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| Question | Answer |
| Atoms vs Molecules | Matter is composed of tiny particles called atoms. Atom: smallest part of an element that is still that element. Molecule: Two or more atoms joined and acting as a unit. |
| Subscripts | Used when more than one atom is in the molecule. |
| Uncertainty in Measurement | A digit that must be estimated is called uncertain. A measurement always has some degree of uncertainty. Record the certain digits and the first uncertain digit (the estimated number). |
| Accuracy vs Precision | Precision:Degree of agreement among several measurements of the same quantity. Accuracy: Agreement of a particular value with the true value. |
| Sig Fig Rules For Zeroes | 1. Nonzero integers always count as significant figures. 2. Leading zeros are zeros that precede all the nonzero digits. These do not count as significant figures. 3.Captive zeros are zeros between nonzero digits. These always count as significant figures. 4. Trailing zeros are zeros at the right end of the number. They are significant only if the number contains a decimal point. |
| sig figs for exact numbers | Exact numbers have an infinite number of significant figures. |
| Exponential or Scientific Notation | 1. c (10^y) 10>c >1 2. Sig figs shown in number easily: 3.00 x 10^2 has two sig figs 3. Advantages: Number of significant figures can be easily indicated and there are fewer zeros are needed to write a very large or very small number. |
| Sig figs in Multiplication/ Division | For multiplication or division, the number of significant figures in the result is the same as the number in the least precise measurement used in the calculation. 1.342 × 5.5 = 7.381 --> 7.4 5.5= least precise so answer should have 2 sig figs |
| Sig figs in Subtraction/ Addition | answer has same number of decimal places as the least precise measurement used in the calculation |
| Dimensional Analysis | Use when converting a given result from one system of units to another. Used in stoichiometry (Chapter 3) |
| Three Systems of Measuring Temp | Fahrenheit, Celsius, and Kelvin |
| Density | 1. Mass of substance per unit volume of the substance. (open heart calculation.....m/v) 2. Common units are g/cm3 or g/mL. |
| Matter | 1. Anything occupying space and having mass. 2. Matter exists in three states: Solid, Liquid, and Gas. |
| Solids, Liquids, Gasses | 1. S: molecules have strong bonds that remain tightly structured 2. L: molecules are more spread out than liquids 3. G: Really spread part |
| Liquid | Has definite volume but no specific shape. Assumes shape of container. |
| Gas | Has no fixed volume or shape. Takes on the shape and volume of its container. |
| Solid | Rigid Has fixed volume and shape. |
| Mixtures | homogenous: Having visibly indistinguishable parts; solution. heterogeneous: Having visibly distinguishable parts. |
| Compound vs Mixture | Compound: substance made up of more than one atom and bound together chemically Mixture: pure substances combined together physically, has no definite composition, ratios of substance can vary |
| Chemical Change | A given substance becomes a new substance or substances with different properties and different composition. |
| Physical Change | Change in the form of a substance, not in its chemical composition. |
| mole | Unit of counting atoms. Avagadro's number 1mole= 6.02 x 10^23 Molecules |
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