The Periodic Table of The Elements

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Store Organization

Where are some places you have visited that have areas or items organized into categories?

With your table group you will created a map of a store and how it is organized.

You must include:10 items or more

Why are they organized

4 or more colors

This is a presentation

Store Organization

Why is a system of organization important?Organization makes it easier to find objects, provides storage, etc.

What do a store and the periodic table have in common?

The structure and properties of the atoms/elements are used to organize the periodic table just as a grocery store organizes food by its properties.

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Grouping Atoms by Structure

What does the atomic number tell us about atoms?

Atomic # = # of Protons

How do you know the number of electrons in a stable atom?

# of Protons = # of Electrons

Where are electrons located in an atom?In the Electron Cloud, around the Nucleus, in an Energy Level

What names do we give the electrons in the outmost energy level and why are they important?

Valence Electrons and they determine the bonding

Grouping Atoms by Structure

Grouping Atoms by Structure

What patterns do you see?

What do the vertical columns have in common?

Same # of valence electrons

What do the horizontal rows have in common?

Same number of energy level

What changes as you move across the table from left to right?

Increasing atomic # and # of VE

Grouping Atoms by Structure

Tape the card in your binder and record the following

Element Name

Atomic Number

Number of Protons

Number of Electron

Number of Valence Electrons

Number of Energy Levels

The Periodic Table

Arrangement of the known elements based on atomic number and chemical and physical properties.

Divided into three basic categories:Metals

Nonmetals

Metalloids

Basic Organization

The periodic table is organized by:

Atomic structure

Atomic number

Chemical and Physical Properties

Uses of The Periodic Table

The periodic table is useful in predicting:

chemical behavior of the elements

trends

properties of the elements

Atomic Structure ReviewAtoms are made of protons, electrons, and

neutrons.

Elements are atoms of only one type.

Elements are identified by the atomic number (# of protons in nucleus).

Energy Levels ReviewElectrons are arranged in a region around the nucleus called an electron cloud. Energy levels are located within the cloud.

At least 1 energy level and as many as 7 energy levels exist in atoms.

Energy Levels Review

Electrons in levels farther away from the nucleus have more energy.

Inner levels will fill first before outer levels.

Energy Levels & Valence Electrons

Energy levels hold a specific amount of electrons:

1st level = up to 2

2nd level = up to 8

3rd level = up to 8 (first 18 elements only)

Energy Levels & Valence Electrons

The electrons in the outermost level are called valence electrons.

Determine reactivity - how elements will react with others to form compoundsOutermost level does not usually fill completely with electrons

Elements & Reactivity

Reactivity is a chemical property that determines how elements will react with others to form compounds.

Elements & Reactivity

What makes an element reactive?● Number of valence electrons each atom has● When outer levels are full, atoms are stable.● When they are not full, they react:

● gain, lose, or share 1 or 2 electrons.

Elements & ReactivityThe most reactive metals are the elements in Groups 1 and 2.

Elements in Group 1 need seven more electrons to fill their outer level. Elements in Group 2 need six more electrons to fill their outer level.

These groups are known as the “givers” because they easily give up their valence electrons to make a compound.

Videohttp://www.youtube.com/watch?v=xxi6kUbvo94

Elements & ReactivityThe most reactive nonmetals are the elements in Groups 16 and 17.

Elements in Group 16 only need two more electrons to fill their outer level.Elements in Group 17 only need one more electron to fill their outer level.

These groups are known as the “takers” because they easily receive valence electrons to make a compound.

Fluorite

Elements & Reactivity

Reactivity charades (white boards)

Fluorite

Using the Table to Identify Valence Electrons

Elements are grouped into vertical columns because they have similar properties.

These are called groups or families.

Groups are numbered 1-18.

Using the Table to Identify Valence Electrons

Group numbers can help you determine the number of valence electrons:

Group 1 has 1 valence electron.Group 2 has 2 valence electrons.Groups 3–12 are transition metals and have 1 or 2 valence electrons.

Using the Table to Identify Valence Electrons cont.

Groups 13–18 have 10 fewer than the group number. For example:

Group 13 has 3 valence electrons.

