The Periodic Table

1
The Periodic Table

• Chapter 6

2
Development of the modern periodic table

• Section 6.1

3
Antoine Lavoisier

• Late 1700s
• _____ elements (known at time) organized in four
  categories

4
Lothar Meyer/Dmitri Mendeleev

• Mid-late 1800s
• Demonstrated a connection between
  _________________and elemental properties
• Arranged elements with similar chemical
  properties _______________________
• Mendeleev is given more credit because he
  published first

5
Mendeleevs Table
6
Henry Moseley

• Early 1900s
• Realized arranging the elements by atomic mass
  was not the best way some elements ended up in
  columns with elements of different properties
• Discovered atoms have a unique number of protons
  (the ____________________)
• Arranged elements in order of ______________
  ____________________, which resulted in a
  periodic pattern of properties

7
The Modern Periodic Table
8
Modern Periodic Table

• Groups/Families ___________ columns
• Periods ____________ rows

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(Z)
10
Representative Elementstall groups
11
Transition Metals
12
Metalloids along step line (except for
Aluminum)
13
Metals left side
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Properties of Metals

• _______________ heat and electricity
• _____________ (can be hammered into thin sheets)
• ______________ (can be pulled into wires)
• Lustrous (__________) appearance
• Almost all metals are __________ at normal
  temperatures

15
Non-Metals right side (blue)
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Properties of Non-Metals

• Generally lack properties that characterize
  metals
• Show more variation in properties than metals do
• Many are _________ at normal temperatures

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____________ Group 1
18
___________________ Group 2
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_____________ Group 7
20
________________ Group 8
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Classification of the elements

• Section 6.2

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Organizing the Elements byElectron Configuration

• Valence electrons
• Electrons in the outermost principal energy level
• Number of valence electrons correspond to the
  representative elements ___________________
  (Group 1 has 1 valence electron, Group 2 has 2
  valence electrons, Group 13 has 3 because it is
  the 3rd representative group, etc)
• Energy level of valence electrons correspond to
  the __________________ (Period 4 valence
  electrons are in the 4th energy level and so on)

23
The s-, p-, d-, and f-Block Elements

• We saw these with our little cheat sheets
• This shows which __________ is being filled

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Periodic trends

• Section 6.3

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What are Periodic Trends?

• Many properties of the elements change in a
  predictable way, based on their location in the
  periodic table
• We will look at the following properties
• ________________
• _________________
• ________________________ the energy reqd to
  remove an electron from a gaseous atom
• ________________________ ability of an atom to
  attract electrons in a chemical bond

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Atomic Radius

• Trends within periods
• _____________ in atomic radius as you move from
  left to right across a period
• Trends within groups
• General _____________ in atomic radius as you
  move down a group

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Ionic Radius

• An ______ is an atom or bonded group of atoms
  that has a positive or negative charge
• When atoms _______________ and become _________
  ions, they always become _______
• When atoms _______________ and become
  ____________ ions, they become _________

28
Ionic Radius (contd)

• Trends within periods (see Fig 6.14)
• Generally, as you move from left to right across
  a period, the size of the positive ions
  ___________
• Then, beginning in group 15 or 16, the size of
  the much-larger negative ions also gradually
  _________________
• Trends within groups
• As you move down a group, ionic size gradually
  __________________

29
Ionization Energy

• Trends within periods
• Values of first ionization energies generally
  ______________ as you move from left to right
  across a period.
• Trends within groups
• First ionization energies generally ____________
  as you move down a group

30
The Octet Rule

• Atoms tend to gain, lose, or share electrons in
  order to acquire a full set of ______________
  ______________
• Exception ______________ does not want 8 valence
  electrons ? it will usually give up its one
  electron to make a positive ion

31
Electronegativity

• Electronegativity values range from ________
• __________ is the most electronegative atom
  (3.98)
• __________ is the least electronegative atom
  (0.70)
• Many periodic tables list electronegativity
  values as well