Term
| Law of Increasing Disorder: |
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Definition
| Changes occurring in natural systems always proceed in such a way that the total amount of disorder in the universe is either unchanged or increased. If total disorder is increased, the process is irreversible, also known as the second law of thermodynamics. A reversible process does not change the total amount of disorder in the Universe. An irreversible process increases the total amount of disorder in the Universe. Order never increases. |
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| An irreversible process is one that goes in only one direction; its effects often cannot be undone. Most processes which occur in nature are irreversible. There is more disorder/entropy at the end. |
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| A reversible process goes both forward and backward at the same time. Reversible processes are relatively rare in nature. Disorder is the same/ no increase. |
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Definition
| A quantitative measure of disorder. It increases as the disorder increases. It can be calculated mathematically from the probability of obtaining the system in its current state. A number or amount to represent the disorder at the end. |
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Term
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Definition
| : A small piece of the world around which we mentally draw a box and upon which we focus our attention. It may be a beaker containing an ice cube and warm water or a refrigerator or a living organism. |
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| Everything else besides the system. |
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Term
| How does a fridge fit into the idea of entropy? |
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Definition
| The inside increases order (lowering of temperature/ liquids to solids) so there has to be a big increase of disorder in the form of heat, which is expelled by the fan. |
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Term
| The order of energies from highest order to lowest order |
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Definition
Gravitational Potential Energy and Macroscopic Kinetic Energy
Nuclear Potential Energy
Electrical (household)
Chemical
Thermal Energy (heat or microscopic kinetic energy) |
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Term
| .* A salt shaker and a pepper shaker get knocked off the table and break on the floor. Separating the salt and pepper can be considered an irreversible process. Why? |
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Definition
| You would have to expend a huge amount of energy to separate the grains of pepper and salt. |
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Term
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Definition
| Chemical matter that has defined, unchanging chemical composition. It contains one thing. Examples: Gold, Hydrogen. |
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Definition
| Matter that contains two or more atoms in a fixed, definite proportion. New compounds form when the relative proportions of atoms change. Distilled Water. |
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Definition
| Matter that contains only one kind of atom. It is anything on the Periodic Table. |
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| Matter that contains multiple substances. Many mixtures can be physically separated into their pure components. |
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| A mixture containing two or more compounds, at least one which is a liquid. Examples are orange juice and salt water. |
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Term
| Networking or extended-bonding substances: |
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Definition
| Substances in which every atom or ion interacts strongly with many neighbors. An extended network of linked atoms or ions form. Distinct molecules or ion pairs do not exist in these materials. It has a repeating pattern. Examples are crystals, ice alloys, and diamonds. |
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Definition
| A solid solution of metals. Examples are steel, white gold, bronze, and brass. |
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| Matter that exists as single molecules in the solid, liquid, and gaseous states. |
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| Dry stuff mixed together. Examples are skittles, cement, and cookies. |
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| At least two substances with two or more atoms mixed together. |
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Definition
| Molecules that contain only carbon and hydrogen atoms. Examples are butane, octane, propane (elements of gas). |
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Term
| What governs whether a chemical reaction will happen? |
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Definition
| The fact that if energy decreases, entropy increases. |
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Term
| Mass Spectroscopy measures... |
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Definition
| ...the weight of individual pieces of a substance and compares it to the total weight. |
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Term
| Vibrational Spectroscopy measures... |
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Definition
| ...the energies of the vibrations under infrared light. |
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| Electronic Spectroscopy measures... |
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Definition
| ...Patterns of energy absorption in the light spectrum. |
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Term
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Definition
| Standing electron probability waves for molecules. These standing wave shapes and sizes are different from those fore individual atoms because of the multiple atomic nuclei. Bonds form because electrons have a lower energy than before they bonded. |
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Term
| the two types of orbitals: |
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Definition
| Bonding Molecular Orbitals and Anti-Bonding Molecular Orbitals |
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Term
| Bonding Molecular Orbitals: |
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Definition
