Chemistry - Secondary school study sheets / Exam Preparation
Carbon - Carbon Structure, Allotropes of Carbon,
Carbon Dioxide & Monoxide, Carbonates, Calcium
Oxide (with Properties & Uses)
General Information
Subject: Chemistry
Topic: Carbon Structure, Allotropes of Carbon, Reactions, Carbon
Dioxide & Monoxide, Carbonates, Calcium Oxide
Grade Secondary school
Content: Compact, exam-oriented learning script with all relevant
topics, questions and sample problems.
1
,Chemistry - Secondary school study sheets / Exam Preparation
1. Structure of Carbon
1.1 Atomic structure of carbon
1.2 Properties of carbon
1.3 Uses of carbon
2. Allotropes of Carbon
3.1 Diamond: structure, hardness, insulation
3.2 Graphite: layers, conductivity, uses
3.3 Fullerene (C60): molecular shape and potential applications
3. Allotrope Review Questions
4.1 Comparison of structures and properties
4.2 Practical examples and test questions
4. Reactions of Carbon
5.1 Combustion reactions
5.2 Oxidation and reduction processes
5. Carbon and its relationship to carbon dioxide and carbon monoxide
Carbon Dioxide (CO₂)
6.1 Physical properties and structure
6.2 Role in the carbon cycle
6.3 Laboratory and industrial tests
Carbon Monoxide (CO)
7.1 Properties of Carbon Monoxide
7.2 Industrial relevance
6. Carbonates
8.1 Structure and examples (e.g., CaCO₃)
8.2 Chemical reactions and decomposition
8.3 Testing methods (limewater test, etc.)
7. Calcium Oxide (Quicklime)
9.1 Properties and uses
9.2 Testing for calcium oxide
2
,Chemistry - Secondary school study sheets / Exam Preparation
1. The structure of carbon
1. Define carbon:
Carbon is a chemical element with 6 protons, 6 neutrons and 6 electrons. Likewise, it forms a
constituent of a large number of naturally occurring substances such as coal, rocks, fossil fuels,
carbonates, and organic matter. In addition, it can be found in small amounts (approx. 0.03% by
volume) as carbon dioxide in the air.
2. Properties of carbon:
-The element of carbon C can be found in the group 4 and in the second period of the periodic
table
-Due to is position on the periodic table its usually has the tendency to form extensive networks of
covalent bonds with other elements
-Carbon is non-metal as it is non-lustrous, non-malleable, and non-ductile in nature
-Possess many different allotropes such as diamond, graphite and fullerenes
-It has a melting point of 3652 °C and boiling point of 4827 °C
-Carbon can react with oxygen to produce carbon dioxide (CO2) and carbon monoxide (CO
-Carbon does not dissolve in, or react with, water or acids
-Can both act as a reducing or oxidizing agent
3. Uses of carbon:
-Makes up for 18% of the human body. The food we eat contains an important source of energy
which we call carbohydrates. Carbohydrates are nothing but elements of carbon itself.
-Carbon in its diamond form is used in jewelry but can also be used for industrial purposes.
-Amorphous carbon is used to make inks and paints. It is also used in batteries.
-Graphite is used as the lead in your pencils. It is also used in the production of steel.
-One of the most important uses of carbon is carbon dating in which carbon can be used to
measure the age of fossils through observing a special form of carbon called Carbon-14. The
release of this carbon-14 is recorded to estimate the life of the said organic substance.
3
, Chemistry - Secondary school study sheets / Exam Preparation
2. Recognize the three allotropes of carbon and list their properties as well as uses
1. What are allotropes:
Allotropy is the existence of the same element in the same physical state in two or more different
forms (structures). In all three allotropes, the carbon atoms are joined by strong covalent bonds,
but in such different arrangements that the properties of the allotropes are very different.
2. The three main allotropes of carbon:
1. Diamond:
A diamond is one giant molecule of carbon atoms which are colorless and transparent.
Bonding structure:
Every carbon atom uses sp3 hybridization in order to bond to its neighbors by four strong covalent
bonds, leaving no free electrons and no ions with each of the other four carbon atoms.
Consequently, strong covalent bonds exist between the carbon atoms throughout the structure,
producing one single, giant, crystal molecule. The strength of bonding makes diamond very hard,
non-volatile, and resistant to melting and to chemical attack. Furthermore, since all four valence
electrons per C atom are involved in bond formation, no free (mobile) electrons are available for
conduction thus making them good insulators.
Uses:
-As diamonds are so hard and durable, their use has centered on cutting, drilling and polishing
certain objects. Very small diamond particles are embedded into saw blades, drill bits and grinding
wheels to increase their ability to cut tough materials.
-Diamond windows are made from very thin diamond membranes and used to cover openings in
lasers, vacuum chambers as well as x-ray machines.
