Atomic Structure and Subatomic Particles

Flashcards covering the structure of the atom, subatomic particles, atomic number, mass number, isotopes, nuclide symbols, and ion charges based on lecture notes.

Rutherford's Gold Foil Experiment

An experiment developed in 1911 that helped establish the structure of the atom.

Nucleus

The dense core of an atom, containing protons and neutrons.

Protons

Positively charged particles found within the nucleus of an atom.

Neutrons

Particles with no charge found within the nucleus, which help to stabilize it.

Electrons

Particles found in the 'empty space' outside the nucleus.

Neutral Atom

An atom in which the number of protons equals the number of electrons.

Electron (properties)

A subatomic particle with a relative charge of -1 and a relative mass of 0.005 amu.

Proton (properties)

A subatomic particle with a relative charge of +1 and a relative mass of 1 amu.

Neutron (properties)

A subatomic particle with a relative charge of 0 and a relative mass of 1 amu.

Atomic Number (Z)

Equal to the number of protons in the nucleus of an atom and is unique to every element on the Periodic Table.

Isotopes

Atoms with the same atomic number (same number of protons) but different numbers of neutrons, resulting in different physical properties but the same chemical properties.

Mass Number (A)

Equal to the sum of the number of protons and neutrons in the nucleus of an atom (A = #p + #n).

Nuclide Symbols

Symbols used to represent isotopes of an element, showing the atomic number (Z), mass number (A), and element symbol, and optionally the charge.

Ion

An atom or molecule that has gained or lost one or more electrons, resulting in a net electrical charge.

Charge on a Nuclide Symbol

Indicated on the upper right-hand corner of a nuclide symbol, it results from the addition or loss of electrons to atoms.

Electron Loss

Results in a positive charge on the ion (+1 for each electron lost).

Electron Gain

Results in a negative charge on the ion (-1 for each electron gained).

Calculating number of electrons in an ion

Determined by the formula: # electrons = Z – charge.