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Chapter 5 Chemical Periodicity Classification of the Elements OBJECTIVES: �Explain why you can infer the properties of an element based on those of other elements in the periodic table. �Use electron configurations to classify elements as noble gases, representative elements, transition metals, or inner transition metals. GHS Honors Chem GHS Honors Chem Periodic Table Revisited Mendeleev’s Table � Russian scientist Dmitri Mendeleev � Grouped elements in columns by similar taught chemistry in terms of properties in order of increasing atomic properties. mass. � Mid 1800’s - molar masses of � Found some inconsistencies - felt that elements were known. the properties were more important than the mass, so switched order. � Wrote down the elements in order of � Also found some gaps. increasing mass. � Must be undiscovered elements. � Found a pattern of repeating � Predicted their properties before they properties. were found. GHS Honors Chem GHS Honors Chem Mendeleev's Periodic Table The Modern Periodic Table (1871) � Elements are still grouped by properties. � Similar properties are in the same column. � In 1913, Moseley changed the order to increasing atomic number. � This added a column of elements Mendeleev didn’t know about. � The noble gases weren’t found because they didn’t react with anything. GHS Honors Chem GHS Honors Chem 1 � Horizontal rows are called Periods Vertical columns called groups � There are 7 periods Elements are placed in columns by 1 similar properties 2 Also called families 3 4 5 6 7 GHS Honors Chem GHS Honors Chem The elements in the A groups are called the REPRESENTATIVE 8A 1A elements 0 The group B are called the 2A outer s or p filling 3A 4A 5A 6A7A transition elements These are called the inner transition elements, and they belong here GHS Honors Chem GHS Honors Chem � Group 1A are the alkali metals � Group 7A is called the Halogens � Group 2A are the alkaline earth metals � Group 8A are the Noble Gases GHS Honors Chem GHS Honors Chem 2 Why is the Periodic Table arranged H 1 Group 1A Alkali metals in Groups and Periods? 1 1s • 1 Valence Electron Li 2 1 • s1 configuration 3 1s 2s � The part of the atom another atom sees 2 2 6 1 • Become +1 ions to is the electron cloud. Na 1s 2s 2p 3s obtain the OCTET of More importantly the outside orbitals. 11 electrons � K 2 2 6 2 6 1 19 1s 2s 2p 3s 3p 4s � The orbitals fill up in a regular pattern. Rb 2 2 6 2 6 2 10 6 1 � The outside orbital electron 37 1s 2s 2p 3s 3p 4s 3d 4p 5s configuration, or VALENCE electron Cs 2 2 6 2 6 2 10 6 2 10 6 1 configuration, repeats. 55 1s 2s 2p 3s 3p 4s 3d 4p 5s 4d 5p 6s � The properties of atoms repeat. Fr 2 2 6 2 6 2 10 6 2 10 6 2 87 1s 2s 2p 3s 3p 4s 3d 4p 5s 4d 5p 6s 4 14 10 6 1 f 5d 6p 7s GHS Honors Chem GHS Honors Chem Group 2A Alkaline Earth Metals Group 7A Halogens 2 2 • 2 Valence Electrons • 7 Valence Electrons 4Be: 1s 2s • s2 configuration 2 5 • Become +2 ions to • s p configuration 2 2 5 2 2 6 2 • Become -1 ions to achieve 1s 2s 2p 9F 12Mg: 1s 2s 2p 3s obtain OCTET of 2 2 6 2 6 2 their octet of electrons 2 2 6 2 5 20Ca: 1s 2s 2p 3s 3p 4s electrons 1s 2s 2p 3s 3p 17Cl 2 2 6 2 6 2 10 5 2 2 6 2 6 2 10 6 2 1s 2s 2p 3s 3p 4s 3d 4p 35Br 38Sr: 1s 2s 2p 3s 3p 4s 3d 4p 5s 2 2 6 2 6 2 10 6 2 10 5 2 2 6 2 6 2 10 6 2 10 1s 2s 2p 3s 3p 4s 3d 4p 5s 4d 5p 53I 56Ba: 1s 2s 2p 3s 3p 4s 3d 4p 5s 4d 2 2 6 2 6 2 10 6 2 10 6 2 14 10 5 6 2 1s 2s 2p 3s 3p 4s 3d 4p 5s 4d 5p 6s 4f 5d 6p 85At 5p 6s 2 2 6 2 6 2 10 6 2 10 6 88Ra: 1s 2s 2p 3s 3p 4s 3d 4p 5s 4d 5p 2 14 10 6 2 6s 4f 5d 6p 7s GHS Honors Chem GHS Honors Chem Group 8A Noble Gases 2He Can we determine an element • 8 Valence Electrons 1s 2 simply from the Valence Electron 2 6 • s p configuration Ne 2 2 6 Configuration? • Not reactive, have their 1s 2s 2p 10 octet of electrons 2 2 6 2 6 Ar 1s 2s 2p 3s 3p 18 Let’s try it … 2 2 6 2 6 2 10 6 Kr 1s 2s 2p 3s 3p 4s 3d 4p 36 1. 3s2 Mg 2 2 6 2 6 2 10 6 2 10 6 2 4 1s 2s 2p 3s 3p 4s 3d 4p 5s 4d 5p Xe 2. 5s 5p Te 54 2 6 2 2 6 2 6 2 10 6 2 10 3. 4s 3d Fe 1s 2s 2p 3s 3p 4s 3d 4p 5s 4d Rn 6 2 14 10 6 86 5p 6s 4f 5d 6p GHS Honors Chem GHS Honors Chem 3 Lewis Dot Structures Lewis Dot Structures � Lewis Dot structures are helpful in K The number of unpaired visualizing bonding between atoms. dots corresponds to Ca the number of bonds � Dots correspond to the number of In that the atom can valence electrons. These are the form in a compound. electrons that are involved in C interactions between atoms. P What about ions? � Dots are placed around the element’s 2- symbol, 1 at a time, until pairing is S 0 necessary. Br- F GHS Honors Chem GHS Honors Chem Lewis Dot Structures GHS Honors Chem 4
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