What is the trend in group 1 elements?

What is the trend in group 1 elements?

Group 1 elements are known as Alkali Metals. They are called s-block elements because their highest energy electrons appear in the s subshell. Progressing down group 1, the atomic radius increases due to the extra shell of electrons for each element. Going down the group, the first ionisation energy decreases.

Which best describes how electrons fill orbitals in the periodic table?

Answer: The statement that best describes how electrons fill orbitals in the periodic table is “Electrons fill orbitals in order of their increasing energy from left to right”.

Is carbon a main group element?

In chemistry and atomic physics, the main group is the group of elements (sometimes called the representative elements) whose lightest members are represented by helium, lithium, beryllium, boron, carbon, nitrogen, oxygen, and fluorine as arranged in the periodic table of the elements.

Which groups are somewhat reactive?

Alkali metals (Group 1) elements are soft, very reactive metals; Alkaline Earth metals (Group 2) are somewhat reactive metals that react easily with oxygen; Halogens (Group 17) are very reactive non-metals; Noble Gases (Group 18) are non-reactive, non-metals that are gases.

Which two groups of elements are the most reactive?

Group 1: Hydrogen and Alkali Metals It is the most common element in the universe. All the other elements in group 1 are alkali metals. They are the most reactive of all metals, and along with the elements in group 17, the most reactive elements.

Why is fluorine a reactive element?

The thing that makes fluorine so reactive is its electronegativity. Electronegativity is the tendency of an atom to attract a shared pair of electrons. Therefore, since fluorine has a higher electronegatvity than chlorine, fluorine is more reactive.

What is chlorine reactive to?

Chlorine is intermediate in reactivity between fluorine and bromine, and is one of the most reactive elements. Chlorine tends to react with compounds including M–M, M–H, or M–C bonds to form M–Cl bonds.