front 1 Homogeneous Mixture | back 1 Mixture with uniform density throughout and no distinguishable coponents. |
front 2 Heterogeneous Mixture | back 2 Mixture in which the components are readily distinguished. |
front 3 Physical Change | back 3 A change in which the checmical composition of a substance remains the same. |
front 4 Chemical Change | back 4 A change in which the chemical bonds are broken and reformed to create a new and different substance. |
front 5 Element | back 5 The simplest of substances and is represented by a specific letter or combinations of letters. |
front 6 Compounds | back 6 Combinations of eleements in whole number ratios. |
front 7 Law of Conservation of Mass | back 7 Mass cannot be created or destroyed during a chemical reaction. |
front 8 Chemical Reaction | back 8 The breaking of bonds and the reforming of new bonds to create new chemical compounds with different chemical forumulas and different chemical properties. |
front 9 Five main types of chemical reactions. | back 9 syntehesis, decomposition, combusion, single replacement, double replacement |
front 10 Syntehsis Reaction | back 10 Two elements combine to form a product. |
front 11 Decomposition Reaction | back 11 The breaking of a compound into component parts. |
front 12 Combustion Reaction | back 12 The reaction of a compound or element with oxygen. In the combusiton of a hydrocarbon carbon dioxide and water are produced. |
front 13 Replacement Reactions | back 13 Reaction involoving ionic compounds. The reactivity of the ionic compounds determines whether the reaction will take place or not. Can be single replacement or double replacement reaction. |
front 14 Single Replacement Reaction | back 14 Reaction between a more active metal reacting with an ionic compound containing a less active metal to produce a new compound ex. copper wire reacting with aqueous silver nitrate. |
front 15 Double Replacement Reaction | back 15 Reaction involving two ionic compounds where the positive ion from one compound combines with the negative ion of the other compound. The result it two new ionic compounds that have switches partners. |
front 16 Atomic Number | back 16 The number of protons in a given element. |
front 17 Atomic Weight/ Atomic mass number | back 17 An average of the masses of each of the iostopes of an element as they occur in mature. (Represents the number of protons and the number of neutrons in an element because electrons essentially have no mass). |
front 18 Calculating the number of neutrons in a given isotope of an element. | back 18 Subtract the atomic number from the mass number. |
front 19 Charge of Elements in Group IA | back 19 +1 |
front 20 Charge of Elements in Group IIA | back 20 +2 |
front 21 Charge of Elements in Group IIIA | back 21 +3 |
front 22 How do you calculate density? | back 22 d = m/v |
front 23 Specific Gravity | back 23 Density of an object realtive to water. No units. |
front 24 Kinetic Energy | back 24 Energy of motion. |
front 25 Potential Energy | back 25 Stored energy. |
front 26 Heat | back 26 Form of energy, measured in calories. |
front 27 calorie | back 27 The amount of heat necessary to raise the temperature of 1g of water by 1 degree celsius. |
front 28 Mixture | back 28 Combination of two or more pure substances. |
front 29 Isotope | back 29 Atoms with the same number of protons but different numbers of neutrons. |
front 30 Noble Gases | back 30 Elements in group 8A of the periodic table. Have no charge and are gases under normal conditions. (Helium, Neon, Argon, Krypton, Xenon, Radon) |
front 31 Electron Configuration | back 31 Shell Electrons (max)
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front 32 Halogens | back 32 Elements of group 7A. Have a charge of -1. Fluorine, Chlorine, Bromine, Iodine. Form compounds with sodium in the form NaX. |
front 33 Alkali Metals | back 33 Elements of group 1A. Have a charge of +1. Lithium, Sodium, Potassium, Rubidium, Cesium. React with water to form hydrogen gas and a metal hydroxide (MOH) + H2. Also from compounds with the halogens in the form MX. Ex. NaCl. |
front 34 Anion | back 34 An ion with a negative charge. |
front 35 Cation | back 35 An ion with a positive charge. |
front 36 Ionic bond | back 36 A chemical bond resulting from the attraction between a positive ion and a negative ion. |
front 37 Covalent Bond | back 37 A chemical bond resulting from the sharing of electrons between two atoms. |
front 38 Polar covlaent bond | back 38 A covalent bond between two atoms where electrons are not shared equally between the two atoms. |
front 39 Dipole | back 39 Created when atoms are joined by a polar covalent bond. The positive end of a dipole in one compound will be attracted to the negative dipole in another compound creating weak attraction between the two compounds. |
front 40 Strongest type of chemical bond. | back 40 Covalent bond |
front 41 Weakest typ of chemical bond. | back 41 Ionic bond |
front 42 Strongest of intermolecular forces. | back 42 Hydrogen bond |
front 43 Weakest of intermolecular forces. | back 43 Dispersion forces. |
front 44 Hydrogen bond. | back 44 Attraction for a hydrogen atom by a highly electronegative element. Generally involve fluorine, chlorine, oxygen, and nitrogen. |
front 45 Dispersion Forces | back 45 Temporary dipole created when moving electrons within an element or compound concentrate themselves on one side of an atom. Usually found in nonpolar covalent compounds. |
front 46 Van der Walls forces | back 46 Another name for dispersion forces, dipole interactions. |
front 47 Charge of elements in group VA. | back 47 -3 |
front 48 Charge of elements in group VI A | back 48 -2 |
front 49 Charge of elements in group VII A | back 49 -1 |
front 50 How many known elements are there? | back 50 109 |
front 51 What is a mole. | back 51 An amount of an element equal to its atomic weight in grams. Also described by the amount of a substance that contains 6.02 x 10 23rd particles of that substance. |
front 52 What is alpha radiation? | back 52 The emission of helium ions that consist of 2 protons and 2 neutrons (thus having a +2 charge). Alpha particles can be stopped by a piece of paper. |
front 53 What is beta radiation? | back 53 The product of the decomposition of a neutron and is composed of high energy high-speed electrons. They are negatively charged and have basically no mass. Beta particles can be stopped by aluminum foil. |
front 54 What is gamma radiation? | back 54 High-energy electromagnetic radition that lacks charge and mass. Gamma radiation can be stopped by several feet of concrete or several inches of lead. |
front 55 Radioactivity | back 55 The emission of particle sfrom an unstable nucleus. Exists in three forms alpha, beta, and gama radiation. |
front 56 Molar mass | back 56 The mass of one mole of a compound. |
front 57 Sublimation | back 57 When a substance changes from a solid to a gas without first becoming a liquid. |
front 58 Ideal gas law | back 58 PV=nRT (n is equal to the number of moles of the substance and R is the gas constant 0.082) |
front 59 Molarity | back 59 The number of moles of solute in 1 liter of solution. |
front 60 Redox reactions | back 60 Reactions that involve the transfer of electrons from one element to another. |
front 61 Oxidation | back 61 The loss of electrons in an redox reaction. |
front 62 Reduction | back 62 The gain of electrons in a redox reaction. |
front 63 Rules for determining oxidation state. | back 63 1. Elemental atoms have an oxidation number of zero.
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front 64 Acids | back 64 - act as hydrogen-ion donors.
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front 65 Bases | back 65 - produce OH- in solution.
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front 66 Neutralization | back 66 Process which occurs when an acid and a base react tot produce a salt and water. The result is a pH near 7. |