Structure of Atoms and Charged Particles

A model proposing that atoms have a positively charged nucleus at the center and electrons revolve around it.

The central positively charged part of an atom containing protons and neutrons.

Rutherford's model failed to explain why electrons wouldn't spiral into the nucleus due to energy loss.

Bohr proposed that electrons move in fixed orbits without losing energy.

The stable orbits where electrons reside, also known as energy shells.

A neutral subatomic particle in the nucleus with mass nearly equal to a proton.

The rule stating that the outermost shell can hold a maximum of 8 electrons.

The formula 2n^2 indicates the number of electrons in an orbit, where n is the orbit number.

A theory proposing the atom has a small nucleus with positive charge and electrons surrounding it.

Doubly-charged helium ions used in Rutherford's experiments.

An experiment where alpha particles are shot at gold foil to study atomic structure.

Change in direction of alpha particles due to interactions with atomic structures.

Most of an atom's volume is empty as most alpha particles passed through.

Rutherford concluded that positive charge is located in a small part of the atom.

The nucleus is about 10,000 times smaller than the atom's radius.

Most alpha particles passed through the foil, few were deflected significantly.

An atom consists of protons, neutrons, and electrons, with protons and neutrons in the nucleus.

Positively charged particles located in the nucleus of an atom, discovered by E. Goldstein as canal rays.

Negatively charged particles that orbit around the nucleus of an atom, discovered by J.J. Thomson.

Proposed that an atom is a positively charged sphere with embedded electrons, resembling a watermelon.

Positively charged radiations discovered by E. Goldstein, leading to the identification of protons.

Dalton's theory failed as it claimed atoms were indivisible, contradicting the existence of subatomic particles.

Atoms of the same element with different masses, contradicting Dalton's claim of uniformity among atoms.

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

Weighted average of an element's isotopes based on their natural abundance.

Atoms of different elements that share the same mass number.

The number of protons in an atom, defining the element.

Electrons in the outermost shell of an atom.

An atom's combining capacity and tendency to react with others.

Atoms with full outermost shells, showing little chemical activity.

Valency of hydrogen is 1, as it can lose 1 electron.

Subtract the number of outer shell electrons from 8 for valency.

Isotopes can be used in nuclear reactors, cancer treatment, and medical diagnoses.