Unit 1.3 Review Sheet

Vocabulary flashcards covering scientists, principles, periodic trends, element classifications, and electron configurations from the Unit 1.3 Review Sheet.

Dalton

Scientist credited with foundational atomic theory concepts reviewed in Unit 1.3.

Thomson

Scientist credited with key discoveries and concepts in atomic structure reviewed in Unit 1.3.

Rutherford

Scientist credited with foundational concepts regarding atomic structure in Unit 1.3.

Bohr

Scientist credited with key concepts regarding atomic structure and electron orbits in Unit 1.3.

Schrodinger

Scientist credited with key quantum mechanical model concepts of the atom in Unit 1.3.

Mendeleev

Scientist credited with foundational concepts regarding the organization of the periodic table.

Aufbau principle

A fundamental principle required for determining and writing electron configurations of elements.

Hund’s Rule

A principle applied when filling orbitals to determine electron arrangement and the number of unpaired electrons.

Pauli Exclusion Principle

A core principle governing electron occupancy within orbitals when writing electron configurations.

Alkali metals

A specific group of elements located on the periodic table whose placement must be known.

Alkaline earth metals

A group of elements located on the periodic table whose placement is reviewed in Unit 1.3.

Transition metals

A specific category and block of metallic elements on the periodic table.

Halogens

A group of nonmetal elements whose position on the periodic table is tested in Unit 1.3.

Noble gases

A group of elements on the periodic table used as shorthand reference points when writing noble gas configurations.

Metals

A major classification of elements situated on the periodic table.

Nonmetals

A classification of elements located on the periodic table, distinct from metals and metalloids.

Metalloids

Elements situated between metals and nonmetals on the periodic table.

Atomic radii

A periodic trend evaluated in Unit 1.3 to compare atom sizes, such as between C and Sn or Mg and P.

Ionization energy

A periodic trend analyzed in Unit 1.3 to compare elements such as F vs I or Li vs O.

Electronegativity

A periodic trend analyzed in Unit 1.3 to compare elements such as Na vs Rb or K vs Br.

Noble gas configuration

An abbreviated form of writing electron configurations using the symbol of the preceding noble gas.

Unpaired electrons

Electrons occupying an orbital alone, which must be determined for elements like Sodium, Chlorine, Krypton, and Nickel.