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IB Chemistry:Topic 10: Organic Chemistry

IB Chemistry: Topic 10: Organic Chemistry Hydrocarbons and an Introduction to Halogenoalkanes CONTENTS General Information Aliphatic Hydrocarbons o Alkanes o Alkenes o Alkynes o  Cyclic Forms Aromatic Hydrocarbons Introduction to Halogenoalkanes GENERAL INFORMATION As...

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10.6 – Reaction Pathways

10.6 - Reaction Pathways The different reactions that are possible for organic compounds are explained in more detail in previous sections. Some are outlined in this section too. It is important to be able to manipulate the reactions and create combinations that will...

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10.5 – Halogenoalkanes

10.5 - Halogenoalkanes     The halogens are the seventh group on the periodic table, including elements such as fluorine, chlorine, bromine and iodine. Halogenoalkanes have a halogen bonded to the skeleton of the alkane. They have the general formula: Where...

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10.4 – Alcohols

10.4 - Alcohols Alcohols have the general formula: 10.4.1 - Describe, using equations, the complete combustion of alcohols Alcohols will not affect the pH of a solution as they do not behave as bases and are weaker acids than water. Alcohols are useful fuels because...

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10.3 – Alkenes

10.3 – Alkenes 10.3.1 - Describe, using equations, the reactions of alkenes with hydrogen and halogens Alkenes undergo addition reactions. This is when two substances react to form a single substance. Alkenes are more reactive that alkanes, as the double bond can be...

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10.2 – Alkanes

10.2 – Alkanes 10.2.1 - Explain the low reactivity of alkanes in terms of bond enthalpies and bond polarity Alkanes are saturated hydrocarbons. They are non-polar molecules, so they are insoluble in water, along with being less dense that water. In their pure form,...

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10.1 – Introduction to Organic Chemistry

10.1 – Introduction to Organic Chemistry 10.1.1 - Describe the features of a homologous series Compounds of carbon that are in a homologous series have common characteristics. One of these is that they are all hydrocarbons, meaning that they are made up of carbon and...

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9.5 – Electrolytic Cells

9.5 – Electrolytic Cells Electrolysis is used to isolate highly reactive metals, such as sodium and potassium, which would not react in a voltaic cell, but require electrical energy for the reaction to occur. The reactions taking place here are non-spontaneous. 9.5.1...

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9.3 – Reactivity

9.3 – Reactivity 9.3.1 - Deduce a reactivity series based on the chemical behaviour of a groups of oxidising and reducing agents When a metal is replaced by another metal in a compound, this is called a metal displacement reaction. For this to occur, the metal in the...

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9.4 – Voltaic Cells

9.4 – Voltaic Cells 9.4.1 - Explain how a redox reaction is used to produce electricity in a voltaic cell In a half-cell, a metal electrode is placed in an aqueous solution of its ions. Two half cells are connected to form a voltaic cell, allowing electrons to flow...

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9.2 – Redox Equations

9.2 – Redox Equations 9.2.1 - Deduce simple oxidation and reduction half-equations given the species involved in a redox reaction   The half equations break up the whole equation to show what is happening with each element or molecule. Since one element or...

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9.1 – Introduction to Oxidation and Reduction

9.1 – Introduction to Oxidation and Reduction 9.1.1 - Define oxidation and reduction in terms of electron loss and gain Oxidation – The loss of electrons from a substance. This may happen through the gain of oxygen or loss of hydrogen Reduction – The gain of...

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The Position of Equilibrium

Deduce the equilibrium constant expression (Kc) from the equation for a homogeneous reaction  A homogenous reaction is when the reactants and the products are all in the same state. The equilibrium law shows that the concentration of reactants and products have a...

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Dynamic Equilibrium

Outline the characteristics of chemical and physical systems in a state of equilibrium Open system – When a reaction occurs in an unsealed container Closed system – When a reaction occurs in a sealed container, and it is possible to reach equilibrium. When a reaction...

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Collision Theory

Collision Theory Describe the kinetic theory in terms of the movement of particles whose average energy is proportional to temperature in Kelvin  All particles – whether they are in a liquid, gaseous or solid state – move in some way. These types include vibration,...

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Rates of Reaction

Rates of Reaction Define the term rate of reaction  The change in concentration of reactants or products with time. In other words, how quickly the reactants are converted into products. These are expressed in mol dm-3 s-1. If you substitute products in here, then the...

