Ionic bonds form a giant lattice structure Sodium chloride is an ionic compound formed by the reaction between the metal sodium and the nonmetal chlorine During the reaction one electron is transferred from each sodium atom to each chlorine atom ID: 1043691
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3. Ionic bonding(metal + non-metal)Ionic bonds form a giant lattice structure
4. Sodium chloride is an ionic compound formed by the reaction between the metal sodium and the non-metal chlorine.During the reaction, one electron is transferred from each sodium atom to each chlorine atom.sodiumNachlorineClsodium chlorideNaCl+Sodium chloride
5. Sodium chlorideClNaNaSodium has 1 electron in its outer shell. If it loses this electron, it will have no partially-filled shells.Chlorine has 7 electrons in its outer shell. If it gains 1 electron, it will completely fill its outer shell.2.8.12.8.7[2.8]+[2.8.8]-Cl+-
6. Sodium chlorideThe positive sodium ions and the negative chloride ions are strongly attracted to each other and form an ionic bond.Na+Cl-
7. Lithium OxideLi2.1[2]+LiO2.6[2.8]2-2-Li+Li+O
8. Magnesium fluorideMg2.8.2[2.8]2+F2.7[2.8]-FMgFF2+--
9. Magnesium OxideExplain how magnesium oxide is formed.Magnesium loses 2 electronsOxygen gains 2 electronMagnesium becomes 2+ ionOxygen becomes 2- ionHeld to together in ionic lattice
10. Calcium chloride - CaCl2Explain how CaCl2 is formed:Calcium loses 2 electronsEach chlorine atom gains 1 electronTwo chlorine atoms neededForms ionic bond
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14. Covalent bonding(non-metal + non-metal)Simple moleculesGiant covalent structures
15. HYDROGENH H Another hydrogen atom also needs one electron to complete its outer shell Hydrogen atom needs one electron to complete its outer shell atoms share a pair of electrons to form a single covalent bondA hydrogen MOLECULE is formedH HHHWAYS TO REPRESENT THE MOLECULESimple molecules
16. HYDROGEN CHLORIDEClHHydrogen atom also needs one electron to complete its outer shell Chlorine atom needs one electron to complete its outer shell atoms share a pair of electrons to form a single covalent bondH Cl H ClWAYS TO REPRESENT THE MOLECULESimple molecules
17. AMMONIANEach hydrogen atom needs one electron to complete its outer shell Nitrogen atom needs 3 electrons to complete its outer shell Nitrogen can only share 3 of its 5 electrons otherwise it will exceed the maximum of 8A LONE PAIR REMAINSHHHH N HHH N HHWAYS TO REPRESENTTHE MOLECULESimple molecules
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19. Covalent bonding - moleculesHydrogen - H2 (g)Oxygen - O2 (g)Chlorine - Cl2 (g)Methane – CH4 (g)Hydrogen chlorideHCl (g)Water – H2O (l)Ammonia – NH3 (g)
20. Limitations of using models – doesn’t show the shape
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24. In a metal the atoms LOSE SEVERAL OF THEIR OUTER ELECTRONS which drift around between the metal ions as FREE ELECTRONS.Atoms become POSITIVE ions because they have LOST electronsFree (“delocalised”) electrons
25. Metals have a structure of positive metal ions held together by a “sea” of electrons – causes electrostatic attractionWe call these electrons delocalized Ions are arranged in layersForms a giant lattice structureMetallic bonding
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30. Predicting states using melting and boiling pointsSubstanceMelting Point (˚C)Boiling Point (˚C)State at room temperatureWater099.98LiquidCarbon Dioxide-78-57GasMethane-182-164GasHydrogen-259.1-252.8GasAmmonia-77.73-33.34GasSolidLiquidGasMelting pointBoiling point
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32. State Symbols(s) – solid(l) – liquid(g) – gas(aq) – dissolved in waterNaOH (aq) → Na+ (aq) + OH– (aq)
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34. High Melting point – lots of ENERGY needed to break the strong bonds (strong electrostatic attraction)Solubility - Can dissolve in water which enables the ions to moveConduction - When MOLTEN or DISSOLVED IN WATER, ionic compounds can conduct electricity because the ions can carry current/charge (not electricity)Properties of ionic compounds – giant lattices
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41. Covalent bonding – simple moleculesHydrogen - H2 (g)Oxygen - O2 (g)Chlorine - Cl2 (g)Methane – CH4 (g)Hydrogen chlorideHCl (g)Water – H2O (l)Ammonia – NH3 (g)Properties of covalent compoundsA covalent bond is a shared pair of electronsSubstances that consist of simple molecules are gases, liquids or solids that have relatively low melting points and boiling points due to weak intermolecular bondsThey do not conduct electricity because the molecules do not have an overall electric charge. No free electrons or ions.
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47. Molecules are linked with strong covalent bondsIntermolecular forces between polymers are relatively strongPolymers are usually solid at room temperaturePolymers
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50. Carbon structures - diamondDiamondDiamond is made only from carbon atoms.Every carbon makes four covalent bonds to achieve a full outer shell.Every carbon atom is bonded to four other carbon atoms.This means the structure keeps on growing!We make a Giant Covalent Structure.Giant covalent structure of diamondKey properties – Diamond is very hard.High melting points – because it has strong covalent bonds (which take a lot of energy to break)
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52. Carbon structures - graphiteGraphiteGraphite is made only from carbon atoms.Every carbon makes 3 covalent bonds to achieve a full outer shell.Forms hexagonal rings, arranged in layersWeak intermolecular forces between the layersEvery carbon atom is bonded to three other carbon atomsGiant covalent structure of graphiteKey properties – Graphite is very soft.Slippery – arranged in layersHigh melting pointConducts electricity – free electrons
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61. Conducts electricity and heatDelocalised electrons can move through the structureMalleableIons arranged in layers so ions are able to slide over each otherHigh melting and boiling pointsIons held together by strong electrostatic attraction so needs a lot of energy to break the bondsMetallic bonding – giant structures
62. Metallic bonding - alloysAlloys Mixture of metals of different sizes.Distorts the layers Layers can’t slide
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70. Besides graphite and diamond, carbon can also form another type of giant covalent structure. Fullerenes (named after the scientists that discovered them) are made by conjoined hexagonal carbon ringsCovalent bonding - GiantPossible uses of Fullerenes in the future could be:Drug deliveryIn lubricantsAs catalysts in reactionsTo make carbon nanotubes to reinforce structures
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72. Nano particlesStructures that are 1-100nm in size, or of the order of a few hundred atomsParticle nameSymbol Diameter (nm)Diameter (m)Nano particleSmaller than PM2.5100 – 2500 nm1 x 10-7m – 2.5 x 10-6 mCoarse particlePM102500nm – 10 000 nm2.5 x 10-6 m – 1 x 10-5 m
73. Nano particles
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75. NanoparticlesAdvantagesDisadvantagesLarge surface area makes them effective catalysts.Nanotubes can be used in small scale circuits as nanowires.So small they can enter the skin and therefore the bloodstream.Easily become airborne, breathing in can potentially damage the lungs.Nanoparticles are present in sun screensMay be used to develop faster computers, lighter construction materials and new coatings
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