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Atomic Structure
Science - Atomic Structure
| Term | Definition |
|---|---|
| Atomos | Democritus “How small is small?” Indivisible, the smalles form of matter and the purest |
| Atom | Purest form of matter and is indivisible, sort of |
| Atom: | Protons, neutrons, and electrons |
| Atomic # = | # of protons |
| Atomic Mass # = | # of protons + # of neutrons (rounded to the nearest whole number) |
| Mass # - atomic # = | # of neutrons |
| An atom is electrically neutral when | The # of electrons = the # of protons |
| Radioactive | When atoms have a major difference of the # of p+ and the # of n0 |
| Atoms have the same # of e- | React very similarly when forming compounds |
| Ions | Atoms that have a charge |
| Charge determines by? | # of e- lost or gained |
| Never a gain or loss of | Protons |
| Ions - charge equal | To the # of e- lost or gained |
| Allotropes | Molecules of the same element with different structures, which gives them different chemical properties |
| Allotropes ex. | O, O2, and O3 |
| Isotopes | Atoms with the same element with the same atomic # but with a different mass # |
| Isotopes are also | Atoms with the same # of protons and a different # of neutrons |
| Why do isotopes have different properties? | The different # of neutrons causes them to have different properties |
| Weighted Average Isotopic Mass | The isotope in the greatest abundance on Earth, it’s mass has the greatest influence on the overall mass of the element because it is weighted |
| Weighted Average Isotopic Mass: Steps | 1. Convert all the percentages to decimal by dividing by 100. 2. Multiply the decimal by the mass # of each isotope. Place these calculations in parentheses. 3. Add the answers together. *Your answer should always be very close to the mass # of the i |
| The gain or loss of e- is always from the last energy level | For an ion |
| Electrons are held in the orbit | Due to the attraction to the + nucleus and the energy they give off as they orbit |
| The amount of energy an e- has determines | How far away it can get from the nucleus |
| The more energy the ________ it can go | Further away |
| Kinetic energy | Is the energy produced in an object |
| Potential energy | Is the energy stored in an object |
| Spectral lines | The principle energy level that an e- occupies has to do with how much energy it has |
| The amount of energy the e- has | Determines how much it can resist the (+) attraction of the nucleus |
| The more energy the ________ a PEL it will occupy | Further away (Ground State) |
| Ground State | Electron is “stable” |
| When a “free” e- hits an e- in a PEL | There is a transfer of kinetic energy |
| Transfer of kinetic energy allows e- | To move to a further energy level |
| Excited State | e- is unstable |
| To return to Ground State | e- has to give off the excess energy it gained |
| Spectral lines are produced | When e- returns to ground state |
| The color of the Spectral lines produced is | Unique to each element on the P.T. so Spectral lines are used for element identification |
| Electron-Dot Notation | Kernel, Valence Shell, and E-dot notation (Lewis Structure) |
| Kernel | All the parts of the atom excluding the outermost energy level |
| Valence Shell | The outermost energy level |
| The e- on the valence shell are the most significant because | They are the e- involved in bonding when the atom forms a compound |
| E-dot notation (Lewis Structures) | Invented to just represent the atom and its valence e- |
| Last number in the e- configuration | Is the number of valence e- |
| E-dot notation step: | Take the symbol or the element and surround it with dots = to the # of valence e- |
| No element has more than _____ valence e- | 8 |
| The number of valence e- determines | An element’s chemical characteristics |
| If two different atoms have the same # of val. e- | Then they have similar chemical properties |
| Quantum Mechanics | Invented by Albert Einstein |
| 1st Quantum # | Represents the number of the floor in the “Hotel” = # of the PEL; Maximum # n can be equal to is 7 |
| 2nd Quantum # | Represents the number of rooms that are on that floor. = # of orbitals on the PEL |
| 3rd Quantum # | Is the maximum # of people that can fit on that floor. = the maximum number of e- that can exist on that PEL |
| n= | # of the PEL (floor of the hotel) |
| n2= | The number of orbitals per PEL |
| (2n2)= | Maximum number of e- per PEL |
| Orbital Notation | Each “floor” or PEL starts w/ an s-sub level which is made up of one orbital (or box), that can hold 2 e- (arrows going in opposite directions) |
| The s-sub level is found on every PEL and is | The first sub level is filled with electrons on every PEL |
| Depending on the number of orbitals or rooms on that floor | The next type of rooms are a a p-sub level made of 3 orbitals connected |
| Before it has two | Each orbital must have one e- in it |
| The p-sub level is found on | PEL’s 2-7 |
| The next sub level is called a d-sub level | It is made up of 5 orbitals connected |
| D-sub level is found on | PEL’s 3-7 |
| The last sub level is the f-sub level | Is made up of 7 orbitals connected and is filled just like the p and d sub levels |
| F-sub level is found on | PEL’s 4-7 |
Created by:
Alisha-248
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