Examples of metal in the following topics:
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- Metallic bonding may be described as the sharing of free electrons among a lattice of positively charged metal ions.
- Metallic bonding may be described as the sharing of free electrons among a lattice of positively charged metal ions.
- While ionic bonds join metals to nonmetals, and covalent bonds join nonmetals to nonmetals, metallic bonds are responsible for the bonding between metal atoms.
- The characteristics of metallic bonds explain a number of the unique properties of metals:
- Metals are shiny.
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- Alternative methods of preparing a wide variety of organometallic compounds generally involve an exchange reaction in which a given metal is either moved to a new location or replaced by a new metal, which may include B, Al, Ti, V, Fe, Ni, Cu, Mo, Ru, Pd, Sn, Pt, Hg & Pb.
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- A native metal is any metal that is found in its metallic form in nature, either pure or as an alloy.
- This is why only the less reactive metals such as gold and platinum are found as native metals.
- Native metals were prehistoric man's only access to metal.
- When a metal ore is an ionic compound of that metal and a non-metal, the ore must usually be smelted (or heated with a reducing agent) to extract the pure metal.
- Describe the characteristics of metal alloys and the natural occurence of native metals.
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- Metals are usually malleable, ductile, and shiny.
- Metals are shiny and lustrous with a high density.
- For example, hitting a metal with a hammer will "dent" the metal, not shatter it into pieces.
- This is very instrumental in the conductivity of the metal.
- Sodium metal is soft enough to be cut with a plastic knife.
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- Metallic crystals are held together by metallic bonds, electrostatic interactions between cations and delocalized electrons.
- These interactions are called metallic bonds.
- Atoms in metals are arranged like closely-packed spheres, and two packing patterns are particularly common: body-centered cubic, wherein each metal is surrounded by eight equivalent metals, and face-centered cubic, in which the metals are surrounded by six neighboring atoms.
- Some metals (the alkali and alkaline earth metals) have low density, low hardness, and low melting points.
- The high density of most metals is due to the tightly packed crystal lattice of the metallic structure.
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- Ligands create a complex when forming coordinate bonds with transition metals ions; the transition metal ion acts as a Lewis acid, and the ligand acts as a Lewis base.
- Nearly all compounds formed by the transition metals can be viewed as collections of the Lewis bases—or ligands—bound to the metal, which functions as the Lewis acid.
- One coordination chemistry's applications is using Lewis bases to modify the activity and selectivity of metal catalysts in order to create useful metal-ligand complexes in biochemistry and medicine.
- Examples of several metals (V, Mn, Re, Fe, Ir) in coordination complexes with various ligands.
- All these metals act as Lewis acids, accepting electron pairs from their ligands.
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- Metallic properties tend to decrease across a period and increase down a periodic group.
- Keep in mind that group names can give clues about the elements' metallic properties.
- Elements with low electronegativity tend to have more metallic properties.
- Metals tend to form positive ions, and like charges repel, so how do metal atoms stay bonded together in a solid?
- Families of the periodic table are often grouped by metallic properties.
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- Corrosion is commonly discussed in reference to metals, which corrode electrochemically.
- During the corrosion process, a metal atom at the surface dissolves into an aqueous solution, leaving the metal with excess negatively charged ions.
- The conductive properties of metal enable the oxidation and reduction steps that occur during corrosion to take place at separate sites on the metal's surface.
- The conductivity allows electrons to flow from the anodic to cathodic regions of the metal.
- The higher a metal's reduction potential, the less likely it is to be oxidized.
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- Metal ores are generally oxides, sulfides and silicates of "native" metals (such as native copper) that are not commonly concentrated in the Earth's crust.
- Extractive metallurgy is the practice of removing valuable metals from an ore and refining the extracted raw metals into a purer form.
- In order to convert a metal oxide or sulfide to a purer metal, the ore must be reduced physically, chemically, or electrolytically.
- Ore bodies often contain more than one valuable metal.
- Additionally, a concentrate may contain more than one valuable metal.
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- All the alkali metals react with water, with the heavier alkali metals reacting more vigorously than the lighter ones.
- The oxides are much less reactive than the pure metals.
- In this case, the metal is a basic anhydride.
- All the discovered alkali metals occur in nature.
- Most alkali metals have many different applications.