Chemistry Periodic Table Quiz

Dobereiner's Triad theory groups elements into sets of three, where the middle element's atomic mass is roughly the average of the other two's. This arrangement reveals similar chemical properties within the triad.

Newlands' Law of Octaves suggests that when elements are arranged in increasing atomic mass order, every eighth element exhibits similar properties to the first. This creates a pattern of repeating properties like musical octaves.

Dobereiner's Triad theory wasn't applicable to all elements, suggesting limitations in its ability to predict properties or classify elements accurately. It was a stepping stone towards a more comprehensive understanding of chemical properties.

Newlands' Law of Octaves worked well until calcium, after which it broke down. This suggests that while the periodic nature of elements was evident, a more refined organization was needed for the entire periodic table.

In periods 2 and 3, the similarity in properties occurs in every ninth element, not every eighth. This is because the properties of elements are more complex than initially understood and are not solely determined by atomic mass order.

A law stating that elements are arranged in a table based on increasing atomic mass, and that their chemical and physical properties repeat at regular intervals.

A Russian chemist who developed the first version of the periodic table.

A group of elements with similar chemical properties.

Elements that were not yet discovered when Mendeleev made his table.

Mendeleev's predictions about the properties of elements that were not yet discovered.

The element gallium (eka-aluminium) was discovered later in 1874, confirming Mendeleev's predictions.

The element germanium (eka-silicon) was discovered later in 1886, again supporting Mendeleev's predictions.

Mendeleev's table allowed him to predict the existence and properties of elements that were yet to be discovered.

A fundamental theory that states that all matter is made up of tiny, indivisible particles called atoms.

States that atoms are not indivisible, but are made up of even smaller particles called subatomic particles. These particles include protons, neutrons, and electrons.

The number of protons in the nucleus of an atom.

The total number of protons and neutrons in the nucleus of an atom.

Atoms of the same element that have the same number of protons but different numbers of neutrons.

The average mass of all the isotopes of an element.

A model that describes the structure of an atom. Describes the atom as a positively charged sphere with electrons embedded throughout like raisins in a pudding.

A model that describes the structure of an atom. Describes the atom as a dense, positively charged nucleus surrounded by negatively charged electrons that orbit the nucleus.

A model that describes the structure of an atom. Describes the atom as having electrons orbiting the nucleus in specific energy levels or shells, also known as Bohr's model

A model that describes the structure of an atom using quantum mechanics. It's more complex than Bohr's model and predicts the probability of finding an electron at a particular point in space.

The outermost energy level or shell of an atom that contains electrons.

The arrangement of electrons in an atom's energy levels.

A process of determining the electron configuration of an atom.

The minimum energy state of an atom.

An excited state where an atom absorbs energy and moves to a higher energy level.

The process in which an electron absorbs energy and moves to a higher energy level.