Unit 2 Study Guide
Unit 2 Study Guide CHMY 121IN-001
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This 2 page Study Guide was uploaded by Ashlyn Fortner on Thursday October 1, 2015. The Study Guide belongs to CHMY 121IN-001 at Montana State University taught by Goodman, Candace Kay in Fall 2015. Since its upload, it has received 101 views. For similar materials see Intro to General Chemistry in Chemistry and Biochemistry at Montana State University.
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Date Created: 10/01/15
9 9 9 9 9 9 9 9 9 9 9 9 99 9 99 9 9 99 9 99 Unit g Study Guide Maximum Electron Capacity gt N15 Electron shells Energy of shells How Bohr s model can predict hydrogen spectra How energy is released during relaxation Failures of Bohr s model Subshells of each shell gt S p d f Electron con guration gt 1s2 Noble gas notation gt Short hand notation Heisenberg uncertainty principle Shape of orbitals gt S p d f Hund s rule to occupy orbitals Why atoms stick together gt Properties of noble gases are important to this Octet Rule to compound formation gt Elements combine so they have 8 valence electrons in each shell What holds atoms together gt Chemical bonds I Strongest type of reaction between atoms How do nonmetal bonds form gt Diatomic molecules Chemical bonding gt Covalent I Formed by shared electrons gt Ionic Naming gt Covalent compounds I Use pre xes for numbers I First element never used with mono gt Ionic compounds I Name of rst element with the second element ending in ide 4 steps to determine how to draw a Lewis dot structure gt Count number of valence electrons I Sum of group numbers gt Connect the atoms I Central atom is typically listed rst gt Fill in remaining valence electrons I Outer atoms rst gt If atoms don t have full octet I Trade pair of electrons for a bond between atoms Determine the molecular shape gt Based on electron groups around the central atom 3D Shape VSEPR Theory gt Valence Shell Electron Pair Repulsion I Electrons are negative I Will repel each other I Shape of molecule will be where electron pairs are as far 9 69 O 69 away from each other as possible 00 To determine structure gt Draw a valid Lewis dot structure gt Count electron groups around central atoms gt Determine electron group geometry gt Determine nal molecular geometry by ignoring lone pairs left over
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