Class 10 Exam > Class 10 Videos > Science Class 10 > Covalent Bonding & Versatile Nature of Carbon
Covalent Bonding & Versatile Nature of Carbon Video Lecture | Science Class 10
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FAQs on Covalent Bonding & Versatile Nature of Carbon Video Lecture - Science Class 10
| 1. What is covalent bonding and how does it occur? |  |
Ans. Covalent bonding is a type of chemical bonding in which atoms share electrons to form a stable molecule. It occurs when two non-metal atoms come together and share their valence electrons to achieve a stable electron configuration. This sharing of electrons creates a strong bond between the atoms.
| 2. How does carbon exhibit versatile bonding properties? | |
Ans. Carbon exhibits versatile bonding properties due to its unique electron configuration. Carbon has four valence electrons, allowing it to form covalent bonds with up to four other atoms. It can form single, double, or triple bonds with other carbon atoms or different elements, resulting in a wide range of organic compounds with diverse structures and properties.
| 3. What are the characteristics of covalent compounds formed by carbon? | |
Ans. Covalent compounds formed by carbon, also known as organic compounds, have several characteristics. They are generally nonpolar or have low polarity, have low melting and boiling points, and are often insoluble in water. They can have a variety of physical and chemical properties depending on the arrangement and functional groups present in the compound.
| 4. How does the versatile nature of carbon contribute to the diversity of life? | |
Ans. The versatile nature of carbon allows it to form the complex molecules found in living organisms. Carbon-based compounds, such as carbohydrates, lipids, proteins, and nucleic acids, play vital roles in biological processes. The ability of carbon to form different bonds and structures enables the vast diversity of organic molecules necessary for life's functions and processes.
| 5. What are some examples of organic compounds that demonstrate the versatile nature of carbon? | |
Ans. Some examples of organic compounds that demonstrate the versatile nature of carbon include methane (CH4), ethene (C2H4), ethanol (C2H5OH), and glucose (C6H12O6). Methane and ethene are hydrocarbons, while ethanol is an alcohol and glucose is a carbohydrate. These compounds showcase the different bonding arrangements and functional groups that carbon can form, highlighting its versatile nature.
Text Transcript from Video
0:0:0: did you know that carbon is not your
0:0:2: average element but a superstar that
0:0:4: forms more compounds than all other
0:0:6: elements combined
0:0:8: from the tires on your car to the
0:0:10: bubbles in your favorite soft drink
0:0:12: carbon is everywhere
0:0:14: and here is the most incredible fact
0:0:16: every living structure on this planet is
0:0:19: carbon based
0:0:21: that's right we literally or our very
0:0:23: existence to this element and that's why
0:0:26: a whole chapter is dedicated to this
0:0:28: remarkable element
0:0:30: in this video we will get to know some
0:0:32: interesting details about carbon such as
0:0:34: what are carbon compounds
0:0:37: the type of bonding in carbon compounds
0:0:40: characteristics of covalent compounds
0:0:42: versatile nature of carbon
0:0:45: so let's begin
0:0:47: what are carbon compounds
0:0:49: carbon compounds are defined as chemical
0:0:52: substances containing carbon
0:0:54: carbon combines with a lot of elements
0:0:57: like hydrogen oxygen nitrogen and sulfur
0:1:1: to form countless carbon compounds
0:1:3: and guess what
0:1:5: the number of these carbon compounds
0:1:8: exceeds 3 million
0:1:10: these compounds are used in clothes
0:1:12: medicines books food fertilizers fuels
0:1:16: and a whole lot more
0:1:18: so carbon is literally everywhere around
0:1:21: us
0:1:22: but how does carbon combined with so
0:1:24: many different elements
0:1:26: it is because of covalent bonding
0:1:29: before we dive into the explanation of
0:1:31: covalent bond let's understand why
0:1:34: elements actually form bonds
0:1:36: elements bond to form compounds in order
0:1:39: to become stable
0:1:41: an element can achieve stability by
0:1:43: completing its outermost shell
0:1:46: for example hydrogen has one electron in
0:1:49: its outermost shell and it needs one
0:1:51: more electron in its outermost shell to
0:1:54: become stable
0:1:55: similarly oxygen has six electrons in
0:1:58: its last shell and needs two more
