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1periodictableandatomicstructurelearningoutcomes 140308200450-phpapp02

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This document outlines the learning outcomes for the topic of periodic table and atomic structure in Leaving Certificate Chemistry in Ireland. It includes 3 sections - the periodic table and atomic structure, atomic structure, and radioactivity. For each section, it lists the key concepts students should understand, such as describing trends in the periodic table, outlining the historical development of atomic theory, and defining and explaining terms like isotopes, ionization energy, and oxidation and reduction reactions. It provides a detailed overview of the essential knowledge students are expected to retain about fundamental chemical concepts relating to the periodic table, atomic structure, and radioactivity.

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Learning Outcomes Leaving Certificate Chemistry 1 Periodic table and atomic structure Each topic has a set of boxes which the pupil can tick to show how well they understanding or how well they know the topic. This is useful for revision. Bold text indicates Higher Level. 1.1 The periodic table of elements. (3 class periods) By the end of this section pupils should be able to Good Fair Poor describe the periodic table as a list of elements arranged so as to demonstrate trends in their physical and chemical properties define the term element associate the first 36 elements with their elemental symbols distinguish between elements and compounds state the principle resemblances of elements within each main group, in particular alkali metals, alkaline earth metals, halogens and noble gases describe the reaction between water and lithium, sodium and potassium having seen the reaction demonstrated describe by means of a chemical equation the reaction between water and lithium, sodium and potassium having seen the reaction demonstrated outline the history of the idea of elements, including the contributions of the Greeks, Boyle, Davy and Moseley outline the contributions of Mendeleev, Dobereiner, Newlands and Moseley to the structure of the modern periodic table compare mendeleev’s periodic table with the modern periodic table arrange elements in order of relative atromic mass and note differences with modern periodic table 1.2 Atomic Structure (6 class periods) By the end of this section pupils should be able Good Fair Poor outline the historical development of atomic theory (outline principles only, mathematical treatment not required): Dalton: atomic theory; Crookes: vacuum tubes, cathode rays; Stoney: naming of the electron; Thomson: negative charge of the electron; e/m for electrons (experimental details not required); Millikan: magnitude of charge of electrons as shown by oil drop experiment (experimental details not required);
Learning Outcomes Leaving Certificate Chemistry Rutherford: discovery of the nucleus as shown by the particle scattering experiment; discovery of protons in nuclei of various atoms; Bohr: model of the atom; Chadwick: discovery of the neutron. recall that matter is composed of particles, which may be atoms, molecules or ions define an atom appreciate that atoms are minute particles state the law of conservation of mass describe, relative mass, relative charge and location of a proton, neutron, and electron in an atom define atomic number (Z) mass number(A) define relative atomic mass (Ar) using the C12 scale define isotope describe the composition of isotopes using hydrogen and carbon as examples describe how a mass spectrometer can be used to determine relative atomic mass describe the principles on which the Mass Spectrometer is based explain the fundamental processes that occur in a mass spectrometer calculate the approximate relative atomic masses from abundance of isotopes of given mass number 1.3 Radioactivity (2 class periods) By the end of this section pupils should be able Good Fair Poor define radioactivity describe the nature and penetrating ability of alpha, beta and gamma radiation give one example each of the following: an α emitter, a β emitter and a γ- emitter explain how radiation is detected having seen a demonstration / video ( principles of a geiger muller tube not required) define radioisotopes define and explain half life (non-mathematical treatment)
Learning Outcomes Leaving Certificate Chemistry give a historical outline of:  Becquerel’s discovery of radiation from uranium salts  Marie and Pierre Curie’s discovery of polonium and radium comment on the widespread occurrence of radioactivity distinguish between a chemical reaction and a nuclear reaction (simple equations required, confine to α and β emissions) state three uses of radioactivity, including food irradiation and the use of 60 Co for cancer treatment explain how 14 C is used for age determination (calculations not required) 1.4 Electronic Structure of Atoms (11 class periods) By the end of this section pupils should be able Good Fair Poor define and explain energy levels in atoms describe the organization of particles in atoms of elements numbers 1-20 classify the first twenty elements in the periodic table on the basis of the number of outer electrons list the numbers of electrons in each main energy level in atoms of elements nos. 1–20 describe and explain the emission spectrum of the hydrogen atom using the Balmer series in the emission spectrum as an example describe and explain the absorption spectrum use flame tests to provide evidence that energy is absorbed or released in discrete units when electrons move from one energy level to another explain how flame tests provide evidence that energy is absorbed or released in discrete units when electrons move from one energy level to another relate energy levels in atoms to everyday applications such as sodium street lights and fireworks discuss the uses of atomic absorption spectrometry (AAS) as an analytical technique illustrate how line spectra provide evidence for energy levels use a spectroscope or a spectrometer to view emission spectra of elements define and explain energy sub-levels state the Heisenberg uncertainty principle state the dual wave-particle nature of the electron (mathematical treatment not required)
