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• Hydrocarbons

Unsaturated Hydrocarbons

What are unsaturated hydrocarbons.

Unsaturated hydrocarbons are organic compounds that are entirely made up of carbon and hydrogen atoms and consist of a double or a triple bond between two adjacent carbon atoms. For example, CH 3 CH 2 CH=CH 2 (n-Butylene) & CH 3 CH=CH 2 (Propylene) The difference in the chemical formulae of saturated and unsaturated hydrocarbons is illustrated below.

In the IUPAC nomenclature of unsaturated hydrocarbons, the position of the double or triple bond is either described by a number written before the name of the compound (as in 2,4 pentadiene) or by a number written before the suffix, ‘-ene’ or ‘-yne’ (as in pent-2-ene).

The physical properties of saturated hydrocarbons and unsaturated hydrocarbons are quite similar. These types of hydrocarbons (except aromatic hydrocarbons) are quite reactive and tend to undergo addition reactions with elemental halogens, hydrogen halides, alcohols, and many other compounds.

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Types of unsaturated hydrocarbons, uses of unsaturated hydrocarbons.

Unsaturated hydrocarbons , based on the types of bonds they contain, can be classified into alkenes, alkynes, and aromatic hydrocarbons. The different types of organic compounds that can be classified as unsaturated hydrocarbons are briefly discussed below.

• The hydrocarbons that contain at least one double bond between two adjacent carbon atoms are called alkenes or olefins. The simplest alkene is ethylene (or ethene), given by the chemical formula C 2 H 4 .
• Alkenes containing only one double bond and having no functional groups or substituents attached to them can be generalized to the chemical formula C n H 2n .
• Hydrocarbons containing a minimum of one triple bond between two carbon atoms that are positioned adjacent to each other are referred to as alkynes . The alkyne with the simplest structure is acetylene (systematic IUPAC name: ethyne) with the chemical formula C 2 H 2 .
• The alkynes that have only one carbon-carbon triple bond and have no functional or substituent groups attached to them can be generalized to the chemical formula C n H 2n-2
• Cyclic hydrocarbons that contain at least one double or triple bond between two carbon atoms are also considered to be unsaturated hydrocarbons, one such example being cyclopentene (C 5 H 8 ).
• Although Aromatic Hydrocarbons (ring-shaped hydrocarbons containing delocalised pi electrons) can be considered unsaturated hydrocarbons, but they are generally referred to as aromatic compounds because they are relatively stable and do not share similar properties with other such unsaturated compounds.

In order to check whether a given hydrocarbon is unsaturated, bromine water can be added to it. Should the bromine water become decolourised, the hydrocarbon in question is unsaturated. If a white precipitate is formed, the hydrocarbon sample is phenol or aniline. It can be noted that benzene does not decolourise the bromine water.

Some uses of compounds belonging to the unsaturated hydrocarbon category are listed below.

• Many fruits can be artificially ripened with the help of alkenes.
• Mustard gas, a poisonous gas used in chemical warfare, can be created with the help of alkenes.
• Unsaturated hydrocarbons are extremely useful organic compounds in the manufacturing of plastics.
• LDPE, which is a low-density variation of polyethylene, is used in the manufacturing of grocery bags
• Polystyrene is used in making egg cartons, disposable cups, and other convenient products.
• Industrial chemicals such as alcohol include the usage of alkenes in their manufacturing process.
• Some unsaturated hydrocarbons are used as general anaesthetics.
• Many organic compounds of high industrial importance are manufactured with the help of alkynes.

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Saturated and unsaturated compounds.

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• Unsaturated Hydrocarbons

Discover the intriguing world of unsaturated hydrocarbons through this comprehensive guide. Dive into a detailed explanation of what unsaturated hydrocarbons are and their unique attributes. Explore various types and examples, uncovering the diverse range and classifications of unsaturated hydrocarbons found in our world. You will then gain insight into the practical uses and applications of these substances in both everyday life and industrial contexts. Finally, learn about the vital chemical tests used to analyse these compounds and see how they compare with their saturated counterparts. This is a scientific journey not to be missed by those keen to deepen their chemistry knowledge.

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What is the significance of the term 'unsaturated' in unsaturated hydrocarbons?

How does the food industry utilise unsaturated hydrocarbons, particularly alkenes?

What difference can the bromine water test detect between saturated and unsaturated hydrocarbons?

What are the three common types of unsaturated hydrocarbons?

What is the key differentiation between saturated and unsaturated hydrocarbons?

What is the process of hydrogenation in the context of hydrocarbons?

Which unsaturated hydrocarbon is extensively used in the plastic production industry?

What are unsaturated hydrocarbons?

What are the two primary types of unsaturated hydrocarbons?

What distinctive features does benzene have as an aromatic hydrocarbon?

What role do unsaturated hydrocarbons, such as alkenes and aromatic hydrocarbons, play in vehicle fuels?

