Use LEFT and RIGHT arrow keys to navigate between flashcards;
Use UP and DOWN arrow keys to flip the card;
H to show hint;
A reads text to speech;
34 Cards in this Set
- Front
- Back
|
matter vs. energy |
matter- anything that occupies space and has mass
energy- the capacity to do work, or to put matter into motion |
|
|
potential vs. kinetic energy |
potential energy- stored energy, inactive energy that has the potential or capability to do work but is not presently doing so
kinetic energy- energy in action |
|
|
Major energy forms |
-chemical energy is the form stored in the bonds of chemical substances -electrical energy results from movement of charged particles -mechanical energy is energy directly involved in moving matter -radiant energy or electromagnetic energy is energy that travels in waves |
|
|
Define chemical elements and what are the 4 major elements that form the bulk of body matter |
Chemical elements are unique substances that cannot be broken down into simpler substances by ordinary chemical methods. The 4 major elements in the human body are oxygen, carbon, hydrogen, and nitrogen |
|
|
Define atom. List subatomic particles of the atomic structure. |
An atom is the basic particle/building block of a chemical element. Includes... -nucleus, located in the center of the atom, positively charged, accounts for nearly entire mass of atom -protons, located in nucleus, positively charged, 1 atomic mass unit -neutron, located in nucleus, neutrally charged, 1 atomic mass unit -electron, located in orbital ring, negatively charges, 0 atomic mass units |
|
|
Atomic number |
# of protons written as a subscript to the left of its atomic symbol indirectly tells us the # of electrons in atom as well |
|
|
Atomic mass |
protons + neutrons written as superscript to left of atomic symbol
|
|
|
Atomic weight |
an average of the relative weights (mass numbers) of all the isotopes of an element, taking into account their relative abundance |
|
|
Isotope |
Structural variations of elements which have the same number of protons and electrons, but differ in the number of neutrons that they contain |
|
|
Radioisotope |
The heavier isotopes of many elements are unstable and their atoms decompose spontaneously into more stable forms. This process of atomic decay is called radioactivity, and isotopes that exhibit this behavior are called radioisotopes |
|
|
Define molecule |
Most atoms do not exist in the free state, but instead are chemically combined with other atoms. Such a combination of two or more atoms held together by chemical bonds is called a molecule |
|
|
Compound vs. mixture |
compound- when two or more different kinds of atoms bind, they form molecules of a compound
mixture- substances composed of two or more components that are physically intermixed |
|
|
Solution vs. Colloids vs. Suspensions |
-solutions are homogenous mixtures of components that may be gases, liquids, or solids (ex: air and seawater) -colloids, also called emulsions, are heterogeneous mixtures that often appear translucent or milky (ex: jello) -suspensions are heterogenous mixtures with large, often visible solutes that ten to settle out (ex: sand and water) |
|
|
Role of electrons in chemical bonding; octect rule |
When the outermost energy level of an atom contains eight electrons, the atom is stable and unreactive. On the other hand, atoms in which the outermost energy level contains fewer than eight electrons tend to gain, lose, or share electrons with other atoms to achieve stability |
|
|
Ionic bonds |
a chemical bond between atoms formed by the transfer of one or more electrons from one atom to another |
|
|
Covalent bonds |
electron sharing produces molecules in which the shared electrons occupy a single orbital common to both atoms and constitute covalent bonds |
|
|
Hydrogen bonds |
Hydrogen bonds form when a hydrogen atom, already covalently linked to one electronegative atom (usually nitrogen or oxygen), is attracted by another electron hungry atom, so that a "bridge" forms between them -weak bonds -important as intramolecular bonds -help maintain and stabilize structures |
|
|
polar vs. nonpolar |
-nonpolar molecules are electrically balanced and do not have separate + and - poles of charge
-polar molecules have unequal electron pair sharing, resulting in a more + pole and a more - pole |
|
|
3 major types of chemical reactions |
-synthesis reactions are the basis of constructive, or anabolic, activities in body cells, such as joining small molecules called amino acids into large protein molecules (A + B = AB) -decomposition reaction occurs when a molecule is broken down into smaller molecules or its constituent atoms (AB = A + B) -exchange or displacement reactions involved both synthesis and decomposition; bonds are both made and broken (AB + C = AC + B) |
|
|
Oxidized vs. Reduced |
oxidized = losing electrons reduced = gaining electrons |
|
|
Explain why chemical reactions in the body are often irreversible |
