Covalent Bonding & Versatile Nature of Carbon Video Lecture | Science Class 10

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