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Understanding Unsaturated Hydrocarbons

Unsaturated hydrocarbons are a significant topic that you ought to understand if you wish to excel in your Chemistry endeavours. Their presence is everywhere, from the fuel you use to power your automobiles to the plastic products that are integral parts of your daily life.

Defining Unsaturated Hydrocarbons: The Unsaturated Hydrocarbons Meaning

So, what exactly are Unsaturated Hydrocarbons?

An Unsaturated Hydrocarbon is a type of hydrocarbon that contains double or triple carbon-carbon bonds. This implies there are fewer hydrogen atoms attached to the carbon chain compared to saturated hydrocarbons.

Interestingly, the term 'Unsaturated' in Unsaturated Hydrocarbons indicates that if additional hydrogen is available, they can react to form a new compound, effectively becoming 'saturated'.

Unpacking the main components of Unsaturated Hydrocarbons

Unsaturated Hydrocarbons are generally composed of Carbon and Hydrogen atoms. However, it's the arrangement of these atoms, specifically the double and triple bonds between carbon atoms, that grant them their unique properties and reactivity. Here, we'll break down their structure into their fundamental components.

Carbon-Carbon Double Bonds: Alkenes are Unsaturated Hydrocarbons that contain at least one carbon-carbon double bond. This bond is denoted by the symbol '=' in chemical structures. For example, Ethene (\(C_2H_4\)) is the simplest alkene.

Carbon-Carbon Triple Bonds: Alkynes, another type of Unsaturated Hydrocarbons, contain at least one carbon-carbon triple bond. This bond is denoted by the symbol '≡' in chemical structures. An example of an alkyne is Ethyne (\(C_2H_2\)), commonly known as acetylene.

Now that you understand the basic components of Unsaturated Hydrocarbons, further study would lead to understanding their reactions, how they are represented in structural formulas, and their uses in various industries. This foundation will also help make later topics like isomers, polymerization, and substitutions easier for you to grasp.

Look around you, and you'll notice Unsaturated Hydrocarbons are all around. For instance, the ethylene gas (\(C_2H_4\)) used to hasten the ripening of fruits is an Alkene, an Unsaturated Hydrocarbon.

Different Types of Unsaturated Hydrocarbons: Examples

In the world of chemistry, unsaturated hydrocarbons are distinguished by double or triple bonds between the carbon atoms. The presence of these extra bonds imbues unsaturated hydrocarbons with their characteristic reactivity. Within this collection, there are three common types, namely, alkenes, alkynes, and aromatic hydrocarbons. Each presents unique properties and applications.

Exploration of diverse Unsaturated Hydrocarbons Examples

Unsaturated hydrocarbons play pivotal roles in many industries, as they are crucial for a myriad of reactions and processes. These hydrocarbons mainly fall into the categories of alkenes, alkynes, and aromatic hydrocarbons. Let's explore these in more detail.

Alkenes: These are a type of unsaturated hydrocarbon where carbon atoms are connected via at least one double bond. This bestows upon them a greater degree of reactivity compared to their saturated counterparts. Some everyday examples of alkenes include:

• Ethene (\(C_2H_4\)) – It's extensively used in the plastic production industry.
• Propene (\(C_3H_6\)) – It undergoes polymerisation to create polypropylene, a common type of plastic.

Alkynes: These unsaturated hydrocarbons stand out due to the presence of a triple bond between carbon atoms. The high energy associated with a triple bond conveys a high level of reactivity. Alkynes include compounds like:

• Ethyne (\(C_2H_2\)) – Famously known as acetylene, it's used for welding and metal cutting due to its ability to produce a very hot flame.
• Propyne (\(C_3H_4\)) – Less common than acetylene but used in organic synthesis.

Aromatic Hydrocarbons: Present as cyclic compounds with alternating double and single carbon-carbon bonds. Their stability and aromaticity make them a fascinating study. Examples include:

• Benzene (\(C_6H_6\)) – It's a starting material in the production of a vast number of chemicals including plastics, resins, synthetic fibres , rubber, dyes, detergents, pharmaceuticals, and explosives.
• Toluene (\(C_7H_8\)) – It serves as a solvent and a precursor to other chemical compounds.

Classification of Unsaturated Hydrocarbons

Differentiating between the various types of unsaturated hydrocarbons is essential to comprehending their unique properties and applications. Here, the classification is largely based on the number and nature of carbon-carbon bonds.

The simplest form of classification breaks down unsaturated hydrocarbons into the three following types:

• Alkenes: Contains at least one carbon-carbon double bond, denoted by a '=', in their molecular structure.
• Alkynes: Contains at least one carbon-carbon triple bond, represented by '≡' in chemical formulas.
• Aromatic Hydrocarbons: Formed by cyclic arrangements of carbon atoms, alternating between single and double bonds. This arrangement generates a distinctive ring-like pattern, granting them ' aromaticity ' or unique stability.

To fully appreciate the roles of these unsaturated hydrocarbons, you must delve into their chemical reactions and interactions, their physical and chemical properties, and, importantly, their significant industrial applications. Mastering these intricate details will undoubtedly make other areas of chemistry, such as organic synthesis, polymer chemistry, and even biochemistry, much easier to comprehend.

