1. What is Chemistry? The study of the composition, structure,
& properties of substances and changes
it undergo.
A chemical is any substance that has a part in a chemical rxn or is produced.
Practical Uses
Clothing – synthetic fabric
Nonstick cookware - Teflon
Pharmaceuticals - medications

2. Categories of Science Concerned with living things Concerned with non
i. Biological –
ii. Physical -
Concerned with non
living things

3. Branches of Chemistry Organic – Study of living - contains carbon.
Inorganic – study of non-living – no carbon.
Physical – study of properties, transformations,
and interrelationship of energy and matter.

4. Branches of Chemistry
Analytical – identification of substances & study of
composition of materials
Biochemistry – Process that occurs in living things
connects biological processes w/ chemical processes.
Theoretical – the use of math & computers to understand
the principles behind observed chemical behavior
and to design and predict the properties of new
compounds.

5. Matter & Its Properties
Atom – the smallest particle of an element that retains the properties of that element.
Elements – A substance that cannot be changed into a simpler substance under normal lab conditions

6. Physical Properties
Properties – characteristics enabling us to distinguish differences in matter.
Physical properties – can be observed or
measured w/o changing the identity of material
Extensive physical properties – depends on the amount of
matter. (mass, length, volume).
Intensive physical properties – does not depend on mass,
melting pt, boiling pt, density, color, ductile,
malleable, crystal shape, etc.

7. Physical Change
A physical change is the changing of a substance does not alter the chemical composition.
It can change states.
Cutting, grinding, expanding

8. States of Matter Neither definite shape or volume
Solid
Liquid
Gas
Plasma
Definite shape & volume
Definite volume, not shape
Neither definite shape or volume
Gaseous system with ions

9. Chemical Properties/Changes
Alters chemical identification.
Chemical reaction-
Reactants -> Products
Reactants are the substances you start off with
And they then react and yields a new product.
Ex. Wood burning, matches, letting milk stand so it
can turn sour, iron rust, tarnishing silver.
Na + Cl  NaCl
Charcoal + O2  CO2
Fe + O2  Fe2O3

10. Physical or Chemical ?
Physical
Chemical

11. Classification of Matter
Mixtures – retain own composition & properties.
Heterogeneous – Not uniform
Homogeneous – Uniform
Pure substance – has a fixed composition. Are either compd. or elements.
Elements – is on the periodic chart. (Simplest form)
compounds – chemically combined ex. NaCl
Every sample has exactly the same characteristic prop.
Every sample has exactly the same composition.
ex. H2O % H, % O

12. Distillation
Method for physically separating a mixture of liquids or a solid dissolved in a liquid

13. Matter & Energy a. Matter – Occupies space and has mass.
Inertia – Resistance to change in motion.
Weight Vs. Mass -
Weight is the measure of gravitational pull.
Mass is quantity of matter.
Law of conservation of mass:
Mass is neither created nor destroyed.

14. Energy – Ability to do work or cause change
Types of Energy -
Kinetic Energy – in the form of motion
Potential Energy – Stored energy
depends on composition or position
Law of Conservation of Energy
Energy can change form, but it cannot be
Created nor destroyed under ordinary cond.

15. Energy and changes in matter
Exothermic – produce heat. Energy is released in the form of heat.
H + O  H2O + Heat
Endothermic – gain heat. Energy,
in a form of heat, is absorbed.
Ex. Melting ice

16. Periodic Table Families or Groups – Vertical columns, # 1 – 18
Periodic Table Families or Groups – Vertical columns, # 1 – Elements share properties.
Periods – horizontal rows
Metals – Good conductors of heat & electricity.
Shiny, luster, malleable, ductile, tensil.
Non-Metals – Poor conductors of heat/electricity.
Metalliods – Share characteristics of metals & nonmetals.
Semiconductors
Noble Gases – unreactive gases.

17. Symbols for elements
IUPAC – International Union of Pure & Applied Chemistry
O – oxygen H –
N - Na -
Sb stibium – antimony
Cu cuprum – copper
Au Aurum – gold
Ag Argentum – silver
Na Natrium – sodium

18. Scientific method- logical approach to solutions of problems
Parts –
Observations – collecting data
Quantitative & Qualitative
Generalizing – Organize, analyze, & classify
Hypothesis – testable statement
Testing - experimenting
Theory – Explains why things occur. Broad generalization that
explains a body of facts or phenomena. Model
Law – Describes a variety of scientific behavior

19. Types of Data Qualitative – descriptive nonnumeric results
Quantitative – gives definite, usually numeric, results
Number
Unit

