Carbon has 4 main allotropes - graphite, diamond, fullerene, and graphene. It is the chemical element with atomic number 6 and is a nonmetal. Carbon is widely found in nature and living organisms. Its allotropes have varying properties - diamond is the hardest material, graphite is an electrical conductor, fullerenes are spherical structures, and graphene is a strong two-dimensional material.
Carbon belongs to the group IV of the periodic table.
It has four electrons in its outermost orbit, so its valency is four.
Carbon is a non-metal.
Why so many Carbon Compounds in nature
Because carbon is chemically unique.
Only carbon atoms have the ability to combine with themselves to form long chains
The number of carbon compounds is larger than that of all other elements put together.
Occurrence of carbon
The name ‘carbon’ is derived from the Latin
word ‘carbo’ meaning coal. Carbon is found in
nature in free as well as compound state. Carbon in
the free state is found as diamond and graphite, and
in the combined state in the following compounds.
1. As carbon dioxide and in the form of carbonates
such as calcium carbonate, marble, calamine
(ZnCO3)
2. Fossil fuel – coal, petroleum, natural gas
3. Carbonaceous nutrients – carbohydrates,
proteins, fats
4. Natural fibres – cotton, wool, silk
Properties of carbon
Allotropic nature of Carbon
Allotropy - Some elements occur in nature in more than one form. The chemical properties
of these different forms are the same but their physical properties are different. This
property of elements is called allotropy. Like carbon, sulphur and phosphorus also exhibit
allotropy.
Allotropes of carbon
A. Crystalline forms
1. A crystalline form has a regular and definite arrangement of atoms.
2. They have high melting points and boiling points.
3. A crystalline form has a definite geometrical shape, sharp edges and plane surfaces.
* CARBON is the chemical element with symbol C and atomic number 6. As a member of group IV on the periodic table, it is nonmetallic and tetravalent—making four electrons available to form covalent chemical bonds.
* Bonding in Carbon-Covalent Bond
* Allotropes of Carbon
* Graphite
* Diamond
* Fullerenes
* Organic Chemistry
* Isomerism
* Soaps
Carbon belongs to the group IV of the periodic table.
It has four electrons in its outermost orbit, so its valency is four.
Carbon is a non-metal.
Why so many Carbon Compounds in nature
Because carbon is chemically unique.
Only carbon atoms have the ability to combine with themselves to form long chains
The number of carbon compounds is larger than that of all other elements put together.
Occurrence of carbon
The name ‘carbon’ is derived from the Latin
word ‘carbo’ meaning coal. Carbon is found in
nature in free as well as compound state. Carbon in
the free state is found as diamond and graphite, and
in the combined state in the following compounds.
1. As carbon dioxide and in the form of carbonates
such as calcium carbonate, marble, calamine
(ZnCO3)
2. Fossil fuel – coal, petroleum, natural gas
3. Carbonaceous nutrients – carbohydrates,
proteins, fats
4. Natural fibres – cotton, wool, silk
Properties of carbon
Allotropic nature of Carbon
Allotropy - Some elements occur in nature in more than one form. The chemical properties
of these different forms are the same but their physical properties are different. This
property of elements is called allotropy. Like carbon, sulphur and phosphorus also exhibit
allotropy.
Allotropes of carbon
A. Crystalline forms
1. A crystalline form has a regular and definite arrangement of atoms.
2. They have high melting points and boiling points.
3. A crystalline form has a definite geometrical shape, sharp edges and plane surfaces.
* CARBON is the chemical element with symbol C and atomic number 6. As a member of group IV on the periodic table, it is nonmetallic and tetravalent—making four electrons available to form covalent chemical bonds.
* Bonding in Carbon-Covalent Bond
* Allotropes of Carbon
* Graphite
* Diamond
* Fullerenes
* Organic Chemistry
* Isomerism
* Soaps
Myself being as a class 10 CBSE student; I understand the difficulties faced by the students.
so refer this presentation to have a well understanding over a difficult chapter.
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Allotropes of carbon
Carbon is capable of forming many allotropes due to its valency. Well known forms of carbon include diamond and graphite. In recent decades many more allotropes and forms of carbon have been discovered and researched including ball shapes such as buckminsterfullerene and sheets such as graphene. Larger scale structures of carbon include nanotubes, nanobuds and nanoribbons. Other unusual forms of carbon exist at very high temperature or extreme pressures.
Formation of covalent bonds
Formulas of molecular compounds
LEWIS STRUCTURE
Molecules of Elements
Molecules of Compounds
Non-Polar Covalent Bond
Polar Covalent Bond
Uses of Covalent bonds Real life application
Myself being as a class 10 CBSE student; I understand the difficulties faced by the students.
so refer this presentation to have a well understanding over a difficult chapter.
PLEASE DO FOLLOW ME FOR FURTHER UPDATES!!
Allotropes of carbon
Carbon is capable of forming many allotropes due to its valency. Well known forms of carbon include diamond and graphite. In recent decades many more allotropes and forms of carbon have been discovered and researched including ball shapes such as buckminsterfullerene and sheets such as graphene. Larger scale structures of carbon include nanotubes, nanobuds and nanoribbons. Other unusual forms of carbon exist at very high temperature or extreme pressures.
Formation of covalent bonds
Formulas of molecular compounds
LEWIS STRUCTURE
Molecules of Elements
Molecules of Compounds
Non-Polar Covalent Bond
Polar Covalent Bond
Uses of Covalent bonds Real life application
Carbon being the most versatile element on this earth is also the most important element for mankind. Carbon (from Latin: carbo "coal") is a chemical element with the symbol C and atomic number 6. It is nonmetallic and tetravalent—making four electrons available to form covalent chemical bonds. It belongs to group 14 of the periodic table. Carbon makes up only about 0.025 percent of Earth's crust.