Learning Outcomes Leaving Certificate Chemistry define and explain atomic orbitals describe the shapes of s and p orbitals build up the electronic structure of the first 36 elements derive the electronic configurations of ions of s- and p block elements only describe the arrangement of electrons in individual orbitals of p- block atoms define and explain atomic radius explain the general trends in values of atomic radii (covalent radii only)  down a group  across a period (main group elements only) define and explain first ionisation energy explain the general trends in first ionisation energy values:  down a group  across a period (main group elements) and explain the exceptions to the general trends across a period define and explain second and successive ionisation energies describe how second and successive ionisation energies provide evidence for energy levels recognise the relationship and trends in successive ionisation energies of an individual element explain how chemical properties of elements depend on their electronic structure explain how atomic radius, screening effect and nuclear charge account for general trends in properties of elements in groups I and VII 1.5 Oxidation and Reduction (7 class periods) By the end of this section pupils should be able Good Fair Poor define oxidation and reduction in terms of electron transfer use simple examples , e.g. Na with Cl2, Mg with O2, Zn with Cu2+ to describe oxidation and reduction in terms of electron transfer apply knowledge of oxidation and reduction to explain the rusting of iron define oxidising agent and reducing agent arrange the electrochemical series of metals in order of their ease of oxidation (reactions, other than displacement reactions, not required)
Learning Outcomes Leaving Certificate Chemistry carry out an experiment to show that halogens act as oxidising agents(reactions with bromides, iodides, Fe2+ and sulfites; half equations only required) carry out an experiment to demonstrate the displacement reactions of metals (Zn with Cu2+, Mg with Cu2+) explain what happens at each electrode during the electrolysis of:  copper sulfate solution with copper electrodes  acidified water with inert electrodes (half equations only required) describe and account for the observations of what happens at each electrode during the electrolysis of (teacher demo)  aqueous sodium sulfate (using universal indicator)  aqueous potassium iodide (using phenolphthalein indicator) with inert electrodes (half equations only required) describe the extraction of copper by displacements using scrap iron describe and explain ionic movement as observed during teacher demonstration describe the following electrolytic processes: purification of copper, chrome and nickel plating. Give one everyday application of chrome and nickel plating e.g. cutlery

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1periodictableandatomicstructurelearningoutcomes 140308200450-phpapp02

  • 1. Learning Outcomes Leaving Certificate Chemistry 1 Periodic table and atomic structure Each topic has a set of boxes which the pupil can tick to show how well they understanding or how well they know the topic. This is useful for revision. Bold text indicates Higher Level. 1.1 The periodic table of elements. (3 class periods) By the end of this section pupils should be able to Good Fair Poor describe the periodic table as a list of elements arranged so as to demonstrate trends in their physical and chemical properties define the term element associate the first 36 elements with their elemental symbols distinguish between elements and compounds state the principle resemblances of elements within each main group, in particular alkali metals, alkaline earth metals, halogens and noble gases describe the reaction between water and lithium, sodium and potassium having seen the reaction demonstrated describe by means of a chemical equation the reaction between water and lithium, sodium and potassium having seen the reaction demonstrated outline the history of the idea of elements, including the contributions of the Greeks, Boyle, Davy and Moseley outline the contributions of Mendeleev, Dobereiner, Newlands and Moseley to the structure of the modern periodic table compare mendeleev’s periodic table with the modern periodic table arrange elements in order of relative atromic mass and note differences with modern periodic table 1.2 Atomic Structure (6 class periods) By the end of this section pupils should be able Good Fair Poor outline the historical development of atomic theory (outline principles only, mathematical treatment not required): Dalton: atomic theory; Crookes: vacuum tubes, cathode rays; Stoney: naming of the electron; Thomson: negative charge of the electron; e/m for electrons (experimental details not required); Millikan: magnitude of charge of electrons as shown by oil drop experiment (experimental details not required);
