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The Why and How of Ions

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The Why and How of Ions Featuring the Return of Bohr-Rutherford Diagrams and the Periodic Table – PowerPoint PPT presentation

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Title: The Why and How of Ions


1
The Why and How of Ions
Featuring the Return of Bohr-Rutherford Diagrams
and the Periodic Table
2
Bohr-Rutherford Diagrams
  • Bohr-Rutherford diagrams (or simply Bohr
    diagrams) are used to show the arrangement of
    electrons in the atom, e.g.

3
How To Draw Bohr Diagrams
  1. Find your element on the periodic table.
  2. Determine the number of electrons, which for a
    neutral atom is equal to the number of ?

4
How To Draw Bohr Diagrams
  1. Find your element on the periodic table.
  2. Determine the number of electrons, which for a
    neutral atom is equal to the number of protons,
    which is equal to the ?

5
How To Draw Bohr Diagrams
  1. Find your element on the periodic table.
  2. Determine the number of electrons, which for a
    neutral atom is equal to the number of protons,
    which is equal to the atomic number.

6
How To Draw Bohr Diagrams
  • 3) Determine which period (row) your element is
    in.
  • Elements in the 1st period have one energy level
    or shell.
  • Elements in the 2nd period have two, and so on.

7
How To Draw Bohr Diagrams
  • 4) Draw a nucleus with the element symbol (and
    optionally, the s of protons and neutrons)
    inside.
  • 5) Draw the shells around the nucleus.
  • Carbon is in the 2nd period, so it has two energy
    levels or shells.

C
8
How To Draw Bohr Diagrams
  • 6) Add the electrons.
  • Carbon has 6 electrons.
  • The first shell can only hold ?

C
9
How To Draw Bohr Diagrams
  • 6) Add the electrons.
  • Carbon has 6 electrons.
  • The first shell can only hold 2 electrons.

C
10
How To Draw Bohr Diagrams
  • You need to add 4 more so these go in the 2nd
    shell.
  • The 2nd shell can hold up to ?

C
11
How To Draw Bohr Diagrams
  • You need to add 4 more so these go in the 2nd
    shell.
  • The 2nd shell can hold up to 8 electrons the 3rd
    shell can hold 18, but the elements in the first
    few periods only use 8 electrons.

C
12
How To Draw Bohr Diagrams
  • 7) Check your work Count your electrons per
    shell and your total electrons!

C
13
Bohr Diagrams Practice
  • Try drawing Bohr diagram for each of the
    following elements on your own
  • H
  • He
  • O
  • Al
  • Ne
  • K

C
14
Bohr Diagrams Practice
  • Try drawing Bohr diagram for each of the
    following elements on your own
  • H 1 electron
  • He
  • O
  • Al
  • Ne
  • K

H
15
Bohr Diagrams Practice
  • Try drawing Bohr diagram for each of the
    following elements on your own
  • H
  • He - 2 electrons
  • O
  • Al
  • Ne
  • K

He
16
Bohr Diagrams Practice
  • Try drawing Bohr diagram for each of the
    following elements on your own
  • H
  • He
  • O - 8 electrons
  • Al
  • Ne
  • K

O
17
Bohr Diagrams Practice
  • Try drawing Bohr diagram for each of the
    following elements on your own
  • H
  • He
  • O
  • Al - 13 electrons
  • Ne
  • K

Al
18
Bohr Diagrams Practice
  • Try drawing Bohr diagram for each of the
    following elements on your own
  • H
  • He
  • O
  • Al
  • Ne - 10 electrons
  • K

Ne
19
Bohr Diagrams Practice
  • Try drawing Bohr diagram for each of the
    following elements on your own
  • H
  • He
  • O
  • Al
  • Ne
  • K - 19 electrons

K
20
Lewis Dot Diagrams
  • The electrons in the outermost shell are called ?

21
Lewis Dot Diagrams
  • The electrons in the outermost shell are called
    valence electrons.

22
Lewis Dot Diagrams
  • The electrons in the outermost shell are called
    valence electrons.
  • Lewis Dot Diagrams are abbreviated Bohr Diagrams
    that show just these outermost electrons, e.g.

23
Valence Electrons and Families
  • Note that both hydrogen (H) and potassium (K)
    have just ? electron in their outermost shell.
  • Note also that these elements are both found in
    the ? column of the periodic table.
  • This is not a coincidence!

24
Valence Electrons and Families
  • Note that both hydrogen (H) and potassium (K)
    have just 1 electron in their outermost shell.
  • Note also that these elements are both found in
    the ? column of the periodic table.
  • This is not a coincidence!

25
Valence Electrons and Groups
  • Note that both hydrogen (H) and potassium (K)
    have just 1 electron in their outermost shell.
  • Note also that these elements are both found in
    the 1st column of the periodic table.
  • This is not a coincidence!

26
Valence Electrons and Groups
  • All elements in the same group (column) have the
    same number of electrons in their outermost
    shell.
  • It is these electrons that determine the behavior
    of the element, including how it reacts with
    other elements and how it forms ions.

27
Valence Electrons and Groups
  • Lets look at these groups or families in more
    detail. . . .

28
ALKALI METALS
  • 1 valence electron
  • (Hydrogen is not officially a member)
  • Soft and silvery metals
  • Very reactive, esp. with water

29
ALKALINE EARTH METALS
  • 2 valence electrons
  • White and malleable
  • Reactive, but less so

30
TRANSITION METALS
  • (the Groups in the middle)

31
BORON FAMILY
  • 3 valence electrons
  • Most are metals
  • Boron is a metalloid.

32
CARBON FAMILY
  • 4 valence electrons
  • Contains metals, metalloids, and a non-metal
    carbon (C)

33
NITROGEN FAMILY
  • 5 valence electrons
  • Contains metals, metalloids, and non-metals

34
OXYGEN FAMILY
  • 6 valence electrons
  • Mostly non-metals
  • Reactive

35
Halogens
  • 7 valence electrons
  • All are non-metals
  • Very reactive

36
Noble Gases
  • Full outer shell
  • Exist as gases
  • Not reactive with other elements
  • Do not form ions.

37
The Why of Ions
  • The Noble Gases do not react and do not form ions
    because they already have what all atoms want
    full outer shells.

38
The How of Ions
  • Atoms will either gain electrons to fill their
    outer shell (as in the case of the non-metal
    chlorine)

39
The How of Ions
  • or lose electrons to go down to their last full
    shell (as in the case of the metal sodium)

40
Tune in next time. . . .
  • More details on the formation of ions will be
    revealed tomorrow.
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