Summary
Summary Chapter 6 - Shapes of Molecules
- Institution
- OCR
OCR CHEMISTRY A-LEVEL SHAPES OF MOLECULES SUMMARY.
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SHAp t s O f MO L E l U l E I iE L E L T RO N G E O M E T RY S HA P E N A ME BO ND EG
P A l RS ANGLE
2 BONDING LINEAR LINEAR 1800 tho
TRIGONALPLANARTRIGONALPINARILOBF
3BONDING
4 BONDING TETRAHEDRAL TETRAHEDRAL 109.50 Hy
Ha.on
g.on.ua ina.ona man.m mam
6 BONDING OCTAHEDRAL 90TOCTAHEDRAL
TETRAHEDRAL 3BONDINT
PYRAMIDICAL 107 NH
the
2 BONDING TETRAHEDRAL NON LINEAR 104.5 Belli
LIONEL
4 BONDING OCTAHEDRAL SQUARE PLANAR 90 Xefy
L LONT I I l
2 DO U B I E BO NDS L I N E A R
I TR I P I E I I S I NGL E L I N t A R
I DO U B L t t 2 S I NG L E T R l G ON A L P L A NA R
WHEN L ONE P A l R T A R E S P L Al E Of B O N D
P AI R BO ND A NG L E D E C R E A SE S B Y 2.50
R E P U L S l 0 N B E T W EE N LO N t B O ND I NG
G R E A T E R T H A N BO ND B O N D S 0 A N GL E
I N C R E A S t S B t T Wt E N P A l R t D E L R E A S t
B ET W E E N B O N D B O N D
T A K E S HA P E AS E L E C T RO N S R E P t L t A CH
O T H ER S O T A R E P O S I T I ON A S FA R A P A R T
A S P O S S I B L E W H E R E MU T U A L R E P U L S I ONS
Ml N I M I S t D
I N T E R MO L E C U L A R f O R C E S
3 T Y P E S O f A T T RAL T l O N i
H Y D R O G E N BO N D S
P E R MA N E N T D I P U L t D I P U L E I N T t RA l T l ON
I ND U L E D D I P U L t D I P U L E I N T E R A L T l O N S
D I P O l E MO L E C U l t l O R P A R T Of MO L E C V L E
W I T H PO S I T I V E t N EG A T l V t EN D
SAME A S POL A R
PE RMA NE N T D I P O L t OC C U R S W HE N 2 AT O MS
, N N OCCUR W N
S HAR I N G SET OF
ELECTRONS IN SINGLE
COVALENT BOND HAVE
SIGNIFICANTLY
DIFFERENT
ELECTRONEGATIVITY
ELECTRONEGATIVITY VA IVE GIVEN TO ATOM
WHICH SHOWS ABILITY
Of ATOM TO ATTRACT
PAIR Of ELECTRONS
IN COVALENT BOND
TOWARDS ITSELF
GENERAL TRENDS INELECTRONEGATIVITY
GROUP 7 MOST THE N b THEN 5
of LUORINE MOST ELECTRONEGATIVE ATUM
GROUPS I VERY 4 NOT
CARBON 1 HYDROGEN SIMILAR VALUES
NOT POL AR TO GET HER
PERMANENT DI PO LE DI POL E INTERACTIONS
WHEN MOLECULES THAT HAVE PERMANENT
DIPOLES COME TOGETHER THEY WILL
ARRANGE THEMSELVES SO VE AND t VE
ENDS O f MOLECULES ATTRACT ONE ANOTHER
MORE ELECTRONEGATIVE AT OM L
LESS ft
CAN BE
H
PO LARI NON POLAR
H
EG C POLAR
g H
PERMANENT DIPOLESAS VECTORS CANCELOUTeg.IO
g gNO
C DIRECTION Of CHARGE CANCEL
Cl NONPOLAR AS
OUT
Cl
INDUCED DIPOLE SMALL ELECTROSTATIC
ATTRACTIONS CAUSED BY
MOVEMENT Of ELECTRONS
WITHIN COVALENT BONDS
Of MOLECULES THAT WOULD
OTHERWISE HAVE NO
PERMANENT D I POL t
IND U C t D D I POL t DIPOLE INTERACTIONS
AS ONE MOLECULE APPROACHES ANOTHER
THE ELECTRONS Of 1 OR BOTH ARE
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