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Chap 8 - Chem
| Question | Answer |
|---|---|
| What is an electron configuration? | A description of the orbitals occupied by electrons. |
| In a orbital diagram, a half arrow pointing up means what? | It is used to represent an electron in an orbital with a spin up. |
| If there are 2 electrons in an orbital, then their spins must be in what directions? | opposite |
| What is the max amount of electrons per orbital? | 2 |
| What is the Pauli Exclusion principle? | No orbital may have more than two electrons, and they must have opposite spins. (one arrow up, the other down). |
| The lower the value of the ___________, the less energy the sublevel has | principle quantum number |
| Are electrons are more or less attracted to a nucleus with a 2+ charge than a nucleus with a 1+ charge? | more |
| What is "ground state"? | The lowest energy level of an electron. |
| What is Hunds rule? | When filling orbitals that have the same energy (degenerate), place one electron in each before completing pairs (parallel spins-half arrows pointing up). |
| What is the Aufbau principle? | Energy levels and sublevels fill from lowest energy to high? |
| In an atom, then number of these must equal the number of protons. | electrons |
| What is an electron configuration? | The electron configuration is a listing of the sublevels in order of filling with the number of electrons in that sublevel written as a superscript. |
| What are valence electrons? | Usually the highest level s and p electrons. |
| What is important about transition metals and valence electrons? | The concept of the valence electron is less useful for a transition metal than for a main group element because they are less predictable. |
| Electrons in lower energy shells are called what? | core electrons |
| The chemical properties of elements are largely determined by what electrons? | valence electrons. |
| What is the electron configuration of Cr? | [Ar] 4s^1 3d^5 |
| What is the electron configuration of Cu? | [Ar] 4s^1 3d^10 |
| What is the electron configuration of Mo? | [Kr] 5s^1 4d^5 |
| What is the electron configuration of Ru? | [Kr] 5s^1 4d^7 |
| What is the electron configuration of Pd? | [Kr] 5s^0 4d^10 |
| The noble gases usually have 8 valence electrons, but this one only has 2. Which is it? | He |
| Why are noble gases so nonreactive? | They have completely full valence shells (s & p sublevels). |
| The average size of an element's atoms. | atomic radius |
| The size of an atom is related to the distance the _______ electrons are from the nucleus. | valence |
| Traversing down a group adds a ___________. | principal energy level. |
| The size of an atom gets ________ down the column of the periodic table. | larger |
| What is Ionization Energy (IE)? | Minimum energy needed to remove an electron from an atom or ion |
| Electron configurations that result in unpaired electrons mean that the atom or ion will have a net magnetic field; this is called _________. | paramagnetism |
| Electron configurations that result in all paired electrons mean that the atom or ion will have no magnetic field; this is called __________. | diamagnetism |
| Outer electrons are _________ from the nucleus by the core electrons and so are harder to hold onto. | shielded. |
| The shielding causes the outer electrons to....? | move further away from the nucleus |
| Atomic radii of transition metals are ___________ across the d block. | roughly the same size |
| Atomic size decreases as you move from across a _______. | period. |
| Atomic size increases as you move down a ________. | group. |
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