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Bond Enthalpies

Bond Enthalpies Define the term average bond enthalpy  Average Bond Enthalpy - The amount of energy required to break one mole of bonds in the gaseous state averaged across a range of compounds containing that bond. For example, in determining the bond enthalpy of...

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Hess’s Law

Hess’s Law Determine the enthalpy change of a reaction that is the sum of two or three reaction with known enthalpy changes The energy difference between two states is independent of the route between them e. The heat evolved or absorbed in a chemical process is the...

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Calculation of Enthalpy Changes

Calculation of Enthalpy Changes Calculate the heat energy change when the temperature of a pure substance is changed Specific Heat Capacity – Symbol c – The amount of heat energy required to raise the temperature of 1.00g of the substance by 1.00°C or 1.00K The...

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Exothermic and Endothermic Reactions

Exothermic and Endothermic Reactions Define the terms exothermic reaction, endothermic reaction and standard enthalpy change of reaction  Exothermic Reaction - A reaction that causes the temperature of the surroundings to increase. Energy is lost, or released, in the...

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Physical Properties

Physical Properties Compare and explain the properties of substances resulting from different types of bonding Type of bonding Ionic Metallic Covalent molecular Covalent network lattice Melting and boiling point Very high Medium to high Low Very high Why Packed...

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Metallic Bonding

Describe the metallic bonds as the electrostatic attraction between a lattice of positive ions and delocalised electrons Metals form a 3D lattice of cations surrounded by a 'sea' of delocalised electrons. Only the valence electrons become delocalised. The electrons in...

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Intermolecular Forces

Intermolecular Forces   4.3.1  - Describe the types of intermolecular forces (attractions between molecules that have temporary dipoles or hydrogen bonding) and explain how they arise from the structural features of molecules Intermolecular forces are the bonds...

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Covalent Bonding

Covalent Bonding   Describe the covalent bond as the electrostatic attraction between a pair of electrons and positively-charged nuclei Outer shell electrons interact and rearrange themselves into a more stable arrangement that has lower chemical energy. The...

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Ionic Bonding

Describe the ionic bond as the electrostatic attraction between oppositely charged ions Ions are formed when electrons are transferred from a metal atom to a non-metal atom in order to produce a full outer shell for both ions. The metal will have a positive charge,...

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The Periodic Table

- The Periodic Table 3.1.1  - Describe the arrangement of elements in the periodic table in order of increasing atomic number Elements in the periodic table are arranged in order of increasing atomic number (Z). There is a division between metals and non-metals....

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Electron Arrangement

Electron Arrangement Describe the electromagnetic spectrum Light consists of electromagnetic waves. Electromagnetic waves can travel through space or matter. A wavelength is the distance between two successive crests. The velocity of travel, c, is related to its...

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The Mass Spectrometer

The Mass Spectrometer Describe and explain the operation of a mass spectrometer Mass spectrometers are very complex, and are made up of a number of components, each of which performs a particular function. The principle behind it is that the movement of charged...

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The Atom

The Atom State the position of protons, neutrons and electrons in the atom Atoms are made up of a nucleus containing positively charged protons and neutral neutrons, with negatively charged electrons moving around the nucleus in shells. State the relative masses and...

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Solutions

Solutions   Distinguish between the terms solute, solvent, solution and concentration (g dm-3 and mol dm-3)   Solute - This is the substance which has been dissolved.   Solvent - The bulk substance in which the solute was dissolved   Solution - This is made...

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Chemical Equations

Chemical Equations Deduce chemical equations when all the reactants and products are given Chemical formulas are shorthand representations of compounds. Chemical reactions are represented by equations using the chemical formulas and symbols of the substances involved...

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Formulas

Formulas  Define the terms relative atomic mass (Ar) and relative molecular mass (Mr)   Relative Atomic Mass (Ar) - The weighted mean of the masses of the naturally occurring isotopes, on a scale in which the mass of an atom of the carbon-12 isotope is 12 units...

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The Mole

The Mole Apply the mole concept to substances A mole is the name given to a certain quantity. It represents 6.02 x 1023 particles. This number is also known as Avogadro's constant, symbolised L. L = 6.02 x 1023 mol-1 To apply this concept to substances, we use it like...

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