Komperda. Electron Configuration and Orbital Notation
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1 Electron Configuration and Orbital Notation
2 Dmitri Mendeleyev Father of the Modern P.T.
3 Periods and Group Period horizontal row on P.T. Each period represents an energy level (think back to models of the atom) Atoms in period 1 have 1 energy level, atoms in period 5 have 5 energy levels Group vertical column P.T. Also known as families
4 Where are the electrons? -The Bohr Atom Komperda Bohr Model Based on Line Emission Spectrum of Hydrogen Atoms consists of nucleus and energy Levels Stated electrons followed specific circular paths called orbits
5 Quantum Mechanical Model Consists of Energy levels, sublevels, and orbitals Key Points: 1. Electrons do not follow orbits, nor can location be known exactly 2. Electrons are located within orbitals (probable location of electron)
6 Sublevel (also called subshell) Found within energy levels Designated by s, p, d, or f Letter corresponds to orbital shapes found in sublevel s sublevel (1 orbital)
7 The p sublevels (three orbitals) Komperda The d sublevel (five orbitals)
8 The f sublevel (7 orbitals) Komperda
9 Relative size of the 1s, 2s, 3s orbitals Komperda
10
11 Orbitals Generalized location of electron You know I m probably in this room all day, you just don t know if I m at my desk or in the storeroom or walking around Does not have sharp edges 1 orbital can contain a maximum of 2 electrons
12 Electron Configuration Electron configuration: description of what sublevels and orbitals are filled by electrons in any given atom (like a roadmap of the electrons in an atom) Determined by the number of electrons the atom has Governed by 3 rules!
13 e- configuration rules Aufbau Principle: an electron occupies the lowest energy level & orbital available Pauli Exclusion Principle: only two electrons can occupy any orbital, and they must have opposite spins Hund s Rule: Each orbital in a given sublevel (s, p, d, or f orbital) must have 1 electron before any can have two
14 Electron Configurations 14 how many electrons in that orbital Nitrogen: 1s 2 2s 2 2p 3 energy level orbital (atomic number = 7) Tro's Introductory Chemistry, Chapter 9
15 Outline the sections on your blank periodic table to match this diagram. Use different colors for each sublevel.
16 Orbital Notation - Pictures Using the periodic table from the previous slide, we can also create picture representations of the electron configuration (called orbital notation) We use arrows ( ) to represent the electrons Remember those three rules: Fill lowest energy levels first Any subshell with multiple orbitals must get one arrow in each orbital first (in the same direction) before doubling up Two arrows in each orbital (one up, one down)
17 Orbital Notation ctd Each s subshell only has 1 orbital (holding 2 arrows) Each p subshell has 3 orbitals (holding 2 arrows each = 6) Each d subshell has 5 orbitals (holding 2 arrows each = 10) The orbitals are represented by boxes or just lines 1s 2s 2p 3s 3p
18 Orbital Notation Example Write the orbital notation for Oxygen How many electrons (arrows) does neutral oxygen have? 8 _ _ 1s 2s 2p
19 Shorthand Noble Gas Notation Group 18 on the periodic table are called the Noble Gases --- To create a shorthand for electron configuration, we use the noble gases as a reference For example, the electron configuration of silicon is: 1s 2 2s 2 2p 6 3s 2 3p 2 to write the shorthand, we find which Noble gas comes before silicon --- Neon (Ne) Neon s electron configuration is: 1s 2 2s 2 2p 6 The noble gas notation for silicon then would be: [Ne]3s 2 3p 2
20 Noble Gas Notation Practice Write the noble gas notation for manganese First, find which noble gas comes before manganese--- Ar Full electron configuration: Argon Noble Gas Notation: 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 5 [Ar]4s 2 3d 5
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