Atomic Properties and Ionization Energy Quiz

Connected to MO theory, it describes a continuum of overlapping orbitals, where the lowest energy orbitals have no nodes between neighboring atoms, and the highest energy orbitals have nodes between every pair of neighbors. The energy separation between neighboring orbitals approaches zero, creating a near-continuous energy spectrum.

Forms between s orbitals.

Forms between p orbitals.

<p>Conductors have partially filled bands at low energy levels which allow electrons to be easily promoted. Vigorous vibrations due to thermal energy can disrupt the band structure and decrease conductivity.</p> Signup and view all the answers

<p>Insulators have filled bands with a large energy differential separating them, where the filled band is called the valence band, and the next higher band is called the conduction band.</p> Signup and view all the answers

<p>Extrinsic semiconductor</p> Signup and view all the answers

<p>Energy required to remove the least tightly bound electron from a neutral atom in the gas phase.</p> Signup and view all the answers

<p>Highest at top right, smaller electron means harder to remove.</p> Signup and view all the answers

<p>It serves to maximize the stabilizing interactions while minimizing the destabilizing interactions among electrons.</p> Signup and view all the answers

<p>Pie, stabilizing, result of electrons pairing in degenerate orbitals with parallel spin.</p> Signup and view all the answers

<p>Destabilizing, coulomb interaction, energy of electron-electron repulsion in a filled orbital.</p> Signup and view all the answers

<p>High energy electrons; they already contain more energy so they require less energy input.</p> Signup and view all the answers

<p>The first electron to be ionized will come from the 4s orbital; the other s electron will enter the d orbital.</p> Signup and view all the answers

<p>Reduction in atomic radius following the lanthanide series, contrary to the overall trend observed for the periodic table.</p> Signup and view all the answers

<p>Elements 57-71, first appearance of f orbitals where electrons added will have a higher effective nuclear charge, shrinking the radius.</p> Signup and view all the answers

<p>They determine the effective nuclear charge, Zeff = Z - sigma, where sigma is the sum of the number of electrons in a given subshell multiplied by a weighting coefficient.</p> Signup and view all the answers

<p>The reduction in charge attraction between the nucleus and electrons due to electrons between the nucleus and the electron in question.</p> Signup and view all the answers

<p>When an electron of a higher atomic orbital is found within the shell of electrons of a lower atomic number.</p> Signup and view all the answers

<p>The difference in energy for a neutral gaseous atom and the gaseous anion; more positive means more stable with the additional electron.</p> Signup and view all the answers

<p>Overall measure of an atom's ability to attract electrons to itself when part of a compound.</p> Signup and view all the answers

<p>An atom's ability to be distorted by an electric field, which can result in partial positive or negative charges.</p> Signup and view all the answers

<p>Systems involving multiple electrons are much more complex and require the use of quantum mechanics.</p> Signup and view all the answers

<p>E = -13.6 eV * (Z^2/n^2), where h is Planck’s constant.</p> Signup and view all the answers

<p>Joules, wavenumber, inverse centimeters.</p> Signup and view all the answers

<p>Principle quantum number, defines energy and size of orbital.</p> Signup and view all the answers

<p>Orbital angular momentum quantum number, defines the magnitude of the orbital angular momentum.</p> Signup and view all the answers

<p>Magnetic quantum number, describes the orientation of the angular momentum.</p> Signup and view all the answers

<p>Spin magnetic quantum number, defines intrinsic angular momentum of an electron.</p> Signup and view all the answers

<p>(R(r)), along with the angular wavefunction, gives us the orbitals.</p> Signup and view all the answers

<p>A plot of R^2(r)r^2, indicating the probability of finding an electron at a certain distance from the nucleus.</p> Signup and view all the answers

<p>The most probable distance to find the electron in a one proton, one electron system is 52.9 picometers.</p> Signup and view all the answers

<p>L=0=s, L=1=p, L=2=d, L=3=f, L=4=g.</p> Signup and view all the answers

<p>When degenerate orbitals are available, electrons occupy separate orbitals with parallel spin.</p> Signup and view all the answers

<p>No more than two electrons can occupy a single orbital, and to do so, their spins must be paired.</p> Signup and view all the answers

<p>Valence Shell Electron Pair Repulsion.</p> Signup and view all the answers

<p>Lone pair &gt; multiple bonds &gt; single bonds.</p> Signup and view all the answers

<p>Explains chemical bonding by considering the overlap of atomic orbitals.</p> Signup and view all the answers

<p>Explains bonding where the number of equivalent bonds exceeds the number of valence orbitals.</p> Signup and view all the answers

<p>It pushes strongly against all other substituents, governing the shape of a molecule.</p> Signup and view all the answers

<p>An improvement over valence bond theory, extending the description of bonding to all atoms in a molecule.</p> Signup and view all the answers

<p>Orbital approximation and linear combinations of atomic orbitals.</p> Signup and view all the answers

<p>The wave function describing all of the electrons of a molecule can be written as a product of the one-electron wave functions.</p> Signup and view all the answers

<p>The superposition of multiple atomic orbitals of the same type along with weighting coefficients.</p> Signup and view all the answers

<p>The 1s orbitals combine to form a lower energy sigma orbital and a higher energy antibonding sigma orbital.</p> Signup and view all the answers

<p>2s orbitals combine to form bonding and antibonding molecular orbitals.</p> Signup and view all the answers

