Slide 1 / 163 Slide 2 / 163 Chemistry The Periodic Table 2015-11-16 www.njctl.org Slide 3 / 163 Slide 4 / 163 Table of Contents: The Periodic Table Click on the topic to go to that section · Periodic Table The Periodic Table · Periodic Table & Electron Configurations · Effective Nuclear Charge · Periodic Trends: Atomic Radius · Periodic Trends: Ionization Energy · Periodic Trends: Electronegativity · Periodic Trends: Metallic Character Return to Table of Contents Slide 5 / 163 Slide 6 / 163 Identifying Properties of Atoms Identifying Properties of Atoms Now that we know where We can look at them as individual yet (or approximately where) interacting chemicals, and we are to find the parts of atoms, able to group them based, not only on we can start to the properties they present when in understand how these isolation, but also the properties they factors all come together reveal when exposed to other to affect how we view the elements or compounds. elements.
Slide 7 / 163 Slide 8 / 163 "Periodic" Table of Elements "Periodic" Table of Elements The Periodic Table of Elements Why is one of the most useful tools ever created by humans contains physical and chemical called the "Periodic Table"? information about every element that matter can be made of in the When scientists were organizing the known elements, they Universe. noticed that certain patterns of chemical and physical behavior kept repeating themselves. The Pillars of Creation, part of the Eagle Nebula shown to the right, These elements *is a cloud of interstellar gases are all shiny 7,000 light years from Earth made Courtesy of Hubble Telescope metals and react up of the same gaseous elements violently in water. found on the Periodic Table. *NASA recently captured this image; however, the Pillars of Creation no longer exists. The Eagle Nebula was destroyed by a Supernova around 6000 years ago, but from These elements our viewpoint, it will be visible for another 1000 years. are all very stable gases. Slide 9 / 163 Slide 10 / 163 "Periodic" Table of Elements "Periodic" Table of Elements These patterns were so predictable that Dmitri Mendeleev, the scientist who formulated the Periodic Law, was actually able to predict the existence of elements #31 and #32 and their approximate masses before they were discovered based on the existing patterns of known elements. Gallium, 31 Ga Germanium, 32 Ge Mendeleev's work preceded the discovery of subatomic particles. Slide 11 / 163 Slide 12 / 163 History of the Periodic Table Periodic Table Mendeleev argued that elemental The periodic table is made of rows and columns: properties are periodic functions of their atomic weights. Rows in the periodic table are called Periods. Columns in the periodic table are called Groups. We now know that element properties are periodic functions of their atomic number. Groups are sometimes referred to as Families , but "groups" is more traditional. Atoms are listed on the periodic table in rows, based on number of protons.
Slide 13 / 163 Slide 14 / 163 1 The elements in the Periodic Table are arranged from left groups to right in order of increasing ___. A mass 1 2 B number of neutrons periods 3 4 C number of protons 5 6 * D number of protons and electrons 7 ** * 6 ** 7 Slide 15 / 163 Slide 16 / 163 2 What is the atomic number for the element in 3 What is the atomic number for the element period 3, group 16? in period 5, group 3? Slide 17 / 163 Slide 18 / 163 Groups of Elements Metals, Nonmetals, and Metalloids The periodic table can be divided into metals (blue) and nonmetals (yellow) . A few elements retain some of the properties of metals and nonmetals, they are called metalloids (pink). B metals metalloids nonmetals Si Ge As Sb Te ? Enjoy Tom Lehrer's Famous Element Song!
