Alkali Metals

Alkali metals are from Group 1 of the Periodic table and have a single electron in their outer shell. Alkaline-Earth metals are in group 2 of the periodic table and have 2 electrons in their outer shell.

1. Alkali metals are soft and highly reactive.

2. They have low melting points and densities.

The reactivity of alkali metals increases as you move down Group 1 from lithium to francium. This trend is due to the decreasing ionization energy, which makes it easier for the alkali metals to lose their outermost electron and become more reactive.

Alkali metals have 1 electron in their outer shell, which makes them highly reactive. They easily lose this electron to form positively charged ions, making them good reducing agents. This electron configuration and reactivity are key factors influencing the properties of alkali metals.

Alkali metals such as sodium and potassium are difficult to detect in qualitative analysis schemes because they are highly reactive and can easily form compounds with other elements in the solution, making their distinctive properties harder to identify. Their reactivity can also cause interference with other ions in the solution, leading to false positive or negative results in the analysis.

Francium and cesium, the two with the highest atomic numbers.

Table salt is formed from sodium ion ( an alkali metal) and chloride ion ( a halogen)

Forces have an indirect impact on the atomic radius of alkali metals. As you move down a group of alkali metals in the periodic table, the atomic radius typically increases due to increased electron shells. The forces between the electrons and nucleus (electrostatic forces) contribute to the overall size of the atom in terms of atomic radius.

Alkali metals have a low density because they have a single valence electron that is loosely held, leading to larger atomic size and lower atomic mass. This results in a less compact arrangement of atoms, contributing to the low density observed in alkali metals.

From BCIT.ca: The alkali metals show a decrease in melting points and boiling points due to the weaker metallic bonds between atoms as their size increase down the group.
From AUS-e-TUTE: melting point decreases down the Group as the elements become less metallic in nature
From okstate.edu: As one goes down the Periodic Table, the metallic radius of alkali metals increases. The increase in radius results in much decreased attractive forces between atoms within the liquid metals, resulting in a decrease in heat of vaporization and boiling points [and melting points] because less heat is needed to separate atoms from the liquid [or solid] state within the larger alkali metals. See Web Links to the left for the original sources.

Yes, iron is considered a transition metal. Transition metals are characterized by their partially filled d orbitals in the outermost shell of electrons, which gives them unique properties such as forming colored compounds and catalyzing reactions. Iron fits this criteria and is commonly classified as a transition metal in the periodic table.

The electron configuration is why they react.

The Alkali metals have one electron in their outer shell and to complete their outer shell need 7 more electrons. They can give, take or share electrons with other atoms.

This is when the Halogens come in handy. The Halogens have 7 electrons in their outer shells, and need one more to complete the outer shell.

These can react very easily because they have both the perfect amounts to fill their outer shells and become compounds. Other atoms with other amounts to become atoms not ions needs another element to react with.

Hope this helps, Matt.

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The elements designated as alkali metals are lithium (Li), sodium (Na), potassium (K), rubidium (Rb), cesium (Cs), and francium (Fr). They are all located in Group 1 of the periodic table. Alkali metals are highly reactive and tend to form ionic compounds with nonmetals.

Calcium is the alkaline earth metal that has electrons in exactly three energy levels. Its electron configuration is [Ar] 4s2, and it has two electrons in the 4s orbital and a total of three energy levels.

Gold is the least active metal because it does not easily react with other elements or substances. It is highly resistant to corrosion and oxidation, making it a popular choice for jewelry and other applications where durability is important.

Since metal is a conductor the electrons easily transfer throughout the entire object therefore the temporary charge put on one part by the wool will discharge by traveling through the rod to your hand, thus grounding it.

Alkali metals are extremely reactive because they have one electron in their outermost energy level, which they readily lose to achieve a stable configuration. This loss of an electron results in the formation of a positively charged ion, making alkali metals highly reactive with substances that can gain an electron easily, such as water and halogens.

The outer electron configuration of an alkali metal is one electron in the s subshell. This electron is easily lost to form a cation with a full valence shell, resulting in the high reactivity of alkali metals.

Metals typically have high electrical and thermal conductivity, malleability, ductility, and shiny luster. They tend to be solid at room temperature (except for mercury), are typically good at forming alloys, and can exhibit metallic bonding.

They occupy all but the extreme top left, position (H) and the top right corner of the Periodic table.

Woo! Long list, but here it is:

Sodium

Potassium

Rubidium

Cesium

Francium

Beryllium

Magnesium

Calcium

Strontium

Barium

Radium

Aluminum

Gallium

Indium

Tin

Thallium

Lead

Bismuth

Element 113 - Ununtrium - will probably be a basic metal.

Element 114 - Ununquadium - will probably be a basic metal.

Element 115 - Ununpentium - will probably be a basic metal.

Element 116 - Ununhexium - will probably be a basic metal.

Scandium

Titanium

Vanadium

Chromium

Manganese

Iron

Cobalt

Nickel

Copper

Zinc

Yttrium

Zirconium

Niobium

Molybdenum

Technetium

Ruthenium

Rhodium

Palladium

Silver

Cadmium

Lanthanum

Hafnium

Tantalum

Tungsten

Rhenium

Osmium

Iridium

Platinum

Gold

Mercury

Actinium

Rutherfordium

Dubnium

Seaborgium

Bohrium

Hassium

Meitnerium

Darmstadtium

Roentgenium

Element 112 - Ununbium - Presumably will be a transition metal.

Cerium

Praseodymium

Neodymium

Promethium

Samarium

Europium

Gadolinium

Terbium

Dysprosium

Holmium

Erbium

Thulium

Ytterbium

Lutetium

Thorium

Protactinium

Uranium

Neptunium

Plutonium

Americium

Curium

Berkelium

Californium

Einsteinium

Fermium

Mendelevium

Nobelium

Lawrencium

Krypton is a gas, one of the noble or intert gases.

When an alkali metal is placed in water it will float and produce a gas like hydrogen which ignites in the presence of oxygen - producing a flame. The reactions get more and more vigorous as you move down the group.

I may only be a grade 9 student but I think I may know this. Lithium, Sodium and Potassium are HIGHLY reactive to water. Lithium lightly sizzles when it reacts with water, and it produces a small amount of gas. Sodium reacts a little more, it bubbles on the water and creates a large amount of gas. Potassium has the most violent reaction to water, it actually pops when it comes into contact. It really explodes when you put it in water. It almost produces a red flame on top of the water.

So you see, they are ordered by the level of reactivity.

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Francium is the most reactive and electronegative chemical element; unfortunately is extremely rare and currently not available for chemical experiments. Also is very radioactive.

The increasing order of reactivity with water is: Lithium, Sodium, Potassium, Rubidium, Caesium, Francium.

The reactivity of chemical elements is controlled by their electronegativity; this parameter is decreasing from lithium to francium. The minimal electronegativity is equivalent to maximal reactivity.