Flashcards
Trends in the Periodic table
Cards in this deck (24)
- 1First ionization energy of an atom (def)The minimum energy required to remove the outermost, most loosely bound electron from one mole of a gaseous element in its neutral ground state
- 26 factors that influence the First ionization energy of an atomEnergy levels, Nuclear charge, Effective nuclear charge, screening effect, atomic radius, stability of full and 1/2 filled sublevels
- 3Explain in relation to FIE: Energy levelsThe more energy levels the further away the outermost electron will be from nuclear charge.
Not held as strongly.
Decrease in ionization energy. - 4Explain in relation to FIE: Nuclear chargeThe more protons the greater the nuclear charge.
A stronger force will increase ionization energy. - 5Explain in relation to FIE: Effective nuclear chargeNuclear charge when shielding effect is accounted for
- 6Explain in relation to FIE: Screening effectMore full inner shells will shield nuclear charge.
Decrease in ionisation energy - 7Explain in relation to FIE: Atomic radiusThe greater the radius the further the outermost electron is from the nucleus.
Less of a hold.
Decrease in ionisation energy - 8Explain in relation to FIE: Stability of full and 1/2 filled sub levelsA full sub-level is more stable than a 1/2 filled sub-level.
A 1/2 filled sub-level is more stable than a partially filled sub-level.
Full or 1/2 filled sublevel
will not want to become partially filled.
Increase inionization.
G2→ full s sub-level.
G5→ 1/2 filled p sub-level.
(As greater energy is required it proves the existence of sub-levels) - 9Second Ionisation Energy (def)The minimum energy required to remove the 2nd most outermost, most loosely bound electron from one mole of a charged gaseous species in its ground state
- 10Atomic radius (def)Atomic radius is 1/2 the distance from the centre of nuclei of 2 of the same atoms joined by a single covalent bond
- 11Trend of atomic radius in the periodic tableThe atomic radius gets bigger as it goes down the periodic table
But further down it gets smaller as it goes across the table - 124 factors that affect the atomic radius of an atomEnergy levels, nuclear charge, effective nuclear charge, screening effect.
- 13Explain in relation to Atomic Radius: Energy levelsIncreased energy levels means Outermost electrons are further from the nucleus ie greater atomic radius
- 14Explain in relation to Atomic radius: Nuclear chargeThe larger the nuclear charge, the more the electrons are pulled towards the nucleus. Decrease in atomic radius
- 15Explain in relation to atomic radius: Screening effectThe screening effect lessens the pull on the outer electrons from the nucleus. Increase in Atomic radius
- 16Explain in relation to atomic radius: Effective nuclear chargeThe nuclear charge with the screening effect taken into account
- 17Why does Atomic Radius decrease across the periodic table?Increase in effective nuclear charge, as nuclear charge increases (more protons) but shielding effect doesn't. Same amount of energy levels.
- 18Why does Atomic Radius increase down the periodic table?More energy levels. Change in nuclear charge combatted by increased shielding effect due to more energy levels. Therefore there is a decrease in effective nuclear charge
- 19Electro-negativity (def)The relative attraction an atom has for a shared pair of electrons in a covalent bond
- 204 Factors that effect the electronegativity of an elementEnergy levels, Nuclear charge, Effective nuclear charge, Screening effect
- 21Explain in relation to Electronegativity: Energy levelsThe more energy levels the further away valence electrons are from the nucleus, not held onto as tightly, decrease in electronegativity.
- 22Explain in relation to electronegativity: Nuclear chargeThe stronger the nuclear charge, the stronger the hold an atom has to valence electrons, increase in electronegativity.
- 23Explain in relation to electronegativity: Screening effectFilled energy levels diminish the nuclear charge on valence electrons, lessening the electronegative value
- 24Explain in relation to electronegativity: Effective nuclear chargeNuclear charge with screening effect taken into account
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- Flashcards on Trends in the Periodic table , created by Siobhan Lee on 06/11/2017.
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