Slide 19 / 163 Slide 20 / 163 Group 1 Alkali Metals Special Groups (very reactive metals) Some groups have distinctive properties and are given special names. Alkali Metals Alkaline Earth Metals Alkali Metals Noble Gases Halogens Transition Metals Slide 21 / 163 Slide 22 / 163 Groups 3 - 12 Transition Metals Group 2 Alkaline Earth Metals (low reactivity, typical metals) (reactive metals) Alkaline Earth Metals Transition Metals Slide 23 / 163 Slide 24 / 163 Group 17 Halogens Group 16 Oxygen Family (highly reactive, nonmetals) (elements of fire) Halogens
Slide 25 / 163 Slide 26 / 163 Group 18 Noble Gases (nearly inert) Major Groups of the Periodic Table Alkaline Earth Metals Noble Gases Noble Gases Alkali Metals Halogens Transition Metals Slide 27 / 163 Slide 28 / 163 4 To which group on the periodic table does Iodine 5 To which group on the periodic table does Neon belong? belong? Alkali Metals Noble Gases A A Alkali Metals B Transition Metals B C Noble Gases Transition Metals C Alkaline Earth Metals Halogens D D Slide 29 / 163 Slide 30 / 163 6 To which group on the periodic table does 7 To which group on the periodic table does Iron Fluorine belong? belong? A Alkali Metals A Alkali Metals Transition Metals Transition Metals B B Noble Gases C Halogens C Halogens D Alkaline Earth Metals D
Slide 31 / 163 Slide 32 / 163 8 To which group on the periodic table does 9 Two elements are studied. One with atomic Beryllium belong? number X and one with atomic number X+1. It is known that element X is a Noble Gas. Which A Alkali Metals group on the periodic table is X+1 in? B Transition Metals Transition Metals A C Halogens Halogens B D Alkaline Earth Metals C Alkali Metals D There is no way to tell Slide 33 / 163 Slide 34 / 163 Periodic Table & Electron Configuration The elements are arranged by groups with Alkaline Earth Metals Alkali Metals Noble Gases similar reactivity. Halogens Periodic Table & Electron How an element Transition Metals Configurations reacts depends on how its electrons are arranged . . . . . . we now know that elements in the same groups, with the same chemical properties have very similar electron configurations. Return to Table of Contents Slide 35 / 163 Slide 36 / 163 Periodic Table & Electron Configuration Periodic Table & Electron Configuration 1A 2A 8A 1 2 18 3A 4A 5A 6A 7A 13 14 15 16 17 8B } 3B 4B 5B 6B 7B 1B 2B Click here to view an Interactive Periodic Table 3 4 5 6 7 8 9 10 11 12 that shows orbitals for each Element Click here for an electron orbital game. There are two methods for labeling the groups, the older method shown in black on the top and the newer method shown in blue on the bottom.
Slide 37 / 163 Slide 38 / 163 Group Names 10 The highlighted elements below are in the ___. Electron Group Name Group # Characteristic A s block Configuration B d block Alkali Metals 1 s 1 ending Very reactive C p block Alkaline Earth 2 s 2 ending Reactive D f block Metals Somewhat Transition ns 2 , (n-1)d 3-12 (d block) reactive, typical ending Metals metals Somewhat Inner Transition ns 2 , (n-2)f f block reactive, Metals ending radioactive Halogens 17 s 2 p 5 ending Highly reactive Noble Gases 18 s 2 p 6 ending Nonreactive Slide 39 / 163 Slide 40 / 163 11 The highlighted elements below are in the ___. 12 The highlighted elements below are in the ___. A s block A s block B d block B d block C p block C p block D f block D f block Slide 41 / 163 Slide 42 / 163 13 Elements in each group on the Periodic Table have 14 The electron configuration ending ns 2 p 6 belongs in which similar ___. group of the periodic table? A Alkali Metals A mass B Alkaline Earth Metals B number of neutrons C Halogens D Noble Gases C number of protons and electrons D electron configurations
Slide 43 / 163 Slide 44 / 163 Periodic Table with f block in Place 15 An unknown element has an electron configuration ending in s 2 . It is most likely in which group? Here is the Periodic Table with the f block in sequence. Why isn't this the more commonly used version of the table? A Alkaline Earth Metals 1s 1s B Halogens 2s 2p 3s 3p C Alkali Metals 4s 4p 3d 5s 5p 4d D Transition Metals 57 71 6s 4f 5d 6p La Lu 89 103 5f 7s 6d 7p Ac Lr Slide 45 / 163 Slide 46 / 163 Shorthand Configurations Shorthand Configurations Example: Sodium (Na) Noble Gas elements are used to write shortened electron configurations. To write a Shorthand Configuration for an element: (1) Write the Symbol of the Noble Gas element from the row before it in brackets [ ]. (2) Add the remaining electrons by starting at the s orbital of the row that the element is in until the configuration is complete. Electron Configuration: 1s 2 2s 2 2p 6 3s 1 Neon's electron configuration Shorthand Configuration: [ Ne ] 3s 1 Slide 47 / 163 Slide 48 / 163 Fill in Shorthand Configurations 16 What would be the expected "shorthand" electron configuration for Sulfur (S)? Shorthand Configuration Element A [He]3s 2 3p 4 Slide for Answers B [Ar]3s 2 4p 4 C [Ne]3s 2 3p 3 D [Ne]3s 2 3p 4
Recommend
More recommend
