Term
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Definition
- Do not contain carbon
- Formed between metals and nonmetals
- Ionic bonding |
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Term
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Definition
- Must contain carbon
- Usually large
- Covalently Bonded
- Formed between interactions between nonmeatals |
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Term
| Polar Solvent properties of water |
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Definition
| They orient themselves with their slightly negative ends toward the positive ends of the solutes, and vice versa, first attracting the solute molecules, and then surrounding them. This explains why ionic compounds and other small reactive molecules dissociate in water, their ions separating from each other and becoming evenly scattered in the water forming true solutions. |
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Term
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Definition
| Example: foods are digested to their building blocks by adding a water molecule to each bond to be broken. Water added is decomposing the substance. |
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Term
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Definition
| When large carbohydrate or protein molecules are synthesized from smaller molecules, a water molecule is removed for every bond formed. |
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Term
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Definition
| form when a hydrogen atom is attracted by another electron-hungry atom, so that a "bridge" forms between them. |
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Term
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Definition
| important intramolecular bonds, which hold different parts of a single large molecule in a specific three-dimensional shape. Some large biological molecules, such as proteins and DNA, have numerous ____________ that help maintain and stabilize their structures. |
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Term
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Definition
Acids are proton (hydrogen ion) donors
(release H+ in solution)
HCl → H+ + Cl– |
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Term
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Definition
- Bases are proton acceptors (take up H+ from solution)
- NaOH → Na+ + OH–
- OH– accepts an available proton (H+)
- OH– + H+ → H2O |
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Term
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Definition
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Term
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Definition
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Term
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Definition
| homeostasis of acid-base balance in carefully regulated by the kidneys and lungs and by chemical systems (proteins and other types of molecules) called ______ |
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Term
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Definition
| resist abrupt and large swings in the pH of body fluids by releasing hydrogen ions (acting as acids) when the pH begins to rise and by binding hydroge ions (acting as bases) when the pH drops. |
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Term
| because blood comes into close contact with nearly every blood cell. Normally, blood pH varies within a very narrow range (7.35 to 7.45) If blood pH varies from these limits by more than a few tenths, it may be fatal. |
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Definition
| Why is regulation of pH particularly critical to the body? |
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Term
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Definition
| an ionic compound containing cations other than H+ and anions other than the hydroxyl ion (OH-) |
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Term
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Definition
-dissociate in water
- Ions (electrolytes) conduct electrical currents in solution |
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Term
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Definition
Common Uses of Electrolytes:
Muscle Contraction |
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Term
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Definition
Common Uses of Electrolytes:
Nerve Impulses |
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Term
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Definition
Common Uses of Electrolytes:
Blood Clotting |
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Term
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Definition
Common Uses of Electrolytes:
Bone Development |
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Term
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Definition
Common Uses of Electrolytes:
Co-enzymes (help facilitate a reaction) |
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Term
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Definition
Common Uses of Electrolytes:
Formation of ATP,DNA, and RNA |
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Term
| Homeostatic role of the kidneys |
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Definition
| maintaining proper ionic balance in our body fluids |
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Term
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Definition
| the substance that is dissolved in a solution |
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Term
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Definition
| usually liquids such as water |
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Term
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Definition
| homogeneous mixtures of components that may be gases, liquids, or solids. Example: air we breathe ( a mixture of gases) and sea water (a mixture of salts, which are solids, and water) |
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Term
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Definition
| a group of molecules that includes sugars and starches, represent 1-2% of cell mass. Contain carbon, hydrogen, and oxygen, and generally the hydrogen and oxygen atoms occur in the same 2:1 ratio as in water |
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Term
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Definition
| Function: Major source of cellular fuel |
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Term
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Definition
| single-chain or single-ring structures containing from three to seven carbon atoms. |
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Term
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Definition
Examples
Glucose
Fructose
Galactose
Deoxyribose
Ribose |
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Term
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Definition
| formed when two monosaccharides are joined by dehydration synthesis. A water molecule is lost as the bond is made. |
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Term
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Definition
Disaccharides:
Glucose+Fructose |
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Term
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Definition
Disaccharides:
Glucose+Glucose |
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Term
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Definition
Disaccharides:
Galactose+Glucose |
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Term
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Definition
| polymers of simple sugars linked together by dehydration synthesis. Ideal storage products. They lack the sweetness of simple and double sugars. |
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Term
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Definition
| Two examples of polysaccharides |
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Term
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Definition
| the storage carbohydrate formed by plants |
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Term
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Definition
| the storage carbohydrate of animal tissues |
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Term
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Definition
| Organic compound formed of carbon, hydrogen, and oxygen; examples are fats and cholesterol. Do not have the same 2 to 1 hydrogen oxygen atom ratio as carbohydrates |
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Term
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Definition
| Function: energy storage, insulation in the body, and protection |
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Term
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Definition
| involves attaching three fatty acid chains to a single glycerol molecule by dehydration synthesis. |
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Term
| Neutral Fats (Triglycerides) |
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Definition
| Consist of fatty acid chains and glycerol; also called triglycerides or triacylglycerols. Commonly known as oils when liquid. |
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Term
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Definition
Function:
provide the body's most efficient and compact form of store energy, and when they are oxidized, they yield large amounts of energy |
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Term
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Definition
| Fatty acid chains with only single covalent bonds between carbon atoms |
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Term
| Unsatturated (mono and ply unsaturated) |
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Definition
| fatty acids that contain one or more double bonds between carbon atoms |
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Term
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Definition
| although the hydrocarbon portion of the molecule in nonpolar (the tail) and interacts only with nonpolar molecules, the phosphorous-containing part (the head) is polar and attracts other polar or charged particles, such as water or ions. |
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Term
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Definition
| Function: used as the chief material for building cellular membranes |
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Term
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Definition
| Group of chemical substances including certain hormones and cholesterol; they are fat soluble and contain little oxygen. |
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Term
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Definition
| single most important molecule in our steroid chemistry |
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Term
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Definition
| found in cell membranes and is the raw material for synthesis of vitamin D. steroid hormones, and bile salts. |
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Term
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Definition
| long chains of amino acids joined together by dehydration synthesis, with the amine end of the amino acid linked to the acid end of the next |
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Term
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Definition
| How many amino acids are there? |
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Term
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Definition
| Bond joining the amine group of one amino acid to the acid carboxyl group of a second amino acid with the loss of a water molecule. |
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Term
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Definition
| The sequence of amino acids forms the polypeptide chain |
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Term
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Definition
| The primary chain forms spirals(alpha helices) and sheets (betas sheets) |
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Term
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Definition
| superimposed on secondary structure. alpha helices and/or beta sheets are folded up to form a compact goubluar molecule held together by intramolecular bonds. |
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Term
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Definition
| Two or more polypeptide chains, each with its own tertiary structure, combine to form a functional protein. |
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Term
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Definition
| it replicates itself before a cell divides, ensuring that it provides the basic instructions for building every protein in the body. |
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Term
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Definition
| it provides basic instructions for building every protein in the body |
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Term
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Definition
| Building block of nucleic acids; consists of a sugar, a nitrogen-containing base, and a phosphate group. |
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Term
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Definition
| What are the 4 bases of DNA |
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Term
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Definition
| What is the pentose sugar of DNA? |
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Term
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Definition
| located outside of the nucleus |
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Term
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Definition
| What are the four RNA bases? |
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Term
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Definition
| the primary energy-transferring molecule in cells and it provides a form of energy that is immediately usable by all body cells |
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Term
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Definition
| an adenine- containing RNA nucleotide to which two additional phosphate groups have been added. |
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