Gibbs

Trends in Different groups in the Periodic Table: 

Trends in Different groups in the Periodic Table By Jonathan Gibbs

Alkali MetalsProperties: 

Alkali Metals Properties · They are never found in elemental form in nature · Very soft · stored under mineral oil in laboratory to keep from reacting · tarnish easily · have low melting points and low density · silver colored

Properties (continued): 

Properties (continued) · When moving down the group the elements have ·  decreasing electronegativity ·  decreasing melting and boiling point ·   decreasing melting and boiling point ·  decreasing melting and boiling point ·  increasing reactivity

Alkali metals reaction with water: 

Alkali metals reaction with water ovigorous reactions with water o reactions worsen as you move down the group o Alkali metal + water → Alkali metal hydroxide + hydrogen gas o  Reactions can cause flames and sometimes explosions

Alkali metals reaction with ammonia : 

Alkali metals reaction with ammonia dissolve in liquid ammonia to give blue solutions that are paramagnetic Saturated solutions are a deep purple color.

Alkaline earth metals: 

Alkaline earth metals beryllium (Be), magnesium (Mg), calcium (Ca), strontium (Sr), barium (Ba) and radium (Ra) Well characterised homologous behaviour down the group Always combined with nonmetals in nature Some are very important nutrients silvery colored, soft, low-density metal two electrons in their outermost shell

Alkaline earth metals (continued): 

Alkaline earth metals (continued) the energetically preferred state of achieving a filled electron shell is to lose two electrons to form doubly charged positive ions react readily with halogens to form ionic with water, though not as rapidly as the alkali metals, to form strongly alkaline (basic) hydroxides Beryllium is an exception: It does not react with water or steam, and its halides are covalent

Lanthanide: 

Lanthanide comprises the 15 elements with atomic numbers 57 through 71, from lanthanum to lutetium All lanthanides are f-block elements, corresponding to the filling of the 4f electron shell, except for lutetium which is a d-block lanthanide fairly abundant in nature Cerium is the 26th most abundant element in the Earth's crust occur as trivalent cations in nature two of the lathanides have radioactive isotopes with long half-lives They obey the Oddo-Harkins rule, which states that odd-numbered elements are less abundant than their even-numbered neighbors. widely used in lasers

Lanthanide (Continued): 

Lanthanide (Continued) deflect UV and Infrared electromagnetic radiation and are commonly used in the production of sunglass lenses Due to their specific electronic configurations, lanthanide atoms tend to lose three electrons All lanthanides closely resemble lanthanum shiny and silvery-white and tarnish easily when exposed to air are used to make steel react violently with most nonmetals are relatively soft but their hardness increases with their atomic number Lanthanides burn in air high melting and boiling points

Actinide: 

Actinide encompasses the 15 chemical elements that lie between actinium and lawrencium on the periodic table, with atomic numbers 89 – 103 display less similarity in their chemical properties than the lanthanide series radioactive Only thorium and uranium occur naturally in the earth's crust in anything more than trace quantities Neptunium and Plutonium have been known to show up naturally in trace amounts in uranium ores as a result of decay or bombardment The remaining actinides were discovered in nuclear fallout, or were synthesized in particle collide The latter half of the series possess exceedingly short half-lives.

Transition Metals: 

Transition Metals 40 chemical elements 21 to 30, 39 to 48, 71 to 80, and 103 to 112 Less reactive Hard metals Used in jewelry and constructions element whose atom has an incomplete d sub-shell, or which can give rise to cations with an incomplete d sub-shell

Transition Metals (Continued): 

Transition Metals (Continued) They often form colored compounds They can have a variety of different oxidation states At least one of their compounds has an incomplete d-electron subshell. They are often good catalysts They are silvery-blue at room temperature (except copper and gold). They are solids at room temperature (except mercury). They form complex ions (aqua ones included). They are often paramagnetic.

