Atomic Structure (IB)

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Isotopes

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

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Mass Spectrometer

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

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24 Terms

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Isotopes

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

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Mass Spectrometer

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

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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

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Atomic Orbitals

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

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Bohr Model

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

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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

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Pauli Exclusion Principle

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

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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

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Aufbau Principle

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

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Degenerate Orbitals

atomic orbitals within a sub-level are of equal energy

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Condensed electron Configuration

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

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Exceptions of Aufbau Principles

Copper and Chromium

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Orbital Diagrams

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

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Line Spectra

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

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Absorption Line Spectra

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

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Emission line spectra

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

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Violet Light

light of shortest wavelength

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Red Light

light of longest wavelength

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Hydrogen Emission Spectrum

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

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Ultraviolet radiation

has an electron Transition of N = 1

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Visible Light

has an electron Transition of N = 2

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Infared Radiation

has an electron Transition of N = 3

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Electromagnetic Spectrum

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

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Atomic Sublevels

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