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ANATOMY & PHYSIOLOGY Chapter 2: Introductory Chemistry Concepts of Matter matter - anything that occupies space and has mass - may be changed both physically and chemically physical change - does not alter nature of substance i.e.) change in state - ice to water chemical change - does change composition of substance i.e.) fermentation of grapes Concepts of Matter states of matter a. Gas no definite shape; no definite volume. i.e.) air b. Liquid definite volume; conforms to shape of container i.e.) blood; interstitial fluid c. Solid – definite shape and volume i.e.) bones d. Plasma Chemical Reactions energy 1. mass-less; does not take up space 2. measured by its effect on matter 3. ability to do work or to put matter into motion Chemical Reactions Energy All forms of energy (4) exhibit both: a. kinetic energy • when energy is moving objects; actually doing work - causing an effect b. potential energy • inactive or stored energy Concepts of Energy 4 forms of energy chemical energy • energy stored in the bonds of chemical substances and released when bonds are broken electrical energy • energy resulting from movement of charged particles Concepts of Energy 4 forms of energy radiant energy • energy that travels in waves; energy of the electromagnetic spectrum mechanical energy • directly involved in putting matter into motion Concepts of Energy energy form conversion 1. energy is easily converted from one form to another 2. energy conversions are inefficient; some of the initial energy supply is lost (unusable) to the environment as heat ?Question? The statement has been made that “some energy is lost in every energy transformation.” Explain the meaning of this statement. Is it really lost? If not, where is it? Intro to Chemistry Chemical Elements and atoms elements unique substance that cannot be decomposed or broken down into simpler substances by ordinary chemical methods 118 (120) discovered elements; 92 occur naturally; 26 (28) produced artificially 4 different elements make up most of the body Chemical Elements and atoms • four most abundant (making up 96 % of body’s mass) these elements are O,C,H & N • elements that make up approx. 3.8 % include Ca, P, K, S, Na, Cl, Mg, Fe • trace elements - additional 14 elements present in tiny amounts make up the balance of approx. 0.2% -include: Al, B, Cr, Co, Cu, F, I, Mn, Mo, Se, Si, Sn, V, Zn Chemical Elements and atoms Atoms a. building block of an element b. smallest particle that still retains its specific properties c. two basic parts: nucleus and one or more electrons Chemical Elements and atoms Atoms d. an atom is a cluster of smaller (subatomic) particles and can be split into these e. an atom loses the unique properties of its elements when it is split in its subparticles Atomic Structure subatomic particles • three basic particles differing in their: a. mass, b. electrical charge, and c. location within the atom • the electrical charge of a particle is a measure of its ability to attract or repel other charged particles subatomic particles 1. proton – positive charge 2. neutron– neutral charge 3. electron – negative charge subatomic particles all atoms are electrically neutral; the number of protons must be balanced by the number of its electrons protons and neutrons are clustered at the nucleus subatomic particles electrons orbit around the nucleus, forming a negatively charged electron cloud most of the volume of an atom is empty space, and nearly all of the mass is concentrated in the nucleus Differentiating elements/atoms to identify a particular element: a. atomic number • equal to the number of protons its atom contains b. mass number • the sum of the protons and neutrons in its nucleus Differentiating elements/atoms atoms of different elements are composed of different numbers of subatomic particles again, number of protons and electrons are equal; number of neutrons vary light atoms tend to have equal number of protons, electrons, and neutrons larger atoms have more neutrons than protons and electrons Differentiating elements/atoms isotopes • atoms of almost all elements exhibit two or more structural variations called isotopes 1. isotopes have the same number of protons and electrons, but vary in the number of neutrons they contain - thus, 2. has the same atomic number (same chemical properties) of the element, but has a different atomic mass 3. an element’s lightest isotope is more abundant than its heavier forms Differentiating elements/atoms radioisotopes • heavier isotopes of certain elements are unstable and decompose to become more stable 1. radioactivity – spontaneous atomic decay that involves: a. ejection of particles i. alpha (least penetrating) ii. beta b. electromagnetic energy i. gamma rays (most penetrating)