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ORGANIZING THE ELEMENTS

3/8/16 Objective:

Students will be able to describe how

elements belonging to a group or period are

interrelated on the periodic table.

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6.1 Organizing the Elements

In a self-service store, the products are grouped according to similar characteristics. With a logical classification system, finding and comparing products is easy. You will learn how elements are arranged in the periodic table and what that arrangement reveals about the elements.

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Organizing the Elements > Searching For an Organizing Principle

Elements are organized using their

properties. Chlorine, bromine, and iodine

have very similar chemical properties.

They are all in group 7A.

6.1

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Organizing the Elements >

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Mendeleev’s Periodic Table

Mendeleev’s Periodic Table

How did Mendeleev organize his

periodic table?

6.1

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Organizing the Elements > Mendeleev’s Periodic Table

Mendeleev arranged the elements in his

periodic table in order of increasing

atomic mass.

This first table was used to predict the

properties of undiscovered elements. The

presence of Gallium was predicted based on

this table

Problem- some elements didn’t line up with

other elements that had similar properties

Example: I and Te were out of place

6.1

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Organizing the Elements > Mendeleev’s Periodic Table

An Early Version of Mendeleev’s Periodic Table

6.1

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Organizing the Elements >

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The Periodic Law

The Periodic Law

How is the modern periodic table

organized?

Moseley developed the organization

used in the modern periodic table.

6.1

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Organizing the Elements > The Periodic Law

In the modern periodic table elements are

arranged in order of increasing atomic

number.

Atomic number = # of protons

Protons are in the nucleus

Nucleus has a positive charge

6.1

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Organizing the Elements > The Periodic Law

The periodic law: When elements are arranged in order of increasing atomic number, there is a periodic repetition of their physical and chemical properties.

• The properties of the elements within a period change as you move across a period from left to right.

• The pattern of properties within a period repeats as you move from one period to the next.

6.1

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Organizing the Elements > Groups and Periods

Remember that:

a group is a vertical column

a period is a horizontal row

Groups have similar properties because they have the same number of valence electrons

For groups 1A-8A the number of valence electrons matches the group number (with the exception of He)

For groups 1B-8B the number of valence electrons is 1 or 2 and must be found using electron configurations.

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Organizing the Elements > Metals, Nonmetals, and Metalloids

Three classes of elements are metals,

nonmetals, and metalloids.

Across a period, the properties of elements

become less metallic and more nonmetallic.

Use the following slides to help you color in

the 3 classes of elements using colored

pencils.

6.1

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Organizing the Elements > Metals, Nonmetals, and Metalloids

Metals, Metalloids, and Nonmetals in the Periodic Table

6.1

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Organizing the Elements > Metals, Nonmetals, and Metalloids

Metals, Metalloids, and Nonmetals in the Periodic Table

6.1

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Organizing the Elements > Metals, Nonmetals, and Metalloids

Metals, Metalloids, and Nonmetals in the Periodic Table

6.1

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Organizing the Elements > Metals, Nonmetals, and Metalloids

Metals, Metalloids, and Nonmetals in the Periodic Table

6.1

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Organizing the Elements > Metals, Nonmetals, and Metalloids

Metals

Metals are good conductors of heat and electric

current.

• 80% of elements are metals.

• Metals have a high luster, are ductile, and are

malleable.

6.1

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Organizing the Elements > Metals, Nonmetals, and Metalloids

Uses of Iron, Copper, and Aluminum

6.1

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Organizing the Elements > Metals, Nonmetals, and Metalloids

Uses of Iron, Copper, and Aluminum

6.1

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Organizing the Elements > Metals, Nonmetals, and Metalloids

Uses of Iron, Copper, and Aluminum

6.1

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Organizing the Elements > Metals, Nonmetals, and Metalloids

Nonmetals

In general, nonmetals are poor conductors of heat and electric current.

• Most nonmetals are gases at room temperature.

• A few nonmetals are solids, such as sulfur and phosphorus. These solids are brittle.

• One nonmetal, bromine, is a dark-red liquid.

6.1

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Organizing the Elements > Metals, Nonmetals, and Metalloids

Metalloids

A metalloid generally has some properties of

metals and some properties of nonmetals.

The behavior of a metalloid can be controlled by

changing conditions.

A metalloid may be brittle, lustrous, and a good

conductor, like silicon.

6.1

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Organizing the Elements > Metals, Nonmetals, and Metalloids

If a small amount of boron is mixed with silicon,

the mixture is a good conductor of electric

current. Silicon can be cut into wafers, and used

to make computer chips.

6.1

6.1 SECTION QUIZ

1. The modern periodic table has elements

arranged in order of

colors.

melting and boiling points.

increasing atomic mass.

increasing atomic number.

