atomic structure Flashcards

Question

What is the effect of fragmentation in mass spectrometry?

Answer 1

Molecular ions break into smaller particles

Answer 2

1s² 2s² 2p⁶ 3s² 3p⁶ 4s¹ 3d⁵

Answer 3

1s² 2s² 2p⁶ 3s² 3p⁶ 4s¹ 3d¹⁰

Answer 4

The energy needed to remove 1 electron from each atom of an element in one mole of gaseous atoms

Answer 5

Atomic radius, nuclear charge, electron shielding

Answer 6

Second ionisation energy

Answer 7

The energy needed to remove 1 electron from each atom of an element in one mole of gaseous atoms to form one mole of gaseous ions with a 1+ charge. ## Footnote Ionisation energy is a key concept in understanding how atoms interact with energy and other atoms.

Answer 8

The energy needed to remove 1 electron from each ion of an element in 1 mole of gaseous +1 ions to form 1 mole of gaseous ions with a +2 charge. ## Footnote This concept illustrates the increasing energy required to remove additional electrons from an atom.

Answer 9

The smaller the atomic radius, the higher the first ionisation energy. ## Footnote This is due to the outer electron being more strongly attracted to the nucleus in smaller atoms.

Answer 10

The higher the nuclear charge, the higher the first ionisation energy. ## Footnote A higher nuclear charge results in a smaller atomic radius and a stronger attraction of outer electrons to the nucleus.

Answer 11

The more shielding, the lower the first ionisation energy. ## Footnote Inner shells repel outer electrons, making them easier to lose.

Answer 12

Ionisation energy increases across a period due to higher nuclear charge and smaller atomic radius. ## Footnote Outer electrons are more attracted to the nucleus while shielding remains constant.

Answer 13

Ionisation energy decreases down a group due to larger atomic radius and increased shielding. ## Footnote Outer electrons are less attracted to the nucleus, making them easier to lose.

Answer 14

There is a dip in first ionisation energy due to moving to a new energy level with higher energy. ## Footnote The S to P subshell transition results in electrons being further away from the nucleus and more shielding.

Answer 15

There is a dip in first ionisation energy due to electron repulsion in the p subshell. ## Footnote In group 5, each orbital has one electron; in group 6, one orbital has two electrons, causing repulsion.

Answer 16

Successive ionisation energies refer to the increasing energy required to remove more electrons from an increasingly positive ion. ## Footnote Each electron removed leads to a stronger attraction to the nucleus.

Answer 17

There is a sudden rise in ionisation energy each time a new shell is broken into. ## Footnote For example, sodium shows a significant jump in ionisation energy from the first to the second electron.

Answer 18

Ionisation energy increases because each electron removed is from an increasingly positive ion. ## Footnote For magnesium, the second ionisation energy is greater than the first due to stronger attraction after the first electron is removed.

Answer 19

A sudden jump in ionisation energy indicates that another shell has been entered. ## Footnote The drop in ionisation energy between group 2 and 3 suggests the presence of subshells.