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Chamberlain College of Nursing: CHEM120 Midterm Exam Guide (Latest-2022) / CHEM 120 Midterm Exam Guide / CHEM 120 Midterm Review/ CHEM120 Midterm Review | Complete and Latest Guide |
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  • Chamberlain College Of Nursing

Chamberlain College of Nursing: CHEM120 Midterm Exam Guide (Latest-2022) / CHEM 120 Midterm Exam Guide / CHEM 120 Midterm Review/ CHEM120 Midterm Review | Complete and Latest Guide |

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  • February 21, 2022
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  • chamberlain college of nursing chem120 midterm exam guide latest 2022 chem 120 midterm exam guide chem 120 midterm review chem120 midterm review | complete and latest guide |

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CHEM 120: 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 & 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

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