Studied by 1 personchemical bonds
the attractive forces that hold atoms together
ionic bond
A chemical bond resulting from the attraction between oppositely charged ions.
covalent bond
A chemical bond that involves sharing a pair of electrons between atoms in a molecule
metallic bond
a bond formed by the attraction between positively charged metal ions and the electrons around them
Lewis symbol
the representation of an atom that shows valence electrons as dots around the symbol of the element
octet rule
States that atoms lose, gain or share electrons in order to acquire a full set of eight valence electrons
lattice energy
the energy released when one mole of an ionic crystalline compound is formed from gaseous ions
single bond
a covalent bond in which two atoms share one pair of electrons
double bond
A covalent bond in which two pairs of electrons are shared between two atoms
triple bond
a covalent bond in which two atoms share three pairs of electrons
bond length
the average distance between the nuclei of two bonded atoms
bond polarity
a measure of how equally or unequally the electrons in any covalent bond are shared
polar covalent bond
A covalent bond in which electrons are not shared equally
nonpolar covalent bond
a covalent bond in which the electrons are shared equally by the two atoms
Electronegativity
A measure of the ability of an atom in a chemical compound to attract electrons
polar molecule
A molecule that has electrically charged areas.
Dipole
created by equal but opposite charges that are separated by a short distance
formal charge
The number of valence electrons in an isolated atom minus the number of electrons assigned to the atom in the Lewis structure
resonance structure
one of the two or more equally valid electron dot structures of a molecule or polyatomic ion
bond angle
the angle formed by two bonds to the same atom
VSEPR theory
Valence-shell electron-pair repulsion theory; because electron pairs repel, molecules adjust their shapes so that valence electron pairs are as far apart as possible
electron domain
in the VSEPR model, a region about a central atom in which an electron pair is concentrated
bonding pair
an electron pair found in the space between two atoms
nonbonding pairs
two paired valence electrons that tend not to participate in a chemical bond
bond dipole
separation of electrical charge created when atoms with different electronegativities form a covalent bond
hybrid orbitals
orbitals of equal energy produced by the combination of two or more orbitals on the same atom
Hybridization
the mixing of several atomic orbitals to form the same total number of equivalent hybrid orbitals
sp hybridization
linear; bond angle: 180
a type of bonding where the 2s orbital mixes with only one of the three p-orbitals resulting in two sp orbitals and two remaining unchanged p orbitals
sp2 hybridization
Trigonal planar structure
sp2 hybridization creates 3 identical orbitals of intermediate energy and length and leaves one unhybridized p orbital
3 effective pairs of electrons surround the carbon (double bond treated
as one effective pair)
sp3 hybridization
A type of hybridization that results from the combination of the s orbital and all three p orbitals in the second energy level of carbon, resulting in four hybrid orbitals and occurs when a carbon atom is bonded to four other atoms. The geometric arrangement of those four hybrid orbitals is called tetrahedral.
sigma bond
a bond formed when two atomic orbitals combine to form a molecular orbital that is symmetrical around the axis connecting the two atomic nuclei
pi bond
a bond that is formed when parallel orbitals overlap to share electrons.
metallic solids
solids that have metal atoms occupying the crystal lattice and held together by metallic bonding
ionic solids
solids whose composite units are ions; they generally have high melting points
covalent network solids
solids in which the units that make up the three-dimensional network are joined by covalent bonds
molecular solids
solids whose composite units are molecules
crystalline solid
A solid that is made up of crystals in which particles are arranged in a regular, repeating pattern
amorphous solid
A solid made up of particles that are not arranged in a regular pattern
Alloys
a mixture composed of two or more elements, at least one of which is a metal
substitutional alloy
some of the host metal atoms are replaced by other metal atoms of similar sizes
interstitial alloy
a mixture formed when small atoms fill holes in a metallic crystal
electron sea model
Proposes that all metal atoms in a metallic solid contribute their valence electrons to form a "sea" of electrons, and can explain properties of metallic solids such as malleability, conduction, and ductility.
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