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P.S. Ch. 17 Vocab
Vocab only
| Term | Definition |
|---|---|
| Element | Any pure substance that is made of only one kind of atom |
| Ancient Greeks | were the first to define elements as the basic building blocks of matter. |
| Aristotle | believed in four elements air, fire, earth and water |
| Alchemy | included aspects of chemistry, philosophy, religion, metallurgy, medicine, and art. |
| Many alchemists | considered shifty, and their main objective was to make gold out of valueless materials like leat. They purified substances that were later understood to be elements though. |
| Alchemy | became a real science in the 17th and 18th centuries. |
| Isaac Newton Robert Boyle and Antoine Lavoisier | believed that true scientific knowledge was gained by observing, experimenting, and reasoning |
| Monotonic Elements | He, Ne, Ar, Kr, Xe, Rn |
| Monotonic Elements | have 1 atom in natural state |
| Diatomic Elements | 2 atoms in natural state |
| Diatomic Elements | Hydrogen, Nitrogen, Oxygen, Fluorine, Chlorine, Bromine, Iodine |
| Dmitri Mendeleev | Arranged the elements into what eventually became the periodic table used today |
| Johann Dobereiner | In 1829 a chemist placed elements in order of increasing MASS, the middle element often displayed properties that were mid-way between the other 2. With his, almost all the groups contained 3 elements so he called them TRIADS. |
| Johann Dobereiner | His idea was important because new elements became better understood, chemist started to recognize patterns in properties. |
| Periodicity | The repetition of certain properties at regular intervals when elements were placed in order of atomic MASS |
| John Newlands | Arranged the elements in the table in order of the their increasing atomic masses. When arranged in seven columns he noted that in most cases every 8th element had similar properties. He called these octaves. |
| Dmitri Mendeleev | Organized elements by increasing atomic masses as well. He arranged the cards until he had grouped similar elements in rows. His has IMPORTANT feature....BLANK SPOTS! These were spots for undiscovered elements. He credited for our current periodic table. |
| Dmitri Mendeleev | He called the principle that the properties of elements vary in a periodic or recurring pattern with their atomic MASSES the Periodic Law. |
| Periodic law | The principle that the properties of elements vary in a periodic or recurring pattern with their atomic masses |
| Henry Moseley | Discovered how to use x-rays to count the protons in an atom's nucleus to find an elements atomic number. |
| Henry Moseley | Arranged the elements in order of increasing atomic number. Led to the revision of the periodic law of elements. NOW it is the properties of the elements vary with their atomic NUMBERS in a periodic way. |
| Metals | They belong to families with relatively few valence electrons. These valence electrons are not held very strongly and are easily removed. |
| Metals | If it were not for these "loose" electrons, metals would not have a metallic luster (shiny), be malleable (can be molded), ductile (make long stringy wires), or conduct electricity. |
| Non-metals | Hold their electrons tightly, so their properties are very different from metals |
| Metals | Luster, Malleable, Conduct electricity, Ductile (long skinny strings like copper wires or ducts) |
| Non-metals | Lack luster, Brittle, Don't conduct electricity, Are not ductile |
| Periods or Series | The horizontal rows of the periodic table |
| Similar | The elements in the same period do NOT have ______________ properties |
| Period number | Tells how many MAIN ENERGY LEVELS the elements in that period have in their GROUND STATE. |
| Ground state | Lowest energy state for the electrons |
| Period number | Equals the energy level containing the valence electrons |
| Number of valence electrons | Is important in determining the chemical and many physical properties of an element |
| Distance between its valence electrons and nucleus | Many properties of an atom depend on the _______________________________________________________________________________. |
| More, larger | The ________ energy levels an atom has, the __________ it is. |
| Larger | The __________ it is, the farther the valence electrons are from the nucleus |
| Attraction, weaker | Thus the ____________ of the nucleus on the valence electrons is __________. |
| The Second Law of Thermodynamics | The tendency for atoms to form bonds is governed by |
| The Second Law of Thermodynamics | This states that ALL NATURAL PROCESSES MOVE TOWARD A STATE OF MINIMUM ENERGY |
| Octet rule | Atoms generally are most stable when they have a full 8 electrons in their valence energy level. Some exceptions are Hydrogen ( 1 electron, 1 energy that only holds 2 electrons max), and the next 3 elements Li,Be,B,He too. |
| Gain, lose, share | Atoms can _______, __________, or ___________ electrons to get to the octet |
| Ions | When atoms gain and lose electrons they make ________. These have charges. Then the opposite charges are attracted to each other |
| Electron affinity | Deals with the strength of attraction of electrons to UNBONDED ATOMS |
| High, lose, small | Atoms with _______ electron affinities will take or share electrons from other atoms. Atoms with low electrons will _________ their valence electrons or have a very _______ part in sharing them when bonding. |
| Electronegativity | Deals with an atom's ability to attract and hold electrons when BONDED TO OTHER ATOMS. |
| more, more | The _____ electronegative the ____ more likely it will take electrons. |
| Fluorine | Strongest/most electronegative |
| Francium | Weakest/Least electronegative |
| Covalent bonds | Non-metal/non-metal = sharing electrons (work together) |
| Ionic bonds | Metal/non-metal = giving away and taking electrons |
| Ionic bonds | Happens when there is a BIG difference in the electronegativities of the elements |
| Metallic bonds | Metal/metal = everyone shares the electrons |
| Electron Sea Theory | Atoms with weak electronegativities usually have only a few loosely held valence electrons. These atoms bond by sharing their easily lost electrons among many atoms. These mobile electrons are not associated with any specific nucleus. |
| Electron Sea Theory | Electrons move freely/easily = malleable Socialism = equally sharing electrons |
Created by:
MaryCox
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