The Periodic Table

Unit 3

Origins In 1817, Johann

Dobereiner found that the properties of the metals calcium, barium and strontium were very similar. He grouped these elements in a triad.

Origins (Cont.)

In 1863, John Newlands arranged the elements in order of their increasing atomic masses. He noted that there appeared to be a repetition of similar properties every eighth element.

The Law of Octaves shows the same properties repeated every eight elements.

Dimitri Mendeleev In 1860’s, Dimitri Mendeleev

studied elements and also believed that the properties of the elements were a function of their atomic masses.

However, he believed that similar properties occurred after periods (horizontal rows) that could vary in length.

Mendeleev (Cont.) In 1869 he published his first

periodic table, leaving some blank spots in order to group all the elements with similar properties in the same column.

He explained the blank spots were for elements not yet discovered, but in 1871 he predicted their atomic mass and properties.

The Periodic Law His predictions were very nearly

correct. Mendeleev stated that the properties of the elements are a periodic function of their atomic masses. This is called the periodic law.

For his work, he is known as the Father of the Periodic Table.

The Modern Periodic Law There was a problem with this

arrangement. Henry Moseley found the reason for these exceptions to Mendeleev’s periodic law.

Moseley’s X-ray experiments showed that elements were positioned better if done by their atomic number.

The modern statement of the periodic law is the properties of the elements are a periodic function of their atomic numbers.

The Modern Periodic Table A horizontal row is referred to as

a period. A vertical column is referred to

as a group or family. There are 18 groups in the

periodic table.

Stability of Atoms One of the primary rules in

chemistry is that atoms with a full outer level are particularly stable (less reactive).

For all such elements, except hydrogen & helium, the outer level contains 8 electrons, these outer electrons are called an octet.

The fact that eight electrons in the outer level render an atom unreactive is called the octet rule.

Characteristics of Metals: Hard and shiny Conduct heat and

electricity Malleable &

ductile They are to the

left of the stair step.

Have only a few electrons in their outer level Gold &

Copper

o They tend to lose electrons to become positive ions.

Characteristics of Non-metals: Gases or brittle solids

at room temperature Dull and they are

insulators Are to the right of the

stair step Have more electrons

in their outer level Can share their

electrons or gain electrons to become negative ions.

Carbon & Sulfur

Metalloids They are elements right

along the stair steps on the chart. (Except Al)

Metalloids share characteristics of both metals and non-metals.

For example, Silicon is shiny like a metal, but is brittle and is not a good conductor of electricity.

Column IA: Alkali Metals Alkali metals have a

silvery appearance and are soft enough to be cut with a knife.

They are extremely reactive with moisture and are never found as free elements in nature.

Potassium in water

Column IIA: Alkaline Earth Metals Alkaline earth metals are harder,

denser and stronger than alkali metals.

They are less reactive but are never found as free elements in nature.

Pure Calcium is too reactive to be free in nature but can be found in Marble, Calcium Carbonate (CaCO3).

Transition Metals They occupy columns IIIB – IIB. They are typically less reactive

than alkali or alkaline earth metals.

Some are so unreactive they do not easily form compounds and exist in nature as free elements.

Palladium, Platinum and Gold are transition metals.

Column VIIA: Halogens The halogens are the most reactive

nonmetals. They react vigorously with most metals to

form “salts”. Fluorine and chlorine are gases at room

temperature.

Bromine is a reddish liquid.

Iodine is a dark purple solid.

Physical Properties of Halogens

Demo04-2.mov

Column VIIIA: Noble Gases First discovered in 1894 when

Argon was discovered. Noble gases were undetected

due to their total lack of chemical reactivity.

They have full valence shells, 8 valence electrons, with the exception of Helium which has 2.

The Lanthanides and Actinides Lanthanides contain elements from

#58, Cerium, to 71, Lutetium in the top pullout row.

Actinides contain elements from #90, Thorium, to 103, Lawrencium in the bottom pullout row.

Both series are off of group IIIB and are in periods 6 & 7 respectively and are metals.

Practice

WS #1 – Blank Ptable WS #1 Make your Own Periodic Tabl

e

Periodicity Periodicity of properties can be

observed in any group on the periodic table.

The reason for periodicity is explained in the arrangement of electrons around the nucleus.

Periodicity There are trends in these

properties as you go down in a group or across in a period.

NOTE: When discussing trends in properties, the Noble gases are never included.

Atomic Radius It measures the size of the atom Decreases as you go across a

period (left to right). Increases as you go down a

group because you add another level of electrons.

Ionic Radius

First Ionization Energy The energy needed to remove

the most loosely held electron from an atom.

It increases as you go across a period (left to right).

It decreases down a group.

Electron Affinity Electron Affinity is the attraction

of an atom for an electron. The electron affinity increases

as you go across a period (left to right) and decreases as you go down a group.

In general, as electron affinity increases, an increase in ionization energy can be expected.

Electronegativity The relative tendency of an atom

to attract electrons to itself when it is bonded to another atom.

Electronegativities of elements have the same trend as ionization energy and electron affinity.

Conceptual Short Cut!

As the atomic radius gets smaller, the: valence electrons are closer to the

nucleus, nucleus pulls harder on the electrons, Ionization energy, electron affinity, and

electronegativity will increase.

Periodic Trends SummaryAll arrows show increases!!

Zeff : Solution for Difficult Problems

Effective Nuclear Charge: Zeff

Zeff = Z – S Where:

Z = atomic number S = # of shielded (non-valence) electrons

The higher the Zeff, the greater pull of the positive nucleus on the valence electrons, which means a smaller atomic radius

Zeff Continued

Example: Mg vs. Mg2+

Zeff for Mg = 12 -10 n= +2 Zeff for Mg2+ = 12 – 2 = +10 Therefore: the effective positive charge

on Mg2+ is WAY bigger, which means the nucleus pulls on the outer electrons WAY harder, and the atom is subsequently WAY smaller.

Higher Zeff = smaller atomic radius

Electronegativity Cont. The most reactive metals (lower left)

have the lowest electronegativities. Fluorine, a nonmetal, is the most

electronegative element with a value of 4.0.

The difference in values for two elements tells you how the elements are bonded together when they combine with each other.

Electronegativity Cont. If the difference in electronegativity

values between 2 elements is below 1.7, it indicates a covalent bond.

If it is greater than 1.7, an ionic bond is indicated.

Reactivity Trend

Some metals and nonmetals are more reactive then others.

The easier it is for a metal to lose electrons, and the easier it is for a nonmetal to gain electrons, the more reactive they are.

Reactivity of Metals Lose electrons and become

positive ions. The farther the valence

electrons are from the nucleus, the less the protons pull and the easier (takes less energy) it is to remove an electron .

Reactivity increases down a group and decreases across a period.

What is the most reactive metal?

Reactivity of Non-Metals Gain electrons and become negative

ions. The closer the valence electrons are

to the nucleus, the more the protons pull and the easier it is to pull in an electron.

Reactivity decreases down a group and increases across a period.

What is the most reactive non-metal?

Metal/Nonmetal Reactivity

Most reactive metals – bottom, left

Most reactive nonmetals – top, right

Practice

WS #2 Periodic Trends WS #2 Periodic Trends