Naminat0r A&P Ch. 2 Part 1
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71 terms
Terms | Definitions |
|---|---|
 What is Matter? | • Anything that has mass and occupies space |
| What are the 3 states of matter and their meanings? | 1. Solid—definite shape and volume 2. Liquid—definite volume, changeable shape 3. Gas—changeable shape and volume |
| What is Energy? | • Capacity to do work or put matter into motion |
| What are the 2 types of energy? | • Kinetic—energy in action • Potential—stored (inactive) energy |
| What are the 4 forms of energy? | • Chemical energy • Electrical energy • Mechanical energy • Radiant or electromagnetic energy |
| What is Chemical Energy? | stored in bonds of chemical substances |
| What is Electrical Energy? | results from movement of charged particles |
| What is Mechanical Energy? | directly involved in moving matter |
| What is Radiant or electromagnetic energy? | exhibits wavelike properties (i.e., visible light, ultraviolet light, and X-rays) |
| 1) What can be converted from one form to another? 2) What is inefficient? | 1) Energy 2) • Conversion is inefficient because some energy is "lost" as heat |
| What are elements? | • Cannot be broken down by ordinary chemical means |
| What are Elements unique properties? | • Physical properties Are detectable with our senses, or are measurable • Chemical properties How atoms interact (bond) with one another |
| What are Atoms? | Unique building blocks for each element |
| What are atomic symbols? | one- or two-letter chemical shorthand for each element |
| What are the major elements of the Human Body? | • Oxygen (O) • Carbon (C) • Hydrogen (H) • Nitrogen (N) |
| What lesser elements of the human body takes about _%? | • Calcium (Ca), phosphorus (P), potassium (K), sulfur (S), sodium (Na), chlorine (Cl), magnesium (Mg), iodine (I), and iron (Fe) 3.9% |
| What trace elements take __ of the human body? | • < 0.01% of body mass • Part of enzymes, e.g., chromium (Cr), manganese (Mn), and zinc (Zn) |
| 1) What determines atomic structure? 2) What does the nucleus consist of? | • Determined by numbers of subatomic particles • Nucleus consists of neutrons and protons |
| What are Neutrons? | • No charge • Mass = 1 atomic mass unit (amu) |
| What are Protons? | • Positive charge • Mass = 1 amu |
| What are Electrons? | • Orbit nucleus • Equal in number to protons in atom • Negative charge • 1/2000 the mass of a proton (0 amu) |
| 1) What is the Orbital model? 2) What is it's purpose? | 1) Current model used by chemists 2) • Depicts probable regions of greatest electron density (an electron cloud) • Useful for predicting chemical behavior of atoms |
| 1) What is the Planetary model and what is it's faults? | 1) oversimplified, outdated model 2) Incorrectly depicts fixed circular electron paths |
| How can someone identify elements? | • Atoms of different elements contain different numbers of subatomic particles |
| What is the Atomic Number? | number of protons in nucleus |
| What is Mass Number? | mass of the protons and neutrons • Mass numbers of atoms of an element are not all identical |
| What is an Isotope? | • Isotopes are structural variations of elements that differ in the number of neutrons they contain |
| What is atomic weight? | average of mass numbers of all isotopes |
| What is Radioisotopes and it's characteristics? | • Spontaneous decay (radioactivity) • Similar chemistry to stable isotopes • Can be detected with scanners |
| How is it useful in biological research and medicine? | • Cause damage to living tissue: • Useful against localized cancers • Radon from uranium decay causes lung cancer |
| What do atoms chemically combine to become? | molecules and compounds |
| What is an molecule? | two or more atoms bonded together (e.g., H2 or C6H12O6) |
| What is an compound? | two or more different kinds of atoms bonded together (e.g., C6H12O6) |
| What is a mixture? | • Two or more components physically intermixed • Most matter exists as mixtures |
| What are 3 types of mixtures? | • Solutions • Colloids • Suspensions |
| What is solution? | • Homogeneous mixtures • Usually transparent, e.g., atmospheric air or seawater |
| What are 2 types of solutions? | • Solvent Present in greatest amount, usually a liquid • Solute(s) Present in smaller amounts |
| How are solutions expressed? | • Percent, or parts per 100 parts • Milligrams per deciliter (mg/dl) • Molarity, or moles per liter (M) |
| What is 1 mole? | the atomic weight of an element or molecular weight (sum of atomic weights) of a compound in grams |
| What is Avogadro's number? | 1 mole of any substance contains 6.02 X 10 to the 23 molecules (Avogadro's number) |
