Chemistry Practice questions for ionisation energy, electronegativity, periodic trends, atomic and ionic radii
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Course
Chemistry
Institution
11th Grade
This document contains helpful practice questions with explanations for ionisation energies, electronegativity, atomic and ionic radii, with analysis of graphs and periodic trends.
Explain how you would us the below graph to determine the Explain how atomic radius differs from an ionic radius.
electron configuration of potassium. Superficially, atomic radius is defined as the distance
between an atom's nucleus and its outermost electron
shell, whilst ionic radius is the distance between an
atom's nucleus and its ionized valence shell - either
having lost, or gained electrons to chemical bonding.
Though both phenomenon exhibit periodicity by
decreasing across a period and increasing down a group,
the ionic radius of a cation will be larger, and of a anion -
smaller, than of the atom's neutral state. Such occurs
because the removal of e-'s from an atom will increase the
exertion of electrostatic force on remaining energy levels -
reducing it size, whilst gaining electrons increases ionic
radius, as successive energy levels will be in less
proximity to the nucleus, and so there is less nuclear
attraction to exert and pull on outermost shells.
Describe the electron shielding effect.
The electron shielding affect is the decrease in
electrostatic attraction between a positively charged
nucleus and valence electrons from the screening of inner
The graph depicts potassium as a neutral atom, with the change in electrons. With each successive increase of energy levels,
energy required to ionize its energy shells and successively remove more electrons are necessitated to occupy space, and so
one of its 19 e-. From periodic trends, the lower the principle the subsequent attraction between the valence shell and
quantum number is, the more energetic the level and the greater nucleus decreases, as the electrostatic force between the
electrostatic forces are exerted on the shell, which lessens when 'n' charged particles is hindered by core energy levels; thus,
increases. Thus, where there are substantial decreases in ionization electrons are more loosely held in outer-most shells.
energy, is where a successive energy level is denoted; therefore,
potassium is comprised of 4 energy levels, with one e- observable
when n=4, 8 e- within each core level, and 2 e- observable when
n=1. Adhering to the convention of denoting electron configurations, Determine which element would have a greater ionisation
potassium's is denoted below… energy.
1s2 2s2 2p6 3s2 3p6 4s1. Al or Cl.
Both elements are located in period 3. IE increases across
a period with increasing valency of elements. Thus,
chlorine is expected to be of a higher IE value; this is
List three reasons why chlorine is regarded as a non-metal corroborated by the electron configuration of Cl's valence
shell, where it would be less likely to lose 7e- - deferring
Chlorine is denoted as non-metal, because it exhibits a smaller away from stability and necessitating more energy, than to
atomic radii, and thus high ionization energy and electronegativity more efficiently gain one and satisfy the octet rule.
values. Such occurs, because chlorine's valence shell is comprised N or Sb.
of 7 electrons in the 3rd energy level; thus, there is great Both elements are located in group 15. Ionization energy
electrostatic attraction between the positive charge of the nucleus decreases down a group; thus, Nitrogen is of a lower IE.
and increasing stability of a proximate, outermost shell. Therefore, This is corroborated by the electron configuration of N,
it is less energetically favorable to ionise chlorine's valence shell - where the atom is comprised of two, more proximate
deferring away from stability, than to exhibit a greater affinity to energy levels, contrary to the five energy levels of
gaining an electron to achieve stable configuration of successive Antimony. Therefore, there is greater electrostatic
noble gas. attraction between the positively charged nucleus and
outermost e- - necessitating more energy to ionise
Would you expect a reaction of sodium with water to be more or valence shell, whilst the shielding of nuclear attraction
less vigorous than that of potassium? Explain why. between the charged particles from core e- is greater in
Sb, decreasing its IE.
A reaction of sodium with water would be less vigorous than that Rb or As.
with potassium. Both alkali metals reside in the first group, IE energy decreases down a group and increases across a
although potassium is comprised of an added, 4th energy level, period; thus, Arsenic would be of a greater IE. This is
where its one valence electron resides. With each successive corroborated by the electron configuration of As, where it
quantum number, the electrostatic attraction between positively is comprised of 5 valence e- in the 4th energy level. Thus,
charged protons and outermost electrons of potassium decreases, there is greater electrostatic attraction between the
with excess shielding of attraction from core electrons. Thus, the increasing stability of the outermost shell and proximity to
valence electron is more loosely retained, and so it is more nucleus. Therefore, the element is less likely to ionise
energetically favorable to ionise its outer energy level to achieve valence shell to lose e-, compared to the greater likelihood
stable configuration of previous noble gas. of Rb, where less IE would be necessitated to remove 1e
to achieve stable configuration.
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