aboriginal peoples and chemistry list 5 ways aboriginal...

Aboriginal Peoples and Chemistry

List 5 ways Aboriginal peoples used chemicals:

Safety

List 5 pieces of info provided on a MSDS

What are the 3 ways in which WHMIS informs workers about chemicals?

Classification of Matter

Chemical and Physical Properties

Matter

Mixtures

Heterogeneous Homogeneous

Pure Substances

Compounds Elements

Chemical Properties

• describe reactivity of a substance

•

Physical Properties

• describe physical appearance of a substance

Color and Label the periodic table…

Metals and Non-Metals

State Appearance Conductivity Malleability and

ductility

Metals

Non-metals

Metalloids

Developing Atomic Theories

Dalton’s Atom

Theory

Gas Discharge Tube

Describe:

How did they use gas discharge tubes to provide evidence of electrons (JJ Thompson)?

Kelvin / Thompson Model

Describe:

Rutherford’s Experiment

Describe:

Restate Rutherford’s logic in developing his view of the atom

↓

↓

↓

↓

Define:

Nucleus:

Electron:

Empty Space:

Discuss Rutherford’s reasoning for the NEUTRON…

What is an isotope?

What did Niels Bohr mean by “energy levels” for

electrons?

A Working Model of the Atom

Subatomic Particle Relative Charge Symbol Mass (g) Radius (m)

How can the number of neutrons be calculated in different isotopes of the same element?

Electron Dot Diagram

Draw each diagram….

B F S

Name: _____________________________________

Atomic Number and Mass Number

Name Mass Number Atomic

Number

Number of

Protons

Number of

Neutrons

carbon-14 14 6 6 8

hydrogen-1 1 1

hydrogen-2 2 1

carbon-12

oxygen-18

4 2

20 10

64 29

35 45

7 7

16 16

20 21

9 10

26 30

53 74

calcium-40

119 50

26 33

208 82

silver-108

mercury-201

Unit A—Energy and Matter in Chemical Change Unit Support

L ine Master 4

Define:

ION-

Cation-

Anion-

What is a stable octet?


L ine Master 6

Name: _____________________________________

Atoms and Ions I

Symbol Number of

Protons

Number of

Electrons

Electric Charge

Li+ 3 2 1+

C 6 6 0

F− 9 10 1−

Mg2+

K+

Li

S2−

He

18 0

8 2−

17 1−

11 0

Ca2+

18

Fe3+

23

Fe2+

24

78 1+

78 2+

82 78

30 30


L ine Master 7

Name: _____________________________________

Atoms and Ions II

Name Symbol Mass

Number

Atomic

Number

Protons Neutrons Electrons Electric

Charge

fluorine atom F 19 9 9 10 9 0

nitride ion N3−

15 7 7 8 10 3−

boron atom 11

carbon atom 14

aluminium

ion

14 3+

gold ion 116 1+

40 19 0

79 35 35

19 18 1−

16 16 2−

Ag 110

cesium ion 77 1+

I− 125

Forming Compounds

Descibe:

Forming Ionic Compounds

Properties of

Ionic Compounds

Naming Ionic Compounds

1.

2.

3.

How to write an ionic compound formula

1.

2.

3.

4.

5.


L ine Master 8

Name: _____________________________________

Ionic Compounds—Univalent Metal Ions

1. If the following pairs of elements were mixed and heated, they would combine into solid ionic

compounds. Write the name and formula of each compound formed.

Name Formula

a) silver and iodine silver iodide AgI(s)

b) magnesium and oxygen

c) magnesium and bromine

d) calcium and nitrogen

e) zinc and selenium

f) sodium and sulfur

g) barium and phosphorus

h) aluminium and fluorine

i) potassium and chlorine

j) silver and oxygen

continued...

Unit A—Energy and Matter in Chemical Change

2. Write the correct names for each of the following compounds.

a) MgCI2

b) Ag3N

c) CsF

d) CdO

e) MgBr2

f) Al2O3

g) NaI

h) K2S

i) BaS

j) Li3P

Ionic Compounds Worksheet Name: ______________

A. Write the name of each of the following ionic compounds:

1. LiCl(s) ________________ 2. KBr(s) ______________

3. CaCl2(s) ________________ 4. MgO(s) ______________

5. KF(s) ________________ 6. K2O(s) ______________

7. CaO(s) ________________ 8. BeF2(s) ______________

9. AlI3(s) ________________ 10. SrS(s) ______________

11. Rb3P(s) ________________ 12. Fr2O(s) ______________

13. MgCl2(s) ________________ 14. CaF2(s) ______________

B. Write the chemical formula for each of the following ionic compounds:

1. sodium fluoride ___________ 2. barium bromide _________

3. magnesium fluoride __________ 4. aluminum chloride _______

5. lithium bromide _________ 6. potassium nitride ________

7. magnesium sulfide ___________ 8. strontium sulfide ________

9. calcium iodide ___________ 10. cesium fluoride _________

11. lithium phosphide __________ 12. aluminum oxide _________

AND: Complete practice problem 1 on page 43

Multivalent Ionic Compounds

1.

