Classification of Matter and the Math of Chemistry
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69 Terms
The study of matter; its composition, properties, and the changes/transformations it can undergo
Anything that has mass and occupies space/has volume
The amount of material/matter in an object
The amount of space an object occupies
A state of matter with fixed shape and fixed volume; particles are in a fixed arrangement and solids are not easily compressed
A state of matter with fixed volume but no fixed shape; it takes the shape of its container and is not very compressible
A state of matter with no fixed shape or volume; it fills its container, has very low density, and is highly compressible
A property that can be observed or measured without changing the substance’s composition (ex: melting point, density, color, magnetism)
A property that describes how a substance can be converted into another substance (ex: ability to rust, burn, or tarnish
A property described in terms of appearance, not numbers or units (ex: color, odor, taste)
A property described with a number and unit (ex: 25.0 mL, 2.5 g, 37 °C)
A property that does NOT depend on the amount of substance present (ex: density, temperature, boiling point, color)
A property that DOES depend on the amount of substance present (ex: mass, volume)
A change that alters the form, state, or appearance of a substance without changing its composition (ex: changes of state, cutting, grinding)
A change in which one or more substances are converted into new substances with new properties (a chemical reaction)
Changes of state (melting, boiling, freezing, sublimation), dissolving, cutting, grinding, crushing
Burning, rusting, toasting, tarnishing, gas burning in air, reacting with acid
Change in color or odor, formation of a gas (bubbles), formation of a precipitate (solid), change in light or heat
Matter composed of only a single component (atom or molecule) with constant composition; cannot be separated into other pure substances by physical changes
A pure substance made of only one type of atom; cannot be broken down into simpler substances by chemical changes
A pure substance composed of two or more elements chemically combined in a definite ratio; can be broken down into simpler substances by chemical changes
Elements contain only one type of atom and cannot be broken down by chemical changes; compounds contain two or more elements chemically combined and can be broken down into simpler substances with different properties
A chemical change is required to change elements into compounds and to break compounds back into elements
Matter that consists of two or more substances physically mixed, not chemically combined; components can be separated by physical means
A mixture with uniform composition throughout; different parts are not visible (ex: air, salt water, rubbing alcohol)
A mixture with non-uniform composition; different parts are visible and may have different compositions (ex: muddy water, pasta and sauce, paint)
A method that separates a dissolved solid from a liquid by allowing the liquid to vaporize, leaving the solid behind
A separation technique that uses a porous barrier (like filter paper) to separate a solid from a liquid in a heterogeneous mixture
A separation technique that separates liquids based on differences in their boiling points; the more volatile component boils first, is condensed, and collected
A separation technique that separates components of a mixture based on how they move along a stationary phase; different components travel at different speeds
Every measurement has two components: a number and a unit
A description without numbers or units (ex: “blue,” “cloudy,” “has a pungent odor”)
A measurement that includes a number and a unit (ex: 25.0 mL, 2.5 g, 37 °C)
How close a measurement is to the true or accepted value
How close repeated measurements are to each other (the reproducibility of a measurement)
An error inherent in the measurement or instrument that makes results consistently too high or too low; minimized by calibrating instruments and correcting the procedure
Error related to the estimation of the last digit in a measurement; causes measurements to vary in both directions around the true value; minimized by repeated measurements and averaging
All the certain digits in a measured number plus one estimated digit; they show the precision of the measurement and measuring device
To reflect the uncertainty of measurements and avoid implying more certainty than the data support in calculated answers
All nonzero digits (1–9) are always significant
Leading zeros (before the first nonzero digit) are never significant
Embedded zeros (between nonzero digits) are always significant
With a decimal point, trailing zeros are significant (27.00 has 4 sig figs); without a decimal, trailing zeros are not significant (30,000 has 1 sig fig)
The result must have the same number of decimal places as the quantity with the fewest decimal places
The result must have the same number of significant figures as the quantity with the fewest significant figures in the calculation
Writing a number in the form M × 10ⁿ, where 1 ≤ M < 10 and n is an integer (positive or negative)
Move the decimal point left until one nonzero digit remains to its left; the number of places moved is a positive exponent
Move the decimal point right until one nonzero digit remains to its left; the number of places moved is a negative exponent
pico (p, 10⁻¹²), nano (n, 10⁻⁹), micro (µ, 10⁻⁶), milli (m, 10⁻³), centi (c, 10⁻²), kilo (k, 10³), mega (M, 10⁶)
The base SI units are: kilogram (kg) for mass, meter (m) for length, and second (s) for time
Liter (L) and milliliter (mL), and cubic centimeter (cm³); 1 cm³ = 1 mL
Solids in g/cm³, liquids in g/mL, gases in g/L
A method of problem solving using conversion factors to change units while keeping track of units
(1) Find where you start and where you want to go. (2) Write any needed equalities. (3) Make conversion factors from the equalities. (4) Set up conversions so units cancel step by step. (5) Multiply numbers on top and divide by numbers on bottom once only desired units remain
A statement that shows the same measurement in two different units (for example, 1 in = 2.54 cm, 1 kg = 1000 g)
A ratio made from an equality and equal to 1 (for example, 2.54 cm/1 in or 1 in/2.54 cm) used to convert from one unit to another
A measure of how hot or cold an object is compared to another; it indicates the direction of heat flow (from higher temperature to lower temperature)
The temperature 0 K, at which all molecular motion stops
Temperature conversion: Celsius to Kelvin
K = °C + 273
°F = 1.8(°C) + 32
°C = (°F − 32) ÷ 1.8
A physical property that relates mass to volume; d = m ÷ V
The relationship d = m/V, where d is density, m is mass, and V is volume
Solids: g/cm³; liquids: g/mL; gases: g/L
Rearrange d = m/V to m = d × V and multiply density by volume to find mass
Rearrange d = m/V to V = m ÷ d and divide mass by density to find volume
A method for finding the volume of an irregular solid by measuring how much the water level in a graduated cylinder rises when the object is submerged; volume of the object equals (final volume − initial volume)
Use displacement to find the object’s volume, measure its mass, then calculate density with d = m ÷ V
Use density as an equality (for example, 3.8 g = 1 mL) to write conversion factors (3.8 g/1 mL or 1 mL/3.8 g) and convert between mass and volume in dimensional analysis problems