Midterm Chemistry Review – Flashcards
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| Quantitative Observations |
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| specific, describe sth in terms of numbers |
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| Qualitative Observations |
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| rather general, use words to describe an object or event |
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| Scientific Method |
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| a process of studying natural phenomena that involves making observations, forming laws and theories, and testing theories by experimentation. |
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| Hypothesis |
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| a possible explanation for the observation |
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| Theory |
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| a set of assumption put forth to explain some aspect of the observed behavior of matter |
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| Natural Law |
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| a statement that expresses generally observed behavior. |
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| Units |
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| Volume |
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| Mass |
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| Conversion Factor |
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| the ratio. ex: 2.54cm/1inch |
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| Equivalence Statement |
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| ex: 2.54cm=1inch |
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| Dimensional Analysis |
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| changing one unit to another via conversion factors (base on the equivalent statement between the units) |
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| Density |
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| Specific Gravity |
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| the ratio of the density of a given liquid to the density of water at 4dC. density/density -> no units |
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| Matter |
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| any materials of the universe |
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| State of Matter |
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| solid, liquid, gas |
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| Physical Properties |
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| a characteristic of a substance that can change without the substance becoming different substance |
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| Chemical Properties |
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| the ability of a substance to change to a different substance |
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| Physical Change |
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| a change in the form of a substance, but not in its chemical nature; chemical bonds are not broken in a physical change |
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| Chemical Change |
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| the change of substances into other substances through a reorganization of the atoms; a chemical reaction |
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| Element |
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| a substance that cannot be decomposed into simpler substances by chemical or physical means. it consists of atoms all having the same atomic number. |
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| Compound |
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| a substance with constant composition that can be broken down with elements by chemical processes. |
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| Mixture |
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| a material of variable composition of 2 or more substances |
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| Pure Substance |
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| a substance with constant composition |
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| Homogeneous Mixture |
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| a mixture that is the same through out, a solution |
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| Heterogeneous Mixture |
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| a mixture that has different properties in different regions of the mixture |
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| Solution |
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| a homogeneous mixture |
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| Distillation |
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| a method for separating the components of a liquid mixture that depends on differences on the ease of vaporization of the components |
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| Filtration |
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| a method for separating the components of a mixture containing a solid and a liquid. |
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| Energy |
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| the capacity to do work or to cause the flow of heat |
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| Kinetic Energy |
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| energy of motion |
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| Potential Energy |
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| energy of position |
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| Calorie |
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| a unit of measurement for energy; 1 calorie equal the quantity of energy required to heat 1 g of H2O by 1 degree 1cal = 4.184J |
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| Joule |
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| 4.184J = 1cal |
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| Specific Heat / Specific Heat Capacity |
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| the amount of energy required to raise the temperature of 1g of a substance by 1 Celsius degree |
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| Atom |
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| fundamental unit of which elements are composed |
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| Compound, formula |
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| Proton |
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| a positively charged particle in an atomic nucleus |
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| Electron |
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| a negatively charged particle that occupies the space around the nucleus of an atom |
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| Neutron |
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| a particle in the atomic nucleus with a mass approximately equal to that of the proton but with no charge |
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| Isotopes |
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| atom of the same element(the same number of protons) that have different number of neutrons. They have identical atomic numbers but different mass numbers. |
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| Atomic Number |
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| the number of protons in the nucleus of an atom, unique to each element |
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| Mass Number |
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| the total number of protons and neutrons in the atomic nucleus of an atom |
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| Atomic Mass |
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| Nuclear Symbol |
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| includes Symbol, mass number, atomic number, charge (for cation or anion) |
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| Hyphen Notation |
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| [name of element] - [mass number] |
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| Diatomic Molecules |
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| a molecule composed of 2 atoms |
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| Ions, cations, anions |
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| an atom or a group of atoms that has a net positive or negative charge. cation(+) / anion(-) |
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| Dalton's Atomic Theory |
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| 1. Elements are made of tiny particles called atoms. 2. All atoms of a given element are identical. 3. The atoms of a given element are different from those of any other element. 4. Atoms of one element can combine with atoms of other elements to form compounds. A given compounds always has the same relative numbers and type of atoms. 5. Atoms are indivisible in chemical processes. That is, atoms are not created or destroyed in chemical reactions. A chemical reaction simply changes the way the atoms are grouped together. |
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| Changes in Dalton's Atomic Theory |
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| 2. Atoms ARE NOT identical ->isotopes 4. They ARE DIVISIBLE. |
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| Particles and Equipments used by Thompson |
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| Particles and Equipments used by Millikan |
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| oil drop experiment - charge/mass/ratio of an electron |
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| Particles and Equipments used by Rutherford |
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| Gold foil experiment - gold foil, alpha particle |
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| Particles and Equipments used by Chadwick |
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| Atomic Notation |
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| nuclear notation |
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| Ionization Energy |
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| the quantity of energy required to move an electron from a gaseous atom or ion |
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| Electronegativity |
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| a tendency of an atom in a molecule to attract shared electrons to itself |
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| Atomic Radii (size) |
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| increase: to the right, down. |
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| Alkali Metals |
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| group 1 |
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| Alkaline Earth Metals |
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| group 2 |
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| Transition Metals |
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| group 3 - 13 |
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| Lanthanides |
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| series/group of 14 elements following lanthanum on the periodic table, in which the 4f orbitals are being filled |
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| Actinides |
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| series/group of 14 elements following actinium on the periodic table is which the 5f orbitals are being filled |
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| Metals |
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| an element that gives up electrons relatively easily and is typically lustrous, malleable and a good conductor of heat and electricity |
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| Non-metals |
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| an element that does not exhibit metallic characteristics. Chemically, a typical nonmetal accepts electrons from a metal. |
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| Metalloid |
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| semi metal, an element that has both metallic and nonmetallic properties |
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| Noble Gases |
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| last group on periodic table, consists of 8 elements |
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| Group |
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| vertical column of elements having the same electron configuration and similar chemical properties |
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| Period |
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| a horizontal row in the periodic table |
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| Oxidation Number/State |
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| a concept that provides a way to keep track of electron in oxidation-reduction reactions according to certain rules |
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| Trends in Periodic Table |
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| 1. size: increases when go to the left and downward 2. electronegativity: increases when go to the right and upward 3. ionization energy: increases when go to the right and upward ==>reason: #'s of energy levels (left/right) and atomic number (up/down) |
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| Reactant |
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| Product |
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