CBSE Class 10th Covalent Bonding in Carbon Compounds Details & Preparations Downloads
This exploration is not merely an academic pursuit but a quest to empower students with the knowledge and skills that lay the foundation for a profound understanding of chemistry. Through the lens of CBSE NCERT resources, we embark on a learning adventure that demystifies the intricacies of covalent bonding in carbon compounds, providing students with the tools they need to navigate the complex world of organic chemistry with confidence and curiosity.
Unlocking the Secrets of Covalent Bonding in Carbon Compounds: A Comprehensive Guide with CBSE NCERT Download Resources
Understanding Covalent Bonding:
Covalent bonding is a type of chemical bond where atoms share electrons to achieve a more stable electron configuration. In the case of carbon compounds, this form of bonding is prevalent and plays a pivotal role in shaping the diverse array of molecules found in nature. To comprehend covalent bonding in carbon compounds, we must delve into the structure of carbon atoms.
Carbon, with an atomic number of 6, has four valence electrons in its outer shell. To achieve stability, carbon atoms readily form covalent bonds by sharing electrons with other atoms, including carbon itself. This ability to bond with other carbon atoms and a variety of other elements gives rise to the vast complexity and diversity observed in organic compounds.
The Tetrahedral Structure of Carbon Compounds:
One of the defining features of covalent bonding in carbon compounds is the tetrahedral arrangement of atoms around a carbon atom. Due to its ability to form four covalent bonds, carbon often adopts a tetrahedral geometry, creating a three-dimensional structure that influences the properties of the resulting molecules.
Methane (CH₄) serves as an illustrative example. In methane, each of the four hydrogen atoms forms a covalent bond with the central carbon atom, resulting in a tetrahedral configuration. This molecular geometry is a consequence of the sharing of electrons in the covalent bonds, reflecting the principle that electrons repel each other, causing the atoms to arrange themselves in a manner that minimizes electrostatic repulsion.
Versatility of Carbon Compounds:
The versatility of carbon compounds arises from carbon's ability to form single, double, and triple bonds with other atoms, including carbon itself. These multiple bonding options lead to the formation of a diverse range of molecules, each with unique properties and functions.
For instance, the presence of double bonds in compounds like ethene (C₂H₄) imparts distinct characteristics, such as increased reactivity and the potential for polymerization. The study of covalent bonding in carbon compounds is thus essential for understanding the behavior of these molecules in various chemical reactions.
Covalent bonding can be achieved in two ways:
- Sharing of electrons between atoms of the same kind, for example, formation of H2, Cl2, O2, etc.
- Sharing of electrons between atoms of different kinds, for example, formation of CH4, H2O, NH3, etc.
Covalent Bonding in Carbon Atom
As per the electronic configuration of carbon, it needs to gain or lose 4 electrons to become stable, which seems impossible as:
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Carbon cannot gain 4 electrons to become C4-, because it will be tough for 6 protons to hold 10 electrons, and so the atom will become unstable.
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Carbon cannot lose 4 electrons to become C4+ because it would require a large amount of energy to remove 4 electrons. Also, the C4+ would have only 2 electrons held by the proton, which will again become unstable.
Carbon cannot gain or donate electrons, so to complete its nearest noble gas configuration it shares electrons to form a covalent bond.
Properties of Covalent Bond
If the normal valence of an atom is not satisfied by sharing a single electron pair between atoms, the atoms may share more than one electron pair between them. Some of the properties of covalent bonds are listed below:
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Covalent bonding does not result in the formation of new electrons. The bond only pairs them.
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They are very powerful chemical bonds that exist between atoms.
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A covalent bond normally contains an energy of about ~80 kilocalories per mole (kcal/mol).
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Covalent bonds rarely break spontaneously after it is formed.
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Covalent bonds are directional, where the atoms that are bonded showcase specific orientations relative to one another.
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Most compounds having covalent bonds exhibit relatively low melting points and boiling points.
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Compounds with covalent bonds usually have lower enthalpies of vaporization and fusion.
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Compounds formed by covalent bonding don’t conduct electricity due to the lack of free electrons.
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Covalent compounds are not soluble in water.
What Is the Octet Rule?
All atoms except noble gases have less than eight electrons in their valence shell. In other words, the valence shells of these atoms do not have stable configurations. Therefore, they combine with each other or with other atoms to attain stable electronic configurations.