This presentation is prepared in view of engineering chemistry syllabus. It is useful for Engineering, Sciences and their research to understand basics of chemistry.
Carbon is unique among the elements because its atoms can form an endless variety of molecules with an endless variety of sizes, shapes, and chemical properties.
Carbon part 1
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Richard's aventures in two entangled wonderlandsRichard Gill
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Professional air quality monitoring systems provide immediate, on-site data for analysis, compliance, and decision-making.
Monitor common gases, weather parameters, particulates.
Slide 1: Title Slide
Extrachromosomal Inheritance
Slide 2: Introduction to Extrachromosomal Inheritance
Definition: Extrachromosomal inheritance refers to the transmission of genetic material that is not found within the nucleus.
Key Components: Involves genes located in mitochondria, chloroplasts, and plasmids.
Slide 3: Mitochondrial Inheritance
Mitochondria: Organelles responsible for energy production.
Mitochondrial DNA (mtDNA): Circular DNA molecule found in mitochondria.
Inheritance Pattern: Maternally inherited, meaning it is passed from mothers to all their offspring.
Diseases: Examples include Leber’s hereditary optic neuropathy (LHON) and mitochondrial myopathy.
Slide 4: Chloroplast Inheritance
Chloroplasts: Organelles responsible for photosynthesis in plants.
Chloroplast DNA (cpDNA): Circular DNA molecule found in chloroplasts.
Inheritance Pattern: Often maternally inherited in most plants, but can vary in some species.
Examples: Variegation in plants, where leaf color patterns are determined by chloroplast DNA.
Slide 5: Plasmid Inheritance
Plasmids: Small, circular DNA molecules found in bacteria and some eukaryotes.
Features: Can carry antibiotic resistance genes and can be transferred between cells through processes like conjugation.
Significance: Important in biotechnology for gene cloning and genetic engineering.
Slide 6: Mechanisms of Extrachromosomal Inheritance
Non-Mendelian Patterns: Do not follow Mendel’s laws of inheritance.
Cytoplasmic Segregation: During cell division, organelles like mitochondria and chloroplasts are randomly distributed to daughter cells.
Heteroplasmy: Presence of more than one type of organellar genome within a cell, leading to variation in expression.
Slide 7: Examples of Extrachromosomal Inheritance
Four O’clock Plant (Mirabilis jalapa): Shows variegated leaves due to different cpDNA in leaf cells.
Petite Mutants in Yeast: Result from mutations in mitochondrial DNA affecting respiration.
Slide 8: Importance of Extrachromosomal Inheritance
Evolution: Provides insight into the evolution of eukaryotic cells.
Medicine: Understanding mitochondrial inheritance helps in diagnosing and treating mitochondrial diseases.
Agriculture: Chloroplast inheritance can be used in plant breeding and genetic modification.
Slide 9: Recent Research and Advances
Gene Editing: Techniques like CRISPR-Cas9 are being used to edit mitochondrial and chloroplast DNA.
Therapies: Development of mitochondrial replacement therapy (MRT) for preventing mitochondrial diseases.
Slide 10: Conclusion
Summary: Extrachromosomal inheritance involves the transmission of genetic material outside the nucleus and plays a crucial role in genetics, medicine, and biotechnology.
Future Directions: Continued research and technological advancements hold promise for new treatments and applications.
Slide 11: Questions and Discussion
Invite Audience: Open the floor for any questions or further discussion on the topic.
2. • carbon is from the Latin word “carbo” meaning charcoal.
• It was first recognized as an element in the
second half of the 18th centaury name
A.L Lavoisier proposed carbon in 1789.
• Found naturally both can also be created
Artificially
• Carbon is found in the atmosphere inside the earths crust
And in all living organisms.
• Carbon is present in fuel like wood, charcoal, coke petroleum,
gas biogas etc.
3. Carbon is the chemical element with symbol c
and the atomic number 6. as a member of
group 14 on the periodic table, it is
non-metallic and tetravalent- making
four electron available to form covalent
chemical bonds. There are three naturally
occurring isotopes with c12 and c13 being
stable while c14 is radioactive.
4. • Allotropes are different forms
of the same element in the
same physical state.
Carbon has 4-allotropes-
• graphite
• diamond
• fullerene
• graphene.
5. • Each carbon atom is covalently bonded to 4 others,
tetrahedrally arranged in regular
repeating pattern with bond
Angles of 109.5
• It is the hardest known natural substance.
• Density: 3.51g cm per cube.
6. • All electrons are bonded’ non conductor
of electricity.
• Lustrous crystal
• Polished for jewelry and
ornamentation; Used in tools and
machinery for grinding and cutting glass
7. • each carbon atom is bonded in a sphere of 60 carbon atoms,
consisting of 12 pentagons and 20 hexagons.
• The structure is closed spherical cage in which each carbon is
bonded to 3 others.
8. • density: 1.72g cm per cube
• Easily accepts electron to form ions.
• Yellow crystalline solid
• Reacts with K to make superconducting crystalline material;
related forms are used to make nanotubes for the electronics
industry catalysts and lubricants.
9.
10. • Graphene is an allotrope of carbon in the form of a two
dimensional, atomic-scale, honey-comb lattice.
• Graphene is the strongest material ever found, it is more than
40 times stronger than diamond.
• Graphene is rigid and perfect thermal conductor.
• Graphene has a large number of application in optical
electronics, ultra filtration, super capacitors.
11.
12. • Unlike diamond, graphite is an
electrical conductor.
• The most stable form of
carbon.
• Graphite powder is used as a
dry lubricant.