As we go down a group, the outermost electron of an atom is placed in a shell that is further from the nucleus. This means it experiences the electrostatic attraction Going down the group, the first ionisation energy decreases. There is more shielding between the nucleus and the outer electrons and the distance between the Progressing down group 2, the atomic radius increases due to the extra shell of electrons for each element. Going down the group, the first ionisation energy DOWN a Group: Atomic radius INCREASES as you go DOWN a Group because each successive Period (row) has an additional occupied energy level. If you
Progressing down group 2, the atomic radius increases due to the extra shell of electrons for each element. Going down the group, the first ionisation energy decreases. There is more shielding between the nucleus and the outer electrons and the distance between the nucleus and the outer electron increases and therefore the force of attraction between the nucleus and outer most electrons is reduced. The covalent radius (a measure of how large individual atoms are) shows different trends if you are moving across a period or down a group. A comparison of the relative covalent radii of atoms is Trends in atomic radius down a group It is fairly obvious that the atoms get bigger as you go down groups. The reason is equally obvious - you are adding extra layers of electrons. Trends in atomic radius across periods
Going down the group, the first ionisation energy decreases. There is more shielding between the nucleus and the outer electrons and the distance between the Progressing down group 2, the atomic radius increases due to the extra shell of electrons for each element. Going down the group, the first ionisation energy
Down a group, \(n\) increases and \(Z_{eff}\) increases slightly; the ionization energy decreases. Electron Affinity Trends As the name suggests, electron affinity is the ability of an atom to accept an electron. The general trend of atomic radius is that it increases as you move down a group, and decreases as you move to the right across a period. Atomic radius can be linked to core charge. CORE CHARGE = PROTONS - NON-VALENCE ELECTRONS. The core charge is simply an expression of the attractive force that the centre of - The number of energy levels increases as you move down a group as the number of electrons increases. Each subsequent energy level is further from the nucleus than the last. Therefore, the atomic radius increases as the group and energy levels increase.
The covalent radius (a measure of how large individual atoms are) shows different trends if you are moving across a period or down a group. A comparison of the relative covalent radii of atoms is Trends in atomic radius down a group It is fairly obvious that the atoms get bigger as you go down groups. The reason is equally obvious - you are adding extra layers of electrons. Trends in atomic radius across periods Non-metals Period - reactivity increases as you go from the left to the right across a period. Group - reactivity decreases as you go down the group. The farther right and up you go on the periodic table, the higher the electronegativity, resulting in a more vigorous exchange of electron. From top to bottom down a group, electronegativity decreases. This is because atomic number increases down a group, and thus there is an increased distance between the valence electrons and nucleus, or a greater atomic radius. Important exceptions of the above rules include the noble gases, lanthanides, and actinides. Trends in energy of valence electrons: ⚛ The valence shell electrons of elements in the same Period of the Periodic Table occupy the same energy level (shell). 1 . ⚛ Going down a Group of the Periodic Table from top to bottom, the energy of the valence shell electrons increases.