Chemistry

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Chemistry

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The study of the composition, structure, and properties of matter, the processes that matter undergoes, and the energy changes that accompany these processes.

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Instruments are used to...

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Extend our ability to observe and make measurements.

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X-ray diffraction patterns

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Patterns that appear that can be analyzed to reveal the arrangement of atoms, molecules, or other patterns that make up the material.

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Organic chemistry

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The study of most carbon-containing compounds.

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Inorganic chemistry

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The study of non-organic substances, many of which have organic fragments bonded to metals (organometallics).

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Physical chemistry

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The study of the properties and changes of matter and their relation to energy.

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Analyitical chemistry

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The identification of the components and composition of materials.

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Biochemistry

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The study of substances and processes occurring in living things.

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Theoretical chemistry

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The use of mathematics and computers to understand the principles behind observed chemical behavior and to design and predict the properties of new compounds.

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Chemical

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Any substance that has a definite composition.

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Basic research

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Is carried out for the sake of increasing knowledge, such as how and why a specific reaction occurs and what the properties of a substance are.

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Applied research

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Is generally carried out to solve a problem.

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Technological Development

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Typically involves the production and use of products that improve our quality of life.

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Volume

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The amount of three-dimensional space an object occupies.

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Mass

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A measure of the amount of matter. It is the measurement you make using a balance.

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Matter

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Anything that has mass and takes up space.

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Atom

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The smallest unit of an element that maintains the chemical identity of that element.

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Element

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A pure substance that cannot be broken down into simpler, stable substances and is made of one type of atom.

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Compound

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A substance that can be broken down into simpler stable substances. Each compound is made from the atoms of two or more elements that are chemically bonded.

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Molecule

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The smallest unit of an element or compound that retains all of the properties of that element or compound.

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Extensive properties

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Depend on the amount of matter that is present. (such as volume, mass, amount of energy in a substance).

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Intensive properties

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Do not depend on the amount of matter present. (Such as melting point, boiling point, density, ability to conduct electricity and to transfer energy as heat). Intensive properties are the same for a given substance regardless of how much of the substance is present.

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Physical property

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A characteristic that can be observed or measured without changing the identity of the substance. (Describe the substance itself) (e.x. melting and boiling points).

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Physical change

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A change in a substance that does not involve a change in the identity of the substance. (e.x. grinding, cutting, melting, boiling a material)

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Change of state

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A physical change of a substance from one state to another.

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Solid state

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Has definite volume and definite shape.

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Liquid state

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Has a definite volume but an indefinite shape; it assumes the shape of its container.

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Gas state

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Has neither definite volume nor definite shape.

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Plasma

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A high-temperature physical state of matter in which atoms lose most of their electrons, particles that make up atoms. (Found in fluorescent bulbs).

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Chemical property

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Relates to a substance's ability to undergo changes that transform it into different substances.

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Chemical change or chemical reaction

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A change in which one or more substances are converted into different substances.

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Reactants

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The substances that react in a chemical change.

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Products

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The substances that are formed by the chemical change.

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Combustion

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Burning

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Law of conservation of energy

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Although energy can be absorbed or released in a change, it is not destroyed or created. It simply assumes a different form.

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Mixture

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A blend of two or more kinds of matter, each of which retains its own identity and properties. (Components can be separated)

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Homogeneous

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Mixtures that are uniform in composition. They have the same proportion of components throughout. Are also called solutions.

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Heterogeneous

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Mixtures that are not uniform throughout.

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Pure Substance

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(Is homogeneous) Has a fixed composition and differs from a mixture in the following ways:

1. Every sample of a given pure substance has exactly the same characteristic properties.

2. Every sample of a given pure substance has exactly the same composition.

(They are either compounds or elements).

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Scientific method

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A logical approach to solving problems by observing and collecting data, formulating hypotheses, and formulating theories that are supported by data.

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Observing

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The use of senses to obtain information.

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Quantative Data

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Numerical information.

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Qualitative Data

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Non-numerical information.

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System

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A specific portion of matter in a given region of space that has been selected for study during an experiment or observation.

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Hypothesis

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A testable statement. It serves as a basis for making predictions and for carrying out further experiments.

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Controls

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The experimental conditions that remain constant.

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Variable

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Any experimental condition that changes.

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Model

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More than a physical object; it is often n explanation of how phenomena occur and how data or events are related.

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Theory

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A broad generalization that explains a body of facts or phenomena.

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Quantity

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Something that has magnitude, size, or amount.

(not same as measurement)

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Weight

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A measure of the gravitational pull on matter.

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Density

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The ratio of mass to volume, or mass divided by volume.

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Conversion factor

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A ratio derived from the equality between two different units that can be used to convert from one unit to the other.

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Dimensional Analysis

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A mathematical technique that allows you to use units to solve problems involving measurements.

Quantity sought= quantity given x conversion factor

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Accuracy

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Refers to the closeness of measurements to the correct or accepted value of the quantity measured.

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Precision

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Refers to the closeness of a set of measurements of the same quantity made in the same way.

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Percentage error

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(compares value of experiment with the correct or accepted value) Calculated by:

Experimental value - Accepted value divided by accepted value x 100

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Significant figures

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In a measurement consist of all the digits known with certainty plus one final digit, which is somewhat uncertain or is estimated.

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Scientific Notation

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Numbers are written in the form M x 10^n. where the factor M is a number greater than or equal to 1 but less than 10 and n is a whole number.

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Directly proportional

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If dividing one quantity by the other gives a constant value.

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Inversely proportional

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If the product of two quantities is constant.

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Pressure

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The force per unit area on a surface.

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Barometer

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A device used to measure atmospheric pressure.

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Partial pressure

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The pressure of each gas in a mixture.

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Dalton's law of partial pressures

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States that the total pressure of a gas mixture is the sum of the partial pressures of the component gases.