Science 10 Chemistry Review Name: __________

(Worksheet) Date: __________

Block: __________

The following prescribed learning objectives will be tested on the provincial exam. Use the following as a guide to help you review for the exam. Be sure to use information in your Data Booklet to help you answer some of the questions

It is expected that students will:

10D1 research and illustrate the development of our understanding of the structure of matter from early times to the present

10D2 describe the arrangement of subatomic particles (electrons, protons, neutrons) in elements

· Bohr Model of elements 1 to 20

10D3 distinguish among atoms, isotopes, and ions

10D4 explain how chemical and physical characteristics of substances are due to differences in the bonding of their constituent parts

10D5 demonstrate a knowledge of chemical formulae and balanced chemical equations

· including ionic and covalent compounds

· including writing names, formulae, and balanced equations

10D6 give evidence for and classify the following chemical reactions: synthesis, decomposition, replacement, and acid-base

· including single and double replacement

· including neutralization

Part 1. Concepts

1. Define the following:

a) Science

b) Scientific Method (also list the 5 steps)

c) Ionic compound

d) Covalent compound

e) Atom

f) Cation

g) Anion

h) Diatomic

i) Molecule

2. I am an element; use the information below to discover who I am.

a) I have 31 protons. gallium

b) I am neutral and have 15 electrons. phosphorus

c) I have 48 neutrons and am an alkali. rubidium

d) I have 10 neutrons and am a halogen. fluorine

e) I have 18 electrons, am an anion in group 5. phosphide ion

f) I have 10 electrons, am a cation in group 2. magnesium

g) I have 45 neutrons. bromine

3. Draw Bohr diagrams for (include the three representations for each):

Calcium atom Ca --- 2 e^- --- --- 8 e^- --- --- 8 e^- --- --- 2 e^- --- 20 p^+	Calcium Ion Ca^2+ --- 8 e^- --- --- 8 e^- --- --- 2 e^- --- 20 p^+
Fluorine atom F --- 7 e^- --- --- 2 e^- --- 9 p^+	Fluoride Ion F^- --- 8 e^- --- --- 2 e^- --- 9 p^+
Sodium atom --- 1 e^- --- --- 8 e^- --- --- 2 e^- --- 11 p^+	Sodium ion --- 8 e^- --- --- 2 e^- --- 11 p^+
Chlorine atom --- 7 e^- --- --- 8 e^- --- --- 2 e^- --- 17 p^+	Chloride ion ---- 8 e^- --- ---- 8 e^- --- ---- 2 e^- --- 17 p^+

4. Complete the chart.

	Proton	Electron	Neutron
Symbol	p^+	e^-	n^0
Charge	+1	-1	0
Mass	1 amu	1/1837 amu	1 amu
Location	nucleus	orbiting nucleus	nucleus

5. State five properties of metals.

all solids (except Hg), all silver (except Au and Cu), shiny, malleable and ductile, good conductor of heat and electricity

6. State five properties of nonmetals.

could be solid, liquid or gas, various colors including colorless, dull (not shiny), solids are crumbly, poor conductor of heat and electricity

7. List the properties of acids and bases.

Acids – taste sour, conduct electricity, turn blue litmus red, and corrode active metals

Bases – taste bitter, conduct electricity, turn red litmus blue, and feel slippery

8. Complete the chart.

	Symbol	Atomic Number	Mass Number	p^+	n^o	e^-	charge
a)	^231Ra	88	231	88	143	88	0
b)	^212Po	84	212	84	128	84	0
c)	^3517Cl	17	35	17	18	17	0
d)	^7335Br	35	73	35	38	35	0
f)	^10747Ag	47	107	47	60	47	0
g)	^6629Cu^2+	29	66	29	37	27	+2
h)	^189F^-	9	18	9	9	10	-1
i)	^12753I^-	53	127	53	74	54	-1
j)	^3617Cl^-	17	36	17	19	18	-1
k)	^2713Al^3+	13	27	13	14	10	+3
m)	^5324Cr^3+	24	53	24	29	21	+3
n)	^5325Mn	25	53	25	28	25	0

9. Describe the model of the atom put forth by:

a) Dalton

b) Thomson

c) Rutherford

d) Bohr

Part 2. Name or write the formula for each ionic compound.

