1. Introduction to Matter and Qualitative Analysis

2. Welcome
While we are waiting for everyone to arrive, attempt the following problems before we begin
Page 2  Questions 1 through 15

3. Particle Theory - Review
All Matter is made up of extremely tiny particles
Each Pure substance has its own kind of particles, different from the particles of other pure substances
Particles are always moving -Particles at a higher temperature are generally moving faster, on average than particles at a lower temperature.
Particles attract each other

4. What is matter? Anything that has: So pretty much everything. Mass
Volume
So pretty much everything.

5. Physical Properties
Physical Properties- The characteristics of a substance.
There are three states of matter, what are they?
Solid
Liquid
Gas
All three of these states are physical states of matter.

6. Physical Properties of Solids, Liquids and Gases
Phase
Structure
Movement of Particles
Shape of Sample
Density
Compressibility
Solid
- Particles closely packed
- Particles in fixed positions
- Vibration
-Definite shape
-Volume of its own
-Usually more dense than liquid or gas
-Cannot be compressed significantly
Liquid
-Particles Closely packed
- Particles not fixed in position
- Rotation
- Translation (slower)
- Takes shape of container
- Volume of its own
- Usually less dense than solid
- Cannot be compressed significantly
Gas
- Particles widely spaced
- Rotation,
- Translation (fast)
- Occupies entire volume of container
- Much less dense than solid or liquid
- Can be easily compressed

7. Physical Properties
Physical property observations can be made using several senses.
Sight
Smell
Touch
Taste
Sound – This can only give additional information about the others

8. Physical Properties Colour/ appearance Texture Odour Clarity Taste
Colourless, white, black, shiny, dull,
Fine, course, smooth, gritty
Odourless, spicy, sharp, burnt,
Transparent, Translucent opaque
Sweet, sour, salty, buttery

9. Typical physical properties
Hardness- The measure of the resistance of a solid to being scratched or dented. A harder Material will dent a softer one.
Rank the following from hardest to softest. Steel nails, chalk, glass, diamond.
Diamond ˃ Steel nails ˃ Glass ˃ Chalk
Malleability- The ability to be hammered or bent into different shapes
Example Aluminum foil.
Brittle – Shatters easily

10. Typical physical properties
Ductility- Can be pulled into a wire.
Example: Copper wires
Melting and Boiling Points - The temperatures at which substances change states.
Ex Water: MP = 0ºC , BP = 100 ºC

11. Typical physical properties
Crystal Form – The solid forms of minerals
Example – Sodium chloride = table salt
Solubility- The ability a substance to dissolve in a solvent.
Eample: salt is soluble in water where pepper is not.

12. Typical physical properties
Viscosity- Refers to how easily a liquid flows: the thicker the liquid the more viscous it is.
Density – The amount of mass per unit volume of that matter. (kg / cm3)

13. Chemical properties (3)
A chemical property describes the behaviour of a substance as it becomes a new substance

14. Chemical Properties
1. Combustibility is the ability of a substance to burn. In order to burn a substance requires Oxygen

15. Chemical Properties
Light sensitivity is a chemical property of that can cause new substances to form when light hits it.

16. Chemical Properties
3. Reacting with an acid is a chemical property where when acid is poured on a substance it produces a gas and bubbles.

17. Classification Of Matter
Pure Substances
Element
Compound
Mixture
Mechanical Mixture
Suspension
Solution

18. Pure Substance
A substance with constant composition. Can be classified an either an element or as a compound.
Examples: Table salt (sodium chloride, NaCl), sugar (sucrose, C12H22O11), water (H2O), iron (Fe), copper (Cu), and oxygen (O2).

19. Element
A substance that cannot be separated into two or more substances by ordinary chemical (or physical) means. We use the term ordinary chemical means to exclude nuclear reactions. Elements are composed of only one kind of atom.
Examples: Iron (Fe), copper (Cu), and oxygen (O2).

20. Compound
A substance that contains two or more elements, in definite proportion by weight. The composition of a pure compound will be invariant, regardless of the method of preparation. Compounds are composed of more than one kind of atom.
The term molecule is often used for the smallest unit of a compound that still retains all of the properties of the compound.
Examples: Table salt (sodium chloride, NaCl), sugar (sucrose, C12H22O11), and water (H2O).

21. Mixture
Two or more substances, combined in varying proportions - each retaining its own specific properties. The components of a mixture can be separated by physical means, i.e. without the making and breaking of chemical bonds.
Examples: Air, table salt thoroughly dissolved in water, milk, wood, and concrete.

