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Questions and Answers
What happens to atomic radii as you move across a period?
What happens to atomic radii as you move across a period?
Noble gases have atomic radii because they form intramolecular bonds.
Noble gases have atomic radii because they form intramolecular bonds.
False (B)
What is the first ionisation energy?
What is the first ionisation energy?
The minimum energy required to completely remove the most loosely bound electron from a neutral gaseous state.
As you move down a group in the periodic table, atomic radii tend to ______.
As you move down a group in the periodic table, atomic radii tend to ______.
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Which factor primarily causes the decrease in atomic radius across a period?
Which factor primarily causes the decrease in atomic radius across a period?
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Match the following terms with their definitions:
Match the following terms with their definitions:
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Increasing atomic radius leads to an increase in first ionisation energy down a group.
Increasing atomic radius leads to an increase in first ionisation energy down a group.
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The presence of a _______ or half-full p sub-level contributes to higher ionisation values.
The presence of a _______ or half-full p sub-level contributes to higher ionisation values.
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Flashcards
Atomic Radius
Atomic Radius
Half the distance between nuclei of two bonded atoms of the same element.
Atomic Radius Trend Across a Period
Atomic Radius Trend Across a Period
Decreases due to increasing nuclear charge.
Atomic Radius Trend Down a Group
Atomic Radius Trend Down a Group
Increases due to new energy levels and screening effect.
Ionisation Energy
Ionisation Energy
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Ionisation Energy Trend Across a Period
Ionisation Energy Trend Across a Period
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Ionisation Energy Trend Down a Group
Ionisation Energy Trend Down a Group
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2nd Ionisation Energy
2nd Ionisation Energy
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Electronegativity
Electronegativity
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Study Notes
Atomic Radii Trends
- Atomic radius is half the distance between two identical atoms bonded together.
- Atomic radii decrease across a period because of increasing nuclear charge. Nuclear charge is the attraction between electrons and protons.
- Atomic radii increase down a group due to new energy levels and screening effects. Screening is when outer electrons are shielded from the positive protons by full inner electron shells. This effect counteracts increasing positive charge.
- Noble gases (group 8) do not form atomic radii as they are stable and do not form intramolecular bonds.
Ionization Energy Trends
- First ionization energy is the energy needed to remove the most loosely bound electron from a neutral gaseous atom.
- First ionization energy increases across a period because of increasing nuclear charge and decreasing atomic radius.
- First ionization energy decreases down a group due to increasing atomic radius and screening effects.
- Exceptions: Half-filled or fully filled electron subshells (p or d) have extra stability, resulting in slightly higher ionization values.
Electronegativity Trends
- Electronegativity is an atom's ability to attract shared electrons in a covalent bond.
- Electronegativity increases across a period due to increasing nuclear charge and decreasing atomic radius.
- Electronegativity decreases down a group due to increasing atomic radius and screening effects.
Trends within Groups
- Group 1 (Alkali Metals): Highly reactive metals with low first ionization energies. Reactivity increases down the group as atomic radius increases.
- Group 7 (Halogens): Highly reactive nonmetals needing one more electron to be stable. Reactivity decreases down the group as electronegativity decreases.
Additional Notes on Ionization Energy
- Second ionization energy measures the energy to remove an electron from a positively charged ion.
- Ionization energy increases with each electron removed because the positive charge increases, leading to stronger attraction between the nucleus and remaining electrons.:
- Ionization energy shows peaks at the removal of electrons from half-filled or full subshells due to extra stability. Larger jumps correspond to changing energy levels.
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Description
This quiz covers the trends in atomic radii and ionization energy in the periodic table. Understand how nuclear charge and shielding effects influence these properties across periods and down groups. Test your knowledge on these fundamental concepts in chemistry.
