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CHM 106
Chapter 1 Study stack
| Question | Answer |
|---|---|
| table that displays all known chemical elements in a systematic way | periodic table |
| a horizontal row of elements in the periodic table | period |
| a vertical column of elements in the periodic table; also called a family | group |
| the highly reactive metallic elements located in Group 1 of the periodic table high thermal and electrical conductivity, lustre, ductility, and malleability that are characteristic | alkali metals |
| the reactive metallic elements located in Group 2 of the periodic table | alkaline-earth metals |
| the elements that are good conductors of heat and electricity, properties include luster, malleable, high melting points, high density | metals |
| the elements that are usually poor conductors of heat and electricity , properties include gaseous, brittle, and not conductive | nonmetals |
| the metallic elements located in Groups 3–12 of the periodic table elements that have partially filled orbitals. | transition metals |
| Anything that has mass and takes up space | matter |
| An element, only consisting of one substance Hydrogen, Carbon | Pure matter |
| Combination of two or more substances Air we breath, Koolaid, concrete | Mixture |
| Mixture with composition is the same throughout Brass, Koolaid | Homogenous |
| Mixture that can be separated Blood, Trail mix | Heterogenous |
| Two or more elements combined Water, Carbon dioxide | Compound |
| 3 different states of matter | Gas, Liquid, Solid |
| A change that results in the matter changing, however the identity is the same. Freezing water into ice, tearing paper | Physical change |
| A change that results in the chemical identity of a substance. This change is not reversible. Changing from a creating bubbles, heat, light or sparks. Burning wood, baking a cake, vinegar and baking soda | Chemical change |
| Energy takes on various forms, but it is never created or destroyed | Law of conservation |
| Ability to do work | Energy |
| The energy of motion | Kinetic energy |
| Stored energy | Potential energy |
| a substance that takes part in and undergoes change during a reaction. | Reactant |
| a substance that is present at the end of a chemical reaction | Product |
| chemical equation in which the number of each type of atom is equal on the two sides of the equation | Balanced chemical equation |
| refers to how close measurements of the same item are to each other | Precision |
| refers to how close a measurement is to the true or accepted value. | Accuracy |
| the number of digits in a value, often a measurement, that contribute to the degree of accuracy of the value 41g = 2 sig fig 15.3 = 3 0.03 = 1 20.34= 4 | Significant figure |
| a way of writing very large or very small numbers 6.5 ✕ 10^8 or 650,000,000 | Scientific notation |
| Modern day version of the metric system | International System of Units |
| SI unit for temperature | Celcius |
| SI unit for temperature- used in chemistry most often | Kelvin |
| calories in one joule | 4.184 |
| SI unit for energy | Joule |
| A nutritional unit that represents 1000 units | Calorie or Kilocalorie (Cal) |
| Amount of energy needed that raises the temperature of one gram of water by one degree Celsius | calorie |
| SI unit for Volume | Liter |
| Celcius = ____Fahrenheit | 1.8 |
| Kelvin = Celsius + ? | 273 |
| Comparison (also called ratio) of a substance’s mass to its volume One gram of water = 1.0g/mL D=M/V | Density |
| How many mm in a meter? | 1000 |
| How many m in a cm? | 0.01 |
| How many g in a mg? | 1000 |
| How many cL in a L? | 100 |
| Part of the chemical formulas of the reactants and products that indicate the number of atoms of the preceding element | Subscripts |
| Balance this equation Fe + Cl2 = FeCl3 | 2 Fe + 3 Cl2 = 2 FeCl3 |
| Balance this equation C6H5COOH + O2 = CO2 + H2O | 2 C6H5COOH + 15 O2 = 14 CO2 + 6 H2O |
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