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SHAPES AND MOLE4
| Question | Answer |
|---|---|
| ELECTRONS IN NEIGHBOURS ALSO | OSCILLATE AND CAUSE TEMP DIPOLE WHEN POS END NEXT TO NEG END , |
| HOW ARE TEMP DIPOLE FORMED | ELECTRON CONSTANTLY MOVING POS AND NEG END HALF A SECOND LATER THE POLARITY CHANGES AND THE POS END INDUCED A NEGATIVE CHARGE ON A MOLECULE. |
| ZIGGY ARROW FOR | INTERMOLECULAR FORCES. |
| INSTANTANEOUS INDUCED DIPOLE DIPOLE ARE | STRONG AND THEN PERMANENT. |
| STRENGTH DEPEND ON NUMBER OF | ELECTRONS IN THE MOLECULE |
| WHY AT AT ROOM TEMP IODINE IS A SOLID CHLORINE A GAS | BECAUSE THE LONDON FORCES BETWEEN THE IODINE MOLECULES (106 ELECTRONS) IS STRONGER THAN THE CHLORINE (34 ELECTRONS). |
| THE LONDON FORCES BETWEEN H-CL MOLECULE STRONGER THAN METHANE AS | HAS MORE ELECTRONS. |
| THE STRENGTH INSTANTANEOUS INDUCE DIPOLE ALSO DEPENDS ON | SHAPE AND PINTS OF CONTACT E/.G C(CH3)4 HAS FEWER PINTS OF CONTACT THAN LARGER MOLECULES. |
| LONDON FORCES -EXIST BETWEEN | ALL COVALENT MOLECULES EVEN NOBLE GASSES, |
| THE BONDING TEMP OF NOBLE GAS VERY LOW | COZ NO BONDING ELECTRONS. |
| HYDROGEN IS | SMALLEST HAS NO SHIELDING ELECTRONS IS PARTIALLY EXPOSED NUCLEUS. |
| WHY CAN’T CHLORINE HYDROGEN BOIND? | CHLORINE ATOM IS TOO LARGE TO FORM A HYDROGEN BOND. ONLY SMALL FON-. |
| THE POS HYDROGEN FORMS BOND | WITH NEGATIVE ADJACENT FLUORINE MOLECULE. F-H-F BOND ANGLE 180 DEGREES. |
| THE H-F-H BOND ANGLE IS | 109.5 SO HAS ZIGZAG CHAIN. |
| ALL COMPOUND WITH –OH GROUP FORM | HYDROGEN BONDS .E.G WATER . |
| HYDROGEN BONDING IN WATER IS STRONG THAN H-F BECAUSE | THERE ARE MORE HYDROGEN BONDS PER MOLECULES IN WATER THAN H-F , BUT H-F IS VERY STRONG. |
| WATER BOILS AT | 100DEGREES CELSIUS, |
| H-F BOILS AT | 20 DEGREES CELSIUS. |
| WHAT DOES WATER BP SHOW | THE SUM OF INTERMOLECULAR FORCE IN WATER IS HIGHER. |
| SOLID WATER IS LESS | DENSE THAN LIQUID. – |
| WHY IS SOLID WATER LESS DENSE THAN WATER | BECAUSE ICE CRYSTALS CONTAIN INTERLOCKING RINGS OF SIX WATER MOLES HELD BY HYDROGEN BONDS. |
| WHAT ARE THE INTERLOCKING RINGS HELD BY | HYDROGEN BONDS |
| THE DISTANCE BETWEEN MOLECULES OPPOSITE IN ICE THE RING | IS LARGE. |
| WHEN ICE MELTS | THE RING STRUCTURE DESTROYED AND THE AVERAGE DISTANCE APART OF THE MOLECULES DECREASE CAUSING THE DENSITY TO INCREASES. |
| ALCOHOL HAS –OH GROUPS THUS | CAN FORM HYDROGEN BONDS WITH OTHER ALCOHOL OR WHEN DISSOLVE IN WATER WITH OTHER WATER MOLECULES. |
| HYDROGEN BONDING THROUGH NITROGEN WHEN NITROGEN FORMS 3 BONDS IT HAS | A LONE PAIR |
| IF BOND TO HYDROGEN NITROGE | BECOMES NEGATIVE. SO CAN FORM HYDROGEN BONDS . E.G. IN AMMONIA. |
| PRIMARY AMINE GROUPS –NH2 FORM | INTERMOLECULAR HYDROGEN BONDS E.G. GLYCINE (AMINO ACID). |
| WHAT ARE AMIINO ACIDS HELD BY IN PROTIENS | HELD BY HYDROGEN BONDS IN THE NH2 AND COOH GROUP. |
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ufuoma
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