Group 15 has 5 valence electrons.

Group 18 has 8 valence electrons.

Group 1: Alkali MetalsContains: Metals

Valence Electrons: 1

Reactivity: Very Reactive

Properties: solids

soft

react violently with water

shiny

low density

Sodium

Group 2: Alkaline-Earth Metals

Contains: Metals

Valence Electrons: 2

Reactivity: very reactive, but less reactive than alkali metals (Group 1)

Properties: Solids

Silver colored

More dense than alkali metals

Magnesium

Groups 3-12 Transition Metals

Contain: Metals

Valence electrons: 1 or 2

Reactivity: less reactive than alkali and alkaline-earth metals

Properties:Higher density

Good conductors of heat and electricity

Copper

Groups 3-12 Transition Metals

Below Main TableContain: The Lanthanide and Actinide Series

These two rows are pulled out of sequence and placed below the main table to keep the table from being too wide.Lanthanides are #’s 58–71.Actinides are #’s 90–103.

Plutonium

Groups 3-12 Rare Earth Elements ~ Lanthanides

Lanthanides follow the transition metal # 57 Lanthanum in Period 6.

Valence electrons: 3

Reactivity: Very reactive

Properties:● High luster, but tarnish easily ● High conductivity for electricity● Very small differences between them

Cerium

Groups 3-12 Rare Earth Elements ~ Actinides

Actinides follow the transition metal # 89 Actinium in Period 7

Valence electrons: 3 (but up to 6)

Reactivity: unstableAll are radioactiveMost made in laboratories

Uranium

Metalloids A zig-zag line that separates metals from metalloids

Elements from Groups 13–17 contain some metalloids.

These elements have characteristics of metals and nonmetals.

Group 13: Boron Group

Group 13: Boron Group

Contains: 1 metalloid and 4 metals

Valence Electrons: 3

Reactivity: Reactive

Other shared properties:Solid at room temperature

Boron

Group 14: Carbon Group

Contains: 1 non-metal, 2 metalloids, and 3 metals

Valence Electrons: 4

Reactivity: Varies

Other shared properties: Solid at room temperature

Carbon

Group 15: Nitrogen Group

Contains: 2 non-metals, 2 metalloids, and 1 metal

Valence electrons: 5

Reactivity: Varies

Other shared properties: All but N are solid at room temperature

Nitrogen

Group 16: Oxygen Group

Contains: 3 non-metals, 1 metalloid, and 2 metals

Valence Electrons: 6

Reactivity: Reactive

Other shared properties: All but O are solid at room temperature.

Oxygen

Groups 17 : Halogens

Contain: Nonmetals

Valence Electrons: 7

Reactivity: Very reactive

Other shared properties● Poor conductors of electric current● React violently with alkali metals to

form salts● Never found uncombined in nature

Chlorine Gas

Group 18 Noble GasesContains: Nonmetals

Valence Electrons: 8 (2 for He)

Reactivity: Unreactive (least reactive group)

Other shared properties: Colorless, odorless gases at room temperatureOutermost energy level fullAll found in atmosphere

Neon

Hydrogen Stands ApartH is set apart because its properties do not match any single group.

Valence electrons: 1

Reactivity: very, but loses the 1 electron easily

Properties:Similar to those of non-metals rather than metals

Hydrogen in it’s Plasma state

Movie or APP

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PeriodsPeriods run horizontally across the Periodic Table

Periods are numbered 1–7

All the elements in a period will have the same number of energy levels, which contain electrons. Examples:

Period 1 atoms have 1 energy level.

Period 2 atoms have 2 energy levels.

Period 5 atoms have 5 energy levels.

Mimio

Periods ContinuedMoving from left to right across a period, each element has one more electron in the outer shell of its atom than the element before it.

This leads to a fairly regular pattern of change in the chemical behavior of the elements across a period.

Mimio

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Brief history of the Periodic Table

When Who What Picture

Open History of the Periodic Table paper in eBackPack into uPad

Ancient Greece

In Ancient Greece, people believed that there were only four elements…..

