Nursing Chemistry Module 1: Sections 1-2

Module 1: Section 1 focuses on general chemistry topics like, atomic theory, elements, isotopes and atomic weights, the periodic table, valence electrons and electron dot symbols, ions and ionic bonding. We also look at naming ions and polyatomic ions, formulas and naming of ionic compounds, covalent Bonds, Lewis structures and molecular shapes, polar and non-polar covalent bonds and molecules. And finally naming binary molecular compounds.

Section 2 looks at balancing chemical equations, neutralization, combustion and oxidation reduction reactions, the mole and molar mass relationship, Chemical Stoichiometry, molarity and acid base chemistry.

Module 1: Section 1 Atomic and Molecular Properties

Review and study these Power Point Lecture slides to help answer the upcoming questions. The lecture slides are very animated and should be downloaded and viewed in "Slide Show" to get the most benefit from them.

Module 1 Section 1 Read only

1.  Place the correct values in the areas in the table below

  • P
  • e-
  • 0
  • N
  • +1
  • 1.672622 e-24
  • -1
  • 1.674927 e-24
  • 9.109328 e-28

2.  Atomic make up: Fill in the blank

The  is a small region of the atom ~about 10 million times smaller than the diameter of the atom. But contains 99.99% the mass of the atom.

3.  Atoms: Fill in the blanks

Atoms of different elements differ from each other according to how many they contain

4.  Drop a pin on the isotope with 34 protons and 45 neutrons.

5.  Calculate the average atomic weight of Sulfur if it naturally contained two isotopes of which 30% is S-30 and 70% is S-33.

  • 32.07
  • 32.10
  • 32.00
  • 33.23
  • 31.09

6.  Drop a pin on the atom that has only two isotopes, one is 62% at 78 amu and the other is 38% at 83 amu.

7.  Drop a pin on the the heaviest transition metal and the noble gas.

8.  Drop a pin on the correct compound formula for a salt made with magnesium and chlorine.

9. Drop a pin on the correct compound formula for aluminum sulfide.

10. Drag and place the name to the correct polyatomic ions

  • Acetate
  • Dichromate
  • Chlorate
  • Chromate
  • Bicarbonate
  • Sulfite
  • Hydrogen phosphate
  • Sulfate
  • Nitrate
  • Permanganate
  • Dihydrogen phosphate

11. Drop a pin on the correct compound formula for calcium phosphate

12.  Fill in the blanks question

In a , atoms “share” some or all of their valence electrons in such a manner as to achieve a noble gas configuration about each atom.

13.  What type of bond forms when two atoms share 6 electrons?

  • Single ionic bond
  • double ionic bond
  • single covalent bond
  • double coavlent bond
  • triple ionic bond
  • triple covalent bond

14.  Fill in the blanks.

is the ability of an atom during bond formation to attract electrons from its bonding partner.  The higher the , the stronger is the atom’s electron attracting ability.

15.  Rank the bonds in order of largest to smallest polarity. Place the bond with the largest polarity on top and the smallest polarity on bottom.

  • B-F
  • C-F
  • N-F
  • O-F

16.  Draw the Lewis structure for a molecule with one phosphorous (central) atom and 3 hydrogen atoms and choose all that apply.

  • tetrahedral electron pair geometry
  • trigonal planar electron pair geometry
  • trigonal pyramidal molecular geometry
  • tetrahedral molecular geometry
  • one lone pair of electrons on the central atom
  • 2 lone pairs of electrons on the central atom
  • no lone pairs on the central atom

17. Draw the Lewis structure for the molecule shown and use it to answer the next 5 question.

Using the skeleton structure above and finish the Lewis structure and use it to answer the next 5 questions.

18.  What was the total number of valence electrons needed in the Lewis structure from question 17?

  • 6
  • 8
  • 12
  • 16
  • 24

19.  How many double bonds were needed in the Lewis structure from question 17.

  • 0
  • 1
  • 2
  • 3

20.  What is electron pair geometry for the Lewis structure from question 17?

  • Linear
  • Trigonal planar
  • Tetrahedral
  • Square planar
  • Trigonal pyramidal

21. What is molecular geometry for the Lewis structure from question 17?

  • Linear
  • Tetrahedral
  • Bent
  • Trigonal pyramidal
  • Trigonal planar

22.  How many lone pairs of electrons are on the central atom on the Lewis structure from question 17?

  • 0
  • 1
  • 2
  • 3

23.  Drag and place the molecule name to its formula.

  • tricarbon dioxide
  • dinitrogen monoxide
  • nitrogen dioxide
  • carbon dioxide
  • dicarbon tetroxide
  • dinitrogen tetroxide

