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Atomic structure explorer

Build atoms and ions from protons, neutrons and electrons, find relative atomic mass from a mass spectrum, fill shells and orbitals, and plot real ionisation energies.

Back to topics: Atomic Structure (H1 Chemistry)Atomic Structure (H2 Chemistry)The Particulate Nature of Matter (G2 Science (Chemistry))The Particulate Nature of Matter (G3 Science (Chemistry))Chemical Calculations (G2 Science (Chemistry))Chemical Calculations (G3 Science (Chemistry))The Particulate Nature of Matter (G3 Pure Chemistry / O-Level Chemistry)The Periodic Table (H1 Chemistry)The Periodic Table (H2 Chemistry)The Mole Concept and Stoichiometry (H1 Chemistry)Stoichiometry (H2 Chemistry)Stoichiometry & The Mole Concept (G3 Pure Chemistry / O-Level Chemistry)

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Learning objectives

  • state the relative charges and approximate relative masses of a proton, a neutron and an electron
  • describe, with the aid of diagrams, the structure of an atom as consisting of protons and neutrons (nucleons) in the nucleus and electrons arranged in shells (energy levels) (knowledge of s, p, d and f classification is not required; a copy of the Periodic Table will be available in the examination)
  • define proton (atomic) number and nucleon (mass) number
  • interpret and use nuclide notations such as ¹²₆C
  • define the term isotopes
  • deduce the numbers of protons, neutrons and electrons in atoms and ions given proton and nucleon numbers.
  • define relative atomic mass, Ar
  • describe, with the aid of diagrams, the structure of an atom as consisting of protons and neutrons (nucleons) in the nucleus and electrons arranged in shells (energy levels) (knowledge of s, p, d and f classification is not required; a copy of the Periodic Table will be available in Papers 1 and 2)
  • interpret and use nuclide notations such as 126 C
  • identify and describe protons, neutrons and electrons in terms of their relative charges and relative masses
  • describe the distribution of mass and charges within an atom
  • deduce the numbers of protons, neutrons and electrons present in both atoms and ions given proton and nucleon numbers (and charge)
  • — describe the contribution of protons and neutrons to atomic nuclei in terms of proton number and nucleon number
  • — distinguish between isotopes on the basis of different numbers of neutrons present
  • describe the number and relative energies of the s, p and d orbitals for the principal quantum numbers 1, 2 and 3 and also the 4s and 4p orbitals
  • state the electronic configuration of atoms and ions given the proton number (and charge)
  • explain the factors influencing the ionisation energies of elements (see the Data Booklet) (see also Section 4)
  • deduce the electronic configurations of elements from successive ionisation energy data
  • interpret successive ionisation energy data of an element in terms of the position of that element within the Periodic Table
  • define the terms relative atomic, isotopic, molecular and formula mass
  • calculate the relative atomic mass of an element given the relative abundances of its isotopes
  • recognise variation in the electronic configurations across a Period and down a Group
  • describe and explain qualitatively the general trends and variations in atomic radius, ionic radius, first ionisation energy and electronegativity: — across a Period in terms of shielding and nuclear charge
  • describe and explain qualitatively the general trends and variations in atomic radius, ionic radius, first ionisation energy and electronegativity: — down a Group in terms of increasing number of electron shells, shielding and nuclear charge
  • Subatomic Particles, Isotopes, Ions
  • Atomic Orbitals: Energies and Shapes
  • Orbitals and Electron Configuration
  • First Ionisation Energy Trends
  • Successive Ionisation Energies
  • Mole and Avogadro Constant
  • Periodic Trends (Radius, IE, EN)

6 protons and 6 neutrons in the nucleus, 6 electrons in shells 2, 4: a carbon-12 atom.

Nucleon number
12
Charge
0
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Course

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0 of 4 done

  1. Build an atom of carbon-12, then change it into carbon-14. (not done yet)

  2. Make a sodium ion, Na⁺, and a chloride ion, Cl⁻. (not done yet)

  3. In the mass spectrum of chlorine, make the two peaks the same height. (not done yet)

  4. Remove sodium's electrons one at a time until the energy needed jumps. (not done yet)

Does this count towards my progress?