<p>Due to the difference in MO diagram's relative energies of the bonding orbitals pi and sigma.</p> Signup and view all the answers

<p>H bonds through 2p and 2s orbitals; relative energies of the atomic orbitals are crucial.</p> Signup and view all the answers

<p>Relative energies are taken into account; more electronegative means lower energy orbitals.</p> Signup and view all the answers

<p>4sigma &gt; 2pi &gt; 3sigma &gt; 1pi &gt; 2sigma &gt; 1sigma.</p> Signup and view all the answers

<p>Must use approximations of MO theory, creating a cumulative approximation of atomic orbitals.</p> Signup and view all the answers

<p>a, b = non-degenerate, e = doubly degenerate, t = triple degenerate.</p> Signup and view all the answers

<p>Lowest = a (non-degenerate), intermediate = e, highest = t.</p> Signup and view all the answers

<p>A method to assess overall bond strength between two atoms in a molecule.</p> Signup and view all the answers

<p>(bonding - antibonding) / 2.</p> Signup and view all the answers

<p>A bonding orbital lies lower in energy than its substituent atomic orbitals.</p> Signup and view all the answers

<p>A nonbonding orbital is equal in energy to its corresponding atomic orbitals.</p> Signup and view all the answers

<p>An antibonding orbital lies higher in energy than its substituent atomic orbitals.</p> Signup and view all the answers

<p>Highest occupied molecular orbital, indicates the highest energy electrons reside.</p> Signup and view all the answers

<p>Lowest unoccupied molecular orbital, it is the energy level directly above the HOMO.</p> Signup and view all the answers

<p>Critical to electron structure; when excited, an electron is promoted from HOMO to LUMO.</p> Signup and view all the answers

<p>Occurs if there are two unpaired electrons.</p> Signup and view all the answers

<p>The bonding and ordering of metals into pure solids or solid solutions.</p> Signup and view all the answers

<p>Ions of different elements held together in rigid arrays due to attraction between opposite charges.</p> Signup and view all the answers

<p>A 3D infinite array of lattice points defining the repeating structure of a crystal.</p> Signup and view all the answers

<p>An imaginary, parallel sided region from which the entire crystal can be built.</p> Signup and view all the answers

<p>Cubic, tetragonal, orthorhombic, monoclinic, triclinic, rhombohedral, hexagonal.</p> Signup and view all the answers

<p>Contains only one lattice point.</p> Signup and view all the answers

<p>Contains two lattice points per unit cell.</p> Signup and view all the answers

<p>Contains four lattice points per unit cell.</p> Signup and view all the answers

<p>Structure type with the least unfilled space.</p> Signup and view all the answers

<p>The number of nearest neighbors, the number of spheres a single sphere touches in the unit cell.</p> Signup and view all the answers

<p>ABCABC repeating layer of spheres.</p> Signup and view all the answers

<p>Same as cubic close packed.</p> Signup and view all the answers

<p>Unoccupied space between spheres; can be octahedral or tetrahedral.</p> Signup and view all the answers

<p>The ability of a metal to adopt different crystal structures based on temperature and pressure.</p> Signup and view all the answers

<p>A blend of different metals, more formally called a solid solution.</p> Signup and view all the answers

<p>When solute metal atoms take up the positions of solvent metal atoms in the crystal structure.</p> Signup and view all the answers

<p>When solute metal atoms occupy positions in the holes of the solvent crystal structure.</p> Signup and view all the answers

<p>The standard enthalpy change accompanying the formation of a gas of ions from a solid.</p> Signup and view all the answers

<p>A flow chart used to determine the lattice enthalpies and other parameters governing how a solid behaves.</p> Signup and view all the answers

<p>Non-electrostatic contributions to the lattice enthalpy.</p> Signup and view all the answers

<p>Substance that exhibits variable composition but retains the same structure type.</p> Signup and view all the answers

<p>A substance with electric conductivity that decreases as temperature increases.</p> Signup and view all the answers

<p>A substance with electric conductivity that increases as temperature increases.</p> Signup and view all the answers

<p>Negligible conduction, but if measurable, it increases with temperature.</p> Signup and view all the answers

<p>Substances that have zero resistance below a critical temperature.</p> Signup and view all the answers

<p>A near continuous array of energy levels due to many symmetrically oriented atomic orbitals.</p> Signup and view all the answers

<p>A separation of bands, due to the absence of energy values for the molecular orbital.</p> Signup and view all the answers

<p>The bands built from s and p orbitals.</p> Signup and view all the answers

<p>The highest occupied energy level in a solid at T=0.</p> Signup and view all the answers

<p>Atomic radii of elements within 15% of each other and compatible crystal structures.</p> Signup and view all the answers

<p>Small atom must not transfer electrons; must have a radius enough to fit in the hole (0.414 * radius of metal).</p> Signup and view all the answers

<p>Lattice enthalpy.</p> Signup and view all the answers

<p>If high charge and small distance, strongly stabilizing.</p> Signup and view all the answers

<p>Small charge and large distance make the solid unstable.</p> Signup and view all the answers

<p>Allows us to estimate the lattice enthalpy from charge and separation at T=0.</p> Signup and view all the answers

<p>Solubility is a product of lattice enthalpy and hydration enthalpy.</p> Signup and view all the answers

<p>Ordering of water molecules around a dissolved ion.</p> Signup and view all the answers