Measurement and
the Metric System
Quantitative observations
Measurement
 Fundamental
Direct
measurement
Indirect
 Derived
measurement
quantities
Calculations
Density
Heat
quantities
energy
Rules for Significant
Measurements
 One
place past the smallest
calibration
 Indicates
where uncertainty is
 Communicate
instrument
precision of the
Protocols for deriving
quantities

Multiplication and division

Addition and subtraction

Rounding values
Metric System

Developed in France in 1795

Revised and called International
System of Measurements (SI) in 1960

Based on units of 10
SI Base Units
Quantity
symbol
Length
SI base
unit
Meter
Mass
gram
g
Temperature
Time
Kelvin
Celsius
Second
K
oC
s
Liquid volume
Liter
L
Amount of
substance
Mole
mol
m
Memorize these !!!!!
* “unit” refers to “base unit”

1 Kilo = 1 x 103 units

1Giga(G) = 1 x 109 units

1 Hecto = 1 x 102 units

1Mega(M) = 1 x 106units

1 Deka = 1 x 101 units

1 x 106 Micro(µ) = 1 unit

Basic unit = 1

1 x 109 Nano(n) = 1 unit

1 x 101 deci (d) = 1 unit

1 x 1012 Pico(p) = 1 unit

1 x 102 centi (c)= 1 unit

1 x 103 milli(m) = 1 unit
Conversions Practice
Density

Amount of matter per unit volume
 Water:
 Iron:
 Lead
1.000 g/ ml at 25C
7.87 g/cm3
11.3 g/cm3
Density
is calculated by:
D = mass
volume
Density

Density is the amount of matter in a
given space (volume)

D = mass

volume
Density

Measuring liquid volume
 Volume
displacement
Density

Measuring solid volume
 Cube

= length x width x height
2
Cylinder = V =πr h
Density

Ex: A solid displaces 45.67 ml of water
and has a mass of 98.5 grams. Calculate
its density. Is it a block of lead?
Density practice
Specific gravity
 Comparison
of the ratio of the
density of a substance to the
density of liquid water at 4C
 (1.00g/ml)
Temperature Scales

Temperature is the measure of the
average kinetic energy of a system.

Implies molecular motion

Celsius temperature

Kelvin temperature
Temperature Scales
Fahrenheit Celsius Kelvin
Water
Boils
Water
Freezes
Molecular
Motion
Stops
212oF
100oC
373 K
32oF
0o C
273 K
-460oF
-273oC
0 K
(absolute
zero)
Converting between
Temperature Scales
Fahrenheit and Celsius:
oC
= 5/9 (oF-32)
oF
= (9/5 x oC)+32
Ex.What is the Celsius value for 60.0oF?
oC = 5/9(60-32)
oC = 5/9(28)
oC = 15.55
oC
=15.6
From Celsius to Kelvin:
oC
K =
+ 273
Ex.80.0oC would be what value on the Kelvin
scale?
K
= 80 +
K = 353
273
Heat and Specific Heat

Heat is the flow of thermal energy
in a system

Heat flows from hotter to cooler
 Ice

cubes!
Heat can flow into or out of a
system
Heat and Specific Heat
 Heat
transfer that causes
temperature changes simply
change in KINETIC ENERGY
 Heat
transfer that causes phase
changes imply change in
POTENTIAL ENERGY
The Joule

Metric unit of energy

4.18 joules raises 1.00g of water
1C.
 This
is the SPECIFIC HEAT OF WATER!
Percent Composition
When you see %, think……
Part
X
100
=
%
Whole
Percent Composition
 percent
by mass
% composition = Mass of element
x 100%
mass of compound
Terms to review

Fundamental and derived quantities

Precision and accuracy

Matter

Mass

Volume

Density

Significant Figures

% composition

Scientific notation

Metric system

Dimensional analysis