Log in. Study now. See Answer. Best Answer. Study guides. Chemistry 20 cards. How does a buffer work. What happens in a neutralization reaction. What is a conjugate acid-base pair. Why is water considered to be neutral. Physics 20 cards. Which term explains whether an object's velocity has increased or decreased over time. Which of these is a characteristic of nonmetals. What is the only factor needed to calculate change in velocity due to acceleration of gravity 9.
What term is used to describe splitting a large atomic nucleus into two smaller ones. Vaping Study Guide 3 cards. Propylene Glycol. Q: What forces are associated with solids? Write your answer Related questions. Which forces are associated with solids? What forces hold molecular solids together?
Why can liquids change shape but solids cannot? What forces hold molecular solids? What forces holds molecular solids together? What kind of forces hold molecular solids together?
Which type of motion is associated with solids? What forces hold ionic solids together? Why do molecular solids have lower boiling points than ionic solids? A crystalline solid can be represented by its unit cell, which is the smallest identical unit that when stacked together produces the characteristic three-dimensional structure. Solids are characterized by an extended three-dimensional arrangement of atoms, ions, or molecules in which the components are generally locked into their positions.
The components can be arranged in a regular repeating three-dimensional array. The smallest repeating unit of a crystal lattice is the unit cell. The major types of solids are ionic, molecular, covalent, and metallic. Ionic solids consist of positively and negatively charged ions held together by electrostatic forces; the strength of the bonding is reflected in the lattice energy.
Ionic solids tend to have high melting points and are rather hard. Molecular solids are held together by relatively weak forces, such as dipole—dipole interactions, hydrogen bonds, and London dispersion forces. Metallic solids have unusual properties. Type of Solid Forms of Unit Particles Forces Between Particles Properties Examples Molecular Atoms of molecules London dispersion, dipole-dipole forces, hydrogen bonds Fairly soft, low to moderately high melting point, poor thermal and electrical conduction Argon, methane, sucrose, dry ice Covalent-network Atoms connected in a network of covalent bonds Covalent bonds Very hard, very high melting point, often poor thermal and electrical conduction Diamond, quartz Ionic Positive and negative ions Electrostatic attractions Hard and brittle, high melting point, poor thermal and electrical conduction Typical salts Metallic atoms Metallic bonds Soft to very hard, low to very high melting point, excellent thermal and electrical conduction, malleable and ductile All metallic elements Assumes the shape of the portion of the container it occupies Does not expand to fill container Is virtually incompressible Diffusion within a liquid occurs slowly Flows readily.
Retains its own shape and volume Is virtually incompressible Diffusion within a solid occurs extremely slowly Does not flow. Atoms of molecules. London dispersion, dipole-dipole forces, hydrogen bonds. Fairly soft, low to moderately high melting point, poor thermal and electrical conduction. Argon, methane, sucrose, dry ice. The gradual softening of an amorphous material differs dramatically from the distinct melting of a crystalline solid.
This results from the structural nonequivalence of the molecules in the amorphous solid. Some forces are weaker than others, and when an amorphous material is heated, the weakest intermolecular attractions break first.
As the temperature is increased further, the stronger attractions are broken. Thus amorphous materials soften over a range of temperatures. Carbon is an essential element in our world. The unique properties of carbon atoms allow the existence of carbon-based life forms such as ourselves. Carbon forms a huge variety of substances that we use on a daily basis, including those shown in [link]. You may be familiar with diamond and graphite, the two most common allotropes of carbon.
Allotropes are different structural forms of the same element. Diamond is one of the hardest-known substances, whereas graphite is soft enough to be used as pencil lead.
These very different properties stem from the different arrangements of the carbon atoms in the different allotropes. You may be less familiar with a recently discovered form of carbon: graphene. Graphene was first isolated in by using tape to peel off thinner and thinner layers from graphite.
It is essentially a single sheet one atom thick of graphite. Graphene, illustrated in [link] , is not only strong and lightweight, but it is also an excellent conductor of electricity and heat. These properties may prove very useful in a wide range of applications, such as vastly improved computer chips and circuits, better batteries and solar cells, and stronger and lighter structural materials.
In a crystalline solid, the atoms, ions, or molecules are arranged in a definite repeating pattern, but occasional defects may occur in the pattern. Several types of defects are known, as illustrated in [link]. Vacancies are defects that occur when positions that should contain atoms or ions are vacant. Less commonly, some atoms or ions in a crystal may occupy positions, called interstitial sites , located between the regular positions for atoms.
Other distortions are found in impure crystals, as, for example, when the cations, anions, or molecules of the impurity are too large to fit into the regular positions without distorting the structure.
Trace amounts of impurities are sometimes added to a crystal a process known as doping in order to create defects in the structure that yield desirable changes in its properties.
For example, silicon crystals are doped with varying amounts of different elements to yield suitable electrical properties for their use in the manufacture of semiconductors and computer chips.
Some substances form crystalline solids consisting of particles in a very organized structure; others form amorphous noncrystalline solids with an internal structure that is not ordered. The main types of crystalline solids are ionic solids, metallic solids, covalent network solids, and molecular solids.
The properties of the different kinds of crystalline solids are due to the types of particles of which they consist, the arrangements of the particles, and the strengths of the attractions between them. Because their particles experience identical attractions, crystalline solids have distinct melting temperatures; the particles in amorphous solids experience a range of interactions, so they soften gradually and melt over a range of temperatures. Some crystalline solids have defects in the definite repeating pattern of their particles.
These defects which include vacancies, atoms or ions not in the regular positions, and impurities change physical properties such as electrical conductivity, which is exploited in the silicon crystals used to manufacture computer chips. At very low temperatures oxygen, O 2 , freezes and forms a crystalline solid. Which best describes these crystals?
As it cools, olive oil slowly solidifies and forms a solid over a range of temperatures. Which best describes the solid? Ice has a crystalline structure stabilized by hydrogen bonding.
0コメント