1. AP Notes Chapter 1 Matter & Measurement
Chemistry is the study of the nature of ______ and its ____________.
Matter is anything that has ____ in unit (_) and occupies _____ in unit (_).
Matter exists in several different ______ based on the excitation or ____ in unit (_) of the particles.
matter
interactions g
mass
space L
phases
heat J

2. Elements can be represented by _____, _______, ________ and _______.
Matter composed of only one type of _____ is classified as an __________.
114 accepted elements are listed on the periodic table. Names, symbols- some with ______ origins
Elements can be represented by
_____, _______, ________ and _______.
Know your element symbols and names!
1.1Elements & Atoms
atom
element
foreign
Names, symbols, diagrams models

3. An _____ is the smallest particle of an element that retains the ______________________ of that element.
Elements with similar _________ are grouped in the periodic table.
Characteristics or properties must be definable and even measurable.
atom
characteristic properties
properties

4. 1.2 Compounds and Molecules
When two or more different elements combine together a ________ _________ is formed.
The composition (kind and number) of a atoms in a compound can be represented by a ________ _______.
Compounds may consist of ____ (charged particles) or _________ (discrete units of atoms).
chemical compound
chemical formula
ions
molecules

5. 1.3 Physical Properties
Physical properties can be observed without changing the ___________ of a substance.
Height, weight or mass, size and color are a few physical properties (Table 1.1)
_________ properties depend on amounts and _________ properties do not.
Composition
Extensive
Intensive

6. Temperature
Temperature is a measure of the
_______ ______ ______ .
Different temperature scales, all are talking about the same height of mercury or alcohol.
Derive a equation for converting ºF to ºC
Kelvin scale is an ________ scale there is no temperature below 0K.
Kelvin temperatures = ºC
Kelvin temperatures are _______ related to kinetic energy (the motion of particles).
average kinetic energy
absolute
directly

7. Density
Density
Ratio of mass to volume
D = m in units of g
V mL
Useful for identifying a compound
Useful for predicting weight
An ________________ does not depend on what the material is
Volume and hence density are temperature dependant
Intrinsic property

8. 0ºC = 32ºF
0ºC
32ºF

9. 100ºC = 212ºF
0ºC = 32ºF
0ºC
100ºC
212ºF
32ºF

10. 100ºC = 212ºF
0ºC = 32ºF
100ºC = 180ºF
0ºC
100ºC
212ºF
32ºF

11. 100ºC = 212ºF
0ºC = 32ºF
100ºC = 180ºF
10ºC = 18ºF
5ºC = 9ºF
1ºC = 9ºF 5
0ºC
100ºC
212ºF
32ºF
So 5ºC = 1ºF 9

12. (0,32) = (C1,F1)
(100,212) = (C2,F2) ºF ºC

13. 1.4 Physical and Chemical Change
Changes in physical properties are called physical changes
Changes in reactants to form new products are caused by a chemical change or chemical reaction
Chemical properties of materials are observable only through a chemical change and represented in a chemical equation

14. Scientific Method
A way of solving problems
Observation- what is seen or measured
Hypothesis- educated guess of why things behave the way they do. (possible explanation)
Experiment- designed to test hypothesis
leads to new observations,
and the cycle goes on

15. After many cycles, a broad, generalizable explanation is developed for why things behave the way they do
Theory – is formed to define a WHY
Also regular patterns of how things behave the same in different systems emerges
Law – is written to explain HOW
Laws are summaries of observations

16. Theories have predictive value.
The true test of a theory is if it can predict new behaviors.
If the prediction is wrong, the theory must be changed.
Theory- why
Law - how

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

18. 1.5 Classifying Matter
Kinetic-molecular theory
Helps us interpret properties of matter
– matter is composed of tiny particles
– particles are continuously in motion
– in solids they vibrate usually in a regular array
– in liquids & gases more free to move
Kinetic energy – force of motion of particles

19. Observing and describing these particles at the Macroscopic level is the world around us
Attempting to describe these particles at the Submicroscopic or particulate level requires models that represent what we think the particles look like and act like

20. Matter Heterogeneous Homogeneous Solution Pure Substance Element
Classifying Matter
Matter
Heterogeneous
Homogeneous
Solution
Pure Substance
Element
Compound

21. 1.6 Units of Measurement
Matter must be explainable to others which means that individuals communicating must agree on type and units of measurement or at least be able to convert measures between each others measure
Qualitative – it is blue, (what shade of blue)
Quantitative – it is 4 inches, (well how long is an inch)
A common system of measure is needed