4
Carbon - Carbon Structure, Allotropes of Carbon,
Carbon Dioxide & Monoxide, Carbonates, Calcium
Oxide (with Properties & Uses)
General Information
Subject: Chemistry
Topic: Carbon Structure, Allotropes of Carbon, Reactions, Carbon
Dioxide & Monoxide, Carbonates, Calcium Oxide
Grade Secondary school
Content: Compact, exam-oriented learning script with all relevant
topics, questions and sample problems.
1
,Chemistry - Secondary school study sheets / Exam Preparation
1. Structure of Carbon
1.1 Atomic structure of carbon
1.2 Properties of carbon
1.3 Uses of carbon
2. Allotropes of Carbon
3.1 Diamond: structure, hardness, insulation
3.2 Graphite: layers, conductivity, uses
3.3 Fullerene (C60): molecular shape and potential applications
3. Allotrope Review Questions
4.1 Comparison of structures and properties
4.2 Practical examples and test questions
4. Reactions of Carbon
5.1 Combustion reactions
5.2 Oxidation and reduction processes
5. Carbon and its relationship to carbon dioxide and carbon monoxide
Carbon Dioxide (CO₂)
6.1 Physical properties and structure
6.2 Role in the carbon cycle
6.3 Laboratory and industrial tests
Carbon Monoxide (CO)
7.1 Properties of Carbon Monoxide
7.2 Industrial relevance
6. Carbonates
8.1 Structure and examples (e.g., CaCO₃)
8.2 Chemical reactions and decomposition
8.3 Testing methods (limewater test, etc.)
7. Calcium Oxide (Quicklime)
9.1 Properties and uses
9.2 Testing for calcium oxide
2
,Chemistry - Secondary school study sheets / Exam Preparation
1. The structure of carbon
1. Define carbon:
Carbon is a chemical element with 6 protons, 6 neutrons and 6 electrons. Likewise, it forms a
constituent of a large number of naturally occurring substances such as coal, rocks, fossil fuels,
carbonates, and organic matter. In addition, it can be found in small amounts (approx. 0.03% by
volume) as carbon dioxide in the air.
2. Properties of carbon:
-The element of carbon C can be found in the group 4 and in the second period of the periodic
table
-Due to is position on the periodic table its usually has the tendency to form extensive networks of
covalent bonds with other elements
-Carbon is non-metal as it is non-lustrous, non-malleable, and non-ductile in nature
-Possess many different allotropes such as diamond, graphite and fullerenes
-It has a melting point of 3652 °C and boiling point of 4827 °C
-Carbon can react with oxygen to produce carbon dioxide (CO2) and carbon monoxide (CO
-Carbon does not dissolve in, or react with, water or acids
-Can both act as a reducing or oxidizing agent
3. Uses of carbon:
-Makes up for 18% of the human body. The food we eat contains an important source of energy
which we call carbohydrates. Carbohydrates are nothing but elements of carbon itself.
-Carbon in its diamond form is used in jewelry but can also be used for industrial purposes.
-Amorphous carbon is used to make inks and paints. It is also used in batteries.
-Graphite is used as the lead in your pencils. It is also used in the production of steel.
-One of the most important uses of carbon is carbon dating in which carbon can be used to
measure the age of fossils through observing a special form of carbon called Carbon-14. The
release of this carbon-14 is recorded to estimate the life of the said organic substance.
3
, Chemistry - Secondary school study sheets / Exam Preparation
2. Recognize the three allotropes of carbon and list their properties as well as uses
1. What are allotropes:
Allotropy is the existence of the same element in the same physical state in two or more different
forms (structures). In all three allotropes, the carbon atoms are joined by strong covalent bonds,
but in such different arrangements that the properties of the allotropes are very different.
2. The three main allotropes of carbon:
1. Diamond:
A diamond is one giant molecule of carbon atoms which are colorless and transparent.
Bonding structure:
Every carbon atom uses sp3 hybridization in order to bond to its neighbors by four strong covalent
bonds, leaving no free electrons and no ions with each of the other four carbon atoms.
Consequently, strong covalent bonds exist between the carbon atoms throughout the structure,
producing one single, giant, crystal molecule. The strength of bonding makes diamond very hard,
non-volatile, and resistant to melting and to chemical attack. Furthermore, since all four valence
electrons per C atom are involved in bond formation, no free (mobile) electrons are available for
conduction thus making them good insulators.
Uses:
-As diamonds are so hard and durable, their use has centered on cutting, drilling and polishing
certain objects. Very small diamond particles are embedded into saw blades, drill bits and grinding
wheels to increase their ability to cut tough materials.
-Diamond windows are made from very thin diamond membranes and used to cover openings in
lasers, vacuum chambers as well as x-ray machines.
4
