Geography and Trends of the Periodic Table

Period

Horizontal rows in the periodic table.

Group

Vertical columns in the periodic table.

Metals

Elements that conduct electricity and heat.

Nonmetals

Elements that lack metallic properties.

Blocks

Sections of the periodic table: S, P, D, F.

Alkali Metals

Group 1 elements, highly reactive.

Noble Gases

Group 18 elements, chemically inert, contains pefect valence shells

Alkaline-Earth Metals

Group 2 elements, reactive but less than alkali.

Transition Metals

Elements found in groups 3-12.

Periodic Law

Similar properties occur periodically by atomic number.

Atomic Radius

Distance from nucleus to outermost electron.

Ionization Energy

Energy needed to remove an electron.

Electronegativity

Ability to attract OR steal electrons from other atoms.

Activity

Reactivity of an element.

Ions

Charged atoms with unequal protons and electrons.

Valence Electrons

Outermost electrons determining chemical properties.

Quantum Mechanical Theory

Describes electron behavior in atoms.

Octet Rule

Atoms gain, lose, or share electrons for stability typically of 8.

Common Ion Charges

Typical charges for elements in groups.

Electron Configuration

Distribution of electrons in atomic orbitals.

Stable Elements

Elements with full valence electron shells.

D-block

Transition metals in the periodic table.

Inner Transition Metals

Lanthanides and actinides series.

Periodic Trends

Predictable changes in element properties.

Exceptions to Trends

Not all elements follow predicted trends.

How does electronegativity increase?

up and to the right

Why does electronegativity increase as you go up?

the more protons mean the the nuclear charge is increasing causing a greater force of attraction

How does atomic radius increase?

down and to the left

Why does atomic radius increase as you go down a group?

fewer protons means the nuclear charge decrease which reduces the attraction between nucleus and outermost electrons

How does Ionization (IE) increase?

UP and to the RIGHT

Why does IE increase across a period and to the right?

more protons means the nuclear charge is increasing causing a greater force of attraction between the nucleus and outermost electrons.