Organization of the Periodic Table

Groups/Families

Vertical columns (#1-18)

Elements in the same group have similar chemical properties b/c they have the same # of valence electrons

Periods

Horizontal rows (#1-7)

Elements in the same period occupy the same highest principal energy shell (level)

Metals

Make up majority of the periodic table

Properties of Metals

-Located to the left of the 'staircase'

-Most elements are metals

-Most are solid (except Ag)

-Malleable

-Ductile

-Lustrous

-Hard

-Good conductors of heat and electricity

-Lose electrons to form positive ions

Metallic properties increase going down a group and decrease across a period (Francium is the most metallic)

Nonmetals

Relatively few in number, are varied more in properties than metals

Properties of Nonmetals

-Most are gasses (except Br:Liquid)

-Brittle

-Nonmalleable

-Not ductile

-Dull (no luster)

-Poor conductors of heat and energy

-Gain electrons to for negative ions

Semi-Metals (Metalloids)

Have properties of both metals and non-metals

Properties of Metalloids

-Elements (B, Si, Ge, As, Sb, Te)

-Display both metallic and nonmetallic properties

Transition Metals

Groups 3-12

Form colorful ions

Properties of Transition Metals

-Hard solids with high melting points (except Hg)

-Forms ions that have color

-The number of valence electrons will vary and are removed from the p and d sublevels

-Less reactive than group 1&2

Lanthanide Series

Atomic #58-71 also known as 'rare earth metals'

Actinide Series

Atomic #90-103, radioactive and most are synthetically made

Noble Gases

Group 18, not reactive in nature due to full valence shell, found ALONE

Properties of Noble Gases

-Group 18 elements

-Generally unreactive in nature due to full valence shell

-Helium is a noble gas, even though it has 2 valence electrons and all others have 8

-Exist alone in nature

Alkali Metals

Group 1, most reactive set of metals

Francium is the most reactive metal

Alkaline Earth Metals

Group 2, second most reactive metals on the periodic table

Halogens

Group 17, most reactive non-metals

Solids, Liquids, and Gases

Most elements exist in nature as solids

-Exceptions

Liquids: Mercury (Hg) and Bromine (Br)

Gases: Hydrogen (H), Nitrogen (N), Oxygen (O), Florine (F), Chlorine (Cl), and all of group 18

Diatomic Elements

Exist in nature as atoms bonded together

Ex) Br, I, N, Cl, H, O, F

s, p, d, and f blocks

S block: Groups 1&2

P block: Groups 13-18

D block: 3-12

F block: Lanthanide & Actinide series

Allotropes

Non metals of the same element that can exist as different substances while in the same phase or state of matter. Due to how the atoms are bonded to each other, allotropes have different molecular structures. Each substance will have its own physical and chemical properties

Metallic Character

As you travel down a group, the metallicity increases

As you travel across a period, the metallicity decreases

Atomic Radius

The distance from the nucleus to the outermost energy level

As you go down a group AR increases

As you go across a period AR decreases

Why does the AR increase as you move down a group?

-Closer to Fr

-More energy levels are added

-Distance from nucleus increases

Why does the AR decrease as you move across a period?

-# of electrons + protons increase

-Nucleus is bigger

-Nucleus has a greater pull/attraction for the electrons

Ionization Energy

The energy needed to remove an electron

As you go down a group IE decreases

As you do across a period IE increases

Why does the IE decrease as you go down a group?

-Become more metallic

-More energy levels

-Electrons can be removed easily

Why does the IE increase as you move across a period?

-More protons

-The attraction for electrons is greater

-You become less metallic, gain electrons easily

Electronegativity

A measure fot the attraction of electrons

Scale 0-4.0

As you move down a group EN decreases

As you move across a period EN increases

Why does EN decrease as you move down a group?

-Become more metallic

-Metals lose electrons

Why does EN increase as you move up a period?

-As you move across elements become non-metallic

-Non-metals gain electrons

Why do noble gases have such high IE but no EN?

-Don't need to gain/lose electrons

-Already have 8 Valence electrons

-Lots of energy needed to lose an electron

Ionic Radius

Formed as a result of the gain/loss of electrons

Metals tend to...

-Lose electrons

-Ionic Radius will DECREASE

-Atomic Radius>Ionic Radius

Non-metals tend to...

-Gain electrons

-Ionic Radius will INCREASE

-Atomic Radius

Bonding of Alkali Metals (Group 1)

-Usually found as a compound, highly reactive alone

-Elemental form can be obtained by electrolysis of their compound

Why is Hydrogen in the same column as Group 1 metals but separated from it?

Hydrogen doesn't have the same chemical/physical properties as these metals. Can form either positive or negative ions

S-Block

Valence electrons in s orbital

P-Block

Groups 13-18

Valence electrons in p orbital

Carbon group

-Contains 3 types of elements

-C is a non-metal, Si & GE are metalloids, Sn & Pb are metals

Nitrogen group

-Contains 3 types of elements

-N & P are non-metals, As & Sb are metalloids, Bi is a metal

Oxygen Group

-Contains 3 types of elements

-O & S are non-metals, Se & Te are metalloids, and Po is a metal