Chapter 1 1 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 4

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 ____________

7 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 → Products Ethanol + Oxygen → Carbon dioxide + Water

LAW OF CONSERVATION OF MASS Matter can neither be created nor destroyed.

9 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 10

• 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

12 Chapter 1.6 Elements and Compounds

water → hydrogen + oxygen

13 Chapter 1.7 Discovery and Abundance of the Elements 88 naturally occurring elements demo of samples 29 elements synthesized

Figure 1.10

14 Chapter 1.8 Names and Chemical Symbols of the Elements

Only the first letters of chemical symbols are capitalized! Co Element CO 2 elements in a compound Nickel Magnesium Sodium Potassium

16 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 _________ ___________

19 Chapter 1.10 Chemical Formulas H2O _______ C9H8O4 Aspirin Al2(SO4)3 2 Al

3 SO4 groups = ___ S + ___ O