Download elements - ghostnet surfers 2

SCIENCE PRESENTATION!!!
ALKALI METALS

The alkali metals have very similar properties: they are all shiny, soft,
highly reactive metals at standard temperature and pressure[6] They
can all be cut easily with a knife due to their softness, exposing a
shiny surface that tarnishes rapidly in air due to oxidation by
atmospheric moisture andoxygen.[6] Because of their high reactivity,
they must be stored under oil to prevent reaction with air,[10] and are
found naturally only in salts and never as the free element. All the
discovered alkali metals occur in nature: in order of abundance,
sodium is the most abundant, followed by potassium, lithium,
rubidium, caesium, and finally francium, which is very rare due to its
extremely high radioactivity and thus occurs only intraces due to its
presence in natural decay chains
ALKI EARTH METALS

The alkaline earth metals are a group of chemical elements in
the periodic table with very similar properties. They are all shiny,
silvery-white, somewhat reactive metals at standard temperature and
pressure[1] and readily lose their two outermost electrons to
form cations with charge 2+ and an oxidation state, or oxidation
number of +2.[2] In the modern IUPACnomenclature, the alkaline earth
metals comprise the group 2 elements.[n 1]

The alkaline earth metals
are beryllium (Be), magnesium (Mg), calcium (Ca), strontium (Sr), bari
um (Ba), and radium (Ra).[4]This group lies in the s-block of the
periodic table

Noble gases

The noble gases make a group of chemical elements with similar
properties: under standard conditions, they are all odorless, colorless,
monatomic gases with very low chemical reactivity. The six noble
gases that occur naturally are helium (He), neon (Ne), argon (Ar),
krypton (Kr), xenon (Xe), and the radioactive radon (Rn). noble-gaslike properties,[1] instead of the group 18 element ununoctium.[2]
Noble gases are typically highly unreactive except when under
particular extreme conditions. The inertness of noble gases makes
them very suitable in applications where reactions are not wanted.
For example: argon is used in lightbulbs to prevent the hot tungsten
filament from oxidizing; also, helium is breathed by deep-sea divers
to prevent oxygen and nitrogen toxicity
Halogens

The halogens or halogen elements (/ˈhælɵdʒɨn/) are a group in the periodic
table consisting of five chemically related elements: fluorine (F), chlorine
(Cl), bromine (Br), iodine (I), and astatine (At). The artificially created
element 117 (ununseptium) may also be a halogen. In the modern IUPAC
nomenclature, this group is known as group 17.


The group of halogens is the only periodic table group that contains elements
in all three familiar states of matter at standard temperature and pressure.
All of the halogens form acids when bonded to hydrogen. Most halogens are
typically produced from minerals or salts. The middle halogens, that is,
chlorine, bromine and iodine, are often used as disinfectants. The halogens
are also all toxic.
Nonmetals

a nonmetal (or non-metal) is a chemical element that mostly lacks metallic
attributes. Physically, nonmetals tend to be highly volatile (easily vaporised),
have low elasticity, and are good insulators of heat and electricity;
chemically, they tend to have high ionisation energy and electronegativity
values, and gain or share electrons when they react with other elements or
compounds. (carbon, phosphorus, sulfur, selenium, and iodine).
Metalloids

Typical metalloids have a metallic appearance but they are brittle and only
fair conductors of electricity. Chemically, they mostly behave as nonmetals.
They can form alloys with metals. Most of their other physical and chemical
properties are intermediate in nature. Metalloids are usually too brittle to
have any structural uses. They and their compounds are used in alloys,
biological agents, catalysts, flame retardants, glasses, optical storage and
optoelectronics, pyrotechnics, semiconductors and electronics.

boron, silicon, germanium, arsenic, antimony and tellurium.
Transition metals


Because they possess the properties of metals, the transition elements are
also known as the transition metals. These elements are very hard, with high
melting points and boiling points. Moving from left to right across the periodic
table, the five d orbitals become more filled. The d electrons are loosely
bound, which contributes to the high electrical conductivity and malleability
of the transition elements. The transition elements have low ionization
energies. They exhibit a wide range of oxidation states or positively charged
forms. The positive oxidation states allow transition elements to form many
different ionic and partially ionic compounds. The formation of complexes
causes the d orbitals to split into two energy sublevels, which enables many
of the complexes to absorb specific frequencies of light. Thus, the complexes
form characteristic colored solutions and compounds. Complexation reactions
sometimes enhance the relatively low solubility of some compounds.
Rare earth elements

As defined by IUPAC, a rare earth element (REE) or rare earth metal is one of a set
of seventeen chemical elements in the periodic table, specifically the fifteen
lanthanides plus scandium and yttrium.[2] Scandium and yttrium are considered
rare earth elements because they tend to occur in the same ore deposits as the
lanthanides and exhibit similar chemical properties.



Despite their name, rare earth elements (with the exception of the radioactive
promethium) are relatively plentiful in the Earth's crust, with cerium being the
25th most abundant element at 68 parts per million (similar to copper). However,
because of their geochemical properties, rare earth elements are typically
dispersed and not often found concentrated as rare earth minerals in economically
exploitable ore deposits.[3] It was the very scarcity of these minerals (previously
called "earths") that led to the term "rare earth". The first such mineral discovered
was gadolinite, a compound of cerium, yttrium, iron, silicon and other elements.
This mineral was extracted from a mine in the village of Ytterby in Sweden;
several of the rare earth elements bear names derived from this location.
Other metals

Other Metals are a term used in Periodic Chemistry when classifying the
chemical elements. Each element can usually be classified as a metal or a
non-metal based on their general Chemical and Physical Properties. Other
Metals are any of the metallic elements within Groups 13, 14, and 15 in the
Periodic Table (see the List of Other metals). The majority of metals have
higher densities than the majority of non-metals. The elements classed as
Other Metals do not exhibit variable oxidation states, and their valence
electrons are only present in their outer shell.