2.

3.

4.


L ine Master 9

Name: _____________________________________

Ionic Compounds—Multivalent Metal Ions

1. If the following pairs of elements were mixed and heated, they would combine into solid ionic

compounds. In this worksheet, use the most common ionic form of the multivalent metal ion.

The most common form is listed first in the periodic table. For example, iron exists as both 2+

and 3+ ions, with iron(III) being the most common.

Name Formula

a) iron and sulfur iron(III) sulfide Fe2S3(s)

b) copper and oxygen

c) manganese and fluorine

d) gold and nitrogen

e) chromium and chlorine

f) platinum and

phosphorus

g) nickel and oxygen

h) cobalt and bromine

i) tungsten and iodine

j) manganese and sulfur

continued...


2. Write the correct name for each of the following compounds. The charge on the multivalent

ion is not given by the periodic table. It is determined by the charge of the non-metal and the

subscripts that appear in the formula.

a) FeCl2(s) iron(II) chloride

b) FeBr3(s)

c) CrS(s)

d) SnO2(s)

e) Pb3N2(s)

f) HgI2(s)

g) CrO3(s)

h) MnF4(s)

i) Cu2O(s)

j) AuI3(s)

Polyatomic Ionic Compounds

1.

2.

3.


L ine Master 10

Name: _____________________________________

Ionic Compounds—Polyatomic Ions

The names and charges of polyatomic ions can be found in lists and need not be memorized. It is a

good idea, however, to get to know the more common ones introduced in the practice below.

Remember to form the name by combining the positive and negative ion:

