The Periodic Table of

The Elements

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

Divided into three basic categories:MetalsNonmetalsMetalloids

The Periodic Table

Basic Organization

The periodic table is organized by:

Atomic structureAtomic numberChemical 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 compounds

Outermost level does not usually fill completely with electrons

Due Today

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Due TomorrowInterpreting the Periodic TableWarm Up LogCurrent Event

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 & Reactivity The 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.Video

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

Elements & Reactivity The 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

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.

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Group 1: Alkali MetalsContains: MetalsValence Electrons: 1Reactivity: Very

ReactiveProperties:

solidssoftreact violently with watershiny low densitySodium

Group 2: Alkaline-Earth Metals

Contains: MetalsValence Electrons: 2Reactivity: very reactive,

but less reactive than alkali metals (Group 1)

Properties: SolidsSilver coloredMore dense than alkali

metalsMagnesium

Groups 3-12 Transition Metals

Contain: MetalsValence electrons: 1 or 2Reactivity: less reactive

than alkali and alkaline-earth metals

Properties:Higher densityGood conductors of heat and

electricityCopper

Groups 3-12 Transition MetalsBelow Main Table

Contain: The Lanthanide and Actinide SeriesThese 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: 3Reactivity: Very reactiveProperties:

● 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

laboratoriesUranium

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 GroupContains: 1 metalloid and 4

metalsValence Electrons: 3Reactivity: ReactiveOther shared properties:

Solid at room temperature

Boron

Group 14: Carbon Group

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

Valence Electrons: 4Reactivity: VariesOther shared properties:

Solid at room temperature

Carbon

Group 15: Nitrogen Group

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

Valence electrons: 5Reactivity: VariesOther 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: 6Reactivity: ReactiveOther shared properties:

All but O are solid at room temperature.

Oxygen

Groups 17 : Halogens

Contain: NonmetalsValence Electrons: 7Reactivity: Very reactiveOther shared properties

● Poor conductors of electric current

● React violently with alkali metals to form salts

● Never found uncombined in natureChlorine Gas

Group 18 Noble Gases

Contains: NonmetalsValence Electrons: 8 (2

for He)Reactivity: Unreactive

(least reactive group)Other shared properties:

Colorless, odorless gases at room temperature

Outermost energy level full

All found in atmosphereNeon

Hydrogen Stands Apart

H 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

Warm Up

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PeriodsPeriods run horizontally across the

Periodic TablePeriods are numbered 1–7All 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

Quiz Quiz Trade

Brief History of the Periodic Table

Brief history of the periodic Table

When

Who What

Ancient Greece

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

EarthFireWater 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 Brand

1649Made the first scientific

discovery of an element

PhosphorusHe isolated from urine,

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

A.E. Beguyer de Chancourtois

1817Listed 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 Newlands

1863Classified 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 Meyer

1864, 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 Rayleigh

1895Discovered 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 Rutherford

1911Studied nuclei

which led to the concept of nuclear charge

Positive Charge and Protons

Henry Mosely

1913 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 Seaborg 1940 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

Warm Up

Brief History of the Periodic Table

Did the grouping change once you started posting them on the board?

Was it easier to group the atoms once you understood the property needed to group them?

Do you think that the periodic table will remain in the same form as it is now?

Patterns

Next blank page of you spiral title PatternsNumber 1-5 and leave 3 lines between

each number

Periodic Trends

What 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

Atomic Number INCREASES Metalic Properties INCREASES Valence Electrons Down a Group

Remain the Same Valence Electrons Across a Period

INCREASE

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

Warm UpAgree or Disagree and Why

Warm Up

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After the Test

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