1. Chemistry: The Study of Matter
Chapter 1
Chemistry: The Study of Matter

2. What is Chemistry?
The study of matter, its composition, properties, and the changes it undergoes
Applied Chemistry is the using of chemistry to attain certain goals, in fields like medicine, agriculture, and manufacturing
Pure Chemistry gathers knowledge for knowledge sake

3. Which Comes First? Applied Chemistry Pure Chemistry
usually comes first, applied later
Called technology
Or engineering
Pure chemistry can explain behavior that has been used without knowing why
Steel swords
Can’t be good or bad
Can be good or bad depending on use

4. Applied Chemistry Material Design Scale Plastics Paints Nanotechnology
Macroscopic- Big enough to see
Microscopic- Too small to see unaided
Nanotechnology- manipulating individual atoms and molecules

5. Applied Chemistry Energy
Ability to do work
Different types can be converted to each other
Conservation
More efficient conversion
Insulation
Production –new sources
Storage- batteries, fuel cells

6. Applied Chemistry Agriculture Medicine
Production- fertilizers, soil tests
Protection – pesticide, herbicide
Medicine
Drugs
Materials- hips, artificial skin
Biotechnology- using organisms as a means of production

7. Applied Chemistry Environment- Pollution Astronomy Eliminate sources
Treatment once polluted
Astronomy
Remote analysis of stars from their light
Analysis of extraterrestrial samples

8. Branches of Chemistry
Analytical Chemistry -studies composition of substances.
Organic Chemistry -compounds containing carbon
Inorganic Chemistry -substances without carbon
Biochemistry- Chemistry of living things
Physical Chemistry studies behavior of substances
rates and mechanisms of reactions
energy transfers

9. Alchemy Forerunner of chemistry Mystical- search for perfection
Practical- developed glassware and techniques used today
Tried to change elements
Faulty assumptions and lack of logic led them astray

10. Chemistry is A natural science A language with its own vocabulary
A way of thinking

11. Scientific Method A way of solving problems or answering questions
Starts with observation- noting and recording facts
Hypothesis- an educated guess as to the cause of the problem or answer to the question

12. Scientific Method Experiment- designed to test the hypothesis
Only two possible answers
1) hypothesis is right
2) hypothesis is wrong
Generates data observations from experiments
Modify hypothesis- repeat the cycle

13. Variables
Controlled experiment- Only want one thing to change at a time in a laboratory.
Manipulated variable- What you change or control directly
Also called independent variable
Responding variable – What changes as a result. No direct control
Also called dependent variable

14. Law Modify Observations Theory (Model) Hypothesis Experiment
Prediction
Modify
Experiment
Law
Experiment

15. Observations Hypothesis Experiment Cycle repeats many times.
The hypothesis gets more and more certain.
Becomes a theory
A thoroughly tested model that explains why things behave a certain way.
Observations
Hypothesis
Experiment

16. Theory can never be proven.
Useful because they predict behavior
Help us form mental pictures of processes (models)
Observations
Hypothesis
Experiment

17. Another outcome is that certain behavior is repeated many times
Scientific Law is developed
Description of how things behave
Law - how
Theory- why
Observations
Hypothesis
Experiment

18. Law Modify Observations Theory (Model) Hypothesis Experiment
Prediction
Modify
Experiment
Experiment
Law

19. Law vs. Theory
Theory can’t be proved; always the possibility that a new experiment will disprove a theory
Law described a natural phenomenon, but does not attempt to explain it

20. Communication Use Journals Describe procedures, methods, and findings
Do research
Write article
Describe procedures, methods, and findings
Submit for peer review
Sent back for editing
Publish
Letters to editor respond.

21. Frame of Reference What is it?
Physics Definition- system of objects that are not moving with respect to one another
Dictionary Definition- set of ideas, facts, or circumstances within which something exists.
What does Frame of Reference mean to the world of Chemistry?