0:2:0: electrons to become stable as its
0:2:3: outermost shell completes at eight
0:2:5: electrons
0:2:6: so remember the elements we are going to
0:2:9: study in class 10 need 8 electrons in
0:2:12: their outermost shell to become stable
0:2:14: and the only exception is hydrogen that
0:2:17: needs two electrons
0:2:19: now these elements can get these
0:2:21: electrons from other elements and that
0:2:23: is called chemical bonding
0:2:25: atoms of different elements can bond
0:2:27: together through either ionic or
0:2:29: covalent bonds
0:2:31: ionic bonds occur when one atom loses
0:2:34: one or more electrons to another atom
0:2:37: which then gains those electrons
0:2:40: ionic bonds occur between metals and
0:2:42: non-metals
0:2:44: for example sodium n a and chlorine CL
0:2:48: can form an ionic bond to create sodium
0:2:51: chloride NaCl also known as stable salt
0:2:55: ium loses one electron to become a
0:2:58: positively charged ion in a positive
0:3:0: while chlorine gains that electron to
0:3:3: become negatively charged ion CL
0:3:6: negative
0:3:7: the resulting attraction between an
0:3:9: A-Plus and cl forms the ionic bond in an
0:3:12: ACL
0:3:13: on the contrary covalent bonds occur
0:3:16: when two atoms share one or more pairs
0:3:18: of electrons
0:3:20: this type of bond typically occurs
0:3:22: between non-metals
0:3:24: for example a chlorine atom has seven
0:3:27: electrons in its outermost shell and it
0:3:30: needs one more electron to become stable
0:3:33: when two chlorine atoms come together
0:3:36: they share one electron each forming a
0:3:39: covalent bond or C LCL Bond
0:3:42: remember in covalent bond each shared
0:3:45: electron belongs to both the atoms it is
0:3:47: being shared with
0:3:49: now both chlorine atoms have eight
0:3:51: electrons
0:3:53: this sharing of electrons leads to the
0:3:55: formation of the cl2 molecule
0:3:58: after a quick explanation of different
0:4:0: kinds of bonding now let's discuss
0:4:3: bonding in carbon
0:4:5: carbon has six electrons and its
0:4:7: electronic configuration is 2 4.
0:4:10: which means that it will need four more
0:4:12: electrons to become stable
0:4:15: now will it become stable by forming
0:4:17: ionic bond or covalent bond
0:4:20: as mentioned before carbon forms
0:4:22: covalent bonds
0:4:24: but why it does not form ionic bonds
0:4:27: the reason is that it cannot gain
0:4:29: electrons because the size of carbon is
0:4:32: small and it cannot hold four more
0:4:34: electrons
0:4:36: it cannot lose electrons because a lot
0:4:38: of energy is required to lose four
0:4:40: electrons
0:4:42: so the only option carbon has is to
0:4:44: share electrons to form covalent bonds
0:4:48: we understand the concept of covalent
0:4:50: bonding is new to you so let's solidify
0:4:53: our understanding with examples of
0:4:55: covalent bonds in compounds such as
0:4:57: hydrogen hydrochloric acid oxygen
0:5:0: nitrogen and methane
0:5:2: before continuing with the video here is
0:5:5: an important note
0:5:7: questions from ncrt are usually asked in
0:5:10: the exam from this chapter so make sure
0:5:12: to practice all the ncrt questions
0:5:16: solutions to ncrt questions are provided
0:5:19: on the edurev app which are written by
0:5:21: experts now let's begin with simplest of
0:5:25: all molecules hydrogen H2
0:5:28: hydrogen molecule is made up of two
0:5:31: hydrogen atoms that share their
0:5:33: electrons with each other
0:5:35: each hydrogen atom has only one electron
0:5:38: which means it has an incomplete
0:5:40: outermost shell
0:5:41: but when to hydrogen atoms come together
0:5:44: they can share their electrons to
0:5:46: complete their outermost shell
0:5:48: this sharing of electrons forms the
0:5:51: covalent bond also known as the HH Bond
0:5:55: now let's talk about hydrochloric acid
0:5:58: HCL
0:6:0: hydrochloric acid is made up of hydrogen
0:6:2: and chlorine atoms
0:6:4: hydrogen has one electron in its
0:6:7: outermost shell while chlorine has seven
0:6:10: to become stable the hydrogen atom
0:6:13: shares its electron with the chlorine
0:6:15: atom forming a covalent bond
0:6:18: this sharing of electrons leads to the
0:6:21: formation of the HCL molecule
0:6:23: moving on to the oxygen molecule O2
0:6:27: an oxygen atom has six electrons in its
0:6:30: outermost shell and leads to more
0:6:31: electrons
0:6:33: when two oxygen atoms come together they
0:6:36: share two electrons each forming a
0:6:38: double covalent bond
0:6:40: this sharing of electrons leads to the
