1. Chapter 1 Chemistry: The Science of Matter
Section 1.1: The Puzzle of Matter
Section 1.2: Properties and Changes of Matter

2. Section 1.1 Objectives Classify matter according to its composition.
Distinguish among elements, compounds, homogeneous mixtures, and heterogeneous mixtures.
Relate the properties of matter to its structure.

3. Composition, Structure and Behavior
Chemistry- the science that investigates and explains the structure and properties of matter.
Matter- anything that takes up space and has mass
Mass- the measure of the amount of matter that an object contains

4. Matter Matter is all around you. What isn’t matter Phone Your neighbor
The desk
The metal of your chair
The air you are breathing
What isn’t matter
Heat
Light
Thoughts
Ideas
Radio waves
Magnetic fields

5. Mass On earth we equate mass with weight.
A bowling ball has a larger mass than a tennis ball.
I have more mass than the text book.

6. Matter
The structure of matter refers to its composition-what is it made of and how is it organized
The properties of matter describe the characteristics and behavior of matter.
Changes matter undergoes

7. Comparing Composition and Behavior (Figure 1.2 page 5)
Salt and Water
Salt is Na and Cl
Water is H and O
You can wash you hair in water, but not in salt. And you sprinkle water over popcorn.
Aspirin and Sucrose
Both are composed of C, H, and O
You wouldn’t use aspirin to sweeten cereal or use sucrose for a headache

8. Properties
You can determine some of the properties of a particular chunk of matter by examination and manipulation.
What is its color?
Is it a solid, liquid or gas?
Is it soft or hard?
Does it dissolve in water?

9. Properties of Iron Strong, but can be flattened and stretched
Does not dissolve in water
Turns to a liquid at high temperatures
Is a gray, shiny solid
Is attracted to a magnet
Conduct electricity

10. Properties and Composition
You may be able to determine many properties of a piece of matter by examining it and doing some simple tests.
However, you can not determine what it is composed of just by looking at it.

11. Examining Matter: The Macroscopic View of Matter
The macroscopic view of matter is one in which you touch, smell, taste and see.

12. The Submicroscopic View of Matter
Gives you a glimpse into the world of atoms
You cannot see this world even with the most powerful microscopic.
Matter is made up of atoms
Atoms are so small that a period at the end of a sentence is made up of 100,000,000,000,000,000,000 (100 quintillion) carbon atoms.
If you could count all 100 quintillion atoms at a rate of three per second it would take you a trillion years to finish counting.

13. Macro, micro, submicro Macroscopic – I can see with my “naked” eye
Microscopic – I need a microscope to see
Submicroscopic – I can’t see even with the most powerful microscope

14. Scanning Tunneling Microscope (STM)
Although you cannot see atoms the STM can produce images on a computer screen that show the location of individual atoms.
Platinum

15. Using Models in Chemistry
In chemistry you will use macroscopic and sub-microscopic models to understand certain concepts.
Scientific model- a thinking device, built on experimentation, that helps us to understand and explain macroscopic observations.

16. Models
A model for the atom was discussed in Greece about 2,500 years ago. However, this was not a scientific model.
The scientific model of the atom was not proposed until the 1800’s and it has with stood much experimentation with little changes.

17. Classifying Matter Matter can be classified by its composition
There are two main types of classifications
Qualitative- an observation made without measurement.
Quantitative- an observation made with measurement

18. Qualitative vs. Quantitative
There are students in this room
Sucrose contains carbon, oxygen and hydrogen
Quantitative
There are 24 students in this room
Sucrose contains 42.1 g of carbon, 51.4 g of oxygen and 6.5 g of hydrogen.

19. Pure vs. Mixture Matter can be classified by its purity.
Is the matter pure or is it a mixture?
Pure in chemistry means it contains only the same substance.
Substance- matter with the same fixed composition and properties.
Can be an element or a compound
Any sample of pure matter is a substance

20. Substances
The bag of sugar you buy at the store is pure sucrose. It all has the same properties and a fixed composition. Therefore, it is a substance.

21. Mixed Matter Mixed matter is referred to as a mixture.
Mixture- combination of two or more substances in which the basic identity of the substances are not changed.
Mixtures do not have a specific composition.
Mixtures can be separated into its components by physical means.

