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CHEM

1) Dipole moments are caused by partial charges between polar atoms in a molecule. The net dipole moment is the sum of the vectors of individual dipole moments. 2) Hydrogen bonds are a special type of dipole-dipole interaction between hydrogen and highly electronegative atoms like nitrogen, oxygen, or fluorine. They influence properties like boiling point and solubility. 3) London dispersion forces are temporary dipole-dipole attractions between non-polar molecules caused by the random motion of electrons. They include van der Waals forces.

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18 views10 pages

CHEM

1) Dipole moments are caused by partial charges between polar atoms in a molecule. The net dipole moment is the sum of the vectors of individual dipole moments. 2) Hydrogen bonds are a special type of dipole-dipole interaction between hydrogen and highly electronegative atoms like nitrogen, oxygen, or fluorine. They influence properties like boiling point and solubility. 3) London dispersion forces are temporary dipole-dipole attractions between non-polar molecules caused by the random motion of electrons. They include van der Waals forces.

Uploaded by

mohamedgouda52008
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We take content rights seriously. If you suspect this is your content, claim it here.
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Dipole Moments and The net Dipole moment

The dipole bonds are from the partially positive to the partially
negative atoms ( that is the direction ) and its magnitude is the
difference between their polarity. The net Dipole moment is the
summation of the vectors of the dipole moments

The less negative part of the atom is PARTIALLY Positive and the
other part is partially negative

That difference of polarity between Polar atoms causes them to have


a DIPOLE DIPOLE INTERACTION as SHOWN IN THE FOLLOWING FEGURE

A special type of DIPOLE DIPOLE Bond is Hydrogen bond. it happens


when hydrogen makes a dipole dipole bonds with Nitrogen or Oxygen or
Fluorine. It increases the boiling point of the molecules and
increases its water souliabilty of that molcule. Water and amonia
are two examples AS SHWON IN THE FOLLLOWING FEGURE

London dispersion forces are forces that happens in non-polar


molcoules when electrons (Due to their random motion) Become
predominant in one side. That causes the atom to have one PARTIALLY
NEGATIVE and one PARTIALLY POSITIVE Sides. This can cause other
nearby atoms to become also charged that creates a temporary force
between the molcuols called a LONDON DISPERSION FORCES or VAN DER
WALLS INTERACRIONS. Those forces are shown in the following Figure
Polarity :
ion-ion > ion-dipole(ex: NaCl and H2O) > dipole-dipole (Hydrogen
bonds are strongest it's present in N O F) > Van Der Waals

Lewis Structure
Oxygen => 2 Bonds and 2 pairs Lone Electrons
Carbon => 4 Bonds
Nitrogen => 3 Bonds and 1 pair of lone Electrons
Hydrogen => 1 Bond
Whenever Atoms form Bonds that are less than the bonds they normally
form they carry a negative charge. And whenever Atoms from Bonds
more than they normally form, they carry a positive charge. as shown
in this FIGURE ⬇️

Organic Compounds
carbon and Hydrogen in them can be detected using Lassaigne’s Test

1. organic compounds are mixed with CuO


2. The mixture is then heated
3. when heated hydrogen reacts with CuO Producing Water vapor
4. The water vapor reacts with copper sulfate producing CuSO4.5H2O
which is the cause for the blue color
5. Carbon reacts with CuO producing carbon dioxide
6. carbon dioxide is then passed through lime water turning it milky
7. The following reactions are present
8.

9.

10.

Saturated hydrocarbons are organic compounds where every carbon


is singly bonded with a hydrogen (also known as Alkanes). that
single bond is really hard to break as it requires the energy of
ultraviolet rays

Angle between carbons in the chain is 109.5°


triple and double bonds between carbons are more easily broken

Alkanes

They have similar chemical properties and their physical


properties change gradually as shown in the following figure
Alkyels (are just Alkenes which have lost one electron)
Alkynes have the general formula CnH2n-2
Alkens have the general formula CnH2n
Alkanes have the general formula CnH2n+2
Alkyels have the general formula CnH2n+1
The number of Isomers for a given alkane is 2^(n-4) + 1 where n
is the number of carbons in a given chain
Isomers have the same molecular formula

sterio isomers have different 3D shape


enantiomers have opposite shapes
structrual isomers have different bonds
geometeric Isomers are shown in the above figure

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