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