Chemistry 1010 Final Clemson University test with verified solutions 2024 latest update.

Molecule Unit of matter that results when two or more atoms are joined by covalent bonds Ionic Bond A bond resulting from the electrostatic attraction of a cation for an anion. Brainpower Read More Nonpolar Covalent Bond A bond characterized by an even distribution of charge; electrons in the bonds are shared equally by the two atoms Polar Covalent Bond A bond resulting from unequal sharing of bonding pairs of electrons between atoms Polyatomic Ions Charged group of one or more atoms joined together by covalent bonds Electrostatic Potential The energy a charged particle has due to its position relative to another charged particle; directly proportional to the product of the charges of the particles; inversely proportional to the distance between the particles Lattice Energy The energy released when 1 mole of an ionic compound forms from its free ions in the gas phase Bond Energy The energy needed to break 1 mole of a particular covalent bond in a molecule or polyatomic ion in the gas phase. Octet Rule Atoms of main group elements make bonds by gaining, losing, or sharing electrons to achieve a valence shell containing 8 electrons, or four electron pairs Bond Length Distance between two bonded atoms at their minimum potential energy, that is, the average distance between two bonded atoms Bonding Pair Pair of electrons shared between two atoms Lone Pair Pair of electrons that is not shared between two atoms Electronegativity A relative measure of the ability of an atom in a chemical compound to attract electrons Resonance Characteristic of electron distributions when two or more equivalent Lewis structures can be drawn for one compound Resonance Structure One of two or more Lewis structures with the same arrangement of atoms but different arrangements of bonding pairs of electrons Resonance Stabilization The stability of a molecular structure due to delocalization of its electrons Formal Charge Value calculated for an atom in a molecule or polyatomic ion by determining the difference between the number of valence electrons in the free atom and the sum of lone-pair electrons plus half of the electrons in the atom's bonding pairs Bond Order The number of bonds between atoms: 1 for a single bond, 2 for a double bond, and 3 for a triple bond Bonds are Broken Energy is released Bonds are Formed Energy is absorbed Bond Angle The angle (in degrees) defined by lines joining the centers of two atoms to a third atom to which they are chemically bonded Electronic Geometry The 3D arrangements of bonding pairs and lone pairs of electrons around a central atom Molecular Geometry The 3D arrangement of atoms in a molecule Bond Dipole Separation of electrical charge created when atoms with different electronegativities form a covalent bond Hybridization In valence bond theory, the mixing of atomic orbitals to generate new sets of orbitals that then are available to form covalent bonds with other atoms Hybrid Atomic Orbital In valence bond theory, one of a set of equivalent orbitals about an atom created when specific atomic orbitals are mixed Molecular Orbital A region of characteristic shape and energy where electrons in a molecule are located Bonding Orbital Term in Molecular Orbital Theory describing regions of increased electron density between nuclear centers that serve to hold atoms together in molecules Antibonding Orbital Term in Molecular Orbital Theory describing regions of electron density in a molecule that destabilize the molecule because they do not increase the electron density between nuclear centers Polar Bonds Bond between 2 atoms that have a large difference in electronegativity Polar Molecule A molecule that has a partial positive end and a partial negative end because of unequal sharing of electrons Valence Bond Theory Provides a readily visualized orbital picture of how electron pairs are shared in a covalent bond Atomic Orbital A wave function whose square gives the probability of finding an electron within a given region of space in an atom Molecular Orbital A wave function whose square gives the probability of finding an electron within a given region of space in a molecule Intramolecular Forces Any force that holds together the atoms making up a molecule or compound Intermolecular Forces Forces of attraction or repulsion between neighboring particles Dipole Moment Quantitative expression of the polarity of a molecule Temporary Dipole Intermolecular force between nonpolar molecules caused by the presence of temporary dipoles within the molecules. Permanent Dipole Permanent separation of electrical charge in a molecule due to unequal distributions of bonding and/or lone pairs of electrons Van der Waals Force Any interaction between neutral atoms and molecules including hydrogen bonds, other dipole-dipole interactions, and London dispersion forces. (Does not apply to interactions involving ions) London Dispersion Force An intermolecular force between molecules caused by the presence of temporary dipoles in the molecules Ion-Dipole Interaction Attractive force between an ion and a molecule that has a permanent dipole Dipole-Dipole Interaction Attraction between regions of polar molecules that have partial charges of the opposite sign Hydrogen Bond Strongest dipole-dipole interaction, which occurs between a hydrogen atom bonded to a N,O,F atom and another N,O,F atom. Polarizability Relative ease with which the electron cloud in a molecule, ion, or atom can be distorted, including a temporary dipole Sphere of Hydration The cluster of water molecules surrounding an ion in an aqueous solution Alcohol An organic compound whose molecular structure includes a hydroxyl group bonded to a carbon atom that is not bonded to any other functional groups Solvent The component of a solution that is present in the greatest amount