Studied by 3 peopleIodine heptafloride
________ (IF7) can be written so that sulfur has twelve valence electrons.
Vander Waals
________ Forces: attractions between the molecules that are the two weakest attractions between molecules.
VSEPR
According to the ________ theory, the repulsion between electron pairs causes molecular shapes to adjust so that the valence- electron pairs stay as far apart as possible.
Covalent Bond
________: joins two atoms together that are sharing a pair of electrons.
Nitrogen dioxide
________ (NO2) has an odd number of valence electrons and therefore does not satisfy the octet rule.
temperature
They have low in ________ melting points and boiling points.
Nonpolar
________ and caused by temporary asymmetrical dispersion of electrons around it.
Octet Rule
The ________: electron sharing usually occurs so that the atoms attain the electron configurations of noble gases (each having eight valence electrons)
Polar covalent bond
________: the electrons are shared unequally.
Formula Unit
________: the base of an ionic compound NaCl is an ionic compound so the ________ are Na and Cl.
Atoms
________ form double or triple covalent bonds if they can attain a noble gas structure by sharing two pairs or three pairs of electrons.
Phosphorus pentachloride
________ (PCl5) can be written so that phosphorus has ten valence electrons.
Dipole Dipole interactions
________: when polar molecules are attracted to each other.
Boron Trifluoride
________ (BF3) can be written so that boron only has 6 valence electrons.
Dipole
________: in a polar molecule, one end of the molecule is slightly negative and the other slightly more positive.
Molecule
________: a neutral group of atoms joined together by covalent bonds.
Intermolecular forces
________ (IMF): weaker than either ionic or covalent bonds but are responsible for determining the state of matter a molecular compound is at a given temperature and a molecules melting point and boiling point.
Hybridization
________: several atomic orbitals mix to form the same total number of equivalent hybrid orbitals because their bond lengths are identical and their bond energies are identical.
London Dispersion
________ forces: the weakest of all molecular interactions.
Nonpolar covalent bond
________: when the bonding electrons are shared equally.
Metallic bonds
________: metal + metal, structured by delocalized electrons.
Sulfur hexafluoride
________ (SF6) can be written so that sulfur has twelve valence electrons.
Hydrogen bonds
________: when a hydrogen atom bonds to a very electronegative atom (Nitrogen, Oxygen, or Fluorine)
Network solids
________ (or network crystals: solids in which all of the atoms are covalently bonded to each other.
octet rule
The ________ can not be satisfied in molecules whose total number of valence electrons is an odd number.
ionic bonds
metals + nonmetals
Metallic bonds
metal + metal, structured by delocalized electrons
Covalent (molecular) bonds
nonmetal + nonmetals
Molecule
a neutral group of atoms joined together by covalent bonds
Diatomic Molecule
a molecule consisting of two atoms
Molecular Compound
a compound composed of molecules
Formula Unit
the base of an ionic compound NaCl is an ionic compound so the formula units are Na and Cl
Molecule
base unit of a molecular compound
Molecular Formula
a chemical formula of a molecular compound that shows how many atoms of each element a molecule contains
The Octet Rule
electron sharing usually occurs so that the atoms attain the electron configurations of noble gases (each having eight valence electrons)
Covalent Bond
joins two atoms together that are sharing a pair of electrons
Lone Pair
a pair of valence electrons that is not shared between atoms
Double covalent bond
a bond that involves two shared pairs of electrons
Triple covalent bond
a bond formed by sharing three pairs of electrons
Coordinate Covalent bond
a covalent bond in which one atom contributes both bonding electrons
Bond dissociation energy
The energy required to break the bond between two covalently bonded atoms
Nonpolar covalent bond
when the bonding electrons are shared equally
Polar covalent bond
the electrons are shared unequally
Dipole
in a polar molecule, one end of the molecule is slightly negative and the other slightly more positive
molecular orbitals
orbitals that apply to the entire molecule when two atoms combine and their orbitals overlap
Bonding orbital
a molecular orbital that can be occupied by two electrons of a covalent bond
Sigma bonds
formed when two atomic orbitals combine to form a molecular orbital that is symmetrical around the axis and connects two atomic nuclei
Pi bonds
the second bond area formed in a double bond
hybridization
several atomic orbitals mix to form the same total number of equivalent hybrid orbitals because their bond lengths are identical and their bond energies are identical
inter
between
Intra
within
Intermolecular forces (IMF)
weaker than either ionic or covalent bonds but are responsible for determining the state of matter a molecular compound is at a given temperature and a molecules melting point and boiling point
Vander Waals Forces
attractions between the molecules that are the two weakest attractions between molecules
Dipole/Dipole interactions
when polar molecules are attracted to each other
London Dispersion forces
the weakest of all molecular interactions
Hydrogen bonds
when a hydrogen atom bonds to a very electronegative atom (Nitrogen, Oxygen, or Fluorine)
network solids (or network crystals
solids in which all of the atoms are covalently bonded to each other
Note
Flashcard