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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. |