Practical Uses: Unsaturated Hydrocarbons Applications

Unsaturated hydrocarbons, owing to their reactivity and unique properties, find extensive use across diverse sectors. From the plastics sitting on your desk to the fuels that power your vehicle, you interact with products derived from these chemical compounds daily. Nonetheless, the study of unsaturated hydrocarbons isn't merely confined to academic intrigue — their practical applications are sweeping and transcend diverse sectors.

How we utilise Unsaturated Hydrocarbons: Applications in everyday life

Given the significance of unsaturated hydrocarbons, a broader understanding of their applications enriches your comprehension of how chemistry links with our everyday lives. Here, the emphasis will be on the practical applications of unsaturated hydrocarbons, demonstrating that their realm spans beyond textbooks and laboratory experiments.

For starters, consider the fuel being consumed by vehicles. Unsaturated hydrocarbons, especially aromatic hydrocarbons, play a crucial role as constituents of petrol and diesel. Some common examples include toulene and xylene . They are essential due to their energy content and the fact that they burn cleaner than their counterparts, contributing to fewer harmful emissions.

Unsaturated hydrocarbons also form the backbone of the plastic industry. The versatility of these compounds allows them to be manipulated into various forms, making them the ideal raw material for plastic production. For instance, polyethylene and polypropylene , two types of plastics ubiquitous in everyday life, originate from alkenes — a type of unsaturated hydrocarbon.

Furthermore, these hydrocarbons play an indispensable role in the synthesis of many industrial chemicals. Alkenes such as ethene and propene, for instance, serve as feedstock in the synthesis of a variety of chemicals including alcohols , alkyl halides , and detergents , thanks to their reactivity and accessibility.

Lastly, unsaturated hydrocarbons, particularly alkenes, feature prominently in the food industry. Ripening of fruits is stimulated by ethene (also known as ethylene ), a gas produced by some fruit species. The commercial cultivation of fruits exploits this characteristic, employing synthesized ethylene to hasten the ripening process, ensuring that fruits reach the market at their peak.

Industrial applications of Unsaturated Hydrocarbons

Delving further into the industrial domain, it becomes evident that unsaturated hydrocarbons are pivotal to manifold operations. Their intrinsic reactivity and ease of manipulation make them indispensable to a host of chemical processes.

The role of unsaturated hydrocarbons in the production of plastics is an example of their industrial significance. Consider, for example, polyvinyl chloride (PVC), a durable plastic derived from ethene (an alkene). PVC is widely used in the construction industry for products such as pipes, window frames, and roofing sheets due to its resistance to environmental elements.

Other alkenes, like propene, act as the foundation for the production of polypropylene , another common plastic. Its high tensile strength and resistance to chemical degradation make it suitable for a variety of applications, ranging from packaging materials to automotive parts.

In the realm of energy production, unsaturated hydrocarbons, particularly aromatic hydrocarbons like benzene, toluene, and xylene, are essential components of petrol . The high calorific values of these hydrocarbons make them ideal for use as fuel, emitting significant amounts of energy when burned.

Further, the reactivity of unsaturated hydrocarbons becomes a boon in the realm of chemical synthesis . Whether in creating dyes, detergents, or synthetic fibres , their use as feedstock is prolific.

Ultimately, the industrial applications of unsaturated hydrocarbons are as diverse as the compounds themselves. Whether it's serving as the backbone for polymeric materials, fuelling vehicles, or acting as a feedstock for countless industrial processes, their practical significance is vast and truly remarkable.

Analysing Unsaturated Hydrocarbons: The Chemical Test

A critical element in chemistry is confirming the identity of compounds, and unsaturated hydrocarbons are no exception. Since these molecules have double or triple bonds, they exhibit certain behaviour under specific conditions. As such, there are dedicated chemical tests to confirm the presence of unsaturated hydrocarbons in a compound, chiefly among these, the bromine water test.

Conducting a Chemical Test for Unsaturated Hydrocarbons

Unsaturated hydrocarbons, due to their unique features, undergo certain reactions that provide reliable confirmation of their existence. These tests play crucial roles in laboratories, industrial setups, and educational institutions where the identification of compounds is necessary.

An effective technique to detect the presence of unsaturated hydrocarbons is the bromine water test, also known as the bromine test. The premise of this test hinges on the reaction between bromine and unsaturated hydrocarbons. Unsaturated hydrocarbons, upon reacting with bromine water, will add bromine across their multiple bonds, thus decolourising bromine water's original brown colour.

To carry out this test, you introduce bromine water to the sample suspected of containing unsaturated hydrocarbons. On adding the bromine water – which is characteristically brown due to the presence of elemental bromine (Br 2 ) – the liquid should lose its colour if unsaturated hydrocarbons are present. This is because the double or triple bonds characteristic of unsaturated hydrocarbons will break and react with the bromine atoms, resulting in a halogenated compound and water.

