Atomic Structure (IB)

Isotopes

Atoms of the same element with the same number of protons but different numbers of neutrons, leading to different mass numbers.

Mass Spectrometer

Instrument used to determine the relative atomic masses of elements by analyzing the mass-to-charge ratio of ions.

Steps to Calculate Relative Atomic Mass

1. The sample being studied would be vaporized to form a gas

2. It is bombarded with high-energy electrons, producing positive ions (+1)

3. The positive ions are accelerated in an electric field

4. The positive ions are deflected in a magnetic field depending on the mass ot charge ratio (m/z)

5. The ions with a higher m/z are deflected less in the magnetic field

6. The positive ions reach the detector, where they produce a mess spectrum

Atomic Orbitals

Regions in space where electrons are likely to be found within an atom.

Bohr Model

an atomic orbital model that concludes that electrons exist in energy levels

Principle Energy Levels

assigned numbers with n = 1 being the closest to the nucleus and of lowest energy, with the higher numbers being further from the nucleus

Pauli Exclusion Principle

States that no two electrons in an atom can have the same set of quantum numbers.

Heisenberg’s Uncertainty Principle

It is not possible to know, at th same time, the exact position and momentum of an electron. Instead, only a probability can be stated than an electron will be somewher in a given region of space

Aufbau Principle

Electrons fill the lowest energy atomic orbitals first within a main energy level.

Degenerate Orbitals

atomic orbitals within a sub-level are of equal energy

Condensed electron Configuration

a shorthand version of writing the electron configuration for atoms or ions using noble gasses

Exceptions of Aufbau Principles

Copper and Chromium

Orbital Diagrams

Representations of electron configurations in atomic orbitals using boxes and arrows.

Line Spectra

Patterns of wavelengths emitted or absorbed by electrons transitioning between energy levels in atoms.

Absorption Line Spectra

produced when electrons absorb energy and transition from lower to higher energy levels

Emission line spectra

produced when electrons emit energy and transmission from higher to lower energy levels

Violet Light

light of shortest wavelength

Red Light

light of longest wavelength

Hydrogen Emission Spectrum

Spectrum produced when electrons in hydrogen atoms transition between energy levels, emitting specific wavelengths of light.

Ultraviolet radiation

has an electron Transition of N = 1

Visible Light

has an electron Transition of N = 2

Infared Radiation

has an electron Transition of N = 3

Electromagnetic Spectrum

The complete range of all types of radiation that has both electric and magnetic fields and travels in waves

Atomic Sublevels

Main atomic energy levels split into s, p, d, f