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?