Page 2: Mass Spectra Analysis and Detection

This page details the separation and detection stages of mass spectrometry, including the interpretation of mass spectra for different elements.

Definition: Mass spectra show the abundance of ions plotted against their mass-to-charge ratio (m/z).

Example: The mass spectrum of bromine shows characteristic isotope patterns that help identify the element.

Highlight: The flight tube separation process relies on the principle that lighter ions travel faster than heavier ones when given the same kinetic energy.

Vocabulary: Isotopes are atoms of the same element with different numbers of neutrons.

Page 3: Electron Configuration and Orbital Structure

The third page explores the detailed structure of atomic shells, subshells, and orbitals, providing a comprehensive view of electron configuration.

Definition: Electron configuration describes how electrons are distributed in an atom's orbital structure.

Highlight: Shells are divided into subshells (s, p, d, f), each containing specific numbers of orbitals and electrons.

Example: The first shell contains only an s orbital with 2 electrons, while the second shell has both s and p orbitals holding up to 8 electrons total.

Vocabulary: Orbitals are regions in an atom where electrons are most likely to be found.

Electronic Configuration

This section explores the complex arrangement of electrons in atomic shells and subshells. The orbital structure determines chemical properties and behavior.

Definition: Shells are divided into subshells containing orbitals, with each orbital holding two electrons.

Highlight: The filling order of orbitals follows increasing energy levels: 1s→2s→2p→3s→3p→4s→3d→4p→5s→4d→5p→6s.

Example: Special exceptions exist for elements like Chromium (Cr) and Copper (Cu) in their orbital filling patterns.

Ionisation Energy Principles

The page covers ionisation energy and factors affecting electron removal from atoms. Electron impact and electrospray ionisation differences become apparent in their applications.

Definition: First ionisation energy is the energy required to remove one mole of electrons from one mole of gaseous atoms.

Highlight: Nuclear charge, atomic radius, and shielding are key factors affecting ionisation energy.

Example: Increased nuclear charge leads to higher ionisation energy due to stronger attraction to outer electrons.

Page 1: Fundamental Particles and Ionisation Techniques

The first page introduces fundamental atomic particles and mass spectrometry concepts. It explains how Time of Flight (TOF) mass spectrometry works as an analytical method for identifying elements and determining relative molecular mass.

Definition: Time of Flight (TOF) mass spectrometry is an analytical technique used to identify elements and determine their relative molecular mass by measuring the time particles take to travel a fixed distance.

Highlight: Two main ionisation techniques are presented: Electron Impact and Electrospray Ionisation, each suited for different types of substances.

Example: Electron Impact ionisation is particularly effective for substances with low molecular mass like CH₂ or CO₂, while Electrospray ionisation works better for larger molecules like proteins.

Vocabulary: Ionisation refers to the process of creating charged particles by adding or removing electrons.