| What are Colloids? | • Heterogeneous translucent mixtures, e.g., cytosol • Large solute particles that do not settle out • Undergo sol-gel transformations |
| What is suspensions? | • Heterogeneous mixtures, e.g., blood • Large visible solutes tend to settle out |
| What separates MIXTURE vs. Compounds? | • No chemical bonding between components • Can be separated physically, such as by straining or filtering • Heterogeneous or homogeneous |
| What separates mixture vs. COMPOUNDS? | • Can be separated only by breaking bonds • All are homogeneous |
| How are Chemical Bounds used in Orbital Model? | • Electrons occupy up to seven electron shells (energy levels) around nucleus • Octet rule: Except for the first shell which is full with two electrons, atoms interact in a manner to have eight electrons in their outermost energy level (valence shell) |
| What are Chemically Inert Elements? | • Stable and unreactive • Outermost energy level fully occupied or contains eight electrons |
| What are Chemically Reactive Elements? | • Outermost energy level not fully occupied by electrons • Tend to gain, lose, or share electrons (form bonds) with other atoms to achieve stability |
| What are 3 types of Chemical Bonds? | • Ionic • Covalent • Hydrogen |
| What are Ionic Bonds? | • Ions are formed by transfer of valence shell electrons between atoms |
| What are Anions? | • Anions (- charge) have gained one or more electrons |
| What are Cations? | • Cations (+ charge) have lost one or more electrons |
| What results in an Ionic bond? | • Attraction of opposite charges |
| How does an Ionic Bond form? | • Ionic compounds form crystals instead of individual molecules |
| What is a Covalent Bond? | • Formed by sharing of two or more valence shell electrons • Allows each atom to fill its valence shell at least part of the time |
| How is a Covalent Bond's Sharing? | • Sharing of electrons may be equal or unequal • Equal sharing produces electrically balanced nonpolar molecules |
| What is special about unequal sharing in Covalent Bonds? | • Unequal sharing by atoms with different electron-attracting abilities produces polar molecules |
| What is Electronegative? | • Atoms with six or seven valence shell electrons are electronegative, e.g., oxygen |
| What is Electropositive? | • Atoms with one or two valence shell electrons are electropositive, e.g., sodium |
| What is hydrogen bond? What does it also act as? | • Attractive force between electropositive hydrogen of one molecule and an electronegative atom of another molecule • Also act as intramolecular bonds, holding a large molecule in a three-dimensional shape |
| What are Chemical Reactions? | • Occur when chemical bonds are formed, rearranged, or broken • Represented as chemical equations |
| What do Chemical Equations contain? | • Molecular formula for each reactant and product • Relative amounts of reactants and products, which should balance |
| What are the 3 patterns of Chemical Reactions? | Synthesis (combination) reactions • Decomposition reactions • Exchange reactions |
| What is Synthesis Reactions? | • A + B --> AB • Always involve bond formation • Anabolic |
| What is Decomposition Reactions? | • AB --> A + B • Reverse synthesis reactions • Involve breaking of bonds • Catabolic |
| What are Exchange Reactions? | • AB + C --> AC + B • Also called displacement reactions • Bonds are both made and broken |
| What are Oxidation-Reduction (Redox) Reactions? | • Decomposition reactions: Reactions in which fuel is broken down for energy • Also called exchange reactions because electrons are exchanged or shared differently Electron donors lose electrons and are oxidized Electron acceptors receive electrons and become reduced |
| What is Exergonic Reactions? And a example? | 1) Release Energy 2) Catatonic reactions |
| What is Endergonic Reactions? And a example? | products contain more potential energy than did reactants • Anabolic reactions |
| 1) What can all chemical reactions do theoretically? 2) When does Chemical equilibrium occur? 3) What biological reactions are irreversible due to? | 1) • All chemical reactions are theoretically reversible 2) • Chemical equilibrium occurs if neither a forward nor reverse reaction is dominant 3) Energy requirements and Removal of products |
| How is rate of reaction influenced? 1) If temperature goes up 2) If particle size goes down 3) If concentration of reactant goes up | • If temperature goes up, rate goes up • If particle size goes down, rate goes up • If concentration of reactant goes up, rate goes up |
| 1) What is catalyst? 2) What is an example of biological catalyst? | 1) Rate goes up without being chemically changed 2) Enzyme |
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