Day 1 skills review

DAY 1, Terms to know:

Sections 1.1-1.8 Isomers, valence electrons, octet rule, lone pair, ion, formal charge, subshell, orbital, electronegativity, polarity, node, wavefunction sign, wavesign, electron configuration, orbital diagram, atomic orbital, molecular orbital, bonding, antibonding

DAY 1, Specific outcomes and skills that may be tested on exam 1:

Sections 1.1-1.8

• Be able to predict the number of bonds each relevant atom typically has.
• Be able to explain how the energy changes as covalent bonds get stretch or compressed and WHY and why there is an optimal length for each covalent bond between atoms.
• Be able to determine the number of protons, neutron, and electrons in an atom, and how many electrons are valence electrons.
• Be able to draw Lewis structures for molecules including molecules with heteroatoms and with single, double, and/or triple bonds with the most reasonable location for all bonding pairs of electrons and all lone pairs.
• Be able to calculate formal charge for any atom given how many bonds and how many lone pairs it has. Given an atom with a formal charge shown, know how to determine how many bonding and lone pair electrons are around it.
• Be able to count electrons around an atom to determine whether an atom has a complete octet and also count electrons around an atom to determine the formal charge of an atom.
• Be able to explain the difference between an energy level, subshell, and orbital.
• Be able to determine the relative electronegativity of atoms based on periodic trends.
• Be able to determine the relative polarity of individual bonds.
• Be able to explain how the shapes of the orbitals vary for s and p orbitals.
• Be able to describe how electrons have wave properties and how the wavesign squared gives the shapes of the orbitals and location of greatest electron density.
• Be able to explain how the wavesign is different from the charge.
• Be able to identify and/or describe where the nodes are for the orbitals in the first and second energy levels as well as the 3s.
• Be able to write electron configurations and orbital diagrams
• Be able to describe how both constructive and destructive interference work for wavefunctions and how they yield bonds and antibonds with specific shapes including both pi and sigma bonds.
• Be able to explain how atomic orbitals overlap and that the number of molecular orbitals that result is equal to the number of atomic orbitals overlapping.
• Be able to explain how electrons are more stable in the bonding MO than in the antibonding and two reasons why that relate to electronic repulsions and attractions.
• Be able to explain how each bonding MO is lower in energy than the nonbonding by the same quantity that anitbonding MO is greater in energy than nonbonding.
• Be able to draw the bonding and antibonding energies for small molecules involving two atoms bonding and how having electrons in the bonding and antibonding orbitals relates to the octet rule and how entropy plays into the likelihood of bonds forming.
• Be able to explain that molecular orbitals may have many nodes and assymetrical shapes, but 1 orbital can still only hold a maximum of 2 electrons.

Complete these problems outside of class until you are confident you have learned the SKILLS in this section outlined on the study guide and we will review some of them next class period. 1.5  1.9  1.10  1.12  1.13  1.14  1.15  1.16  1.17  1.18  1.37  1.40  1.42  1.45  1.47