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) + 2H 2 O (l)  2NaOH (aq) + H 2(g)  alkaline solutions are “basic” solutions pH

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 elements They 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 H 2(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” block Groups

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 metalloid Germanium is also a metalloid Indium 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 3 rd. Bromine is a diatomic liquid, found in “seltzer” Iodine is a diatomic solid that sublimes at room temperature.

Part III “d” and “f” block Groups d block f block

Transition Metals are “d” block Can form multiple positive ions with different charges.  e.g. Iron will for either a Fe 2+ or Fe 3+ ion  Tin will form either a Sn 2+ or Sn 4+ 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.