Grade 9
  1. Matter and its nature  1.1. Introduction to matter  1.2. Physical and chemical properties of matter  1.3. States of matter  1.3.1. Solid state  1.3.2. Fluid state  1.3.3. Gaseous state  1.3.4. Plasma and Bose–Einstein condensate  1.4. Changes in the states of matter  1.4.1. Melting and freezing  1.4.2. Evaporation and Condensation  1.4.3. Sublimation and deposition  1.5. Classification of matter  1.6. Elements, Compounds, and Mixtures  1.7. Pure substances and impurities  1.8. Separation Techniques  1.8.1. Filtration  1.8.2. Distillation  1.8.3. Crystallization  1.8.4. Chromatography  1.8.5. Centrifugation  1.8.6. Sublimation  1.8.7. Decantation and sedimentation
  2. Atomic Structure  2.1. Discovery of atoms  2.2. Dalton's atomic theory  2.3. Structure of the atom  2.4. Subatomic particles  2.5. Atomic number and mass number  2.6. Isotopes and Isobars  2.7. Electronic configuration  2.8. Bohr's atomic model  2.9. Modern Atomic Model (Quantum Mechanical Model - Introduction)  2.10. Valency and chemical bonding
  3. C hemical reactions and equations  3.1. Introduction to Chemical Reactions  3.2. Chemical Equation Formulation  3.3. Balancing Chemical Equations  3.4. Types of Chemical Reactions  3.4.1. Combination Reactions  3.4.2. Decomposition reactions  3.4.3. Displacement reactions  3.4.4. Double displacement reactions  3.4.5. Redox reactions  3.4.6. Endothermic and Exothermic Reactions  3.5. Effects of chemical reactions  3.6. Energy Changes in Chemical Reactions  3.7. Catalysts and their role in reactions
  4. Periodic table and periodicity  4.1. History of Periodic Classification  4.2. Mendeleev's periodic table  4.3. Modern Periodic Table  4.4. Periods and groups in the periodic table and periodicity  4.5. Trends in the Periodic Table  4.5.1. Atomic size  4.5.2. Ionization Energy  4.5.3. Electron affinity  4.5.4. Electronegativity  4.5.5. Metallic and Non-Metallic Properties  4.6. Noble gases and their properties
  5. Chemical bond  5.1. Introduction to Chemical Bonding  5.2. Types of chemical bonds  5.2.1. Ionic bond  5.2.2. Covalent bond  5.2.3. Metallic bond  5.2.4. Hydrogen bonding  5.2.5. Van der Waals force  5.3. Properties of Ionic and Covalent Compounds  5.4. Molecular Structure and Geometry (VSEPR Theory - Basics)
  6. Acids, Bases and Salts  6.1. Introduction to Acids and Bases  6.2. Properties of Acids  6.3. Properties of bases  6.4. pH scale and its importance  6.5. Indicators and their uses  6.6. Neutralization reactions  6.7. Strength of Acids and Bases (Strong vs. Weak)  6.8. Preparation of salts  6.9. Uses of acids, bases and salts in daily life
  7. Metals and Nonmetals  7.1. Physical Properties of Metals  7.2. Physical Properties of Nonmetals  7.3. Chemical properties of metals  7.4. Chemical Properties of Nonmetals  7.5. Reactivity Series of Metals  7.6. Extraction of metals  7.7. Corrosion and its prevention  7.8. uses of metals and nonmetals
  8. Carbon and its compounds  8.1. Introduction to Carbon  8.2. Allotropes of carbon (diamond, graphite, fullerene)  8.3. Hydrocarbons  8.3.1. Hydrocarbons  8.3.2. Alkene  8.3.3. Alkynes  8.4. Functional groups in organic chemistry  8.5. Isomerism in organic compounds  8.6. Alcohols and Carboxylic Acids  8.7. Soaps and detergents  8.8. Polymers (Introduction to Natural and Synthetic Polymers)
  9. Solutions and Mixtures  9.1. Types of mixtures  9.2. Homogeneous and Heterogeneous Mixtures  9.3. Concentration of solutions  9.4. Solubility and factors affecting solubility  9.5. Suspensions and Colloids  9.6. Saturated, unsaturated and supersaturated solutions
  10. Air and atmosphere  10.1. Composition of air  10.2. Role of gases in the atmosphere  10.4. Acid rain and its effects  10.5. Greenhouse effect and global warming  10.6. Ozone layer and its depletion  10.7. Air pollution control measures
  11. Water and its importance  11.1. Composition and properties of water  11.2. Hardness of water (temporary and permanent hardness)  11.3. Causes of water pollution  11.4. Effects of Water Pollution  11.5. Water purification methods (filtration, boiling, chlorination)
  12. Industrial Chemistry  12.1. Introduction to Industrial Chemistry  12.2. Important industrial chemicals (sulfuric acid, ammonia, sodium hydroxide)  12.3. Chemical processes in industry  12.4. Uses of Industrial Chemistry in Daily Life  12.5. Environmental impact of industrial chemical processes

Grade 9 → Carbon and its compounds ↓


Introduction to Carbon


Carbon is an essential element in chemistry, known for its versatile nature. It is the backbone of all life forms on Earth and forms many more compounds than any other element. In this document, we will explore the basics of carbon, its importance, properties, and some of the common compounds it forms.

