Lewis structures
Geometry
Metallic bonding
Intermolecular forces
Misc
200
The 2D diagram drawn, that shows us the presence of bonds, lone pairs, and free radicals.
What is the lewis structure?
200
Theory that was developed to help us model the different shapes we see in covalently bonded molecules.
What is VSEPR Theory
200
The three types of bonding.
What are ionic bonds, covalent bonds, and metallic bonds
200
The forces between ionic atoms.
What are electrostatic forces?
200
A molecule with an uneven distribution of electrical charge, resulting in distinct positive and negative regions.
What is a polar molecule?
400
Draw the lewis structure for SO2
400
The two types of electron domains
What are Bonding and non bonding; lone pair and bonds
400
The structure formed when metal atoms bond with other metal atoms
What is a Crystal lattice?
bonus: body centered and face centered
400
The two categories of intermolecular forces.
What are hydrogen bonding and van der waals forces.
400
A molecule with an even distribution of electrical charge, meaning it lacks positive or negative poles.
What is a non-polar molecule?
600
When multiple lewis structures represent the same compound due to multiple bonding options.
What is a resonance structure?
600
The two shapes we look at to determine the 3D structure of a molecule
What are electron domain geometry and the molecular geometry
600
The physical properties of metallic bonding
What are malleability, thermal conductivity, electrical conductivity, and luster?
600
The strongest intermolecular force, that must be between H-F, H-O, or H-N.
What is hydrogen bonding?
600
Why is hydrogen bonding the cause of ice having a lower density than water?
The partial charges are interacting and spread out, causing a crystal like lattice structure to form. This creates more space than in liquid water, resulting in ice less dense.
800
Draw the lewis structure for SF6
800
The electron domain geometry and the molecular geometry for H3P.
What is Tetrahedral and trigonal pyramidal?
800
When the metal atoms overlap their valence shells to share electrons, but because of empty d orbitals, electrons get shared among all the atoms
What is delocalization?
800
The three types of van der Waals forces in order from strongest to weakest.
What are keesom, debye, and london dispersion.
800
the forces between a molecule with a permanent dipole and a nonpolar molecule.
What are Debye forces?
1000
The bonding angle between atoms decreases in the presence of this.
What are lone pairs?
1000
The electron domain geometry and the molecular geometry for NHCl2.
What is tetrahedral and trigonal pyramidal?
1000
The reason metals are good conductors and the reason for the luster of metals
What are free electrons and empty d orbitals reflecting light?
1000
The force displayed when there are two molecules with permanent dipoles interacting.
What is a Keesom force?
1000
When the electrons surrounding an atom all end up on the same side of the atom as they move around their orbitals.
What is an instantaneous dipole?