Podcast
Questions and Answers
What is formed between atoms by the sharing of a pair of electrons?
What is formed between atoms by the sharing of a pair of electrons?
A covalent bond
Where does covalent bonding usually occur?
Where does covalent bonding usually occur?
In most non-metallic elements and compounds of nonmetals
What is the nature of the bonds formed when atoms share electrons?
What is the nature of the bonds formed when atoms share electrons?
Strong
Covalent bonds are the result of electrostatic attractions between the positively charged nuclei of the atoms and the pairs of negative electrons that are shared between them.
Covalent bonds are the result of electrostatic attractions between the positively charged nuclei of the atoms and the pairs of negative electrons that are shared between them.
Which of the following molecules are examples of diatomic molecules?
Which of the following molecules are examples of diatomic molecules?
Which of the following are considered inorganic molecules?
Which of the following are considered inorganic molecules?
Which of the following are organic molecules containing up to two carbon atoms?
Which of the following are organic molecules containing up to two carbon atoms?
Substances that consist of small molecules are typically gases or liquids with low boiling and melting points.
Substances that consist of small molecules are typically gases or liquids with low boiling and melting points.
What type of forces are responsible for the attraction between small molecules?
What type of forces are responsible for the attraction between small molecules?
Substances that consist of small molecules can conduct electricity.
Substances that consist of small molecules can conduct electricity.
As the relative molecular mass of substances with simple molecular structures increases, their melting and boiling points tend to increase.
As the relative molecular mass of substances with simple molecular structures increases, their melting and boiling points tend to increase.
Substances with giant covalent structures are typically solids with very high melting points.
Substances with giant covalent structures are typically solids with very high melting points.
All atoms in giant covalent structures are linked to other atoms by strong covalent bonds.
All atoms in giant covalent structures are linked to other atoms by strong covalent bonds.
What property must be overcome to melt or boil substances with giant covalent structures?
What property must be overcome to melt or boil substances with giant covalent structures?
How many other carbon atoms is each carbon atom in diamond joined to?
How many other carbon atoms is each carbon atom in diamond joined to?
Diamond conducts electricity.
Diamond conducts electricity.
How many other carbon atoms is each carbon atom in graphite bonded to?
How many other carbon atoms is each carbon atom in graphite bonded to?
The layers in graphite are held together by strong covalent bonds.
The layers in graphite are held together by strong covalent bonds.
Graphite is slippery because of the weak intermolecular forces between its layers.
Graphite is slippery because of the weak intermolecular forces between its layers.
One electron from each carbon atom in graphite is delocalized.
One electron from each carbon atom in graphite is delocalized.
Graphite is a good conductor of electricity.
Graphite is a good conductor of electricity.
Diamond is a good conductor of electricity.
Diamond is a good conductor of electricity.
What form of carbon is a single layer of graphite?
What form of carbon is a single layer of graphite?
Fullerenes are molecules of carbon atoms with hollow shapes.
Fullerenes are molecules of carbon atoms with hollow shapes.
The structure of fullerenes is based entirely on hexagonal rings of carbon atoms.
The structure of fullerenes is based entirely on hexagonal rings of carbon atoms.
What is the name of the first fullerene discovered?
What is the name of the first fullerene discovered?
What are cylindrical fullerenes known as?
What are cylindrical fullerenes known as?
Covalent compounds typically conduct electricity.
Covalent compounds typically conduct electricity.
Which of the following are exceptions to the rule that covalent compounds do not conduct electricity?
Which of the following are exceptions to the rule that covalent compounds do not conduct electricity?
Flashcards
Covalent bond
Covalent bond
A type of bond formed when two atoms share a pair of electrons. It's commonly seen in non-metallic elements and compounds. These shared electron pairs create strong bonds between atoms.
Electrostatic attraction in covalent bonding
Electrostatic attraction in covalent bonding
The electrostatic attraction between the positive nuclei of atoms and the negatively charged shared electron pairs within a covalent bond.
Dot-and-cross diagrams
Dot-and-cross diagrams
A diagram that uses dots and crosses to represent the shared electrons in a covalent bond. It helps visualize the sharing arrangement of atoms.
Diatomic molecule
Diatomic molecule
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Inorganic molecule
Inorganic molecule
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Organic molecule
Organic molecule
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Substances with simple molecular structures
Substances with simple molecular structures
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Intermolecular forces
Intermolecular forces
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Melting and boiling points relationship with molecular mass
Melting and boiling points relationship with molecular mass
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Giant covalent structures
Giant covalent structures
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Diamond
Diamond
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Graphite
Graphite
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Graphene
Graphene
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Fullerenes
Fullerenes
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Carbon nanotubes
Carbon nanotubes
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Electrical conductivity of covalent compounds
Electrical conductivity of covalent compounds
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Study Notes
Covalent Bonding
- A covalent bond forms when atoms share a pair of electrons.
- Covalent bonding is common in non-metals and their compounds.
- The shared electrons are attracted to the positively charged nuclei of both atoms, creating a strong bond.
- Dot-and-cross diagrams represent covalent bonds, showing the arrangement of shared electrons.
Examples of Covalent Molecules
- Diatomic molecules (e.g., Hâ‚‚, Oâ‚‚, Nâ‚‚, halogens)
- Hydrogen halides (e.g., HCl)
- Inorganic molecules (e.g., H₂O, NH₃, CO₂)
- Organic molecules (e.g., methane, ethane, ethene)
Properties of Simple Molecular Substances
- Gases or liquids at room temperature due to weak intermolecular forces.
- Low melting and boiling points as intermolecular forces are easily overcome.
- Do not conduct electricity as they have no overall charge.
- Intermolecular forces increase with increasing molecular size, thus increasing melting and boiling points.
Properties of Giant Covalent Structures
- Solids with very high melting and boiling points.
- Strong covalent bonds between atoms.
- Do not conduct electricity usually, except graphite and graphene.
Diamond Structure
- Each carbon atom forms four covalent bonds with neighbouring carbon atoms.
- Very hard and high melting point due to strong covalent bonds.
- Does not conduct electricity.
Graphite Structure
- Carbon atoms form layers of hexagonal rings.
- Weak forces between layers allow them to slide, making graphite soft and slippery.
- Conduct electricity due to delocalised electrons.
Fullerene Structure
- Carbon atoms form closed cages or tubes, e.g., Buckminsterfullerene (C₆₀).
- Different properties, and nanotechnological uses because of shape and size.
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