Atomic Structure and Principles of Applied Science

Flashcards covering the history of atomic theory, subatomic particle properties, isotopes, and unit course information based on the BTEC Level 3 Applied Science curriculum.

Democritus (400 BC)

Proposed 'Atomos', describing them as the building blocks of matter where the shape of an atom explains the behavior of elements.

John Dalton (1803)

Proposed the Solid Sphere model, stating the atom is a solid indivisible sphere.

J.J. Thomson (1897)

Proposed the Plum Pudding model, where negative electrons are embedded in a sea of positive charges.

Ernest Rutherford (1911)

Proposed the Nuclear model, where positive charges are located within a central nucleus.

Niels Bohr (1913)

Proposed the Planetary model, describing electrons as restricted in circular orbits with different energy levels.

Erwin Schrödinger (1926)

Proposed the Quantum model, where electrons are in clouds surrounding the nucleus and this cloud is less dense.

Proton (Relative Mass and Charge)

Has a relative mass of $1$ and a charge of $+1$.

Neutron (Relative Mass and Charge)

Has a relative mass of $1$ and a charge of $0$.

Electron (Relative Mass and Charge)

Has a relative mass of $1/2000$ and a charge of $-1$.

Proton (Mass in grams)

$$1.6727 \times 10^{-24}\,g$$

Neutron (Mass in grams)

$$1.6750 \times 10^{-24}\,g$$

Electron (Mass in grams)

$$9.110 \times 10^{-28}\,g$$

Atomic number

The number of protons in the nucleus of an atom.

Mass number

The total number of protons plus the number of neutrons in an atom.

Isotopes

Atoms of the same element that have different mass numbers because they have different numbers of neutrons in their nucleus.

Bohr Model

A model explaining atomic spectra by describing electrons as occupying fixed energy levels or shells.

Number of Neutrons formula

$$\text{Number of Neutrons} = \text{Atomic Mass} - \text{Atomic Number}$$

Unit 1 Externally Assessed Components

Chemistry (06/01/2026 a.m.), Physics (06/01/2026 p.m.), and Biology (07/01/2026 p.m.).

Unit 2 Aim A

Extraction and chromatography (Chemistry internal assessment).

Unit 2 Aim B

Calorimetry and cooling curves (Physics internal assessment).

Unit 2 Aim C

Titration and colorimetry (Chemistry internal assessment).