Periodic Table Vocabulary Review

Vocabulary flashcards covering key terms from the Periodic Table lecture notes. The cards focus on definitions and core concepts such as groups, periods, energy levels, valence electrons, and the major element families.

Periodic Table

An arrangement of the known elements based on atomic number and chemical/physical properties; divided into Metals, Nonmetals, and Metalloids.

Atomic number

The number of protons in an atom's nucleus; identifies the element.

Metals

One of the three basic categories of the periodic table.

Nonmetals

One of the three basic categories of the periodic table.

Metalloids

Elements with characteristics of metals and nonmetals; located along the zig-zag line separating metals from nonmetals (Groups 13–17 contain some).

Atomic structure

Atoms are made of protons, neutrons, and electrons; elements are atoms of only one type.

Electron cloud

Region around the nucleus where electrons are located; energy levels are located within the cloud.

Energy levels

Regions around the nucleus that hold electrons; atoms have 1–7 energy levels.

Valence electrons

Electrons in the outermost energy level; determine reactivity; outer level often not full.

Groups (families)

Vertical columns in the periodic table; groups are numbered 1–18 and have similar properties; same number of valence electrons.

Periods

Horizontal rows (1–7) in the periodic table; elements in a period have the same number of energy levels.

Hydrogen stands apart

Hydrogen has 1 valence electron and is very reactive; its properties resemble nonmetals more than metals.

Group 1: Alkali metals

Metals with 1 valence electron; very reactive; solids; soft; shiny; react violently with water; low density.

Group 2: Alkaline-Earth Metals

Metals with 2 valence electrons; very reactive but less than Group 1; solids; silver-colored; more dense than Group 1.

Groups 3–12: Transition Metals

Metals with 1 or 2 valence electrons; less reactive than Groups 1–2; higher density; good conductors of heat and electricity.

Lanthanides

Lanthanide series (rare earth elements) in the range 58–71; valence electrons ~3; very reactive with high luster and conductivity; tarnish easily.

Actinides

Actinide series (rare earth elements) in the range 90–103; valence electrons ~3 (up to 6); reactive, unstable, all radioactive; most made in laboratories.

Group 13: Boron Group

Contains 1 metalloid and 4 metals; valence electrons ~3; reactive; solid at room temperature.

Group 14: Carbon Group

Contains 1 non-metal, 2 metalloids, and 3 metals; valence electrons ~4; solid at room temperature.

Group 15: Nitrogen Group

Contains 2 non-metals, 2 metalloids, and 1 metal; valence electrons ~5; all but N are solid at room temperature.

Group 16: Oxygen Group

Contains 3 non-metals, 1 metalloid, and 2 metals; valence electrons ~6; all but O are solid at room temperature.

Group 17: Halogens

Nonmetals; very reactive; poor conductors of electricity; react violently with alkali metals to form salts; never found uncombined in nature.

Group 18: Noble Gases

Nonmetals; valence electrons 8 (2 for He); unreactive; colorless, odorless gases at room temperature; outer energy level full; found in the atmosphere.

Hydrogen stands apart

Hydrogen has 1 valence electron; very reactive; properties similar to nonmetals rather than metals; stands apart from other groups.

Period

Horizontal rows (1–7) of the periodic table; all elements in a period have the same number of energy levels.

Energy level filling rule

Across a period, each element has one more electron in its outer shell than the previous element, leading to regular changes in chemical behavior.

Reactivity

A chemical property that determines how elements will react with others to form compounds.

Givers

The most reactive metals (Groups 1 and 2) that readily give up valence electrons to form compounds.

Takers

The most reactive nonmetals (Groups 6 and 7) that readily receive valence electrons to form compounds.

Valence electrons by group

Group numbers help determine the number of valence electrons (e.g., Group 1 has 1 valence electron; Group 2 has 2).