Chemical bonding

• Chemical bonds are strong forces of attraction that hold atoms or ions together in a substance.
• In a chemical bond, the electrons are shared between the atoms.
• Chemical bonds can be ionic, covalent, or metalic.
• Ionic bonds are formed when a positively charged species interacts with a negatively charged species.
• Covalent bonds are formed when two species share electrons.
• Electron configuration of ion [Ne] is represented as N/A.
• Electron gain or loss is represented by the change in ion formation, where a loss is represented by a negative charge and a gain is represented by a positive charge.
• The number of electrons in valence shells is 37.
• Group number 121516 is represented by the period 3 elements A and Ar.
• Write the chemical symbol for the positive ion first and the chemical symbol for the negative ion second.
• Electron configuration of ion [Ar] is represented as N/A.
• To identify the positive ion (cation) and the negative ion (anion) in an ionic compound, follow these rules:
• Each ionic compound is found in a crystal lattice structure.
• Find the chemical symbol for the ions, either in the periodic table or in the table of polyatomic ions.
• If you don't know the charge, use the group rule to determine the charge for the present elements and the Roman numbers or superscripts.
• The chemical formula for ionic compounds is known as a formula unit.
• Determine the charges of the ions.
• Metallic bonds are formed when a positively charged species interacts with a negatively charged species.
• In ionic bonding, the electrons are shared between the atoms.
• Chemical bonding and structure involve the arrangement of atoms through the sharing of electrons.
• In covalent bonding, the electrons are shared between the atoms.
• Covalent bonding occurs when atoms share pairs of valence electrons.
• The Lewis structures for the following molecules can be drawn: PF5, IF4, XeF6.
• Below will be able to expand or contract by making use of its energetically accessible, or by lowering d-subshell for binding.
• In metallic bonding, the electrons are shared between the atoms.
• B F3 is the bond order in a coordinate covalent bond.
• C lF4 is the bond order in a coordinate covalent bond.
• S Cl6 is the bond order in a coordinate covalent bond.
• Electrostatic attraction is a force between negatively charged and positively charged atoms.
• Naming and forming compounds for molecular compounds are based on the principle of naming and forming compounds for molecular compounds.
• Naming conventions for molecular compounds, also known as coordination compounds, are based on the principle of naming and forming compounds for molecular compounds.
• Covalent bonds can be formed between elements such as O2 or CO2.
• Covalent bonds form between atoms of relatively high electronegativity, typically non-metals.
• Delocalized electrons exist in any molecule for which there is more than one possible resonance structure.
• Delocalized electrons exist in any molecule for which there is more than one possible Lewis structure.
• In some molecules, delocalized electrons are shared between more than two nuclei and are described as being delocalized.
• Delocalized electrons give greater stability to a molecule or polyatomic ion.
• Delocalized electrons exist in any molecule for which there is more than one possible covalent structure.
• Carbonate, CO32-0, is a pure covalent molecule.
• Exceptions to the octet rule include very small atoms forming stable compounds with less than 8 valence electrons.