22. Metric System Every measurement has two parts Number Scale (unit)
SI system (le Systeme International) based on the metric system
Prefix + base unit
Prefix tells you the power of 10 to multiply by - decimal system -easy conversions

23. Metric System Base Units - must be definable or derivable
Mass - kilogram (kg)
Length- meter (m)
Time - second (s)
Temperature- Kelvin (K)
Electric current- ampere (amp, A)
Amount of substance- mole (mol)

24. Base Unit grams, Liters, meters 100
Prefixes
giga- G 1,000,000,
mega - M 1,000,
kilo - K 1,
Hecto - H 1,
Deka - D 1,
Base Unit grams, Liters, meters 100
deci- d
centi- c
milli- m
micro- m
nano- n

25. Deriving or describing density
Deriving the Liter
Liter is defined as the volume of 1 dm3
gram is the mass of 1 cm3 of water at 25oC where then 1Kg of water is the mass of 1 L of water.
Deriving or describing density
Density is the proportional relationship between an objects mass and its volume, D = m/V

26. Mass and Weight Mass is measure of resistance to change in motion
Weight is force of gravity.
Sometimes used interchangeably
Mass can’t change, weight can

27. 1.7 Using Numerical Information
Systematic error is in same direction each time
Better precision implies better accuracy
You can have precision without accuracy
You can’t have accuracy without precision
How well is a measure known?
Significance

28. Accuracy vs. Precision

29. Accuracy
Absolute error (AE) = exp - known
% Accuracy = |%AE|

30. Relative error (RE) = exp - average
Precision
Relative error (RE) = exp - average
% Precision = |%RE|

31. Error
Error = experimental – accepted

32. Significant figures Meaningful digits in a MEASUREMENT
Exact numbers are counted, have unlimited significant figures
If it is measured or estimated, it has sig figs.
If not it is exact.
All numbers except zero are significant.
Some zeros are, some aren’t

33. Which zeroes count? In between other sig figs does
Before the first number doesn’t
After the last number counts iff
it is after the decimal point
the decimal point is written in
sig figs
sig figs

34. Doing the math
Multiplication and division, same number of sig figs in answer as the least in the problem
Addition and subtraction, same number of decimal places in answer as least in problem.

35. Using the units to solve problems
1.8 Problem Solving
Conversion of a given measurement to a desired quantity by means of mathematical relationship of data
Dimensional Analysis
Using the units to solve problems

36. Dimensional Analysis Use conversion factors to change the units
1 foot = 12 inches (equivalence statement)
12 in = = 1 ft ft in
Every equality gives 2 conversion factors
multiply by the one that will give you the correct units in your answer.

37. How Many Millimeters in 6.78 inches?
Given: 6.78 in.
Need: millimeters
Connections: 2.54 cm = 1 in.
1cm = 10mm

38. Sample Distance Problems
11 yards = 2 rod
40 rods = 1 furlong
8 furlongs = 1 mile
The Kentucky Derby race is 1.25 miles. How long is the race in rods, furlongs, meters, and kilometers?
A marathon race is 26 miles, 385 yards. What is this distance in rods, furlongs, meters, and kilometers?

39. Sample Mass Problem
Apothecaries (druggists) use the following set of measures in the English system:
20 grains ap = 1 scruple (exact)
3 scruples = 1 dram ap (exact)
8 dram ap = 1 oz. ap (exact)
1 dram ap = g
What is the mass of 1 scruple in grams?

40. How Many Liters in 1.0 Cubic Yard?
Volume Problem
How Many Liters in 1.0 Cubic Yard?
Given: 1 yd3
Need: Liters
Connections: 1 yd = 36 in cm = 1 in mL = 1 cm3

41. Sample Speed Problem
Science fiction often uses nautical analogies to describe space travel. If the starship U.S.S. Enterprise is traveling at warp factor 1.71, what is its speed in knots?
Warp 1.71 = 5.00 times the speed of light
speed of light = 3.00 x 108 m/s
1 knot = 2000 yd/h exactly

42. Sample Problem
The speed of light is 3.00 x 108 m/s. How far will a beam of light travel in 1.00 ns?

43. Density
Density
Ratio of mass to volume
D = m in units of g
V mL
Useful for identifying a compound
Useful for predicting weight
An ________________ does not depend on what the material is
Volume and hence density are temperature dependant
Intrinsic property

44. Sample Density Problem 1
An empty container weighs g. Filled with carbon tetrachloride (density 1.53 g/cm3 ) the container weighs g. What is the volume of the container?

45. Sample Density Problem 2
A 55.0 gal drum weighs 82.0 lbs. when empty. What will the total mass be when filled with ethanol?
density g/cm3
1 gal = 3.78 L
1 lb = 454 g