24.  Drop a Pin on the correct electron pair and molecular geometry

25.  Drop a Pin on the correct electron pair and molecular geometry

26.  Drop a Pin on the correct electron pair and molecular geometry

27.  Select all that are true regarding the image below.

  • electron pair geometry is trigonal pyramidal
  • electron pair geometry is tetrahedral
  • molecular geometry is trigonal pyramidal
  • molecular geometry is tetrahedral
  • polar molecule
  • non-polar molecule

28.  Select all that are true regarding the image below.

  • electron pair geometry is trigonal bent
  • electron pair geometry is trigonal planar
  • molecular geometry is trigonal pyramidal
  • molecular geometry is trigonal planar
  • molecular geometry is bent
  • non-polar molecule
  • polar molecule

29. Drop a pin on any molecule shown below that has dipole-dipole interactions.

30. Drop a pin on any molecule shown below that has London dispersion forces only.

31. Drop a pin on any molecule shown below that has hydrogen bonding capabilities.

32. Intermolecular force

Module 1: Section 2 Equations, the Mole, and Chemical Formulas Stoichiometry and Acids and Bases

Review and study these Power Point Lecture slides to help answer the upcoming questions. The lecture slides are very animated and should be downloaded and viewed in "Slide Show" to get the most benefit from them.

Module 1 Section 2 Read only

1. Fill in the blanks question

A describes the identities and relative amounts of reactants and products in a chemeical reaction.

2. Fill in the blanks question

The , substances formed during the reaction, have different properties from the , the original substances that combine in a chemical reaction

3. Balance the following equation using whole number coefficients. Drag and place the correct coefficient to each component.

  • 15
  • 14
  • 16
  • 2

4. Balance the following equation. Drag and place the correct coefficient to the component.

  • 1
  • 3
  • 2

5. Drop a pin on the salt that forms when nitric acid is neutralized with barium hydroxide

6.  Drop a pin on the correct oxidation number for sulfur (S).

7. Drop a pin on the correct oxidation number for the chromium atom.

8. Drop a pin on the correct oxidation number for the carbon (C) atom.

9. Drag a place the correct value to each statement.

  • 3
  • 18.4
  • 10.8

10. How many grams are in 3.6 moles of sodium carbonate?

  • 106 grams of sodium carbonate
  • 381.5 grams of sodium carbonate
  • 209.5 grams of sodium carbonate
  • 67.8 grams of sodium carbonate

11. How many moles are in 5.6 grams of calcium chloride?

  • 111 moles of calcium chloride
  • 1.5 moles of calcium chloride
  • 0.05 moles of calcium chloride
  • 0.15 moles of calcium chloride
  • 2.5 moles of calcium chloride

12. Balance the equation and us it to answer the next 4 questions.

13. Which of the following statements is FALSE concerning the stoichiometric relationships found in the balanced equation from question 12?

  • 1 mole of pentane will react with excess oxygen forming 5 moles of carbon dioxide
  • 1.5 moles of pentane will react with excess oxygen forming 9 moles of water
  • 8 moles of oxygen will react with excess pentane forming 5 moles of carbon dioxide
  • 2 moles of pentane will react with excess oxygen forming 15 moles of carbon dioxide
  • 3 moles of pentane with excess oxygen will form 18 moles of water.

14. Referring to question 12. How many moles of carbon dioxide will form when 2.6 moles of pentane react with excess oxygen?

  • 2.6 moles of carbon dioxide
  • 5.2 moles of carbon dioxide
  • 7.8 moles of carbon dioxide
  • 13.0 moles of carbon dioxide
  • 15.6 moles of carbon dioxide

15. If you wanted to form 18.95 moles of water how many moles of oxygen would you need to react with excess pentane? (Based on the balanced equation from question 12)

  • 25.27 moles of oxygen
  • 2.37 moles of oxygen
  • 8.0 moles of oxygen
  • 1.33 moles of oxygen

16. What is the maximum number of moles of carbon dioxide that would form if you reacted 2 moles of pentane with 15.2 moles of oxygen? (based on the balanced equation from question 12)

  • 10 moles of carbon dioxide
  • 5 moles of carbon dioxide
  • 9.5 moles of carbon dioxide
  • 0.63 moles of carbon dioxide

17. Drag and place the quantities to correctly solve the stoichiometric calculation.

  • 1 mol H_2
  • 2.0 g H_2
  • 2 mol NH_3
  • 3 mol H_2
  • 17 g NH_3
  • 1 mol NH_3

18. Drop a pin on the mass of water formed when 35.0 grams of methane reacts with excess oxygen.

19. Calculate the molar concentration when 3.8 grams of NaCl is dissolved in enough water to make 350.0 ml of solution.

  • 3.8 M NaCl
  • 0.00018 M NaCl
  • 0.19 M NaCl
  • .350 M NaCl
  • none of these

20.  Calculate the molar concentration of potassium ions when 50.6 grams of potassium sulfate is dissolved in enough water to make 500.0 ml of solution.

  • 0.58 M K+
  • 0.29 M K+
  • 1.16 M K+
  • 3.32 M K+
  • none of these

21.  Calculate the volume of 2.50 M HCl needed to react with 200.0 ml of a 3.50 M NaOH soluiton.

  • 150.0 ml of HCl solution
  • 200.0 ml of HCl solution
  • 280.0 ml of HCl solution
  • 350.0 ml of HCl solution
  • none of these

22.  Drop a pin on all properties related to bases

23.  Drop a pin on any of the following that are acid-base conjugate pairs

24.  Drag and place the name next to the correct formula.

  • hydrochloric acid
  • magnesium hydroxide
  • sulfuric acid
  • nitric acid
  • calcium hydroxide
  • hydroiodic acid
  • potassium hyudroxide
  • sodium hydroxide
  • hydrobromic acid
  • lithium hydroxide

25. Calculate the molarity of a solution made by dissolving 5.0 g (mw=40 g/mol) of NaOH in enough water to make 500 milliters of solution.

  • 5.0 M
  • 0.25 M
  • 1.25 M
  • 3.0 M
  • 0.50 M

26.  Calculate the molarity of hydroxide ions (OH-) in a solution prepared by dissolving 60.0 grams of sodium hydroxide in enough water to make 300 ml of solution?

  • 1.5 M
  • 5.0 M
  • 3.5 M
  • 2.0 M
  • 1.0 M

27. Calculate the concentration of the hydroxide ion (OH-) after dissolving 1.5 g of magnesium hydroxide in enough water to make 1.6 liters of solution.

  • 1.0 M
  • 1.3 M
  • 0.032 M
  • 0.016 M
  • 2.5 M

28. Calculate the hydrogen ion (H+) concentration after dissolving 3.5 g (mw=81/mol) of HBr in enough water to make 500 milliliters of solution.

  • 0.086 M
  • 1.0 M
  • 0.05 M
  • 2.5 M
  • 1.5 M

29.  Calculate the pH of a nitric acid solution made by dissolving 2.1 g nitric acid in enough water to make 300 milliliters of solution.

  • pH = 1.45
  • pH = 0.95
  • pH = 6.07
  • pH = 7.00
  • pH = 11.12

30. Calculate the pH of a sodium hydroxide solution made by dissolving 3.1 g sodium hydroxide in enough water to make 500 milliliters of solution.

  • pH = 0.81
  • pH = -0.81
  • pH = -13.19
  • pH = 13.19
  • none of these

31. Calculate the pH of a magnesium hydroxide solution made by dissolving 4.5 g magnesium hydroxide in enough water to make 800 milliliters of solution.

  • pH = 1.01
  • pH = -1.01
  • pH = -12.98
  • pH = 12.98
  • none of these

32. Fill in the blanks question

A reaction results when equal amounts of a strong acid and base react, forming an ionic compound and water.   The ionic compound that forms is called a

33. What salt is formed when potassium hydroxide reacts with hydrobromic acid?

  • sodium chloride
  • potassium hydride
  • potassium bromide
  • bromic hydride
  • potassium chloride

34.  Drop a pin on the correct compound formula for the salt formed when calcium hydroxide reacts with nitric acid.

35. Calculate the molarity of a nitric acid solution if 300.0 ml of the solution neutralizes 500.00 ml of a 0.40 M sodium hydroxide solution.

  • 1.0 M nitric acid
  • 2.7 M nitric acid
  • 0.12 M nitric acid
  • 0.67 M nitric acid
  • none of these

36.  Calculate the pH of a buffer solution of 0.35 M acetic acid and 0.39 M sodium acetate (conjugate base of acetic acid) and the pKa of acetic acid is 4.75

  • pH = 6.80
  • pH = 7.00
  • pH = 4.80
  • pH = 9.20
  • None of these