22. Homogeneous Mixture
Mixture in which the properties and composition are uniform throughout the sample. Such mixtures are termed solutions. Examples: Air and table salt thoroughly dissolved in water

23. Heterogeneous Mixture
Mixture in which the properties and composition are not uniform throughout the sample. Examples: Sand, Salads, chocolate chip cookies
- You will be able to see different substances in the mixture.

24. Suspension
A cloudy mixture in which tiny particles of one substance are held within another.
Can be separated out when the mixture is poured through filter paper.
A suspension is also a heterogeneous mixture.

25. Physical changes
In a physical change, the substance involved remains the same. The substance may change form or state, however. All changes of state are physical changes.
There are other physical changes that are not changes of state. Dissolving is a physical change. When sugar is dissolved it spreads out in the water but the sugar is still sugar. If the water was boiled off there would be sugar left over. Most Physical changes can be reversed.

26. Chemical changes
In a chemical Change the substance is changed into one or more different substances. The new substances have different properties from the original substance. Most chemical changes are difficult to reverse and most cannot be. The new substances are not likely to combine and form the original substance.
Often during a chemical change you cannot see the change that has occurred in the substance, but you can observe the results of the change. There are clues that suggest that a chemical change has taken place.

27. Building Scientific Knowledge

28. Clues that a chemical change has occurred
Evidence
Change in colour
Final product(s) may have a different colour than the colours of the starting material(s).

29. Clues that a chemical change has occurred
Evidence
Formation of a solid (precipitate)
Final materials may include a substance in a state that differs from the staring material(s): Precipitate

30. Clues that a chemical change has occurred
Evidence
Formation of a gas
Final materials may include a substance in a state that differs from the starting material(s); commonly, a gas

31. Clues that a chemical change has occurred
Evidence
Release / absorption of heat or light
Energy (light, electricity, sound or most commonly heat) is given off or absorbed.

32. Clues that a chemical change has occurred
Evidence
The change is difficult to reverse
The change cannot be reversed or it is difficult to.

33. Qualitative Analysis
Qualitative analysis: Involves determining the composition of an unknown compound or mixture. This is usually done by investigating its physical and chemical properties.

34. Quantitative Analysis
Refers to analyses in which the amount or concentration may be determined (estimated) and expressed as a numerical value in appropriate units.
Qualitative Analysis may take place without Quantitative Analysis, but Quantitative Analysis requires the identification (qualification) of the analyte for which numerical estimates are given.

35. Observation and Inference
A statement that is based on what you see, hear, taste, touch and smell.
Inference:
A judgement or opinion that is based on observations and/or conclusions

36. When trying to identify a sample of matter we
In chemistry we use these two components of qualitative analysis frequently.
When trying to identify a sample of matter we
Observe the sample, and then
Infer what it is based on what we know about other matter.

37. Empirical Knowledge and Theoretical Knowledge
Knowledge coming directly from observations
It describes what is being observed
Theoretical Knowledge:
Knowledge based on ideas that are created to explain observations
We explain things by using theories that we know.

38. Theory: Model: A explanation of a large number of related observations
Ex. Theory of relativity , Theory of evolution  
Model:
A model is a way of representing a theory or idea.
A model can change over time
Ex. The model of the atom , a globe of the earth.

39. How to light a Bunsen burner
Step 1
The first step is to check for safety - lab coat on, long hair tied back, safety glasses on, books and papers away from the flame, apparatus set up not too close to the edge of the table...

40. How to light a Bunsen burner
Step 2
The second step is to look at the holes.  Check that the holes are closed.  The holes can be adjusted to let in more or less air by turning the collar(see photos below).
Open Closed

41. How to light a Bunsen burner
Step 3
Hold the sparker in one hand above the burner and turn on the gas with the other.
As soon as you turn the gas on start sparking.
NOTE: some have an extra gas valve to them. Look before you light it.

42. How to light a Bunsen burner
Step 4
Adjust the flame by turning the collar so that you have the appropriate flame for the experiment (usually the medium blue flame). 

43. How to light a Bunsen burner
Step 5
During the experiment, stay vigilant so that if a problem occurs, you are ready to turn off the flame quickly.  This means that you should not leave your bench unattended. 

44. Now its your turn
Everyone in the class must show that the know how to do this properly before they can continue with the activity.

