Title: Name:
Author: Peggy Lawson
Company: Lawson Family

Chemistry 30
Review of Basic Chemistry

1.	Name the following elements.  Spelling counts:

	H	________________________

	S	________________________

	Cl	________________________

	C	________________________

	N	________________________

	Na	________________________

	Pb	________________________

	Ag	________________________

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

	gold (Au)		copper (Cu)

2.	Write the symbols for the following elements.  

	sodium	______________

	phosphorus	_____________

	fluorine	______________

	magnesium	_____________

	potassium	______________

	calcium	_____________

	zinc	______________

	iron	_____________

4.	Using a periodic table, record the atomic mass for the following elements to one decimal place:

	chlorine (Cl)		calcium (Ca)	

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
| 82 | | | 125 |
| | | 18 | 40 |
barium | | 137 | | |
| | 89 | | | 50

6.	Match the unit with its description:

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

7.	Complete the following questions concerning the element oxygen:

a. | Number of protons | |
b. | Electron configuration | |
c. | Number of electrons (neutral atom) | |
d. | Number of valence electrons | |
e. | Electron-dot diagram (Lewis dot) | |
f. | Ion most commonly formed by oxygen | |
g. | Is the ion in part (f) an anion or a cation? | |
h. | Define these terms: | |
| Anion - |
| Cation - |

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	_________________	b.  carbon and oxygen		_______________________

10.	Define these terms:

		ionic bond - 	____________________________________________________

		covalent bond -	____________________________________________________

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

SO_4 | | | NH_4 |
NO_3 | | | OH |
PO_4 | | | CO_3 |
CrO_4 | | | Cr_2O_7 |
12.	Write chemical formulas for the compounds:

a. | sodium chloride | | | e. | magnesium fluoride |
b. | ammonium sulfate | | | f. | lead(II) phosphate |
c. | potassium nitrate | | | g. | dinitrogen pentoxide |
d. | calcium hydroxide | | | h. | sulphur trioxide |

13.	Name the following:

a. | CO |
b. | CO_2 |
c. | Na_2SO_4 |
d. | H_2O_2 |
e. | (NH_4)_2CO_3 |

14.	List the seven diatomic molecules, using proper notation:  

15.	Calculate the molar masses of the following:

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

16.		Solve for x:

a. | | b. | | c. |

	

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

		a.	List the reactant(s) in this reaction	______________________________

		b.	List the product(s)		______________________________

		c.	Write a balanced equation for the reaction, including physical states

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

			Therefore, is the reaction endothermic or exothermic?  ________________________

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

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.

	b.	Convert 275 mL to litres.

	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   +        HCl             ZnCl_2   +        H_2

	b.	        Fe_2(SO_4)_3     +         KOH             K_2SO_4      +         Fe(OH)_3

	c.	        Fe   +        O_2              Fe_2O_3

20.	Predict the products of the following reactions:

	a.	     Na_3PO_4     +        HCl              __________________________________

	b.	    Mg      +       H_2CO_3               ___________________________________

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

22.	Perform 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

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)

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

Chemistry 30 – Review of Chemistry 20