Periodic Trends Mr. Dellamorte Fenger High School Chemistry.

Periodic Trends

Mr. DellamorteFenger High School

Chemistry

Groups

Vertical Columns of periodic table

Periods

Horizontal rows of periodic table

4 Blocks of Periodic Table S-block

Groups 1+2 (total of 2 groups) electrons in s orbital

P-block Groups 13-18 (total of 6 groups) electrons in p orbital

D-block Transition Metals electrons start to fill d orbitals

F-block Inner transition Metals Electrons start to fill f-orbitals

Part I – Atomic Size

Atomic Radius

Measures as distance from nucleus to nucleus and divided by 2.

Unit commonly used is pm picometer= 10-12m

Example: iodine atomic radius 140pm

How does atomic radius change across a period?

It is smaller to the right.

Why?

More protons in the nucleus higher electrical force pulls electrons closer to nucleus.

How does atomic radius change down a group?

It is larger down the group.

Why?

Valence electrons are at higher energy levels and are not bound as tightly to the nucleus because they are screened or shielded ( pushed away) by other electrons in inner levels.

Note

There are some exceptions. Example column 13.

The Periodic Table and Atomic Radius

Example:

Which is larger: a lithium atom or a fluorine atom?

A lithium atom

Example:

Which is larger: an arsenic atom or a sulfur atom?

An arsenic atom

Part II – Ionization Energy

Ionization energy

Ionization energy is the amount of energy needed to remove an electron from a gaseous atom. First ionization energy – 1+ Second ionization energy – 2+

Ion

Cation - Positive ion removal of electron

Anion - Negative ion addition of electron

How does ionization energy change down a group?

The first ionization energy decreases as you move down a group.

Why? The size of the atom increases. Electron is further from the nucleus.

The first ionization energy increases as you move from left to right across a period.

Why? Nuclear charge increases while

shielding is constant. Attraction of the electron to the

nucleus increases.

How does ionization energy change across a period?

Ionic size

Metallic elements easily lose electrons.

Non-metals more readily gain electrons.

How does losing or gaining an electron effect the size of the atom

(ion) ?

Positive ions

Positive ions are always smaller than the neutral atom. Loss of outer shell electrons.

Negative Ions

Negative ions are always larger than the neutral atom. Gaining electrons.

Ion size trends in periods.

Going from left to right there is a decrease in size of positive ions.

Starting with group 5, there is sharp increase followed by a decrease in the size of the anion as you move from left to right.

Ion size trends in columns.

Ion size increases as you move down a column for both positive and negative ions

Electronegativity: the ability of an atom in a bond to pull on the electron. (Linus Pauling)

Electronegativity When electrons are shared by two

atoms a covalent bond is formed.

When the atoms are the same they pull on the electrons equally. Example, H-H.

When the atoms are different, the atoms pull on the electrons unevenly. Example, HCl

Trends in Electronegativity

Electronegativity generally decreases as you move down a group.

Electronegativity of the representative elements (Group A elements) increases as you move across a period.

Electronegativities of Some Elements

Element Pauling scale F 4.0 Cl 3.0 O 3.5N 3.0 S 2.5C 2.5H 2.1Na 0.9Cs 0.7

Note

Most electronegative element is F (EN 4.0)

Least electronegative stable element is Cs

(EN 0.7)

SummaryShielding is constantAtomic Radius decreasesIonization energy increasesElectronegativity increasesNuclear charge increases

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