of the 20th century, when it expressed the only known relationship among the elements.

History of the periodic law

The early years of the 19th century witnessed a rapid development in analytical chemistry—the art of distinguishing different chemical substances—and the consequent building up of a vast body of knowledge of the chemical and physical properties of both elements and compounds . This rapid expansion of chemical knowledge soon necessitated classification , for on the classification of chemical knowledge are based not only the systematized literature of chemistry but also the laboratory arts by which chemistry is passed on as a living science from one generation of chemists to another. Relationships were discerned more readily among the compounds than among the elements; it thus occurred that the classification of elements lagged many years behind that of compounds. In fact, no general agreement had been reached among chemists as to the classification of elements for nearly half a century after the systems of classification of compounds had become established in general use.

J.W. Döbereiner in 1817 showed that the combining weight, meaning atomic weight , of strontium lies midway between those of calcium and barium , and some years later he showed that other such “ triads ” exist (chlorine, bromine , and iodine [halogens] and lithium , sodium , and potassium [alkali metals]). J.-B.-A. Dumas, L. Gmelin, E. Lenssen, Max von Pettenkofer, and J.P. Cooke expanded Döbereiner’s suggestions between 1827 and 1858 by showing that similar relationships extended further than the triads of elements, fluorine being added to the halogens and magnesium to the alkaline-earth metals, while oxygen , sulfur , selenium , and tellurium were classed as one family and nitrogen , phosphorus , arsenic , antimony , and bismuth as another family of elements.

Attempts were later made to show that the atomic weights of the elements could be expressed by an arithmetic function , and in 1862 A.-E.-B. de Chancourtois proposed a classification of the elements based on the new values of atomic weights given by Stanislao Cannizzaro’s system of 1858. De Chancourtois plotted the atomic weights on the surface of a cylinder with a circumference of 16 units, corresponding to the approximate atomic weight of oxygen. The resulting helical curve brought closely related elements onto corresponding points above or below one another on the cylinder, and he suggested in consequence that “the properties of the elements are the properties of numbers,” a remarkable prediction in the light of modern knowledge.

Classification of the elements

In 1864, J.A.R. Newlands proposed classifying the elements in the order of increasing atomic weights, the elements being assigned ordinal numbers from unity upward and divided into seven groups having properties closely related to the first seven of the elements then known: hydrogen , lithium, beryllium , boron , carbon , nitrogen, and oxygen. This relationship was termed the law of octaves, by analogy with the seven intervals of the musical scale.

Then in 1869, as a result of an extensive correlation of the properties and the atomic weights of the elements, with special attention to valency (that is, the number of single bonds the element can form), Mendeleev proposed the periodic law, by which “the elements arranged according to the magnitude of atomic weights show a periodic change of properties.” Lothar Meyer had independently reached a similar conclusion, published after the appearance of Mendeleev’s paper.