name = positive ion + negative ion

COMBINE IONS FORMULA NAME

iron(II) & nitrate Fe2+

NO3− Fe(NO3)2(s) iron(II) nitrate

aluminium & nitrate Al3+

NO3− Al(NO3)3(s) aluminium nitrate

sodium & sulfate

lead(IV) & sulfate

magnesium &

carbonate

gold(III) & sulfite

zinc &

hydrogencarbonate

ammonium & nitrate

copper(I) & phosphate

silver & hydroxide

aluminium &

hydroxide

lead(II) & phosphate

potassium & acetate

manganese(V) &

sulfate

Polyatomic Ionic Compounds Worksheet Name: ______________

A. Write the name of each of the following compounds:

1. CuCO3(s) ________________ 2. Cu2CO3(s) _____________

3. NaNO3(s) ________________ 4. CuHCO3(s) _____________

5. CaSO4(s) ________________ 6. Mg(OH)2(s) ____________

7. Sr(ClO2)2(s) ______________ 8. Na2Cr2O7(s) ___________

9. Ba(CH3COO)2(s) ___________ 10. KSCN(s) ______________

11. LiNO2(s) ________________ 12. LiNO3(s) ______________

13. FeSO4(s) ________________ 14. NaOH(s) ______________

B. Write the chemical formula for each of the following compounds:

1. magnesium sulfate __________ 2. ammonium hydroxide __________

3. sodium phosphate __________ 4. copper (II) nitrate ___________

5. ammonium chloride __________ 6. calcium sulfite _______________

7. sodium hydrogensulfite ________ 8. nickel (II) phosphate __________

9. barium hydroxide ___________ 10. iron (III) carbonate __________

11. copper (I) permanganate ______ 12. iron (II) carbonate __________

All Ionic Compounds Worksheet

Write the chemical formula Name each compound

for each compound

1. calcium carbonate a. IrO2

2. beryllium oxide b. RaS

3. lithium fluoride c. MgO

4. nickel (ll) bromide d. CaCl2

5. lead (ll) chloride e. SnBr2

6. ammonium hydroxide f. KOH

7. silver phosphate g. Al2O3

8. magnesium acetate h. Ti(NO3)4

9. rubidium sulfide i. AgClO4

10. potassium permanganate j. Sr3(PO4)2

11. barium nitride k. PtO

12. strontium sulfate l. CuI

13. strontium sulfite m. Cu2CO3

14. lithium hydroxide n. AgCH3COO

15. iron (lll) oxide o. NaNO3

16. titanium (lV) iodide p. Cr2(OOCCOO)3


L ine Master 11

Name: _____________________________________

All Ionic Compounds

I. Write the formula for each compound.

1) calcium acetate

2) potassium chloride

3) ammonium carbonate

4) sodium nitride

5) titanium(IV) hypochlorite

6) iron(III) sulfide

7) zinc dichromate

8) platinum(IV) oxide

9) aluminium hydroxide

10) mercury(II) nitrate

11) strontium fluoride

12) tin(IV) hydrogenoxalate

13) calcium peroxide

14) gold(I) sulfate

15) lead(IV) thiocyanate

16) nickel(III) sulfide

continued...


II. Write the name of each compound.

17) CsI(s)

18) SnCl4(s)

19) Cr(NO3)3(s)

20) (NH4)3PO4(s)

21) Cu2SO4(s)

22) Mg(H2PO4)2(s)

23) Na2S2O3(s)

24) AgClO3(s)

25) Zn(OH)2(s)

Solubility

Properties of acids and bases

Very Soluble

Slightly Soluble

Properties of Acids Identifying Acids

Classical Naming of Acids IUPAC Naming of Acids

Acids

Neutralization Reactions

Properties of Bases Identifying Bases

Naming Bases

Bases

Ionic Compounds, Acids, & Bases Worksheet

Chemical Name Chemical Formula Ionic, Acid, or Base

rubidium oxide

strontium hydroxide

HNO2(aq)

iron (II) iodide

NaOH(aq)

CrO(s)

Pb(NO3)4(aq)

aqueous hydrogen

sulfate

Ag3PO4(s)

potassium hydroxide

HCl(g)

HCl(aq)

lithium fluoride

aluminum phosphide

acetic acid

beryllium sulphide

CuF(s)

Au2Se(s)

Ti(OH)3(aq)

hydroiodic acid

SnO2(s)

C6H5COOH(aq)

lithium hydroxide

ZnBr2(s)

platinum (IV) chlorate

Describe

Forming Molecular

Compounds

Properties of

Molecular Compounds

Molecular Prefixes

Molecular Prefixes

Common Hydrogen

Compounds

diatomic & polyatomic

molecular elements


L ine Master 12

Name: _____________________________________

Binary Molecular Compounds

A. Write the correct name for each compound below. Use prefixes to indicate the number of atoms of

each element in the name of the molecular compound. (Remember: The prefix “mono-” is not used

with the name of the first element.)

1 atom: mono- 3 atoms: tri- 5 atoms: penta- 7 atoms: hepta 9 atoms: nona-

2 atoms: di- 4 atoms: tetra- 6 atoms: hexa 8 atoms: octa- 10 atoms: deca-

1) BrCl3

2) BN

3) N2O3

4) NI3

5) SF6

6) XeF4

7) PCl3

8) CH4

9) PCl5

10) P2O5

11) S2Cl2

12) ICl2

13) NH3

14) P4O10

15) H2O

16) OF2

continued...


B. Write the correct formula for each compound below. Use subscripts to indicate the number of

atoms of each element in the formula (never reduce).

1) chlorine monoxide

2) sulfur hexachloride

3) dinitrogen monoxide

4) nitrogen trifluoride

5) sulfur tetrachloride

6) xenon trioxide

7) carbon dioxide

8) boron trichloride

9) diphosphorus pentoxide

10) phosphorus trichloride

11) sulfur dioxide

12) bromine pentafluoride

13) disulfur dichloride

14) boron trifluoride

15) tetraarsenic decoxide

16) silicon tetrachloride

Ionic and Molecular Compounds Worksheet Name: ______________

A. Write the name of each of the following compounds and state if it is ionic or

molecular. If ionic, state the solubility:

1. MgBr2 ________________ 2. KHSO4 __________________

3. CF4 ________________ 4. Ca(OH)2 __________________

5. N2Br4 ________________ 6. P2O5 __________________

7. NH3 ________________ 8. (NH4)3PO4 _________________

9. SO3 ________________ 10. NaOH __________________

11. CuSO4 ________________ 12. PCl3 __________________

13. CH4 ________________ 14. FeI3 __________________

B. Write the formula of each of the following compounds and state if it is ionic or

molecular. If ionic, state the solubility:

1. sulfur hexafluoride ___________ 2. silver phosphate ____________

3. phosphorus pentachloride ________ 4. sodium iodide _______________

5. manganese (II) chloride _________ 6. nitrogen trifluoride ___________

7. sodium perchlorate ___________ 8. methanol ______________

9. cobalt (II) permanganate ___________ 10. silicon tetrafluoride __________

11. ammonia _____________ 12. aluminum oxide _________

What is a chemical reaction?

