Chemistry Periodic Table Quiz

The Russian chemist who first organized the elements by atomic mass in 1869.

A chart that organizes the chemical elements by increasing atomic number, showing the recurring patterns of their properties.

A measure of the average mass of an atom of an element, used by Mendeleev to organize his periodic table.

A chemical element that was predicted by Mendeleev to exist, but wasn't discovered until later.

A chemical element that was predicted by Mendeleev to exist, but wasn't discovered until later.

A chemical element that was predicted by Mendeleev to exist, but wasn't discovered until later.

A group of elements that are very unreactive, located at the far right of the periodic table.

The first noble gas discovered in 1894, also known as inert gas.

A noble (or inert) gas discovered by William Ramsay in 1895.

A noble (or inert) gas discovered by William Ramsay in 1895.

A noble (or inert) gas discovered by William Ramsay in 1895.

An English physicist who rearranged the periodic table by atomic number in 1911.

The principle stating that the chemical properties of elements are periodic functions of their atomic number.

The number of protons in the nucleus of an element, which defines the element's identity.

Electrons that occupy the outermost energy level of an atom, responsible for chemical bonding.

Energy levels in an atom, also called electron shells, that influence the element's period in the periodic table.

Subdivisions within principle energy levels, designated as s, p, d, and f, which determine the element's placement within the periodic table.

Elements located in Groups 1, 2, and 13-18 of the periodic table, representing the majority of elements.

A number that indicates the number of valence electrons in an element, determining its reactivity.

The arrangement of electrons within the orbitals of an atom, indicating its chemical behavior and bonding properties.

Specific regions within an atom where electrons are likely to be found, dictated by their energy levels.

Elements that occur naturally on Earth, making up almost all the matter we know.

Moseley's contribution was to use atomic number rather than atomic mass to arrange the periodic table, resulting in a more accurate and logical organization.

Vertical columns in the periodic table, each representing a group of elements with similar chemical properties.

Horizontal rows in the periodic table, each representing a period and a specific principle energy level of the elements.

The atomic number (number of protons) of an element dictates its chemical properties, which are periodic functions of the atomic number. This means that elements with similar atomic numbers will have similar chemical properties.

Elements that occur naturally on Earth, making up the majority of the matter we know. Some examples include Carbon, Oxygen, Hydrogen, Nitrogen, Phosphorus, and Calcium.

The number of protons within an atom’s nucleus defines its identity. This number, referred to as the atomic number, governs the arrangement of an element within the periodic table and greatly influences its chemical properties.

The electrons occupying the outermost shell of an atom are called valence electrons. They are responsible for an element’s chemical behavior and are directly involved in the formation of chemical bonds. In a neutral atom, the number of valence electrons is equal to the group number.

These levels, also known as electron shells, are filled with electrons according to the Aufbau principle and Hund’s rule. The number of energy levels determines the period of an atom in the periodic table.

Sublevels represent the arrangement of electrons within each principle energy level, differentiating among electronic orbitals like s, p, d, and f. The periodic table can be segmented into different blocks based on these sublevels, reflecting the element’s reactivity.

The periodic table can be segmented into columns known as 'groups.’ These elements share similarities in their chemical properties and bonding tendencies. The main group elements, located in groups 1, 2, and 13-18, represent the majority of elements in the periodic table.

The group number of an element within the periodic table indicates the number of valence electrons it possesses. Valence electrons represent the electrons in the outermost shell of an atom that drive chemical reactions and bond formation.

The electron configuration of an element describes the specific arrangement of electrons in its atomic orbitals. This arrangement is governed by the Aufbau principle and Hund’s rule.

Sublevels are specific regions within an atom where electrons are likely to be found. These sublevels, designated as s, p, d, and f, are influenced by their energy levels.