45. Homework “The Burning Candle” lab on page 11 Do this now
Class / Homework – page 12 # 1- 6
Do this later

46. Questions
Classify each of the following statements as either an inference or an observation
The wood does not burn because it is wet
The boiling point of methanol is 67.5 C
The light that a glow stick emits can be prolonged if the glow stick is placed in a fridge
The temperature of a metal increased due to an increase in the vibrations of the atoms within it.
There is 125mL of water in the flask

47. 2. “Theories cannot be prove; they can only be supported with experiment evidence” Comment on this statement 3. Explain how models are useful for conveying a theory or idea 4. Using a concept map, illustrate how the following terms are interconnected: empirical knowledge, inference, observation, theory.

48. 5. In a court of law, responses from witnesses who state opinions are often stuck from the record. Give reasons why a lawyer may want a witness to make statements based on observations rather than inferences. 6. Qualitative chemical analysis involves identifying a substance through diagnostic tests. Diagnostic test are based on physical and chemical properties of substances. Is qualitative analysis empirical or Theoretical. Give reasons.

49. The periodic Table

50. The Foundation of the periodic Table
Dmitri Mendeleev devised and published the periodic table in in 1869.
Mendeleev found he could arrange the 65 elements that were then known in a grid or table so that each element had:
1. A higher atomic weight than the one on its left.
2. Similar chemical properties to other elements in the same column.
He did not know about orbits at this time

51. Dmitri Mendeleev
He noticed gaps in the table and predicted where elements would fit and their properties before they were discovered.

52. Henry Moseley
In 1913, Henry Moseley, who worked with Rutherford, showed it is atomic number (charge) and not (as Mendeleev had proposed) atomic weight that is most fundamental to the chemical properties of any element. Like Mendeleev, Moseley was able to predict correctly the existence of new elements based on his work.

53. The Periodic Table
Today the elements are still arranged in order of increasing atomic number (Z) as you go from left to right across the table.
We also know an element's chemistry is determined by the way its electrons are arranged - its electron configuration.

54. Other table features Important Features of the Table
The elements are also organized in two fashions horizontal vertical and horizontal lines called groups and periods.
Groups- elements with similar chemical properties in a vertical column in the main part of the table;
Period – elements, arranged in a horizontal row, whose properties change from metallic on the left to non-metallic on the right

55. Other table features
Staircase line – A zigzag line that separates metals (to the left) from non-metals (to the right) ;

56. Chemical Groups The alkali Metals
Soft, silver colour elements; solids at SATP; exhibit metallic properties; react violently with water to form basic solutions and liberate hydrogen gas; react with halogens to form compounds similar to sodium chloride; stored under oil in a vacuum to prevent reaction with air.

57. Chemical Groups The alkaline Earth Metals
Light, very reactive metals; solids at SATP; exhibit metallic properties; form oxide coating when exposed to air; react with oxygen to form oxides with the general formula MO(s); all except beryllium will react with hydrogen to form hydrides with the general chemical formula XH2; react with water to liberate Hydrogen gas.

58. Chemical Groups Transition Metals
Exhibit a wide range of chemical and physical properties; characteristically strong, hard metals with high MP; good conductors of electricity; variable reactivity form ions with variable charges many react with oxygen to form oxides; some will react with solutions of strong acids to form hydrogen gas.

59. Chemical Groups Halogens
May be solids, liquids, or gasses at SATP; exhibit non-metallic properties – not lustrous and non-conductors of electricity; extremely reactive, with fluorine being the most reactive; react readily with hydrogen and metals.

60. Chemical Groups Noble Gases
Gases at SATP; low melting and boiling point; extremely uncreative, making them especially interesting to chemists;

61. Chemical Groups Representative Elements
Include metals and non-metals from Groups 1, 2, and 13 through 17; may be solids, liquids, or gases as SATP; called representative because they most closely follow the periodic law; many form colourful compounds.

62. Chemical Groups Rare Earth Elements
The rare earth elements can be divided into lanthanides (elements ) and actinides (elements ). The naturally occurring rare earths are found on earth in only very small amounts. The actinides include most of the well-known elements that take part in or are produced by nuclear reactions. No element with atomic number higher than 92 occurs naturally. These elements are produced artificially in nuclear reactors or particle accelerators.

63. Work Homework: Do the Questions on Page 2 Questions 1 through 15
 Homework:  Read Appendix B2: Safety In the Laboratory      Pages 480 to 484  
Homework: Page 12    Section 1.2 Questions 1 through 6
Candle lab