0:6:42: formation of the O2 molecule which is
0:6:45: responsible for the air we breathe
0:6:47: now nitrogen has an atomic number of
0:6:50: seven with five electrons in its valence
0:6:53: shell and needs three more electrons
0:6:56: two nitrogen atoms share three electrons
0:6:59: each to form a stable and two molecule
0:7:2: the nitrogen molecule has a triple
0:7:4: covalent bond between the two nitrogen
0:7:6: atoms
0:7:8: let's discuss covalent bonding in a
0:7:11: carbon compound such as methane
0:7:13: the methane molecule is made up of
0:7:16: carbon and four hydrogen atoms
0:7:19: carbon will form covalent bonds with
0:7:21: four hydrogen atoms where each hydrogen
0:7:24: atom shares an electron and the carbon
0:7:27: shares one electron each with the
0:7:28: hydrogen atoms
0:7:30: the total number of electrons in carbon
0:7:33: now is 8 and the total number of
0:7:35: electrons in each hydrogen is two which
0:7:38: completes its outer shell
0:7:40: from all the examples discussed it is
0:7:43: clear that covalent bonds are of three
0:7:45: types
0:7:46: single double and triple
0:7:49: a single covalent bond is formed by the
0:7:52: sharing of one pair of electrons between
0:7:54: two atoms
0:7:56: for example in hydrogen molecule
0:7:59: a double covalent bond is formed by the
0:8:1: sharing of two pairs of electrons
0:8:3: between the two combining atoms
0:8:6: example of double bond is oxygen
0:8:8: molecule
0:8:9: a triple bond is formed by the sharing
0:8:12: of three pairs of electrons between the
0:8:14: two combining atoms
0:8:16: for example nitrogen molecule
0:8:19: moving on to one of the most important
0:8:22: topic of this chapter characteristics of
0:8:24: covalent compounds
0:8:26: covalent compounds have low melting and
0:8:29: boiling points which means they can
0:8:31: easily turn from a solid to a liquid or
0:8:33: gas when heated
0:8:35: this is because intermolecular forces in
0:8:38: covalent compounds are weaker than those
0:8:40: in ionic compounds
0:8:42: they also tend to dissolve easily
0:8:44: inorganic solvents like alcohol but they
0:8:47: are not very soluble in water
0:8:50: this is because water molecules have a
0:8:52: strong attraction to each other making
0:8:55: it difficult for other molecules to
0:8:57: dissolve
0:8:58: finally covalent compounds do not
0:9:1: conduct electricity
0:9:3: this is because electricity is carried
0:9:5: by charged particles like ions or free
0:9:8: electrons and covalent compounds don't
0:9:11: have any charged particles that can
0:9:13: carry electricity
0:9:15: now in the beginning of the video we
0:9:17: discussed how there are millions of
0:9:19: carbon compounds known to man
0:9:22: it is clearly evident that something is
0:9:24: different with carbon but what is it
0:9:26: that makes it so unique
0:9:28: it is a versatile nature of carbon that
0:9:30: helps carbon to form a large number of
0:9:33: compounds
0:9:34: mainly The Versatile nature of carbon is
0:9:37: due to properties of carbon
0:9:39: tetrivilency and catenation
0:9:42: the first property is tetravilancy
0:9:45: Tetra means four which means that the
0:9:47: valency of carbon is four
0:9:49: the four valency of carbon means that it
0:9:52: can combine and form bonds with four
0:9:55: other atoms of carbon or atoms of other
0:9:57: elements such as fluorine chlorine
0:10:0: hydrogen Etc
0:10:2: we have seen the example of methane
0:10:4: where the carbon combines with four
0:10:6: hydrogen
0:10:7: these bonds made by carbon are strong
0:10:10: making these compounds very stable
0:10:13: but what does it mean by carbon
0:10:15: compounds being stable
0:10:17: it means that carbon compounds do not
0:10:19: break and carbon is able to hold other
0:10:22: elements close to it
0:10:24: this is because the size of the carbon
0:10:26: is small and it can hold on to the
0:10:28: shared pair of electrons hence making
0:10:31: the bonds strong and carbon compounds
0:10:33: stable
0:10:34: the next property is catenation
0:10:37: the carbon can combine with other
0:10:39: carbons to form long chains which can be
0:10:42: either straight branched or in the form
0:10:44: of rings
0:10:45: this property of carbon to form bonds
0:10:48: with other atoms of carbon giving rise
0:10:50: to Long carbon chains is called
0:10:52: catenation
0:10:54: similar properties are shown by silicon
0:10:56: but its extent is less as compared to
0:10:59: carbon
0:11:0: these are the two properties responsible
0:11:2: for a large number of carbon compounds