22. Separating Mixtures One way is by physical changes.
Physical change- a change in matter that does not involve a change in the identity of individual substances.
Boiling
Freezing
Melting
Evaporation
Dissolving
Crystallization

23. Physical Properties
Separation by physical changes takes advantage of the physical properties of the mixture.
Physical properties- characteristics that a sample of matter exhibits without any changes in its identity
Solubility
Melting and boiling point
Color
Density
Electrical conductivity
Physical state (solid, liquid or gas)

24. Types of Mixture There are two types of mixtures: Heterogeneous
Hetero means “different”
Homogeneous
Homo means “the same”

25. Heterogeneous Mixture
Heterogeneous Mixture- a mixture that does not have a uniform composition.
You can see the different composition.
Examples:
Granite
Chef Salad
Lucky Charms Cereal
Orange Juice with pulp

26. Homogeneous Mixture
Homogeneous Mixture- a mixture with a uniform composition.
You cannot tell that it is composed of more than one substance
Another name is a solution
Examples:
Salt water
Tea
Sugar water

27. Solutions
Homogeneous mixture
Examples:
Salt water
Gasoline
Air
Steel

28. Alloys
Alloys- solid solutions that contain different metals and sometimes nonmetallic substance
Table 1.1 page 23

29. Table 1.1 Some Common Alloys
Name of Alloy
% Composition
Stainless Steel
73-79% iron (Fe)
14-18% chromium (Cr)
7-9% nickel (Ni)
Bronze
70-95% copper (Cu)
1-25% zinc (Zn)
1-18% tin (Sn)
Brass
50-80% copper (Cu)
20-50% zinc (Zn)
Sterling Silver
92.5% silver (Ag)
7.5% copper (Cu)
14-karat gold
58% gold (Au)
14-28% silver (Ag)
14-28% copper (Cu)
18-karat white gold
75% gold (Au)
12.5% silver (Ag)
12.5% copper (Cu)
Solder (electronic)
63% tin (Sn)
37% lead (Pb)

30. Solutions
When you are dissolving a substance into another substance there are two important terms:
Solute – the substance being dissolved
Solvent – the dissolving agent
Salt Water
Solute = NaCl
Solvent = H2O

31. Aqueous Solution
Aqueous Solution- a solution in which the solvent is water.
Examples:
Soda
Tea
Contact-lens cleaner
Clear cleaning liquids
Most processes of life take place in aqueous solutions.

32. Substance: Pure Matter
You and everything around you is made up of chemicals.

33. Elements: The Building Blocks
If you classify an unknown piece of matter as pure; it means that it is made up of one substance
There are two types of substances
Compounds
Elements

34. Elements
Elements- a substance that cannot be broken down into simpler substances.
Simplest form of matter
Building blocks for other types of matter
All substance in the universe are:
Elements
Compounds formed from elements
Or mixtures of elements and compound

35. Elements 118 elements Examples:
Gold
Carbon
Lead
Elements combine to form millions of compounds.
Chemical elements are often referred to as the building blocks of matter

36. Elements 118 elements 90 occur naturally The remainder are synthesized
Less than half of these are abundant
The remainder are synthesized

37. Organizing the Elements
Elements are organized in the Periodic Table
The periodic table tells you:
Name
Symbol
Atomic mass

38. Symbols The symbols of the elements are extremely important to know.
You will only have to know the most common ones.
The symbols are a one to two letter representation of the elements.
Not all the symbols are the first or second letter of the elements name

39. Symbols
Oxygen O
Hydrogen H
Bromine Br
Chlorine Cl

40. Table 1.2 Some Historic Chemical Symbols
Element
Symbol
Origin
Language
Antimony Sb
Stibium
Latin
Copper Cu
Cuprum
Gold Au
Aurum
Iron Fe
Ferrum
Lead Pb
Plumbum
Potassium K
Kalium
Silver Ag
Argentum
Sodium Na
Natrium
Tin Sn
Stannum
Tungsten W
Wolfram
german

41. Compounds Are More Than One Element
Compound – a chemical combination of two or more different elements joined together in a fixed proportion.
Every compound has its own fixed composition
Therefore, every compound has unique chemical and physical properties.
The properties of a compound are different from the properties of the elements that make them up.

42. Compounds More than 10 million are known (still growing)
New natural compounds are being isolated from plants and colonies of bacteria.
New compounds are also being synthesized in labs.
Examples
Sucrose
Salt
Water

43. Formulas of Compounds
Formula – a combination of the chemical symbols that show what elements make up a compound and the number of atoms of each element.
Sucrose: Aspartame:

44. Table 1.3 Some Common Compounds
Compound Name
Formula
Acetaminophen
C8H9NO2
Acetic Acid
C2H4O2
Ammonia
NH3
Aspartame
C14H18N2O5
Propane
C3H8
Salt
NaCl
Sodium Hydroxide
NaOH
Sucrose
C12H22O11
Water
H2O

45. Review What is the difference between an element and a compound?
What is the difference between a homogeneous mixture and a heterogeneous mixture?
What is the difference between a mixture and a compound?