Periodic%20Table:%20Bell%20Ringer

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Periodic Table Bell Ringer

• What does a period and a group refer to on the
  periodic table?
• What period and group is Bromine on?
• What element is on period 5 and group 10?
• For homework, how did you classify the elements
  on the periodic table?

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Periodic Table
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Metallic Properties
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Non-metallic Properties
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History of the Periodic Table

• Dmitri Mendeleev
• Russian chemists and teacher
• When organized elements into groups by similar
  chemical properties,
• he observed the periods increasing in atomic
  mass.
• His organization system was successful at
  predicting undiscovered elements.
• Do you observe any inconsistencies with his
  organization system?

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History of Periodic Table

• Henry Moseley
• British Physicists
• Observed that when elements were placed in groups
  by chemical properties, the periods consistently
  increased by atomic number.
• Currently accepted organization system for
  elements.

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Bell Ringer Periodic Table

• 1. How is the current periodic table arranged?
• 2. Classify the following properties as metallic
  or non-metallic.
• a. ductile b. low density c. high luster
  d. insulator
• 3. What element is on period 3 group 16?
• 4. Circle the elements below that have similar
  chemical properties
• Carbon (C) Nitrogen (N) Silicon (Si) Boron
  (B)

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Organization of Periodic Table

• Why do elements in the same group have similar
  chemical properties?

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Valence Electrons

• Electrons in the highest energy level of an
  elements atom.
• Calculate using short-hand electron
  configuration.
• Determines the chemical reactivity of an element.

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Periodic Table Bell Ringer

• 1. a. What period and group is Aluminum on?
• b. What element is in period 4 group 2 ?
• 2. Circle the elements below that have similar
  chemical properties.
• Carbon (C), Nitrogen, (N), Silicon (Si), Boron
  (B)
• 3. What are valence electrons?
• 4. Why is it important to know the number of
  valence electrons an element can have?

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Short-Hand Electron Configuration

• Short -hand configuration targets valence
  electrons
• Ex.
• Sulfur (S) Ne 2s22p4 6 valence
  electrons

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Valence Electrons Worksheet Key

• 1. 7 ve- 11. 1ve-
• 2. 5ve- 12. 2ve-
• 3. 2ve- 13. 4ve-
• 4. 5ve- 14. 7ve-
• 5. 2ve- 15. 6ve-
• 6. 8ve- 16. 2ve-
• 7. 1ve- 17. 3ve-
• 8. 2ve- 18. 1ve-
• 9. 2ve- 19. 8ve-
• 10. 6ve- 20. 2ve-

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Organization of Periodic Table

• Why do elements in the same group have similar
  chemical properties?

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Periodic Table Lab Valence Electrons
Lab grps grp 1 ve- grp 2 ve- grp 3-12 ve- grp 13 ve- grp 14 ve- grp 15 ve- grp 16 ve- grp17 ve- grp18 ve-
A
B
C
D
What can be concluded from the data table?
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Periodic Table Valence Electrons
Lab grps grp 1 ve- grp 2 ve- grp 3-12 ve- grp 13 ve- grp 14 ve- grp 15 ve- grp 16 ve- grp17 ve- grp18 ve-
A 1 2 2 3 4 5 6 7 8
B 1 2 2 3 4 5 6 7 2
C 1 2 2 3 4 5 6 7 8
D 1 2 2 3 4 5 6 7 8
What can be concluded from the data table?
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Common Periodic Table Groups
Periodic Groups Group Valence Electrons Chemical Properties
Alkali Metals 1 1 ve- Highly Reactive metals Only needs to lose 1 ve- to reach STABILITY. Depends on lower energy level that is filled.
Alkaline-Earth Metals 2 2ve- Reactive Only needs to lose 2 ve- to reach STABILITY. Depends on lower energy level that is filled.
Transitional Metals 3-12 2ve- Reactive Varies in amount of valence electrons lost to reach STABILITY. Depends on lower energy level that is filled.
Halogens 17 Highly Reactive non-metals. Only needs to gain 1 ve- to reach STABILITY. Depends on filling up outer energy level.
Noble Gases 18 Inert non-metal gases. Not reactive elements. Very STABLE elements because outermost energy level is filled, 8ve. Exception 2 ve for He.
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Chemical Stability

• Metals
• Will lose ve- to reach stability.
• Form cations ( charged atoms)
• Non-metals
• Will gain ve- to reach stability.
• Form anions (- charged atoms)

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Chemical Stability

• Determine what type of ion each element below
  would form to reach maximum stability.
• a. Sodium Na1
• b. Oxygen O2-
• c. Argon Ar
• d. Phosphorus P3-
• e. Chromium Cr2

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Bell Ringer Chemical Stability

• Write down what comes to mind when you think
  about chemical stability for elements.
• 2. Label your periodic table with the following
  groups
• Alkali metals (Group 1)
• Alkaline earth metals (Group 2)
• Halogens (Group 17)
• Noble gases (Group 18)
• Transitional metals (Group 3-12)

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Periodic Table and Groups
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Ions and Chemical Stability Lab

• In pairs, look at 16 different elements and
  answer the following questions
• Metal or non-metal
• Neutral, anion, or cation.
• Symbol and specific charge if needed.
• neutral if element is naturally stable (noble
  gas)
• anion non-metal not naturally stable
• cation metals

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Size of an Ion
Use the diagram below to determine what happens
to the size of an atom when it becomes an ion.
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Size of a Cation
A cation is smaller than its parent atom. Why?
Because metals will lose an energy level in the
process of becoming a cation.
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Size of a Cation
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Size of an Anion
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Size of an Anion
A anion is larger than its parent isotope. Why?
Repulsion force increases as more electrons are
added to the outer most energy level. Swells
the energy level.
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Size of an Anion
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Size of Ions

• Circle the atom that is larger in size.
• Ca or Ca2
• S or S2-
• Circle the atom that is smaller in size.
• a. Al or Al3
• b. N or N 3-

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Bell Ringer Chemical Stability

• a. Most stable group on periodic table?
  Explain.
• b. Most reactive metallic group? Explain.
• c. Most reactive non-metallic group?
  Explain.
• 2. Predict what type of ion each element below
  would form to reach maximum stability.
• a. Cesium b. Selenium c.
  Helium
• 3. Identify which atom is larger in each example
  below.
• a. Al or Al3 b. Br or Br 1-

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Periodic Trends
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Periodic Properties and Trends

• Atomic Radius
• -Size of an atom.
• Distance from nucleus to highest energy level for
  that atom. (picometers, pm).
• Ionization Energy
• Energy required to remove an electron from an
  atom.
• Energy required to form a cation.

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Periodic Trends Atomic Radius
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Periodic Trends Atomic Radius
Across a Period Down a Group
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Periodic Trends Ionization Energy
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Periodic Trends Ionization Energy
Across a Period Down a Group
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Exit Slip

• Use your graph on atomic radius and ionization
  energy answer these questions
• Rank the following elements from largest to
  smallest in size. Explain your results.
• Ar, Mg, S Al
• Rank the following elements from smallest to
  largest in ionization energy. Explain your
  results.
• Ne, Ar, He

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Periodic Table

• Representative Elements tall groups .
• Transitional Elements short groups.

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Hydrogen Lab