Unit #4- The Quantum Model of the Atom and Periodic Properties
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elkimbrell on October 31, 2011
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37 terms
Terms | Definitions |
|---|---|
 The Heisenberg Uncertainty Prinicple | This principle states that you cannot determine both the speed and the location of a particular electron at the same time. |
| deBroglie | He investigated the photoelectric effect and determined that electrons had wave-like behavior along with particle behavior and this wave-like behavior gave them a certain frequency. |
| the photoelectric effect | is the energy given off when light strikes metal. |
| Erwin Schrodinger | stated that electrons have both wavelike properties and particle properties and developed an equation that treated electrons in atoms as waves. |
| Max Planck | suggested that hot objects emit energy in small, specific amounts called quanta. |
| Albert Einstein | stated that electromagnetic radiation had wavelike properties, that particles will "stream" and that each particle of light carries a certain a of quantum energy. |
| principle | the quantum number that indicates the size of an atom. |
| azimuthal or angular momentum | the quantum number that indicates the sublevels of the main energy levels. |
| magnetic | the quantum number that indicates the orientation of the electrons on an "x", "y", "z" axis. |
| spin | the quantum number that indicates the direction in which the electrrons are traveling. |
| Hund's Rule | electrons remain unpaired as long as possible before pairing due to their like changes. |
| ECN | a shorthand method used to write the electron configuration of elements. |
| shorthand ECN | uses noble gases to represent sublevels that are perfectly filled. |
| ionic bonds | form between metals and nonmetals and produce compounds with high melting points that are also hard and brittle. Forms by transfer of valence electrons. |
| valence electrons | electrons found in the last main level of an atom. |
| covalent bonds | form when valence electrons are shared between two or more atoms, usually nonmetals. |
| Dmitri Mendeleev | published the first periodic table. |
| noble gases | were originally left out of the first periodic table because they hadn't been discovered yet. |
| Henry Moseley | came up with the periodic law. |
| group 1 | called the Alkali Metals. |
| group 2 | called the Alkaline Earth Metals |
| groups 3-12 | the Transition metals. |
| groups 13-16 | have no name but make the transition from metals to nonmetals. |
| group 17 | called the Halogens. |
| group 18 | called the Noble Gases |
| alkali metals | have one valence electron, exlpode when placed in water and form very strong bases. |
| alkaline earth metals | have two valence electrons, found in many compounds in nature, such as limestone and chlorophyll. |
| transition metals | vary in the number of valence electrons and are known for their brightly colored compounds. |
| halogens | have seven valence electrons, the most active nonmetals, adn can form very strong acids, such as HCI, hydrocholoric stomach acid |
| noble gases | all but helium have 8 valence electrons, all are gases, all perfect, all non-reactive, all inert. |
| atomic radius | one-half of the distance between the nuclei that are bonded together. |
| ionization energy | energy required to remove valence electrons from an atom. |
| electronegativity | the measure of the ability of an atom to attract shared electrons. |
| electron affinity | the attraction an atom has for shared electrons. |
| ions | changed particles |
| cations | postive ions, usually metals. These elements donate valence electrons to another element so that they and the element they are donating to can form a stable compound. |
| anions | negative ions, usually nonmetals. These elements receive valence electrons from another element so that they and the element donating these electrons can form a stable compound. |
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