3.2 using the periodic table. objectives relate an element’s valence electron structure to its...

3.2 Using the Periodic Table

Objectives Relate an element’s valence

electron structure to its position in the periodic table.

Use the periodic table to classify an element as a metal, nonmetal, or metalloid.

Compare the properties of metals, nonmetals, and metalloids.

New Vocabulary to Look for… Period Group Noble gas Metal Transition element Lanthanide Actinide Nonmetal Metalloid semiconductor

Relationship of the Periodic Table to Atomic Structure Periodic tables contain a vast array of

information on the elements. You will learn to use the periodic table

to gather information about the elements and group of elements we are studying.

Modern periodic table is arranged according to increasing atomic number.

What information does the atomic number tell us?

Periods and Groups The horizontal rows of the periodic

table are called periods. The vertical columns are referred

to as groups. Groups are also called families of

elements. Elements in the same group have

similar properties.

Atomic Structure of Elements Within a Period Each period starts with a group 1

element, which has 1 valence electron. As you move across a period the

number of valence electrons increases. Moving from 1, 2, 13, 14, 15, 16, 17, 18.

Group 1 elements have one electron at a higher energy level than the noble gas of the preceding period.

Atomic Structure of Elements Within a Group The number of valence electrons

can be predicted using the periodic table. Group 1 has 1 valence electron Group 2 has 2 valence electrons Groups 13-18 have the second digit of

valence electrons. 13 has 3 valence electrons 14 has 4 valence electrons Fig. 3.8 p. 98

Noble Gases Group 18 have the periodic table. They have 8 valence electrons,

except for He which only has 2 Full energy levels Generally unreactive or inert Ne, He, Ar

Noble Gases

Halogens Greek meaning “salt former” Form salt like compounds Group 17 7 valence electrons F, Cl, Br, I

Alkali Metal Group 1 (except H) 1 valence electron Li, Na, K

Alkali Metals

Alkaline Earth Metals Group 2 2 valence electrons Be, Mg, Ca, Ba

Valence Electrons-Properties Valence electrons help to

determine the physical and chemical properties

Groups have similar properties b/c they have the same number of valence electrons

Fig. 3.9 p. 99 Electrons in Energy Levels-Group 16

Physical States and Classes of Elements

Physical States of the Elements The physical states of the elements are

show on the periodic table on p. 92-93. Most elements are solids at room

temperature Only two are liquids. What are they?

A.B.

All the gases except hydrogen are in the upper right corner of the table. List some.

Gallium

Classifying Elements Elements are classified into groups

Metals Nonmetals Metalloids

Majority of elements are metals Left side and center

Nonmetals Upper right corner

Metalloids Along the boundary b/t metals and nonmetals

Metals Have luster Conduct heat Good conductors of electricity Most have high boiling pts. Malleable Ductile Most are solid Only one metal is in the liquid state.

Metals Most are located in Groups 1-13 Transition Elements- Elements in

Group 3-12 (all metals) Iron (Fe), nickel (Ni), Copper (Cu), Zinc

(Zn) Some of period 7 are synthetic and

radioactive The transition elements have a less

predictable behavior and properties than the other metals

Transition Elements

Transition Elements

Transition Elements

Metals Elements with the atomic numbers

58-71 and 90-103 are placed below the main table

If they were part of the main table it would be extremely wide

Known as the inner transition elements

Many were unknown in Mendeleev’s time

Inner Transition Elements

Lanthanides First series of inner transition

elements 14 elements 58-71 Also called rare earth elements-

abundance 0.01% All have similar properties

Actinides Second series of inner transition

elements 90-103 Radioactive None beyond uranium occur in

nature Unpredictable-complex structures

Nonmetals Nonmetals are abundant in nature Oxygen and nitrogen make up 99%

of our atmosphere Carbon is found in more

compounds than all the other elements combined.

Nonmetals Don’t conduct electricity Poor conductors of heat Brittle when solid Many are gases at room temp. Solids lack luster Melting points and boiling points are low Table 3.5 p. 105 Properties of Metals

and Nonmetals

Metalloids Have properties of both metals and

nonmetals Located between the metals and

nonmetals Si, Ge and As are semiconductor

Does not conduct electricity as well as a metal, but does better than a nonmetal

Si semiconductors made the computer revolution possible.

Atomic Structure of Metals, Metalloids and Nonmetals

Differences occur b/c of the different arrangements of electrons

Number, arrangement of valence electrons along with how tightly they are held in the atom determines the behavior.

Valence electrons in Metals Loosely bound Free to move in the solid metal Easily lost Freedom of movement =

conductivity

Valence electrons in Nonmetals and Metalloids

Tightly held Not easily lost

Chemical Reactions and Electrons

Metals tend to lose valence electrons

Nonmetals tend to share or gain electrons

General Properties and Uses of Metals, Nonmetals and Metalloids1. Familiar Metals

Jewelry, figurines, electrical circuits2. Some Lanthanides and Actinides

Compounds of europium and ytterbium – picture tubes of TV

Neodymium – high powered lasers3. Carbon and Some Other Nonmetals

Carbon: Coal, natural gas, oil, graphite, diamonds Bromine and Iodine – halogen lamps

4. Metalloids Silicon – electronic devices

Page 106-107

Semiconductors Metalloids that do not conduct

electricity as well as metals, but better than nonmetals

Uses Television Computer Handheld electronic games Calculators

Semiconductors –Electrons and Electricity An electrical current is flowing electrons. Metals conduct electricity well because

the electron are not tightly held by the nucleus and are therefore free to move. Copper wire

At room temperature Si is not a good conductor. Its four electrons are tightly held by the nucleus. In order to make it a good conductor it must

be doped with another element.

Silicon (Si)

Doping of Si By adding small amounts of P to Si

a good conductor is created. P has five valence electrons. This

adds an extra electron which is free to move = electrical conductivity.

n-type semiconductor (negatively charged)

Doping of Si By adding B to Si a good conductor

is created B has three valence electrons. The

shortage of electrons creates “holes” in which the electrons can move = electrical conductivity.

p-type semiconductor (positively charged)

Diodes The combination of n-type and p-

type semiconductors is a diode. Permits electrical flow in only one

direction Negative terminal to positive terminal

Transistors Key components in electrical

circuits, amplifying the electrical signal. npn-junction pnp-junction

Review

1. Where are the halogens, noble gases, alkali metals, alkaline earth metals, lanthanide and the actinides located? Give me an example of each?

2. What are the characteristics of a metal, nonmetal and metalloid?

3. How many valence electrons does Li have?

Using the Periodic Table