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