0:11:4: and that's why carbon compounds is an
0:11:7: entire chapter in itself we hope that
0:11:10: you have understood the topic
0:11:12: and now you should start studying this
0:11:15: chapter with the edurev app as you get
0:11:17: with your lectures notes variety of
0:11:20: questions like McQ tests short and long
0:11:23: answer questions sample papers and so
0:11:26: much more for all the chapters of each
0:11:29: subject
0:11:30: it's like having the entire School in
0:11:32: your pocket
0:0:2: average element but a superstar that
0:0:4: forms more compounds than all other
0:0:6: elements combined
0:0:8: from the tires on your car to the
0:0:10: bubbles in your favorite soft drink
0:0:12: carbon is everywhere
0:0:14: and here is the most incredible fact
0:0:16: every living structure on this planet is
0:0:19: carbon based
0:0:21: that's right we literally or our very
0:0:23: existence to this element and that's why
0:0:26: a whole chapter is dedicated to this
0:0:28: remarkable element
0:0:30: in this video we will get to know some
0:0:32: interesting details about carbon such as
0:0:34: what are carbon compounds
0:0:37: the type of bonding in carbon compounds
0:0:40: characteristics of covalent compounds
0:0:42: versatile nature of carbon
0:0:45: so let's begin
0:0:47: what are carbon compounds
0:0:49: carbon compounds are defined as chemical
0:0:52: substances containing carbon
0:0:54: carbon combines with a lot of elements
0:0:57: like hydrogen oxygen nitrogen and sulfur
0:1:1: to form countless carbon compounds
0:1:3: and guess what
0:1:5: the number of these carbon compounds
0:1:8: exceeds 3 million
0:1:10: these compounds are used in clothes
0:1:12: medicines books food fertilizers fuels
0:1:16: and a whole lot more
0:1:18: so carbon is literally everywhere around
0:1:21: us
0:1:22: but how does carbon combined with so
0:1:24: many different elements
0:1:26: it is because of covalent bonding
0:1:29: before we dive into the explanation of
0:1:31: covalent bond let's understand why
0:1:34: elements actually form bonds
0:1:36: elements bond to form compounds in order
0:1:39: to become stable
0:1:41: an element can achieve stability by
0:1:43: completing its outermost shell
0:1:46: for example hydrogen has one electron in
0:1:49: its outermost shell and it needs one
0:1:51: more electron in its outermost shell to
0:1:54: become stable
0:1:55: similarly oxygen has six electrons in
0:1:58: its last shell and needs two more
0:2:0: electrons to become stable as its
0:2:3: outermost shell completes at eight
0:2:5: electrons
0:2:6: so remember the elements we are going to
0:2:9: study in class 10 need 8 electrons in
0:2:12: their outermost shell to become stable
0:2:14: and the only exception is hydrogen that
0:2:17: needs two electrons
0:2:19: now these elements can get these
0:2:21: electrons from other elements and that
0:2:23: is called chemical bonding
0:2:25: atoms of different elements can bond
0:2:27: together through either ionic or
0:2:29: covalent bonds
0:2:31: ionic bonds occur when one atom loses
0:2:34: one or more electrons to another atom
0:2:37: which then gains those electrons
0:2:40: ionic bonds occur between metals and
0:2:42: non-metals
0:2:44: for example sodium n a and chlorine CL
0:2:48: can form an ionic bond to create sodium
0:2:51: chloride NaCl also known as stable salt
0:2:55: ium loses one electron to become a
0:2:58: positively charged ion in a positive
0:3:0: while chlorine gains that electron to
0:3:3: become negatively charged ion CL
0:3:6: negative
0:3:7: the resulting attraction between an
0:3:9: A-Plus and cl forms the ionic bond in an
0:3:12: ACL
0:3:13: on the contrary covalent bonds occur
0:3:16: when two atoms share one or more pairs
0:3:18: of electrons
0:3:20: this type of bond typically occurs
0:3:22: between non-metals
0:3:24: for example a chlorine atom has seven
0:3:27: electrons in its outermost shell and it
0:3:30: needs one more electron to become stable
0:3:33: when two chlorine atoms come together
0:3:36: they share one electron each forming a
0:3:39: covalent bond or C LCL Bond
0:3:42: remember in covalent bond each shared
0:3:45: electron belongs to both the atoms it is
0:3:47: being shared with
0:3:49: now both chlorine atoms have eight
0:3:51: electrons
0:3:53: this sharing of electrons leads to the
0:3:55: formation of the cl2 molecule
0:3:58: after a quick explanation of different
0:4:0: kinds of bonding now let's discuss
0:4:3: bonding in carbon
0:4:5: carbon has six electrons and its
0:4:7: electronic configuration is 2 4.
