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S.Spałek

Trends in the Periodic Table

QuestionAnswer
What is the different name for atomic radius ? Covalent radius
Define atomic radius. This is Half the distance between the nuclei of two atoms of the same element that are joined together by single covalent bond.
From what reasons the values of the atomic radius increase down the groups in the Periodic Table ? 1. New energy level (shell) 2. Screening effect or inner electrons.
From what reasons the values of the atomic radius decrease across a period in the Periodic Table ? 1. Increase in effective nuclear charge. 2. No increase in the screening effect.
From what reasons the values of the first ionisation energy decrease down a group in the Periodic Table ? 1. Increasing atomic radious. 2. Screening effect or inner electrons.
From what reasons the values of the first ionisation energy increase across a period in the Periodic Table ? 1. Increase in effective nuclear charge. 2. Decreasing atomic radious.
Define second ionisation energy. This is the energy required to remove an electron from an ion with one positive charge in the gaseous state.
From what reasons the values of electronegativity increase across the periods in the Periodic Table ? 1. Increasing effective nuclear charge. 2. Decreasing atomic radious.
From what reasons the values of electronegativity decrease down the groups in the Periodic Table ? 1. Increasing atomic radious. 2. Screening effect or inner electrons.
All of the alkali metals are... ? Very reactive.
The chemical properties of elements are largely determined by...? the number of electrons in the outermost energy level.
how do we need to stored the potassium ? In the Oil.
Define bond length. This is the distance between the nuclei of two atoms, which are covalently bonded.
Define first ionization energy. This is the energy required to completely remove the most loosely bound electron from a neutral gaseous atom.
How are called Nobel gases ? Inert
Do not exist freely in nature. Halogens
Reacting with oxygen. Alkali metal + Oxygen → Metal Oxide
Reacting with water. Alkali metal + Water → Metal hydroxide + Hydrogen
Reacting with Acid. Alkali metal + Acid → Metal Chloride + Hydrogen
First ionization Na → Na^+ + e^-
Second ionization Na^+ → Na^2+ + e^-