THE PERIODIC TABLEThe Periodic Table was first put together by Demitri Mendeleev.

MENDELEEV’S TABLE (~1872)

Arranged according to increasing atomic mass

Elements with similar properties placed in the same vertical column

Missing elements were yet to be discovered and were left blank on the table

HENRY MOSELEY – (1887-1915)

British Physicist determined the atomic numbers of the elements

He arranged the periodic table in order of atomic number

His periodic table is the one used today

PERIODS –

horizontal rows of the Periodic Table There are 7 Periods

PERIODIC LAW – When the elements are arranged in order

of increasing atomic number, there is a periodic repetition of their physical and chemical properties.

GROUPS –

vertical columns of elements on the Periodic Table

Groups are also known as families because they have similar properties.

REPRESENTATIVE ELEMENTS

Group A elements

Alkali Metals – Group 1-A elements Alkaline Earth Metals – Group 2-A

elements Halogens – Group 7-A elements Noble Gases – Group 0 elements

GROUP B ELEMENTS

Transition Metals – In the middle of the Periodic Table

Inner Transition Metals (rare earth metals) – bottom of the Periodic Table

Please label your periodic table with the following:

Color the families as follows: Alkali metals – red Alkaline earth metals – yellow Halogens – green Noble gases – blue

Please outline the representative elements in purple and the transition metals in orange.

Make a key to your colors on the top of the page along with definitions of each family in your own words.

CLASSIFICATION OF ELEMENTS Metals – found on the left-side of the Periodic Table Nonmetals – found on the right-hand side of the Periodic Table Metalloids (or semi-metals) – along the stair-step line

Properties are intermediate between metals and nonmetals

Metals are… Malleable – can be

hammered into sheets Ductile – can be drawn

into wires Shiny or Lustrous Good conductors/poor

insulators of heat and electricity

All solids at room temperature except Hg

Non-metals are… Brittle but often form

crystals Dull Good insulators/poor or

non-conductors of heat and electricity

Solids, liquids and gases at room temperature

Metalloids Have properties that are

intermediate between metals and nonmetals.

CLASSIFICATION OF ELEMENTS

Please label your periodic table with the metals, nonmetals and metalloids. Add definitions of these groups on the top of the page.

WEDNESDAY BELLWORK

What group or family do the following elements belong to?

  F Ag Ar Xe H Sr

HOMEWORK Which scientist first proposed the atom was mostly empty space?

The modern periodic table is arranged in order of increasing atomic _________.

a. mass b. charge c. number d. radius

Along the periodic chart, groups and families are located vertically/horizontally, and periods are located vertically/horizontally. (Circle the best choice)

The Halogens are group ______________.

a.1A b. 2A c. 6A d. 7A

14.1 – CLASSIFICATION OF THE ELEMENTS

History of the Periodic Table (A Review) Mendeleev- arranged elements in order of increasing

atomic mass Moseley- arranged elements in order of increasing

atomic number Periodic Law- When the elements are arranged in

order of increasing atomic number, there is a periodic pattern in their physical and chemical properties.

Periodic Trends

The arrangement of the Periodic Table also provides scientists with a general idea of periodic trends. We will now examine those trends. You are responsible for the trends in boldface and underlined print ONLY.

Effective Nuclear Charge (Zeff)

The pull the nucleus exerts on the electrons.

The larger the Zeff, the tighter the electrons are pulled and the smaller the atom.

Trend: Zeff is highest near the top right of the periodic table

Write this trend on the appropriate periodic table in your flip book.

Question

Which elements in the following pairs would have the highest Zeff? Mg or Cl Rb or Sr Al or At

14.2 – PERIODIC TRENDS• Atomic radius – one-half the

distance between the nuclei of two like atoms in a diatomic molecule (ex: Cl2)

• The more energy levels present, the larger the atom.

• When comparing atoms that all have similar energy levels, the atoms with the largest nuclei (and thus greatest number of protons) will have the smallest radii.

• Trend: atomic radius increases from right to left and from top to bottom.

• Write the trend in your flipbook

Atomic Radius

Increasing Atomic Radius

Incr

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BIGGEST

SMALLEST

Question

Place the following elements in order of increasing atomic radius. Ca, C, Ra, Br

• Ionization energy - energy required to overcome the attraction of the nuclear charge and remove on electron from a gaseous atom to form an ion.• 1st ionization energy: the energy required to

remove the first electron• 2nd ionization energy: the energy required to

remove the second electron• 3rd ionization energy: the energy required

removing the second electron• Trend: ionization energy increases from left to right

and bottom to top.• Please write this trend onto your flipbook.

Periodic Trends: Ionization Energy

Question

What electron do you think would be easiest to remove, the first, second, or third? Why?

Ionization Energy

Increasing Ionization Energy

Incr

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nerg

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• Ion Size • Anions, or atoms that have gained electrons, are larger

than the atoms from which they were formed.• The negative charge means more electrons are

present causing the size of the ion to be larger.• Cations, which are atoms that have lost electrons, are

smaller than the atoms from which they were formed.• The positive charge means fewer electrons are

surrounding the nucleus, thus pulling the existing electrons closer and causing the ion to be smaller.

• Trend: ionic radius increases from right to left and from top to bottom.

• Please add this trend to your flipbook.

Periodic Trends: Ion Size

Ionic Radius

Increasing Ionic Radius

Incr

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onic

Rad

ius

Question

What is larger; an atom of nitrogen or its anion? Why?

• Electronegativity – the tendency for the atoms of the element to attract electrons when they are chemically combined with atoms of another element

• Note: Nobel gases don’t have any electronegativity because their orbitals are filled so they don‘t bond with other elements.

• Trend: electronegativity increases from left to right and bottom to top.

• Please add this trend to your flipbook.

Periodic Trends: Electronegativity

Electronegativity

Increasing Electronegativity

Incr

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lect

rone

gati

vityHIGHEST

Question

If hydrogen and fluorine made a bond, which atom would have more bonded electrons near its nucleus?

THURSDAY BELLWORK: • Place the following elements in order of increasing

atomic radius.Ca, C, Ra, Br

• Place the following elements in order of decreasing ion size.Fr, Ag, Cl, He

WEDNESDAY HOMEWORK: Which group of the periodic table has the highest ionization

energies?

1A b. 2A c. 3A d. 7A

Which of the following elements is in the same period as chlorine?

a. carbon b. magnesium c. nitrogen d. oxygen

How does atomic radius change from left to right across a period in a periodic table?

THURSDAY BELLWORK:  

1. Which elements in the following pairs would have the highest Zeff?

Mg or Cl Rb or Sr Al or At

2. Which has the largest electronegativity?a. chlorine b. sodium c. carbon d. fluorine

THURSDAY HOMEWORK:What is true of the electron configurations of the noble gases?

a. The outermost s and p sublevels are filled.b. The outermost s and p sublevels are partially filled. c. The outermost s and d sublevels are very close in energy and have electrons in them.d. The outermost s and f sublevels are very close in energy and have electrons in them.

 Which of the following elements has the smallest atomic radius?

a. Ne b. Ar c. Kr d. Xe