Term
| the study of matter and chages in matter best describes the science of |
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Definition
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| chemistry may be least useful in studying |
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Definition
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Definition
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Term
| chemistry is defines as the study of the compostion and structure of materials and |
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Definition
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Term
| study of all composition and structure of materials and the changes that materials undergo best describes the science of |
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Definition
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Term
| study of the composition and structure of materials and the changes that materials undergo best describes the science of |
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Definition
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Term
| chemistry may be most useful in studying |
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Definition
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| the branch of chemistry that includes the study of materials and processes that occurring in living things is |
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Definition
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Term
| the branch of chemistry that is concerned with the identification and composition of materials is |
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Definition
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Term
| the study of substances containing carbon is |
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Definition
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Term
| organic chemistry, inorganic chemistry, and physical chemistry are not |
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Definition
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Term
| the branch of chemistry concerned with the properties, changes, and relationships between energy and matter is |
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Definition
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Definition
| application of scientific knowledge to solve problems |
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Term
| an example of technology is |
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Definition
| the use of a new antibiotic to fight an infection |
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Definition
| carried out for the sake of increasing knowledge |
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Definition
| carried out to solve a problem |
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Term
| a physical property may be investigated by |
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Definition
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Term
| chemical properties include |
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Definition
| changes that alter the identity of a substance |
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Term
| two features that distinguish matter are |
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Definition
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Term
| one chemical property of matter is |
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Definition
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Term
| an example of an extensive physical property is |
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Definition
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Term
| which of the following is an intensive physical property: volume, length, color, or mass |
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Definition
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Term
| a chemical change occurs when |
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Definition
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Term
| the melting of candle wax is classified as a physical change because it |
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Definition
| produces no new substance |
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Term
| an example of a chemical change is |
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Definition
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Term
| a physical change occurs when a |
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Definition
| glue gun melts a glue stick |
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Term
| the particles in a solid are |
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Definition
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Term
| the state of matter in which a material is most likely to resist compression is the |
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Definition
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Term
| the state of matter in which a material has definite shape and definite volume is the |
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Definition
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Term
| the state of matter in which particles are rigidly held in fixed positions is the |
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Definition
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Term
| a substance classified as a fluid contains particles that |
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Definition
| may slide past each other |
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Term
| the state of matter in which a material has a definite volume but no definite shape is the |
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Definition
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Term
| under ordinary conditions of temperature and pressure, the particles in a gas are |
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Definition
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Term
| a list of pure substances could include |
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Definition
| vitamin C (absorbic acid) |
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Term
| the substances that are chemically bound together are |
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Definition
| the elements that compose water |
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Term
| physical means can be used to separate |
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Definition
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Term
| the most useful source of chemical information about the elements is a |
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Definition
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Term
| a horizontal row of blocks in the periodic table is called a(n) |
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Definition
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Term
| elements in a group in the periodic table can be expected to have similar |
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Definition
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Term
| a vertical column of blocks in the periodic table is called a(n) |
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Definition
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Term
| the elements that border the zigzag line in the periodic table are |
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Definition
