1. Introduction to Chemistry
Health and Medicine
Sanitation systems
Surgery with anesthesia
Vaccines and antibiotics
Gene therapy
Energy and the Environment
Fossil fuels
Solar energy
Nuclear energy

2. Introduction to Chemistry
Materials and Technology
Polymers, ceramics, liquid crystals
Room-temperature superconductors?
Molecular computing?
Food and Agriculture
Genetically modified crops
“Natural” pesticides
Specialized fertilizers

3. Introduction to Chemistry
Macroscopic
Microscopic

4. Introduction to Chemistry
Chemistry is the study of matter and the changes it undergoes.
Matter is anything that occupies space and has mass.
A substance is a form of matter that has a definite composition and distinct properties.
liquid nitrogen
gold ingots
silicon crystals

5. Introduction to Chemistry
A mixture is a combination of two or more substances in which the substances retain their distinct identities.
INSPIRING CREATIVE AND INNOVATIVE MINDS

6. Introduction to Chemistry
Homogenous mixture – composition of the mixture is the same throughout
soft drink, milk, solder
Heterogeneous mixture – composition is not uniform throughout
cement,
iron filings in sand
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7. Introduction to Chemistry
Physical means can be used to separate a mixture into its pure components.
distillation
magnet
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8. Introduction to Chemistry
An element is a substance that cannot be separated into simpler substances by chemical means.
114 elements have been identified
82 elements occur naturally on Earth
gold, aluminum, lead, oxygen, carbon, sulfur
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9. Introduction to Chemistry
INSPIRING CREATIVE AND INNOVATIVE MINDS

10. Introduction to Chemistry
A compound is a substance composed of atoms of two or more elements chemically united in fixed proportions.
Compounds can only be separated into their pure components (elements) by chemical means.
lithium fluoride
quartz
dry ice – carbon dioxide
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11. Introduction to Chemistry.
INSPIRING CREATIVE AND INNOVATIVE MINDS

12. Matter is made up of very tiny discrete particles
Particle Theory of Matter :
Matter is made up of very tiny discrete particles

13. Introduction to Chemistry
A Comparison: The Three States of Matter
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16. Introduction to Chemistry
The Three States of Matter: Effect of a Hot Poker on a Block of Ice
solid
liquid
gas
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17. Introduction to Chemistry
Types of Changes
A physical change does not alter the composition or identity of a substance.
ice melting
sugar dissolving
in water
A chemical change alters the composition or identity of the substance(s) involved.
hydrogen burns in air to form water
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18. The Properties of Chemical Substance
Physical properties are those that can be observed without changing the identity of the substance.
examples : color, density,mass, boiling point
Chemical properties are properties that describe how a substance changes into a completely different substance.
examples : flammability and corrosion/oxidation resistance .

19. Extensive and Intensive Properties
An extensive property of a material depends
upon how much matter is being considered.
mass
length
volume
An intensive property of a material does not depend upon how much matter is being considered.
density
temperature
color

20. Measurement in Chemistry

21. Measurement in Chemistry

22. Matter - anything that occupies space and has mass
mass – measure of the quantity of matter
SI unit of mass is the kilogram (kg)
1 kg = 1000 g = 1 x 103 g
weight – force that gravity exerts on an object
weight = c x mass
on earth, c = 1.0
on moon, c ~ 0.1
A 1 kg bar will weigh
1 kg on earth
0.1 kg on moon

23. A Comparison of Temperature Scales
Measurement in Chemistry
A Comparison of Temperature Scales
K = 0C
K = 0 0C
K = 100 0C
0F = x 0C + 32 9 5
32 0F = 0 0C
212 0F = 100 0C

24. EXAMPLES
A person has fever of 102.5F. What is this temperature in C?
(2) The temperature of the hottest place in California is 134F. What is this temperature reading in C? in kelvins?

