Unit 5: Periodic Table

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• Unit 5 Periodic Table
• Part 3 The 18 Groups of the Modern Periodic Table

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Alkali Metals

• Group 1 or 1A
• 1 valence electron
• give up 1 valence electron when bonding to to
  become more stable (full valence shell).
  Therefore, they become 1 ions.

• Alkali means ashes. Sodium and potassium are
  present in the ashes of burned plants.

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Alkali Metals cont

• Very reactive. Will react with water and air!
  (Stored in oil.)
• Soft enough to be cut by a butter knife.
• The members of this group are (Not Hydrogen)
• Li He2s1
• Na Ne3s1
• K Ar4s1
• Rb Kr5s1
• Cs Xe6s1
• Fr Rn7s1

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Placement on Periodic Table

• Li 1s22s1
• Na 1s22s22p63s1
• K 1s22s22p63s23p64s1
• Li, Na, K all have 1 valence e-
• All are found in group 1 or IA
• Li in pd. 2 Na in pd. 3 K in pd. 4

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Alkaline Earth Metals

• Group 2 or 2A.
• 2 valence electrons
• give up 2 valence electrons when bonding to
  become more stable. (full valence shell)
  Therefore they become 2 ions.
• Obtained from alkaline earths. Earths were
  substances unchanged by fire.

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Alkaline Earth Metals cont

• Alkaline Earth Metals are also very reactive.
  (Not as reactive as group I or 1A)
• Higher densities and melting points than the
  alkali metals.
• Found in mineral deposits (Earths).

The members of this group are Be He2s2 Mg
Ne3s2Ca Ar4s2 Sr Kr5s2
Ba Xe6s2 Ra Rn7s2
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Transition Metals

• Groups 3 12
• Play an important role in living organisms, are
  extremely valuable as strong structurally useful
  materials.
• Vary greatly in properties and abundance.
• Most have high densities and high melting points.
• Number of valence electrons varies, therefore
  ionic charge varies.

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Inner Transition Metals

• Lanthanide and Actinide Series elements
• (f block elements)
• Properties similar to Transition Metals
• Many are man-made
• Many are naturally radioactive (Large, unstable
  nuclei. Ratio of neutrons to protons is high)
• Have two valence electrons. (after 6s2, 7s2)

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The Boron Group

• Group 13 or 3A.
• 3 valence electrons
• give up 3 valence electrons when bonding to
  become more stable. (full valence shell)
  Therefore they will become 3 ions.
• The members of this group are
• B He2s22p1
  Al Ne3s23p1
• Ga Ar4s24p1
  In Kr5s25p1
• Tl Xe6s26p1

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Placement on Periodic Table

• B 1s22s22p1
• Al 1s22s22p63s23p1
• Ga 1s22s22p63s23p64s23d104p1
• B, Al, Ga all have 3 valence e-
• All are found in group 13 or IIIA
• B in pd. 2 Al in pd. 3 Ga in pd. 4

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The Carbon Group

• Group 14 or 4A.
• 4 valence electrons
• give up, share or accept 4 valence electrons to
  become more stable. (full valence shell)
  Therefore they can become 4 or 4 ions.
• The members of this group are
• C He2s22p2
  Si Ne3s23p2
• Ge Ar4s24p2
  Sn Kr5s25p2
• Pb Xe6s26p2

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The Nitrogen Group

• Group 15 or 5A.
• 5 valence electrons
• accept 3 more electrons to become stable. (full
  valence shell) Therefore they become 3 ions.
• The members of this group are
• N He2s22p3
  P Ne3s23p3
• As Ar4s24p3
  Sb
  Kr5s25p3
• Bi Xe6s26p3

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Placement on Periodic Table

• N 1s22s22p3
• P 1s22s22p63s23p3
• As 1s22s22p63s23p64s23d104p3
• N, P, As all have 5 valence e-
• All are found in group 15 or VA
• N in pd. 2 P in pd. 3 As in pd. 4

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The Oxygen Group

• Group 16 or 6A.
• These elements have 6 valence electrons. They
  will accept 2 more to become more stable. (full
  valence shell) Therefore they become 2 ions.
• The members of this group are
• O He2s22p4 S
  Ne3s23p4
• Se Ar4s24p4
  Te Kr5s25p4
• Po Xe6s26p4

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The Halogen Group

• Group 17 or 7A.
• These elements have 7 valence electrons. They
  will accept 1 more to become more stable. (full
  valence shell) Therefore they become 1 ions.
• Comes from the Greek word which means salt
  former.

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The Halogen Group

• The Halogens are very reactive nonmetals and
  exist in elemental form as diatomic molecules.
• (F2, Cl2, Br2, I2, At2)
• The members of this group are
• F He2s22p5
• Cl Ne3s23p5
• Br Ar4s24p5
  I Kr5s25p5
• At Xe6s26p5

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Placement on Periodic Table

• F 1s22s22p5
• Cl 1s22s22p63s23p5
• Br 1s22s22p63s23p64s23d104p5
• F, Cl, Br all have 7 valence e-
• All are found in group 17 or VIIA
• F in pd. 2 Cl in pd. 3 Br in pd. 4

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The Noble Gases

• Group 18 or 8A.
• These elements have 8 valence electrons. (Except
  helium, which has 2) They are already stable, so
  they do not accept or receive electrons. They do
  not typically form ions.
• These elements are very stable.

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The Noble Gases

• Members of this group include
• Helium He 1s2
• Neon Ne 1s2 2s22p6
• Argon Ar 1s2 2s22p6 3s23p6
• Krypton Kr 1s2 2s22p6 3s23p64s23d104p6
• Xenon Xe 1s2 2s22p6 3s23p64s23d104p6
  5s24d105p6
• Radon Rn 1s2 2s22p6 3s23p64s23d104p6
  5s24d105p66s24f145d106p6

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Hydrogen (The one
and only!)

• Has one valence electron, but is not an Alkali
  metal.
• Hydrogen is a nonmetal that exists as a gas under
  normal conditions.
• Colorless, odorless, and composed of H2
  molecules. (Diatomic, like the halogens)
• Most of the Earths hydrogen is combined with
  oxygen as water and carbon in organic compounds
  called hydrocarbons.

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1 IA
Oxygen Group
Halogens
18 VIIIA
? Alkali Metals
Nitrogen Group
2 IIA
17 VIIA
? Alkaline Earth Metals
13 IIIA
14 IVA
15 VA
16 VIA
Carbon Group
1 2 3 4 5 6 7
1 2 3 4 5 6 7
Boron Group
Transition Metals
3
8
9
11
12
4
7
5
6
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Noble Gases ?
Lanthanides ?
Actinides ?