The Periodic Table

metals

• lose electrons

• solids (except Hg)

• high melting and boiling points

• good conductors

• malleable

• ductile

• lustrous

non-metals

• gain electrons

• solids

• liquids

• gases

• low melting and boiling points

• insulator (except graphite)

• non-malleable

• non-lustrous

Newland

noticed when elements were arranged by increasing mass, their properties repeated every 8th element

Meyer and Mendelev

demonstrated connection between atomic mass and elemental properties

Moseley

sorted the periodic table by increasing atomic number

periodic law

periodic repition of chemical and physical properties of the lements when they are arranged by increasing atomic number

groups

columns of elements

periods

rows of elements

representative elements

elements in groups 1, 2, and 13-18 of the periodic table that display a wide range of properties and include metals, nonmetals, and metalloids

transition metals

elements in groups 3-12

alkali metals

group 1 (except H), highly reactive

alkaline earth metals

group 2, highly reactive

transition metals

elements that have partially filled d orbitals, known for their ability to form various oxidation states and colored compounds.

inner transition metals

elements found in the f block of the periodic table, including lanthanides and actinides, known for their rare earth properties and radioactivity.

lanthanide series

inner transition metals 57-71

actinide series

inner transition metals 89-103

halogens

group 17, highly reactive elements, non-metals

noble gases

group 18, extremely unreactive elements, non-metals

metalloids

physical and chemical properties of metals and non-metals

ion

any atom or group of atoms that bears one or more positive or negative electrical charges

cations

positively charged ions

anions

negatively charged ions

atomic radius

half the distance between nuclei of identical atoms (decreases across the period) (increases down a group)

ionization energy

the energy required to remove an electron from a gaseous atom; because there is more attraction to the nucleus, more energy must be used to break it (increases across a period) (decreases down a group)

first ionization energy

the energy required for the first electron to be removed; increases for more electrons

octet rule

atoms tend to gain, lose, or share electrons in order to acquire a full set of 8 valence electrons, which is useful for predicting what types of ions an element is likely to form

electronegativity

the relative ability to attract electrons in a chemical bond (increases across a period) (decreases down a group)