General Chemistry_PPT#1_Chapters 0+1

1. Welcome to General
Chemistry 151!!
Instructor: Dr. Lauren Benz
ST-378

2. Chem 151 / Chem 151L
1. This course is intended for science majors/engineering
majors/pre-health students, not a GE.
2. Lecture and lab are co-requisites.
• If you are not enrolled in both lecture &lab (and if you have not previously If you
are not enrolled in both lecture &lab (and if you have not previously passed one
or the other), you will be dropped from 151/151L after add/drop deadline has
passed.
3. If you are able to register for a spot in lab, you may then
add Chem 151, but you cannot register for Chem 151
without being enrolled in a Chem 151L lab.
• Please contact Mrs. Finocchio. Provide name, email, phone, and CRNs of
151/151L sections you are trying to get.
If you have questions, contact Mrs. Finocchio in SCST 381/ debbief@sandiego.edu.

3. Chem 151 / Chem 151L
Chem 151L lab announcements:
 No G Chem lab this week.
 Watch for an email from your lab instructor
regarding your first day of lab and what to
bring.
 The class requires lab spectacles and model
kits, which the Chem Club is selling (see
schedules posted). Cash or check only.

4. Textbook and MasteringChemistry
Bookstore:
• New customized textbook with MasteringChemistry access code (with 4
year access) packaged together = $175.95.
• “customized” = any chapter we don’t use has been removed to help
lower cost of book.
• Located at front end of left aisle. Ask if you cannot find it!
www.masteringchemistry.com:
• Can purchase MasteringChemistry access code directly, with or without
e-text.
• With e-text = $110.00
• Without e-text = $66.00
• Do this option if you have a textbook but don’t have MasteringChemistry
yet, or if you don’t want to purchase a printed book and just want the e-
text.
• This MasteringChem will have the standard 24 months access.
Other sources:
Non-customized version of textbook (various prices) – the book will have
the same page numbers, etc, just a few extra chapters we don't use.

5. Emergency Preparedness
Evacuation Procedure for SCST 133
Primary exit: Via the exits on the first floor: turn left when exiting the room
and walk out the exit at the end of the hall. DO NOT go up the central
staircase! We will meet in front of La Paloma. Wait there for further
instructions (please do not wander off).
DO NOT stand in the street outside the building - the street must remain clear
for emergency vehicles.

6. Expectations for Chem 151:
1. Attend all lectures
- Be on time, and please sit in the back if you must
leave early
- Be courteous to me and others (no texting, no cell
phones, no unauthorized work on computers,
tablets, etc.)
2. Keep up with the reading & work
recommended problems (+ more, time
commitment = 2-3 hours per lecture)
3. Ask questions
4. Prepare for tests—rework problems, work
additional problems and practice exams

7. Support
1. Office hours: 5 hours/week + by
appointment
2. Outside support: chem club
tutoring, math center
3. I will help pace the workload,
and give additional practice
before exams
4. I will try to make it interesting!!!

8. Chemistry: the study of matter
• Nuclear chemistry (fusion, fission)
• Organic chemistry (pharmaceutical
industry, chemical synthesis)
• Analytical chemistry (uses
instrumentation to study various
problems—air & water pollution)
• Biochemistry (biotech companies)
• Inorganic chemistry (materials, catalysis,
etc.)
• Physical chemistry (spectroscopy,
microscopy, etc.)
• Computational chemistry (for those who
don’t like touching chemicals! Make
predictions from theory..)
• Other: science writing (Scientific
American, etc.), patent law, policy,
medical school
Combinations of these
“Interdisciplinary”

9. In order to do controlled experiments in
chemistry (or any science really) we
need to quantify!

10. Multiples of SI units:
1 TW = 1 terawatt
(the power of a
lightening strike)
15 TW = the annual
energy consumption
of the world
Deciliter- in Europe!
3 dL ≈ 12 fl. oz
100 µm = 1 human
hair
0.2 nm ≈ space
between Au atoms
(in solid form)
To read this chart:
“There are 1012 grams in a teragram, 10-12 seconds in a picosecond” and so on.

