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Alcohol | Introduction | Organic Chemistry | B.Sc. 2nd year | 3rd SEM. | Lecture - 3
Alcohol | Introduction | Organic Chemistry | B.Sc. 2nd year | 3rd SEM. | Lecture - 1
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Alcohol | Introduction | Organic Chemistry | B.Sc. 2nd year | 3rd SEM. | Lecture - 2
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00:00- Physical Properties Of Monohydric Alcohols
00:50- Nature Of Monohydric Alcohol
01:05- Structure Of Monohydric Alcohol
02:02- Associated Molecule state Of Monohydric Alcohols
04:00- Boiling Point Of Monohydric Alcohols
04:53- Solubility Of Monohydric Alcohols
06:58- Chemical Properties Of Monohydric Alcohols
07:45- Cleavage Of O-H Bond
17:10- Relative Reactivities Of Alcohol and Acids
Physical Properties of Alcohol
1. The Boiling Point of Alcohols
Alcohols generally have higher boiling points in comparison to other hydrocarbons having equal molecular masses. This is due to the presence of intermolecular hydrogen bonding between hydroxyl groups of alcohol molecules. In general, the boiling point of alcohols increases with an increase in the number of carbon atoms in the aliphatic carbon chain. On the other hand, the boiling point decreases with an increase in branching in aliphatic carbon chains the Van der Waals forces decreases with a decrease in surface area. Thus primary alcohols have a higher boiling point.
2. Solubility of Alcohols
The solubility of alcohol in water is governed by the hydroxyl group present. The hydroxyl group in alcohol is involved in the formation of intermolecular hydrogen bonding. Thus, hydrogen bonds are formed between water and alcohol molecules which make alcohol soluble in water. However, the alkyl group attached to the hydroxyl group is hydrophobic in nature. Thus, the solubility of alcohol decreases with the increase in the size of the alkyl group.
3. The Acidity of Alcohols
Alcohols react with active metals such as sodium, potassium etc. to form the corresponding alkoxide. These reactions of alcohols indicate their acidic nature. The acidic nature of alcohol is due to the polarity of –OH bond. The acidity of alcohols decreases when an electron-donating group is attached to the hydroxyl group as it increases the electron density on the oxygen atom. Thus, primary alcohols are generally more acidic than secondary and tertiary alcohols. Due to the presence of unshared electrons on the oxygen atom, alcohols act as Bronsted bases too.
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Basic Ideas Of Statistical Physics || INTRODUCTION || B. Sc. 2nd year || 3rd Sem. || Lecture - 1
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p - block elements || Introduction || Lecture - 1 || Inorganic Chemistr
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Modern Algebra Group Theory Part 2 #shorts
Modern Algebra Group Theory Part 2 Full Lecture = https://youtu.be/G-_bnP4Y8A0
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Nuclear and Particle Physics - 1 | Lecture-02 | B.Sc.5th SEM.
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p-block elements || General Characteristics of Group 13 Elements || B.Sc. 2nd sem. || Lecture - 2
p - block elements || Introduction || Lecture - 1 || Inorganic Chemistry | B. Sc. 1st year||2nd Sem.
This is General Introduction of P-Block Elements.
There are six groups of p–block elements in the periodic table numbering from 13 to 18. Boron, carbon, nitrogen, oxygen, fluorine and helium head the groups. Their valence shell electronic configuration is ns2np1.Boron in available limited quantities. Aluminium is readily available on our planet. It is the third most abundant element available. P-block metals have classic metal characteristics: they are shiny, they are good conductors of heat and electricity, and they lose electrons easily. Generally, these metals have high melting points and readily react with nonmetals to form ionic compounds.While moving down the group, atomic radius of elements increases. In Boron family, Atomic radius of Ga is less than AI.This is due to the variation of inner core of electronic configuration. The ionisation enthalpy decreases from top to bottom, but, in case of, Boron family, there is an increase and decrease in ionisation energies from Al to Tl. Because d and f electrons have low shielding effect. Electronegativity decreases from B to Al and then it increases this is because of difference in atomic size of elements. The outer electronic configuration of group 13 elements in ns2np1. So,oxidation state is +3. Boron and Aluminium shows oxidation state of +3 whereas, other elements of the group shows oxidation state of +3 and +1. But+1 is most stable oxidation state. Boron family reacts with halogens to form trihalides. Boron does not react with air.
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Condensed Matter Physics || Face Centred Cubic Unit Cell || Lecture - 5 || B.Sc. Tech
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Alcohol | Introduction | Organic Chemistry | B.Sc. 2nd year | 3rd SEM. | Lecture - 5
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Alcohol | Introduction | Organic Chemistry | B.Sc. 2nd year | 3rd SEM. | Lecture - 1
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Chemical Properties of Alcohols
Alcohols exhibit a wide range of spontaneous chemical reactions due to the cleavage of the C-O bond and O-H bond. Some prominent chemical reactions of alcohols are:
1. Oxidation of Alcohol
Alcohols undergo oxidation in the presence of an oxidizing agent to produce aldehydes and ketones which upon further oxidation give carboxylic acids.
Dehydration of Alcohol
Upon treatment with protic acids, alcohols undergo dehydration (removal of a molecule of water) to form alkenes.
Alcohol upon reaction with protic acids tends to lose a molecule of water to form alkenes. These reactions are known as dehydrogenation or dehydration of alcohol.
It is an example of an elimination reaction. Its rate varies for primary, secondary, and tertiary alcohols. This variation of rate can be attributed to the stability of carbocation generated. Since the carbocation is most stable in the case of tertiary alcohols, the rate of dehydration is highest for tertiary alcohols in comparison to secondary and primary alcohols
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p - block elements || Introduction || Lecture - 1 || Inorganic Chemistry | B. Sc. 1st year||2nd Sem.
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p-block elements || General Characteristics of Group 13 Elements, || B.Sc. 2nd sem. || Lecture - 2
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Alcohol | Introduction | Organic Chemistry | B.Sc. 2nd year | 3rd SEM. | Lecture - 1,Alcohols Organic Chemistry, Alcohol
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