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Chem CH 1
| Term | Definition |
|---|---|
| Chemistry | study of the composition of substances (matter) & the changes they undergo |
| Scientific Method | general procedures used in science to problem solve |
| 4 steps of the scientific method | - observation: questions - hypothesis: a tentative assumption - experiment: test - theory: alter, reject, accepting/summarizes, hypothesis |
| Scientific Notation | used to represent vary small or large numbers |
| Positive Exponents | - large #'s move decimal to left |
| Negative Exponents | - small #'s move decimal to right |
| Inexact Numbers | - are obtained through measurements or observation - contains some uncertainty |
| Exact Numbers | are obtained by counting items or from established equivalents |
| Accuracy | close to accepted (true) value |
| Precision | how close values are to each reproducibility |
| Significant Figures | inexact (measured) #'s that have a final digit that is estimated |
| In sig figs how do you measure | measure one past the last calibrated mark place values |
| uncertainty depends on what when measured | depends on the device used to measure |
| sig figs do not apply to | to exact #'s |
| english to english or metric to metric are considered | exact numbers |
| Specific Gravity | compares the density of a substance to a density of water at 4 degrees celsius |
| Density of water equals | 1.00 g/ml |
| what is specific gravity's unit | has no units |
| what measures specific gravity | hydrometer |
| Matter | - anything that exists & takes up space - natural, synthetic - classified by components; |
| Naturally Occurring | it is isolated from natural resources |
| Synthetic | They are produced by chemists in a laboratory |
| Pure Substances | - fixed/definite composition, elements, & compounds - composed of a single component - has a constant composition regardless of the sample size and origin |
| pure substance | cannot be broken down to other pure substances by any physical change |
| Element | - consists of 1 type of atom - can't be broken down by ordinary chemical means pure substance Ex. Ag = gold |
| Compounds | consists of 2+ elements; chemically combined in a definite ratios pure substance Ex. CO = Carbon Monoxide |
| Mixture | - 2+ substances physically mixed not chemically combined, composition varies; can be separated by psychical means - mixtures can be liquid, solid, gas Ex. salt & pepper shaker from Subway |
| States of Matter | - solid - liquid - gas |
| Solid has | - definite volume; definite shape - particles lie close together - particles arranged in a regular 3-dimensional array |
| Liquid has | - definite volume; on definite shape - particles are close together, but move randomly around, sliding past one another |
| Gas has | - no definite volume or shape - particles move randomly & are separated by a distance much larger than their size |
| Properties of Matter | - Physical - Chemical |
| Physical Properties | - color, size, shape, melting point - observed w/o changing its composition |
| Chemical Properties | - flammability, reactivity - observed & changed substance - substance can be converted to another substance |
| Changes of Matter | - physical -chemical |
| physical changes to matter.... | - melting, tearing - change in state - alters a substance w/o changing its composition |
| chemical changes to matter..... | - chemical reaction - converts one material to another - burning paper; rusting |
| disadvantage of the English System.... | units are not systematically related to each other & require memorization |
| SI units | - based on the metric system, - Systeme International - International system of Units was formally adopted as the uniform system of units for science, 1960 |
| Mass | - a measure of the amount of matter in an object - stays the same |
| Weight | - the force that matter feels due to gravity - changes due to location |
| 2 units for volume | - cubic cm (object) - mL (liquid) |
| 1ml = 1 cubic cm = 1 cc | |
| Conversion Factor | term that converts a quantity in one unit to a quantity in another unit |
| goal of a conversion factor.... | setting up the problem to make sure all unwanted units cancel |
| in conversion factor, always arrange the factors so... | that the denominator in one term cancels the numerator in the preceding term |
| Temperature | is a measure of how hot or cold an object is |
| 3 scales used in temperature | - Fahrenheit - Celsius - Kelvin |
| Fahrenheit to Celsius equation | F = (1.8 x C) + 32 |
| Celsius to Fahrenheit equation | C = (F - 32) / 1.8 |
| Celsius to Kelvin | C = K - 273 |
| Kelvin to Celsius | K = C + 273 |
| Density | a physical property that relates the mass of a substance to its volume g/mL |
| density equation | D = M / V |
| density of a substance depends on | temperature |
| solid stat is __________ than the liquid state | more dense |
| as the temperature __________, the density__________ | increases; decreases |
| The ___________ of a substance determines whether it floats or sinks in a liquid. | density |
| A ________ dense substance floats on a ______ dense liquid. | less; more |
| equation for Specific Gravity | specfiic gravity = density of a substance (g/mL)/ density of H20 (g/mL) |
| Units for Specific Gravity | has no units |
| why does specific gravity have no units | all of the units get cancelled out while solving equation |
| what is the density of water at 4 degrees Celsius | 1.00 g/ml |
| the specific gravity of a substances equals___________ | its density, but with no units |
Created by:
eaholmes
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