Chemistry 1: Periodicity and the Development of the Periodic Table

Vocabulary-style flashcards covering the historical development of the periodic table, key scientists, structural components, and major periodic trends.

Fire (Alchemical Symbol)

Represented by an upward-pointing triangle to signify rising heat.

Air (Alchemical Symbol)

Represented by an upward-pointing triangle with a horizontal line to signify blockage.

Water (Alchemical Symbol)

Represented by a downward-pointing triangle to signify falling rain.

Earth (Alchemical Symbol)

Represented by a downward-pointing triangle with a horizontal line to signify weight.

Lavoisier

The scientist credited with creating the first list of known elements.

Döbereiner

The scientist who organized elements into Triads.

de Chancourtois

The scientist who proposed the Telluric Screw.

Newlands

The scientist who formulated the Law of Octaves.

Lothar Meyer

A scientist who demonstrated periodic relationships among elements.

Dmitri Mendeleev

The Father of the Periodic Table ($1869$) who organized elements by atomic mass and predicted properties of missing elements like Gallium, Germanium, and Scandium.

Ramsay

The scientist who discovered the noble gases.

Henry Moseley

The Father of the Modern Periodic Table ($1913$) who used X-ray spectroscopy to determine that elements should be arranged by atomic number.

Seaborg

The scientist who discovered transuranic elements and placed the lanthanide and actinide series at the bottom of the periodic table.

Modern Periodic Law

The principle stating that the physical and chemical properties of elements are periodic functions of their atomic numbers.

Periodicity

The repetition of physical and chemical properties of elements at regular intervals when they are arranged according to increasing atomic number.

Periods

The $7$ horizontal rows in the periodic table; elements in the same row have the same number of occupied energy levels.

Groups/Families

The $18$ vertical columns in the periodic table; elements in the same column have the same number of valence electrons and similar chemical properties.

Periodic Trends

Predictable patterns in the physical and chemical properties of elements as one moves across a period or down a group.

Atomic Radius

The distance from the center of the nucleus to the outermost occupied energy level of an atom.

Ionization Energy

The minimum amount of energy required to remove the outermost electron from a gaseous atom.

Electron Affinity

The energy change that occurs when a neutral gaseous atom gains an electron.

Electronegativity

The ability of an atom to attract shared electrons in a chemical bond, with Fluorine ($F$) being the most electronegative element.

Nuclear Charge

The attractive force for electrons caused by the number of protons in the nucleus.

Shielding Effect

The phenomenon where inner electrons reduce the attractive force felt by outer electrons from the nucleus.