The chemical equation for this reaction is:

\[ RCH=CH2 + Br2 -> RCHBr-CH2Br \]

Where \(RCH=CH2\) represents an alkene (an unsaturated hydrocarbon), \(Br2\) is bromine, and \(RCHBr-CH2Br\) is the halogenated compound formed.

In comparison, saturated hydrocarbons, which do not have these reactive sites (double or triple bonds), will not react with bromine water, and thus the brown colour of the bromine water will remain unchanged.

The bromine test is a striking example of a chemical test for unsaturated hydrocarbons due to its visual impact. The clear change – or lack thereof – delivers a powerful, understandable message even to individuals who might not have extensive chemical knowledge.

Understanding the outcomes of the chemical test for Unsaturated Hydrocarbons

Performing the bromine test presents two main outcomes that provide insight into the compound's nature. However, understanding the principals behind these results is fundamental for interpreting and applying this knowledge accurately.

If the sample contains unsaturated hydrocarbons, the bromine water will lose its brown colour upon addition of the sample. This occurs because the bromine atoms add across the double bond of the unsaturated hydrocarbon, breaking the multiple bonds, and forming a halogenated compound. As a result, the bromine molecules in the water diminish, thus eliminating the brown colour they lend to the water. The disappearance of the brown colour is evidence of the presence of unsaturated hydrocarbons in the mixture.

Alternatively, if the sample comprises saturated hydrocarbons, then the bromine water will retain its brown colour even after the addition of the sample. The absence of double or triple bonds in these compounds means they do not react with the bromine, leaving the bromine concentration in the water unchanged, and thereby maintaining its brown colour. This outcome, i.e., the persistent brown colour, signifies the absence of unsaturated hydrocarbons in the mixture.

While easy to conduct and interpret, it's necessary to consider the bromine test's limitations. This test does not differentiate between alkenes (double bonds) and alkynes (triple bonds). Whether the unsaturated hydrocarbon is an alkene or an alkyne , the bromine will add across the multiple bonds producing a decolourised solution. Consequently, additional tests might be necessary to further characterise the compound.

A clear understanding of these outcomes coupled with thorough knowledge of the reasons behind these results, enables a better comprehension of unsaturated hydrocarbons, their differentiated features, and how, through simple tests, science allows us to dissect, determine, and deliver precise information about the seemingly complex world of chemistry.

In summary, the decolourisation of bromine water indicates the presence of unsaturated hydrocarbons, whereas if the colour remains unchanged, unsaturated hydrocarbons are likely absent. The results of this chemical test afford valuable insights into the molecular structure of the studied compounds, and the ability to distinguish between saturated and unsaturated hydrocarbons forms one of the cornerstones of organic chemistry.

Comparing Saturated and Unsaturated Hydrocarbons

Hydrocarbons, the organic compounds made up of hydrogen and carbon atoms, can be broadly classified into two categories: saturated and unsaturated hydrocarbons. Each comes with characteristic properties that determine their chemical behaviour, reactivity, and their role in various practical applications.

Highlighting the Difference Between Saturated and Unsaturated Hydrocarbons

When comparing saturated and unsaturated hydrocarbons , the differentiation primarily revolves around their structure and the type of bonding between the carbon atoms.

Saturated hydrocarbons, also known as alkanes, contain single bonds between carbon atoms and have the maximum number of hydrogen atoms possible. The formula for an alkane is \(C_nH_{2n+2}\), where \(n\) defines the number of carbon atoms.

On the other hand, unsaturated hydrocarbons can be alkenes, which carry at least one carbon-carbon double bond (\(C_nH_{2n}\)) or alkynes, which have at least one carbon-carbon triple bond (\(C_nH_{2n-2}\)). These compounds have fewer than the maximum possible number of hydrogen atoms, hence the term 'unsaturated'. They are more reactive than their saturated counterparts due to the presence of double or triple bonds.

Here is a concise comparison focusing on their core differences:

• Saturated hydrocarbons contain single C-C bonds, whereas unsaturated hydrocarbons carry double or triple C-C bonds.
• Saturated hydrocarbons maximum number of hydrogen atoms; unsaturated hydrocarbons, carrying fewer hydrogen atoms, do not.
• Saturated hydrocarbons are generally less reactive, while unsaturated hydrocarbons are more reactive due to the presence of multiple bonds.

These differing structures and characteristics of saturated and unsaturated hydrocarbons mean they have different chemical reactivity and thus, different roles in practical applications like fuel production, polymers, and more.

The presence of multiple bonds in unsaturated hydrocarbons alters their reactivity. This is because the pi electrons (electrons in a double bond) are readily available and thus, more susceptible to attack by electrophiles. In contrast, the single bonds in saturated hydrocarbons contain sigma electrons, which are not as easily accessible and therefore make saturated compounds less reactive.

How the Hydrogenation of Unsaturated Hydrocarbons bridges the gap

Understanding the strong contrast between saturated and unsaturated hydrocarbons leads us naturally to the concept of hydrogenation, a process that effectively 'bridges the gap' by converting unsaturated hydrocarbons into saturated ones.

