Chem Unit 2
Quiz yourself by thinking what should be in
each of the black spaces below before clicking
on it to display the answer.
Help!
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| Atoms | composed of electrons, protons, and nuetrons
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| Molecules | combinations of atoms
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| Ions | changed particles
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| Aontoine Lavoisier: Law of Conservation of Mass or Matter (1790) | Total mass remains constant during a chemical reaction; or total mas of reactants=total mass of products
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| Joseph Proust: Law of Constant Composition (law of definite properties) | All samples of a compound have the same composition, or all samples have the same proportion by mass of the elements present.
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| Dalton's Atomic theory of Matter | 1) all mater consists of small, indivisible particles call atoms 2) all atoms of a given element are alike but atom of any one element are different from the atoms of every other element.
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| Compounds | formed when atoms of different elements unite in small whole number ratios (part of atomic theory of matter)
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| Chemical reactions | involve rearrangments of atoms: no atoms are created, destroyed or broken apart in a chemical reaction-dalton say atoms are indvisible and indestructable
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| Law of Multiple Proportions: Dalton | a given set of elements may combine to produce two or more different compounds, each with a unique compound.
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| Thomson 1897 | Discovered electrons through experiments for conduction of electricity by gases at low pressures. led to plum pudding model
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| Robert MIllikan and oil drop experiment | obtained the charge on an electron allowing the calculation of the mass of an electron
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| Rutherford and Gold Foil Experiments | gold foil hit with "a" particles. Some deflected, led to discovery of nucleus w/ protons
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| Protons | mass nearly equal to the H atom. Postive charge=negative electron charge in a nuetral atom
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| Nutrons (chadwick 1932) | mass slightly greater than proton. help disperse the strong repulsion of positive charges
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| A | mass number; protons + nuetrons
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| Z | Atomic Number; number of protons
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| Isotopes | atoms of the same element but different mass number.
Boron -10: 10B
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Boron -11: 11B
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| Ions | atoms gain electrons to become negative ions or anoins. charge=p+ -e-
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| Atomic mass | the relative mass of an atom compared to a standard (carbon-12). It is not equal to the mass number.
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| Isotopic Abundance | the percent or fraction of each isotope found in nature.
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| Radioactive isotopes | unstable and decay over time. They emit other particles and are transformed into other elements
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| Particles Emitted | High speed electrons: B (beta) particles Helium nuclei: Alpha (a) particles High energy light: Gamma (y) particles
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| Metals | shrink, smooth, solid at room temp, good conductor of heat and electricity, malleable (able to become sheet metal) and ducible (drawn into wire)
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| Metaloids | physical and chemical properties of both metals and non-metals
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| Non-metals | low melting and boiling points, brittle, dull-looking solids, porr conductors of heat and electricity
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| Mendeleev | developed modern periodic table according to atomic weight. orgranized table to predict undiscovered elements
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| Periodic law | element properties are periodic functions of their ATOMIC NUMBERS (not wieght)
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| Moseley | arranged the periodic table in order of increasing atomic numbers
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| Molecule | a group of two or more atoms held together ina definite shape by covalent bonds. (shared e-)
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| Empirical | the simplest whole number ratio of elements ina compound. CH20
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| Molecular | gives the ACTUAL number of each kind of atom in a molecule. C6H12O6
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| Structural | show how atoms are attached to one another
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| Ions: cations | positive ions
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| anions | negative ions
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| Polyatomic | a group of atoms w/ a charge
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| Ionic Compounds | cations and anions, held together by electrostate attraction: formulas simplest ratio of numbers of atoms and represent one formula.
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