Earth

Fire

Water

Air

What were scientist looking for when they found the first element

Alchemists

They were looking for the philosopher’s stone, which reputedly could change base metals into gold

Hennig Brand1649

Made the first scientific discovery of an element

Phosphorus

He isolated from urine, a white, waxy material and named it phosphorus (“light bearer”), because it glowed in the dark.

A.E. Beguyer de Chancourtois

1817

Listed elements on a cylinder in order of increasing atomic mass

Johann Dobereiner

1862

Proposed there were triads of three elements in nature with the mass of the middle element being the average of the other two

Law of Triads

Found that the properties of bromine seem halfway between those of chlorine and iodine. He showed that in each triad the mean of the lightest and heaviest atomic weights approximated the atomic weight of the middle element.

In other words…. 4………6.......8

John Newlands1863

Classified the 56 known elements into a table with 11 groups based on properties. He proposed that any element will behave similar to the 8th element following it.

Law of Octaves

Lothar Meyer1864, German

Developed a shortened version of the table only showing half of the known elements.

Elements were listed in order of atomic mass and differences in behavior were due to mass.

He published a longer version in 1869 but it wasn’t published until 1870

Dmitri Ivanovich Mendeleev

1869, Russian

Rearranged elements in order of their properties.

He showed a vertical, horizontal and diagonal relationship between the 63 known elements

Predicted three yet-to-be-discovered elements including eke-silicon and eke-boron

Lord Rayleigh1895

Discovered argon and found it didn’t fit in the current groups.

In 1898 he proposed a new group to be called zero group because argon was unreactive (inert)

Ernest Rutherford1911

Studied nuclei which led to the concept of nuclear charge

Positive Charge and Protons

Henry Mosely1913

Published results of x-ray wavelengths of elements which proved the elements are in order of atomic number.

He used increasing atomic numbers and not atomic masses

Glenn Seaborg1940

Discovered plutonium and all elements from 94-102.

He moved the Lanthanides and Actinides below the table.

Discovered 10 different elements to include seaborgium, which was named after him

credited with important contributions to the chemistry of plutonium, part of the Manhattan Project where he helped develop fuel for the second atomic bomb

pioneer in nuclear medicine, most notably iodine-131, which is used in the treatment of thyroid disease.

Quiz Quiz Trade

Various Periodic TableGo to this website and look at the different periodic tables for the rest of class

http://www.meta-synthesis.com/webbook/35_pt/pt_database.php?Button=pre-1900+Formulations

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HomeworkAtom Project due TOMORROW

Watch video due Wednesday

Valence Clue due Thursday

Identifying Unknown Elements due Thursday

Match the Elements due Thursday

Test Friday

PatternsOpen a blank page in uPad

Write Pattern on the top and number 1-6

You will write the question and then answer

You may use your group and iPad to help you find the answers

Be prepared for discussion

Patterns

Open your labeled periodic table from Friday

Complete

Periodic TrendsWhat does periodic mean?

Recurring at regular intervals

What does trend mean? A pattern of gradual change or movement

What might be a good definition for periodic trends? Are the tendencies of certain characteristics of the atoms to increase or decrease along a row or column of the periodic table of elements

What are some of the patterns found in the periodic table?

Average atomic mass increases right to left and top to bottom

How does the arrangement of the periodic table allow for the prediction of undiscovered elements and their properties?

Patterns

Do you think the periodic table will remain the same as it is today?

Atomic Number INCREASES

Metalic Properties INCREASES

Valence Electrons Down a Group Remain the Same

Valence Electrons Across a Period INCREASE

Example Homework Problems

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Today’s Plan

Test Review

Start Project

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The following elements all belong to the same period: Ne, Ar, Kr, and Xe. 

Disagree because they all have different numbers of energy levels.

The following elements all belong to the same group/family:  H, Li, Na, and K.

Agree because they all have the same number of valence electrons.

All elements in group 13 have 3 valence electrons.

Agree because all elements in group 13 have ten less than stated, and all elements in a group have the same number of valence electrons.

The chemical reactivity of an element is determined by its protons.

Disagree because the reactivity is determined by the number of valence electrons

Agree or Disagree and Why

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