Therefore,
“The tendency of atoms of various elements to attain stable configuration of eight electrons in their valence shells is the cause of chemical combination”
and”
“The principle of attaining the maximum of eight electrons in the valence shell of atoms is called the octet rule.
Conditions for Writing the Lewis Dot Structures
- Sharing of an electron pair between the atoms results in the formation of covalent bonds.
- During bond formation, each bond consists of two electrons which are contributed by each one of the combining atoms.
- By the mutual sharing of electrons, each atom attains an octet configuration in its valence shell.
Electron dot structures of covalent molecules are written with respect to the octet rule. According to this rule, all the atoms in the molecule will have eight electrons in their valence shell except the hydrogen atom. Hydrogen will have only two electrons because only two electrons complete its first shell to attain helium configuration.
Thus the elements of group 17, such as Cl, would share one electron to attain a stable octet; the elements of group 16, such as O and S, would share two electrons; the elements of group 15 would share three electrons and so on.
For Example, the oxygen atom, which has six electrons in its valence shell, completes its octet by sharing its two electrons with two hydrogen atoms to form a water molecule.
CBSE Class 10th Downloadable Resources:
1. CBSE Class 10th Topic Wise Summary | View Page / Download |
2. CBSE Class 10th NCERT Books | View Page / Download |
3. CBSE Class 10th NCERT Solutions | View Page / Download |
4. CBSE Class 10th Exemplar | View Page / Download |
5. CBSE Class 10th Previous Year Papers | View Page / Download |
6. CBSE Class 10th Sample Papers | View Page / Download |
7. CBSE Class 10th Question Bank | View Page / Download |
8. CBSE Class 10th Topic Wise Revision Notes | View Page / Download |
9. CBSE Class 10th Last Minutes Preparation Resources (LMP) | View Page / Download |
10. CBSE Class 10th Best Reference Books | View Page / Download |
11. CBSE Class 10th Formula Booklet | View Page / Download |
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SAMPLE PRACTICE QUESTION
Q:1 What is covalent bonding in carbon compounds?
Ans: Covalent bonding involves the sharing of electrons between carbon atoms, creating stable molecular structures.
Q:2 How does CBSE NCERT Download assist in understanding covalent bonding?
Ans: CBSE NCERT Download provides comprehensive resources, aiding students in grasping the complexities of covalent bonding in carbon compounds.
Q:3 Why is the tetrahedral structure significant in carbon compounds?
Ans: The tetrahedral arrangement results from carbon forming four covalent bonds, influencing the three-dimensional geometry and properties of molecules.
Q:4 How does the versatility of carbon compounds contribute to their diversity?
Ans: Carbon's ability to form single, double, and triple bonds allows for diverse molecular structures, influencing the unique properties of different carbon compounds.
Q:5 In what ways does covalent bonding impact the reactivity of carbon compounds?
Ans: Covalent bonding influences the reactivity of carbon compounds, with single, double, and triple bonds exhibiting varying levels of chemical reactivity.
CBSE CLASS 10 Mathematics Chapters |
Chapter1: Real Numbers |
Chapter2: Polynomials |
Chapter3: Pair of Linear Equations in Two Variables |
Chapter4: Quadratic Equations |
Chapter5: Arithmetic Progressions |
Chapter6: Triangles |
Chapter7: Coordinate Geometry |
Chapter8: Introduction to Trigonometry |
Chapter9: Some Applications of Trigonometry |
Chapter10: Circles |
Chapter11: Areas Related to Circles |
Chapter12: Surface Areas and Volumes |
Chapter13: Statistics |
Chapter14: Probability |
CBSE CLASS 10 Science Chapters |
Chapter1: Chemical Reactions and Equations |
Chapter2: Acids, Bases and Salts |
Chapter3: Metals and Non-metals |
Chapter4: Carbon and its Compounds |
Versatile nature of Carbon |
Nomenclature of carbon Compounds |
Differences Between Saturated and Unsaturated Hydrocarbons |
Ethanol and Ethanoic Acid |
Chapter5: Life Processes |
Chapter6: Control and Coordination |
Chapter7: How do Organisms Reproduce? |
Chapter8: Heredity |
Chapter9: Light – Reflection and Refraction |
Chapter10: The Human Eye and the Colourful World |
Chapter11: Electricity |
Chapter12: Magnetic Effects of Electric Current |
Chapter13: Our Environment |
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