What are the properties of metals? Where are metals found on the periodic table?

The periodic table is a comprehensive chart that organizes all the known elements based on their atomic number, electron configurations, and recurring chemical properties. Elements are arranged in rows, known as periods, and columns, called groups or families. Metals, which are the focus of our interest, predominantly occupy the left side and the center of the periodic table. Each metal is placed according to its atomic structure, which neatly correlates with its metallic properties.

Metals are distinguished by a set of properties that make them incredibly useful in various applications. Their luster gives them a shiny appearance, especially when freshly cut or polished. Metals typically have high density and exhibit high melting and boiling points compared to non-metals. Another key characteristic is malleability, which allows metals to be hammered or rolled into thin sheets without breaking. Coupled with ductility, the ability to be drawn into wires, metals are immensely versatile. Their conductivity is also a standout property, with metals being excellent conductors of both heat and electricity. Lastly, metals are inclined to lose electrons and form cations or positive ions in chemical reactions.

Conductivity in metals is a result of the movement of free electrons within their structure. Unlike ionic compounds where ions are fixed in positions, metals have a sea of delocalized electrons that are not bound to any particular atom. These free electrons act as charge carriers and can move easily throughout the metallic lattice, allowing metals to conduct heat and electricity efficiently. This property is crucial in applications ranging from power transmission to the functioning of electronic devices.

Alkali metals are the group 1 elements, excluding hydrogen, and are characterized by their single valence electron which makes them highly reactive. They are soft, have a low density, and display increasing reactivity as you move down the group. Alkali metals include lithium, sodium, and potassium, among others, and they readily lose their single valence electron to form +1 cations. In their pure form, they have a shiny luster but tarnish quickly when exposed to air due to their reactivity.

Right next to the alkali metals on the periodic table are the alkaline earth metals, belonging to group 2. These include beryllium, magnesium, calcium, and others. With two valence electrons, alkaline earth metals form +2 cations and are less reactive than alkali metals. They still share many common metallic properties such as luster and high conductivity of heat and electricity. They are also more dense and have higher melting points compared to alkali metals.

Transition metals are found in the d-block of the periodic table and are known for their ability to form various oxidation states and colored compounds. These metals, including iron, copper, and gold, have an electron configuration that allows the presence of unpaired d-electrons. This feature grants them interesting magnetic and catalytic properties. Transition metals are also noted for their strength, resistance to corrosion, and metallic luster. They are widely used in construction, wiring, and as catalysts in industrial reactions.

The lanthanides consist of elements 57 through 71 and are part of the f-block of the periodic table. These metals are also referred to as the 'rare earth elements,' although they are not particularly rare. Lanthanides are known for their high magnetic susceptibility and phosphorescence, which are valuable in various high-tech applications. They are typically shiny and silvery in appearance but react slowly with water and oxidize quickly in air.

Below the lanthanides are the actinides, occupying elements 89 through 103. These metals are all radioactive, with only the first four (actinium through plutonium) occurring naturally. The rest are synthetic and have been created in laboratories. Actinides are characterized by their highly radioactive nature and are used in nuclear reactors and weapons. They are also dense and have complex electron configurations that lead to a variety of oxidation states and chemical behaviors.