Atomic Radii and Ionization Energy Trends
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Questions and Answers

What is the primary reason for the large decrease in first ionisation energy between elements R and S?

  • R has a smaller atomic number than S.
  • R has a full outer lower sub-level. (correct)
  • S has a completely filled outer shell.
  • S has a higher electron affinity than R.

Which statement correctly explains why element H has a lower first ionisation energy compared to element G?

  • H's electron configuration is more stable than that of G.
  • H is a noble gas while G is a transition metal.
  • H has fewer electrons than G.
  • G has a half-filled 2p sub-level which is more stable. (correct)

Which of the following explains the trend of increasing electronegativity across a period in the periodic table?

  • Increasing effective nuclear charge. (correct)
  • Increasing atomic radius.
  • Decreasing effective nuclear charge.
  • Decreasing electron shielding effect.

Which of the following compounds does not contain intermolecular hydrogen bonds?

<p>Hydrogen chloride, HCl (B)</p> Signup and view all the answers

What is the main reason why the boiling point of ammonia is significantly lower than that of water?

<p>Water has stronger hydrogen bonding than ammonia. (D)</p> Signup and view all the answers

What happens to the ionisation energy as you move from left to right across a period?

<p>It increases (A)</p> Signup and view all the answers

Which of the following pairs illustrates an exception to the general trend of ionisation energy in the second period?

<p>Beryllium and Boron (B)</p> Signup and view all the answers

Why is the ionisation energy of Boron less than that of Beryllium?

<p>Boron has a half-filled outer shell (C)</p> Signup and view all the answers

What is the Second Ionisation Energy?

<p>Energy needed to remove an electron from a positively charged ion in gaseous state (A)</p> Signup and view all the answers

What would be expected when removing the first electron from potassium considering its electron configuration?

<p>It requires minimal energy due to the stability of 4s (D)</p> Signup and view all the answers

Why does the second ionisation energy increase significantly after the first electron is removed from potassium?

<p>The remaining electrons experience less shielding (A)</p> Signup and view all the answers

What general trend does the ionisation energy exhibit when an electron is removed from filled subshells?

<p>It increases due to added stability (D)</p> Signup and view all the answers

Which of the following elements would generally have the highest ionisation energy?

<p>Nitrogen (A)</p> Signup and view all the answers

What primarily causes the decrease in electronegativity as you move down a group in the Periodic Table?

<p>Increasing atomic radius (D)</p> Signup and view all the answers

Which trend describes why electronegativity increases across a period?

<p>Decreasing atomic radius (B)</p> Signup and view all the answers

Which group of elements is known for having very low first ionization energy values?

<p>Alkali metals (C)</p> Signup and view all the answers

What is the general reaction of alkali metals with water?

<p>They produce metal hydroxides and hydrogen gas. (D)</p> Signup and view all the answers

As you go down the alkali metal group, which property increases with reactivity?

<p>Screening effect (B)</p> Signup and view all the answers

What product is formed when potassium reacts with oxygen?

<p>Potassium Oxide (C)</p> Signup and view all the answers

What effect does decreasing atomic radius have across a period regarding electronegativity?

<p>It increases electronegativity. (B)</p> Signup and view all the answers

Why do alkali metals not occur free in nature?

<p>They are too reactive and easily form compounds. (C)</p> Signup and view all the answers

What is the primary reason Alkali Metals are stored under oil?

<p>To prevent reaction with oxygen in the air (B)</p> Signup and view all the answers

Which statement accurately describes the trend in reactivity of Alkali Metals?

<p>Reactivity increases as you move down the group (D)</p> Signup and view all the answers

What trend is observed for the electronegativity of Halogens as you move down the group?

<p>Electronegativity decreases (C)</p> Signup and view all the answers

Which Halogen is known to be the most electronegative?

<p>Fluorine (D)</p> Signup and view all the answers

What does the first ionisation energy value of an element represent?

<p>Energy needed to remove the most loosely-bound electron (B)</p> Signup and view all the answers

Why is the first ionisation energy of silicon greater than that of aluminum?

<p>Silicon has a greater nuclear charge (B)</p> Signup and view all the answers

What experimental evidence supports the existence of energy levels in atoms?

<p>Line emission spectrum (A)</p> Signup and view all the answers

What happens to the first ionisation energy as you move from carbon to silicon?

<p>It decreases (D)</p> Signup and view all the answers

What happens to the atomic radius as you move down a group in the Periodic Table?

<p>It increases due to additional energy levels. (D)</p> Signup and view all the answers

Which factor primarily causes the decrease in atomic radius across a period?

<p>Increased effective nuclear charge. (B)</p> Signup and view all the answers

How do atomic radii and ionisation energy trends correlate across a period?

<p>Atomic radii decrease while ionisation energy increases. (D)</p> Signup and view all the answers

Which statement best describes the ionisation energy trend down a group?

<p>It decreases due to increased atomic radius and shielding. (A)</p> Signup and view all the answers

What is the main reason for the increase in the first ionisation energy across a period?

<p>Increase in effective nuclear charge. (A)</p> Signup and view all the answers

What role do inner electrons play in determining the ionisation energy?

<p>They contribute to the screening effect, making outer electrons easier to remove. (B)</p> Signup and view all the answers

What describes the atomic radius and ionisation energy trends as you move from left to right across a period?

<p>Atomic radius decreases while ionisation energy increases. (A)</p> Signup and view all the answers

Which of the following would result in a lower first ionisation energy?

