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
• Solid
• Liquid
• Gas
• Exists in fourth state in space
• Plasma

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Solids

• Definite shape and volume
• Particles tightly packed
• Crystalline salt, sugar, quartz
• Amorphous solids no regular, geometric pattern

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Liquids

• Definite volume
• Not a definite shape (Takes shape of container)
• Particles have more energy
• Particles can move freely

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Gases

• Indefinite volume
• No definite shape
• Particles have high energy level
• Particles move independently of one another

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Substances and Mixtures

• Pure Substance a particular kind of matter with
  a definite, fixed composition
• Elements (copper, gold, oxygen)
• Compounds (sugar, salt, water)
• Mixture a blend of two or more pure substances
• Not chemically combined

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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
• Visibly different parts
• Chocolate chip cookies granite
• Two or more phases (usually)
• Homogeneous mixtures
• Different parts not visible (uniform throughout)
• One phase
• Seawater air

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Separating Mixtures

• Do NOT cause chemical changes
• Heterogeneous Mixtures
• Filtration

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Separating Mixtures

• Homogeneous Mixtures
• Distillation

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Separating Mixtures

• Homogeneous Mixtures
• Chromatography

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Separating Mixtures

• Homogeneous Mixtures
• Crystallization

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Pure Substances

• Elements
• A substance that cannot be separated into simpler
  substances
• Compound
• Two or more elements combined through a chemical
  reaction
• Different properties than elements which compose
  it

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Elements

• 111 presently known elements
• Building blocks of all substances
• At room temperature
• 2 liquid
• 11 gases
• All others solid
• Figure 3.3 distribution of elements in
  galaxies, earths crust, seawater and air, and
  human bodies

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Elements

• Names of the elements
• Greek
• Latin
• German
• Properties of elements
• Scientist who discovered it
• Location where discovered

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Elements

• Arranged in the Periodic Table (inside front
  cover)
• Symbols
• One or two letters
• Usually part of name (Table 3.3, pg 52)
• Some symbols are Latin/Greek name (Table 3.4,
  pg 52)

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Elements

• Classificiation
• Metal
• Nonmetal
• Metalloid
• See Table 3.5 (page 54)

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Elements

• Metals
• Usually solid at room temperature
• Good conductors of heat and electricity
• High luster
• Ductile
• Malleable
• High melting point high density
• Usually dont combine with each other
• Readily combine with nonmetals

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Elements

• Nonmetals
• Solids (C, P, S, Se, I) Liquid (Br) Gases (all
  others)
• Poor conductors of heat and electricity no
  luster
• Low melting point low density
• Will combine with each other (CO2)
• Will combine with metals or metalloids
• Some found uncombined in nature (noble gases)

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Elements

• Metalloids
• Have properties of both metals and nonmetals
• Some used for semiconductors in electronics

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Compounds

• Two or more elements chemically combined
• New properties
• Definite proportions
• Can be chemically separated
• Molecular or Ionic

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Compounds

• Molecular
• Held together with covalent bonds
• Molecule smallest uncharged individual unit of
  a compound
• Water is an example

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Compounds

• Ionic
• Ion positively or negatively charged atom or
  group of atoms
• Cation positive
• Anion negative
• Held together by ionic bond attraction between
  positive and negative charges

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Compounds

• Diatomic Molecules
• Always only 2 atoms
• 7 naturally occurring
• Hydrogen, oxygen, nitrogen, flourine, chlorine,
  bromine, iodine
• H2, O2, N2, F2, Cl2, Br2, I2,

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Chemical Formulas

• Abbreviations for compounds
• Symbols and ratios of atoms
• Sodium Chloride (NaCl)
• 1 atom of sodium for every 1 atom of chlorine
• Number 1 not usually written

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Chemical Formulas

• Subscript indicates of atoms present
• H2O has 2 Hydrogen atoms and 1 Oxygen atom
• H2SO4 has
• NaOH has
• C6H12O6 has

2 hydrogen atoms, 1 sulfur atom, 4 oxygen atoms
1 sodium atom, 1 oxygen atom, 1 hydrogen atom
6 carbon atoms, 12 hydrogen atoms, and
6 oxygen atoms
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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
• Calcium Nitrate
• Ca(NO3)2 has 1 calcium, 2 nitrogen, and 6 oxygen
  atoms
• Ba3(PO4)2 has

3 barium, 2 phosphorus, and 8 oxygen atoms
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Chemical Formulas

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