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Term
| the reason for organizing, analyzing, and classifying data is |
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Definition
| to find relationships among the data |
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Term
| which of the following observations is quantitative: liquid turns blue litmus paper red; liquid boils at 100C; liquid tastes bitter; liquid is cloudy |
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Definition
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Term
| quantitative observations are recorded using |
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Definition
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Term
| qualitative observations are recorded using |
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Definition
| non-numerical information |
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Term
| a testable statement used for making predictions and carrying out further experiments is a |
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Definition
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Term
| a plausible explanation of a body of observed natural phenomena is a scientific |
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Definition
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Term
| the validity of scientific concepts is evaluated by |
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Definition
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Term
| a theory is an accepted explanation of an observed phenomenon until |
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Definition
| repeated data and observation conflict with the theory |
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Term
| standards are chosen because they |
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Definition
| are reproducible in another laboratory |
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Term
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Definition
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Term
| all of the following describe measurement standards except: avoid ambiguity; must be unchanging; need not agree with a previously defined size; confusion eliminated when correct measurement applied |
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Definition
| standard need not agree with a previously defined size |
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Term
| all of the following describe a unit except: unite compares what is being measured with a previously defined size; usually preceded by a number; usually is not important in finding a solution to a problem; or choice of unit depends on quantify being measured |
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Definition
| a unit is usually not important in finding a solution to a problem |
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Term
| all of the following are examples of unites except: weight; kilometer; gram; teaspoon |
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Definition
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Term
| all but one of these units are SI base units: kilogram; second;liter; Kelvin |
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Definition
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Term
| the SI standard units for length and mass are |
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Definition
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Term
| the metric unit for length that is closest to the thickness of a dime is the |
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Definition
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Term
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Definition
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Term
| the symbols for units of length is order from smallest to largest are |
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Definition
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Term
| the symbol for the metric unit used to measure mass is |
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Definition
|
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Term
| the quantity of matter per unit volume is |
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Definition
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Term
| a quantity that describes the concentration of matter is |
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Definition
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Term
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Definition
|
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Term
|
Definition
|
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Term
| the standard unit for mass is the |
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Definition
|
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Term
| a volume of 1 cubic centimeter is equivalent to |
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Definition
|
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Term
| the symbol that represents the measured unit for volume is |
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Definition
|
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Term
| the SI base unit for time is the |
|
Definition
|
|
Term
| the unite abbreviation for time is |
|
Definition
|
|
Term
| the most appropriate SI unit for measuring the length of an automobile is the |
|
Definition
|
|
Term
| the SI base unit for length is the |
|
Definition
|
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Term
| all of the following are SI units for density except: kb/m3; g/mL; g/cm3; g/m2 |
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Definition
|
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Term
| a change in the force of Earth's gravity on an object will affect its |
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Definition
|
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Term
| a measure of Earth's gravitational pull on matter is |
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Definition
|
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Term
| a true statement about mass is that |
|
Definition
| mass is determined by comparing the mass of an object with a set of standard masses that are part of a balance |
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Term
| to determine density the quantities that must be measured are |
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Definition
|
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Term
| the relationship between the mass m of a material, its volume V, and its density D is |
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Definition
|
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Term
| to calculate the density of an object, |
|
Definition
| divide its mass by its volume |
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Term
| when density is measured, |
|
Definition
| the temperature should be specified |
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Term
| which statement about density is true? |
|
Definition
| density is a physical property |
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Term
| the density of aluminum is 2.70 g/cm3. The volume of a solid piece of aluminum is 1.50 cm3. Find its mass. |
|
Definition
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Term
| the mass of a 5.00cm3 sample of gold is 96.5 g. The density of gold is |
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Definition
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Term
