Periodic Trends Flashcards
Definition - Ionisation Energy
The energy required to remove one mole of electrons, from one mole of gaseous atoms to produce one mole of gaseous + ions
Trend down group + justification - Ionisation Energy
Decreases. An increased number of electron shells decreases attraction from protons in the nucleus to valence electrons, making them easier to remove.
Trend across period + justification - Ionisation Energy
Increases. An increased number of protons in the nucleus, with electrons added to the same energy levels increases the attraction from the protons to the valence electrons, making them harder to remove.
Defintion - Electronegativity
The attraction between the nucleus and shared bonding electrons.
Trend down group + justification - Electronegativity
Decreases. An increased number of electron shells decreases attraction from protons in the nucleus to valence electrons, making the element less electronegative.
Trend across period + justification - Electronegativity
Increases. An increased number of protons in the nucleus, with electrons added to the same energy levels increases the attraction from the protons to the valence electrons, making the element more electronegative.
Defintion - Atomic Radius
Distance from nucleus to valence electrons
Trend down group + justification - Atomic Radius
Increases. An increased number of electron shells decreases attraction from protons in the nucleus to valence electrons, making the radius bigger.
Trend across period + justification - Atomic Radius
Decreases. An increased number of protons in the nucleus, with electrons added to the same energy levels increases the attraction from the protons to the valence electrons, making the radius smaller.
Compare radii atom to anion + justification
Anion (-) has a larger radius than the atom. The number of protons stays the same and electrons are added to the same shell. Increases valence electron-electron repulsion, which causes the radii to increase.
Compare atom to cation (Na to Na+) + justification
Cation(+) has a smaller radius than the atom. The number of protons stays the same, when the valence electron is removed an entire energy level is removed. Increasing the attraction from protons to valence electrons and making the radius smaller.
Compare atom to cation (Mg to Mg+) + justification
Cation(+) has a smaller radius than the atom. The number of protons stays the same, when the valence electron is removed there is less valence electron-electron repulsion, and greater attraction from the protons to valence electrons, making the radius smaller.