1. Why should You learn Chemistry?
Required
Pharmacists
Doctors
Dentists
Chem Engineer, etc.
Need it to pass Standardized Exams, Boards, etc.
MCAT
PCAT
DAT
OAT, etc
Understanding of Nature
Drug Design: Manipulate molecules for better medicine
Better utilize Energy: Manipulate molecules for better fuels
Better understand Life: Biochemistry/Molecular Biology
Create better technology

2. Outline of presentation
What is Chemistry?
Analytical Chemistry
What is in a sample?
How much is present?
Biochemistry- study of life’s chemistry
Inorganic Chemistry- all other elements except carbon
Separation Science
Organic chemistry- study of carbon compounds
Physical Chemistry- study of chemical events based on natural physical phenomenom

3. Organic Chemistry is the study of compounds that consist of carbon atoms

4. What is so special about Carbon?
Interesting facts:
46 million chemical compounds are known in nature.
99% of them contain carbon (thus organic)
Why??

5. Biochemistry “What are the unique chemical foundations of all life and what is different”

6. Why should you Learn Biological Chemistry: Drug Design
What knowledge is required for drug design?
Know structures of protein targets in the body
Biochemistry
Molecular Biology
Know how to manipulate organic molecules to create new compounds with specific properties
Organic chemistry
Chemical Synthesis
Sildenafil

7. Analytical Chemistry: Science of Chemical Analysis

8. Careers in Chemistry Chemist/Biochemist Chemical Engineer
Industrial Chemist
Chemical Technician
B.S. (4yr), M.S. (6-7yr), Ph.D. (8-12 yr)

9. Matter and MeasurementBy
Doba D. Jackson, Ph.D.
Associate Professor of Chemistry
& Biochemistry
Huntingdon College

10. Matter and Measurement Learning outcomes
Describe the different elements and states of matter and their general physical properties
Distinguish between different classes of matter.
Distinguish between Physical processes and chemical processes
Distinguish between exact and uncertainty in numbers, also to express numbers with proper significant figures.

11. Chemistry and the Elements

12. The arrangement of the periodic table allows for many properties to be determined by looking at an element’s location.

13. Elements and the Periodic Table
Main Groups
columns 1A – 2A (2 groups)
columns 3A – 8A (6 groups)
Transition Metals:
3B–2B
(8 groups, 10 columns)
Inner Transition Metals: 14 groups; 3B - 4B
lanthanides
actinides

14. Some Chemical Properties of the Elements
Property: Any characteristic that can be used to describe or identify matter.
Intensive Properties: Do not depend on sample size.
temperature
melting point
Extensive Properties: Do depend on sample size.
length
volume

15. Properties of the Elements
Physical Properties: Characteristics that do not involve a change in a sample’s chemical makeup.
Chemical Properties: Characteristics that do involve a change in a sample’s chemical makeup.
Chemical properties and chemical changes are often considered to be synonymous.

16. Some Chemical Properties of Alkali Metals

17. Some Chemical Properties of Alkaline Earth Metals

18. Some Chemical Properties of the Halogens

19. Some Chemical Properties of the Noble Gases

20. Some Chemical Properties of the Elements
Nonmetals
Metals

21. Some Chemical Properties of the Semimetals (Metaloids)
Semimetals are also known as metalloids.
Semiconductors and semimetals are not synonymous.

22. Experimentation and Measurement
The U.S. is officially on the metric system, but it’s voluntary.
All other units are derived from these fundamental units.

24. Mass and its Measurement
Mass: Amount of matter in an object.
Matter: Describes anything with a physical presence—anything you can touch, taste, or smell.
Weight: Measures the force with which gravity pulls on an object.

25. Mass and Its Measurement

26. Accuracy and Precision
Chapter 1: Atoms: Matter and Measurement
6/10/2018
Accuracy and Precision
Accuracy: How close to the true value a given measurement is.
Percent error
Average
Precision: How well a number of independent measurements agree with each other.
Standard Deviation
Least squares fit analysis
Copyright © 2010 Pearson Prentice Hall, Inc.