-chemical reactions that release energy when going in one direction will not go in the opposite direction unless energy is put back into the system -if a product of a reaction is continuously removed from the reaction site, it is unavailable to take part in the reverse reaction |
|
|
Factors that affect chemical reaction rates |
temperature (higher temp = quicker reaction), concentration of particles (more particles = quicker reaction), particle size (smaller particle = quicker reaction), catalysts |
|
|
Hydrolysis reactions vs. dehydration synthesis |
-hydrolysis reactions are decomposition reactions that work by adding a water molecule to each bond to be broken -dehydration synthesis synthesizes molecules by removing a water molecule for every bond formed |
|
|
Explain important of water and salts to body homeostasis |
-water for fluid balance, kidneys regulate volumes of water and salts, goal is for amount of water consumed to remain in balance with amount of water excreted -sodium balance critical to osmoregularity |
|
|
Acid vs. base |
-an acid is a substance that releases hydrogen ions (H+), also defined as proton donors -a base is a substance that takes up hydrogen ions, also defined as a proton acceptor |
|
|
Explain the concept of pH |
-the relative concentration of hydrogen ions in a solution is measured in concentration units called pH -the pH scale runs from 0 to 14 and is logarithmic, each successive change of one pH unit represents a tenfold change in hydrogen ion concentration |
|
|
Carbohydrates: building blocks, structure, function |
-group of molecules that includes all sugars and starches -monosaccharides are building blocks (glucose, fructose, galactose, deoxyribose, ribose) -usually carbon, hydrogen, and oxygen atoms occur in the ratio 1: 2: 1 -disaccharide is formed when 2 monosaccharides are joined by dehydration synthesis (sucrose, maltose, lactose) -polysaccharides are long chains of simple sugars linked together, called polymers (glycogen) -major functions: provide a ready, easily used source of cellular fuel |
|
|
Lipids: building blocks, structure, function |
-lipids include triglycerides, phospholipids, and steroids -triglyceride is composed of 2 types of building blocks: fatty acids and glycerol in a 3: 1 ratio of fatty acids to glycerol (saturated = only a single covalent bond between carbon atoms, form a solid/ unsaturated = contain one or more double bonds between carbon atoms, kink in bonds means fat cannot solidify). Protects body organs, major source of stored energy -phospholipids are modified triglycerides, they are diglycerides with a phosphorous-containing group and two, rather than three, fatty acid chains. Chief component of cell membranes -steroids: cholesterol is the structural basis for manufacture of all body steroids |
|
|
Proteins: building blocks, structure, function |
-building blocks of proteins are molecules called amino acids, consists of basic group called an amine group and an organic acid group, all amino acids are identical except for a single group of atoms called their R group -proteins are made up of amino acids joined together by peptide bonds -thousands of functions |
|
|
4 levels of protein structure |
-primary structure = linear sequence of amino acids composing the polypeptide chain -secondary structure = shape of polypeptide chain, alpha-helix or beta-pleated -tertiary structure = achieved when alpha-helix or beta-pleated structure folds upon one another to produce a compact ball-like or globular molecule -quaternary structure = when two or more polypeptide chains aggregate in a regular manner to form a complex protein |
|
|
Describe function of molecular chaperone |
all cells contain a call of unrelated globular proteins called molecular chaperones which help proteins achieve their functional three-dimensional structure -prevent incorrect folding, aid desired folding, help translocate proteins across cell membranes, promote breakdown of damaged proteins |
|
|
Explain general mechanism of enzyme activity |
-enzymes are globular proteins that act as biological catalysts -enzymes allow reactions to occur by decreasing the amount of activation energy required -enzymes are not involved in the reactions themselves and are not changed or used up by the reaction -3 steps in mechanism of enzyme action: enzymes active site binds with substrate, the enzyme-substrate complex undergoes internal rearrangements that form the product, the enzyme releases the product of the reaction |
|
|
DNA vs. RNA |
-DNA: located in nucleus, functions as the genetic material, directs protein synthesis, replicates itself before cell division, deoxyribose as sugar, bases of AGCT, double strand coiled into a double helix
-RNA: located in cytoplasm, function is to carry out the genetic instructions for protein synthesis, sugar is ribose, bases of AGCU, single strange that is straight or folded |
|
|
Role of ATP in cell metabolism |
ATP is the universal energy compound of body cells. Some of the energy liberated by the breakdown of glucose and other food fuels is captured in the bonds of ATP molecules and transferred via coupled reactions to energy-consuming reactions |
