PHYSICAL PROPERTIES OF THE PERIOD 3 OXIDES These pages explain the relationship between the physical properties of the oxides of Period 3 elements (sodium to chlorine) and their structures. Argon is obviously omitted because it doesn't form an oxide. A quick summary of the trends The oxides The oxides we'll be looking at are: |Na2O |MgO |Al2O3 |SiO2 |P4O10 |SO3 |Cl2O7 | | | | | |P4O6 |SO2 |Cl2O
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a) Name and formula of substances | Name | Formula | Bonding Type | | Metal (Stainless steel) | Fe3C | Metallic Bonding | | Plastic (Polystyrene) | - CH2CHCl | Covalent Molecular | | Glass | SiO2 | Covalent Network | b) Sketch/Plan of diagram | Chemistry Task 2: Bonding Class: Group 4 | c) Properties of Substances | Substance | Property | | Metal(Stainless Steel) | * Shiny hence providing the item an attractive appearance. * Good reflector of infrared
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P1: To outline the key features of the periodic table, atomic structure and chemical bonding. Atomic Structure and Periodicity In modern chemistry and physics it is agreed that the atom is made up of 3 key components: electrons, protons and neutrons. On the periodic table the position of an atom is decided by the number of protons and neutrons in the nucleus of the atom. The proton, electron and neutron all have different characteristic regarding mass and charge these are as follows:
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dot and cross; correct charges 2 [4] 4. shared pair of electrons i.e. ‘shared electrons’ is worth 1 mark. pair of electrons for second mark [2] 5. H2O: all correct including lone pairs around O CO2: correct covalent bonds around carbon lone pairs added around oxygen atoms (must be ‘dot AND cross’ or electron source clearly shown (different coloured for source is OK) [3] Even
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C2 Revision list Topic 1 Atomic structure and the periodic table ● Explain how Mendeleev arranged the elements, known at that time, in a periodic table by using properties of these elements and their compounds and used his table to predict the existence and properties of some elements not then discovered ● Classify elements as metals or non-metals according to their position in the periodic table ● Describe the structure of an atom as a nucleus containing protons and neutrons, surrounded by
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Ionic substances must be neutral so the total charge of anions must equal the total charge of cations; the formula of the ionic compound states the ratio that must exist to create this balance The structure that is formed as a result of this attraction of ions is a 3-dimensional crystalline structure known as an ionic lattice (fixed arrangement of ions based on a repeating pattern) • • For sodium chloride, each Na+
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Non-bonding pair of electrons, also known as lone pair of electrons are those pairs of electrons that are not used in the covalent bonding between the atoms. All the above Lewis dot structures are of covalent bonds between atoms. The attraction in covalent bonds are an electrostatic one between the positive charge of the nuclei and the negative charge of the electrons. The first molecule of H-Cl has a bond order of 1, a single bond. The
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Atoms, Molecules and Ions. AN ATOM is the smallest particle of an element. They cannot be split into smaller particles in chemical reactions. Iron is made of iron atoms (Fe). Sulphur is made of sulphur atoms (S) A MOLECULE is a small group of atoms joined together. The atoms may be the same (e.g. O2) or different (e.g. H2O). The chemical formula shows the number and type of atoms present. Non-metal compounds are made of molecules: Carbon dioxide contains CO2 molecules Methane (natural gas)
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polarities Drawing Lewis structure and calculate the formal charge Forms of Chemical Bonds 1) Intramolecular bond – forces hold the atoms _______ a molecule • Ionic / Electrovalent Bond • Covalent Bond • Metallic Bond 2) Intermolecular bond – forces ________ the molecules • Hydrogen bonding • Van der Waals 3) Co-ordinate / Dative Bond FHSC1114 Physical Chemistry Chapter Scopes • • • • Electrovalent / ionic bonding Covalent bonding Co-ordinate / dative covalent bonding Intermolecular
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