SHAPES AND MOLE3
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| TO DRAW OCTAHEDARL | ONE LINE GOING UP AND DOWN, 2 WEDGES AT BOTTOM 2 DOTTED LINES UPWARDS. METAL IONS ARE HYDRATED ... WITH OXYGEN OF SIX WATER MOLECULES DATIVE BONDED TO THE CENTRAL ATOM. THESE IONS ARE OCTAHEDRAL .E.G. [CR(H20)6]3+ AND [MG(H2O)6]2+.
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| SUMMARY | WORK OUT THE NUMBER OF LONE AND SIGMA BONDS AROUND CENTRAL ATOMS. GIVES ARRANGEMENT OF ELECTRONS.
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| REPULSION OF THE BONDS PAIRS AND LONE PAIRS | REDUCES THE BOND ANGLE.
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| POLARITY IN H2 AND CL2 – THE AVERAGE POSITION OF BONDING ELECTRONS IS | HALFWAY BETWEEN THE CENTRES
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| BUT IN BONDS OF ATOM OF DOFF ELEMENTS |
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| (HF H20) IN HF | THE ELECTRON CLOSER TO F BECAUSE MORE ELECTRONEGATIVE.
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| ELECTRONEGATIVE IS THE ABILITY | OF AN ELEMENT TO ATTRACT A PAIR OF ELECTRONS IN A COVALENT BOND AND WITHDRAWN ELECTRON DENSITY.
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| IN P TABLE THE ELECTRONEGATIVITY | INCREASE ACROSS PERIOD DECREASES DOWN A GROUP. BUT OXYGEN HAS 2ND HIGHEST ELECTRONEGATIVITY.
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| WHEN 2 COVALENTLY BONDED ELEMENT HAVE DIFF ELECTRONEGATIVITIES | ON HAS SLIGHT POS AND NEG, THEY ARE POLAR.
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| THE BOND ELECTRONS DRAWN TOWARDS | THE MORE ELECTRONEGATIVE ELEMENT MAKING IT NEGATIVE.
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| COVALENT BOND | POLAR 100%,
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| IF HIGH DIFFERENCE IN ELECTRONEGATIVITY | THEN IONIC.
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| SHAPE AND POLARITY BONDS IN CH3CL AND CCL4 | ARE POLAR.
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| THE CH3CL IS POLAR BECAUSE | THE C-CL POLARITY IS NO CANCELLED OUT.
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| BUT CCL4 IS NOT POLAR BECAUSE | THE POLARITIES IN EACH C-CL BONDS CANCEL OUT AS SYMMETRICAL.
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| IS NH3 POLAR | NO, HAS 3 POLAR BONDS AND A LONE PAIR DO NOT CANCEL SO IS POLAR.
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| TRIGONAL PLANAR MOLE SO3, BECL3 ARE | NON POLAR COZ POLARITIES DON’T CANCEL.
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| H20 IS V SHAPED (POLAR) | POLARITIES DON’T CANCEL.
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| CO2 IS LINEAR & | THE POLARITIES CANCEL.
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| TO TEST FOR POLAR CAN USE | WATER FROM BURETTE AND BALLOON WHICH HAS BEEN RUBBED ON WOOL – STATIC ELECTRICITY.
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| WILL THE POLAR MOLECULE BE ATTRACO THE BALOON ? WHY? | YES AND BEACAUSE OF STAIC ELECTRICITY
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| POLARITY OF A MOLECULE MEASURE BY | THE DIPOLE MOMENT
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| FOR A DIATOMIC ELEMENT – E.G HCL IS DEFINED BY | THE DIFFERENCE IN CHARGES X THE DISTANCE BETWEEN THE H & THE CL. FOR A POLYATOMIC ELEMENT MORE COMPLICATED.
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| POLARITY SHOWN AS | ARROW WITH PLUS AT ONE END
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| THE ARROW POINTS TO | THE NEGATIVE ATOM IN THE BOND.
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| 7 TYPES OF INTERACTION/INTERMOLECULAR ION BETWEEN | 2 IONS 250 KLMOL-1.
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| ATOM –ATOM INTERACTION IN A | COVALENT BOND 400.
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| PERMANENT DIPOLE DIPOLE- IS BTWEEN | POLAR MOLECULES 1.5 ,
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| INSTANTANEOUS INDUCED DIPOLE DIPOLE BETWEEN | ALL TYPES OF MOLECULES 1OKJMOL-1. ALKANES
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| HYDROGEN BONDING BETWEEN | HFON.20KJMOL-1.
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| ION ION BOND IS A | ELECTROSTATIC ATTRACTION BETWEEN POSITIVE AND NEGATIVE ION,
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| IN A ION ION BOND THE STRENGTH IS PROPORTION TO | THE PRODUCT OF IT CHARGES AND IN INVERSELY PROPORTIONALLY TO THE SUM OF THE IONIC RADII.
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| ATOMS BONDS ARE BETWEEN | ARE COVALENT BONDS
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| COVALENT BONDS IS AN | ATTRACTION OF 2 NUCLEI FOR THE SHARED ELECTRONS IN THE BOND,
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| SHORT BONDS ARE STRONGER | THAN LONG BONDS.
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| ION ELECTRON BONDS ARE BETWEEN | FORCES IN A METAL , SMALL METAL ION BOND MORE STRONGLY THAN LARGE,
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| MORE DELOCALISED ELECTRONS | THE STRONGER THE BOND.
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| ION WATER MOLECULES | WATER IS POLAR HAS POS AND NEG., THE NEG OXYGEN IS ATTRACTED T THE POS METAL ION AND H THE HYDROGEN ION ATTRACTED TO THE NEG METAL IONS.,
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| ONE OF THE LONE PAIRS OF ELECTRONS IN THE OXYGEN FORMS | A DATIVE COVALENT BOND WITH THE EMPTY ORBITAL IN A METAL CATION = HYDRATED ION.
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| FORCES BETWEEN COVALENTLY BONDED MOLECULES ARE | INTERMOLECULAR FORCES – PERMANENT DIPOLE DIPOLE , INSTANTANEOUS INDUCES DIPOLE FORCES, HYDROGEN BONDS.
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| PERMANENT DIPOLE DIPOLE - MOLECULES WITH PERMANENT DIPOLE CAN | ATTRACT NEIGHBOURING MOLECULES.
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| THE DIPOLE LINE UP SO THE POSITIVE END IS NEXT TO THE NEGATIVE END OF ANOTHER MOLECULE. = INTERMOLECULAR FORCES. |
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| POSITIVE END IS NEXT TO THE NEGATIVE END OF ANOTHER MOLECULE CALLED | INTERMOLECULAR FORCES
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| INSTANTANEOUS INDUCED DIPOLE DIPOLE FORCES DISPERSION /LONDON FORCES. THE ELECTRONS | CONSTANTLY MOVING AROUND ITS CAUSES TEMPORARY DIPOLE.
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