CHEM-C 101 1st EditionExam # 2 StudyGuide (Chapters 4, 5, 6)List of Concepts and Terms to UnderstandChapter 4:-E=hcλ= hν-ν =cλ- E = energy (Joules); c = speed of light (m/s); h=Plank’s constant (J·s); λ = wavelength (needs to be converted to meters to cancel with speed of light); ν= frequency (s-1)- Be able to calculate energy or frequency at a given wavelength or determine wavelength or frequency given energy. (If given energy in eV you need to convert to J)- Electronic Configurations: way electrons are arranged in shells and sub-shells (be able to determine elements based on their electronic configurations or write the electronic configuration given an element)- Predict chemical formulas of molecules formed in a reaction (ie: Mg and Cl  MgCl2)- Understand principal quantum number (n)  n= number of sub-shells- Be able to determine that maximum number of electrons based on quantum number (ie: n = 3 has 18 max electrons due to an s, p, and d orbital - 3s3p3d)- Tell how many valence electrons an element has using the periodic table- Ground State vs. Excited State- Know the s, p, d, and f orbital blocks on the periodic table and the maximum amount of electrons each can hold- Metals prefer to lose valence electrons; Non-metals prefer to gain valence electrons- Atomic Radius Trend – which directions does it increase on the periodic table- Octet Rule – 8 electrons to have a valence shell configuration like a noble gas  stableChapter 5:- Ionic bonding = metal + non-metal - Oppositely charged ions  electrostatic force (Coulombic attraction)- Ionic Lattice (crystalline vs. amorphous)- Lattice Energy - Molecule – collection of atoms bound together- Covalent Bond = non-metal + non-metal/metalloid (attraction from valence electrons being SHARED between two nuclei)- Bond formation releases energy; Bond breaking takes energy- Understand how to draw Lewis Dot Diagrams and determine how many electron pairs there are (bonded or lone pairs)  bonded are shared between two atoms, lone pairs belong to a single atom- Multiple Covalent Bonds  determine when a double or triple bond should be present- Resonance – dot diagrams that differ only by arrangement of electrons- Polyatomic ions – ions from many atoms (ie: NO3-, NH4+, PO43-)- Electronegativity – atom’s ability to attract the shared electrons to itself (understand the periodictable trend; which directions does it increase)- Nomenclature – naming of compoundBinary Compound – made of two elementsUnderstand how to name binary ionic (normal and systematically), binary covalent, polyatomic ion names, and acids- Exceptions to the Octet Rule : Octet Deficient (ie: B or Be) and Expanded Octet (ie: P, S, I)Note: Not all exceptions are listed here, there are more exceptionsChapter 6:- Shape of Molecules based on VSEPR theory (valence electrons repel one another)- Understand what the importance of using wedges and dashed lines in shape drawings- Steric # = # electron groups = # atoms attached + # lone pairs (multiple bonds count as one electron group)- Determine Shape: (Step-wise)1. Lewis Dot Diagram2. Count Steric #3. Use steric # to determine arrangement4. Pretend lone pairs are invisible to determine shape- Polarity – Intermolecular forces (know how to determine if a molecule is polar or non-polar)- Dipoles of bonds and Molecular dipole moments- Be able to determine if a molecule has polarity overall- Know VSEPR Shape ideas for Steric # 2-6  linear, trigonal planar, tetrahedral, trigonal bipyramidal, and octahedral (also know all possible shapes that can be made by the presence of lone pairs in these arrangements; cheat sheet from class)Look at the “Skills to Know” section at the end of each chapter to reviewNOTE: PART OF CHAPTER 7 MAY OR MAY NOT BE ADDED, PROF. EDWARDS WILL LET YOU