PERIODIC PATTERNSUnit 4 – Periodic Table

Mr. DiBiasio

What patterns exist on the periodic table?

Lesson Essential Question:

METALLIC TREND

INCREASE

S

INC

REA

SE

S

ATOMIC RADIUS

Radius is the distance from the center of the nucleus to the “edge” of the electron cloud.

Atomic radii are usually measured in picometers (pm) or angstroms (Å). An angstrom is

1 x 10-10 m.

ATOMIC RADIUS

BROMINE = Br2

Since a cloud’s edge is difficult to define, scientists use define covalent radius, or half the distance between the nuclei of 2 bonded atoms.

2.86 Å1.43 Å 1.43 Å

ATOMIC RADII TRENDS

As you go down a family the n value increases making the radius larger.

DOWN A FAMILY OR GROUP WHY?

INC

REA

SES

ATOMIC RADII TRENDS

As you go across a period the number of protons increases, (nuclear charge) pulling the electrons in tighter making the radius smaller.

ACROSS A PERIOD WHY?

IONS - remember

Metals Lose electrons

becoming positive.

Calcium – Ca [Ar]4s2

Loses 4s2 e-s becoming

Ca+2 and [Ar] Noble gas

Configuration. (Octet Rule)

Nonmetals Gain electrons

becoming negative.

Chlorine – Cl [Ne]3s23p5

Gains one e- becoming Cl-1 and [Ar] Noble gas configuration.

(Octet Rule)

IONS – How can I remember?

Metals Nonmetals

This is Ann ion - ANIONShe is unhappy and

negative.

This is Cat-ion - CATIONHe is a “plussy”

cat!

IONIC RADII TRENDS

As you go down a family the n value increases making the radius larger.

DOWN A FAMILY OR GROUP WHY?

INC

REA

SES

IONIC RADII TRENDS

For the metals the nuclear charge is greater than then number of electrons pulling them in tighter making the radius smaller.

At the nonmetals the radius gets larger because the ion has gained electrons.

ACROSS A PERIOD WHY?DECREASES then INCREASE

METALLIC ATOM AND ION COMPARISON

NONMETALLIC ATOM AND ION COMPARISON

Why do the Noble Gases not have an ionic Radius?

ATOM AND ION COMPARISON

Why does Hydrogen not have an ionic Radius?

As more electrons are added to atoms, the inner layers of electrons shield the outer electrons from the nucleus.The effective nuclear charge on those outer electrons is less, and so the outer electrons are less tightly held

Shielding Effect

Example of Shielding Effect

The energy required to remove an electron from an atom is ionization energy. (measured in kilojoules, kJ)

Ionization Energy

IONIZATION ENERGY

The larger the atom is, the easier its electrons are to remove.

Ionization energy and atomic radius are inversely proportional.

Ionization energy is always endothermic, that is energy is added to the atom to remove the electron.

IONIZATION TREND

INCREASES

INC

REA

SE

S

is a measure of the energy change when an electron is added to a neutral atom to form a negative ion

Electron Affinity

ELECTRON AFFINITYWhy do the Alkaline Earth Metals and Noble Gases not have measurable Electron Affinities?

is a measure of the tendency of an atom to attract a bonding pair of electrons.

Electronegativity

ELECTRONEGATIVITY

In Summary….Electronegativity

Ele

ctro

negati

vit

y