Wiki User. KCl is an ionic bond. A bond cannot be both covalent and ionic. A bond can be covalent, ionic or metallic.
In covalent bonding electrons are shared, electrons are transferred in ionic bonding and electrons move about in a sea of electrons in metallic bonds. Covalent bond. It is in a Ionic bond. Covalent bond is more common than ionic bond. It is a covalent bond. It has a covalent bond.
Covalent Bond. This bond is covalent. The bond is covalent. Log in. Chemical Bonding. Study now. See Answer. Best Answer. Study guides. Chemistry 20 cards. To name a monatomic anion change the suffix of the element's name to. The electron geometry of a water molecule is even though the molecular geometry is bent. Is Dihydrogen monoxide an example of a nonpolar molecule. The number of pairs of electrons in a covalent bond equals the bond order. Differentiate qualitative observation from quantitative observation.
Hydrogen bonding is a term describing an attractive interaction between a hydrogen atom from a molecule or a molecular fragment X—H in which X is more electronegative than H, and an atom or a group of atoms in the same or a different molecule, in which there is evidence of bond formation.
The attractive interaction in a hydrogen bond typically has a strong electrostatic contribution, but dispersion forces and weak covalent bonding are also present. In metallic solids and network solids, however, chemical bonds hold the individual chemical subunits together. The crystal is essential a single, macroscopic molecule with continuous chemical bonding throughout the entire structure. In metallic solids, the valence electrons are no longer exclusively associated with a single atom.
Instead these electrons exist in molecular orbitals that are delocalized over many atoms, producing an electronic band structure. The metallic crystal essentially consists of a set of metal cations in a sea of electrons. This type of chemical bonding is called metallic bonding. You learned previously that an ionic solid consists of positively and negatively charged ions held together by electrostatic forces.
The strength of the attractive forces depends on the charge and size of the ions that compose the lattice and determines many of the physical properties of the crystal. The lattice energy i. In both cases, however, the values are large; that is, simple ionic compounds have high melting points and are relatively hard and brittle solids.
Molecular solids consist of atoms or molecules held to each other by dipole—dipole interactions, London dispersion forces, or hydrogen bonds, or any combination of these. The arrangement of the molecules in solid benzene is as follows:. For similar substances, the strength of the London dispersion forces increases smoothly with increasing molecular mass. For example, the melting points of benzene C 6 H 6 , naphthalene C 10 H 8 , and anthracene C 14 H 10 , with one, two, and three fused aromatic rings, are 5.
The enthalpies of fusion also increase smoothly within the series: benzene 9. If the molecules have shapes that cannot pack together efficiently in the crystal, however, then the melting points and the enthalpies of fusion tend to be unexpectedly low because the molecules are unable to arrange themselves to optimize intermolecular interactions.
Self-healing rubber is an example of a molecular solid with the potential for significant commercial applications. The material can stretch, but when snapped into pieces it can bond back together again through reestablishment of its hydrogen-bonding network without showing any sign of weakness. Among other applications, it is being studied for its use in adhesives and bicycle tires that will self-heal.
Covalent solids are formed by networks or chains of atoms or molecules held together by covalent bonds. A perfect single crystal of a covalent solid is therefore a single giant molecule. The carbon atoms form six-membered rings. The unit cell of diamond can be described as an fcc array of carbon atoms with four additional carbon atoms inserted into four of the tetrahedral holes. It thus has the zinc blende structure described in Section Elemental silicon has the same structure, as does silicon carbide SiC , which has alternating C and Si atoms.
The structure of crystalline quartz SiO 2 , shown in Section All compounds with the diamond and related structures are hard, high-melting-point solids that are not easily deformed.
Instead, they tend to shatter when subjected to large stresses, and they usually do not conduct electricity very well. It is difficult to deform or melt these and related compounds because strong covalent C—C or Si—Si or polar covalent Si—C or Si—O bonds must be broken, which requires a large input of energy.
Other covalent solids have very different structures. It contains planar networks of six-membered rings of sp2 hybridized carbon atoms in which each carbon is bonded to three others. To completely describe the bonding in graphite, we need a molecular orbital approach similar to the one used for benzene in Chapter 9.
In fact, the C—C distance in graphite In graphite, the two-dimensional planes of carbon atoms are stacked to form a three-dimensional solid; only London dispersion forces hold the layers together. As a result, graphite exhibits properties typical of both covalent and molecular solids. It is also very soft; the layers can easily slide past one another because of the weak interlayer interactions. Finally, graphite is black because it contains an immense number of alternating double bonds, which results in a very small energy difference between the individual molecular orbitals.
Thus light of virtually all wavelengths is absorbed. Diamond, on the other hand, is colorless when pure because it has no delocalized electrons. In network solids, conventional chemical bonds hold the chemical subunits together. The bonding between chemical subunits, however, is identical to that within the subunits, resulting in a continuous network of chemical bonds. One common examples of network solids are diamond a form of pure carbon Carbon exists as a pure element at room temperature in three different forms: graphite the most stable form , diamond, and fullerene.
The structure of diamond is shown at the right in a "ball-and-stick" format. The balls represent the carbon atoms and the sticks represent a covalent bond. Be aware that in the "ball-and-stick" representation the size of the balls do not accurately represent the size of carbon atoms.
In addition, a single stick is drawn to represent a covalent bond irrespective of whether the bond is a single, double, or triple bond or requires resonance structures to represent. The "space-filling" format is an alternate representation that displays atoms as spheres with a radius equal to the van der Waals radius, thus providing a better sense of the size of the atoms.
CC0; H. Bhadeshia via Wikipedia. Notice that diamond is a network solid. The entire solid is an "endless" repetition of carbon atoms bonded to each other by covalent bonds. In the display at the right, the structure is truncated to fit in the display area. The most stable form of carbon is graphite. Graphite consists of sheets of carbon atoms covalently bonded together.
Answer: naphthalene C10H8 is a covalent bond. By Bagus Amin - PM -. Share this. Newer Post Older Post Home.
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