	Chemical Formula	Name Of Compound
1.	K2CO3	potassium carbonate
2.	(NH4)2S	ammonium sulphide
3.	Ca(OH)2	calcium hydroxide
4.	Fe2O3	iron (III) oxide
5.	Mn(ClO2)4	manganese (IV) chlorite
6.	Cr(NO3)3	chromium (III) nitrate
7.	K2Cr2O7	potassium dichromate
8.	MgSO3	magnesium sulphite
9.	NaNO2	sodium nitrite
10.	(NH4)2SO4	ammonium sulfate
11.	NaHCO3	sodium bicarbonate
12.	K3PO4	potassium phosphate
13.	Co(OH)3	cobalt (III) hydroxide
14.	NH4Br	ammonium bromide
15.	Ba(NO3)2	barium nitrate
16.	KMnO4	potassium permanganate
17.	Al2(CO3)3	aluminum carbonate
18.	CuHCO3	copper (I) bicarbonate
19.	Ba(ClO4)2	barium perchlorate
20.	Pb(HS)2	lead (II) hydrogen sulfide

Part 3. Name or write the formula for the following molecular (covalent) compounds:

	Chemical Formula	Name Of Compound
1.	CCl4	carbon tetrachloride
2.	CO2	carbon dioxide
3.	NO2	nitrogen dioxide
4.	S3O4	trisulphur tetraoxide
5.	P2O5	diphosphorus pentaoxide
6.	NI3	nitrogen triiodide
7.	SiO4	silicon tetraoxide
8.	N2O5	dinitrogen pentoxide
9.	SO2	sulfur dioxide
10.	SO3	sulphur trioxide
11.	CO	carbon monoxide
12.	P4O10	tetraphosphorus decaoxide
13.	N2O	dinitrogen monoxide
14.	S4F6	tetrasulphur hexafluoride
15.	N5Br9	pentanitrogen nonabromide
16.	P2Se3	diphosphorus triselenide

Part 4. Balance each equation.

1. __2_ Sb + __5_ Cl₂ à __2_ SbCl₅

2. __2_ FeCl₂ + __1_ Cl₂ à __2_ FeCl₃

3. __1_ P₄ + __6_ I₂ à __4_ PI₃

4. __1_ Na₂S + __2_ HCl à __2_ NaCl + __1_ H₂S

5. __3_ NaOH + __1_ FeCl₃ à __3_ NaCl + __1_ Fe(OH)₃

6. __3_ KOH + __1_ H₃PO₄ à __1_ K₃PO₄ + __3_ H₂O

7. __2_ NaOH + __1_ CuSO₄ à __1_ Na₂SO₄ + __1_ Cu(OH)₂

8. __2_ HNO₃ + __1_ Ca(OH)₂ à __2_ H₂O + __1_ Ca(NO₃)₂

9. __2_ NH₃ + __3_ CuO à __3_ H₂O + __3_ Cu + __1_ N₂

10. __4_ NH₃ + __5_ O₂ à __4_ NO + __6_ H₂O

11. __4_ NH₃ + __7_ O₂ à __4_ NO₂ + __6_ H₂O

12. __2_ NH₃ + __4_ O₂ à __1_ N₂O₅ + __3_ H₂O

13. __1_ P₄ + __10_ N₂O à __2_ P₂O₅ + __10_ N₂

14. __2_ Al + __6_ HCl à __2_ AlCl₃ + __3_ H₂

15. __1_ Zn + __2_ KOH à __1_ K₂ZnO₂ + __1_ H₂

16. __1_ B₂O₃ + __3_ Mg à __3_ MgO + __2_ B

17. __2_ CH₃OH + __3_ O₂ à __4_ H₂O + __2_ CO₂

18. __1_ C₆H₁₂O₆ à __2_ C₂H₅OH + __2_ CO₂

19. __2_ Na + __2_ H₂O à __2_ NaOH + __1_ H₂

20. __2_ PbS + __3_ O₂ à __2_ PbO + __2_ SO₂

21. __1_ SiCl₄ + __4_ Na à __1_ Si + __4_ NaCl

22. __2_ Mg + __1_ CO₂ à __2_ MgO + __1_ C

23. __2_ Al + __3_ H₂SO₄ à __1_ Al₂(SO₄)₃ + __3_ H₂

24. __1_ N₂ + __4_C + __1_Na₂CO₃ à __2_ NaCN + __3_ CO

Part 5. State the reaction type and balance each equation.

Write / Balance:	Type:
1. 4 Al (s) + 3 O2 (g) à 2 Al2O3 (s)	Synthesis
2. 2 HCl (aq) + 1 Ca(OH)2 (aq) à 2 HOH (l) + 1 CaCl2 (aq)	Neut
3. 1 CH4 (g) + 2 O2 (g) à 1 CO2 (g) + 2 H2O (g)	Combustion
4. 1 Zn (s) + 1 Pb(CH3COO)2 (aq) à 1 Pb (s) + 1 Zn(CH3COO)2 (aq)	SR
5. 1 SO3 (g) + 1 H2O (l) à 1 H2SO4 (aq)	Synthesis
6. 2 HgO (s) à 2 Hg (l) + 1 O2 (g)	Decomp
7. 2 NaI (aq) + 1 Pb(NO3)2 (aq) à 1 PbI2 (s) + 2 NaNO3 (aq)	DR
8. 1 Cl2 (aq) + 2 NaI (aq) à 1 I2 (aq) + 2 NaCl (aq)	SR
9. 1 Al2(SO4)3 (aq) + 3 Ca(OH)2 (aq) à 2 Al(OH)3 (s) + 3 CaSO4 (s)	DR
10. __2_ H2O (l) à 2 H2 (g) + O2 (g)	Decomp
11. __2_ Na (s) + __1_ Cl2 (g) à 2 NaCl (s)	Synthesis
12. __1_ Ca (s) + __2_ HOH (l) à Ca(OH)2 (s) + H2 (g)	SR
13. __3_ H2SO4 (aq) + __2_ Al(OH)3 (s) à 6 H2O (l) + Al2(SO4)3 (aq)	Neut
14. __1_ Cl2 (aq) + __2_ KBr (aq) à 2 KCl (aq) + Br2 (aq)	SR
15. __1_ Na2CO3 (aq) + __1_ Ca(OH)2 (aq) à 2 NaOH (aq) + CaCO3 (s)	DR

Part 6. Bonding.

1. Describe the characteristics of ionic bonding and use Na and Cl atoms to show how an ionic bond is formed (the mechanism).

Characteristics

Ø It involves a transfer of electrons between metal atoms and nonmetal atoms. Ø Metals lose electrons to obtain a filled valence shell. Nonmetals gain electrons to obtain a filled valence shell. Ø The atoms become ions (a cation and an anion – which are simply charged atoms!!) Ø The ions are held together in an alternating pattern of ions called an ionic crystal lattice. The ions are held together by an electrostatic attraction (opposite charges attract!). Ø The resulting compound is a large collection of ions, which we simplify to a formula unit (simplest ratio of ions).

Mechanism

Ø There is a transfer of an electron from a metal to a nonmetal forming ions. Ions are attracted to each other forming ionic crystal lattice.

2. Describe the characteristics of covalent bonding and use two H atoms to show how a covalent bond is formed (the mechanism).

Characteristics	Ø Occurs between nonmetal atoms, which share electrons. Ø Each atom contributes one electron (forming a shared pair of electrons) that spends “time” with each atom. Ø Atoms that bond this way make up molecules.
Mechanism	Ø There is a mutual attraction between one atom’s nucleus (+ve charge) and another atom’s electron (-ve charge). This pulls the atoms together. Ø The two atoms overlap their valence shells and share a pair of electrons (note the pair of electrons in the overlap area).

Part 7. Periodic Table.

1. Describe the location of each chemical family on the periodic table below:

A

B

C

D

E

2. State several chemical and physical properties of each chemical family.

Noble gases - not reactive, gas, low melting and boiling points, complete valence shell

Alkali Metals - soft metal, low density, low melting point, low boiling point, reactive with water

Halogens - brightly colored, high density, low melting point, very reactive

3. State the Law of Conservation of mass.

Mass can neither be created nor destroyed; it may only change form.

4. a) What is Mendeleev famous for? Creating the first periodic table.

b) State the Periodic Law. If the elements are arranged according to an increasing atomic mass order, a pattern can be seen in which the properties of the elements reoccur on a regular basis.

5. Explain the concept of isotopes and provide an example.

Isotopes are atoms of the same element that have different masses due to a different number of neutrons. Isotopes of an element are the same in every way except for their masses since they have different numbers of neutrons - e.g. chlorine-35 has 18 neutrons while chlorine-37 have 20. These two atoms behave in exactly the same way.