What is combined?

What is formed?

5 pieces of evidence?

Reactants

Exothermic Reaction

Products

Endothermic Reaction

Conservation of Mass

Word Equation Chemical Equation

Balancing Equations

Rules

Steps

Balanced

Coefficients

States

Tips and Examples

Tips


L ine Master 17

Name: _____________________________________

Balancing Formula Equations 1

Balance the following chemical equations:

a) _____ Na(s) + _____ O2(g) _____ Na2O(s)

b) _____ Al(s) + _____ Cl2(g) _____ AlCl3(s)

c) _____ N2(g) + _____ O2(g) _____ NO2(g)

d) _____ HI(g) _____ H2(g) + _____ I2(s)

e) _____ NH3(g) _____ H2(g) + _____ N2(g)

f) _____ Al2S3(s) _____ Al(s) + _____ S8(s)

g) _____ BN(s) + _____ Cl2(g) _____ BCl3(g) + _____ N2(g)

h) _____ SnF4(aq) + _____ Cr(s) _____ CrF3(aq) + _____ Sn(s)

i) _____ Mg(s) + _____ HCl(aq) _____ MgCl2(aq) + _____ H2(g)

j) _____ (NH4)3PO4(aq) + _____ CaBr2(aq) _____ Ca3(PO4)2(s) + _____ NH4Br(aq)

k) _____ Pb(NO3)4(aq) + _____ K2Cr2O7(aq) _____ Pb(Cr2O7)2(s) + _____ KNO3(aq)

l) _____ AgClO4(aq) + _____ Na3PO4(aq) _____ NaClO4(aq) + _____ Ag3PO4(s)

m) _____ HCl(aq) + _____ Ca(OH)2(s) _____ CaCl2(aq) + _____ H2O(l)

n) _____ CH3COOH(aq) + _____ Ba(OH)2(aq) _____ Ba(CH3COO)2(aq) + _____ H2O(l)

o) _____ C3H8(g) + _____ O2(g) _____ CO2(g) + _____ H2O(g)

p) _____ C6H14(l) + _____ O2(g) _____ CO2(g) + _____ H2O(g)

q) _____ C3H6OS2(s) + _____ O2(g) _____ CO2(g) + _____ H2O(g) + _____ SO2(g)


L ine Master 18

Name: _____________________________________

Balancing Formula Equations 2

Balance the following chemical equations:

a) _____ Pb(s) + _____ O2(g) _____ PbO(s)

b) _____ N2(g) + _____ H2(g) _____ NH3(g)

c) _____ Na(s) + _____ H2O(l) _____ NaOH(aq) + _____ H2(g)

d) _____ C4H10(g) + _____ O2(g) _____ CO2(g) + _____ H2O(g)

e) _____ H3PO4(aq) + _____ KOH(aq) _____ K3PO4(aq) + _____ H2O(l)

f) _____ C5H12(l) + _____ O2(g) _____ CO2(g) + _____ H2O(g)

g) _____ Zn3N2(s) + _____ H2O(l) _____ Zn(OH)2(aq) + _____ NH3(g)

h) _____ Fe3O4(s) + _____ H2(g) _____ Fe(s) + _____ H2O(l)

i) _____ Al(s) + _____ H2SO4(aq) _____ H2(g) + _____ Al2(SO4)3(aq)

j) _____ CrS(s) + _____ O2(g) _____ CrO(s) + _____ SO2(g)

k) _____ HClO3(aq) + _____ HCl(aq) _____ H2O(l) + _____ Cl2(g)

l) _____ CaC2(s) + _____ AsBr3(aq) _____ C(s) + _____ As(s) + _____ CaBr2(aq)

m) _____ 4 NH3(g) + _____ 5 O2(g) _____ 4 NO(g) + _____ 6 H2O(l)

n) _____ HNO3(aq) + _____ NO(g) _____ NO2(g) + _____ H2O(l)

o) _____ Al(NO3)3(aq) + _____ NaOH(aq) _____ NaNO3(aq) + _____ Al(OH)3(s)

p) _____ C2H5OH(l) + _____ O2(g) _____ CO2(g) + _____ H2O(g)

q) _____ NaIO3(s) _____ NaI(s) + _____ O2(g)


L ine Master 16

Name: _____________________________________

Writing Formula Equations from Word Equations

In the following exercises, recall that many of the non-metal elements exist as molecules, such as

H2(g) or S8(s). Refer to Table A2.9 on page 48 of Science 10 for the chemical formulas of molecular

elements.