20. Graphing Directly proportional Inversely proportional Types of Graphs:
Title graph
Label axis – numbers & units
Choose Scale
Independent variable – X – axis (Usually Time)
Dependent variable – Y – axis
Plot Points
Draw Best Fit Line
Directly proportional Inversely proportional
Dividing 1 by the other If product is constant
gives a constant value
Types of Graphs:
Line graph Bar graph Pie/ circle graph

21. Pie Graph Data Gender # of ppl Elderly 27 Women 13 Men 6 Children 15
To get percentages:
Gender
# of ppl
Elderly 27
Women 13
Men 6
Children 15
Total 61
Get part / whole # X 100
44.3 %
Elderly: 27/61 X 100 =
21.3 %
9.8 %
24.6 %
Women
Men
Children
Total
100 %
Degrees: = X
159.5 °

22. Units of Measurement-SI system
Standards of Measurement
SI – International System of Units
1. Based on units of ten, makes it easier to use
2. Used world wide
SI Base Units - (pg 34)
Fundamental SI Units
Qty Symbol Unit name Unit abbreviation
Length l Meter m
Mass m Kilogram kg
Volume V Liter L
Time t second s
Temperature T kelvin K
Amount of substance n mole mol

23. SI Units Kilo hecto deka base deci centi milli
King Henry Died by Drinking Chocolate Milk
There are 1000 base units in one kilo
There are 1000 milli in one base unit

24. Derived SI Units D = 10.8 g 4.0 cm3 D = 2.7 g/cm3 D = m/v
Density = Mass/volume
Volume = l X w X h
Find the density of a piece of aluminum w/ a
volume of 4.0 cm3 and a mass of 10.8 g.
D = 10.8 g
4.0 cm3
D = 2.7 g/cm3
D = m/v

25. Derived Units Density D = 453.3 g 123.0 ml
What is the density of a block of marble with a
mass of g and a Volume of ml?
D = m v
D = g
123.0 ml
D = 3.685g/ml

26. Accuracy Vs. Precision
ACCURACY – Refers to the agreement of a particular value with the true value.
PRECISION – Refers to the degree of
agreement among several elements
of the same quantity.

27. Precise
Precise & Accurate
Neither

29. Percent Error
Accepted value - Experimental value
Percent error =
accepted value.
X 100
What is the percent error for a mass measurement of 17.7 g, given that the correct value is 21.2 g?
% error = g g
21.2 g
16.5 % error
X 100 =

30. Significant Figures All digits known plus one final digit
Measurements from equipment

31. Counting Significant Figures
All non-zero numbers are significant
Zeros
* Leading zeros – never
* Captive zeros – Always
* Trailing zeros
* With a decimal – count
* Without a decimal – don’t count

32. 3 Questions for Zeros Is there a number in front? Is it trapped?
No – Not significant
Yes – May be… go to #2 & #3
Is it trapped?
Yes - It is significant
Is there a Decimal?
No – Not Significant
Yes – It is significant

33. Counting Significant Figures
3440. cm
910 m L kg km

34. Calculations – multiplication & Division
* The answer is rounded off to the same number of significant figures as in the measurement with the fewest sig. Fig.
13.0 ml
* ml X ml =
* g / 0.04 cm3 =
62.5
60 g/cm3

35. Calculations – Addition & Subtraction
Results should be rounded off so that the final digit is in the same place as the number with the fewest digits. \
213.67
____
55.08
– =
55.075
. \
311.67
Rounding
312.
Less than 5 = stay the same
More than 5 = increase one
If 5 = if odd increase by one
if even leave it alone

36. | | | Scientific Notation 4.6 X 10 –4 cm 2.4 X 10 -1 g 5.02 X 10 4 m
Must be a number from 1 to 9 !!!!!!!!! |
* g (2 significant figures)
2.4 X g |
* m (3 significant figures)
5.02 X 10 4 m |
* cm (2 significant figures)
4.6 X 10 –4 cm

37. SI - Prefixes Kilo, hecto, deka, Base, deci, centi, milli
Grams, liters, meters
Kilo, hecto, deka, Base, deci, centi, milli
King Henry Dances barbarically down center maine
King Henry Died by drinking chocolate milk
1.0 Kg = g
1.0 hg = 100 g
1.0 dag = 10 g
Grams, liters, meters
10 dg = 1.0 g
100 cg = 1.0 g
1 000 mg = 1.0 g

38. Chemistry Dominoes Rules
Don’t slam or throw dominoes
Take turns
Quickly get quiet when I call for your attention.
To End The Game
The player who makes the connection to the last domino wins
Count up the number of dominoes left on the table. Each domino is 1 point.
Award the winner the points left on the table.

