Where Are Metals on the Periodic Table? Types, Properties

The periodic table of elements is one of the most iconic and useful tools in the field of chemistry. At present, 118 elements are known which have similarities and differences in their properties. These are classified on these properties and are generally named as metal, non-metal and semi-metals in Periodic table. This article will explore the properties, similarities and dissimilarities and other important aspects of these elements

What Are Metals?

Metals are conductors that can lose electrons and give cations. Metals have high thermal and electricity conduction. They are ductile and malleable and used as industrial metals. These are solid at room temperature. They also have high melting and boiling points except Sodium and Potassium. They also possess high densities except for these two. The oxidation states of metals are positive because they are reactive and can lose electron easily. Metals form ionic compounds.

Where are the metals located on the periodic table

These are located on the left side and middle of the periodic table. Metals at the extremely left side have the most metallic characteristics.

How to identify metals in a periodic table?

The left side is designated to metals in periodic table and nonmetals are on the upper right. These are divided by semimetals which are in a diagonal band.

What are metals in 1 to 30 elements?

The metals in 1-30 elements are as:

Which of the first 20 elements are semi-metals?

Types of Metals on the Periodic Table

Metals are divided into further types based on chemical properties and physical properties

Alkali Metals (Group 1)

Alkali metals are located from 1st to 7th periods. These are Lithium, Sodium, Potassium, Rubidium, Cesium and Francium. They have electronic configuration of corresponding [Noble gas] ns1. Alkali refers to basic nature of the metal hydroxides. When the alkali metals react with water, they form alkaline which is a strong base and can neutralize acids.

Alkaline Earth Metals (Group 2)

These are 6 chemical elements. Beryllium, magnesium, calcium, strontium, barium and radium. These are very good conductors of heat and electricity. Normally they have a grey-white lustrous appearance. These are the heaviest elements in the groups. Their melting and boiling points are higher than alkaline metals.

Transition Metals (Groups 3-12)

Transitions metals have oxidation states or valance electron in their outermost shell. These electrons can readily form chemical bonds with other valence electrons or oxidation states like Sodium chloride (NaCl). They are hard and strong and have lustrous appearances. They also have high melting and boiling points. They are also very good conductor heat and electricity.

Other Metals

Transitions metals like aluminum and titanium have a range of applications and are industrial metals. They can be used as catalysts in petroleum and polymer industries. Catalysts have two types of homogeneous (dissolved in solution) and heterogeneous (insoluble in solution).

Lanthanides: Rare Earth Metals

These elements are a family of 15 elements having atomic numbers from 57-71 after the element Lanthanum. These all are discovered in the mineral ore called gadolinite. Lanthanides are rare earth metals and are in period 6.

Actinides: Radioactive Metals

Actinides is a family of 14 elements having atomic numbers from 89-103. They are high radioactive and have unstable nucleus. They can decay into other elements and other particles.

Properties of Metals

Physical and chemical properties of metals are discussed below

Physical Properties

The physical properties of metals are as:

• Have lustrous and shiny appearance
• Good conductors of heat and electricity and used as industrial metals
• Have high melting and boiling points and Density
• They are relatively soft, ductile and malleable
• These are solid at room temperature except for mercury
• These are dense, solid and opaque

Chemical Properties

The chemical properties of metals are as:

• These are corrosive
• Tend to lose electron easily
• They are ionically bond and form ionic compounds
• Normally have basic oxides
• Possess low electronegativity
• These are good reducing agents

How Metals Corrode and How to Prevent It

Corrosion normally occurs when atoms on the metallic surface get oxidized. This damages the entire surface with corrosion. Metals have high reactivity and can lose electrons easily to form ionic compounds. That is why they are corrosive. They lose electrons to oxygen, air or water. Oxygen is a reducing agent, so it oxidizes the metal. corrosion can be prevented in industrial metals by painting, oiling and greasing, galvanizing, electroplating, alloying and sacrificial coating.

Reactivity of Metals

The reactivity of metal is not the same for all. It changes with the trends in periodic table.

Why Does Reactivity Increase Down a Group?

Reactivity of group 1 is the lowest and it increases as you go down. It is because the size of the atom becomes larger. The outermost electron gets far away from nucleus and the attraction becomes weaker. Therefore, electrons can lose easily in the elements to form ionic compounds that are located down int the group.

Metal Reactivity Series

The metal reactivity series is the arrangement of elements in descending order of their reactivity. It is also called the activity series of metals. The arrangement of metals as per reactivity series is Fe > Ni > Sn > Pb > H > Cu > Ag > Au.

Which metals are least reactive?

Metals with the least reactivity are gold, Platinum, silver, Palladium and Osmium and Silver.

Metal Compounds and Ionic Bonding

Metals have ionic bonds. It is an electrostatic force of attraction existing between metal and nonmetals. Metals are positively charged ions in oxidation states like Sodium (Na⁺) and nonmetals have negatively charged ions like chloride (Cl^-). They form ionic compounds. Metals are positive due to losing electrons and to become ionically stable.

Electronegativity in Metals and Its Impact on Bonding

Electronegativity defines the measurement of an atom’s tendency to attract electrons toward itself. It measures the distribution of shared electron between two atoms in a bond. Electronegativity becomes larger if the atoms can attract electrons strongly in the bond.

Metals and Their Charges

Metal and nonmetals are combined and get a resultant ionic bond. Metal loses an electron and becomes a positively charged ion. While nonmetal gain electrons and become negatively charged. Positive charges are called cations. And the anions are negatively charged in oxidation states.

Metalloids: Properties and Their Role in the Periodic Table

Semimetals are the 7 elements in periodic table. These are arranged diagonally between metals and nonmetals. They are boron, silicon, germanium, antimony, arsenic, tellurium and polonium. Semimetals or metalloids physically appeared as metals but are brittle. They also are mild conductors. These elements behave chemically as nonmetals.

Alloys: Combining Metals for Improved Properties

Alloying is the process in which two or more metals are combined with metal or nonmetal. It creates new material which has properties of both the elements. Alloying changes the chemical and physical properties of element and improves their strength, corrosion resistance and other mechanical properties.

Metals vs. Nonmetals: Key Differences

The major differences between metal and nonmetal are as: