Physical Science: 4012-2 Name: Ionic Phenomena Practice test

1. Fill in the answers to the statements using the list below:a) Atom b) electron c) proton d) chargee) hydrogen f) ion g) shell h) neutron

i) These particles are in the nucleus of an atom: ii) The atom is composed of these particles: iii) It has a positive charge: iv) It has a negative charge: v) It has no charge at all:

2. Answer True or False:i) Non-metals are good conductors of heat and electricity:

ii) Non-metals are to the left of the zigzag line of the periodic table:

iii) The proton and electron are of opposite electrical charge

iv) The mass of a neutron is equal to that of a proton:

v) The nucleus contains protons and neutrons.

3. Look up the following elements in the periodic table and write down their respective Shorthand electron configurations:

He H

C B

Ne Al

Na O

S N

4. From the following list, identify which are Isotopes of the same element.

a) 9 protons, 8 electrons, 9 neutronsb) 6 protons, 6 electrons, 7 neutronsc) 1 proton, 1 electron , 0 neutronsd) 6 protons. 7 electrons, 8 neutrons

e) 8 protons, 7 electrons, 7 neutrons

Answer: 5. The periodic table below has letters identifying the sections for the major

groups of elements. Identify with the proper letter(s) the following:

A

F B C D G H

E

I

J

i) Metals: ii) Alkali metals:

iii) Noble Gases iv) Halogens

v) Non-metals vi) Alkaline earth metals

6. Consider the molecule: Li F and answer the following:

i) What type of bond is formed in this molecule: ii) Write the ionization equation for Lithium: iii) Write the ionization equation for Fluorine: iv) What is the ion charge of: Li F

7. Using the electronegativity values, calculate and indicate what type of bond is formed in the water molecule of H2O. (The electronegativities of H and O are 0.4 and 1.7 ).

8. Explain the difference between :

i) an Ionic Bond and a Covalent Bond:Answer:

ii) a Polar and non-Polar Bond:Answer:

9. Draw the Lewis diagram and the structural formula representation for theAmmonia molecule: NH3

Lewis diagram Structural formula

a) Given the following listed information , complete the table below by identifying the Element and whether it is an anion or cation:

No. protons electrons Neutrons Element Anion Cation

a 8 10 8b 1 1 2

c 17 17 19d 12 12 13e 8 8 10

f 17 18 18

g 12 10 12h 1 0 0

10. Indicate how many electrons each of the following elements must gain or loseto satisfy the octet rule and write the Ion charge E.g. gain 2 e- ; O-2.

i) Mg ii) O

iii) Al iv) P

v) Li vi) Cl

11. Using the above information, first complete the ions formed and then use the cross-over rule to complete the molecule formed:

ions:Mg P Al Cl Li O

moleculesMg P Al Cl Li O

12. For each of these elements, show the electro-negativity value,then calculate the difference. Finally indicate the type of bond formed:

Electro-negativity value Difference Bond Mg- P-

Al- Cl-

Li- O-

13. Draw the Lewis diagrams and the structural formula ( if applicable ) for these two molecules that you completed above:

Al & Cl Li & O

14. Classify the following substances as one of the following(Element, Compound, Homogeneous solution or Heterogeneous mixture ):

i) A cupful of dry sugar

ii) Sugar dissolved in water

iii) Orange juice

iv) Pure Silver chain

15. Write the name of each of the following compounds

i) CaO

ii) SrF2

iii) H2S

iv) CaCO3

v) Ba(OH)2

vi) Mg3N2

vii) Na2CO3

16. Provide the chemical formula for the following compounds.

i) Barium fluoride

ii) Potassium sulphate

iii) sulphur trioxide

iv) carbon tetraiodide

v) Sodium chromate

vi) Carbon disulphide

vii) Lithium borate

17. Dissociate the following molecules into its ions. Then indicate whether it is an acid , base or salt.

Molecule: Cation Anion (Acid/Base/Salt )

i) HNO3

ii) AgOH

iii) Li2SO4

iv) HI

v) MgSO4

vi) H2SO4

vii) Al(OH)3

viii) Fe(NO3)2

ix) Zn(OH)2

18. Determine the molar mass of the following compounds using up to 3 decimal places:

i) KBr

ii) NaCl

iii) CCl4

iv) Fe2O3

v) P2O5

vi) Mg3(PO4)2

19. Calculate the number of moles in 100g of the following compounds:

a) Al2O3

b) MgBr2

20. Lab tests on these solutions have provided the results tabled below. From the results. Conclude whether the solution is an acid, base, salt or non of these:

SolutionConducts Red Litmus turns Blue Litmus turns Conclusion

Yes No Red Blue Red Blue1 x x x

2 x x x

3 x x x4 x x x5 x x x6 x x x

7 x x x

21. In each vessel below dissociate the given compounds by showing the relative quantity of ions or molecules contained:

NaCl H2SO4

conducts a little conducts very well

C12H22O11 HCldoes not conduct conducts very well

22. Identify which is the solvent and solute in the following solutions:

Solution Solvent SoluteSoft DrinkGin (40%)Ammonia waterSalt Water

23. Calculate the concentrations of the following solutions and arrange in increasing order of strength:

i) 5 g of salt in 1200 mL of water:

ii) 0.7 Kg of salt in 25 L of water:

iii) 400mg of salt in 250 mL of water:

Answer:

24. Calculate the molar concentration of 4 moles of H2SO4 in 8 litres of water.

25. Calculate the molar concentration of 196 g of H2SO4 in 4 litres of water:

26. Determine the molar mass of the following substances:

i C3H8 ______________________________

ii NH4NO3 ______________________________

iii CH3COOH ______________________________

iv Cu(NO3)2 ______________________________

v P2O5 ______________________________

27. Calculate the number of moles contained in 500g of the following compounds ( i.e. the same compounds from the above calculation):

i C3H8 ______________________________

ii NH4NO3 ______________________________

iii CH3COOH ______________________________

iv Cu(NO3)2 ______________________________

v P2O5 ______________________________

28. Calculate the concentrations of the following solutions which contain varying quantities of Calcium Chloride. Then place the five solutions in order of increasing concentrations.

i 0.4 Kg of CaCl2 in 50L of water __________________________

ii 15g of CaCl2 in 1L of water __________________________.

iii 50g of CaCl2 in 4L of water __________________________

iv 100mg of CaCl2 in 200mL of water __________________________

v 250g of CaCl2 in 0.5 L of water __________________________

Increasing order of Concentration: ________________________________

29. Given the following table with the data for dilutions, calculate the missing quantity in the blank spaces. ( i.e. C1V1 = C2V2 )

Stock Solution Diluted Solution

C1 V1 C2 V2

15mol/L 5 mol/L 350 mL

10 mol/L 125 mL 2.50 mol/L

1 L 2 mol/L 3500 mL

5 mol/L 0.75 Ml 250 mL

8 mol/L 1.5 mol/L 15 L

30. A chemist wants to make a 0.6 mol/litre solution of Mg(OH)2. He has a stock solution available at a concentration of 3 mol/L. If he puts 0.5L of the concentrated solution into a large container, what volume is the final solution?

31. A student wishes to find the concentration of a stock solution whose label has been lost. She puts 750 mL into a 3 litre bottle and fills it to exactly half with water. She then does a titration and discovers that the concentration of the diluted solution is 1.75 mol/L. What is the concentration of the stock solution?

32. The following table contains information on four aqueous solutions identified by the letters A to D. Fill in the missing information for concentration [H+], the pH and the nature of the solution (Acid, Base or Neutral ).

A B C D

[H+] 1 x 10 -9 1 x 10 -3

pH 4

Nature neutral

33. The following table of indicators contains the color changes along with their turning points.

Indicator Color Change Turning PointA red to yellow 4.4 to 6.2B colourless to yellow 5.0 to 7.0C yellow to violet 10.0 to 11.0D yellow to red 7.6 to 9.2

The following results are obtained during a test. What is the pH range for each:

i Result for ‘A’ is yellow, the pH range is ____________________

ii Result for ‘B’ is yellow, the pH range is ____________________

iii Result for ‘C’ is yellow, the pH range is ____________________

iv Result for ‘D’ is yellow, the pH range is ____________________

The solution’s pH range is therefore in the range: __________________________

34. Balance the following chemical reactions:

i) NH3 + Cl2 NH4Cl + N2

ii) CuO + NH3 Cu + H2O + N2

iii) HNO3 + Cu Cu(NO3)2 + NO + H2O

35. i) Balance the equation below.ii) Then indicate the molar quantities of each substance in the reaction.iii) Finally calculate how many moles are required of each substance if 4 moles of H2O are produced

CH4 + O2 CO2 + H2O

moles moles moles moles

moles moles moles 4 moles

36. Calculate the number of moles of carbon dioxide produced by heating 42 moles of NaHCO3 in the following equation. ( Balance equation first ).

NaHCO3 Na2CO3 + CO2 + H2O

37. Write the neutralization equations for the following acid-base pairs:

i HNO3(aq) and KOH(aq) ____________________________________

ii HClO4(aq) and LiOH(aq) ____________________________________

iii HCl(aq) and NH4OH(aq) ____________________________________

iv HI(aq) and NaOH(aq) ____________________________________