| Molecular orbitals that have high electron probability between atomic nuclei in a molecule. When bonding molecular orbitals are occupied by electrons, the high electron density between the nuclei helps hold the nuclei together, contributing to a bond between the atoms. They bond and have a low energy level. |
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Term
| Anti-Bonding Molecular Orbitals |
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Definition
| Molecular orbitals that hav low or no electron probability between atomic nuclei in a molecule and high electron density in areas not between the nuclei. When anti-bonding oribitals are occupied by electrons, the resulting electron density in the anti-bonding orbital helps pull the nuclei apart, weakening any chemical bond that may exist between them. They repel and have a high energy level. |
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Definition
| The starting materials in a chemical reaction, written on the left-hand side of a chemical equation. |
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Definition
| Materials produced in a chemical reaction, written on the right-hand side of a chemical equation. |
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Definition
| The difference between the energy of the isolated reactant molecules and energy of the transition state. If the activation energy is added to a set of reactant molecules, it is possible for them to reach the transition state and go on to form products. Reactants with less than the activation energy to not normally form products. This governs chemical reactions. |
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Definition
| The difference between the entropy or disorder of the isolated reactant molecules and the entropy or disorder of the transition state. Frequently, the activation entropy is unfavorable so that colliding molecules do not always react even if the have sufficient energy to react. This governs chemical reactions. |
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Definition
| A chemical whose presence increases the rate of a chemical reaction without being consumed by the reaction. Catalysts make the energy and or entropy of the transition state more favorable, without affecting thee energies of entropies of the initial reactants or final products. It can lower the energy requirement and/or lower the entropy requirement. |
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| The characteristic o substances that allows them to be worked into desirable shapes or drawn out into wires. The free electrons act as a lubricant to help the atoms slide over each other and they act as a glue to hold the nuclei together. |
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Definition
| The opposite of being transparent. Visible light is absorbed by an opaque object. The free electrons interfere with light waves. |
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| The characteristic of being capable of or producing reflection. The free electrons wiggle up and down and reflect light. |
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| A measure of the degree to which a substance conducts heat. Metals have a high thermal conductivity. Free electrons transfer heat through a material. |
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Definition
| A combination of two or more metals into a single homogeneous substance to attain a desired property. |
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| The chemical bond that binds metal atoms to other metal atoms in forming metal substances. There is one electron held loosely in an outer shell. |
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| A measure of the resistance to the flow of electrical current. |
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Term
| Metals react to heat by becoming... |
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Definition
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Term
| Semi-Conductors react to heat by becoming... |
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| A compound formed between a metal and a non-metal. Ionic compounds are crystalline solids at room temperature. The conduct electricity when molten or dissolved in water. It's ratio of material is in its symbol. |
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| Another name of ionic compounds. |
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Definition
| an electrically charged atom or group of atoms formed by the loss or gain of one or more electrons, as a cation (positive ion), which is created by electron loss and is attracted to the cathode in electrolysis, or as an anion (negative ion), which is created by an electron gain and is attracted to the anode. Ions move in a solution because they are no longer bound. |
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Definition
| Sometimes conducts electricity and sometimes it doesn't. The electrons have to jump the band gap so energy can flow. |
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Definition
| The model used to explain the bonding in ionic compounds. Metal atoms lose electrons, forming positive ions. Non-metal atoms gain electrons forming negative ions. In the salt, positive metal ions are surrounded by negative non-meta ions, and vice versa. It gives away electrons. |
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Term
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Definition
| An atom wants 8 electrons in its out valance shell. |
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Term
| Ionic compound have what type of melting temperatures? |
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Definition
| high melting temperatures. |
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Term
| Salts are clear because... |
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Definition
| ...there are no free electrons to interfere with the light. |
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Term
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Definition
| Materials characterized by chemical bonds that involve sharing electrons. Typically the bonds in covalent substances occur between non-metal atoms. |
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Definition
| A covalent bond involving a pair of electrons shared between the two bound atoms. |
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Definition
| A covalent bond involving two pairs of electrons shard between the two bound atoms. |
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| A covalent bond involving three pairs of electrons shared between the two bound atoms. |
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Definition