| what is the density of 37.72 g of matter whose volume is 6.80 cm3? |
|
Definition
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Term
| the density of sugar is 1.59 g/cm3. The mass of a sample is 4.0g. Find the volume of the sample. |
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Definition
|
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Term
| the mass of a 5.00 cm3 sample of clay is 11g. what is the density of the clay? |
|
Definition
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Term
| the mass of a 6.0 mL sample of kerosene is 4.92 g. The density of kerosene is |
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Definition
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Term
| 100 milliliters is equivalent to |
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Definition
|
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Term
| 10 -2 meter is the same as |
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Definition
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Term
|
Definition
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Term
|
Definition
|
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Term
| 1.06 L of water is equivalent to |
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Definition
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Term
| the number of grams equal to 0.5 kg is |
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Definition
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Term
|
Definition
|
|
Term
| convert -25 degrees C to the kelvin scale |
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Definition
|
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Term
| how many minutes are in 1 week? |
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Definition
|
|
Term
| if 1 inch equals 2.54 cm, how many centimeters equal 1 yard? |
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Definition
|
|
Term
| a measurement that closely agrees with accepted alues is said to be |
|
Definition
|
|
Term
| a measurement is said to have good precision if it |
|
Definition
| agrees closely with other measurements of the same quantity |
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Term
| if some measurements agree closely but differ widely from the actual value, these measurements are |
|
Definition
| precise, but not accurate |
|
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Term
| poor precision in scientific measurement may arise from |
|
Definition
| both human error and the limitations of the measuring instrument |
|
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Term
| precision pertains to all of the following except: reproducibility of measurements; agreement among numerical values; sameness of measurements; closeness of a measurement to an accepted value |
|
Definition
| closeness of a measurement to an accepted value |
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Term
| these values were obtained as the mass of products from the same reaction: 8.83 g; 8.84 g; 8.82 g. The known mass of products from that reaction is 8.60 g. The values are |
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Definition
|
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Term
| five darts strike near the center of the target. Whoever threw the darts is |
|
Definition
| both accurate and precise |
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Term
| a chemist who frequently carries out a complex experiment is likely to have high |
|
Definition
|
|
Term
| when applied to scientific measurements, the words "accuracy" and "precision" |
|
Definition
| have distinctly different meanings |
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Term
| using the same balance, a chemist obtained the values 5.224 g, 5.235 g, and 5.25 g for the mass of a sample. These measurements have |
|
Definition
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|
Term
| when determining the number of significant digits in a measurement, |
|
Definition
| all nonzero digits are significant |
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|
Term
| for numbers less than 0.1, such as 0.06, the zeros to the right of the decimal point but before the first nonzero digit |
|
Definition
| show the decimal place of the first digit |
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|
Term
| to two significant figures, the measurement 0.0255 g should be reported as |
|
Definition
|
|
Term
| in division and multiplication, the answer must not have more significant figures than the |
|
Definition
| number in the calculation with fewest significant figures |
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|
Term
| a sum or difference of whole numbers should be rounded so that the final digit is in the same place as the |
|
Definition
|
|
Term
| the number of significant figures in the measurement 0.000 305 kg is |
|
Definition
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|
Term
| the number of significant figures in the measured value 0.003 20 g is |
|
Definition
|
|
Term
| the measurement that has been expressed to three significant figures is |
|
Definition
|
|
Term
| the number of significant figures in the measurement 170.040 km is |
|
Definition
|
|
Term
| the measurement that has been expressed to four significant figures is |
|
Definition
|
|
Term
| the number of significant figures in the measurement 210 cm is |
|
Definition
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|
Term
| the measurement that has only nonsignificant zeros of the following: 0.0037 mL; 60.0 mL; 400. mL; or 506 mL |
|
Definition
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|
Term
| the number of these that has five significant figures: 23 410; 0.006 52; 0.017 83; 10.292 |
|
Definition
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|
Term
| using a metric ruler with 1 mm divisions, you find the sides of a rectangular piece of plywood are 3.54 cm and 4.85 cm. You calculate that the area is 17.1690 cm2. To the correct number of significant figures, the result should be expressed as |
|
Definition
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|
Term
| when 64.4 is divided by 2.00, the correct number of significant figures in the result is |
|
Definition
|
|
Term
| the dimensions of a rectangular solid are measured to be 1.27 cm, 1.3 cm, and 2.5 cm. The volume should be recorded as |
|
Definition
|
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Term
| three samples of 0.12g, 1.8 g, and 0.562 g are mixed together. The combined mass of all three samples, expressed to the correct number of significant figures, should be recorded as |
|
Definition
|
|
Term
| divide 5.7 m by 2 m. The quotient is correctly reported as |
|
Definition
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|
Term
| the sum of 314. km and 32 km is correctly expressed as |
|
Definition
|
|
Term
| the product of 13 cm and 5.7 cm is correctly reported as |
|
Definition
|
|
Term
| round 1.245 633 501 x 10-8 to four significant figures |
|
Definition
| 1.246 x 10-8 (to 8th power) |
|
|
Term
| the correct number of significant figures that should appear in the answer to the calculation 3.475 x 1.97 + 2.4712 is |
|
Definition
|
|
Term
| how may significant digits should be shown in the product of 1.6 cm and 2.4 cm? |
|
Definition
|
|
Term
| written in scientific notation, the measurement of 9.000 065 cm is |
|
Definition
|
|
Term
| the measurement of 0.020 L is the same as |
|
Definition
|
|
Term
| expressed in scientific notation, 0.0930 m is |
|
Definition
|
|
Term
| the speed of light is 300 000 km/s. In scientific notation, this speed is |