Elemental carbon

Carbon is a chemical element with the symbol C and atomic number 6 It belongs to group 14 of the periodic table. Carbon is a nonmetal and is known for its ability to form strong bonds with other carbon atoms, leading to the formation of various complex structures. This unique bonding ability is important for its role in chemistry and biology.

Properties of carbon

Carbon has several allotropes, which are different forms of the same element. These allotropes include:

  • Diamond: In diamond, each carbon atom is bonded to four other carbon atoms in a tetrahedral structure. This arrangement gives diamond its famous hardness.
  • Graphite: The carbon atoms in graphite are bonded in flat hexagonal structures. Graphite is soft and slippery, which is why it is used as a lubricant and in pencils.
  • Fullerenes: These are molecules composed entirely of carbon that take the shape of hollow spheres, ellipsoids, or tubes. A well-known example is the buckyball, C60.

Visual example of carbon structures

Diamond Lead Fullerenes

Importance of carbon

Carbon is vital for the existence of life. It forms the basis of organic chemistry because it can form stable bonds with many elements, including hydrogen, oxygen, nitrogen, and others. Carbon's ability to form chains and rings is the basis for the structure of carbohydrates, proteins, lipids, and nucleic acids.

Examples of carbon compounds

Carbon forms millions of known compounds. Here are some of the major compounds:

  • Methane (CH4): The simplest hydrocarbon and an important fuel source.
  • Carbon dioxide (CO2): Gas important for photosynthesis in plants and a greenhouse gas.
  • Ethanol (C2H5OH): Used in biofuels and alcoholic beverages.

Chemical bonding in carbon compounds

Carbon atoms form covalent bonds by sharing electron pairs with other atoms. Typical bonding patterns are as follows:

  • Single bond: In a single bond, a pair of electrons is shared between two atoms. Example: In CH4, each hydrogen is singly bonded to a carbon.
  • Double bond: Two pairs of electrons are shared, as in ethylene (C2H4).
  • Triple bond: Three pairs of electrons are shared, as in acetylene (C2H2).

Visual example of bonding

Single bond (CH) Double bond (C=C) Triple bond (C≡C)

The versatility of carbon

Carbon's ability to join in different ways is called catenation. This produces an incredible variety of carbon-based molecules. This versatility is unmatched by any other element, which is why organic chemistry is sometimes called the chemistry of carbon compounds.

Functional groups in carbon compounds

In organic chemistry, functional groups are specific groups of atoms within molecules that determine the chemical properties of those molecules. Some common functional groups include:

  • Hydroxyl group (-OH): Found in alcohols.
  • Carboxyl group (-COOH): Present in carboxylic acids such as vinegar.
  • Amino group (-NH2): A major component of amino acids, the building blocks of proteins.

Visual example of functional groups

Hydroxyl group (-OH) Carboxyl group (-COOH) Amino group (-NH2)

The role of carbon in the environment

Carbon plays an important role in the carbon cycle, which is the process by which carbon is exchanged between the Earth's oceans, soil, rocks, and atmosphere. This cycle is important for maintaining the balance of carbon and supporting life on Earth. Some of the processes involved in the carbon cycle are:

  • Photosynthesis: Plants absorb carbon dioxide (CO2) from the atmosphere and convert it into oxygen and glucose during photosynthesis.
  • Respiration: Animals and plants release carbon back into the atmosphere as carbon dioxide through respiration.
  • Combustion: The burning of fossil fuels releases stored carbon into the atmosphere as CO2.

Conclusion

Carbon is a remarkable element because of its extensive bonding capabilities and presence in thousands of different compounds. Its role in the chemistry of life, the environment, and industrial processes makes it one of the most important elements on the periodic table. Understanding its properties and behaviors helps us understand the vast world of chemistry and the complex balance of the environment.


Grade 9 → 8.1


U
username
0%
completed in Grade 9

← Prev (8)
Carbon and its compounds
Next (8.2) →
Allotropes of carbon (diamond, graphite, fullerene)

Comments 



Introduction to Carbon

https://www.chemistryelite.com/g9/8.1?ceal=en