Transition Metals (Continued): 

Transition Metals (Continued) high tensile strength, density and melting and boiling points multiple stable oxidation states The number of oxidation states of each ion increases up to Mn, after which they decrease. Later transition metals have a stronger attraction between protons and electrons (since there are more of each present), which then would require more energy to remove the electrons. When the elements are in lower oxidation states, they can be found as simple ions. However, transition metals in higher oxidation states are usually bonded covalently to electronegative elements like oxygen or fluorine, forming polyatomic ions such as chromate, vanadate, or permanganate

Transition Metals (Continued): 

Transition Metals (Continued) Ions in higher oxidation states tend to make good oxidizing agents, whereas elements in low oxidation states become reducing agents. The 2+ ions across the period start as strong reducing agents and become more stable. The 3+ ions start stable and become more oxidizing across the period. form good homogeneous or heterogeneous catalysts able to form numerous oxidation states, and as such, are able to form new compounds during a reaction providing an alternative route with a lower overall activation energy Good catalysts

Earth metals: 

Earth metals boron (B), aluminum (Al), gallium (Ga), indium (In), thallium (Tl), and ununtrium (Uut) (unconfirmed). Poor metals Boron is a metalloid The rest are poor metals 3 valence electrons

Carbon Family: 

Carbon Family carbon (C), silicon (Si), germanium (Ge), tin (Sn), lead (Pb), and ununquadium (Uuq). Each of the elements in this group has 4 electrons in its outer energy level Elements important to life and computers Important semiconductors Carbon is the basis of life All look really different The tendency to lose electrons increases as the size of the atom increases Carbon alone forms negative ions Tin and lead both are metals while ununquadium is a synthetic short-lived radioactive metal Can for up to 4 bonds React in similar ways

Pnictogen or Nitrogen Family : 

Pnictogen or Nitrogen Family phosphorus (P), arsenic (As), antimony (Sb), bismuth (Bi) and ununpentium (Uup) (unconfirmed) Nitrogen makes up ¾ atmosphere Important in living things 5 electrons in their outermost shell

Chalcogen: 

Chalcogen oxygen (O), sulfur (S), selenium (Se), tellurium (Te), the radioactive polonium (Po), and the synthetic ununhexium (Uuh). Oxygen is needed for respiration Commonly minerals Oxygen and sulfur are nonmetals polonium, selenium and tellurium are metalloid semiconductors tellurium and selenium is referred to as a metal when in elemental form. common as minerals

Halogen: 

Halogen fluorine, F, chlorine, Cl, bromine, Br, iodine, I, astatine Very reactive Volatile, diatomic non metals Always found combined with another element in nature Used as disinfectants and to strengthen teeth nonmetal elements found in the environment only in compounds or as ions. also be found as natural products in living organisms

Halogen (continued): 

Halogen (continued) In their elemental forms, the halogens exist as diatomic molecules only periodic table group exhibiting all three states of matter. Trends as you move down the list decreasing electronegativity decreasing reactivity Increasing melting and boiling point. Highly reactive harmful or lethal to biological organisms in sufficient quantities Fluorine is the most reactive element in existence

Halogen (Continued): 

Halogen (Continued) Both Chlorine and iodine are used as disinfectants for drinking water, swimming pools, fresh wounds, dishes, and surfaces react with each other to form interhalogen compounds The properties and behaviour of a diatomic interhalogen compound tend to be intermediate between those of its parent halogens Some properties, however, are found in neither parent halogen all form binary compounds with hydrogen

Noble Gases: 

Noble Gases Helium, Neon, Argon, Krypton, Xenon, Radon Highly unreactive monatomic gases Used in neon signs Used in blimps Have a full valence shell occur as odorless, colorless, monatomic gases rarely react with other elements no conventional compounds of helium or neon have yet been prepared.

Noble Gases (Continued): 

Noble Gases (Continued) Xenon and krypton are known to show some reactivity in the laboratory. Recently argon compounds have also been successfully characterised high ionization energies and negligible electro negativities weak inter-atomic forces of attraction, and consequently very low melting points and boiling points. Krypton is also used in lasers, and are used by doctors for eye surgery

Work Cited: 

Work Cited http://www.ucc.ie/academic/chem/dolchem/html/elem/group.html http://www.chemsoc.org/viselements/Pages/pertable_int.htm