Linked from

The 144 pages that link to Covalent bond, each with the reason it gives.

• Carbon dioxideRelated: The carbon–oxygen bonds hold the atoms together in CO₂.

• HydrolysisRelated: Many familiar hydrolysis reactions cleave covalent bonds.

• AlkaneRelated: Single covalent bonds connect carbon atoms in an alkane's carbon skeleton.

• CeramicRelated: Strong directional covalent bonds make many ceramics hard and thermally stable.

• Formal chargeRelated: Formal-charge bookkeeping assigns half of each covalent bond’s electrons to each bonded atom.

• GlassRelated: Strong silicon–oxygen covalent bonds help give silica glass rigidity.

• CarbonRelated: Carbon’s stable covalent bonds underpin its molecular and solid structures.

• Free radicalRelated: Homolytic bond breaking divides a shared pair and leaves one electron on each fragment.

• Octet ruleRelated: Shared bonding pairs count toward the outer shells of both bonded atoms.

• BoronRelated: Boron commonly forms covalent bonds rather than simple ionic bonds.

• Carbon nanotubeRelated: Covalent bonds hold the hexagonal carbon network together.

• BerylliumRelated: Small, highly charged beryllium ions form unusually covalent bonds in many compounds.

• MetalloidRelated: Covalent networks account for the hardness and high melting points of some metalloids.

• Bond angleRelated: Most textbook bond angles describe directions of covalent bonds.

• Cross-linkRelated: Covalent cross-links permanently join polymer chains through shared-electron bonds.

• AmmoniumRelated: The N–H bonds within ammonium are covalent.

• CyanideRelated: The carbon–nitrogen bond within CN⁻ is a strong covalent bond.

• Electron correlationRelated: Accurate bond energies and dissociation behavior often require correlated electrons.

• SeleniumRelated: Covalent bonding shapes selenium’s molecular and crystalline forms.

• Uranium hexafluorideRelated: Uranium–fluorine bonding gives UF₆ its molecular structure and chemical behavior.

• Gilbert N. LewisRelated: Lewis’s electron-pair model gave a foundational account of this bond.

• Phenyl groupRelated: The open valence on phenyl forms a covalent bond to its attachment partner.

• Chemical compoundRelated: Covalent bonds connect atoms in molecular compounds and extended networks.

• Diatomic moleculeRelated: Most stable neutral diatomic molecules are held together by covalent bonds.

• DNA adductRelated: A DNA adduct is defined by covalent attachment to the DNA molecule.

• Amino groupRelated: Shared electron pairs connect the amino nitrogen to hydrogen or carbon atoms.

• Hydrogen halideRelated: The hydrogen–halogen bond is covalent in the gaseous molecules.

• Space-filling modelRelated: Covalent bonds connect the atoms whose positions the model displays.

• Bent molecular geometryRelated: Two bonds from a central atom define the arms of a bent molecular shape.

• NonmetalRelated: Nonmetal atoms commonly bond to one another by sharing electrons.

• PnictogenRelated: Covalent bonding is central to nitrogen and phosphorus compounds, including their hydrides.

• Post-transition metalRelated: Post-transition metals can form covalent compounds more readily than many transition metals.

• Avram HershkoRelated: The discovery showed that ubiquitin becomes covalently attached to proteins slated for degradation.

• Carbon-based lifeRelated: Shared electron pairs link carbon atoms into stable chains, rings, and branches.

• Hydrogen chalcogenideRelated: Covalent bonding holds hydrogen and chalcogen atoms together in common molecular members.

• Hydrogen tellurideRelated: The H–Te bonds are covalent links within the H₂Te molecule.

• Main-group elementRelated: Many main-group nonmetals achieve stable valence shells by sharing electrons.

• SubstituentRelated: Covalent bonds connect substituents to their parent molecules.

• Carbon groupRelated: Sharing electrons lets many group 14 atoms form stable compounds and networks.

• Nitrosyl chlorideRelated: Covalent bonding describes the N–O and N–Cl connections in NOCl.

• Tantalum carbideRelated: Covalent contributions to metal–carbon bonding help make the carbide hard.

• TetradecaneRelated: Tetradecane’s carbon skeleton and C–H bonds are covalent.

• Electron countingRelated: Shared electron pairs must be assigned according to the chosen counting convention.

• Impurity (semiconductors)Related: Valence differences between an impurity and host atoms determine donated or missing bonds.

• Iodic acidRelated: Covalent bonding connects iodine and oxygen in the acid molecule.

• Polymer backboneRelated: Covalent bonds connect atoms along most polymer backbones.

• Silicon tetrachlorideRelated: The Si–Cl bonds give the molecule its tetrahedral structure and reactivity.

• Tin(IV) chlorideRelated: The Sn–Cl bonds are predominantly covalent in molecular tin(IV) chloride.

• Bonding in solidsRelated: Shared electrons link atoms into molecules or extended solid networks.

• Chromyl chlorideRelated: Chromium–oxygen and chromium–chlorine bonding gives the molecule its distinctive composition.