Hydrogenation is a chemical reaction that adds hydrogen (H2) to an unsaturated hydrocarbon, breaking the double or triple carbon bonds and converting it into a saturated hydrocarbon. It's carried out in the presence of a catalyst, often palladium, platinum or nickel, and under specific heat/pressure conditions.

This reaction can be represented generally as follows:

\[ RCH=CH2 + H2 -> RCH2-CH3 \]

This equation illustrates that an alkene (an unsaturated hydrocarbon, herein \(RCH=CH2\)) reacts with hydrogen (H2), under certain conditions, to produce an alkane (a saturated hydrocarbon, herein \(RCH2-CH3\)) which has no multiple bonds and has the maximum number of hydrogen atoms.

The hydrogenation process is widely applied in the industrial production of substances, such as margarine from vegetable oil, or the conversion of alkenes to alkanes in petroleum refining. The fact the unsaturated hydrocarbons can undergo hydrogenation and essentially turn into saturated hydrocarbons is significant, as it allows the reactivity of these compounds to be manipulated according to requirements.

The hydrogenation process offers evidence that although saturated and unsaturated hydrocarbons differ remarkably, they can be inter-converted via chemical reactions, thus establishing their intrinsic link within the fascinating sphere of hydrocarbon chemistry.

Unsaturated Hydrocarbons - Key takeaways

• Unsaturated Hydrocarbons Meaning: These are hydrocarbons that contain double or triple bonds between carbon atoms, including alkenes, alkynes, and aromatic hydrocarbons.
• Examples of Unsaturated Hydrocarbons: Ethene and propene (Alkenes), Ethyne and propyne (Alkynes), Benzene and Toluene (Aromatic Hydrocarbons).
• Unsaturated Hydrocarbons Applications: Wide-ranging applications in various sectors, including fuel (petrol and diesel), plastic production, synthesis of industrial chemicals, and in the food industry for ripening fruits.
• Chemical Test for Unsaturated Hydrocarbons: The bromine water test is commonly used. In this test, bromine water decolorizes when mixed with a sample containing unsaturated hydrocarbons due to the addition of bromine across the multiple bonds of the hydrocarbons.
• Difference between Saturated and Unsaturated Hydrocarbons: Saturated hydrocarbons have single bonds between carbon atoms, while unsaturated hydrocarbons have double or triple bonds. This gives unsaturated hydrocarbons a greater degree of reactivity and applications in various industries.

Flashcards in Unsaturated Hydrocarbons 15

The term 'unsaturated' indicates that these hydrocarbons can react with additional hydrogen to form a new compound, effectively becoming 'saturated'.

The food industry employs unsaturated hydrocarbons, notably alkenes like ethylene, to stimulate fruit ripening. The synthesis of ethylene is used commercially to hasten the ripening process, ensuring fruits reach markets at their peak.

The bromine water test can distinguish between saturated and unsaturated hydrocarbons by the change in colour. Unsaturated hydrocarbons decolourise bromine water, whereas saturated ones leave the colour unchanged.

The three common types of unsaturated hydrocarbons are alkenes, alkynes, and aromatic hydrocarbons.

Saturated hydrocarbons, also known as alkanes, contain single bonds between carbon atoms and have the maximum number of hydrogen atoms. In contrast, unsaturated hydrocarbons either possess double or triple bonds between carbon atoms and have fewer than the maximum possible number of hydrogen atoms.

Hydrogenation is a chemical reaction that adds hydrogen to an unsaturated hydrocarbon, breaking the double or triple carbon bonds and converting it into a saturated hydrocarbon. This reaction is usually catalysed by palladium, platinum or nickel and under specific heat/pressure conditions.

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Home » Science » Chemistry » Organic Chemistry » Difference Between Saturated and Unsaturated Hydrocarbons

Difference Between Saturated and Unsaturated Hydrocarbons

Main difference – saturated vs unsaturated hydrocarbons.

Hydrocarbons are organic compounds that contain only carbon and hydrogen atoms. Hydrocarbons are considered as parent compounds of many organic compounds. The main chain of hydrocarbons is made by the C-C bonds, and hydrogen atoms are attached to carbon atoms in the main chain. Based on the presence of single or multiple bonds between carbon atoms, hydrocarbons are classified into two groups namely; saturated hydrocarbons and unsaturated hydrocarbons. The main difference between saturated and unsaturated hydrocarbon is that saturated hydrocarbons contain only single covalent bonds between carbon atoms, whereas unsaturated hydrocarbons contain at least one double or triple covalent bond in the main chain . Saturated and unsaturated hydrocarbons show different characteristics because of these structural differences.

