"valence electrons are electrons in the outermost shell of an atom"
The outermost electrons of an atom, which are involved in chemical bonding.
Atomic Structure: The arrangement of subatomic particles, including protons, neutrons, and electrons, in an atom.
Electron Configuration: The distribution of electrons in different energy levels or orbitals around an atom's nucleus.
Valence Electrons: The electrons present in the outermost shell of an atom, responsible for chemical bonding.
Lewis Symbols: A representation of electrons in the valence shell using dots and crosses to indicate the outer-shell electrons.
Octet Rule: Atoms tend to gain or lose electrons to obtain a stable, eight-electron configuration in their outer shells.
Ionic Bonds: The electrostatic attraction between a positively charged ion or cation and a negatively charged ion or anion.
Covalent Bonds: The sharing of electrons between two or more atoms to satisfy the octet rule.
Polar Covalent Bonds: Covalent bonds in which the electrons are not shared equally, leading to a partially negative and partially positive end.
Electronegativity: The ability of an atom to attract shared electrons in a covalent bond towards its nucleus.
Bond Length and Bond Energy: The distance between the nuclei of two bonded atoms and the energy required to break a chemical bond.
Resonance Structures: Different ways of arranging electrons in a molecule that can contribute to its overall stability.
Hybridization: The process of mixing different atomic orbitals to form new hybrid orbitals for bonding.
Molecular Shapes: The three-dimensional arrangement of atoms in a molecule, which depends on the nature of the bonds and lone pairs of electrons.
Intermolecular Forces: The attractive or repulsive forces between molecules that determine the physical properties of substances, such as boiling points and solubility.
Metallic Bonds: The delocalized sharing of valence electrons between metal atoms, responsible for the unique properties of metals.
Ionic Bonds: This type of bonding occurs between a metal and a non-metal where the non-metal donates electrons to the metal.
Covalent Bonds: These types of bonds occur between non-metals, where electrons are shared between two atoms.
Metallic Bonds: This type of bonding is found in metals, where the atoms share a sea of electrons, forming a lattice structure.
Polar Covalent Bonds: This is a type of covalent bond where the shared electrons are not equally distributed between the two atoms.
Hydrogen Bonds: This type of bonding occurs between a hydrogen atom and an electronegative atom like nitrogen, oxygen, or fluorine.
Van der Waals Forces: This force arises in between molecules due to the momentary crests and troughs in electron densities.
Dipole-Dipole Interaction: This occurs between two polar molecules in which the positive end of one molecule attracts the negative end of another molecule.
London Dispersion Forces: This force results due to the fluctuating electron distribution around an atom, which causes a temporary dipole moment.
Coordinate Covalent Bonds: This type of bond is formed when one atom donates both of the shared electrons to another atom.
Three-center two-electron bonds: It is also known as banana bond, formed when three atoms share two electrons.
Aromatic Bonds: A type of delocalized bonding where the electrons are shared in a ring-shaped molecule known as an aromatic compound.
Conjugated Double Bonds: This type of bonding occurs between atoms with alternating single and double bonds.
Hydrophobic Interactions: This force arises between non-polar molecules in the presence of water.
Salt Bridges: This bond is formed between an acidic and basic residue of two different amino acids in a protein molecule.
Halogen Bond: This type of bond is formed between a halogen atom and a negative atom like oxygen, nitrogen, etc.
"can participate in the formation of a chemical bond"
"The presence of valence electrons can determine the element's chemical properties"
"a given element's reactivity is highly dependent upon its electronic configuration"
"a valence electron can exist only in the outermost electron shell"
"for a transition metal, a valence electron can also be in an inner shell"
"tends to be chemically inert"
"due to the relatively low energy to remove the extra valence electrons"
"tendency either to gain the missing valence electrons and form a negative ion, or else to share valence electrons and form a covalent bond"
"a valence electron has the ability to absorb or release energy in the form of a photon"
"known as atomic excitation"
"move to an inner shell which is not fully occupied"
"a shared pair forms with both atoms in the bond each contributing one valence electron"
"an atom with a closed shell of valence electrons (corresponding to a noble gas configuration) tends to be chemically inert"
"to remove the extra valence electrons to form a positive ion"
"to gain the missing valence electrons and form a negative ion, or else to share valence electrons and form a covalent bond"
"a valence electron can exist only in the outermost electron shell"
"An energy gain can trigger the electron to move (jump) to an outer shell"
"break free from its associated atom's shell; this is ionization to form a positive ion"
"When an electron loses energy... then it can move to an inner shell which is not fully occupied"