Chapter 8 Flashcards
Cation
An ion that has a positive charge
Formed when valence electrons are removed giving the ion a stable electron configuration
Chemical bond
The force that holds two atoms together
May form by attraction of positive ion and a negative ion
Anion
An ion that has a negative charge
Formed when valence electrons are added to the outer energy level
Ionic bond
The electrostatic force that holds oppositely charged particles together in an ionic compound
Electrolyte
An ionic compound whose aqueous solution conducts an electric current
Lattice energy
The energy required to separate one mole of the ions of an ionic compound which is directly related to the size of the ions bonded is also affected by the charge of the ions
Formula unit
The simplest ratio of ions represented in an ionic compound
Monatomic ion
An ion formed from only one atom
Oxidation number
The positive or negative charge monatomic ion
Polyatomic ion
An ion made up of two or more atoms bonded together that acts as a single unit with a net charge
Oxyanion
A polyatomic ion composed of an element usually a nonmetal bonded to one or more oxygen atoms
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 such as malleability
Conduction
Ductility
Delicalized electrons
The electrons involved in metallic bonding that are free to move easily from one atom to the next throughout the metal and are not attached to a particular atom
Metallic bond
The attraction of a metallic cation for delocalized electrons
Alloy
A mixture of elements that has metallic properties most commonly forms when the elements are either similar in size or the atoms of one element are much smaller than the atoms of the other
Crystal lattice
3d structure of an ionic compound with alternating positive and negative charges
Salt
Metal ion with a monatomic ion except oxygen
Octet rule
Atoms are most stable with 8 valence electrons
Nobel gases are special
Most stable configuration
End in S2 p6
Valence electrons
Outer most electrons
Metals want to
Lose electrons
Non metals want to
Gain electrons
Electron configuration changes how
Increases by one
Except transitions they have 2
Periodic table shows charge by
Valence electrons show the charge
