lattice of positive ions surrounded by a ‘sea’ of mobile delocalised valence electrons. • Metallic bonding is the electrostatic attraction between the delocalised electrons and the positive ions in the metallic lattice. Properties of metals: Property Explanation Relatively high density The particles are very close together. This is because of high electrostatic forces between the sea of valence electrons and the positively charged nucleus. Malleability and Ductility Because metallic bonding is non-directional-meaning
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Lecture 1: Introduction Geology - the study of the Earth‚ the processes that shape it‚ and the resources that could be obtained from it. Main branches Physical Geology - deals with the materials that comprise the Earth and the processes that affect it (e.g.‚ Volcanology‚ Seismology‚ Environmental Geology‚ Engineering Geology‚ Mining Geology‚ Petroleum Geology‚ Mineralogy‚ Petrology‚ Geomorphology‚ Geophysics‚ Geochemistry‚ Planetary Geology) Historical Geology - the study of the origin and
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CHAPTER 5: PERIODIC TABLE Development of the Periodic Table • i) Substance exist: naturally in elemental form Example: Gold‚ Uranium as unstable compound Example: Radioactive compounds as stable compound (majority) How to know whether a substance is a compound OR an element? ii) iii) • • • Grouping system: 1800: 31 elements identified 1865: 63 elements identified Audi Majdan – DMC 101 – KLIUC 1 • Dmitri Mendeleev: i) ii) iii) iv) Develop a system to group
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this table: Ionic Compound Ratio of ions in compound Sodium chloride Na+ : Cl1:1 Magnesium oxide Formula of compound Covalent MgO Ca2+: Cl1:2 CaCl2 Metallic Fill in this table of more complicated ions: Name of ion Formula of ion Calcium hydroxide‚ Ca(OH)2 hydroxide NO3CO32Suphate Example of compound Mg(NO3)2 Sodium carbonate CaSO4 KEY WORDS: Electronic structure Covalent bonding Ionic bonding Proton Electron Ion Giant structure (lattice) Metallic bonding ASSESSMENT: C2 REVISION
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properties: they are usually shiny (they have metallic luster)‚ have a high density‚ are ductile and malleable‚ usually have a high melting point‚ are usually hard‚ are usually a solid at room temperature and conduct electricity‚ heat and sound well. While there are several metals that are low density‚ soft‚ and have low melting points‚ these (the alkali and alkaline earth metals) are extremely reactive‚ and are rarely encountered in their elemental‚ metallic form. The electrical and thermal
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types of bonds are: I. Ionic Bonds III. Metallic Bonds II. Covalent Bonds IV. Intermolecular (van der Waals) forces Ionic Bonds The ionic bond is formed by the attraction between oppositely charged ions. Ionic bonds are formed between metals and nonmetals. Remember that metal atoms lose one or more valence electrons in order to achieve a stable electron arrangement. When a metal atom loses electrons it forms a positive ion or cation. When nonmetals react they gain one or more
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The purpose of this lab was to observe the spectral lines of different light sources (Iodine‚ hydrogen‚ helium‚ krypton‚ mercury‚ neon‚ and argon) and to find the wavelength‚ frequency‚ and energy of the emissions of vaporized metallic ions. First‚ we took spectroscopes to look at each light source. The iodine light source seemed coral to the naked eye. When observed with a spectroscope‚ it was clear that there were many red spectral lines followed by relatively similar quantities of orange‚ yellow
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AS Chemistry Revision-Chemistry for Life 1. Avagadro constant‚ 6.02 x 10²³ number of particles in 1 mole of a substance 2. Empirical formula-simplest ratio of atoms of each element in a compound 3. 4. Model of an atom Particle Mass on relative atomic scale Charge Proton 1 1+ Neutron 1 0 Electron Very small (0.00055) 1- 5. Radioactive isotopes Radiation What is it? Relative charge How does the nucleus change? Stopped by? Deflection in electric field? Alpha α Helium nuclei ⁴₂He +2 2 fewer
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Sydney Schell October 18th‚ 2012 Identifying Metallic Components Introduction: Spectroscopy is the study of the electromagnetic radiation emitted or absorbed by the atoms and molecules. A photon in short is light. Atoms produce light by putting energy in‚ the electron then becomes excited and goes up an energy level‚ the electron then falls back down to its ground state‚ and out comes a photon (light). The electromagnetic spectrum contains color that we can and cannot see. The color blue has
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Chapter 7 same number of valence electrons=behave similarly(chemical properties) ▪ neon gases (neon‚ argon) unreactive in chemical reactions(stable) ▪ Gilbert Lewis-octet rule(atoms tend to achieve electron configuration of gas) ▪ atoms of metallic atoms lose electrons‚ atoms of nonmetal atoms lose or share electrons with another nonmetal elements to achieve a complete octet ▪ to achieve octet‚ change electrons to ge ns2 np6 configuration ▪ remove electrons=ionization ▪ metals in group
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