Chemical Bonding

• Chemical Bonding - Explains how atoms join to form molecules and compounds.
• Ionic Bonds - Formed by electron transfer between metals and non-metals, resulting in charged ions.
• Covalent Bonds - Formed by the sharing of electron pairs between non-metal atoms.
• Metallic Bonds - Involve a "sea of electrons" shared among metal atoms, contributing to properties like conductivity and malleability.
• Polar Covalent Bonds - Have unequal sharing of electron density between atoms, leading to partial charges.
• Non-Polar Covalent Bonds - Have equal sharing of electron density between atoms, resulting in no partial charges.
• Hydrogen Bonds - Special interactions involving hydrogen and highly electronegative atoms (e.g., oxygen, nitrogen, fluorine).
• Ionic Bonding - Electrons are transferred from a metal atom to a non-metal atom.
• Ionic Bonding - Metals lose electrons to become positively charged cations.
• Ionic Bonding - Non-metals gain electrons to become negatively charged anions.
• Ionic Bonding - Opposite charges of cations and anions attract each other, forming this bond.
• Ionic Compounds - Conduct electricity when melted or dissolved in water, as the ions are free to move.
• Ionic Compounds - Generally have high melting and boiling points due to strong electrostatic forces between ions.
• Covalent Bonding - Formed when two atoms share one or more pairs of electrons to achieve a stable electron configuration.
• Covalent Bonding - Atoms share electrons to fill their outer electron shells and achieve a more stable electron configuration.
• Covalent Bonding - Can involve one (single bond), two (double bond), or three (triple bond) shared pairs of electrons.
• Covalent Compounds - Generally have lower melting and boiling points compared to ionic compounds.
• Covalent Compounds - Do not conduct electricity in solid or liquid form as they lack free-moving ions.
• Metallic Bonding - Occurs in metals where electrons are shared among a lattice of metal atoms.
• Metallic Bonding - Creates a “sea of electrons” that move freely around the metal cations.
• Metallic Bonding - Electrons are delocalized and move freely around the positively charged metal ions, which are fixed in place in a lattice structure.
• Metals - Conduct electricity and heat well due to the mobility of free electrons.
• Polar Covalent Bond - A type of covalent bond where electrons are shared unequally between two atoms, leading to partial charges on the atoms.
• Non-Polar Covalent Bond - A covalent bond where electrons are shared equally between two atoms, resulting in no partial charges.
• Polarity of Covalent Bond - Depends on the difference in electronegativity between the two bonded atoms.
• Greater Electronegativity Difference - Leads to more polar bonds.
• Polar Covalent Bonds - Molecules with these bonds may have an overall dipole moment if the molecule has an asymmetric shape.
• Non-Polar Covalent Bonds - Molecules with these bonds or symmetrical polar bonds may have no overall dipole moment.
• Hydrogen Bonding - A special type of dipole-dipole attraction occurring when hydrogen is covalently bonded to a highly electronegative atom (e.g., oxygen, nitrogen, fluorine) and is attracted to a lone pair of electrons on another electronegative atom.
• Hydrogen Bonds - Stronger than other dipole-dipole interactions but weaker than ionic or covalent bonds.
• Hydrogen Bonding - Affects the boiling and melting points of compounds.
• Hydrogen Bonding - Increases solubility in water.
• Hydrogen Bonding - Plays a crucial role in biological structures like proteins and DNA.
• Valence electrons - Electrons in the outermost shell of an atom that are involved in forming chemical bonds.
• Type of orbital - The type of space within an atom where electrons are found, such as s, p, d, and f orbitals.
• Energy level - The specific level of energy where electrons are located within an atom.
• Number of electron - The total number of electrons in an atom, which determines its bonding behavior.
• Chemical bonding - The process by which atoms form new substances by creating chemical bonds through their valence electrons.
• Electric configuration - The arrangement of electrons in the orbitals of an atom.
• Oxygen - An element with the atomic number 8, known for its role in respiration and combustion.