0:4:10: which means that it will need four more
0:4:12: electrons to become stable
0:4:15: now will it become stable by forming
0:4:17: ionic bond or covalent bond
0:4:20: as mentioned before carbon forms
0:4:22: covalent bonds
0:4:24: but why it does not form ionic bonds
0:4:27: the reason is that it cannot gain
0:4:29: electrons because the size of carbon is
0:4:32: small and it cannot hold four more
0:4:34: electrons
0:4:36: it cannot lose electrons because a lot
0:4:38: of energy is required to lose four
0:4:40: electrons
0:4:42: so the only option carbon has is to
0:4:44: share electrons to form covalent bonds
0:4:48: we understand the concept of covalent
0:4:50: bonding is new to you so let's solidify
0:4:53: our understanding with examples of
0:4:55: covalent bonds in compounds such as
0:4:57: hydrogen hydrochloric acid oxygen
0:5:0: nitrogen and methane
0:5:2: before continuing with the video here is
0:5:5: an important note
0:5:7: questions from ncrt are usually asked in
0:5:10: the exam from this chapter so make sure
0:5:12: to practice all the ncrt questions
0:5:16: solutions to ncrt questions are provided
0:5:19: on the edurev app which are written by
0:5:21: experts now let's begin with simplest of
0:5:25: all molecules hydrogen H2
0:5:28: hydrogen molecule is made up of two
0:5:31: hydrogen atoms that share their
0:5:33: electrons with each other
0:5:35: each hydrogen atom has only one electron
0:5:38: which means it has an incomplete
0:5:40: outermost shell
0:5:41: but when to hydrogen atoms come together
0:5:44: they can share their electrons to
0:5:46: complete their outermost shell
0:5:48: this sharing of electrons forms the
0:5:51: covalent bond also known as the HH Bond
0:5:55: now let's talk about hydrochloric acid
0:5:58: HCL
0:6:0: hydrochloric acid is made up of hydrogen
0:6:2: and chlorine atoms
0:6:4: hydrogen has one electron in its
0:6:7: outermost shell while chlorine has seven
0:6:10: to become stable the hydrogen atom
0:6:13: shares its electron with the chlorine
0:6:15: atom forming a covalent bond
0:6:18: this sharing of electrons leads to the
0:6:21: formation of the HCL molecule
0:6:23: moving on to the oxygen molecule O2
0:6:27: an oxygen atom has six electrons in its
0:6:30: outermost shell and leads to more
0:6:31: electrons
0:6:33: when two oxygen atoms come together they
0:6:36: share two electrons each forming a
0:6:38: double covalent bond
0:6:40: this sharing of electrons leads to the
0:6:42: formation of the O2 molecule which is
0:6:45: responsible for the air we breathe
0:6:47: now nitrogen has an atomic number of
0:6:50: seven with five electrons in its valence
0:6:53: shell and needs three more electrons
0:6:56: two nitrogen atoms share three electrons
0:6:59: each to form a stable and two molecule
0:7:2: the nitrogen molecule has a triple
0:7:4: covalent bond between the two nitrogen
0:7:6: atoms
0:7:8: let's discuss covalent bonding in a
0:7:11: carbon compound such as methane
0:7:13: the methane molecule is made up of
0:7:16: carbon and four hydrogen atoms
0:7:19: carbon will form covalent bonds with
0:7:21: four hydrogen atoms where each hydrogen
0:7:24: atom shares an electron and the carbon
0:7:27: shares one electron each with the
0:7:28: hydrogen atoms
0:7:30: the total number of electrons in carbon
0:7:33: now is 8 and the total number of
0:7:35: electrons in each hydrogen is two which
0:7:38: completes its outer shell
0:7:40: from all the examples discussed it is
0:7:43: clear that covalent bonds are of three
0:7:45: types
0:7:46: single double and triple
0:7:49: a single covalent bond is formed by the
0:7:52: sharing of one pair of electrons between
0:7:54: two atoms
0:7:56: for example in hydrogen molecule
0:7:59: a double covalent bond is formed by the
