Help
Options
Didn't know it?
click below
click below
Knew it?
click below
click below
Don't Know
Remaining cards (0)
Know
retry
shuffle
restart
0:00
Embed Code - If you would like this activity on your web page, copy the script below and paste it into your web page.
Normal Size Small Size show me how
Normal Size Small Size show me how
CHEM1211 Exam 4
| Question | Answer |
|---|---|
| Ionization Energy | the energy required to remove an electron from an ion in the gaseous state |
| What is first ionization energy | Energy to remove the first electron |
| Why does ionization energy decrease down a group | Because n increases |
| Why does ionization energy increase across a period | Because Zeff increases |
| Electronegativity | The ability of an atom to attract electrons to itself in a chemical bond |
| Quantum Number Format | (n, l, m sub l, m sub s) |
| n | Principle quantum number, size and energy |
| l | Orbital angular momentum quantum number, shape |
| m sub l | Magnetic quantum number, orientation of orbital |
| m sub s | Electron spin quantum number, orientation of electron spin |
| Principle shell | Orbitals with the same value of n |
| Subshell (sublevel) | Orbitals with the same value of n and l |
| Number of orbitals | 2l+1 |
| s orbital shape | spherical |
| p orbital shape | dumbbell |
| d orbital shape | a lot of dumbbells |
| Node | Zero probability of finding electron density |
| n-1 | Total number of nodes in different orbitals |
| Pauli exclusion principle | No 2 electrons can have the same set of four quantum numbers |
| Degenerate meaning | Orbitals with the same principal number have the same energy |
| Single electron atom | Degenerate |
| Multi electron atom difference | Shielding (screening) and penetration |
| Penetration | The ability of inner (core) electrons to get closer to the nucleus versus outer (valence) electrons |
| Shielding | Because of penetration, the inner electrons shield/screen outer electrons from the nucleus |
| Zeff | Effective nuclear charge, attraction electrons would experience in the absence of intervening electrons |
| Electrons with smaller Zeff values have what | Greater energies |
| Aufbau principle | Electrons fill subshells of the lowest available energy first, and then subshells with the greatest energy |
| Hund's rule | - The lowest energy configuration for an atom is the one having the maximum number of unpaired electrons in a set of degenerate orbitals - Electrons in singly occupied degenerate orbitals must have parallel spins |
| Paramagnetic | Atom or ion that contains unpaired electrons and that is attracted to an external magnetic field |
| Diamagnetic | Atom or ion that in which all electrons are paired and that is not attracted to an external magnetic field |
| Polarizability | The ease of distorting the electron density in an atom or ion |
| Polarizability and atom size relationship | Increasing atom radii increases polarizability (same with ions) |
| Lattice energy | Energy required to separate one mole of a solid ionic compound into its gaseous ions |
| Exothermic | The change in energy when gaseous ions are packed together to form an ionic solid |
| Endothermic | The energy required to separate one mole of a crystalline ionic solid into its gaseous ions |
| Isoelectronic series | Atoms and ions with an identical number of electrons |
| Magnitude and lattice energy relationship | The larger the magnitude, the more favored the lattice energy |
| Ion size and lattice energy relationship | Increased atomic radii decrease energy release |
| Electronegativity | The ability of an atom to attract electrons to itself in a chemical bond |
| Most electronegative element | Fluorine |
| Least electronegative element | Francium |
| Period 2 elements | Especially N,O,F, and Cl- , high electronegativity |
| Unpaired electrons are more likely to? | Form bonds |
| Resonance | When more than one valid Lewis structure can be written for a molecule or ion |
| Resonance hybrid | The actual electronic structure is the average of all resonance structures |
Created by:
ephemeral