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Chapter 8
Periodic Properties of the Elements (Test 3)
| Question | Answer |
|---|---|
| Aufbau procedure | "building up"; adding electrons to one subshell until it's full before moving to the next subshell |
| Pauli Exclusion Principle | a max of 2 electrons per orbital as long as they have opposite spin; no two electrons in an atom can have the same four quantum numbers |
| Hund's Rule | parallel before paired; when filling degenerate orbitals, electrons occupy them singly (one at a time) with parallel spin before pairing up |
| ground state | the lowest energy state |
| excited state | not the lowest energy state |
| degenerate | equal in energy |
| node | a region in space where there is zero probability of finding an electron |
| shell | n (1, 2, 3, ...) |
| subshell | n & l (1s, 2s, 2p, ...) |
| Where is the "s" block found? | the left side |
| Where is the "p" block found? | the right side |
| Where is the "d" block found? | the middle |
| Where is the "f" block found? | the bottom |
| The s block starts with what? | 1s |
| The p block starts with what? | 2p |
| The d block starts with what? | 3d |
| The f block starts with what? | 4f |
| Special electron configurations occur when what are involved? | 1. filled outermost subshells 2. half-filled subshells |
| Which electrons are removed in cations? | the electrons from the outermost shell (which is not necessarily the outermost subshell) |
| isoelectronic | having the same electron configuration |
| paramagnetic | attracted into a magnetic field; having unpaired electrons |
| diamagnetic | slightly repelled by a magnetic field; having all electrons paired |
| valence electrons | outer shell electrons |
| core electrons | inner shell electrons |
| For abbreviated electron configurations... | Put the proceeding noble gas symbol in brackets before writing the valence electrons |
| shielding | the ability of other electrons, especially inner core electrons, to decrease the nuclear attraction for an outer electron |
| effective nuclear charge | the nuclear charge that an electron experiences |
| atomic size trend | increases toward the lower left and decreases toward the upper right |
| ionization energy trend | increases toward the upper right and decreases toward the lower left |
| What is the relationship in size between a cation and its parent atom? | smaller than their parent atom |
| What is the relationship in size between an anion and its parent atom? | larger than their parent atom |
| In an isoelectronic series, what is the trend in size? | size decreases with increasing nuclear charge |
| ionization energy | the energy required to remove an electron from a gaseous atom or ion |
| What are the exceptions in ionization energy? | 1. between column 2 and 13 because it is easier to remove the higher energy p electron than the lower energy s electron. 2. between column 15 and 16 because column 15 has a half-filled subshell |
| When does a "huge jump" occur in ionization energies? | when an inner core electron is removed |
| electron affinity | the energy change (delta E) the occurs when an electron is added to a gaseous atom; some negative and some positive |
| The more electronegative the element, | the more the atom "wants" the electron |
| What groups have positive or near-positive electron affinities? | Groups 2 and 18 |
| What group has the most negative/most exothermic electron affinities? | Group 17 (halogens) |
| What do you use to make individual predictions? | electron configuration and nuclear charge |
Created by:
2nenogirl
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