Untitled Flashcards Set

Isoelectric- having the same number of electrons per atom ion or molecule 

Ionic bond- the electrostatic attraction between oppositely charged ions 

Covalent bond- a chemical bond in which atoms share the bonding electrons 

Bonding electron pair- an electron pair that is involved in bonding found in the space between 2 atoms 

Lewis-  structure a diagram that represents the arrangement of covalent electrons and bonds in a molecule or polyatomic ion

duet rule the observation that the complete outer shell of valence electrons when hydrogen and period 2 metals are involved in bonding

octet rule the observation that many atoms tend to form the most stable substances when they are surrounded by 8 electrons in their valence shells

lone electron pair a pair of valence electrons that is localized to a given atom but not involved in bonding

non-polar covalent bond a covalent bond in which the electrons are shared equally between atoms

polar covalent bond a covalent bond in which the electrons are not shared equally because 1 atom attracts them more strongly than the other atom

electronegativity the ability of an atom in a molecule to attract shared electrons to itself

dipole a separation of positive and negative charges in a region in space

polar molecule a molecule that has a net dipole

non-polar molecule a molecule that has only nonpolar bonds, or a bond dipole sum of zero

Valance electron theory- a theory stating that atomic orbitals overlap to form a new orbital with a pair of opposite spin electrons 

Hybrid orbital- an orbital that forms from the combination of at least two different orbitals 

Hybridization- the process of forming hybrid orbitals from the combination of at least two different orbitals 

Sigma- a bond that is formed when the lobes of 2 orbitas directly overlap end to end

Pi bond- a bond that is formed when the sides of the lobes of 2 orbitals overlap

intramolecular bond the chemical bond within a molecule

intermolecular force a force that causes one molecule to interact with another molecule; occurs between molecules

van der Waals forces many types of intermolecular forces, including dipole– dipole forces, London dispersion forces, and hydrogen bonding

dipole–dipole force the intermolecular force that is caused when the dipoles of polar molecules position their positive and negative ends near each other

hydrogen bond the strong dipole–dipole force that occurs when a hydrogen atom bonded to a highly electronegative atom (oxygen, nitrogen, or fluorine) is attracted to a partially negative  atom on a nearby molecule

London dispersion forces the intermolecular forces that exist in non- polar molecules; they increase as the molecular mass increases

polarizability the ability of a substance to form a dipolar charge distribution

surface tension the resistance of a liquid to increase its surface area

capillary action the spontaneous rising of a liquid in a narrow tube

viscosity the measure of a liquid’s resistance to flow

composite material a material composed of two or more distinct materials that remain separate from each other in the solid phase

metallic crystal a solid with closely packed atoms held together by electrostatic interactions and free-moving electrons

metallic bonding the bonding that holds the nuclei and electrons of metals together

molecular crystal a solid composed of individual molecules held together by intermolecular forces of attraction

covalent network crystal a solid in which the atoms form covalent bonds in an interwoven network

semiconductor a substance that conducts a slight electric current at room temperature but has increasing conductivity at higher temperatures