  • 2. Learning Outcomes Leaving Certificate Chemistry Rutherford: discovery of the nucleus as shown by the particle scattering experiment; discovery of protons in nuclei of various atoms; Bohr: model of the atom; Chadwick: discovery of the neutron. recall that matter is composed of particles, which may be atoms, molecules or ions define an atom appreciate that atoms are minute particles state the law of conservation of mass describe, relative mass, relative charge and location of a proton, neutron, and electron in an atom define atomic number (Z) mass number(A) define relative atomic mass (Ar) using the C12 scale define isotope describe the composition of isotopes using hydrogen and carbon as examples describe how a mass spectrometer can be used to determine relative atomic mass describe the principles on which the Mass Spectrometer is based explain the fundamental processes that occur in a mass spectrometer calculate the approximate relative atomic masses from abundance of isotopes of given mass number 1.3 Radioactivity (2 class periods) By the end of this section pupils should be able Good Fair Poor define radioactivity describe the nature and penetrating ability of alpha, beta and gamma radiation give one example each of the following: an α emitter, a β emitter and a γ- emitter explain how radiation is detected having seen a demonstration / video ( principles of a geiger muller tube not required) define radioisotopes define and explain half life (non-mathematical treatment)
  • 3. Learning Outcomes Leaving Certificate Chemistry give a historical outline of:  Becquerel’s discovery of radiation from uranium salts  Marie and Pierre Curie’s discovery of polonium and radium comment on the widespread occurrence of radioactivity distinguish between a chemical reaction and a nuclear reaction (simple equations required, confine to α and β emissions) state three uses of radioactivity, including food irradiation and the use of 60 Co for cancer treatment explain how 14 C is used for age determination (calculations not required) 1.4 Electronic Structure of Atoms (11 class periods) By the end of this section pupils should be able Good Fair Poor define and explain energy levels in atoms describe the organization of particles in atoms of elements numbers 1-20 classify the first twenty elements in the periodic table on the basis of the number of outer electrons list the numbers of electrons in each main energy level in atoms of elements nos. 1–20 describe and explain the emission spectrum of the hydrogen atom using the Balmer series in the emission spectrum as an example describe and explain the absorption spectrum use flame tests to provide evidence that energy is absorbed or released in discrete units when electrons move from one energy level to another explain how flame tests provide evidence that energy is absorbed or released in discrete units when electrons move from one energy level to another relate energy levels in atoms to everyday applications such as sodium street lights and fireworks discuss the uses of atomic absorption spectrometry (AAS) as an analytical technique illustrate how line spectra provide evidence for energy levels use a spectroscope or a spectrometer to view emission spectra of elements define and explain energy sub-levels state the Heisenberg uncertainty principle state the dual wave-particle nature of the electron (mathematical treatment not required)
  • 4. Learning Outcomes Leaving Certificate Chemistry define and explain atomic orbitals describe the shapes of s and p orbitals build up the electronic structure of the first 36 elements derive the electronic configurations of ions of s- and p block elements only describe the arrangement of electrons in individual orbitals of p- block atoms define and explain atomic radius explain the general trends in values of atomic radii (covalent radii only)  down a group  across a period (main group elements only) define and explain first ionisation energy explain the general trends in first ionisation energy values:  down a group  across a period (main group elements) and explain the exceptions to the general trends across a period define and explain second and successive ionisation energies describe how second and successive ionisation energies provide evidence for energy levels recognise the relationship and trends in successive ionisation energies of an individual element explain how chemical properties of elements depend on their electronic structure explain how atomic radius, screening effect and nuclear charge account for general trends in properties of elements in groups I and VII 1.5 Oxidation and Reduction (7 class periods) By the end of this section pupils should be able Good Fair Poor define oxidation and reduction in terms of electron transfer use simple examples , e.g. Na with Cl2, Mg with O2, Zn with Cu2+ to describe oxidation and reduction in terms of electron transfer apply knowledge of oxidation and reduction to explain the rusting of iron define oxidising agent and reducing agent arrange the electrochemical series of metals in order of their ease of oxidation (reactions, other than displacement reactions, not required)
  • 5. Learning Outcomes Leaving Certificate Chemistry carry out an experiment to show that halogens act as oxidising agents(reactions with bromides, iodides, Fe2+ and sulfites; half equations only required) carry out an experiment to demonstrate the displacement reactions of metals (Zn with Cu2+, Mg with Cu2+) explain what happens at each electrode during the electrolysis of:  copper sulfate solution with copper electrodes  acidified water with inert electrodes (half equations only required) describe and account for the observations of what happens at each electrode during the electrolysis of (teacher demo)  aqueous sodium sulfate (using universal indicator)  aqueous potassium iodide (using phenolphthalein indicator) with inert electrodes (half equations only required) describe the extraction of copper by displacements using scrap iron describe and explain ionic movement as observed during teacher demonstration describe the following electrolytic processes: purification of copper, chrome and nickel plating. Give one everyday application of chrome and nickel plating e.g. cutlery