27. Accuracy and Precision
Chapter 1: Atoms: Matter and Measurement
6/10/2018
Accuracy and Precision
Mass of a Tennis Ball
Measurement #
Bathroom Scale
Lab
Balance
Analytical Balance 1
0.0 kg
54.4 g g 2
54.5 g g 3
0.1 kg
54.3 g
(average)
(0.03 kg)
(54.4 g)
( g)
The bathroom scale is not something one would want to use for scientific measurements!
It is possible to have good precision and poor accuracy. An instrument improperly calibrated, for example.
Poor Accuracy
Poor Precision
Copyright © 2010 Pearson Prentice Hall, Inc.

28. Accuracy and Precision
Chapter 1: Atoms: Matter and Measurement
6/10/2018
Accuracy and Precision
Mass of a Tennis Ball
Measurement #
Bathroom Scale
Lab
Balance
Analytical Balance 1
0.0 kg
54.4 g g 2
54.5 g g 3
0.1 kg
54.3 g
(average)
(0.03 kg)
(54.4 g)
( g)
The data varies in the first decimal place. While the accuracy is reasonable compared to the analytical balance, the precision is not.
Good Accuracy
Poor Precision
Copyright © 2010 Pearson Prentice Hall, Inc.

29. Accuracy and Precision
Chapter 1: Atoms: Matter and Measurement
6/10/2018
Accuracy and Precision
Mass of a Tennis Ball
Measurement #
Bathroom Scale
Lab
Balance
Analytical Balance 1
0.0 kg
54.4 g g 2
54.5 g g 3
0.1 kg
54.3 g
(average)
(0.03 kg)
(54.4 g)
( g)
The assumption is that the analytical balance is properly calibrated.
The data only varies in the fourth decimal place.
Good Accuracy
Good Precision
Copyright © 2010 Pearson Prentice Hall, Inc.

30. Chapter 1: Atoms: Matter and Measurement
Significant Figures
6/10/2018
Rules for counting significant figures:
Zeros in the middle of a number are like any other digit; they are always significant.
Zeros at the beginning of a number are not significant; they act only to locate the decimal point.
Zeros at the end of a number and after the decimal point are always significant.
Zeros at the end of a number and after the decimal point may or may not be significant.
4.803 cm 4 SF
g 3 SF (or 6.61 x 10-3 g)
Use scientific notation in these cases when reporting the results of calculations.
K 5 SF
34,200 m 5 SF
Copyright © 2010 Pearson Prentice Hall, Inc.

31. Chapter 1: Atoms: Matter and Measurement
6/10/2018
Rounding Numbers
Math rules for keeping track of significant figures:
Multiplication or division: The answer can’t have more significant figures than any of the original numbers.
3 SF
11.70 gal
278 mi
= 23.8 mi/gal (mpg)
4 SF
These rules are approximations that work well. A proper analysis would be a more detailed look at error analysis and is often done in a first quarter physical chemistry class for chemistry majors (or something similar).
3 SF
Copyright © 2010 Pearson Prentice Hall, Inc.

32. Chapter 1: Atoms: Matter and Measurement
6/10/2018
Rounding Numbers
Math rules for keeping track of significant figures:
Multiplication or division: The answer can’t have more significant figures than any of the original numbers.
Addition or subtraction: The answer can’t have more digits to the right of the decimal point than any of the original numbers.
2 decimal places
5 decimal places
3.18
3.19
Copyright © 2010 Pearson Prentice Hall, Inc.

33. Dimensional analysis: converting units from one to another
Chapter 1: Atoms: Matter and Measurement
6/10/2018
Dimensional analysis: converting units from one to another
69.5 in
39.37 in
1 m x
= 1.77 m
starting quantity
equivalent quantity
A detriment of dimensional analysis is that it’s possible to get the correct answer without a solid understanding of what one is doing. This can be mitigated by doing a conceptual check or determining a “ballpark” solution and comparing it to the answer calculated using dimensional analysis.
conversion factor
Copyright © 2010 Pearson Prentice Hall, Inc.

34. Accuracy, Precision, and Significant Figures
Significant figures: The total number of digits recorded in a measured or calculated quantity. They come from uncertainty in any measurement.
Generally the last digit in a reported measurement is uncertain (estimated).
Exact numbers and relationships (7 days in a week, 30 students in a class, etc.) effectively have an infinite number of significant figures.

