Atomic Theories and Fundamental Laws in Chemistry Quiz

Democritus proposed the atomic theory asserting that atoms are fundamental, indivisible particles.

The Law of Conservation of Mass states that the total mass in a chemical reaction remains constant; mass cannot be created or destroyed.

The Law of Definite Proportions asserts that a compound always has the same elements in a fixed proportion by mass.

The Law of Conservation of Mass is significant as it declares that matter remains constant in quantity during a chemical reaction.

Rutherford's gold foil experiment demonstrated that atoms have a small, dense nucleus, surrounded by mostly empty space.

John Dalton proposed the modern atomic theory, asserting that atoms of the same element are identical in size, mass, and chemical properties.

JJ Thomson proposed the plum pudding model, suggesting electrons are embedded in a positively charged sphere.

Niels Bohr proposed the planetary model, suggesting electrons orbit the nucleus in fixed paths.

John Dalton proposed the Law of Multiple Proportions, stating that when elements form compounds, their masses combine in small whole-number ratios.

Avogadro's Law states that equal volumes of gases, under the same conditions, contain an equal number of molecules.

The electron was the first subatomic particle to be discovered, indicating the existence of negatively charged particles within atoms.

The Millikan oil drop experiment determined the mass of the electron, a fundamental discovery in atomic physics.

James Chadwick discovered the neutron, an uncharged subatomic particle, completing the understanding of atomic structure.

The discovery of the nucleus, as revealed by Rutherford's experiments, led to the rejection of the plum pudding model of the atom.

Niels Bohr introduced the concept of energy levels to explain the stability of electrons in specific orbits around the nucleus.

Henry Moseley proposed the concept of atomic number, leading to the organization of the periodic table based on atomic number.