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11 & 12
T H E PE R I O D I C TA B L E A N D E L E M E N T S
ORGANIZING BY PROPERTIES:• In 1869, Dmitri Mendeleev published
the first periodic table– Organized by
____________________________________________________________
– Not all rows contained the same number of elements
– Missing elements were indicated by (-) because some elements hadn’t been discovered but he was able to predict the physical and chemical properties of them
ORGANIZING BY PROPERTIES:
• Define periodic law:
• E.g. all of group 1A is reactive in water
ORGANIZING THE PERIODIC TABLE:• Sections of the Periodic Table
– (1)
– (2)
– (3)
– (4)
• Groups of the Periodic Table
• 1A (1) –
• 2A (2) –
• 6A (16) –
• 7A (17) –
• 8A (18 )–
PERIODIC TRENDS:
• In this chapter, we will explain observed trends in…
–Sizes of atoms and ions
– Ionization energy
–Electron Affinity
–Electronegativity
SIZES OF ATOMS• What happens to the radius of an atom as
you go from left to right across the periodic table? Why?
• What happens to the radius of an atom as you go from the top to the bottom of the periodic table? Why?
EXAMPLE #1: SIZE OF ATOMS
• Which has the larger radius: Nickel or Selenium
• Which has the larger radius: Oxygen or Sulfur
• Which has the smaller radius: Sodium or Calcium
• Which has the smaller radius: Copper or Zinc
SIZES OF IONS:
• Ionic size depends upon:–Nuclear charge (+,-)
–The number of electrons
–The orbitals in which electrons reside (s, p, d, f)
SIZES OF IONS: CATIONS• By looking at the image,
describe the difference between the neutral and the corresponding cations:
• As the atom becomes more positive what is happening? Why?
SIZES OF IONS: ANIONS• By looking at the image,
describe the difference between the neutral and the corresponding anions:
• As the atom becomes more negative what is happening? Why?
SIZES OF IONS:
• What happens to ALL ions as you go down a column? Why?
REVIEW: WRITE THE ELECTRON CONFIGURATIONS• Write the electron configuration for the
following:
• Fluorine Ion
• Neon
• Sodium Ion
• What do you notice about these three electron configurations?
EXAMPLE PROBLEM: SIZES OF IONS
• Which has the larger radius: Te2- or Te
• Which has the larger radius: Sr2+ or Sr
• Which has the smaller radius: S2- or Br-
• Which has the smaller radius: Cs1+ or Cs2+ or Cs
IONIZATION ENERGY:• What is ionization energy?
• What is first ionization energy? Second?
IONIZATION ENERGY:• It requires ______________ energy to remove each successive electron
• When all valence electrons have been removed, the ionization energy takes a quantum leap
• REVIEW: What is quantum?
IONIZATION ENERGY:• What happens to the ionization
energy of an atom as you go from left to right across the periodic table? Why?
• What happens to the ionization energy of an atom as you go from the top to the bottom of the periodic table? Why?
ANOMALIES IN IONIZATION ENERGY:• Why does an anomaly occur
between groups 2A and 3A?
ANOMALIES IN IONIZATION ENERGY: • Why does an anomaly occur between
groups VA and VIA?
EXAMPLE PROBLEM: IONIZATION ENERGY• Which has the greatest ionization energy: Nitrogen or Oxygen
• Which has the greatest ionization energy: Mg or Sr
ELECTRON AFFINITY:• What is electron affinity?
• Why does electron affinity increase as you move from left to right across the periodic table?
• Why does electron affinity decrease as you move from bottom to top of the periodic table?
ELECTRONEGATIVITY:• What is electronegativity?
• Why does electronegativity increase when you move from left to right across the periodic table?
• Why does electronegativity decrease when you move from bottom to the top of the periodic table?
EXAMPLE PROBLEM: ELECTRON AFFINITY & ELECTRONEGATIVITY1. Which has the greatest electron affinity: Zn or As
2. Which has the greatest electron affinity: Se or O
3. Which has the least electronegativity: Ag or Sb
4. Which has the least electronegativity: Ba or Mg
FAMILIES OF THE PERIODIC TABLE:
1. Alkali Metals
2. Alkaline Earth Metals3. Transition Metals4. Metalloids
5. Nitrogen Family
6. Oxygen Family7. Halogens8. Noble Gases
PROPERTIES OF METALS:• REVIEW: What are things we already know
about metals?
• ¾ of all known elements are metals
• Why do metals have a low ionization energy?
• Metallic bonds– What does it mean when electrons are
delocalized?
ALKALI METALS:
• What makes the alkali metals special?
• Why are sodium and potassium important?
ALKALINE EARTH METALS:
• What makes the alkaline earth metals special?
• Magnesium and calcium are most important… Why?
ALUMINUM:
• What makes aluminum special?
TRANSITION ELEMENTS:• What makes the transition elements special?
USES OF SPECIFIC TRANSITION METALS:• What are some ways copper is
used?
• What are some ways silver is used?
• What is an alloy? Why are the advantages of using an alloy vs pure metal?
METALLOIDS:
• Why are metalloids special?
• Why is Silicon important?
METALLOIDS AS SEMICONDUCTORS:• Certain impurities can
______________________ conductivity.
– These are called _____________________________.
• Impurities affect silicon in two ways– N-type (acceptor) – boron, aluminum,
nitrogen, gallium, indium
– P-type (donor) – phosphorus, arsenic, antimony, bismuth, lithium
– Junctions: used when you want a flow of electricity in one direction but NOT in the other direction
CARBON – THE ELEMENT OF LIFE:• What makes carbon special?
• What is an allotrope?
NITROGEN FAMILY:
• What makes the nitrogen family special?
NITROGEN FAMILY: PHOSPHORUS• There are 4 different types of
phosphorus:
• What makes white special?
• What makes red special?
OXYGEN FAMILY:
• Why is oxygen special?
• Why is sulfur special?
HALOGEN FAMILY:•What makes the halogens
special?
NOBLE GASES:
• What makes the noble gases special?