Core atomic structure, bonding, stoichiometry, and equilibrium concepts from the IB Chemistry syllabus. Front: the term or formula. Back: definition or formula with a brief usage note.
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- Proton
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Positively charged particle in the nucleus; each has a mass of 1 amu and contributes to mass number- Neutron
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Neutral particle in the nucleus; has a mass of approximately 1 amu and does not affect atomic charge- Electron
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Negatively charged particle that orbits the nucleus in electron shells; determines chemical properties- Atomic number (Z)
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The number of protons in an atom; defines the element and determines its position in the periodic table- Mass number (A)
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The total number of protons and neutrons in an atom's nucleus- Isotope
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Atoms of the same element (same number of protons) that have different numbers of neutrons- Relative atomic mass
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The average mass of an atom of an element compared to 1/12 of a carbon-12 atom; appears on the periodic table- Electron affinity
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The energy change when a gaseous atom gains an electron; usually negative (energy released) for nonmetals- Electronegativity
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The ability of an atom to attract bonding electrons; increases across a period and up a group on the periodic table- Covalent bond
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A bond formed by the sharing of electron pairs between two atoms, typically between nonmetals- Ionic bond
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An electrostatic attraction between ions of opposite charge; formed when electrons are transferred from metal to nonmetal- Metallic bond
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A bond formed by the attraction between metal cations and a delocalized electron sea; accounts for metallic properties- Polar covalent bond
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A covalent bond where electrons are unequally shared due to differences in electronegativity of the atoms- Electronegativity difference determines bond type
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Difference less than 0.5: nonpolar covalent; 0.5 to 1.7: polar covalent; greater than 1.7: ionic- Coordinate covalent bond (dative bond)
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A covalent bond in which both electrons in the shared pair originate from the same atom
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