25. Volume – SI derived unit for volume is cubic meter (m3)
Measurement in Chemistry
Volume – SI derived unit for volume is
cubic meter (m3)
1 cm3 = (1 x 10-2 m)3 = 1 x 10-6 m3
1 L = 1000 mL = 1000 cm3 = 1 dm3
1 dm3 = (1 x 10-1 m)3 = 1 x 10-3 m3
1 mL = 1 cm3

26. Density – SI derived unit for density is kg/m3
Measurement in Chemistry
Density – SI derived unit for density is kg/m3
1 g/cm3 = 1 g/mL = 1000 kg/m3
Measurement in Chemistry
density =
mass
volume
d = m V

27. Measurement in Chemistry

28. Gold is a precious metal that is chemically unreactive.
Measurement in Chemistry
Gold is a precious metal that is chemically unreactive.
It is used mainly in jewelery, dentistry, and electronic devices.
A piece of gold ingot with a mass of 301 g has a volume of
15.6 cm3. Calculate the density of gold.

29. Measurement in Chemistry
Solution We are given the mass and volume and asked to calculate the density. Therefore, from Equation (1.1), we write

30. Measurement in Chemistry
The density of mercury, the only metal that is a liquid at room temperature, is 13.6 g/mL. Calculate the mass of 5.50 mL of the liquid.

31. We rearrange Equation (1.1) to give
Measurement in Chemistry
Solution We are given the density and volume of a liquid and asked to calculate the mass of the liquid.
We rearrange Equation (1.1) to give

32. Exercise: Density
A piece of quartz mineral was added into a graduated cylinder containing 51.2mL water. After adding a quartz, the water level was 65.7mL. The quartz piece weighed 38.4g. What was the density of the quartz

33. Dimensional Analysis Method of Solving Problems
Measurement in Chemistry
Dimensional Analysis Method of Solving Problems
Determine which unit conversion factor(s) are needed
Carry units through calculation
If all units cancel except for the desired unit(s), then the problem was solved correctly.
given quantity x conversion factor = desired quantity
given unit x
= desired unit
desired unit
given unit

34. Measurement in Chemistry
A person’s average daily intake of glucose (a form of sugar) is pound (lb). What is this mass in milligrams (mg)?
(1 lb = g.)

35. Measurement in Chemistry
Strategy The problem can be stated as
? mg = lb
The relationship between pounds and grams is given in the problem. This relationship will enable conversion from pounds to grams.
A metric conversion is then needed to convert grams to milligrams (1 mg = 1 × 10−3 g).
Arrange the appropriate conversion factors so that pounds and grams cancel and the unit milligrams is obtained in your answer.

36. Measurement in Chemistry
The sequence of conversions is
Using the following conversion factors
we obtain the answer in one step:

37. Measurement in Chemistry
An average adult has 5.2 L of blood. What is the volume of blood in m3?

38. Measurement in Chemistry
Strategy
The problem can be stated as
? m3 = 5.2 L
How many conversion factors are needed for this problem?
Recall that 1 L = 1000 cm3 and 1 cm = 1 × 10−2 m.

39. Measurement in Chemistry
Solution We need two conversion factors here: one to convert liters to cm3 and one to convert centimeters to meters:
Because the second conversion factor deals with length (cm and m) and we want volume here, it must therefore be cubed to give
This means that 1 cm3 = 1 × 10−6 m3.

40. Measurement in Chemistry
Now we can write
Check From the preceding conversion factors you can show that 1 L = 1 × 10−3 m3. Therefore, 5 L of blood would be equal to 5 × 10−3 m3, which is close to the answer.

41. Measurement in Chemistry
Liquid nitrogen is obtained from liquefied air and is used to prepare frozen goods and in low-temperature research.
The density of the liquid at its boiling point (−196°C or 77 K) is g/cm3. Convert the density to units of kg/m3.
liquid nitrogen

42. Measurement in Chemistry
Strategy The problem can be stated as
? kg/m3 = g/cm3
Two separate conversions are required for this problem:
Recall that 1 kg = 1000 g and 1 cm = 1 × 10−2 m.

43. Solution we saw that 1 cm3 = 1 ×10−6 m3. The conversion factors are
Finally
Check Because 1 m3 = 1 × 106 cm3, we would expect much more mass in 1 m3 than in 1 cm3. Therefore, the answer is reasonable.