11260123
Descrição
FlashCards por Siobhan Lee, atualizado more than 1 year ago
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Criado por Siobhan Lee
aproximadamente 7 anos atrás
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| Questão | Responda |
| First 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 |
| 6 factors that influence the First ionization energy of an atom | Energy levels, Nuclear charge, Effective nuclear charge, screening effect, atomic radius, stability of full and 1/2 filled sublevels |
| Explain in relation to FIE: Energy levels | The more energy levels the further away the outermost electron will be from nuclear charge. Not held as strongly. Decrease in ionization energy. |
| Explain in relation to FIE: Nuclear charge | The more protons the greater the nuclear charge. A stronger force will increase ionization energy. |
| Explain in relation to FIE: Effective nuclear charge | Nuclear charge when shielding effect is accounted for |
| Explain in relation to FIE: Screening effect | More full inner shells will shield nuclear charge. Decrease in ionisation energy |
| Explain in relation to FIE: Atomic radius | The greater the radius the further the outermost electron is from the nucleus. Less of a hold. Decrease in ionisation energy |
| Explain in relation to FIE: Stability of full and 1/2 filled sub levels | A 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) |
| Second 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 |
| Atomic 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 |
| Trend of atomic radius in the periodic table | The atomic radius gets bigger as it goes down the periodic table But further down it gets smaller as it goes across the table |
| 4 factors that affect the atomic radius of an atom | Energy levels, nuclear charge, effective nuclear charge, screening effect. |
| Explain in relation to Atomic Radius: Energy levels | Increased energy levels means Outermost electrons are further from the nucleus ie greater atomic radius |
| Explain in relation to Atomic radius: Nuclear charge | The larger the nuclear charge, the more the electrons are pulled towards the nucleus. Decrease in atomic radius |
| Explain in relation to atomic radius: Screening effect | The screening effect lessens the pull on the outer electrons from the nucleus. Increase in Atomic radius |
| Explain in relation to atomic radius: Effective nuclear charge | The nuclear charge with the screening effect taken into account |
| Why 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. |
| Why 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 |
| Electro-negativity (def) | The relative attraction an atom has for a shared pair of electrons in a covalent bond |
| 4 Factors that effect the electronegativity of an element | Energy levels, Nuclear charge, Effective nuclear charge, Screening effect |
| Explain in relation to Electronegativity: Energy levels | The more energy levels the further away valence electrons are from the nucleus, not held onto as tightly, decrease in electronegativity. |
| Explain in relation to electronegativity: Nuclear charge | The stronger the nuclear charge, the stronger the hold an atom has to valence electrons, increase in electronegativity. |
| Explain in relation to electronegativity: Screening effect | Filled energy levels diminish the nuclear charge on valence electrons, lessening the electronegative value |
| Explain in relation to electronegativity: Effective nuclear charge | Nuclear charge with screening effect taken into account |
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