Please enable JavaScript.
Coggle requires JavaScript to display documents.
10th Grade Introductory Chemistry Solids Project (Crystalline: Solids of…
10th Grade Introductory Chemistry Solids Project
Amorphous
: Solids that have no definite shape or form.
Glass
Soda-Lime Glass: Contains added substances of sodium oxide (soda) and calcium oxide (lime). The soda lowers the melting point of the silica and the lime stabilizes the silica, allowing it to be resoftened several times, making it extremely workable.
Borosilicate Glass: Contains components of 70% silicone dioxide, 15% sodium oxide, 15% boron trioxide, and 10% calcium oxide. The boron trioxide makes the glass thermal shock resistant, meaning it able to endure extreme cold and heat. It is commonly used in chemistry labs and industrial settings, along with dishware.
Crystal Glass: The main added component of crystal glass is lead(II) oxide (PbO). The lead in the glass reduces the temperature of the glass, making it last longer under flames and therefore easier to shape. This provides a better and cleaner look to the glass. Crystal glass is commonly used in dishware.
Polymers
: Chemical compound with large molecules made of many smaller molecules of the same kind.
DNA: Short for Deoxyribonucleic Acid, DNA is the genetic material in the Eukarya Domain. The structure of DNA is a double helix.
Proteins: Made of and structured of a chain of up to 20 different amino acids. Proteins are the building blocks of tissues, enzymes, horomones, and other important body chemicals.
Crystalline
: Solids of which the components are arranged in a rigid geometric pattern.
Atomic: Atomic Solids are solids in which atoms of an element are bonded to the same type of atoms.
Metallic
: Metallic solids have two simple structures: Cubic Closest Packing, and Hexagonal Closest Packing. Metals that crystallize in Hexagonal Closest Packing are Cadmium, Cobalt, Lithium, Magnesium, Sodium, and Zinc. Metals that crystallize in Cubic Closest Packing are Silver, Aluminum, Copper, Nickel, Lead, and Platinum. These metal atoms are present at the lattice points, and are held together by delocalized covalent bonds.
Covalent Networks: Covalent network solids have covalently bonded molecules at the lattice points, which means that the elements involved are all nonmetals.
Carbon Networks
Diamond
: The molecular structure of diamond consists of a carbon atom bonded singularly with four other carbon atoms. The covalent bonds of the atoms cause the structure to be very strong, and the bonds must be broken before melting can begin. One interesting use of diamonds is in the medical field. Tiny particles of diamond, called nanodiamonds are can be attached to chemotherapy drugs to aid in the treatment of cancer. Since nanodiamonds can't be carried out by the cancer, they allow the anticancer drugs to remain inside the body, thus aiding in the battle against cancer.
Graphite
: Graphite is the most stable form of carbon, and has a structure of sheets covalently bonded together. When mixed with clay, graphite forms the lead in pencils. The reason pencils mark the paper is because the clay causes sheets of graphite to stick to the paper.
Fullerene
: A pure carbon molecule which has a structure resembling a soccerball. Fullerene contains many noble gases such as helium, neon, krypton, and xenon, which can be measured and removed from the fullerene for other uses.
Silicon Dioxide Networks:
Silicon
dioxide is found in three main crystalline forms: quartz the most abundant, tridymite, and cristobalite. Silicon dioxide can also be found naturally as a component of sand. Sand is used to make glass, and quartz is used often in jewelry and test tubes. Major characteristics include a very high melting point of roughly 1700 degrees Celsius (depending on the structure), does not conduct electricity, and is insoluble in water solvents. The structure of a silicon dioxide network is in a word, huge. The molecular geometry of silicon dioxide is AX2 (Linear 180), however as the structure continues 4 oxygen atoms surround a silicon atom forming a tetrahedral (109.5).
Group 8: The lattice points are comprised of different group 8A atoms of Noble Gases. Such examples are neon, argon, krypton, and radon. Group 8A solids are comprised of noble gases held together by London dispersion forces.
Molecular: Discrete molecules are at the lattice points of molecular crystals. They are held together by London dispersion forces when atoms or non polar molecules occupy the lattice points, dipole-dipole forces when polar molecules are at the lattice points, or hydrogen bonding in cases of FON bonded molecules at the lattice points (the latter occurs most notably in the case of water). One example of a molecular solid is ice. Dipole-Dipole and/or London Dispersion bonds hold molecular solids together
Ionic: The Ionic Solids are solids with bonds formed from oppositely charged ions. They also have structures of repeating arrays known as crystal lattices. These lattices can form different patterns of crystal packing, which is when the ions line up into a pattern, packed in side by side: Simple Cubic Packing, Body-Centered Cubic, Hexagonal Packing, and Cubic Close-Packed Arrangement. Ionic bonds hold these solids together.