Key Areas Covered

1. What are Saturated Hydrocarbons       – Definition, Structure, Types, Properties 2. What are Unsaturated Hydrocarbons       – Definition, Structure, Types, Properties 3. What is the difference between Saturated and Unsaturated Hydrocarbons       – Comparison of Key Differences

Key Terms: Hydrocarbons, Saturated Hydrocarbons, Unsaturated Hydrocarbons, Covalent Bonds, Alkanes, Alkenes, Alkynes, Aromatic Hydrocarbons

What are Saturated Hydrocarbons

Hydrocarbons in which all carbon atoms are bonded to other atoms by single covalent bonds are called saturated hydrocarbons. Thus, saturated hydrocarbons do not contain any multiple bonds, including double or triple covalent bonds. In these compounds, each carbon atom is bonded directly to four other atoms. Hence, all carbon atoms are fully occupied by making four bonds. This is why these compounds are called saturated hydrocarbons. Saturated hydrocarbons are the simplest and the least polar organic natural products. Examples of saturated hydrocarbons include alkanes and cycloalkane families of hydrocarbons.

The simplest form of saturated hydrocarbons includes methane (CH 4 ), ethane (C 2 H 6 ), propane (C 3 H 8 ) etc. Saturated hydrocarbons burn and give a blue, non-sooty flame in air. Because of the flammability of saturated hydrocarbons that ultimately release a lot of energy, saturated hydrocarbons are often used as a fuel source of vehicle and airplane engines. Well known LPG or cooking gas is also a saturated hydrocarbon called butane (C 4 H 10 ).  The combustion of alkanes with air will result in carbon dioxide gas, water vapor, heat, and light. Hydrocarbons are usually obtained from fossilized plant and animal matter. Once they are obtained as crude oil , the process called distillation is used to separate various products according to their mass. This whole process is called refining of crude oil.

Figure 1: Ethane

What are Unsaturated Hydrocarbons

Unsaturated hydrocarbons are the hydrocarbons that contain at least one carbon-carbon double or triple bond in their carbon chain or ring. These compounds have similar physical properties to those of saturated hydrocarbons. However, their chemical properties are much different from saturated hydrocarbons mainly due to the presence of multiple bonds. Usually, chemical reactions initiate from locations where multiple bonds are present in the carbon chain. Hence, the reactivity of unsaturated hydrocarbon increases with a number of multiple bonds present in the main chain.

Types of Unsaturated Hydrocarbons

There are three types of unsaturated hydrocarbons, namely; (a) alkenes , which contain one or more double bond (C=C), (b) alkynes , which contains one or more triple bonds (C≡C), and (c) aromatic hydrocarbons , which consist of a delocalized bonding resulting in a six-membered carbon ring. Examples of alkenes include ethene, propene, butene, etc. Acetylene, propyne, butyne are some examples for alkynes. Benzene, toluene, aniline are some common examples of aromatic hydrocarbons. The simplest form of unsaturated hydrocarbon is ethylene, which is important as a plant hormone that triggers the ripening of fruits.

Figure 2: Some Alkynes

Saturated Hydrocarbons:   Saturated hydrocarbons are hydrocarbons with only single covalent bonds.

Unsaturated Hydrocarbons: Unsaturated hydrocarbons are hydrocarbons with multiple covalent bonds (double and triple bonds).

Saturated Hydrocarbons: Alkanes are saturated hydrocarbons.

Unsaturated Hydrocarbons:  Alkenes, alkynes, and aromatic hydrocarbons are types of unsaturated hydrocarbons.

Reactivity 

Saturated Hydrocarbons: Saturated hydrocarbons are less reactive.

Unsaturated Hydrocarbons: Unsaturated hydrocarbons are more reactive.

Burn in air

Saturated Hydrocarbons:  Burning saturated hydrocarbons result in a blue, non-sooty flame.

Unsaturated Hydrocarbons: Burning unsaturated hydrocarbons result in a yellow, sooty flame.

Amount of Carbon and Hydrogen 

Saturated Hydrocarbons: Saturated hydrocarbons have a less amount of carbon and high amount of hydrogen.

Unsaturated Hydrocarbons: Unsaturated hydrocarbons have a high amount of carbon and less amount of hydrogen

Saturated Hydrocarbons:  These are usually obtained from fossilized plant and animal materials.

Unsaturated Hydrocarbons:   These are mainly obtained from plants (plant pigments, waxes, proteins, vegetable oils etc.)

The difference between saturated and unsaturated hydrocarbons depends on the types of bonds they contain.  Saturated hydrocarbons contain only single covalent bonds whereas unsaturated hydrocarbons contain at least one or more double or triple carbon-carbon bond. Hence, unsaturated hydrocarbons are more reactive than saturated hydrocarbons. Saturated hydrocarbons include the alkanes, whereas unsaturated hydrocarbons include alkene, alkynes and aromatic hydrocarbons.

References: 1. Cseke, Leland J., Ara Kirakosyan, Peter B. Kaufman, Sara Warber, James A. Duke, and Harry L. Brielmann. Natural products from plants. Boca Raton, FL: CRC Press, 2006. Print 2. Singh, Lakmir, and Manjit Kaur. Science for Tenth Class Part 2 Physics. N.p.: S. Chand, 2016. Print. 3. Stoker, H. Stephen. General, organic, and biological chemistry. 6th ed. N.p.: Cengage Learning, 2012. Print.

