Download Unit 4 Review - Davis

Unit 4 Review
History of the Periodic Table
Johann Wolfgang Döbereiner
Dmitri Mendeleev
John Newlands
Henry Moseley
Definitions
Periodic Table
Group or Family – vertical column
Alkali Metals – most active metals; stored under oil.
Halogens – most active nonmetals
Noble Gases – relative inactive (inert)
Period or Series – horizontal rows
Row number = number of energy levels
Shielding Effect Nuclear charge – refers to the number of protons
Metal Activity – how easily metals lose electrons to react and form
positive ions
Nonmetal Activity – how easily nonmetals gain electrons to react and
form negative ions
Electronegativity – attraction that one atom for the outer shell
electron of another atom
Ionization Energy – the energy needed to remove the outermost
electron in an atom
The atomic radius is a measure of the size of an atom.
Modern Periodic Law – The properties of the elements are a periodic
function of their atomic numbers. The statement that the physical and
chemical properties of the elements repeat in a regular pattern when
they are arranged in order of increasing atomic number is known as
the periodic law.
Octet Rule – Atoms form bonds to achieve a noble gas configuration
(8 electrons). A filled energy level is a more stable arrangement.
Ions- charged particles, cations (+), anions (-)
Oxidation number
Representative Elements ,Transition and Inner-transition Metals
Because elements in the same group have the same number of valence
electrons, they have similar properties.
Characteristics of Metal, Nonmetals, Metalloids including states
Periodic Trends