| A measure of how strongly atoms attract electrons. Both ionization energy and electron affinity contribute to electronegativity. This affects how much an atom holds onto the electron. If it is a strong hold it is negatively charged. This helps create a dipole.Electronegativity increases for left to right across rows and decreases down columns of the periodic table. |
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Definition
| The separation of positive and negative charge in a polar bond of molecule. Water is a dipole. |
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Definition
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Term
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Definition
| Interactions between hydrogen atoms bound to oxygen, nitrogen, or fluorine with other oxygen, nitrogen, or fluorine atoms. Hydrogen bonds are among the strongest intermolecular interactions. This is a relatively weak bond, but the strongest intermolecular interactions. |
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Definition
| Weak intermolecular attraction arising from the formation of temporary dipoles in non-polar molecules. Also known as van der Waals forces. These occur because of the random motion of molecules. |
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Term
| Hydrogen bonds and electronegativity explain what about water? |
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Definition
| It explains the crystalline structure and why it is liquid at room temperature. |
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Term
| Ionic molecules have what kind of a nucleus? |
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Definition
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Term
| Fats and Oils/ Fatty Acids |
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Definition
| fats and oils are substances that do not dissolve in water, but can dissolve in hydrocarbon liquids. Fats are solid at room temperature; oils are liquid at room temperature. |
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Term
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Definition
| A triglyceride containing three saturated fatty acid molecules.The molecule is filled with the hydrogen spaces. There are no kinks -- it is a straight molecule. |
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Term
| The melting point of saturated fatty acids is... |
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Definition
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Term
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Definition
| : A non-natural form of unsaturated fatty acids in which H atoms are on opposite sides of the double bond. They are straight and stack easily. |
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Term
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Definition
| The interaction between hydrogen atoms bound to oxygen, nitrogen, or fluorine with other oxygen, nitrogen, or fluorine atoms. Hydrogen bonds are among the strongest intermolecular interactions. |
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Term
| Monounsaturated Fats ( as well as poly unsaturated fat) |
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Definition
| Fats containing fatty acids with a single double bond, or more) such as oleic acid.It has one or more kinks. |
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Term
| Cis fats versus Trans Fats |
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Definition
| Cis fats are naturally occurring and the hydrogen atoms are on the top of the bond. Trans fats have the hydrogen on opposite corners of the bond. |
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Definition
| A force that is very short range and extremely strong in relation to the nucleus. It is more important to the nucleus than the electromagnetic force at that range. |
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Term
| Unsaturated fats do not do what well? |
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Definition
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Definition
| building blocks of rocks. |
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Term
| Asbestos can be pulled apart in... |
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Definition
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| Mica can be pulled apart in... |
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Definition
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Term
| Can Quartz be pulled apart? |
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Definition
| No it is a large structure with few weak bonds. |
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| Molecular shapes affect... |
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Definition
| the properties of the crystals. |
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Definition
| An element fires out a alpha particle or helium nucleus and the element loses four in atomic mass and loses two in the atomic number. |
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Definition
| The radioactive decay of an atomic nucleus accompanied by emission of a beta particle. A neutron becomes a proton. The atomic number goes up by one. |
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| The time required for half the nuclei in a sample of a specific isotopic species to undergo radioactive decay. |
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| An element gives out a gamma wave, which releases energy but the atomic number and mass stays the same. |
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| How atoms turn into other atoms. |
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| ...the most stable element. |
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| A nuclear reaction in which nuclei combine to form more massive nuclei with the simultaneous release of energy. |
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Definition
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| A nuclear reaction in which an atomic nucleus, especially a heavy nucleus such as an isotope of uranium, splits into two fragments of comparable mass, releasing energy. |
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| In a nuclear process what changes? |
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Definition
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| Radiometric Dating uses what? |
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Definition
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Term
| Review how to predict a salt equation |
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Definition
K___O_____= K 2 O
Sr ___N____= Sr 3 N 2
Be __P____= Be 3 P 2 |
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