Introduction to Stoichiometry - A Level Chemistry

OCR H432 · 2.1.1 · 2.1.2 · 2.1.3(a)–(c)

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2.1.1(a) isotopes as atoms of the same element with different numbers of neutrons and different masses 2.1.1(b) atomic structure in terms of the numbers of protons, neutrons and electrons for atoms and ions, given the atomic number, mass number and any ionic charge 2.1.1(c) explanation of the terms relative isotopic mass (mass compared with 1/12th mass of carbon-12) and relative atomic mass (weighted mean mass compared with 1/12th mass of carbon-12), based on the mass of a ¹²C atom, the standard for atomic masses 2.1.1(d) use of mass spectrometry in:
(i) the determination of relative isotopic masses and relative abundances of the isotope,
(ii) calculation of the relative atomic mass of an element from the relative abundances of its isotopes 2.1.1(e) use of the terms relative molecular mass, M_r, and relative formula mass and their calculation from relative atomic masses. 2.1.2(a) the writing of formulae of ionic compounds from ionic charges, including:
(i) prediction of ionic charge from the position of an element in the periodic table
(ii) recall of the names and formulae for the following ions: NO₃⁻, CO₃²⁻, SO₄²⁻, OH⁻, NH₄⁺, Zn²⁺ and Ag⁺ 2.1.2(b) construction of balanced chemical equations (including ionic equations), including state symbols, for reactions studied and for unfamiliar reactions given appropriate information. 2.1.3(a) explanation and use of the terms:
(i) amount of substance
(ii) mole (symbol ‘mol’), as the unit for amount of substance
(iii) the Avogadro constant, N_A (the number of particles per mole, 6.02 × 10²³ mol⁻¹)
(iv) molar mass (mass per mole, units g mol⁻¹),
(v) molar gas volume (gas volume per mole, units dm³ mol⁻¹) 2.1.3(b) use of the terms:
(i) empirical formula (the simplest whole number ratio of atoms of each element present in a compound)
(ii) molecular formula (the number and type of atoms of each element in a molecule) 2.1.3(c) calculations of empirical and molecular formulae, from composition by mass or percentage compositions by mass and relative molecular mass

Introduction to Stoichiometry

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