6.1 SECTION QUIZ

2. Mendeleev arranged the elements in his

periodic table in order of increasing

atomic number.

atomic mass.

number of electrons.

number of protons

6.1 SECTION QUIZ

3. Which one of the following is NOT a general

property of metals?

poor conductor of heat and electricity

malleability

having a high luster

ductility

CLASSWORK!

Reading Assignment: Sec 6.1

Written Assignment: p. 166, #1-7

DO NOW ACTIVITY

This will be collected and count as part of your

classwork/participation grade for today.

HOMEWORK CHECK!

Page 166, #1-7 1. Chemists used the properties of elements to sort them into

groups.

2. Mendeleev used atomic mass to organize his periodic table.

3. The elements are arranged in order of increasing atomic number on the modern periodic table.

4. The three broad classes of elements are: metals, metalloids, and nonmetals.

5. a. metal b. metalloid c. nonmetal d. metal

6. B

7. Lithium, Potassium, Rubidium, Cesium, or Francium all have similar properties to Sodium.

HOW ARE ELEMENTS FURTHER CLASSIFIED ON

THE PERIODIC TABLE?

Just like the Atomic Number of an elements

can be similar to your SSN, and the Electron

Configuration of an element is similar to your

fingerprints, the periodic table can tell us

information about each element, just like a

driver’s license or ID card.

CLASSIFYING ELEMENTS SECTION 6.2

3/8/16

Students will understand the correlation

between valence electrons, electron

configuration, and element organization of

the periodic table.

FOUR MAIN CATEGORIES OF ELEMENTS

Transition Metals

Inner Transition Metals

Noble Gases

Representative Elements

USE THIS TO HELP OUTLINE THE CATEGORIES ON YOUR PERIODIC TABLE

FOUR MAIN CATEGORIES OF ELEMENTS

Transition Metals: Group B elements that are

usually displayed in the main body of the

periodic table

metallic elements

outermost s & d sublevels contain electrons

Contain either 1 or 2 valence electrons

Examples of elements: Tungsten (W), Vanadium (V),

Gold (Au), Nickel (Ni)

FOUR MAIN CATEGORIES OF ELEMENTS

Inner transition metals: the elements that

appear below the main body of the periodic

table.

metallic elements

outermost s & nearby f sublevel contain electrons

Lanthanides and actinides

Actinides are all radioactive

Examples of elements: Cerium (Ce), Europium (Eu),

Plutonium (Pu), Californium (Cf)

FOUR MAIN CATEGORIES OF ELEMENTS

Noble Gases- the elements in Group 8A of the periodic table.

s & p sublevels filled

8 valence electrons: ns2 ….np6

Except He, which has 2 valence : 1s2

Inert (not reactive) because of full outer shell of electrons (8 valence electrons)

Examples of elements: Xenon (Xe), Helium (He), Krypton (Kr)

FOUR MAIN CATEGORIES OF ELEMENTS

Representative Elements: also called main group elements and are located in Groups 1A-7A

s & p partly filled

Includes alkali metals, alkaline earth metals, and halogens

Large variation in properties

Examples of elements: Sodium (Na), Calcium (Ca), Nitrogen (N), Tin (Sn)

REPRESENTATIVE ELEMENTS

6.2

REPRESENTATIVE ELEMENTS

6.2

REPRESENTATIVE ELEMENTS

6.2

REPRESENTATIVE ELEMENTS

6.2

ALKALI, ALKALINE EARTH, HALOGENS Alkali Metals- group 1A

very reactive 1 valence electron: ns1

Loses 1 electron to be stable forming +1 charge

Alkaline Earth Metals– group 2A Less reactive than alkali

2 valence electrons: ns2

Loses 2 electrons to be stable, forming +2 charge

Halogens- group 7A Very reactive

Nonmetals

7 valence electrons: ns2….np5

Gains 1 electrons to be stable, forming -1 charge

REVIEW- ELECTRON CONFIGURATIONS FROM

THE PERIODIC TABLE

ELECTRON CONFIGURATIONS IN GROUPS

The Noble Gases

The electron configurations for the first four noble gases

in Group 8A are listed below.

6.2

ELECTRON CONFIGURATIONS IN GROUPS

Alkali Metals

In atoms of the Group 1A elements below, there is only

one electron in the highest occupied energy level.

6.2

ELECTRON CONFIGURATIONS IN GROUPS

Representative Elements

In atoms of the Group 4A elements below, there are four

electrons in the highest occupied energy level.

6.2

CLASSWORK!

Reading Assignment: Section 6.2

Written Assignment: p. 173, #12-15, 17

HOMEWORK!!

Complete the worksheet on comparing and

contrasting different aspects of the periodic

table.