Download Chapter 1 - OSU Chemistry

Chapter 1
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Science
An organized body of knowledge obtained by
observation and experiment.
balloon demo
Scientific Method
A general process by which science evolves.
Qualitative:
no numbers
descriptive
color
smell
taste
Quantitative:
numbers
weight
volume
temperature
time
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Chapter 1.1 Chemistry: The Study of Matter
Chemistry
characteristics
composition
transformations
matter
Matter
has mass
occupies space
Mass
quantity of matter
Weight
mass & gravity
Chapter 1.2
Physical States of Matter
Solid
definite shape and definite volume
Liquid
indefinite shape and definite volume
Gas
indefinite shape and indefinite volume
”______________”
Figure 1.1 in text
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States of matter depend on temperature, pressure,
strength of intermolecular forces
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Chapter 1.3
Properties of Matter
Physical Properties can be observed without
changing the basic identity of the substance
• color, odor, physical state
•
•
•
Chemical Properties describe the way a substance
undergoes or resists change to form a new
substance
• Sodium reacts with water but silver does not
• Ether is highly ____________
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Chapter 1.4
Changes in Matter
Physical Changes - changes in physical appearance
but no changes in chemical composition
• Melting
•
•
Chemical Changes/Reactions - changes in chemical
composition and structure
• Rusting of iron objects
• Burning of __________
demo
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A Chemical Equation is used to represent a
chemical reaction
Reactants
→
Ethanol + Oxygen →
Products
Carbon dioxide + Water
LAW OF CONSERVATION OF MASS
Matter can neither be created nor destroyed.
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Chapter 1.5 Pure Substances and Mixtures
Fig 1.6
A Pure Substance
• has definite and constant __________
• cannot be separated by ____________ means
• has the same properties under the same conditions
Example:
Mixtures
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• Two or more substances
each retains its own identity
• Composition can vary
• Properties can vary with ___________
• Can be separated by __________ means
Homogeneous Mixture - __________
• One visible phase
• Uniform ___________ throughout
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Heterogeneous Mixture
• Two or more visible phases
• Different properties in different phases
Fig 1.5b
potassium dichromate and iron filings
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Chapter 1.6 Elements and Compounds
water → hydrogen + oxygen
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Chapter 1.7 Discovery and Abundance of the Elements
88 naturally occurring elements
29 elements synthesized
Figure 1.10
demo of samples
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Chapter 1.8 Names and Chemical Symbols of the Elements
Only the first letters of chemical symbols are capitalized!
Co
Element
Nickel
Magnesium
Sodium
Potassium
CO
2 elements in a compound
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Chapter 1.9
Atoms and Molecules
Atom = the smallest particle of an element that can
exist and still have the properties of the element.
Figure 1.12
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Molecule = two or more atoms bonded together.
Homoatomic
Fig 1.13
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Heteroatomic – two or more kinds of atoms are present.
From Figure 1.1
diatomic
_________
___________
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Chapter 1.10
Chemical Formulas
H2 O
_______
C9H8O4
Aspirin
Al2(SO4)3
2 Al
3 SO4 groups = ___ S + ___ O