Title: Name:
Author: Peggy Lawson
Last saved by: P Lawson
Company: Lawson Family

Your initials: __________

Name:	ANSWER KEY	Date:  ________________

Chemistry 30
Review of Basic Chemistry

	1.	Name the following elements.  Spelling counts:

H | hydrogen
S | sulphur
Cl | chlorine
C | carbon
N | nitrogen
Na | sodium
Pb | lead
Ag | silver

3.	Using a periodic table, record the atomic number for the following elements:

	gold (Au)	79	copper (Cu)	29

	2.	Write the symbols for the following elements.  
	
sodium | Na
phosphorus | P
fluorine | F
magnesium | Mg
potassium | K
calcium | Ca
zinc | Zn
iron | Fe
	
4.	Using a periodic table, record the atomic mass for the following elements to one decimal place:

	chlorine (Cl)	35.5	calcium (Ca)	40.1

5.	Complete the following table.  Use the information provided in the chart – not a periodic table – to determine atomic masses, but you may refer to a periodic table to name the element.
	
Element | Atomic Number | Atomic Mass | Protons | Neutrons | Electrons
lead | 82 | 207 | 82 | 125 | 82
argon | 18 | 58 | 18 | 40 | 18
barium | 56 | 137 | 56 | 81 | 56
tin | 50 | 89 | 50 | 39 | 50

6.	Match the unit with its description:

F | 1. | amount of substance | | A. | amu or u
C | 2. | density | | B. | g
B | 3. | mass | | C. | g/mL
D | 4. | molar mass | | D. | g/mole
A | 5. | molecular mass | | E. | L
E | 6. | volume | | F. | mole

7.	Complete the following questions concerning the element oxygen:

a. | Number of protons | 8 |
b. | Electron configuration | 1s^2 2s^2 2p^4 |
c. | Number of electrons (neutral atom) | 8 |
d. | Number of valence electrons | 6 |
e. | Electron-dot diagram (Lewis dot) | | (the single dots may be on any of the 4 sides)
f. | Ion most commonly formed by oxygen | O^2- |
g. | Is the ion in part (f) an anion or a cation? | anion |
h. | Define these terms: | |
| Anion - | negative ion formed by gaining electrons
| Cation - | positive ion formed by losing electrons

8.	Draw electron-dot diagrams for:

	a.	potassium		c.	phosphorus	

	b.	nitrogen			d.	krypton	

9.	What type of chemical bond (ionic or covalent) will most likely form between:	

	a. sodium and chlorine	ionic	b.  carbon and oxygen	covalent

10.	Define these terms:

		ionic bond - 	bond formed by the transfer of electrons

		covalent bond -	bond formed by sharing valence electrons

11.	Name and provide the correct charge for these polyatomic ions:

SO_4 | sulphate	SO_4^2- | | NH_4 | ammonium	NH_4^+
NO_3 | nitrate		NO_3^- | | OH | hydroxide	OH^-
PO_4 | phosphate	PO_4^3- | | CO_3 | carbonate	CO_3^2-
CrO_4 | chromate	CrO_4^2- | | Cr_2O_7 | dichromate	Cr_2O_7^2-
12.	Write chemical formulas for the compounds:

a. | sodium chloride | NaCl | | e. | magnesium fluoride | MgF_2
b. | ammonium sulfate | (NH_4)_2SO_4 | | f. | lead(II) phosphate | Pb_3(PO_4)_2
c. | potassium nitrate | KNO_3 | | g. | dinitrogen pentoxide | N_2O_5
d. | calcium hydroxide | Ca(OH)_2 | | h. | sulphur trioxide | SO_3

13.	Name the following:

a. | CO | carbon monoxide
b. | CO_2 | carbon dioxide
c. | Na_2SO_4 | sodium sulphate
d. | H_2O_2 | hydrogen peroxide
e. | (NH_4)_2CO_3 | ammonium carbonate

14.	List the seven diatomic molecules, using proper notation:       H_2     N_2     O_2     F_2     Cl_2     Br_2     I_2

15.	Calculate the molar masses of the following:

	Molar mass – the mass of 1 mole of a substance. Find molar mass by adding together atomic masses of the individual elements.  Atomic mass has the units amu (atomic mass units); molar mass has the units g/mol (NOT g!!!)

	a.	H_2O		b.	CaCO_3	c.	(NH_4)_3PO_4		d.	Al(OH)_3

16.		Solve for x:

a. | | b. | | c. |
| x^2 = (39)(5.2) x^2 = 202.8 x = ± 14 | | 4x = (20)(5) x = | | 2.5 × 10^-8 x = 5.146 × 10^-4

17.		Liquid water is produced when hydrogen gas and oxygen gas combine.

		a.	List the reactant(s) in this reaction	hydrogen and oxygen

		b.	List the product(s)		water

		c.	Write a balanced equation for the reaction, including physical states
		
			2 H_2(g) + O_2 _(g)   → 2 H_2O_(l)

		d.	286 kJ of energy are released during the formation of one mole of water.

