S1.3 Electron configurations HL Flashcards

1
Q

Successive ionisation energies

A

The energies required to remove more and more electrons from an ion that is becoming increasing positive.

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2
Q

Describe the general trend in first ionisation energy (IE) across a period.

A

IE generally increases across a period due to the increasing nuclear charge, which pulls electrons closer, making them harder to remove.

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3
Q

How does first ionisation energy (IE) change down a group?

A

IE decreases down a group because electrons are further from the nucleus, in higher energy levels, and shielded by inner electrons, making them easier to remove.

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4
Q

What causes discontinuities in first ionisation energy (IE) trends?

A

Discontinuities are caused by changes in electron configuration, such as moving from s to p orbitals or encountering half-filled vs. fully filled p orbitals, affecting electron removal ease.

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5
Q

How do you calculate the first IE from the wavelength or frequency of the convergence limit?

A

Use E=hf for frequency or E=hc/λ for wavelength, convert energy from J to kJ, and multiply by Avogadro’s number to get IE in kJ/mol.

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6
Q

What does successive ionisation refer to in chemistry?

A

Successive ionisation refers to the process of removing electrons one at a time from an atom, with each step requiring more energy due to the atom’s increasing positive charge.

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7
Q

How can you deduce the group of an element from its successive ionisation energies?

A

By identifying significant jumps in ionisation energy, which indicate the removal of an electron from a more tightly bound shell. A large increase after removing a specific number of electrons suggests the element’s group in the periodic table.

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8
Q

What does a large increase in ionisation energy after removing three electrons suggest about an element?

A

It suggests that the element belongs to Group 13, as it has three valence electrons.

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