0:8:1: sharing of two pairs of electrons
0:8:3: between the two combining atoms
0:8:6: example of double bond is oxygen
0:8:8: molecule
0:8:9: a triple bond is formed by the sharing
0:8:12: of three pairs of electrons between the
0:8:14: two combining atoms
0:8:16: for example nitrogen molecule
0:8:19: moving on to one of the most important
0:8:22: topic of this chapter characteristics of
0:8:24: covalent compounds
0:8:26: covalent compounds have low melting and
0:8:29: boiling points which means they can
0:8:31: easily turn from a solid to a liquid or
0:8:33: gas when heated
0:8:35: this is because intermolecular forces in
0:8:38: covalent compounds are weaker than those
0:8:40: in ionic compounds
0:8:42: they also tend to dissolve easily
0:8:44: inorganic solvents like alcohol but they
0:8:47: are not very soluble in water
0:8:50: this is because water molecules have a
0:8:52: strong attraction to each other making
0:8:55: it difficult for other molecules to
0:8:57: dissolve
0:8:58: finally covalent compounds do not
0:9:1: conduct electricity
0:9:3: this is because electricity is carried
0:9:5: by charged particles like ions or free
0:9:8: electrons and covalent compounds don't
0:9:11: have any charged particles that can
0:9:13: carry electricity
0:9:15: now in the beginning of the video we
0:9:17: discussed how there are millions of
0:9:19: carbon compounds known to man
0:9:22: it is clearly evident that something is
0:9:24: different with carbon but what is it
0:9:26: that makes it so unique
0:9:28: it is a versatile nature of carbon that
0:9:30: helps carbon to form a large number of
0:9:33: compounds
0:9:34: mainly The Versatile nature of carbon is
0:9:37: due to properties of carbon
0:9:39: tetrivilency and catenation
0:9:42: the first property is tetravilancy
0:9:45: Tetra means four which means that the
0:9:47: valency of carbon is four
0:9:49: the four valency of carbon means that it
0:9:52: can combine and form bonds with four
0:9:55: other atoms of carbon or atoms of other
0:9:57: elements such as fluorine chlorine
0:10:0: hydrogen Etc
0:10:2: we have seen the example of methane
0:10:4: where the carbon combines with four
0:10:6: hydrogen
0:10:7: these bonds made by carbon are strong
0:10:10: making these compounds very stable
0:10:13: but what does it mean by carbon
0:10:15: compounds being stable
0:10:17: it means that carbon compounds do not
0:10:19: break and carbon is able to hold other
0:10:22: elements close to it
0:10:24: this is because the size of the carbon
0:10:26: is small and it can hold on to the
0:10:28: shared pair of electrons hence making
0:10:31: the bonds strong and carbon compounds
0:10:33: stable
0:10:34: the next property is catenation
0:10:37: the carbon can combine with other
0:10:39: carbons to form long chains which can be
0:10:42: either straight branched or in the form
0:10:44: of rings
0:10:45: this property of carbon to form bonds
0:10:48: with other atoms of carbon giving rise
0:10:50: to Long carbon chains is called
0:10:52: catenation
0:10:54: similar properties are shown by silicon
0:10:56: but its extent is less as compared to
0:10:59: carbon
0:11:0: these are the two properties responsible
0:11:2: for a large number of carbon compounds
0:11:4: and that's why carbon compounds is an
0:11:7: entire chapter in itself we hope that
0:11:10: you have understood the topic
0:11:12: and now you should start studying this
0:11:15: chapter with the edurev app as you get
0:11:17: with your lectures notes variety of
0:11:20: questions like McQ tests short and long
0:11:23: answer questions sample papers and so
0:11:26: much more for all the chapters of each
0:11:29: subject
0:11:30: it's like having the entire School in
0:11:32: your pocket
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