			Therefore, is the reaction endothermic or exothermic?   exothermic – energy is released

		e.	Rewrite the equation but now also include the energy term within the equation.

			2 H_2(g) + O_2 _(g)   → 2 H_2O_(l) + 572 kJ

			Important note – the question tells you that 286 kJ are released PER MOLE of water. Since 2 moles of water are produced according to our balanced equation, then 2 x 286 or 572 kJ are released.

			Alternate equation: 	 H_2(g) +  ½ O_2 _(g)   →  H_2O_(l) + 286 kJ

18.	Perform the necessary calculations for the following questions, expressing the final answer to the correct number of significant digits.  It is not necessary to show work.

	a.	An empty beaker has a mass of 32.41 g.  When some water is placed in the beaker, the total mass is 33.7822 g.  Find the mass of the water.

			1.37 g

	b.	Convert 275 mL to litres.

			0.275 mL

	c.	Ethyl alcohol has a density of 0.789 g/mL.  Calculate the mass of 25.0 mL of this liquid.

			

19.	Balance the following equations:

	a.	      Zn   +     2   HCl     →        ZnCl_2   +        H_2

	b.	        Fe_2(SO_4)_3     +     6    KOH     →      3  K_2SO_4      +     2   Fe(OH)_3

	c.	      4  Fe   +      3  O_2     →       2  Fe_2O_3

20.	Predict the products of the following reactions:

	a.	     Na_3PO_4     +     3  HCl      →        H_3PO_4  +  3 NaCl

	b.	    Mg      +       H_2CO_3       →       H_2   +    MgCO_3

21.	Write a net ionic equation for:   Cu(s)  +   2 AgNO_3(aq) →   Cu(NO_3)_2 (aq)   +  2 Ag(s)

		Cu(s) + 2 Ag^+(aq)   → Cu^2+(aq) + 2 Ag(s)

22.	P80erform the following calculations.  Show your work.

	a.	Calculate the mass of 0.500 mol of CO. 

	b.	How many moles of KOH are present in a 25.0 g sample of the substance?

23.	In a reaction between sulfur and oxygen, 80.0 g of sulfur dioxide is formed.  What mass of sulfur was burned?

S + O_2 → SO_2

g S = 

		The next question shows a different approach to solving stoichiometry questions. With a little practice it can make stoichiometry much easier as it helps you set up the conversions correctly.

24.	What mass of silver is precipitated (formed) when 40.0 g of copper reacts with an excess of silver nitrate in solution, according to the following equation:

Cu_(s) + 2 AgNO_3(aq) → Cu(NO_3)_2(aq) + 2 Ag_(s)

	Having trouble with stoichiometry? Try this method. 

	1 – Be sure to begin with a balanced equation. Beneath the equation we will draw a map. Begin with the substance that you are given information about – in this case we know we are dealing with 40.0 g Cu. Our map will involve converting the unit given into moles, because moles are our “bridge”.

	2 – Next, use the coefficients from the balanced equation to convert moles of one substance (Cu) into moles of the substance we want to know about – silver (Ag) in this question.

		To set up the ratio, place the number where you want to go (the Ag) on top and the coefficient where you are coming from (the Cu) on the bottom.

	3 – The final step is to convert moles of the desired material into the desired unit. For this question we are asked to find mass, so our unit is grams.

 				Cu_(s) + 2 AgNO_3(aq) → Cu(NO_3)_2(aq) + 2 Ag_(s)
							Answer
			start	40.0 g	136 g	end here
			here

Step 3

Step 1

					
				0.630 mol Cu			1.26 mol Ag

Step 2

25. (Challenge question) Some antacid products contain aluminium hydroxide, Al(OH)_3, to neutralize excess stomach acid.  What volume of a 0.10 mol/L stomach acid, HCl, can be neutralized by 912 mg of aluminium hydroxide.  The reaction is shown:

				3 HCl 	+	Al(OH)_3 	→ 	AlCl_3 +  3 H_2O

				0.350 L or 350 mL	0.912 g	START HERE

Step 1

Step 3

							

Step 2

				0.0351 mol HCl	0.0117 mol Al(OH)_3

Chemistry 30 – Review of Chemistry 20