StudyXY
RegisterLog in
Back to AI Flashcard MakerChemistry /A-level Chemistry: 3.1.1 Atomic Structure Part 3

A-level Chemistry: 3.1.1 Atomic Structure Part 3

Chemistry24 CardsCreated 2 months ago

This flashcard set explains the concept of ionisation as an endothermic process and covers the key rules and factors that influence ionisation energy. It includes the correct way to write ionisation equations, and discusses how nuclear charge, shielding, and distance from the nucleus affect the ease of removing an electron.

PrintEmbedImportReport

Ionisation is a process ∵ you have to put energy in to ionise atom/molecule

endothermic

Tap or swipe ↕ to flip
Swipe ←→Navigate
1/24

Key Terms

Term
Definition

Ionisation is a process ∵ you have to put energy in to ionise atom/molecule

endothermic

Name 3 rules about ionisation energies

  1. Must use gas state symbol (g) ∵ ionisation energies are measured for gaseous atoms

  2. Always refer to 1 mole of atoms

    3. <...

Name 3 factors that affect ionisation energy

  1. Nuclear Charge

  2. Shielding

  3. Distance from Nucleus

Describe how nuclear charge affects ionisation energy

More protons in nucleus = more positively charged nucleus is & stronger the attraction for electrons

Relative mass for an electron

1/1840

Describe how distance from nucleus affects ionisation energy

Attraction decreases rapidly with distance

(i.e. electron close to nucleus = much more strongly attracted than one further away)

Log in to view all terms

Related Flashcard Decks

Chemistry

CSEC Chemistry: States of Matter and Particulate Theory

This deck covers the fundamental concepts of states of matter and the particulate theory, including diffusion, osmosis, and the characteristics of solids, liquids, and gases.

10 cards
View Deck
Chemistry

Understanding Redox Reactions

This deck covers the fundamental concepts of redox reactions, including definitions of oxidation and reduction, electron transfer, oxidation states, and how to write ionic and half equations.

10 cards
View Deck
Chemistry

Cambridge IGCSE Chemistry Essentials

This deck covers key concepts from the Cambridge IGCSE Chemistry Coursebook, including states of matter, atomic structure, bonding, reactions, organic chemistry, and environmental chemistry.

50 cards
View Deck
Chemistry

Edexcel A Level Chemistry: Exam Questions

This flashcard set provides explanations for molecular shapes and trends in chemical behavior. It covers the geometry of phosphorus (III) chloride due to electron pair repulsion, the thermal stability of nitrates based on cation size and charge, and the increase in boiling points from chlorine to iodine due to stronger London dispersion forces.

8 cards
View Deck
Chemistry

Edexcel A Level Chemistry: 19: Modern Analytical Techniques II

This flashcard set explains the fundamental principles of mass spectrometry, including the formation of molecular ions, the meaning of m/z (mass-to-charge) values, and how high-resolution mass spectrometry provides precise molecular mass measurements.

46 cards
View Deck
Chemistry

Edexcel A Level Chemistry: 18: Organic Chemistry III

This flashcard set introduces aromatic and aliphatic compounds, highlighting the presence or absence of delocalised electrons in hydrocarbon rings. It also describes benzene as an arene and outlines its key physical properties.

89 cards
View Deck

Study Tips

  • Press F to enter focus mode for distraction-free studying
  • Review cards regularly to improve retention
  • Try to recall the answer before flipping the card
  • Share this deck with friends to study together
A-level Chemistry: 3.1.1 Atomic Structure Part 3
TermDefinition

Ionisation is a process ∵ you have to put energy in to ionise atom/molecule

endothermic

Name 3 rules about ionisation energies

  1. Must use gas state symbol (g) ∵ ionisation energies are measured for gaseous atoms

  2. Always refer to 1 mole of atoms

  3. Lower ionisation energy = easier it is to remove from ion

Name 3 factors that affect ionisation energy

  1. Nuclear Charge

  2. Shielding

  3. Distance from Nucleus

Describe how nuclear charge affects ionisation energy

More protons in nucleus = more positively charged nucleus is & stronger the attraction for electrons

Relative mass for an electron

1/1840

Describe how distance from nucleus affects ionisation energy

Attraction decreases rapidly with distance

(i.e. electron close to nucleus = much more strongly attracted than one further away)

What is meant by high ionisation energy?

High ionisation energy = high attraction between electrons & nucleus = more energy needed to remove electron

What provides evidence for shells structure of atoms?

Graph of successive ionisation energies

Within each shell, successive ionisation energies ______

increase

Why does successive ionisation energies increase within each shell?

∵ electrons are being removed from an increasingly positive ion = less repulsion amongst remaining electrons ∴ they're held more strongly by nucleus

When does big jumps in ionisation energy happen?

When a new shell is broken into = an electron is being removed from shell closer to nucleus

Define second ionisation energy

Enthalpy change when 1 mole of gaseous 2+ ions is formed from 1 mole of gaseous 1+ ions

Describe how you can use a successive ionisation energies graph to figure out which group an element belongs to

Count how many electrons are removed before the 1st big jump to find the group number

Describe how you can use a successive ionisation energies graph to predict the electronic structure of elements

Working from right to left, count no. of points there are before each big jump to find how many electrons there are in each shell, starting with the first

Name 2 trends in first ionisation energy

  • 1st ionisation energies of elements down a group of periodic table decrease

  • 1st ionisation energies of elements across a period generally increase

Explain why ionisation energy decreases down Group 2

  1. Atomic radius increases/electron removed further from nucleus

  2. As group is descended more shielding = nucleus' attraction reduces

Both of these factors = make it easier to remove outer electrons = lower ionisation energy

Explain why ionisation energy increases across a Period (2x)

  1. Increased nuclear charge (no. of protons is increases = stronger nuclear attraction)

  2. Extra electrons enter roughly same energy level or similar shielding

Drops between Groups and _ show _____ Structure

Drops between Groups 2 and 3 show Sub-Shell Structure

Describe and explain how aluminium provides evidence for the theory of electron sub-shells

  1. Aluminium's outer electron = in 3p orbital rather than 3s

    • ∵ 3p orbital = slightly higher energy than 3s orbital

      • ∴ electron is found further from nucleus

  2. Additonal electron shielding - 3p orbital has additional shielding provided by 3s2 electrons

  3. Both these factors strong enough to override effect of increased nuclear charge = ionisation energy drops slightly, easier to remove electron

Drops between Groups and Is due to Electron ______

Drops between Groups 5 and 6 Is due to Electron Repulsion

Describe and explain how phosphorus & sulfur provides more evidence for the eletronic structure model

  1. (Shielding identical in phosphorus & sulfur atoms + electron is being removed from an identical orbital)

  2. In phosphorus's case: electron being removed from singly-occupied orbital

  3. But in sulfur: electron removed from paired electrons in 3p orbital

  4. Electron repulsion between 2 electrons = electron easier to remove from pair

Explain why the value of the first ionisation energy of neon is higher than that of sodium (2x)

  • Electron removed from a level of lower energy or e– removed from 2p rather than from 3s

  • Less shielding

Which of Na+ and Mg2+ is the smaller ion? Explain why (2)

Mg2+

Has more protons with same sheilding

Magnesium exists as three isotopes: 24Mg, 25Mg & 26Mg

24Mg percentage = 80%

26Mg percentage = 10%