35. Accuracy, Precision, and Significant Figures1 2 4 3 cm
1.7 cm < length < 1.8 cm
length = 1.74 cm

36. Accuracy, Precision, and Significant Figures
Rules for counting significant figures (left-to-right):
Zeros in the middle of a number are like any other digit; they are always significant.
4.803 cm 4 SF

37. Accuracy, Precision, and Significant Figures
Rules for counting significant figures (left-to-right):
Zeros in the middle of a number are like any other digit; they are always significant.
Zeros at the beginning of a number are not significant; they act only to locate the decimal point.
g 3 SF (or 6.61 x 10-3 g)

38. Accuracy, Precision, and Significant Figures
Rules for counting significant figures (left-to-right):
Zeros in the middle of a number are like any other digit; they are always significant.
Zeros at the beginning of a number are not significant; they act only to locate the decimal point.
Zeros at the end of a number and after the decimal point are always significant.
K 5 SF

39. Accuracy, Precision, and Significant Figures
Rules for counting significant figures (left-to-right):
Zeros in the middle of a number are like any other digit; they are always significant.
Zeros at the beginning of a number are not significant; they act only to locate the decimal point.
Zeros at the end of a number and after the decimal point are always significant.
Zeros at the end of a number and after the decimal point may or may not be significant.
Use scientific notation in these cases when reporting the results of calculations.
34,200 m ? SF

40. Rounding Numbers Math rules for keeping track of significant figures:
Multiplication or division: The answer can’t have more significant figures than any of the original numbers.
3 SF
11.70 gal
278 mi
= 23.8 mi/gal (mpg)
4 SF
These rules are approximations that work well. A proper analysis would be a more detailed look at error analysis and is often done in a first quarter physical chemistry class for chemistry majors (or something similar).
3 SF

41. Rounding Numbers Math rules for keeping track of significant figures:
Multiplication or division: The answer can’t have more significant figures than any of the original numbers.
Addition or subtraction: The answer can’t have more digits to the right of the decimal point than any of the original numbers.
2 decimal places
5 decimal places
3.18
3.19

42. Rounding Numbers Rules for rounding off numbers:
If the first digit you remove is less than 5, round down by dropping it and all following digits.
= 5.66

43. Rounding Numbers Rules for rounding off numbers:
If the first digit you remove is less than 5, round down by dropping it and all following digits.
If the first digit you remove is 6 or greater, round up by adding 1 to the digit on the left.
= 5.7

44. Rounding Numbers Rules for rounding off numbers:
If the first digit you remove is less than 5, round down by dropping it and all following digits.
If the first digit you remove is 6 or greater, round up by adding 1 to the digit on the left.
If the first digit you remove is 5 and there are more nonzero digits following, round up.
Books sometimes use different rules for this one.
= 5.665

45. Rounding Numbers Rules for rounding off numbers:
If the first digit you remove is less than 5, round down by dropping it and all following digits.
If the first digit you remove is 6 or greater, round up by adding 1 to the digit on the left.
If the first digit you remove is 5 and there are more nonzero digits following, round up.
If the digit you remove is a 5 with nothing following, round down.
If there were zeros following that last 5, the rule is the same. =

46. Calculations: Converting from One Unit to Another
Dimensional analysis: A method that uses a conversion factor to convert a quantity expressed with one unit to an equivalent quantity with a different unit.
Conversion factor: States the relationship between two different units.
original quantity x conversion factor = equivalent quantity

47. Calculations: Converting from One Unit to Another
Relationship:
1 m = in
39.37 in
1 m
1 m
39.37 in
Conversion factor: or
converts
in to m
converts
m to in

48. Calculations: Converting from One Unit to Another
Incorrect Method
69.5 in
1 m
39.37 in x
= 2740 in2/m
starting quantity ??
A strength of dimensional analysis is that it makes it easy to verify the units of the answer.
conversion factor

49. Calculations: Converting from One Unit to Another
Correct Method
69.5 in
39.37 in
1 m x
= 1.77 m
starting quantity
equivalent quantity
A detriment of dimensional analysis is that it’s possible to get the correct answer without a solid understanding of what one is doing. This can be mitigated by doing a conceptual check or determining a “ballpark” solution and comparing it to the answer calculated using dimensional analysis.
conversion factor