Chapter 3 Classification of Matter

1
Chapter 3Classification of Matter

• Objectives
• Define and give examples of 3 states of matter
  (3.1 3.2)
• Distinguish between substances and mixtures (3.3
  3.12)
• Understand what elements are (3.4-3.7)
• Distinguish between metals, nonmetals and
  metalloids (3.8)
• Define compounds and diatomic molecules (3.9
  3.10)
• Be able to write chemical formulas (3.11)

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What is Matter?

• Anything that has mass and occupies space
• Composed of atoms
• Exists in three states on earth
• Exists in fourth state in space

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Solids

• Definite
• Particles tightly packed
• Crystalline
• Amorphous solids

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Liquids

• Definite volume
• Not a
• Particles have
• Particles can

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Gases

• Indefinite volume
• No
• Particles have
• Particles

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Substances and Mixtures

• Pure Substance a particular kind of matter with
  a definite, fixed composition
• Mixture

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Matter
Pure substances (homogeneous composition)
Mixtures of two or more substances
Elements
Compounds
Solutions (homogeneous composition one phase)
Heterogeneous mixtures (two or more
phases)
Figure 3.2 (page 48)
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Types of Mixtures

• Heterogeneous mixtures
• Chocolate chip cookies granite
• Homogeneous mixtures

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Separating Mixtures

• Do NOT cause chemical changes
• Heterogeneous Mixtures

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Separating Mixtures

• Homogeneous Mixtures

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Separating Mixtures

• Homogeneous Mixtures

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Separating Mixtures

• Homogeneous Mixtures

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Pure Substances

• Elements
• Compound

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Elements

• 111 presently known elements
• At room temperature
• Figure 3.3 distribution of elements in the

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Elements

• Names of the elements
• Greek
• Latin
• Location where discovered

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Elements

• Arranged in the Periodic Table (inside front
  cover)
• Symbols
• Some symbols are Latin/Greek name (Table 3.4)

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Elements

• Classification
• Metal
• Nonmetal
• Metalloid
• See Table 3.5

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Elements

• Metals
• Usually solid at room temperature
• High luster
• Malleable
• Usually dont combine with each other

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Elements

• Nonmetals
• Solids ( ) Liquid (
  ) Gases (all others)
• Poor conductors
• Low melting point
• Will combine
• Will combine
• Some found uncombined in nature

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Elements

• Metalloids
• Have properties of
• Some used for semiconductors in electronics

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Compounds

• Two or more elements
• New properties
• Can be chemically separated

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Compounds

• Molecular
• Held together with
• Molecule
• Water is an example

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Compounds

• Ionic
• Ion
• Cation
• Anion
• Held together by ionic bond

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Compounds

• Diatomic Molecules
• Always only 2 atoms
• 7 naturally occurring

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Chemical Formulas

• Abbreviations for compounds
• Sodium Chloride (NaCl)

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Chemical Formulas

• Subscript indicates of atoms present
• H2O has 2 Hydrogen atoms and 1 Oxygen atom
• NaOH has

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Chemical Formulas

• Parentheses are used to show when a compound
  contains more than one group of atoms that occurs
  as a unit

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Chemical Formulas

• Show only number and kind of atom
• Do not show arrangement of the atoms or how
  chemically bonded