Ionization Energy Fundamentals
Explore the fundamentals of ionization energy. Understand how energy is needed to overcome the attraction between electrons and the nucleus to remove the valence electron. This lesson covers the concept, definition, and formulas for calculating first, second, and third ionization energies.
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Ionization Energy Fundamentals
Quiz • 20 Questions
Ionization Energy Fundamentals - Flashcards
Flashcards • 11 Cards
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List of Questions20 questions
- Question 1
- Ionization energy is always positive because energy is required to overcome the attraction between the positively charged nucleus and the negatively charged electron in order to remove the electron from the atom.
- Question 2
- A higher number of protons in the nucleus results in a greater positive charge, leading to a stronger attraction for the electrons. This, in turn, increases the ionization energy required to remove an electron.
- Question 3
- As the atomic radius increases, the outermost electrons are further from the nucleus and experience a weaker attraction. Therefore, less energy is required to remove the electron, resulting in a lower ionization energy.
- Question 4
- Electron shielding reduces the effective nuclear charge experienced by the outer electrons. The more inner electrons there are, the higher the shielding, and the less energy needed to ionize the electron.
- Question 5
- Generally, ionization energy increases across a period due to an increase in nuclear charge and a decrease in atomic radius.
- Question 6
- Ionization energy decreases down a group as atomic radius and electron shielding increase. The valence electrons are further from the nucleus and more shielded from its attractive force.
- Question 7
- Each successive ionization requires more energy because after each electron removal, the positive charge of the ion increases, leading to a stronger attraction for the remaining electrons.
- Question 8
- A large jump signifies that the electron was removed from an energy level closer to the nucleus, where it experiences a greater attraction due to less shielding and a shorter distance.
- Question 9
- Boron's valence electron is in the 2p subshell, while Beryllium's valence electron is in the 2s subshell. The higher energy 2p subshell makes Boron's electron easier to remove, hence lower ionization energy.
- Question 10
- Oxygen has paired electrons in its 2p orbitals, which cause repulsion and make it easier to remove one of these electrons, resulting in a lower ionization energy compared to nitrogen, which has unpaired electrons.
- Question 11
- Ionization energy is the energy required to remove one mole of electrons from one mole of gaseous atoms to form one mole of gaseous 1+ ions. It is measured in kJ/mol (kilojoules per mole).
- Question 12
- A valence electron is an electron in the outermost shell of an atom. Ionization energy is the energy required to remove an electron (typically a valence electron) from the atom.
- Question 13
- First ionization energy: X(g) -> X+(g) + e-. Second ionization energy: X+(g) -> X2+(g) + e-. Third ionization energy: X2+(g) -> X3+(g) + e-. Each subsequent ionization requires removing an electron from an increasingly positive ion.
- Question 14
- An endothermic reaction requires the absorption of energy/heat. Ionization energy values are positive and endothermic because energy must be supplied to overcome the attraction between protons and electrons.
- Question 15
- The more inner electrons, the higher the shielding, and the less energy needed to ionize the electron. Shielding increases as you move down a group as you add additional electron energy levels.
- Question 16
- A high nuclear charge means there are more protons in the nucleus, leading to a stronger attraction for electrons, and therefore more energy is required to ionize it.
- Question 17
- Ionization energy decreases as atomic radius increases because the outer electrons are further away from the attractive powers of the nucleus, thus requiring less energy to ionize.
- Question 18
- The charge of the elements as you go down the group increases which will increases ionization energy, however the combination of the 3 factors causes the effect of the charge to be canceled out by the other two factor's.
- Question 19
- As successive electrons are removed, the proton to electron ratio increases, leading to more positive charge attracting the remaining electrons each time and causing higher ionization energy.
- Question 20
- The two main reasons why the first ionization energy may differ from trends are higher orbitals are easier to remove and The paired electrons in orbitals cause a repulsion.
List of Flashcards11 flashcards
- Card 1HintThink about removing an electron from a gaseous atom.Memory TipFirst electron, first ionization energy.
- Card 2HintIt's the electron in the outermost...Memory TipValence = outermost.
- Card 3HintConnected to removing an electron...Memory TipIonize = remove electrons.
- Card 4HintEnters with energy...Memory TipEndo- means 'in', thermic- means 'heat'.
- Card 5HintThe force due to the nucleus's...Memory TipMore protons = higher nuclear charge.
- Card 6HintThink about how far.Memory TipRadius measures from center outwards.
- Card 7HintInner electrons...Memory TipLike a shield protecting from attraction.
- Card 8HintWhat happens to nuclear charge and atomic radius?Memory TipThink across a row.
- Card 9HintWhat happens to the distance from nucleus and shielding?Memory TipThink down a column.
- Card 10HintEach removal is...Memory TipSuccessive needs more energy.
- Card 11HintHow energy level affects amount to remove electron?Memory TipLarge gaps show next energy level.