|
Definition
|
|
Term
| the average distance between the Earth and the moon is 386 000 km. Expressed in scientific notation, this distance is |
|
Definition
|
|
Term
| an analytical balance can measure mass to the nearest 1/10 000 of a gram, 0.0001 g. In scientific notation, the accuracy of the balance would be expressed as |
|
Definition
|
|
Term
| when 1.92 x 10 -6 kg is divided by 6.8 x 10 2 mL, the quotient in kg/mL equals |
|
Definition
|
|
Term
| when 6.02 x 10 23 is multiplied by 9.1 x 10 -31, the product is |
|
Definition
|
|
Term
| the capacity of a Florence flask is 250 mL. Its capacity in liters expressed in scientific notation is |
|
Definition
|
|
Term
| if values for x and y vary as ian inverse proportion |
|
Definition
| their product is a constant |
|
|
Term
| two variables are directly proportional if their ? has a constant value |
|
Definition
|
|
Term
| the graph of a direct proportion is a(n) |
|
Definition
|
|
Term
| two variables are inversely proportional if the ? has a constant value |
|
Definition
|
|
Term
| the graph of an inverse proportion is a)n_ |
|
Definition
|
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Term
| which of the following is not true: y is directly proportional to x; x is a variable; the product of y and x is a constant; or the graph of y versus x should be a straight line |
|
Definition
| the product of y and x is a constant |
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|
Term
| in the expression m = DV, where m is mass, D is density, and V is volume, density is the |
|
Definition
|
|
Term
| which of the following does not describe an inverse proportion between x and y: xy = k; x = k/y; y = k/x; k = ky |
|
Definition
|
|
Term
| which of the following does not describe a direct proportion between x and y: xy = k; x/y = k; y/x = k; x = ky |
|
Definition
|
|
Term
| in the equation density = mass/volume, mass divided by volume as a constant ratio. This means that the |
|
Definition
| equation graphs as a straight line |
|
|
Term
| law of conservation of mass |
|
Definition
| states that mass is neither destroyed nor created during ordinary chemical reactions or physical changes |
|
|
Term
| law of multiple proportions |
|
Definition
| states that 2 or more different compounds are composed of the same 2 elements, then the ratio of the masses of the 2nd element combined with a certain mass of the 1st element is always a ratio of small whole numbers |
|
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Term
|
Definition
| smallest particle of an element that retains the chemical properties of that element |
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|
Term
lse og frginiyr ptopotyiond
:) law of definite proportions |
|
Definition
| fact that a chemical compound contains the same elements in exactly the same proportions by mass regardless of the size of the sample or source of the compound |
|
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Term
|
Definition
| short-range proton-neutron, proton-proton, and neutron-neutron forces hold the nuclear particles together |
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Term
|
Definition
| exactly 1/12 the mass of a carbon-12 atom |
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Term
|
Definition
| the number of protons in the nucleus of each atom of that element |
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Term
|
Definition
| atoms of the same element that have different masses |
|
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Term
|
Definition
| the total number of protons and neutrons in the nucleus of an isotope |
|
|
Term
|
Definition
| general term for any isotope of any element |
|
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Term
|
Definition
| weighted average of the atomic masses of the naturally occurring isotopes of an element |
|
|
Term
|
Definition
| 6.022 x 10 23 is the number of particles in exactly 1 mole of a pure substance |
|
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Term
|
Definition
| mass of 1 mole of a pure substance |
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Term
|
Definition
| amount of a substance that contains as many particles as there are atoms in exactly 12 g of carbon-12 |
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Term
|
Definition
| the emission of a contiguous range of frequencies of electromagnetic radiation |
|
|
Term
| electromagnetic radiation |
|
Definition
| form of energy that exhibits wavelike behavior as it travels through space |
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Term
|
Definition
| all forms of electromagnetic radiation |
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Term
|
Definition
| state where an atom has a higher potential energy then it has at ground state |
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Term
|
Definition
| the number of waves that pass a given point in a specific time |
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Term
|
Definition
| lowest energy state of an atom |
|
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Term
|
Definition
| when a narrow beam of emitted light was shined through a prism, it was separated into a series of specific frequencies of visible light |
|
|
Term
|
Definition
| the emission of electrons from a metal when light shines on a metal |
|
|
Term
|
Definition
| a particle of electromagnetic radiation having zero mass and carrying a quantum of energy |
|
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Term
|
Definition
| the minimum quantity of energy that can be lost or gained by an atom |
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Term
|
Definition
| the distance between corresponding points on adjacent waves |
|
|
Term
| angular momentum quantum number |
|
Definition
| indicates the shape of the orbital "L" |
|
|
Term
| Heisenberg uncertainty principle |
|
Definition
| states that it is impossible to determine simultaneously both the position and velocity of an electron or any other particle |
|
|
Term
|
Definition
| symbolized by m, indicates the orientation of an orbital around nucleus |
|
|
Term
|
Definition
| a 3-dimensional region around the nucleus that indicates the probable location of an electron |
|
|
Term
|
Definition
| symbolized by n. indicates the main energy level occupied by the electron |
|
|
Term
|
Definition
| specify the properties of atomic orbitals and the properties of electrons in orbitals |
|
|
Term
|
Definition
| describes mathematically the wave properties of electrons and other very small particles |
|
|
Term
|
Definition
| has only 2 possible values that indicate the 2 fundamental spin states of an electron in an orbital |
|
|
Term
|
Definition
| an electron occupies the lowest-energy orbital that can receive it |
|
|
Term
|
Definition
| arrangement of electrons in an atom |
|
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Term
|
Definition
| the electron-containing main energy level with the highest principal quantum number |
|
|
Term
|
Definition
| orbitals of equal energy are each occupied by 1 electron before any orbital is occupied by a second electron and all electrons in singly occupied orbitals must have the same spin |
|
|
Term
|
Definition
| electrons that are not in the highest occupied energy level |
|
|
Term
|
Definition
|
|
Term
|
Definition
| an outer main energy level fully occupied by usually 8 electrons |
|
|
Term
| Pauli exclusion principle |
|
Definition
| no 2 electrons in the same atom can have the same set of 4 quantum numbers |
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|
