Examples of ionic crystal in the following topics:
-
- An ionic crystal consists of ions bound together by electrostatic attraction.
- The arrangement of ions in a regular, geometric structure is called a crystal lattice.
- Examples of such crystals are the alkali halides, which include:
- Since ionic salts have a lower energetic configuration than their individual elements, reactions forming ionic solids tend to release energy.
- Halite forms cubic crystals.
-
- Ionic radius (rion) is the radius of an ion, regardless of whether it is an anion or a cation.
- In this way, the sum of ionic radii of a cation and an anion can give us the distance between the ions in a crystal lattice.
- Ionic radii are typically given in units of either picometers (pm) or Angstroms (Å), with 1 Å = 100 pm.
- Nevertheless, ionic radius values are sufficiently transferable to allow periodic trends to be recognized.
- Identify the general trends of the ionic radius size for the periodic table.
-
- Ionic formulas must satisfy the noble gas configurations for the constituent ions and the product compound must be electrically neutral.
- On a macroscopic scale, ionic compounds, such as sodium chloride (NaCl), form a crystalline lattice and are solids at normal temperatures and pressures.
- The ionic composition is then defined by the requirement that the resulting compound be electrically neutral overall.
- A lesson on writing formulas for binary ionic compounds as well as ionic compounds containing polyatomic ions.
- Apply knowledge of ionic bonding to predict the formula of ionic compounds
-
- To answer this question, consider the data on the ionic solid LiF.
- The ionic bonding model is useful for many purposes, however.
- There is nothing wrong with using the term "ionic bond" to describe the interactions between the atoms in the very small class of "ionic solids" such as LiF and NaCl.
- This means that atoms will sit in positions that minimize the amount of space they occupy (like a salt crystal).
- Does this make an ionic bond, a covalent bond, or something in between?
-
- Lattice energy is a measure of the bond strength in an ionic compound.
- Lattice energy is an estimate of the bond strength in ionic compounds.
- The energy value can be estimated using the Born-Haber cycle, or it can be calculated theoretically with an electrostatic examination of the crystal structure.
- Ionic compounds with smaller lattice energies tend to be more soluble in H2O.
- Sodium ions (Na+) and chloride(Cl-) ions, depicted in purple and green respectively, alternate in the crystal lattice of solid NaCl.
-
- Metallic crystals are held together by metallic bonds, electrostatic interactions between cations and delocalized electrons.
- The high density of most metals is due to the tightly packed crystal lattice of the metallic structure.
- In the case of ionic compounds in water solutions, the ions themselves serve this function.
- The same thing holds true of ionic compounds when melted.
- Ionic solids contain the same charge carriers, but because they are fixed in place, these solids are insulators.
-
- Hydrides can be components of discrete molecules, oligomers, polymers, ionic solids, chemisorbed monolayers, bulk metals (interstitial), and other materials.
- Hydrides can be characterized as ionic, covalent, or interstitial hydrides based on their bonding types.
- Most ionic hydrides exist as "binary" materials that involve only two elements, one of which is hydrogen.
- Ionic hydrides are often used as heterogeneous bases and reducing reagents in organic synthesis.
- This is a space-filling model of a crystal of lithium hydride, LiH, a binary halide.
-
- Water is therefore referred to as a solvent: a substance capable of dissolving other polar molecules and ionic compounds.
- When ionic compounds are added to water, individual ions interact with the polar regions of the water molecules during the dissociation process, disrupting their ionic bonds.
- Consider table salt (NaCl, or sodium chloride): when NaCl crystals are added to water, the molecules of NaCl dissociate into Na+ and Cl– ions, and spheres of hydration form around the ions.
-
- Whereas the characteristic melting point of metals and ionic solids is ~1000 °C, most molecular solids melt well below ~300 °C.
- For example, solid phosphorus can crystallize in different allotropes called "white", "red" and "black" phosphorus.
- White phosphorus forms molecular crystals composed of tetrahedral P4 molecules.
- Although white phosphorus is an insulator, the black allotrope, which consists of layers extending over the whole crystal, does conduct electricity.
- However, they can convert into covalent allotropes having atomic chains extending all through the crystal.
-
- This means that the entire crystal is, in effect, one giant molecule.
- Similarly, a covalent solid cannot "melt" in the usual sense, since the entire crystal is one giant molecule.
- When molten, unlike ionic compounds, the substance is still unable to conduct electricity, since the macromolecule consists of uncharged atoms rather than ions.
- Cubic boron nitride adopts a crystal structure, which can be constructed by replacing every two carbon atoms in diamond with one boron atom and one nitrogen atom.