1. Rewrite the following word equations as formula equations and then balance them:

a) solid sodium metal reacts with chlorine gas to produce solid sodium chloride

b) solid potassium metal reacts with oxygen gas to produce solid potassium oxide

c) hydrogen gas reacts with oxygen gas to produce liquid water

d) solid potassium chlorate decomposes into oxygen gas and solid potassium chloride

e) solid aluminium oxide is decomposed into solid aluminium and oxygen gas

f) mercury(II) sulfide is decomposed into liquid mercury and solid sulfur

g) aqueous cobalt(III) nitrate reacts with solid zinc to produce aqueous zinc nitrate and solid

cobalt

continued...


h) fluorine gas reacts with aqueous lead(IV) iodide to produce aqueous lead(IV) fluoride and

solid iodine

i) aqueous gold(III) bromide reacts with solid silver metal to produce solid silver bromide

and solid gold metal

j) aqueous sodium sulfate reacts with aqueous strontium hydroxide to produce aqueous

sodium hydroxide and solid strontium sulfate

k) aqueous thallium(I) hydroxide reacts with aqueous magnesium bromide to produce solid

magnesium hydroxide and solid thallium bromide

l) methane gas reacts with oxygen gas to produce carbon dioxide gas and water vapour

Types of Reactions

Formation

Decomposition

Combustion

Single Replacement

Double Replacement


L ine Master 19

Name: _____________________________________

Classifying and Balancing Chemical Equations

A. Classify the following reactions as: formation, decomposition, single replacement, double

replacement, or combustion.

1. 2 KClO3(s) 2 KCl(s) + 3 O2(g)

2. 3 ZnCl2(aq) + 2 K3PO4(aq) 6 KCl(aq) + Zn3(PO4)2(s)

3. Mg(s) + 2 HCl(aq) MgCl2(aq) + H2(g)

4. 2 H2(g) + O2(g) 2 H2O(g)

5. Al(s) + 3 NiBr2(aq) 2 AlBr3(aq) + 3 Ni(s)

6. 4 Al(s) + 3 O2(g) 2 Al2O3(s)

7. 2 NaCl(s) 2 Na(s) + Cl2(g)

8. CaCl2(s) + F2(g) CaF2(s) + Cl2(g)

9. AgNO3(aq) + KCl(aq) AgCl(s) + KNO3(aq)

10. 2 C2H6(g) + 7 O2(g) 4 CO2(g) + 6 H2O(g)

11. N2(g) + 3 H2(g) 2 NH3(g)

12. 2 H2O2(aq) 2 H2O(l) + O2(g)

13. (NH4)2SO4(aq) + Ba(NO3)2(aq) BaSO4(s) + 2 NH4NO3(aq)

14. MgI2(aq) + Br2(l) MgBr2(aq) + I2(s)

15. SO3(g) + H2O(l) H2SO4(aq)

continued...


B. Balance and classify each chemical equation below.

1. ____ CH4(g) + ____O2(g) ____CO2(g) + ___H2O(g)

2. ____ Na(s) + ____I2(s) ____NaI(s)

3. ____ NaOH(aq) + ____H2SO4(aq) ____Na2SO4(aq) + ____ H2O(l)

4. ____ Fe(s) + ____O2(g) ____Fe2O3(s)

5. ____ Pb(NO3)2(aq) + ____K2CrO4(aq) __ PbCrO4(s) + __KNO3(aq)

6. ____ S8(s) + ____O2(g) ____SO3(g)

7. ____ C3H5(NO3)3(s) __CO2(g) + ____N2(g) + __H2O(l) + ___O2(g)

8. ____ Fe(s) + ____CuCl2(aq) ____FeCl2(aq) + ____Cu(s)

9. ____ C3H8(g) + ____ O2(g) ____CO2(g) + ____H2O(g)

10. ____ CaSO4(aq) + ___AlBr3(aq) ___CaBr2(aq) + ___Al2(SO4)3(s)

Mole

Specific Heat Capacity

Phase Changes

aboriginal peoples and chemistry list 5 ways aboriginal...

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