Chemistry: The Central Science 13th Edition Chapter 1 – Flashcards
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Molecules
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two or more atoms are joined in specific in specific shapes.
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States of Matter
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gas, a liquid, or a solid.
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Gas
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has to fixed volume or shape; rather, it uniformly fills its container.
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Liquid
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has a distinct volume independent of its container and assumes the shape of the portion of the container it occupies.
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Solid
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has both a definite shape and a definite volume.
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Pure Substance
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is matter that has distinct properties and a composition that does not vary from sample to sample.
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Elements
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are substances that cannot be decomposed into simpler substances. On a molecular level, they are made up of one kind of atom. They make up matter.
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Compounds
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Substances composed of two or more elements; they contain two or more atoms.
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Mixtures
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are combinations of two or more substances in which each substance retains its chemical identity.
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Law of constant composition (or Law of definite proportions)
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the observation that the elemental composition of a compound is always the same
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Physical Properties
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can be observed without changing the identity and composition of the substance. Ex- color, odor, density, melting point, boiling point, hardness, etc.
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Chemical Properties
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describe the way a substance may change, or react, to form other substances. Ex- flammability
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Intensive properties
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do not depend on the amount of sample being examined and are particularly useful in chemistry because many of these properties can be used to identify substances.
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Extensive properties
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depends on the amount of sample, with two examples being mass and volume.
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Physical Change
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a substance changes its appearance but not its composition. It is the same substance before and after the change.
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Chemical Change (or Chemical Reaction)
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a substance is transformed into a totally different substance. It is not the same substance before and after the change.
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Distillation
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separating the components of a homogeneous mixture. This process depends on the different abilities of substances to form gases.
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Metric system
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units used for scientific measurements.
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Mass
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is a measurement of the amount of material in an object.
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Temperature
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a measure of hotness or coldness of an object, is a physical property that determines the direction of heat flow.
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Celsius scale
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based on the assignment of 0 degrees being the freezing point of water and 100 degrees being the boiling point of water.
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Kelvin scale
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the SI unit temperature scale.
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Absolute zero
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it is the lowest attainable temperature on the Kelvin scale.
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Derived unit
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is obtained by multiplication or division of one or more based units.
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Precision
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a measure of how closely individual measurements agree with one another.
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accuracy
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refers to how closely individual measurements agree with the correct, or "true," value.
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Significant figures
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in a measured quantity include one estimated digit, the last digit of measurement. It indicates the extent of the uncertainty of the measurement.
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Dimensional analysis
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helps ensure that solutions to problems yield the proper units.
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Conversion factor
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a fraction whose numerator and denomination are the same quantity expressed in different units.
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