Periodic Table
By: Karley Anderson
Location
The transition metals or transition elements traditionally occupy all of the d block of the periodic table. The name transition metal refers to the position in the periodic table of elements. The transition elements represent the successive addition of electrons to the d atomic orbitals of the atoms. In this way, the transition metals represent the transition between group 2 (2A) elements and group 13 (3A) elements.
Charecteristics
- they form colored compounds.
- they are good conductors of heat and electricity.
- they can be hammered or bent into shape easily.
- they are less reactive than alkali metals such as sodium.
- they have high melting points - but mercury is a liquid at room temperature.
Example
Copper pennies is an example of transition metals.
Location
The nonmetals are located on the upper right side of the periodic table. Nonmetals are separated from metals by a line that cuts diagonally through the region of the periodic table containing elements with partially filled p orbitals. Technically the halogens and noble gases are nonmetals, but the nonmetal element group usually is considered to consist of hydrogen, carbon, nitrogen, oxygen, phosphorus, sulfur, and selenium.
Charecteristics
Semi-conductors, which means that they both insulate and conduct electricity. This semi-conducting property makes Metalloids very useful as a computer chip material. Examples of metalloid elements are Silicon and Boron.
Example
Helium
Water
Water
Location
Metals are located on the left side and the middle of the periodic table. Group IA and Group IIA (the alkali metals) are the most active metals. The transition elements, groups IB to VIIIB, are also considered metals. The basic metals are the element to the right of the transition metals. The bottom two rows of elements beneath the body of the periodic table are the lanthanides and actinides, which are also metals.
Charecteristics
- Metals are generally shiny, malleable, and hard. Metals are also good conductors of electricity. ...
- Non-metals do not conduct heat or electricity very well.
- Metalloids share characteristics of both metals and non-metals and are also called semimetals.
Example
copper (), zinc (), gold (), silver (), tin () and lead ().
Location
The lanthanides are located in block 5d of the periodic table. The first 5d transition element is either lanthanum or lutetium, depending on how you interpret the periodic trends of the elements.
Charecteristics
- Silvery-white metals that tarnish when exposed to air, forming their oxides.
- Relatively soft metals. Hardness increases somewhat with higher atomic number.
Location
There are two rows under the periodic table: the lanthanide and actinide series. The lanthanide series can be found naturally on Earth. Only one element in the series is radioactive. The actinide series is much different.
Charecteristics
- All are radioactive.
- Actinides are highly electropositive.
- The metals tarnish readily in air.
- Actinides are very dense metals with distinctive structures. Numerous allotropes may be formed (plutonium has at least 6 allotropes!).
Location
The halogens are five non-metallic elements found in group 17 of the periodic table. The term "halogen" means "salt-former" and compounds containing halogens are called "salts". All halogens have 7 electrons in their outer shells, giving them an oxidation number of -1.
Charecteristics
A unique characteristic of halogens is that they are the only element group that includes elements that belong to all three classical states of matter: solid, liquid, and gas at room temperature. The halogens, as a group, are extremely reactive. In their elemental form, they are found as diatomic molecules.
Example
Fluoride can be found in many everyday products, including toothpaste, vitamin supplements, baby formulas, and even public water. However, overconsumption of fluoride can be fatal.
Location
The alkali metals are a group (column) in the periodic table consisting of the chemical elements lithium (Li), sodium (Na), [note 1] potassium (K), [note 2] rubidium (Rb), caesium (Cs), [note 3] and francium (Fr).
Charecteristics
As with all metals, the alkali metals are malleable, ductile, and are good conductors of heat and electricity. The alkali metals are softer than most other metals. Cesium and francium are the most reactive elements in this group.
Example
Spodumene, an important lithium mineral
Location
The metalloids; boron (B), silicon (Si), germanium (Ge), arsenic (As), antimony (Sb), tellurium (Te), polonium (Po) and astatine (At) are the elements found along the step like line between metals and non-metals of the periodic table.
Charecteristics
- Electronegativities between those of metals and nonmetals
- Ionization energies between those of metals and nonmetals
- Possess some characteristics of metals/some of nonmetals
Example
Metalloid like silicon is a very good semi-conductor. Some of them are used for making transistors. So their uses are basically in the electronic industry.
Location
The halogens are five non-metallic elements found in group 17 of the periodic table. The term "halogen" means "salt-former" and compounds containing halogens are called "salts".
Charecteristics
- Solid- Iodine, Astatine
- Liquid- Bromine
- Gas- Fluorine, Chlorine
Location
So we just covered the alkali metals in Group I. You will find the alkaline earth metals right next door in Group II. This is the second most reactive family of elements in the periodic table. Do you know why they are called alkaline? When these compounds are mixed in solutions, they are likely to form solutions with a pH greater than 7. Those higher pH levels means that they are defined as "basic" or "alkaline" solutions.
Charecteristics
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Not found freely in nature
-
Present in the earth's crust but not in their basic form
-
Distributed in rock structure
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Two electrons in their outer shell
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High boiling points
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High melting points
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Low density
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Low electron affinity
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Low electronegativity
Ionization
Ionization is the process by which an atom or a molecule acquires a negative or positive charge by gaining or losing electrons to form ions, often in conjunction with other chemical changes.
Electronegativity
Electronegativity, symbol χ, is a chemical property that describes the tendency of an atom or a functional group to attract electrons (or electron density) towards itself. An atom's electronegativity is affected by both its atomic number and the distance at which its valence electrons reside from the charged nucleus.
Atomic Radius
The atomic radius of a chemical element is a measure of the size of its atoms, usually the mean or typical distance from the nucleus to the boundary of the surrounding cloud of electrons. Since the boundary is not a well-defined physical entity, there are various non-equivalent definitions of atomic radius.