Chemical Bonding Chemical compounds are formed by the joining of two or more atoms. A stable compound occurs when the total energy of the combination has lower energy than the separated atoms. The bound state implies a net attractive force between the atoms ... a chemical bond. The two extreme cases of chemical bonds are: Covalent Bonds Covalent chemical bonds involve the sharing of a pair of valence electrons by two atoms‚ in contrast to the transfer of electrons in ionic bonds. Such bonds lead
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INTRODUCTION TO CHEMICAL BONDS CHEMICAL BOND Definition: A chemical bond is defined as a force that acts between two or more atoms to hold them together as a stable molecule. Main types of bond: 1. Ionic or electrovalent bond‚ 2. Covalent bond‚ 3. Coordinate covalent bond Forth type of bond: Metallic bond: The type of bonding which holds the atoms together in metal crystal. Valence electron: The electrons in the outer most energy level in an atom that takes part in chemical
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molecules cannot form hydrogen bonds with each other and therefor result in a much lower boiling point than alcohols. 76) Is this statement true or false? “As the electronegativity difference between covalently bonded atoms increases‚ the strength of the bond increases.” There is no particular pattern between electronegativity difference and bond strength. Standardized Test Prep 1) A bond in which two atoms share a pair of electrons is not: c) an ionic bond 2) How many valence electrons
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Grade 10 Science –Chemistry Ionic Compounds Science Perspectives 10 - Section 5.6 Pages 192-195 Compound • A Pure Substance composed of two or more elements in a FIXED RATIO Ionic Compound • A compound made up of one or more positive metal ions (cations) and one or more negative non-metal ions (anions) Ionic Bond • The simultaneous strong attraction of positive and negative ions in an ionic compound. As noted‚ ionic bonding occurs between metals and non-metals. Yet‚ “why
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Shapes of molecules • Covalent molecules with non-octet structures • Shapes of molecules • The VSEPR theory • Molecular crystals of buckminsterfullerene (C60) • Carbon nanotubes Bond polarity and intermolecular forces • Electronegativity and bond polarity • Van der Waals’ forces • Factors affecting the strength of van der Waals’ forces • Hydrogen bonding • Surface tension and viscosity of liquids Topic 6 Microscopic World II Unit 23 Shapes
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Metals and alloys. Hume-Rothery rules. 1. Three types of metals. 2. Alloys. Hume-Rothery rules. 3. Electrical resistance of metallic alloys. 4. Applications of metallic alloys. 5. Steels. Super alloys. 6. Electromigration in thin wires. Three types of metals Metals share common features that define them as a separate class of materials: • Good thermal and electrical conductors (Why?). • Electrical resistance increases with temperature (Why?). • Specific heat grows linearly with temperature
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Topic 5 – Bonding and Structure Revision Notes 1) Introduction • Atoms form bonds to get a full outer shell of electrons • There are three types of bonding: ionic‚ covalent and metallic • The structures produced by forming bonds are either giant or simple • The possible combinations of structure and bonding are giant ionic‚ simple covalent‚ giant covalent and giant metallic • Simple covalent is sometimes called simple molecular • Giant covalent is sometimes called giant
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separate steps resulting in anti-addition. The reagent for halogenation by addition is usually bromine (liquid) or sometimes chlorine (gas). Fluorine is too reactive due to its high electronegativity and small radius. Iodine would react by reversible addition‚ as the low reactivity is due to its lower electronegativity and large size‚ making it a weak
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Chemistry SCH4U-B Lesson 1 Key Questions 1. The development of MRI imaging technology is one useful spinoff of basic research into the structure of the atom. Research‚ however‚ is expensive. Many people argue that the high cost of research outweighs its potential benefits. Provide one argument for‚ and one argument against increasing current
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their reactivity by losing their electrons‚ the increased first ionisation energy across the period does not allow for this‚ and so metals are located at the start of the period where the first ionisation energy is lower. In addition‚ the higher electronegativity towards the end of the period corresponds with the non-metals‚ due to their increased ability to attract and gain electrons to complete their outer shell. As you move across the period‚ the Period 3 elements’ reactivities with water decreases
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