Page 1. 3 Rules for Filling Electrons. Electron Configurations
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1 Electron Spin Quantum Number 1 Diamagnetic: : NOT attracted to a magnetic field- all electrons are paired Paramagnetic: : substance is attracted to a magnetic field. Substance has unpaired electrons. 2 3 Rules for Filling Electrons Aufbau Principle lowest energy to highest energy-regardless of numbers Hund s Rule one electron goes in each orbital before two go in any Pauli s Exclusion Principle no two electrons can have the same exact set of 4 quantum numbers one goes up and the other goes down Electron Configurations 3 After Aufbau came the most modern way of assigning electrons. This way is done by using a number, letter and superscript number. For example 2 The first number is the same as n in quantum numbers. The letter is the conversion of l, when 0,1,2,3 equals s, p, d, f The last superscript number is the combination of m l and s. Page 1
2 4 The Periodic Table is a Map The periodic table is a map to the electron configurations. It is arranged by the AUFBAU principle. For example Let s Write the Electron Configuration for Arsenic by Using only the table 5 Electron Filling Order Writing Atomic Electron Configurations 6 Two ways of writing configs. One is called the spdf notation. spdf notation for H, atomic number = s no. of electrons value of n value of l Page 2
3 Electron Configurations and the Periodic Table 7 Figure Configuration of Arsenic Go from p 3 Writing Atomic Electron Configurations 9 Two ways of writing configs. Other is called the orbital box notation. ORBITAL BOX NOTATION for He, atomic number = 2 1 s 2 Arrows depict electron spin One electron has n = 1, l = 0, m l = 0, m s = + 1/2 Other electron has n = 1, l = 0, m l = 0, m s = - 1/2 Page 3
4 10 Another Way of Showing electron Configuration is through the use of arrows. The orbitals are shown as boxes (or blanks) The electrons are shown as arrows (up or down is one electron) When an orbital is complete, 2 opposite arrows are shown One must go in each before 2 in any(equal sublevel),and a sublevel must be complete before you go to the next. 11 Lithium 12 Group 1A Atomic number = > 3 total electrons Page 4
5 Boron 13 Group 3A Atomic number = > 5 total electrons Carbon 14 Group 4A Atomic number = > 6 total electrons Here we see for the first time HUND S RULE.. When placing electrons in a set of orbitals having the same energy, we place them singly as long as possible. Nitrogen 15 Group 5A Atomic number = > 7 total electrons Page 5
6 Neon 16 Group 8A Atomic number = > 10 total electrons Note that we have reached the end of the 2nd period, and the 2nd shell is full! Aluminum 17 Group 3A Atomic number = [Ne] 2 1 All Group 3A elements have [core] ns 2 np 1 configurations where n is the period number. Phosphorus 18 Group 5A Atomic number = [Ne] 2 3 All Group 5A elements have [core ] ns 2 np 3 configurations where n is the period number. Page 6
7 19 A Glitch? Write the noble gas configuration for 61 Pm. [Xe] 6s 2 5d 1 4f 4 Write the noble gas configuration for 74 W. [Xe] 6s 2 5d 4 4f 14 When the element ends in d add the one to the other d electrons When the element ends in in f show the d 1 electron. Ion Configurations 20 To form anions from elements add 1 or more e- to subshell of highest n [or highest (n + l)]. P [Ne] 2 3 P 3 - [Ne] e- ---> Ion Configurations 21 To form cations from elements remove 1 or more e- from subshell of highest n [or highest (n + l)]. Al [Ne] 2 1-3e- ---> Al 3+ [Ne] Page 7
8 Ion Configurations 22 For transition metals, remove ns electrons and then (n - 1) electrons. Fe [Ar] 2 6 loses 3 electrons ---> Fe 3+ [Ar] 5 Ion Configurations 23 For transition metals, remove ns electrons and then (n - 1) electrons. Fe [Ar] 2 6 loses 2 electrons ---> Fe +2 [Ar] 6 Fe Fe 2+ Ion Configurations 24 For transition metals, remove ns electrons and then (n - 1) electrons. Fe [Ar] 2 6 loses 2 electrons ---> Fe 2+ [Ar] 6 Fe Fe 2+ Fe 3+ Page 8
9 25 What about excited electrons? When an electron is excited, remember it jumps to a higher energy level. Na Na * excited may look like this Add the electrons up to get the atomic number- look for jumping electrons! Page 9
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