| Substances where every atom is linked to other atoms by strong covalent bonds. | Giant Covalent Structures |
| What are substances called where every atom is linked to other atoms by strong covalent bonds? | These substances have giant covalent structures. |
| Chemical bonds formed by the sharing of electron pairs between atoms. | Covalent Bonds |
| What type of bonds hold atoms together in giant covalent structures? | Lots of strong covalent bonds hold atoms together in giant covalent structures. |
| The temperatures at which substances change state from solid to liquid (melting) or liquid to gas (boiling). | Melting and Boiling Points |
| What property do giant covalent substances typically have due to the strong covalent bonds? | Therefore giant covalent substances have very high melting and boiling points. |
| Why do giant covalent substances typically have high melting and boiling points? | It takes a lot of energy to overcome all of the covalent bonds in giant covalent structures. |
| A form of carbon in which each carbon atom is covalently bonded to four other carbon atoms in a three-dimensional lattice structure. | Diamond |
| What is an example of a substance with a giant covalent structure? | Diamond is an example of a giant covalent structure. |
| A form of carbon in which each carbon atom is covalently bonded to three other carbon atoms in flat layers. | Graphite |
| What is another example of a substance with a giant covalent structure, besides diamond? | Graphite is another example of a substance with a giant covalent structure. |
| A chemical element with the symbol C and atomic number 6. | Carbon |
| What elements are found in both diamond and graphite? | Diamond and graphite both contain covalently bonded carbon atoms, as they are two different forms of carbon. |
| A form of carbon in which each carbon atom is covalently bonded to four other carbon atoms in a three-dimensional lattice structure. | Diamond |
| What is the structure of diamond? | Diamond has a giant covalent structure made of carbon atoms. |
| Chemical bonds formed by the sharing of electron pairs between atoms, resulting in a stable molecular structure. | Strong Covalent Bonds |
| What type of bonds hold carbon atoms together in diamond? | Each carbon atom in diamond forms 4 strong covalent bonds with other carbon atoms. |
| The resistance of a material to deformation, indentation, or scratching. | Hardness |
| What property does diamond possess due to its strong covalent bonds? | The strong covalent bonds in diamond make it very hard. |
| The temperatures at which substances change state from solid to liquid (melting) or liquid to gas (boiling). | Melting and Boiling Points |
| Why does diamond have a very high melting and boiling point? | It takes lots of energy to overcome the strong covalent bonds in diamond, so it also has a very high melting and boiling point. |
| The ability of a material to conduct electricity. | Electrical Conductivity |
| Does diamond conduct electricity? Why or why not? | Diamond doesn't conduct electricity because there are no charged particles that are free to move. |
| Instruments or machines used for cutting, shaping, or removing material from a workpiece. | Cutting Tools |
| Why is diamond used in cutting tools? | Diamond is used in cutting tools because it's so hard that it can easily cut most other substances. |
| A form of carbon in which each carbon atom is covalently bonded to three other carbon atoms in flat layers. | Graphite |
| What is the structure of graphite? | Graphite is another giant covalent structure made of carbon atoms. |
| Chemical bonds formed by the sharing of electron pairs between atoms. | Covalent Bonds |
| How many covalent bonds does each carbon atom in graphite form with other carbon atoms? | Each carbon atom in graphite forms 3 covalent bonds with other carbon atoms. |
| A ring-like structure composed of six carbon atoms arranged in a hexagonal shape. | Hexagonal Rings |
| How are the carbon atoms arranged in graphite? | The atoms in graphite are arranged in layers of hexagonal rings. |
| Forces of attraction between molecules. | Intermolecular Forces |
| What type of forces exist between the layers of graphite? | There are no covalent bonds between the layers of graphite, only weak intermolecular forces. |
| The property of a material to be easily compressed, shaped, or deformed. | Softness |
| What property of graphite makes it soft and slippery? | The ability of the layers of graphite to easily slide over each other due to weak intermolecular forces makes graphite soft and slippery. |
| A substance used to reduce friction between surfaces in contact with each other. | Lubricant |
| Why is graphite useful as a lubricant? | The layers of graphite can easily slide over each other due to weak intermolecular forces, making graphite soft and slippery, thus useful as a lubricant. |
| Electrons in a molecule, ion, or solid metal that are not associated with a single atom or covalent bond, but instead are free to move throughout the structure. | Delocalised Electrons |
| Why can graphite conduct electricity? | Graphite can conduct electricity because it has delocalised electrons. |