<p>A larger atomic radius. (C), Increased electron shielding. (D)</p> Signup and view all the answers

Flashcards

Atomic Radius Trend

Atomic radius increases down a group and decreases across a period in the periodic table.

Atomic Radius Definition

Half the distance between the nuclei of two identical atoms bonded together.

Ionization Energy Trend (Down a Group)

Ionization energy decreases down a group because electrons are further from the nucleus, and the shielding effect increases.

Ionization Energy Trend (Across a Period)

Ionization energy increases across a period because nuclear charge increases, pulling the electrons closer.

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Ionization Energy Definition

Minimum energy to remove most loosely bound electron from a neutral gaseous atom.

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Screening Effect

Inner electrons shield outer electrons from the full positive pull of the nucleus.

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Effective Nuclear Charge

The positive charge felt by an electron due to the nucleus, reduced by the shielding effect of other electrons.

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Atomic Radius

Half the distance between the nuclei of bonded atoms.

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Atomic Radius & Ionization Energy

Atomic radius decreasing across a period leads to stronger attraction between nucleus and electrons, increasing ionization energy.

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Ionization Energy Exceptions (Period 2)

Elements with half-filled or completely filled outer electron shells (sublevels) have extra stability, requiring more energy to remove an electron than expected.

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Second Ionization Energy

Energy needed to remove a second electron from a positively charged ion.

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Electron Shielding

Inner electrons shield outer electrons from the full attractive force of the nucleus, making outer electrons easier to remove.

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Energy Levels and Ionization Energy

Higher energy levels are further away from the nucleus and hence have lower ionization energies. Ionization energy increases across a period because of increasing nuclear charge, decreased shielding, and smaller radii.

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Sublevel Stability

Half-filled or completely filled electron sublevels are more stable than partially filled sublevels, requiring more energy to remove an electron.

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Potassium's First Ionization Energy

Removing the 4s electron from Potassium is relatively easy, as it's a lone electron in the outermost level.

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Electron Configuration and Ionization Energy

The arrangement of electrons in different sublevels within atoms determines the stability and ionization energy values.

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Electronegativity Trend (Groups)

Electronegativity decreases down a group in the periodic table.

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Electronegativity Trend (Periods)

Electronegativity increases across a period in the periodic table.

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Alkali Metals Reactivity

Alkali metals are very reactive due to low ionization energy.

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Alkali Metal Reactivity Trend

Reactivity increases down the alkali metal group.

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Alkali Metal Reaction with Oxygen

Alkali metals react with oxygen to form oxides.

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Alkali Metal Reaction with Water

Alkali metals react with water to form hydroxides and release hydrogen gas.

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Alkali Metal Storage

Alkali metals are stored under oil to prevent them from reacting with oxygen in the air.

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First Ionization Energy

The minimum energy required to remove the most loosely bound electron from an isolated gaseous atom in its ground state.

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Why Does Silicon Have a Higher Ionization Energy than Aluminum?

Silicon has a higher ionization energy than aluminum because silicon has a greater nuclear charge and a smaller atomic radius, making it harder to remove an electron.

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Why Does Silicon Have a Lower Ionization Energy than Carbon?

Silicon has a lower ionization energy than carbon because silicon has a larger atomic radius, making it easier to remove an electron.

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Halogen Reactivity Trend

Halogens become less reactive as you move down the periodic table.

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Halogen Properties

Halogens are very electronegative, meaning they have a strong attraction for electrons and are highly reactive. They don't exist freely in nature and must be extracted from compounds.

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Evidence for Energy Levels from Ionization Energies

Sharp increases in ionization energy indicate the removal of an electron from a new shell. Gradual increases occur within the same shell.

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Electronegativity

The relative ability of an atom in a covalent bond to attract the shared pair of electrons towards itself.

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Factors affecting electronegativity across a period

Electronegativity increases across a period due to increasing effective nuclear charge and decreasing atomic radius.

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Hydrogen bonding

A special type of intermolecular force that occurs between molecules containing a hydrogen atom bonded to a highly electronegative atom like oxygen or nitrogen.

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Why ammonia has lower boiling point than water

Ammonia has weaker and less effective hydrogen bonding compared to water, leading to a lower boiling point.

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Half-filled and completely filled electron sublevels

Electron sublevels that are half-filled or completely filled are particularly stable, making it harder to remove an electron from these elements.

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Study Notes

  • Atomic radius is half the distance between two nuclei of the same atom bonded together.
  • Atomic radius increases down a group due to increasing energy levels that are further from the nucleus, and the shielding effect of the inner electrons reducing the pull on outer electrons.
  • Atomic radius decreases across a period due to an increase in effective nuclear charge. The nucleus pulls outer electrons closer, making atoms smaller.
  • First ionization energy is the minimum energy required to remove the most loosely bound electron from a neutral gaseous atom.
  • Ionization energy decreases down a group because increasing atomic radius means the outermost electrons are further from the attractive force of the nucleus.
  • Ionization energy increases across a period due to increased effective nuclear charge pulling the outermost electron more strongly, and decreasing atomic radius.
  • Atoms with half filled or filled outer electron shells require more energy to remove an electron, making them more stable.

Exceptions

  • There are exceptions to these general trends, particularly in the second period where subtle differences in electron configurations lead to variations in ionization energy. For example, there's a dip in ionization energy between Beryllium and Boron.

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Related Documents

Trends in the Periodic Table PDF

Description

Explore the key concepts of atomic radii and ionization energy trends with this quiz. Understand how these properties change across periods and down groups in the periodic table while examining the underlying principles like effective nuclear charge and energy levels. Test your knowledge on the factors influencing these important atomic characteristics.

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