39. Game Play
Each payer draws 1 domino to see who plays first (high domino)
Shuffle (wash) the dominoes
Each player draws 5 dominoes
Player 1 plays a number blank (if no number blank, draw) This is the starting domino
Player 2 plays a number blank. (if no number blank, draw) This is the end domino.
For the rest of the game, players play dominoes that will cancel the top number on the domino
If you can not play, draw 1 domino. This domino may be played.

40. Factor Label ________|__________ Draw your T
Write conversion-equivalent statements to…
Cancel out units
Top – Multiply, Bottom – Divide
The mass of a quarter is 10.4g, how many
milligrams is that?
________|__________ mg
10.4g
1000
= mg
| g
1.0

41. Factor Label km Express a distance of 28. Meters in centimeters
and then in kilometers.
28. m cm
100
= 2,800 cm m
1.0
28. m km
1.0
= km
1000 m

42. Factor Label 3.2 X 10 7sec * 1.0 year = __________________ seconds
1.0 yr
365 days
= 31,536,000 sec
24 hrs
60 min
60 sec
1 yr
1 hr
1 min
1 day
3.2 X 10 7sec

43. Factor Label Dimensional Analysis
1. How many kilograms are in grams?
2. How many liters are in 13.4 kL?
3. A pencil is 7.5 centimeters, how many millimeters?
4. You want to order a bicycle with a 225 mm frame, but the
sizes in the catalog are given only in inches, what should
you order?
5. A student enters a 10.0 km run. How many yards is the run?

44. Quiz 25.3 ft = _______________ mm 7.5 mg = ______________ hg
12.5 kl = _______________ ml
5.4 X 10 –6 km= _________ mm
3.0 L = ________________ cm3
25.0 weeks = ____________ sec

45. Heat & Temperature Temperature – measure of average kinetic energy
Heat – sum of kinetic energy in all of the particles in a sample
A tub of boiling water & a cup full of boiling water

46. Units of Temperature
Celsius
Kelvin
Fahrenheit

47. Heat Transfer
Convection – transfer of heat by the motion of particles in a fluid
Conduction – transfer of heat through matter by colliding particles
Radiation – transfer of energy in the form of electromagnetic waves
Heat always moves from high energy to low energy. (hot to cold)

48. Examples
Hot air balloons
Hot water and cold water mixing
Heating a pan
Boiling water

49. Units of Heat Joule Calorie 1.0 cal = 4.180 joules
The SI unit of heat energy as well as all
Other forms of energy.
Calorimeter – measures the energy absorbed or
released as heat in a chemical or physical change.
1.0 cal = joules

50. Heat Capacity
Amount of heat energy needed to raise the temperature of a sample 1oC

51. Specific Heat Q = m X Cp X DT
Amount of heat energy needed to raise the temperature of 1g of a sample 1oC.
Equation
Q = m X Cp X DT
UNITS
Joules = J
Grams = g
J/g* oC oC
Q = energy lost/ gained
M = mass
Cp = specific heat
DT = delta T = change in temp.

52. Problems 1oC to 41oC and was found to have absorbed
. A 4.0 g sample of glass was heated from
1oC to 41oC and was found to have absorbed
32 J of heat. What is the specific heat of
this type of glass?

53. Problems 1oC to 41oC and was found to have absorbed
. A 4.0 g sample of glass was heated from
1oC to 41oC and was found to have absorbed
32 J of heat. What is the specific heat of
this type of glass?
Q = m Cp DT
m=4.0g
DT=41oC-1oC=40oC
Q=32J
Cp = 0.20J/goC

54. problem
How much heat did the same glass
sample gain when it was heated from
41oC to 71oC?

55. How much heat did the same glass sample gain when it was heated from
problem
How much heat did the same glass
sample gain when it was heated from
41oC to 71oC?
Q = m Cp DT
Q=(4.0g)(0.20J/goC)(30oC)
Q=24J
m=4.0g
DT=71oC-41oC=30oC
Cp=0.20J/goC

56. Quiz 4.5 m = __________ km 899.9 ml = ________ L .54 kg = __________cg
4.5 ml = __________cm3
D = 2.45 g/ml, mass = 12.5 g vol. = ?
Vol = 25.5 ml, mass = 32.3 g D = ?
D = 3.4 g/cm3 vol = 1.5 cm mass = ?
List the things that a graph must contain
(at least 4 things)