| The outermost energy level of an atom, containing the electrons involved in forming bonds with other atoms. | Outer Shell |
| How many electrons does a carbon atom have in its outer shell? | A carbon atom has 4 electrons in its outer shell. |
| Chemical bonds formed by the sharing of electron pairs between atoms. | Covalent Bonds |
| Why are there no free electrons in diamond? | Every carbon atom in diamond forms 4 covalent bonds, so there are no free electrons. |
| The internal energy of an object due to the kinetic energy of its atoms and/or molecules. | Thermal Energy |
| Why is there one free electron in graphite? | In graphite each carbon atom only forms 3 covalent bonds, so they each have 1 free electron. |
| How does the presence of delocalised electrons in graphite affect its ability to conduct heat? | Delocalised electrons can transfer thermal energy, so graphite is a good conductor of heat. |
| A property of matter that causes it to experience a force when placed in an electromagnetic field. | Electric Charge |
| How do delocalised electrons contribute to the conductivity of graphite? | Delocalised electrons can carry an electric charge, making graphite a good conductor of electricity. |
| Conductive materials used to make electrical contacts with non-metallic parts of a circuit. | Electrodes |
| How is graphite used in electronics? | Graphite is useful in making electrodes due to its ability to conduct electricity. |
| A single layer of carbon atoms arranged in a two-dimensional honeycomb lattice structure. | Graphene |
| What is graphene? | Graphene is a single layer of graphite. |
| Having relatively little weight; not heavy. | Lightweight |
| What is one of the notable characteristics of graphene? | Graphene is very light and strong. |
| Having only length and width, with no thickness. | Two-Dimensional |
| How many dimensions does graphene typically have? | Graphene is two-dimensional. |
| The ability of a material to withstand an applied force without yielding or fracturing. | Strength |
| How does the arrangement of carbon atoms in graphene contribute to its strength? | Each carbon atom in graphene forms 3 covalent bonds, contributing to its strength. |
| The ability of a material to conduct electrical current. | Electrical Conductivity |
| How does the presence of delocalised electrons in graphene affect its electrical properties? | Like graphite, graphene is a good conductor of heat and electricity due to its delocalised electrons. |
| Materials made from two or more constituent materials with significantly different physical or chemical properties that, when combined, produce a material with characteristics different from the individual components. | Composite Materials |
| What are materials created by adding graphene to metals, polymers, and ceramics called? | The materials created are called composites. |
| Covalent structures with hollow shapes, typically consisting of rings of carbon atoms. | Fullerenes |
| What are fullerenes? | Fullerenes are covalent structures with hollow shapes, typically consisting of rings of carbon atoms. |
| A molecular structure consisting of atoms arranged in a closed loop or ring. | Ring Structure |
| What are fullerene structures based on? | Fullerene structures are based on rings of carbon atoms. |
| A ring structure consisting of six carbon atoms bonded together in a hexagonal shape. | Hexagonal Ring |
| What is the typical composition of a carbon ring in a fullerene structure? | Each ring usually contains 6 carbon atoms, forming a hexagonal ring. But some fullerenes contain rings with 5 or 7 carbon atoms. |
| A type of fullerene with a spherical shape, containing 60 carbon atoms. | Buckminsterfullerene (C60) |
| Which fullerene was the first to be discovered? | Buckminsterfullerene (C60) was the first fullerene to be discovered. |
| Molecules composed entirely of carbon, usually in the form of hollow spheres, ellipsoids, or tubes. | Fullerenes |
| What properties make fullerenes useful in strengthening materials? | Fullerenes are light and strong, allowing them to strengthen materials without adding much weight. |
| Electrons that are not associated with a single atom or covalent bond but instead are free to move throughout the structure. | Delocalised Electrons |
| How do delocalised electrons contribute to the conductivity of heat and electricity in fullerenes? | Delocalised electrons in fullerenes allow them to conduct heat and electricity effectively. |
| The ratio of the surface area of an object to its volume. | Surface Area to Volume Ratio |
| How does the high surface area to volume ratio of fullerenes make them useful as catalysts? | The high surface area to volume ratio of fullerenes makes them effective catalysts because more reactive sites are available for chemical reactions. |
| Forces of attraction or repulsion between molecules. | Intermolecular Forces |
| How do weak intermolecular forces contribute to the usefulness of fullerenes as lubricants? | Weak intermolecular forces between fullerene molecules make them slippery, making them effective as lubricants. |