22. What is Matter? Matter is anything that takes up space and has mass
Mass is the amount of matter in an object
Mass is resistance to change in motion along a smooth and level surface

23. Types of Matter Substance- a particular kind of matter – pure
Mixture- more than one kind of matter

24. Properties Words that describe matter (adjectives)
Physical Properties- a quality or condition of a substance that can be observed or measured without changing the substance’s composition
Chemical Properties- a property that can be observed by changing the type of substance

25. Examples of Physical Properties
1) Color
2) Solubility
3) Odor
4) Hardness
5) Density
6) Melting Point
7) Boiling Point
8) Size
9) Shape

26. States of Matter Solid- matter that has a definite shape and volume
Liquid- matter that flows and has a fixed volume
Gas- matter that takes up both the shape and volume of a container
Vapor- a substance that is currently a gas but normally is a liquid or solid at room temperature.
Plasma- matter consisting of a gaseous mixture of electrons and positive ions. Not found on Earth

27. Matter Chart Properties: Solid Liquid Gas or Vapor Mass Definite Shape
Rigid
Indefinite
Volume
Temp. Increase
Small Expansion
Moderate Expansion
Large Expansion
Com-
Pressible? No
Yes

28. States of Matter Definite Volume? Definite Shape? Temp. increase
Com-pressible?
Small Expans.
Solid
YES
YES NO
Small Expans.
Liquid NO NO
YES
Large Expans.
Gas NO NO
YES

29. Condense
Freeze
Melt
Evaporate
Solid
Liquid
Gas

31. Physical Changes
Physical Change- alters a substance without changing its composition
Key Terms:
Boil
Freeze
Dissolve
Melt
Condense
Break
Split
Crack
Crush
Cutting

32. Mixtures Mixture- Physical blend of two or more substances
Mixture has variable composition
Two Types of Mixtures
Heterogeneous- not uniform in composition
Homogeneous- completely uniform in compostion

33. Example Heterogeneous Blood Chocolate Chip Cookie Soil Mixed Salad
Homogeneous
Air
Brass
Black Coffee
Motor Oil
Water

34. Solutions Homogeneous Mixture Mixed molecule by molecule
Example: Sugar in Water (same composition as any other portion)
Can occur between any state of matter

35. Common Solutions Gas in Gas- O2 in N (air) Liquid in Gas- Water Vapor
Gas in Liquid- CO2 in Water (soda water)
Liquid in Liquid- Acetic Acid in Water (vinegar)
Solid in Liquid- Kool Aid
Solid in Solid- Copper in Silver (sterling silver)

36. Solutions
Like all mixtures, they keep the properties of the components
Can by separated by physical means
Not easily separated- can be separated

38. The Metric System

39. Measuring The numbers are only half of a measurement. It is 10 long.
10 what?
Numbers without units are meaningless.
How many feet in a yard?
A mile?
A rod?

40. The Metric System Easier to use because it is a decimal system.
Every conversion is by some power of 10.
A metric unit has two parts.
A prefix and a base unit.
prefix tells you how many times to divide or multiply by 10.

41. Base Units Length - meter - more than a yard - m
Mass - grams - about a raisin - g
Time - second - s
Temperature - Kelvin or ºCelsius K or ºC
Energy - Joules- J
Volume - Liter - half of a two liter bottle- L
Amount of substance - mole - mol

42. Prefixes kilo k 1000 times deci d 1/10 centi c 1/100 milli m 1/1000
kilometer - about 0.6 miles
centimeter - less than half an inch
millimeter - the width of a paper clip wire

43. Volume calculated by multiplying L x W x H
Liter the volume of a cube 1 dm (10 cm) on a side
1L = 1 dm3
so 1 L = 10 cm x 10 cm x 10 cm
1 L = 1000 cm3
1/1000 L = 1 cm3
1 mL = 1 cm3

44. Volume 1 L about 1/4 of a gallon - a quart
1 mL is about 20 drops of water or 1 sugar cube

45. Mass Weight is a force. Mass is the amount of matter.
1 gram is defined as the mass of 1 cm3 of water at 4 ºC.
1000 g = 1000 cm3 of water
1 kg = 1 L of water

46. Mass
1 kg = 2.5 lbs
1 g = 1 paper clip
1 mg = 10 grains of salt

47. Converting k h D d c m
how far you have to move on this chart, tells you how far, and which direction to move the decimal place.
The box is the base unit, meters, Liters, grams, etc.

