18 Questions
Why does the first ionisation energy increase along a period?
As a result of greater electrostatic forces of attraction
What causes the decrease in first ionisation energy down a group?
Increasing shielding
Why does the first ionisation energy of Aluminium differ from the expected value?
Single pair of electrons with opposite spin
What does a sudden large increase in successive ionization energies represent?
Change in energy level
Why is more energy required to remove an electron from an orbital closer to the nucleus?
Greater electrostatic forces of attraction
What does the large energy increase in removing an electron closer to the nucleus provide evidence for?
Atomic orbital theory
Which factor contributes to the instability of an atom with unpaired electrons?
Natural repulsion between unpaired electrons
In the example provided, why does the electron configuration change from 3p⁴ to 3p³ 4s¹?
To improve stability
What is ionisation energy defined as?
The energy needed to remove one mole of electrons from one mole of atoms in a gaseous state
Why do successive ionisation energies generally increase?
As more energy is required to overcome increased attraction between nucleus and outer electrons
Which type of electron arrangement is generally more stable?
Arrangement with a single pair of electrons with opposite spin
What effect does increased electron pairing have on the stability of an atom?
Decreases stability
What happens to an atom when it forms an ion?
It loses or gains electrons and becomes charged
What is the purpose of Time of Flight (TOF) Mass Spectrometry?
To determine the overall relative atomic mass of an element
Which step in Mass Spectrometry involves passing a high voltage over the chamber to ionize atoms?
Ionization
What happens during the Acceleration step in Mass Spectrometry?
Ions are accelerated towards a detection plate
In Mass Spectrometry, what role does the magnetic field play during Ion Drift?
It deflects ions into a curved path
What occurs at the Detection step in Mass Spectrometry?
Positively charged ions gain an electron
Learn about the trends in first ionisation energy along a period and down a group in the periodic table. Understand how atomic radius, electrostatic forces of attraction, and shielding influence ionisation energy. Explore how sudden large increases in successive ionisation energies indicate a change in energy level.
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