P. Sci.

1
P. Sci.

• Unit 8
• Periodic Table
• Chapter 5

2
Periodic Law
Atomic Radius
Electro-negativity

• Properties of elements tend to change in a
  regular pattern when elements are arranged in
  order of increasing atomic number, or number of
  protons in their atoms.

Atomic mass
Density
Ionization Energy
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Periodic Table

• The periodic table is arranged in-
• Periods (horizontal) rows
• There are 7 periods
• Groups families (vertical) columns
• There are 18 columns

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• Metals
• all elements on the left side of the table
  (except Hydrogen)
• Non - Metals
• all elements on the right side of the table

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Hydrogen

• Hydrogen (1) 90 of the atoms in the universe
  (diatomic two atoms of the same element in a
  covalent bond H,N,O). Very reactive, both
  covalent and ionic bonds can form

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Metalloids

• elements that share both metal and non-metal
  characteristics the elements on both sides of
  the stair-step line except aluminum.
• Also called semiconductors

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Alkali Metals
H hydrogen

• (Column 1 except Hydrogen) the most reactive
  group do not occur in nature in their elemental
  form. Has one electron in its outer energy level
  
• All (including hydrogen) have 1 valence electron.

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Alkaline Earth Metals

• (Column 2) also reactive also do not occur in
  nature alone (fireworks)
• 2 valence electrons.

Li
Na
K
Rb
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Transition Elements

• (Columns 3 12) stable metals occur in natural
  state.
• usually have 2 3 valence electrons to give up
  to form bonds.

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Mixed groups

• Boron group (13) mixed with both metals and
  non-metals.
• 3 valence electrons

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Mixed groups cont.

• Carbon group (14) mixed with both metals and
  non-metals.
• 4 valence electrons

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Mixed groups cont.

• Nitrogen group (15) mixed tend to share to
  form covalent bonds fertilizers.
• 5 valence electrons

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Mixed groups cont.

• Oxygen group (16) mixed
• 6 Valence electrons

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Halogens

• (17 all nonmetal) very reactive in their
  element form. If combined with a metal forms
  salt. Many are diatomic (F,Cl,Br) Br only
  nonmetal liquid.
• 7 valence electrons

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Noble Gases

• (18) Most stable because outer layer is full.
  No known natural compounds. Helium gas, neon /
  argon in neon lights, argon / krypton in electric
  light-bulbs, used to produce lasers
• 8 valence electrons (full shell)

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Other Groups

• Iron Triad Iron, Cobalt, and Nickel create
  steel and other metal mixtures.

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Other groups cont.

• Coinage group Copper, Silver, and Gold stable
  and malleable and found in nature used to make
  coins.

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Other groups cont.

• Coating metals / Zinc group Zinc, Cadmium, and
  Mercury used to coat or plate other metals
  Mercury only liquid metal (cadmium and mercury
  used in batteries.)

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Other groups cont.

• Lanthanide series
• elements 58 71
• Actinide series
• elements 90 103
• Transuranium
• all elements over 92

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Allotropes

• (recall isotopes) materials made of the same
  element that have different molecular structure.

Diamonds
Graphite
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Thats All
folks
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S-113

• What is the periodic Table?
• How is it arranged?

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S-116

• What subatomic structure is reflected in the
  periodic table?

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Unit 5 The Periodic Table

• SPS4 Students will investigate the arrangement of
  the Periodic Table
• a. Determine the trends of the following
• Number of valence electrons
• Types of ions formed by representative elements
• Location of metals, nonmetals, and metalloids
• Phases at room temperature
• b. Use the Periodic Table to predict the above
  properties for representative elements

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5.1 Organizing the Elements

• How did Mendeleev organize the elements in his
  periodic table?
• What evidence helped verify the usefulness of
  Mendeleevs table?

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5.1 Organizing the Elements How did Mendeleev
organize the elements in his periodic table?

• 1860 Mendeleev organizes the periodic table
• Rows (called periods) by increasing mass
• Later by atomic number
• Columns (called groups or families) by similar
  chemical and physical properties
• Periodic means that properties repeat at
  regular intervals
• Only knew 63 elements
• He predicted the properties of blanks in his
  periodic table

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5.1 Organizing the Elements What evidence helped
verify the usefulness of Mendeleevs table?

• Mendeleev predicted elements
• Eka-aluminum (one below aluminum)
• Soft metal with a low melting point and a density
  of 5.9 g/cm3
• 1875 Gallium (Ga) discovered
• Soft metal, melting point 29.7oC, density of 5.91
  g/cm3
• Proved the patterns could be used to predict
  elements

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S-118

• What two characteristics are used to organize the
  modern periodic table?

