IB Chemistry HL Topic 3

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10 cards   |   Total Attempts: 184
  

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Cards In This Set

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3.1.1: Describe the arrangement of elements in the periodic table in order of increasing atomic number.
Names and symbols of the elements are given in the Chemistry data booklet. The history of the periodic table will not be assessed.
  • Periodic Table is arranged according to increasing atomic number and consists of horizontal rows called periods, and vertical columns called groups (or families). The arrangement is such that elements with similar chemical properties fall directly beneath each other in the same group.
3.1.2: Distinguish between the terms group and period.
  • A period is a series of elements arranged according to increasing atomic number, which begins with the first element having one electron in a new main energy level.

  • A group is a vertical column consisting of elements with the same electron arrangement in their outer energy levels, which gives the group similar chemical properties.
3.1.3: Apply the relationship between the electron arrangement of elements and their position in the periodic table up to Z = 20.
  • Valence electrons are electrons in the outermost energy level (the highest energy level) of an atom and are usually the electrons that take part in a chemical reaction.
  • Properties of elements are chiefly due to the number and arrangement of electrons in the outer energy level of atoms.
3.1.4: Apply the relationship between the number of electrons in the highest occupied energy level for an element and its position in the periodic table.
The number of valence electrons is the same for a group, but increases across a period.
3.2.1: Define the terms first ionization energy and electronegativity.
Electronegativity: The tendency for the atoms of the element to attract electrons when they are chemically combined with another element.
Ionisation energy: The energy that is required (or given out) to overcome the attraction of the nuclear charge and remove an electron from a gaseous atom. Removing 1 electron results in a +1 charge.
3.2.2: Describe and explain the trends in atomic radii, ionic radii, first ionization energies, electronegativities and melting points for the alkali metals and the halogens.
Answer 6
Data for all these properties is listed in the Chemistry data booklet. Explanations for the first four trends should be given in terms of the balance between the attraction of the nucleus for the electrons and the repulsion between electrons. Explanations based on effective nuclear charge are not required.
3.2.3: Describe and explain the trends in atomic radii, ionic radii, first ionization energies and electronegativities for elements across period 3.
Answer 7
See image.
3.2.4: Compare the relative electronegativity values of two or more elements based on their positions in the periodic table.
Compare.
3.3.1: Discuss the similarities and differences in the chemical properties of elements in the same group.
The following reactions should be covered.
  • Alkali metals (Li, Na and K) with water
  • Alkali metals (Li, Na and K) with halogens (Cl2, Br2 and I2)
  • Halogens (Cl2, Br2 and I2) with halide ions (Cl–, Br– and I–)
3.3.2: Discuss the changes in nature, from ionic to covalent and from basic to acidic, of the oxides across period 3.
Answer 10
Equations are required for the reactions of Na2O, MgO, P4O10 and SO3 with water.