1/29
Looks like no tags are added yet.
Name | Mastery | Learn | Test | Matching | Spaced |
|---|
No study sessions yet.
Ionic bonding
attraction between the opposite charges of a cation and an anion, complete transfer of electrons
Lattice energy
the energy required to completely separate a mole of a solid ionic compound into its gaseous ions
Coulomb’s Law
force between to particles based on their charge and size
F= k(Q1Q2/r2)
Covalent bond
bond in which two electrons are shared by two atoms
Bond enthalpy
change in enthalpy required to break a bond
Covalent compounds
relatively weak intermolecular forces, liquid, gases, low melting solids
Ionic compounds
stronger forces, solids with high melting points
Non-polar covalent bonds
electrons shared equally
Polar covalent bonds
electrons not shared equally, one atom pulls more
Electronegativity (EN)
the ability of an atom to attract electrons to itself (determines whether something is polar or non-polar)
Bond polarity
small EN difference = non-polar covalent
mid EN difference = polar covalent
Naming binary molecules
2 non-metal elements in the formula, 2nd element gets “ide” ending, greek prefixes indicate number of atoms
Naming acids
anions ending in “ide” get hydro prefix, “ic” ending and add “acid” to name
anions ending in “ate” get “ic”, ending in “ite” get “ous” ending
Naming hydrates
greek prefixes to indicated number of water molecules
Octet rule
atoms, other than hydrogen, tend to form bonds until surrounded by 8 electrons (have a full octet)
Formal charge
a way of keeping count of electrons, the charges may or may not be real; the electrical charge difference between valence electrons and the number of electrons assigned to each atom
Resonance
a better representation of the model of an atom, must be valid lewis structures (occur when you have more than one option of a location to take electrons from)
Equivalent resonance structures
same formal charge, same number of bond types; low energy (MAJOR) structures contribute more than high energy
molecular geometry
ignores the lone pairs when naming the structure
VSEPR
valence shell electron pair repulsion
Electron domain
region most likely to find electrons in
Electron geometry
arrangement of electron domains around a central atom
non-bonding pairs + repulsion
have greater repulsive forces causes the angles to compress
multiple bonds + repulsion
exert a great repulsive force on adjacent domains causing the angle to compress
Diatomic non-polar molecules
same element (H2, O2)
Diatomic polar molecules
different elements (HCL, CO, NO)
Polyatomic molecules and polarity
molecular geometry determines if there is a dipole and therefore whether it is polar or non-polar (no net dipole = non-polar, dipole moment = polar)
Isomer
same formula, different arrangement of atoms
London dispersion forces
proportional to the number of electrons in the atom
How to tell if a molecule is polar or non-polar based on the geometry?
polar= overall dipole
non-polar= dipoles cancel out