Atoms and the Periodic table

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Slide 71

Learning Check

Identify each of the following elements as

1) metal 2) nonmetal 3) metalloid

A. sodium

B. chlorine

C. silicon

D. iron

E. carbon

Slide 72

Solution

Identify each of the following elements as

1) metal 2) nonmetal 3) metalloid

A. sodium 1 metal

B. chlorine 2 nonmetal

C. silicon 3 metalloid

D. iron 1 metal

E. carbon 2 nonmetal

Slide 73

Learning Check

Match the elements to the description.

A. Metals in Group 4A(14)

1) Sn, Pb 2) C, Si 3) C, Si, Ge, Sn

B. Nonmetals in Group 5A(15)

1) As, Sb, Bi 2) N, P 3) N, P, As, Sb

C. Metalloids in Group 4A(14)

1) C, Si, Ge, 2) Si, Ge 3) Si, Ge, Sn, Pb

Slide 74

Solution

Match the elements to the description.

A. Metals in Group 4A (14)

1) Sn, Pb

B. Nonmetals in Group 5A(15)

2) N, P

C. Metalloids in Group 4A(14)

2) Si, Ge

Slide 75

Exploration of the Periodic Table/ Periodic Reactivity Trends

Run the following web animations/movies.

3.4b:

3.6:

Slide 76

Figure 3.11: Modern periodic table of elements.

Slide 77

Slide 78

Three elements: sulfur (bottom) and diamond (which is carbon, top left), which are main-group nonmetals; and gold (top right), a transition metal.

Slide 79

Chapter Outline

• The Octet Rule

The noble gases of Group VIIIA do not typically form compounds with other atoms.

Atoms with eight valence electrons are particularly stable, an observation called the octet rule.

Atoms form bonds with other atoms to achieve a valence octet.

Slide 80

Electronic Configuration of Noble Gases

Slide 81

Chapter Outline

Lewis Dot Structures

The number of valence electrons is equal to the group number for most of the main group elements.

In Lewis dot structures, the chemical symbol represents the nucleus and the core electrons and dots represent the valence electrons.