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Chemistry Chapters
| Term | Definition |
|---|---|
| Heisenberg Uncertainty principle | It's impossible to know the exact location of an electron in an atom |
| probability | the likelihood of finding the location of electrons |
| Quantum number : n | tells energy level, and how many electrons can fit in each energy level |
| Quantum Number : l | tells sublevels (s, p, d, f) |
| Quantum Number : m | Tells the shape of the orbital |
| Quantum Number : s | tells the spin of electrons (Clockwise or counterclockwise) |
| 2n^2 | Tells how many electrons can be in an energy level |
| S Sublevel | one orbital containing two electrons |
| P Sublevel | 3 orbitals containing six electrons total |
| D sublevel | 5 orbitals containing ten electrons total |
| F sublevel | 7 orbitals containing 14 electrons total |
| orbital | Space occupied by 2 electrons |
| Energy Diagrams | Shows how electrons fill up an atom |
| Pauli Exclusion Principle | no electron within an atom has all 4 quantum numbers the same, no 2 electrons in an atom are alike |
| Electron Configuration | a short-hand method of representing an energy diagram |
| Electron Dot Diagram | used to show outermost valence electrons around an atom |
| Valence electrons | electrons in the highest energy level (s and p are always valence electrons) |
| groups | vertical columns |
| periods | horizontal rows |
| families | groups of elements that have very similar chemical characteristics |
| group 1 | alkali metals |
| group 2 | alkaline earth metals |
| group 17 | halogens |
| group 18 | noble gases |
| metals | left side of periodic table, hard and shiny, lose electrons when chemically reacting, form positive ions, conduct heat and electricity well |
| nonmetals | right side of periodic table, tend to gain electrons when chemically reacting, form negative ions, good insulators, do not conduct heat and electricity well |
| metalloids | separate metals and nonmetals, semi conductors, can gain or lose electrons |
| Lanthanide elements | elements starting with lanthanum at the bottom of the periodic table |
| Actinide elements | elements starting with actinium at the bottom of the periodic table |
| octet rule | elements are more stable when there are 8 electrons around them |
| Why does atomic radius get bigger from top to bottom? | As you go down a group atoms get larger because electrons are in higher energy levels which are further from the nucleus. |
| Why does atomic radius get smaller from left to right? | As you go across the period, the outer electrons are all in the same energy level, and the higher charge means it's getting pulled in further b/c the nuclear charge acts as a magnet |
| ionic radius | radius formed by an ion |
| ion | atom that has gained or lost electrons |
| nonmetal ion | the ion will be larger than the atom due to more electrons in the energy level and like charges want to repel from each other |
| metal ion | the atom will always be larger than the ion because the ion loses electrons which means it will lose an energy level in order to make it stable. |
| Ionization energy | the energy needed to remove one electron from an atom |
| Electron affinity | the ability to gain electrons |
Created by:
24byeri
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