VSEPR Theory
3 bond pairs, no lone pairs.
What is trigonal planar
Lewis dot diagram for Silicon.
Teacher's discretion.
Bonding involves the interaction between the ______ of atoms.
What are valence electrons?
What is down and to the left?
Geometry of H2O.
What is bent?
Amount of valence electrons in CO2.
What is 16?
Explain the difference between ionic and covalent bonds.
What are ionic bonds: atoms exchanging valance electron(s) (one gains, the other loses, charge disparity bonds them together). Covalent bonds are the sharing of electrons between atoms to fill their octets (duets).
Explain why atomic radius has the trend it does.
What is going down the periods, the atoms gain electron shells, going right to left each group has less protons which means the attractive positive force of the nucleus becomes weaker and the electrons are not held as tightly to the nucleus?
Name every molecular geometry from 2 bond pairs to 6 bond pairs. No Lone pairs.
What is Linear, Trigonal Planar, Tetrahedral, Trigonal Bipyramidal, Octahedral?
Lewis structure NH3.
Teacher's discretion.
Explain how ionic bonds can involve more than 2 atoms.
What is valence electrons are distributed evenly.
Explain why the ionization energy trend is up and to the right?
What is the smaller an atomic radius, the harder it is to remove an electron due to the attractive force of the nucleus on the electrons getting greater as electrons are closer to the nucleus.
The bond angles in degrees for each geometric molecular structure, no lone pairs.
What is Linear = 180, Trigonal Planar = 120, Tetrahedral = 109.5, Trigonal Bipyramidal = 90 axial plane, 120 equatorial plane, Octahedral = 90 in both axial and equatorial plane.
The steps for drawing a lewis diagram.
What are 1. count all valence electrons. 2. determine central atom. 3. draw single bonds to the central atom. 4. put all remaining valence electrons on atoms as lone pairs. 5. turn lone pairs into double or triple bonds to give every atom an octet (or duet).
Explain △EN and where each bond type lies on the spectrum.
What is the difference between electronegativity of bonding atoms. What is >1.7 = ionic, 1.7 > polar covalent > 0.5, <0.5 pure covalent.
Explain why electron affinity is up and to the right?
What is when an electron is gained by an atom, energy is released. Atoms that are happy gaining an electron do not require additional energy from outside to keep that electron in their valence shell. Atoms that are unhappy when gaining an extra electron will require extra energy to ensure that electron stays in the valence shell. This net energy (in vs. out) is lower up and to the right, meaning atoms up and to the right like adding one electron more.
Explain why and how lone pairs affect molecular geometry.
What is Like charges repel. Lone pair electrons and bonding electrons are both negatively charged therefore, they want to be as far apart as possible from each other thus changing bond angles.
These criteria determine the central atom.
What are the atom that bonds the most, the atom that there is the least of and/or the most electronegative atom.
Explain why △EN influences whether covalent bonds are polar or pure.
What is higher EN atoms will hold the electron density of the bond closer to them creating a dipole effect. Atoms with lower △EN will not have this dipole effect which will not affect electron density as much.
Explain the difference between electron affinity versus electronegativity.
What is the change in energy when an electron is added to a neutral atom from another atom versus how much an atom can attract electrons in a chemical bond.