Image Courtesy: 1. “Ethane-2D” (Public Domain) via Commons Wikimedia 2. “Alkyne General Formulae V” By Jü – Own work (CC0) via Commons Wikimedia

About the Author: Yashoda

Yashoda has been a freelance writer in the field of biology for about four years. He is an expert in conducting research related to polymer chemistry and nano-technology. He holds a B.Sc. (Hons) degree in Applied Science and a Master of Science degree in Industrial Chemistry.

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8.1 Introduction to Hydrocarbons

Learning Objectives

• Differentiate four classes of hydrocarbons.
• Explain saturated and unsaturated hydrocarbons and how their structures influence their reactivity.

Hydrocarbons are organic compounds that only contain carbon and hydrogen. They are used in a wide variety of applications and on an enormous scale. Hydrocarbons are sources from natural gas and crude oil, the fossil fuel substances taken from underground. These unrefined products are mixtures that are refined in industrial facilities to generate the raw materials used to produce everything from gasoline to plastics, paints, and cosmetics. Hydrocarbons are the simplest organic compounds, but they have interesting physiological effects. These effects depend on the size of the hydrocarbon molecules and the part of the body that is exposed to them.

Hydrocarbons are classified into four main classes: alkanes, alkenes, alkynes, and aromatic hydrocarbons (Figure 8.1.1):

• Alkanes are comprised of [latex]\ce{C}-\ce{C}[/latex] single bonds and have no functional groups.
• They are known as saturated hydrocarbons due to the fact that these molecules have the maximum number of hydrogen atoms possible. In alkanes, each carbon atom forms four single covalent bonds, two with adjacent carbon atoms and two with hydrogen atoms. This results in a structure where each carbon is “saturated” with the maximum number of hydrogen atoms it can hold.
• Methane (Figure 8.1.1) is the simplest alkane, and its molecular formula is [latex]\ce{CH_{4}}[/latex].

• The general formula for alkanes is [latex]\ce{C_{n}H_{2n+2}}[/latex]. This formula indicates that for every [latex]n[/latex] carbon atom, there are [latex]2n+2[/latex] hydrogen atoms. This ensures that each carbon atom is bonded to four other atoms (either other carbon atoms or hydrogen atoms), satisfying the tetravalency of carbon.
• Straight-chain alkanes: they are distinguished by the arrangement of carbon atoms in a continuous, unbranched chain, as shown in Figure 8.1.3.

• Branched alkanes : alkanes can have branching, meaning that instead of forming a straight chain, some carbon atoms may have additional carbon atoms attached to them, as shown in Figure 8.1.4.

• Cyclic alkanes/cycloalkanes : in a cyclic alkane, the carbon atoms are arranged in a ring. The simplest example is cyclopropane [latex]\ce{C_{3}H_{6}}[/latex] is shown in Figure 8.1.5.

• strong single bonds between [latex]\ce{C}-\ce{C}[/latex]  and [latex]\ce{C}-\ce{H}[/latex] and,
• the polarity of [latex]\ce{C}-\ce{C}[/latex] and [latex]\ce{C}-\ce{H}[/latex] bonds. In alkanes, the electrons in single bonds are approximately evenly distributed between the two bonded atoms, making them non-polar. Therefore, no significant positive or negative charge is present on any part of these molecules to attract other ions or molecules. Hence, alkanes are less susceptible to attack by reagents.
• Despite their general lack of reactivity, alkanes can undergo certain reactions under specific conditions. For example, they can undergo combustion (reaction with oxygen to produce carbon dioxide and water) and can be involved in radical reactions under the influence of high-energy conditions.
• Alkanes of low molar mass—those with from 1 to approximately 10 or so carbon atoms—are gases or light liquids that act as anesthetics. Methane, [latex]\ce{CH_{4}}[/latex], is an alkane that is the combustible natural gas you may burn in your furnace to heat your home. Octane, [latex]\ce{C_{8}H_{18}}[/latex], is an alkane that is a component of gasoline. On the skin, liquid alkanes with approximately 5–16 carbon atoms per molecule wash away natural skin oils and cause drying and chapping, while heavier liquid alkanes (those with approximately 17 or more carbon atoms per molecule) act as emollients (skin softeners).
• Alkenes are a class of hydrocarbons characterised by the presence of at least one carbon-carbon double bond in their molecular structure.
• These compounds are part of the larger group of unsaturated hydrocarbons, as they contain fewer hydrogen atoms than the corresponding alkanes (saturated hydrocarbons) with the same number of carbon atoms.
• The general molecular formula for alkenes is [latex]\ce{C_{n}_H_{2n}}[/latex], where [latex]n[/latex] is the number of carbon atoms. The simplest alkene is ethylene with the molecular formula [latex]\ce{C_{2}H_{4}}[/latex] (Figure 8.1.6):

