Keys to the Study of Chemistry
1.1 Some Fundamental Definitions
1.2 The Scientific Approach: Developing a Model
1.3 Chemical Problem Solving
1.4 Measurement in Scientific Study
1.5 Uncertainty in Measurement: Significant Figures
10 November 2014 1
Arrange the following in a concept map
Chemistry
Matter
Physical change
Chemical change
A silver fork rusts
Clothes dry up
under the sun
Solid
Liquid
Gas
Potential energy
Kinetic energy
Position
Motion
Physical
properties
Chemical
properties
Density
Flammability
Melting point
Corrosiveness
Intensive
property
Extensive
property
2
Scientific Method
3
Identify an observation you had this week. Use the
scientific method to understand the observation you
had.
Observation
Hypothesis
Experiment
Model (Theory)
Further Experiment
Conversion Factors Pick the tallest and the shortest person in your group.
For each of them, count how many steps it takes to
walk a distance of 5 meters.
What is the area of the quadrangle outside F-116?
4
SI Units Match the physical quantity (dimension) to its
corresponding unit name and unit abbreviation.
5
Physical Quantity Unit Name Unit Abbreviation
Mass
Length
Time
Temperature
Electric current
Amount of substance
Luminous intensity
mole
kilogram
ampere
kelvin
meter
candela
second
s
K
A
cd
mol
kg
m
Common decimal prefixes used
with SI units Arrange the following prefixes and match to their
respective prefix symbol and exponential notation:
6
Prefix Symbol Exponential notation
micro
kilo
deci
nano
mega
centi
milli
pico
p
n
μ
M
k
c
m
d
1x106
1x10-9
1x10-2
1x103
1x10-12
1x10-6
1x10-1
1x10-3
The Components of Matter
2.1 Elements, Compounds, and Mixtures: An Atomic Overview
2.2 The Observations That Led to an Atomic View of Matter
2.3 Dalton’s Atomic Theory
2.4 The Observations That Led to the Nuclear Atom Model
2.5 The Atomic Theory Today
2.6 Elements: A First Look at the Periodic Table
2.7 Compounds: Introduction to Bonding
2.8 Formulas, Names, and Masses of Compounds
2.9 Classification of Mixtures
7
8 by: RBG
Pure Substances Element: matter that consists of only one kind of
atom
Compound: matter that is composed of two or more
different elements that are chemically bound
together
9
Mixtures Mixture: a group of 2 or more substances that can
be separated using a physical process
Heterogeneous: non-uniform throughout the mixture
Homogeneous: uniform throughout the mixture
10
Learning Check The following scenes represent an atomic-scale
view of three samples of matter. Describe each
sample as an element, compound, or mixture.
11
Mixture Element Compound
Atomic View of Matter 1. Law of Conservation of Mass
2. Law of Definite (or Constant) Composition
3. Law of Multiple Proportions
12
Law of Conservation of Mass The total mass of substances present does not
change during a chemical reaction.
13
Law of Conservation of Mass The total mass of substances present does not
change during a chemical reaction.
14
reactant 1 + reactant 2
total mass
product
total mass =
calcium oxide + carbon dioxide calcium carbonate
CaO + CO2 CaCO3
56.08 g + 44.00 g 100.08 g
Law of Conservation of Mass This law forms the basis for “balanced chemical
equations” in chemistry.
15
Learning Check Assume that a mixture of substances undergoes a
reaction. Which drawing represents a product mixture
consistent with the law of mass conservation?
16
Law of Definite Composition No matter the source, a particular compound is
composed of the same elements in the same parts
(fractions) by mass.
H2O (Manila) = H2O (Davao) = H2O (Australia)
17
Analysis by
Mass
(grams/18.0g)
Mass Fraction
(parts/1.00
part)
Percent by
Mass
(parts/100
parts)
16.0 g oxygen
2.0 g hydrogen
0.89 oxygen
0.11 hydrogen
89% oxygen
11% hydrogen
Practice Exercise A compound of copper and sulfur contains
88.39 g of metal and 44.61 g of nonmetal.
How many grams of copper are in 5264 kg of
compound? How many grams of sulfur?
18
3.498 x 106 g Cu
1.766 x 106 g S
Cu and S CuS
