Intro into Chemistry – Flashcards
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| Chemistry |
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| Science that deals with the composition and properties of matter |
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| Matter |
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| anything that occupies space and displays the properties of mass and energy(inertia) |
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| Compostition |
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| refers the the parts of compounds of a sample of matter and their relative proportions |
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| Properties |
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| re those qualities or attributes that we an use to distinguish one sample of matter from another |
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| Physical Property |
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| is one that a sample of matter displays without chaninging its composition i.e. color staying the same and so forth |
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| Physical Change |
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| when the physical properties of a subject change but its composition stays the same |
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| Chemical Change(reaction) |
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| when one or more kinds of matter are converted to new kinds of matter with different compositions |
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| Chemical Property |
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| the ability or inability of a sample of matter to undergo a change in composition under stated conditions |
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| Atoms |
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| the very tiny units that make up matter |
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| Elements |
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| 114 substances of atoms that make up these pieces that make matter |
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| Compounds |
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| substances comprised of atoms of two or more elements joined together |
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| Molecule |
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| the smallest entity having the same proportions of the constituent atoms as does the compound itself |
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| Substance |
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| is a element or compound that has constant properties throughout a a given sample and from one sample to another |
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| Homogeneous mixture |
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| a solution said to be uniform throughout in both composition and properties |
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| Heterogeneous mixtures |
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| (i.e. sand and water) components of a substance that separate into distinct regions |
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| Solid |
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| where atoms and molecules are in close contact, in sometimes highly organized sections called crystals |
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| Liquid |
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| where the atoms or molecules are separated in somewhat greater distances than that of a solid |
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| Gas |
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| distances of molecules and atoms are very much spread apart. Gas always expands to full container |
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| SI Units |
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| Ssteme Internationale d'Unites, which is the modern version of the metric system used for scientific measuring |
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| Define Units and symbol of Length |
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| meter m |
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| Define Units and symbol of Mass |
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| kilogram kg |
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| Define Units and symbol of Time |
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| second s |
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| Define Units and symbol of Temperature |
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| kelvin K |
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| Define Units and symbol of Amount of Substance |
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| mole mol |
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| Define Units and symbol of Electric Current |
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| ampere A |
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| Define Units and symbol of luminous intensity |
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| candela cd |
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| 10^1 |
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| deca(d) |
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| 10^2 |
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| Hecto(h) |
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| 10^3 |
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| Kilo(k) |
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| 10^6 |
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| Mega(M) |
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| 10^9 |
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| giga(G) |
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| 10^12 |
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| Tera(T) |
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| 10^-1 |
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| Deci(d) |
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| 10^-2 |
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| centi(c) |
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| 10^-3 |
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| milli(m) |
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| 10^6 |
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| micro |
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| 10^9 |
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| nano(n) |
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| Mass |
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| describes the quantity of matter in an object. In SI, mass= 1gram |
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| Celsius |
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| melting point of ice is 0 degrees while the oiling point is 100 |
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| Fahreneit |
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| melting point of ice is 32 degress and the boiling point is 212 |
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| Kelvin |
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| assigns a value of zero to the lowest possible temperature. No negative Kelvin numbers -273.15C =0K |
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| Density |
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| ration of mass to volume, aka mass(m)/volume(v) |
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| Extensive property |
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| where mass and volume are both dependent on the quantity of matter observed |
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| Intensive property |
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| Where mass and volume are independent of amount of matter observed, aka the density is equal on both a glass of water and a pool |
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| Precision |
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| referrs to the degree of reproductivity of a measured quantity, that is closeness of agreement when the same quantity is measured several times |
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| Accuracy |
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| refers to how close a measured value is to accepted or actual value |
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| Law of Conservation of mass |
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| Lavoisier's law that the total mass of a substance present after a chemical reaction is the same as the total mass of substances before the reaction |
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| Law of Constant Composition(definite proportions) |
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| Proust's law that all samples of a compound have the same composition-the same proportions by mass of constituent elements |
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| Daltons Atomic Theory(3 points) |
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| 1.Each element is made of indivisible particles called atoms 2. All atoms of a single element are alike in mass and other properties 3.In each of their compounds different elements combine in simple ratios |
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| Law of multiple proportions |
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| If two elements form more than a single compound, the masses of one element combined with a fixed mass of the second are in the ration of small whole numbers |
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| Cathode ray |
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| type of radiation emitted by negative terminal(cathode) |
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| Electrolysis |
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| the decompositon of a substance either in molten state or in an electrolyte solution, by means of electric current |
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| Protons |
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| positively charged fundamental particles of matter in nuclei of atoms |
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| Neutrons |
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| neutral particles |
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| Atomic number |
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| given number of protons in an atom |
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| Mass number |
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| total number of protons and neutrons in an atom |
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| Neutron number |
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| Mass number - proton number |
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| Isotopes |
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| atoms that have the same atomic number but different mass numbers |
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| Ions |
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| when atoms lose or gain electrons in the course of a chemical reaction, form ions, which carry net charges |
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| Molecular compound |
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| a small number of nonmetal atoms held together by covalent bonds |
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| Chemical formulas |
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| what represents molecular compounds which indicate the elements present and the relative number of atoms of each element |
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| empirical formula |
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| simplest formulas for compounds:shows types of atoms present and their relative numbers |
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| Molecular formula |
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| based on actual molecule of a compound |
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| Structural Formula |
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| shows the order in which atoms are bonded together in a molecule and by what types of bonds |
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| ionic compound |
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| compound made up of positive and negative ions joined together by electrostatic forces of attraction |
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| cation |
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| result of electron transfer that takes an electron away |
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| anion |
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| result of electron transfer that adds an electron, making to be negatively charged |
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| 1 & 2 & 3 & 4 |
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| mono & di & tri & tetra |
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| 5 & 6 & 7 & 8 & 9 & 10 |
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| penta & hexa & hepta & octa & nona & deca |
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