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A+P Test 1 Ch2a
Chem. Level-Inorg.
| Question | Answer |
|---|---|
| # of elements in human body and major ones | 26. 96% H, O, C, and N |
| Atom | Smallest unit of matter |
| Parts of atom | +Protons and neutrons (subatomic particles in nucleus), and -electrons in electron orbits. |
| Distinctive to specific element. | # of Protons |
| Atomic Number | # of Protons |
| Mass Number | # of Protons plus # of Neutrons = mass of nucleus |
| Isotope | Different Mass Number due to change in neutrons |
| Radioactive Isotope | Unstable elements (trying to get rid off extra neutrons) |
| Half Life | Time it takes for half of nucleus (neutrons) to decay to stable form. |
| Pure Atoms have what equal in number | Protons and Electrons |
| Atomic Mass | Average mass of an elements naturally occurring isotopes (usually class to mass #) |
| Ion | Atom with a charge (+ or -) |
| Molecule | Two or more atoms sharing electrons. |
| Compound | Two or more atoms of DIFFERENT elements sharing electrons. |
| Positively charged ion | Cation |
| Negatively charged ion | Anion |
| Free radical and potential danger. | Charged atom with unpaired electrons in outer shell. May take -e from living tissue, killing it. |
| Octet Rule | Atoms like to have a complete outer shell (8 electrons, 2 if in first orbit) |
| Antioxidants | Give e-s to free radicals. The f.r. are then disposed of naturally. |
| 3 types of chemical bonds | ionic, covalent, and hydrogen. |
| hydrogen bond | The attraction between a positively charged H end of a molecule to a negatively charged end (usually O or N) of a molecule. |
| Ionic bond | The attraction of oppositely charged ions, a cation and an anion. One atom gains electrons and one loses electrons |
| Covalent bond | Two or more atoms share electrons. The more atom pairs shared, the stronger the bond. |
| Electrolyte | An ionic compound that breaks into positive and negative ions in solution. |
| Chemical reaction | New bonds form or old bonds break between atoms |
| Starting and ending substances of a chemical reaction. | Reactants and Products (have equal masses) |
| Two principle forms of energy. | potential energy (stored by matter due to its position) kinetic energy (matter in motion) |
| Two types of chemical reactions. | Exergonic (release energy) and endergonic (absorb energy) |
| Energy needed to start a reaction. | Activation Energy |
| Catalyst | Chemical compounds (often enzymes) that speed up chemical reactions by lowering the activation energy needed for a reaction to occur. The catalyst remains UNCHANGED. |
| Inorganic compound | Simple bonded (ionic or covalent), lack carbon (except CO2, HCO3, and H2CO3) |
| Organic compound | Covalent bonds. Long chains of carbon and usually H. |
| parts of a solution | solvent and solute |
| mixture | Combination of elements that are unbonded. |
| Solution properties | A mixture that will not settle out and where the solute particles are evenly dispersed and so small the mixture appears clear. |
| Colloid properties | A mixture that will not settle out. The size of the solute particles are large enough that they disperse light and the mixture appears opaque (milk). |
| Suspension | The solute may mix but will settle out with time (blood). |
| Solution concentrations are usually expressed in this form. | mass/volume percentage |
| Total number of molecules in a volume. | mol/L (to make a 1 mole solution of NaCl, dissolve 1 mole NaCl in enough H2O to equal 1 liter of solution) |
| Avogadro's Number | 6.023 x 10 to the 23rd (# of particles in 1 mole) |
| Mole | 6.023 x 10 to the 23rd particles. The mass of 1 mole in grams of element = atomic mass of element |
| How many grams in 2 moles of C(16)? | 32 grams |
| How many particles in 1 mole of O(12)? | 6.023 x 10 to the 23rd |
| How many particles in 24 grams of O(12)? | 2(6.023 x 10 to the 23rd) |
| How many moles in 32 grams of C(16)? | 2 moles |
| 4 important properties of H20 | 1. High heat of vaporization (takes lots of energy to turn from liquid to gas). 2. High heat capacity (can absorb a lot of energy before increasing in temperature). 3. Water is a great lubricant (due to H bonds) 4. Water is a great solvent. |
| Hydrolysis | Water molecules used to break down larger molecules into smaller molecules which can then be absorbed. |
| Dehydration synthesis reaction | 2 smaller molecules join to form a larger molecule and a water molecule is one of the products. |
| Acid | Substance that dissolves into 1 or more hydrogen (H+) ions (and 1 or more anions). ELECTRON ACCEPTOR |
| Base | Substance that dissolves into 1 or more hydroxide (OH-) ions (and 1 or more cations). ELECTRON DONOR. Removes H+ from a solution. |
| Salt | When dissolved, dissociates into anions and cations, neither of which is H+ or OH-. Often are electrolytes. |
| Base + Acid = | Salt + Water |
| Electrolytes | Ions in solution, creating electrical currents. |
| pH scale | Concentration of H+ acid 1-6.9 neutral 7 (H+=OH-) base 7.1-14 (1 whole number change on scale = 10x H+ cc) |
| Human body pH norm and terms for either side. | Norm 7.35-7.45. More acidic = acidosis. More basic = alkalosis. |
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