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Flashcards by wilsjenn285, updated more than 1 year ago
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Created by wilsjenn285
over 8 years ago
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| Question | Answer |
| Definitions PURE SUBSTANCE - Atoms of only one kind; fixed physical and chemical properties CHEMICAL FAMILY - Groups on the periodic table = alkali metals, alkaline earth metals, transition metals, halogens... etc. MOLECULAR COMPOUND - A pure substance formed by 2 or more non-metals | Definitions POLYATOMIC ION - An ion made up of more than one atom that acts as a single particle ATOMIC NUMBER - The number that is given to each element on the periodic table CHEMICAL TEST - Chemical tests for Hydrogen, Oxygen, and Carbon Dioxide |
| Definitions BALANCED CHEMICAL EQUATION - Both sides of chemical equation have the same amount of each element WORD EQUATION - A chemical equation using only words and not chemical symbols PHYSICAL PROPERTY - The physical attributes of a chemical (EX. 5 senses) | Definitions CHEMICAL PROPERTY - Chemical attributes of a chemcial (EX. what state is it in) MIXTURE - It doesn't have a fixed composition ATOMIC MASS - The mass of an element on the periodic table |
| Definitions VALANCE SHELL - The outermost shell of an element ION - It is a charged particle that results when an atom gains or looses one or more elections ELEMENT - A pure substance that can't be broken down into simpler substances | Defintions IONIC COMPOUND - Consist s of a metal and a non-metal or a group of non metals. They contain ions (+ = Cation, - = Anion) COVALENT BOND - Used to setermine how many bonds each element will form COMPOUND - 2 or more atoms combined SKELETAL EQUATION-a chemical equation |
| Definitions PHYSICAL CHANGE - A change that occurs during a reaction to change the chemical properties of a chemical CHEMICAL CHANGE - A change that occurs during a reaction to change the chemical properties of a chemical - these changes are irreversible | Definitions SUPER 7/HOFBRINCL - Hydrogen, Oxygen, Fluorine, Iodine, Nitrogen, Chlorine, When in a chemcial equation, they always have 2 EX, Cl2, O2, H2, F2, Br2, I2, N2 |
| Conserving Mass - The law of conserving matter states matter can neither be destroyed or created - The energy from the reactants is transferred to the products, that's why they must be balanced | Reactions SYNTHESIS - Take 2 elements and combine them together to produce a single compound EX. O2 + C = CO2 DECOMPOSITION - When a large compound is broken down into smaller parts EX. 2H2O = 2H2 + O2 |
| Reactions SINGLE DISPLACEMENT - When a element reacts with a composition and displaces one of the element out of the compound. Metals can only displace metals, and gasses can only displace gasses EX. 3K2SO4 + 4Al = 1Al(SO4)3 + 6K | Reactions DOUBLE DISPLACEMENT - Two compounds combine and switch their reactants with each other. Metals can only displace metals, and gasses can only displace gasses EX. 1CaBr2 + 1Ba(n03)2 = 1Ca(NO3)2 + 1BaBr2 |
| Reactions COMBUSTION - Two elements combine to produce a compound, water, and energy EX. 2CuH10 + 6O2 = 8CO2 + 10H2O + Energy ACID - An acid and a base combine to produce an ionic compound and water EX. 1HBr + 1KO1 = 1KBr + 1H20 | Elements and the Periodic Table ALKALI METALS - The first group on the periodic table. The elements in the first column on the periodic table ALKALINE EARTH METALS - The second group on the periodic table. The elements in the second column on the periodic table |
| Elements and the Periodic Table HALOGENS - The eighth group on the periodic table. The elements in the 17th column of the period table NOBLE GASSES - The last group on the periodic table. The elements in the 18th column on the periodic table | Charges - The charge on an atom that looses electrons is positive. The charge on the atom that gains electrons is negative |
| Molecular Compounds - Molecular compounds are made from 2 or more atoms sharing electrons between them to fill their valance shells - Find the amount of electrons in the valance shell for the element and balance it with the second element - a proofing system is used to describe how many of each element is in each molecule. If the has only one atom the "mono" prefix isn't written, but ONLY for the first element. 1 = Mono, 2 = DI, 3 = Tri, 4= Tetra, 5 = Penta, 6 = Hecta, 7 = Hepta, 8 = Octa, 9 = Nona, 10 = Deca | Polyatomic Compounds - Groups of non-metals that together form a single ion, most polyatomic ions are called anions - Choose an element from the periodic table and mix it with an anion to produce a polyatomic ion,make sure the chemcials are balanced - Use the symbols given in the chemcial equation and find the element and the anion on the periodic table |
| Ionic Compounds - Consists of a metal and a non-metal or a group of non-metals. They contain ions (+ = Cation, - = Anion) - In and iconic compound, the charge from the cation (+) and the anion (-) must be balanced so that the molecule is neutral. We take multiple of each to achieve neutrality - Find the name of the ion on the periodic table using the chemical symbol. On the second element add ide, ite, or ate in exchange for the last few letters. ONLY on the SECOND element | Acids and Bases ACIDS - Contain H+ - React with metals to produce H2 gas - Taste sour - Acids neutralize bases - Conduct electricity (electrolights) (non-electrolights) - PH < 7 (Less than 7) - PH = Potential Hydrogen - Indicators turn red - Corrosive - Litmus indicator = red - Phenuthaline = clear |
| Acids and Bases BASES - Contain OH- - Taste bitter - Bases neutralize acids - Conduct electricity (electrolights) (non-electrolights) - PH > 7 (Greater than 7) - PH = Potential Hydrogen - Indicators turn pink - Corrosive - Litmus indicators = pink Phenuthaline = pink | COMPLETED CHEMISTRY FOR GRADE 10!!! |
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