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5.2 The Modern Periodic Table

• How is the modern periodic table organized?
• What does the atomic mass of an element depend
  on?
• What categories are used to classify elements on
  the periodic table?
• How do properties vary across a period in the
  periodic table?

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5.2 The Modern Periodic Table How is the modern
periodic table organized?

• Periodic Law
• Elements are arranged in order of increasing
  atomic number (protons)
• Period rows on the periodic table
• As the row number increases outside electrons are
  in higher energy levels
• First energy level hold 2 so hydrogen and
  helium have electrons in first energy level
• Second energy level holds 8 so second row has
  eight elements

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5.2 The Modern Periodic Table How is the modern
periodic table organized?

• Periodic Law
• Properties of elements repeat in predictable ways
  and are used to place element in columns
• Group columns
• Numbered 1-18
• Some have names
• 1 alkali metals
• 2 alkaline earth metals
• 17 halogens
• 18 noble gases

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5.2 The Modern Periodic Table What does the
atomic mass of an element depend on?

• Atomic Mass
• Measured in atomic mass units (u)
• One twelfth of the mass of Carbon-12
• Average Atomic Mass - calculated using weighted
  averages
• The abundance of an isotope (add up to 100)
• Mass of each different isotope

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5.2 The Modern Periodic Table What categories are
used to classify elements on the periodic table?

• Elements are classified in three ways
• Natural vs Man made
• Technetium (Tc)
• All elements above 92

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5.2 The Modern Periodic Table What categories are
used to classify elements on the periodic table?

• Elements are classified in three ways
• State of Matter at room temperature
• Liquids Hg, and Br
• Gases Group 18, H, N, O, F, Cl
• Solids the rest of the elements up to 92

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5.2 The Modern Periodic Table What categories are
used to classify elements on the periodic table?

• Elements are classified in three ways
• Metals, Non-Metals, Metalloids
• Metals Left of zig-zag line
• Transition Metals group 3-12
• Non-Metals right of zig-zag line
• Metalloids touch the zig-zag line, except
  Aluminum

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5.2 The Modern Periodic Table How do properties
vary across a period in the periodic table?

• Changes in properties across a periodic table
• From left to right
• Become less metallic, more nometallic
• More likely to gains electrons, less likely to
  lose them

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S-119

• For the element Iron, answer the following
  questions
• 1. metal, nonmetal, metalloid?
• 2. state of matter at room temperature?
• 3. average atomic mass?
• 4. name of group?
• 5. period?

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5.3 Representative Groups

• Why do the elements in a group have similar
  properties?
• What are some properties of the A groups in the
  periodic table?

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5.3 Representative Groups Why do the elements in
a group have similar properties?

• Valence Electrons
• Electrons in the highest occupied energy level
• Major factor in chemical reactions
• Elements in the same group, have the same valence
  electrons

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5.3 Representative Groups What are some
properties of the A groups?

• Alkali Metals
• Group one
• 1 valence electron
• React by losing 1 electron
• Gain a positive charge
• Highly reactive

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5.3 Representative Groups What are some
properties of the A groups?

• Alkaline Earth Metals
• Group two
• 2 valence electrons
• React by losing 2 electron
• Gain a positive charge
• Less reactive

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5.3 Representative Groups What are some
properties of the A groups?

• Boron Family
• Group 13
• 3 valence electrons
• React by losing 3 electron
• Gain a positive charge

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5.3 Representative Groups What are some
properties of the A groups?

• Carbon Family
• Group 14
• 4 valence electrons
• React by sharing electrons

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5.3 Representative Groups What are some
properties of the A groups?

• Nitrogen Family
• Group 15
• 5 valence electrons
• React by gaining electrons
• Gain negative charge

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5.3 Representative Groups What are some
properties of the A groups?

• Chalcogens (Oxygen Family)
• Group 16
• 6 valence electrons
• React by gaining electrons
• Gain negative charge
• More reactive

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5.3 Representative Groups What are some
properties of the A groups?

• Halogens
• Group 17
• 7 valence electrons
• React by gaining electrons
• Gain negative charge
• Very reactive

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5.3 Representative Groups What are some
properties of the A groups?

• Noble Gases
• Group 18
• 8 valence electrons
• Do not react or form compounds

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5.3 Representative Groups What are some
properties of the A groups?

• Transition Metals (Transition Elements)
• Group 3-12
• 2 valence electrons
• Additional electrons are filling lower energy
  levels
• All have similar properties
• What we think of as Metals

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5.3 Representative Groups What are some
properties of the A groups?

• Actinide and Lanthenide Series
• No group number
• 2 valence electrons
• Additional electrons are filling lower energy
  levels
• Very few things that we deal with on a regular
  basis