Chamberlain collage of nursing chem 120 unit 4 midterm review 2020 Study guide

chamberlain collage of school of nursing chem 120 unit 4 midterm review 2020 study guide

Chamberlain collage of nursing chem 120 unit 4 midterm review 2020 study guide

Preview document (3 of 5 pages)

Chem – Midterm Review 1. The Scientific Method  Hypothesis : a testable educated guess  Experiments: how we test hypotheses o Variable: idea to be tested (only one) o Control: something the variable is tested against; what your testing against o Experimental protocol: how do you do the test? o Results: data generated comparing variable to controls. Includes statistics to show results are meaningful o Conclusion: interpretation of results 2. Density Density (d), of a substance is the quantity of mass (m), per unit of volume (v)  D = m/d; m = d X V; V = m/d 3. Metric; Measurement conversions (metric to metric only)  1 kilometer (km) = 1000 meters (m)  1 meter (m) = 100 centimeters (cm)  1 centimeter (cm) = 10 millimeters (mm)  1 millimeter (mm) = 1000 micrometers (um)  1 kilogram (kg) = 1000 grams (g)  1 gram (g) = 1000 milligrams (mg)  1 milligram (mg) = 1000 micrograms (ug)  1 liter (L) = 1000 milliliters (mL)  1 milliliter (mL) = 1000 microliters (uL)  1 milliliter (ml) = 1 cubic centimeter (cm3) 4. Avagado’s Number, mole  A mole (mol) = 6.02 X 1023 5. Molar Mass  Equal to the atomic mass but expressed as unit grams per mole (g/mol) 6. Atomic Number, atomic mass, isotopes, number of protons, electron, neutrons  Atomic mass is expressed as amu ; is the weighted average  Atomic Number is the number of protons in the nucleus of an atom of any element  Isotopes have the same atomic number but different mass numbers(same number protons different number protons)  Electrons are negatively charged particles in the nucleus  Protons are positively charged particles in the nucleus  Neutrons are neutral, have no electrical charge  Atomic number = the number of protons  Atomic number – (minus) atomic mass = neutrons 7. Calculating Bonds  Subtract the smaller EN value from the larger EN value o 0 – 0.4 = nonpolar covalent o > (greater than) 0.4 – 1.7 = polar covalent o > ( greater than) 1.7 = ionic bond  Ionic bonds is a bond that forms when electrons is being transferred from one form to another form. which results in positive and negative ions.  Cations – are positively charged ions; think of the “t” in cat as a +  Anion – are negatively charged ions  Covalent bond – a bond formed when atoms share electrons  Nonpolar covalent bonds – when the EN is very similar between 2 atoms  Polar covalent – when the EN is different between 2 atoms 8. Naming element from electron orbital configuration  Hydrogen = 1s1  Helium = 1s2  Lithium = 1s22s1  Beryllium = 1s22s2  Boron = 1s22s22p1  Carbon = 1s22s22p2  Nitrogen = 1s22s22p3  Oxygen = 1s22s22p4  Fluorine = 1s22s22p5  Neon = 1s22s22p6  Sodium = 1s22s22p63s1  Magnesium = 1s22s22p63s2  Aluminum = 1s22s22p63s23p1  Silicon = 1s22s22p63s23p2  Phosphorus = 1s22s22p63s23p3  Sulfur = 1s22s22p63s23p4  Chlorine = 1s22s22p63s23p5  Argon = 1s22s22p63s23p6  Potassium = 1s22s22p63s23p64s1  Calcium = 1s22s22p63s23p64s2