C3 Flashcards
Define allotropes of carbon.
Allotropes of carbon are different structural forms of carbon atoms that exist in the same physical state but have different arrangements.
Structure of Diamond?
Diamond consists of carbon atoms arranged in a tetrahedral lattice structure, with each carbon atom bonded to four other carbon atoms.
Properties of Diamond?
Diamond is the hardest known natural material, has high thermal conductivity, is transparent, and has a high refractive index
Structure of Graphene?
Graphene is a single layer of carbon atoms arranged in a two-dimensional honeycomb lattice structure.
Properties of Graphene
Graphene is the thinnest and strongest material known, conducts electricity and heat very well, and has potential applications in electronics and materials science
Structure of Buckminsterfullerene
Buckminsterfullerene is a spherical molecule composed of 60 carbon atoms arranged in a hollow cage-like structure, consisting of 20 hexagons and 12 pentagons
Properties of Buckminsterfullerene
Buckminsterfullerene is stable, conducts electricity, and has potential applications in nanotechnology, medicine, and materials science
Structure of Carbon Nanotubes?
Carbon nanotubes are cylindrical molecules composed of carbon atoms arranged in a hexagonal lattice structure, forming tubes of nanometer-scale diameter
Properties of Carbon Nanotubes?
Carbon nanotubes have high tensile strength, are excellent conductors of electricity, and have potential applications in electronics, materials science, and nanotechnology
Structure of Graphite?
Graphite consists of carbon atoms arranged in layers of hexagonal rings, with weak van der Waals forces between the layers. Each carbon atom is bonded to three other carbon atoms in the same layer.
Properties of Graphite
Graphite is soft, slippery, and a good conductor of electricity due to the presence of delocalized electrons between layers. It is used in pencils, lubricants, and as a moderator in nuclear reactors.
Definition of Covalent Bonding
Covalent bonding is the sharing of electron pairs between atoms to form molecules
How Covalent Bonds Form
Atoms share electrons to achieve a stable electron configuration, usually by filling their outermost energy level (valence shell).
Types of Elements Involved in Covalent Bonding
Covalent bonds typically form between nonmetal atoms, as they have similar electronegativities and tend to share electrons rather than transfer them.
Structure of Covalent Compounds?
Covalent compounds can have simple molecular structures (e.g., H2O, CO2) or giant covalent structures (e.g., diamond, graphite)
Characteristics of Covalent Bonds?
Covalent bonds are strong within molecules but weak between molecules. They have low melting and boiling points compared to ionic compounds.
Examples of Covalent Compounds?
Examples include water (H2O), methane (CH4), ammonia (NH3), carbon dioxide (CO2), and hydrogen chloride (HCl).
Behavior of Covalent Compounds in Water?
Covalent compounds tend to be insoluble or only slightly soluble in water, as they do not dissociate into ions when dissolved.
Definition of Ionic Bonding
Ionic bonding is the transfer of electrons from one atom to another, resulting in the formation of positively and negatively charged ions.
Types of Elements Involved in Ionic Bonding
Ionic bonds typically form between metals and nonmetals, where the metal atom loses electrons to form a positively charged cation, and the nonmetal atom gains electrons to form a negatively charged anion.
Formation of Ionic Compounds
Ionic compounds are formed by the electrostatic attraction between positively and negatively charged ions, resulting in a lattice structure.
Characteristics of Ionic Compounds
Ionic compounds have high melting and boiling points, are brittle, and conduct electricity when dissolved in water or molten state (but not in solid form).
Properties of Ionic Bonds
Ionic bonds are strong electrostatic forces of attraction between oppositely charged ions. They are non-directional and form a three-dimensional lattice structure.
Examples of Ionic Compounds
Examples include sodium chloride (NaCl), potassium iodide (KI), calcium chloride (CaCl2), magnesium oxide (MgO), and aluminum oxide (Al2O3)