• The presence of a double bond introduces a degree of unsaturation into the molecule, allowing alkenes to undergo additional reactions not possible with saturated hydrocarbons.
• The carbon-carbon double bond consists of one sigma (σ) bond, which is formed by the head-on overlap of atomic orbitals, and one pi (π) bond, which is formed by the side-to-side overlap of p orbitals. The presence of the pi bond introduces a degree of rigidity and restricts rotation around the double bond.
• Alkenes are more reactive than alkanes due to the presence of the π bond. The π electrons are more accessible and can participate in various chemical reactions. Alkenes can undergo polymerisation to form polymers. For example, ethene can polymerise to form polyethylene, a widely used plastic.
• Ethene [latex]\ce{C_{2}H_{4}}[/latex] is a gaseous alkene that serves as a cellular signal in fruits to stimulate ripening. Fruits that are sensitive to this signalling molecule can be placed in a paper bag along with an apple – the apple emits ethene gas, setting off the ripening process in the fruit. Commercial fruit packers can make use of this phenomenon by harvesting unripe fruits and then inducing ripening right before shipping them to consumers.
• The bonding in alkenes is trigonal planar, and the molecules are unable to rotate along the axis of the bond. The double bonds thus lead to 120-degree bond angles and a planar triangular geometry around the double bond.
• Alkynes are a class of hydrocarbons characterised by the presence of at least one [latex]\ce{C}-\ce{C}[/latex] triple bond in their molecular structure. Like alkenes, alkynes are unsaturated hydrocarbons, meaning they have fewer hydrogen atoms than the corresponding alkanes with the same number of carbon atoms. The [latex]\ce{C}-\ce{C}[/latex] triple bond consists of one sigma (σ) bond and two pi (π) bonds. The triple bond imparts a degree of rigidity to the molecular structure.
• The general molecular formula for alkynes is [latex]\ce{C_{n}H_{2n-2}}[/latex], where [latex]n[/latex] is the number of carbon atoms. The simplest member of the alkyne family is ethyne with the molecular formula [latex]\ce{C_{2}H_{2}}[/latex] (Figure 8.1.7). The common name of ethyne is acetylene. Acetylene is widely used in oxy-acetylene welding and cutting processes. It is a precursor in the production of polymers. For example, it can polymerise to form polyacetylene, a conductive polymer with potential applications in electronic devices.

• Alkynes are more reactive than alkanes due to the presence of the triple bond and can undergo various chemical reactions like alkenes. The hydrogen atoms attached to the carbon atoms of the triple bond in alkynes are relatively acidic compared to those in alkanes and alkenes. This acidity is a result of the electronegative nature of the adjacent triple bond.
• In alkynes, the geometry around the triple bond is linear (bond angles are 180º), and only one other atom can bond to the alkyne carbon, so there is no rotation.

Aromatic Hydrocarbons

• Aromatic hydrocarbons are a class of organic compounds that contain a cyclic structure with alternating single and double bonds, known as an aromatic ring. In the aromatic ring, each carbon atom is bonded to two other carbon atoms and one hydrogen atom. The electrons in the pi (π) bonds are delocalised, creating a stable, resonant structure.
• Aromatic hydrocarbons are unsaturated, like alkenes and alkynes. Although aromatic hydrocarbons contain double bonds, their reactivity differs from that of typical alkenes. Aromatic compounds are known for their stability and resistance to certain reactions that would break the aromaticity of the ring.
• Benzene ([latex]\ce{C_{6}H_{6}}[/latex]) is the simplest and most well-known aromatic hydrocarbon (Figure 8.1.8). Other common aromatic hydrocarbons include toluene, xylene, naphthalene, and anthracene. Aromatic rings can also be found in many organic compounds, including certain classes of drugs, dyes, and natural products.

• Aromatic hydrocarbons have numerous industrial applications. They are key components in the production of plastics, synthetic fibres, detergents, pharmaceuticals, and many other chemicals.
• Aromatic groups are planar (flat) ring structures and are widespread in nature, so you will see them frequently if you encounter chemical structures in biology classes or in biomedical work.

Key Takeaways

• Hydrocarbons are organic compounds that only contain carbon and hydrogen.
• Hydrocarbons are classified into four main classes: alkanes, alkenes, alkynes, and aromatic hydrocarbons.
• Alkanes are comprised of [latex]\ce{C}-\ce{C}[/latex] single bonds, alkenes consist of one or more [latex]\ce{C}-\ce{C}[/latex] double bond and alkynes are made up of one or more [latex]\ce{C}-\ce{C}[/latex] triple bonds.
• Alkanes are classified as saturated hydrocarbons, while alkenes, alkynes and aromatic hydrocarbons are classified as unsaturated hydrocarbons.
• Alkanes are less reactive compared to other hydrocarbons due to the presence of strong [latex]\ce{C}-\ce{C}[/latex] and [latex]\ce{C}-\ce{H}[/latex] single bonds.

Practice Questions

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