DARK BLACK PRINT IS IMPORTANT MUST-KNOW FOR THE REGENTS

GREY & ORANGE PRINT IS NICE TO KNOW BACKGROUND INFORMATION

More Details on Metals and Nonmetals and Periodic

Table

ACTIVE METALS

Part I “s” block, Groups 1 & 2

s block

Alkali Metals

Group 1 elements 1 valence electron (half filled S – sublevel) most reactive metals. are not found uncombined in nature (elemental) are found as salts that are very soluble in water react with water to make Hydrogen gas and a

solution of the alkali metal hydroxide. (strong bases)

2Na(s) + 2H2O(l) 2NaOH(aq) + H2(g) alkaline solutions are “basic” solutions pH 7.1-14.0

Storage of Alkali Metals

react with water so rapidly and exothermically (gives off lots of energy) that the Hydrogen often burns as it is produced.

are usually stored under oil or kerosene to keep them from reacting with the oxygen or water in the air.

Alkali Metal Manufacturing

Sodium is the only one manufactured on a large scale.

To produce the free metal, sodium ions must be forced to gain electrons (reduction).

The electrolysis (add electricity to break down) of molten sodium chloride makes elemental sodium.

Also produced is Chlorine gas - another useful chemical

General Characteristics of Alkali Metals

low density high conductivity low melting points soft consistency shiny when freshly cut

Alkaline Earth Metals

Group 2 elementsThey have 2 valence electrons (completed S – sublevel) Group 2 are less reactive than Group 1. (but still found

only as compounds in nature) do not need to be stored in oil react with water to produce basic, (alkaline) solutions.

(pH 7.1 – 14.0) Solid Calcium reacts with water to produce H2(g) slowly salts are less soluble than salts from group 1. Sea water has an abundant amount of magnesium and

calcium ions. (2 most commercially useful from Group 2)

Alkali Earth Metal Manufacturing

Lime – is Calcium Oxide (CaO) Slaked Lime – is Calcium Hydroxide (Ca(OH)2) Both are in important to industry

METALS AND NONMETALS

Part II “p” blockGroups 13 - 18

p block

Aluminum and Group 13

Boron is a metalloid (Semiconductor), common in minerals Used to make glass and water softeners

Aluminium is so useful it was once as expensive as silver Most common metal in Earth’s crust.

Gallium is often used in thermometers instead of mercury.

Indium and Thallium are rare.

Carbon and Group 14

Carbon is the building block of all life on Earth

Silicon is an important metalloidGermanium is also a metalloidIndium and Thallium are uncommon

Nitrogen and Group 15

Nitrogen is a diatomic and makes up 78% of the atmosphere The nitrogen in the atmosphere is very stable and

cannot be used directly by living things Very important in fertilizer

Phosphorous is also an important fertilizer. Elemental phosphorous glows.

Arsenic and antimony are metalloids and poisonous

Bismuth is a metal, salts of which are used in antacids.

Oxygen and Group 16

Oxygen is diatomic and the second most electronegative element

Sulfur is a yellow solid that can be stable in its elemental state

Selenium is a micronutrient meaning it’s important for health but you don’t need much of it.

Tellurium and Polonium are uncommon

The Halogens

ALL are highly reactive,Fluorine and Chlorine are diatomic gases but

still extremely reactive.Fluroine is the most electronegative element,

Chlorine is 3rd.Bromine is a diatomic liquid, found in

“seltzer”Iodine is a diatomic solid that sublimes at

room temperature.

Part III “d” and “f” blockGroups 3 - 12

d block

f block

Transition Metals are “d” block

Can form multiple positive ions with different charges. e.g. Iron will for either a Fe2+ or Fe3+ ion Tin will form either a Sn2+ or Sn4+ ion

“f” block Rare Earth Metals

Not truly “rare” but their properties are so similar they are hard to isolate from each other.

Every element more massive than Uranium (92) is human created.