11. Need to remember:
• 1012 Watts in one TW
• 109 Watts in one GW
• 106 Watts in one MW
• 103 Watts in one kW
• 10 deciliters in 1 L
• 100 centimeters in a
meter
• 1000 millimeters in a
meter
• 106 micrometers in a
meter
• 109 nanometers in a
meter
• 1012 picoseconds in a
second
• 1015 femtoseconds in a
second
Larger units: Smaller units:
1.21
Gigawatts!!

12. Some definitions…
• Mass: the amount of matter in an object.
**Not to be confused with “weight” which
measures the force with which gravity
pulls on an object
• Temperature: a measurement of the
kinetic energy of molecular motion (more
detail to come in Ch. 8)

13. Temperature conversions
What is larger: one degree C or one degree F? one degree C or one K?

14. Temperature conversion formulas
• To convert from °C → °F
°F = (9°F /5°C ) x °C + 32°F
• To convert from °F → °C
°C = (5°C /9°F) x (°F - 32°F)
• To convert from °C → K
K = °C + 273
• To convert from °F → K
– First convert to °C, then to K
Remember “PEMDAS”:
(order of operations)
1. Parentheses
2. Exponents
3. Multiplication/division
4. Addition/subtraction
(variables are in red)

15. Derived units
• Unlike the fundamental units (like mass
and temperature), derived units involve a
combination of more than one
fundamental units
– Examples: area (m2), volume (m3), density
(kg/m2), acceleration (m/s2), force (kgm/s2 or
“Newton”), energy (kgm2/s2 or “Joule, J” )

16. Density of some common items
DEMO: CO2 (25°C) = 0.001801 g/cc3????????
Density = mass/volume
Note: 1 cm3 is a cubic centimeter, sometimes called “cc” and is equal to 1 mL

17. Energy
• Kinetic Energy: energy of a moving object
KE = (1/2)mv2 ; m = mass and v = velocity
units: kg m2/s2 = 1 Joule
• Potential Energy: stored energy (can have
many forms, can be due to an object’s
height or can be in the form of chemical
energy)

18. Significant Figures + Rounding
• See rules in Ch. 0
• Refer to class handouts
• When reading glassware…estimate out to
one extra place!!
1mL
5mL
3.3 mL

19. Scientific Notation
Definition: Method of simplifying the writing
of very large and very small quantities
How to express: Find the number, which
when multiplied by 10x, will give you the
number written in the "normal" style
(Examples on board)

20. Conversions
(dimensional analysis)
1. Write down the number that you want to covert
2. Write down your conversion factor(s) to the right of
the number—make sure that you place your units
so that they will cancel
3. Cancel units and multiply or divide (your remaining
unit should be the one that you are converting to)
4. Double check whether or not the answer is
reasonable.
** Note: if your conversion involves a derived unit such as meters squared (m2), you
must also raise the conversion factor to the power of the unit (in this case 2)

21. Example
• A human hair is approximately 100 µm in
diameter. Convert this into meters.
• A football field is 48,000 ft2. How many
square meters is that?

22. Conversions (cont’d)
• Another unit of energy is the calorie:
– 1 calorie = 4.184 J
– 1 Calorie = 1000 calories (note the upper and
lower case distinction—”Calories” are what
are listed on food packaging)
Please make note of these two conversions
for the group exercises..

23. The Mole!!
• The mole is actually a measure of a number
of things (abbreviated “mol”)
• In the same way that a “dozen” contains 12
things, a mole contains 6.022 x 1023 things
• Definition: 12 grams of C (in it’s most
common form, 12C) contains 6.022 x 1023
atoms
• The #s below the elemental symbols on the
periodic table give an elements “molar
mass”, the mass of 1 mole of the pure
element (can be read as “## grams/mole)

