that were produced by specific metallic ions that are shown in a flame. This happens when an electron gains energy; the electron moves from an energy level that’s farthest away and to an empty orbital close to the nucleus with higher levels‚ so one of the electrons gives off energy. A flame test is a visual test where the energy is in the form of a color change and the change can be seen based off it. Therefore‚ different metals emit different color. When a metallic ion is heated in a flame test the
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bonds formed and the importance of the electron in the formation of these new bonds. Materials Boileezers (boiling chips) Desiccant 0.17M acetic acid (acidified water) Solution of Sodium thiosulfate Granular zinc Iodine crystals Zinc ion and iodine-iodide-triiodide ion in water Solid zinc iodide Mineral oil Silver nitrate Magnesium turnings 3M Hydrochloric acid (HCl) solution 2 boiling tubes 1 large tube (we used a small) Pipet Beakers (to hold tubes) Bunsen burner PART 1 Procedure Get a boiling
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groups‚ which are: • Metallic substances • Ionic compounds • Covalent molecular and; • Covalent network substances Metallic substances are substances that are made up of one or more metal. They have regular 3D lattice of positively charged ions. Metallic substances are bond together by metallic bond which has strong electrostatic attraction between the positive ions and the delocalised electrons. These delocalised electrons carry current giving metallic substance the ability to
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compounds of life) while all other compounds are called inorganic compounds. Classification of Compounds: A. Binary Compounds 1. Metal and Non-metal Inorganic compounds composed of just two elements‚ metal cations (positive ions) and non-metal anions (negative ions). These are referred to as metal-nonmetal binary compounds. There are two types of metals‚ some metals form cations with only one charge (e.g.Na+‚ K+) while other cations form
Free Periodic table Atom Chemistry
Contents IONIC BOND 2 METALLIC BOND 9 The "Sea of Electrons" Theory 14 Conductors‚ Insulators and Semiconductors 16 25 IONIC BOND Ionic bond is formed when electron transferred from a valence shell of an atom to the valence shell of another atom. Ionic bond involves electron transfer across two atoms. The atom which donates the electron is called cation which is a positive ion whereas the atom which gains the electron is called anion which is a negative ion. The opposite charge of
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Topic 4 - Bonding 4.1 Ionic bonds 4.1.1 Ionic bond: +ve (cations) and -ve (anions) ions are attracted to each other and form a continuous ionic lattice 4.1.2 Group 1 metals form +1 ions‚ group 2 metals form +2 ions‚ metals in group 3 form +3 ions . Examples : Li+‚ Mg2+‚ Al3+. Greater ease of ionisation Li->Cs is due to the increased electron shielding of the nuclear attraction caused by additional inner shells of electrons. The easier atoms are to ionise‚ the more reactive they
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Hestia Livana Partners : Rachel Gideon‚ Joy Boake‚ Hannah Harper Various Color of Light as the Effect of Electron Emission Objective Observe the characteristic colors produced by certain metallic ions when vaporized in a flame. Identify the unknown metallic ions by means of its flame tests. Background When atoms absorb energy‚ electrons move into higher energy levels‚ and these electrons lose energy by emitting light when they return to lower energy levels. Energy levels are fixed energies
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Subject Content Most of the objectives specified in this section relate to Knowledge with Understanding‚ although some indication has been given as to where the skills of Handling Information and Solving Problems may be developed. Teachers are reminded that‚ in the written papers‚ 40% of the marks are allocated to these higher ’thinking’ skills. In almost every section‚ students should therefore be given practice at dealing with unfamiliar situations so that these higher thinking skills can be developed
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oxide e.g. 4Na (S) + O2 (g) → Na2O (s) Reaction with hydrogen element + hydrogen → hydride e.g. Ca (s) + H2 (g) → CaH2 (s) Reaction between an oxide and water metallic oxide + water → hydroxide * metallic oxide is also known as “basic oxide” e.g. Na2O (s) + H2O (l) → 2NaOH (aq) non-metallic oxide + water → acid * non-metallic oxide is known as “acidic oxide” e.g. SO2 (g) + H2O (l) → H2SO3 (aq) Reaction between active metals and water active metal + water (liquid or gas) → hydroxide
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Bonding structure Metals: metallic bonding Ionic compound (metal +nonmetal): ionic bonding Molecule (nonmetal +nonmetal): covalent bonding 3.1 Metallic Bonding 1) Definition The electrostatic attraction between a lattice if positive ions and delocalized electrons. 2) The strength of metallic bonding (depend on) Delocalized electrons (=valence electrons=Group number) More valence electrons‚ stronger metallic bonding Ionic radii (=distance between nucleus and e-) Greater ionic radius
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