48. k h D d c m Conversions convert 25 mg to grams convert 0.45 km to mm
convert 35 mL to liters
It works because the math works, we are dividing or multiplying by 10 the correct number of times.

49. Which is heavier?
it depends

50. Density How heavy something is for its size.
The ratio of mass to volume for a substance.
D = M / V
Independent of how much of it you have
gold - high density
air low density.

51. Calculating The formula tells you how. Units will be g/mL or g/cm3
A piece of wood has a mass of 11.2 g and a volume of 23 mL what is the density?
A piece of wood has a density of 0.93 g/mL and a volume of 23 mL what is the mass?

52. Floating Lower density floats on higher density.
Ice is less dense than water.
Most wood is less dense than water.
Helium is less dense than air.
A ship is less dense than water.

53. Density of water 1 g of water is 1 mL of water.
density of water is 1 g/mL
at 4ºC
otherwise it is less

54. Measuring Temperature
0ºC
Measuring Temperature
Celsius scale.
water freezes at 0ºC
water boils at 100ºC
body temperature 37ºC
room temperature ºC

55. Measuring Temperature
273 K
Measuring Temperature
Kelvin starts at absolute zero (-273 º C)
degrees are the same size
C = K -273
K = C + 273
Kelvin is always bigger.
Kelvin can never be negative.

56. Temperature is different
from heat.
Temperature is which way heat will flow. (from hot to cold)
Heat is energy, ability to do work.
A drop of boiling water hurts,
kilogram of boiling water kills.

57. Units of heat are calories or Joules
1 calorie is the amount of heat needed to raise the temperature of 1 gram of water by 1ºC.
A food Calorie is really a kilocalorie.
How much energy is absorbed to heat 15 grams of water by 25ºC.
1 calorie = 4.18 J

58. Elements & Compounds Element- simplest form of matter
Elements can’t be separated
Elements are the building block
Smallest part is an atom

59. Compounds Compound- formed by 2 or more elements
Substances that can be separated into simpler substances only by chemical reactions
When broken down, the pieces have completely different properties than the compound
Pure substances
Represented by a formula
Smallest part is a molecule

60. Compound or Mixture Compound Mixture One kind of piece- Molecules
More than one kind -
Molecule or atoms
Making is a
chemical change
physical change
Only one kind
Variable composition

61. What is it? Element, Compound or Mixture Silver Orange Juice Ice Tea
Potassium Chloride
Oxygen
Air
Pine Tree

62. Which is it?
Compound
Mixture
Element

63. Chemical Reactions
One or more substances changing into a new substance
Starting Substance- Reactant
New Substance- Product
Iron + Sulfur  Iron Sulfide

64. How do you know? 6 Ways to Tell Color Change
Energy absorbed or released (temp change)
Gas or Solid Produced
Odor
Precipitate (ppt)- solid that separates from solution
Not easily reversed

65. Conservation of Mass
Law of Conservation of Mass- in a physical or chemical reaction, mass is neither created nor destroyed; it is conserved.
All mass can be accounted for.
Mass of the Reactants = Mass of Products

66. Energy The ability to do work.
Work - cause a change or move an object.
Many types- all can be changed into the other.

67. Types of energy Potential- stored energy
Kinetic Energy- energy something has because its moving
Heat- the energy that moves because of a temperature difference.
Chemical energy- energy released or absorbed in a chemical change.
Electrical energy - energy of moving charges

68. Types of Energy
Radiant Energy- energy that can travel through empty space (light, UV, infrared, radio)
All types of energy can be converted into others.
If you trace the source far enough back, you will end up at nuclear energy.

69. Conservation of Energy
Energy can be neither created or destroyed in ordinary changes (not nuclear), it can only change form.
Its not just a good idea, its the law.