25. Unified atomic mass unit
“(u) or (amu)”
• Another way to read the numbers on the
periodic table
1 amu =
𝑀𝑎𝑠𝑠 𝑜𝑓 𝑜𝑛𝑒 𝑐𝑎𝑟𝑏𝑜𝑛 𝑎𝑡𝑜𝑚 (𝑚𝑜𝑠𝑡 𝑐𝑜𝑚𝑚𝑜𝑛 𝑓𝑜𝑟𝑚)
12
= 1.66  10-24 g
Mo
molybdenum
42
95.94

26. Calculations involving the mole
• A small silicon chip used in a
microcomputer has a mass of 5.68 mg.
– How many moles of Si (atoms) is this?
– How many Si atoms are present in this chip

27. Accuracy & Precision
• both are considered to be general
measurements of uncertainty
• Accuracy: refers to how close to the true
value a given measurement is
• Precision: refers to how well a number of
independent measurements agree with
one another

28. Which one is more precise?
Better accuracy Better precision

29. The Periodic Table
• To the left of the red line: mostly metals (shiny, conductors of electricity & heat)
• To the right of the red line: mostly non-metals (most are gases, solids are brittle)
• Exceptions: circled in blue, “semi-metals” (B, Si, As, Te, At, Ge, Sb—all solids)
http://www.nist.gov/pml/data/periodic.cfm

30. A Brief History
• Prior to 1000 BC: metals were extracted from ores
to form ornaments & weapons, embalming fluids

31. A Brief History
• Prior to 1000 BC: metals were extracted from ores
to form ornaments & weapons, embalming fluids
• 400 BC » Greeks proposed “fire, earth, water, air”
» Democritus believed in “atomos”-indivisible
particles
• Next 2000 years: alchemy, however mercury (Hg),
sulfur (S) and antimony (Sb) were discovered
• Mid 1700s: Joseph Priestly discovered oxygen
• 1829: Johann Doebereiner put together “triads” of
similarly behaving elements
• 1860: Dimitri Mendeleev arranged the elements by
mass and grouped similar elements together—realized
that some were missing, undiscovered

32. Chemistry is relatively young!
“Chemical Geneology”
1.Lauren Benz, Ph.D., 2007
2.Cynthia Friend, Ph.D., 1981
3.Earl Muetterties, Pd.D., 1952
4.Eugene Rochow, Ph.D., 1935
5.Luis Monroe Dennis, B.S., 1886
6.Walther Matthias Hempel, Ph.D., 1873
7.R.W.H. Bunsen, Ph.D., 1830
…keeps going back to 1640

33. from left to right
rows are
called “periods”
going up and down
the columns are called
“groups”
The Periodic Table
Elements in the same group typically
have similar properties.
Main groups
(green-shaded)
Transition metal groups
(yellow-shaded)
http://periodictable.com/Elements/Source-harvardMuseum/index.html

34. The Periodic Table:
main group elements (1A-8A)
Group 1A: “Alkali Metals”: REACTIVE!! all react with water to form basic (or
alkaline) solutions. Soft, silvery
You can visualize this by adding an “indicator” which turns pink when the
solution becomes basic. Ex. Li, Na, K, Rb, Cs, Fr

35. Group 2A: “Alkaline Metals”: less reactive than 1A metals but also reactive.
Also shiny. Ex. Be, Mg, Ca, Sr, Ba, Ra
The Periodic Table:
main group elements (1A-8A)

36. http://www.youtube.com/watch?v=qSr39UwpELo
A Magnesium (Mg) strip burning:

37. The Periodic Table:
main group elements (1A-8A)
Group 7A: “Halogens”: colorful, corrosive nonmetals. Ex. F, Cl, Br, I
(in demo—blue color is from a complex of iodine)

38. The Periodic Table:
main group elements (1A-8A)
Group 8A: “Noble Gases”: all colorless and inert.
Ex. He, Ne, Ar, Kr, Xe

39. Chemical property: characteristic that involves
a change in chemical make up
(1) demo ? (reaction involving color change)
(2) demo ? Potassium (K) reaction with water
Physical property: characteristic that does not
involve a change in chemical make-up (boiling
point, melting point, density)
Demonstration: liquid nitrogen
Boiling point (°C)? - 196°C!!!