Chem.

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matter

Back 1

anything that has mass and occupies space

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chemistry

Back 2

the study of the composition of matter and the changes that matter undergoes

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organic chemistry

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the study of all chemicals containing carbon

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inorganic chemistry

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the study of all chemicals that do not contain carbon

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biochemistry

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the study of the processes that take place in organisms

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analytical chemistry

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the area of study that focuses on the comosition of matter

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physical chemistry

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the area that deals with the mechanism, the rate, and the energy transfer that occurs when matter undergoes change

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pure chemistry

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the pursuit of chemical knowledge for its own sake

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applied chemistry

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reasearch that is directed toward a practical goal or application

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technology

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the means by which a society provides its members with those things needed and desired

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macroscopic

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the world of objects that are large enough to see with the unaided eye

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microscopic

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the world of objects that can be seen only under magnification

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biotechnology

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applies science to the production of biological products or processes. it uses techniques that can alter the DNA in living organisms

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pollutant

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a material found in the air, water, or soil that is harmful to humans or other oganisms

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scientific method

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a logical, systematic approach to the solution of a scientific problem

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observation

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when you use your senses to obtain information

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hypothesis

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a proposed explanination for an observation.

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experiment

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a procedure that is used to test a hypothesis

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manipulated variable

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independent variable, the variable that you change during an experiment

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responding variable

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dependant bariable, the variable that is observed during the experiment

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theory

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a well tested explanation fro a broad sed of observations

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scientific law

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a concise statemnt that summarizes the results of many observations and experiments

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mass

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a measure of the amount of matter the object contains

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volume

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a measure of the space occupied by the object

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extensive property

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a property that depends on the amount of matter in a sample

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intensive property

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a property that depends on the type of matter in a sample, not the amount of matter

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substance

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matter that has a uniform and definite composition

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physical property

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a quality or condition of a substance that can be observed or measured without changing the substance's compostition

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solid

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a form of matter that has a definite shape and volume and is not easily compressed

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liquid

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a form of matter that has an indefinite shape, flows, yet has a fixed folume, and is not easily compressed but tends to expand slightly when heated

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gas

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a form of matter that takes both the shape and volume of its container and is easily compressed

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physical change

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when some properties of a material change but the compositon of the material doesn't change

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vapor

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describes the gaseous state of a substance that is generally a liquid or solid at room temperature, as in water vapor

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mixture

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a physical blend of two or more components

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heterogeneous mixture

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a mixture in which the compositsion isn't uniform throughout

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homogeneous mixture

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a mixture in which the composistion is unifor throught

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solution

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another name for a homogenous mixture. many are liqueds but some are gasses

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phase

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describes any part of a sample with uniform composition and properties. homogeneuous=1phase
heterogeneouse=2+

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filtration

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the process that seperates solid from liquid in a heterogeneuous mixture

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distillation

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when a liquid is bolied to produce a vapor that is then condensed into a liquid

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element

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the simplest form of matter that has a unique set of properties

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compound

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a substance that contains two or more elements chemically combined in a fixed proportion

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chemical symbol

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2 letters, represents an element

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chemical property

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the ability of a substance to undergo a specific chemical change

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chemical reaction

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when one or more substances change into one or more new substances

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reactant

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a substance present at the start fo the reaction

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product

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a subsance produce in the reaction

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precipitate

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a solid that form and settles out of a liquid mixture

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law of conservation of mass

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states that in any physical change or chemical reacton, mass is conserved. Mass is neither created nor destroyed

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measurement

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a quantity tht has both a number and a unit

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scientific notation

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when a given number is writted as the product of 2 numbers: a coefficient and 10 raised to a power

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accuracy

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a measure fo how close a measurment comes to the actual or true value of whatever is measured

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precision

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a measure of how close a series of measuremnts are to one another

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accepted value

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the correct value based on reliabel references

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experimental value

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the value measured in the lab

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error

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the difference between the accepted value and the experimental value

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percent error

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the absolute value of the error divided by the accepted value multiplied by 100%

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significant figures

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a measuremnt that includes all of the digits that are known, plus a last digit that is estimated

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International systor fo Units (SI)

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a revised version of the metric system

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meter

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the SI basic unit of length

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liter

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unit of volume= m^3

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kilogram

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basic SI unit of mass

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gram

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1/1000 of a kilogram

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weight

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a force that measures the pull on a given mass by gravity; a measure of force DIFFERENT THAN MASS

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temperature

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a measure of how hot or cold an object is

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celcius scale

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sets the freezing point of water at 0 and the boiling point at 100

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kelvin scale

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the freezing point fo water is 273.15 K and th the boiling point is 373.15 K. add or subtact 273 to get celcius

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absolute zero

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the zero pint o n the kelvin scale

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energy

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the capacity to do work or to produce heat

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joule

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the SI unit of energy

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calorie

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the quantity of heat that raises the temperature of 1g of pure water by 1 c

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conversion factor

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a ration of equivalent measurements

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dimensional anaylysis

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a way to analyze and solve probles using the units, or dimensions, of the measurements

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density

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the ratio of the mass of an object to its volume

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atom

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the smallest particle of an elemetn that retains its identity in a chemical rection

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Dalton's atomic theory

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1. all elements are composed of atoms
2. atoms of the same element are identical, and different from the atoms of another element
3. atoms of different elements can physically mix together or chemiclaly combine to form substances
4. chemical reactions occur when atoms ar seperated, joined, or rearranged. atoms fo one element are never changed into atoms of another element as a result of a chemical reaciton

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electrons

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negatively charged subatomic particles

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cathode ray

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a glowing beam

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protons

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positively charged subatomic particals. mass is about 1840x electrons

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neutrons

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subatomic particals with no charge. nearly equal mass to protons

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nucleus

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the tiny central core of an atom and is composed of protons and neutrons

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atomic number

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the number of protons in the nucleus of an atom of that element

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mass number

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the total number of protons and neutrons in an atom

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isotopes

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atoms that have the same number of protons but different numbers of neutrons

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atomic mass unit (amu)

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one twelfth of the mass of a standard is carbon -12 atom. way to compare relative masses of atoms using a reference isotope as standard. one twelfth of the mass of a standard is carbon -12 atom.

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atomic mass

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a weighted average mass of the atoms in a naturally occuring sample of the element. reflects both the mass and the relative abundance of th isotopes as they occur in nature

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period

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horizontal row in periodic table

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group

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also called family. vertical column in periodic table. have similar chemical and physical properties

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periodic table

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an arrangement of elements in which the elements are seperated into groups based on a set fo repeating properties