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Chemistry Unit 6
Question | Answer |
---|---|
ionic starts with a | metal |
molecular starts with a | nonmetal |
Ionic has ______ melting points and boiling points | high |
molecular has _______ melting points and boiling points | Generally low |
Molecular compounds can be a ______ | solid, liquid, or gas |
Ionic compounds are ______ | Crystalline solids |
Molecular compound smallest particle known as | molecule |
Ionic compound smallest particle known as | formula unit |
Single Covalent bond | when one pair of electrons is shared between two atoms |
Double Covalent bond | when two pairs of electrons are shared between two atoms |
Triple Covalent bond | when 3 pairs of electrons are shared between 2 atoms |
Magnificent 7 | molecules that have two of the same atoms covalently bonded together |
What is in the Magnificent 7 | N2, O2, F2, Cl2, Br2, I2, H2 |
Coordinate Covalent Bonds | when one of the bonding atoms contribute both electrons in the electron pair |
Polyatomic ions | A covalently bonded group of atoms that has an overall positive or negative charge |
Resonance | when two or more equally valid electron structures can be written for a molecule |
Bond dissociation energy (single bond) | farthest apart, lowest energy needed to break it |
Bond dissociation energy (double bond) | closer together than a single bond, medium energy to break |
Bond dissociation energy (triple bond) | closest together, most energy to break |
sigma bond | single bond |
180 degrees | linear |
120 degrees | Trigonal Planar |
109 degrees | Tetrahedral |
107 degrees | Pyramidal |
105 degrees | Bent |
is polar unequal or equal sharing | unequal sharing |
is nonpolar unequal or equal sharing | equal sharing |
what are the two conditions for a molecule to be polar | one or more bonds within the molecule must be polar the molecule must be asymmetrical |
Intermolecular attractions | attractions between one molecule and a neighboring molecule |
Intramolecular attractions | attractions which hold an individual molecule together (ex. covalent bonds) |
London dispertion forces | non-polar molecules caused by motion of electrons |
Dipole-Dipole | polar molecules dipole-dipole attraction |
Hydrogen Bonding | only H-O, H-F, or H-N bonds |
Network Solids | molecular substances very strong/ very high or no melting point |
IMF means | intermolecular forces (between neighboring particles) |
Intramolecular forces | inside bond |
sigma shape(s) | spheres or dumbells overlapping |
pi shape(s) | dumbell overlapping |
unshared pair of electrons | pairs not in a bond |
shared pair of electrons | in a bond |
lone pair of electrons | unshared pair |
unpaired electron | eletron waiting to be bonded |
VESPR | valence shell electron pair repulsion |
VSEPR theory | because of electron repulsion, valence electron pairs move as far apart as possible. This affects the shape of the molecule |