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chemical bond
mutual electrical attraction between the nuclei and valence electrons of different atoms that binds the atoms together.
Ionic bonding
chemical bonding that results from the electrical attraction between cations and anions
covalent bonding
the sharing of electron pairs between two atoms
Nonpolar-covalent bond
covalent bond in which the bonding electrons are shared evenly by the bonded atoms, resulting in a balanced distribution of electrical charge
Polar bond
a bond with an uneven distribution of charge.
Polar-covalent bond
covalent bond in which the bonded atoms have an unequal attraction for the shared elections.
Molecule
a neutral group of atoms held together by covalent bonds
Molecular compound
a chemical compound whose Simplest units are molecules
Chemical formula
indicates the relative numbers of atoms of each Kind in a chemical compound by using atomic Symbols and numerical Scripts.
molecular formulas
shows the types and numbers of atoms combined in a single molecule of a molecular compound.
Bond energy
energy required to break a chemical bond and for neutral isolated atoms
Electron-dot notation
electron configuration notation in which only the valence electrons of an atom of a particular element are shown, indicated by dots placed around the elements.
Lewis structure
formulas in which atomic symbols represent nuclei and inner-shell electrons, dot-pairs, or dashes between two atomic symbols represent electron pairs in covalent bonds, and dots adjacent to only one atomic symbol represent unshared electrons
structural formula
indicates the Kind, number, arrangement, and bonds but not the unshared atoms in a molecule
single bond
covalent bond in which one pair of electrons is shared between two atoms.
Multiple bonds
multiple covalent bonds.
Resonance
bonding in molecules or ions that cannot be correctly represented by a single lewis structure
Ionic compound
composed of positive and negative ions that are combined so that the numbers of + and - charges are equal
Formula unit
simplest collection of atoms from which an ionic Compounds formula can be written.
Lattice energy
energy released when one more of an ionic crystalline compound is formed from gaseous ions
metallic bonding
the chemical bonding that results from the attraction between metal atoms and the surrounding sea of electrons
Polyatomic ion
a charged group of covalently bonded atoms
Malleability
the ability of a substance to be hammered or beaten into thin sheets.
Ductility
the abilitt of a substance to be drawn, pulled, or extruded through a Small opening to produce a wire.
VSEPR theory
repulsion between the sets of valence-level electrons Surrounding an atom causes these sets to be oriented as far apart as possible.
hybridization
mixing of two or more atomic orbitals of similar energies On the same atom to produce new hybrid atomic orbitals of equal energies.
Hybrid orbitals
orbials of equal energy produced by the combination of to or more orbitals on the same atom.
dipole
created by equal but opposite charges that are separated by a short distance.
Hydrogen bonding
inter molecular force in which a hydrogen atom that is bonded to a highly electronegative atom is attracted to an unshared pair of elections of an electronegative atom in a nearby molecule.
London dispersion forces
intermolecular attractions resulting from the constant motion of electrons und the creation of instantaneous dipoles.
The 7 diatoms found in nature
Hydrogen, Nitrogen, Oxygen, Fluorine, Chlorine, Bromine, and Iodine
most electronegative element
Fluorine (F)
bonds
the shorter bonds are stronger and have higher bonding energy
potential energy
stored energy that results from the position or shape of an object
Far potential energy
high potential energy
because unstable
Close potential energy
minimum potential energy
bc atom is stable
