Concept explainers
(a)
Interpretation:
The element that has a high
Concept Introduction:
The amount of energy required to add an electron to the atom to form negative ion is known as electron affinity. The factors affecting electron affinity are shown below:
- It is inversely proportional to the size of an atom.
- It is directly proportional to the effective nuclear charge.
- It is inversely proportional to the stable electronic configuration.
(b)
Interpretation:
The element that has a high electron affinity from I and Rn should be predicted.
Concept Introduction:
The amount of energy required to add an electron to the atom to form negative ion is known as electron affinity. The factors affecting electron affinity are shown below:
- It is inversely proportional to the size of an atom.
- It is directly proportional to the effective nuclear charge.
- It is inversely proportional to the stable electronic configuration.
(c)
Interpretation:
The element that has a high electron affinity from Ba and Te should be predicted.
Concept Introduction:
The amount of energy required to add an electron to the atom to form negative ion is known as electron affinity. The factors affecting electron affinity are shown below:
- It is inversely proportional to the size of an atom.
- It is directly proportional to the effective nuclear charge.
- It is inversely proportional to the stable electronic configuration.
(d)
Interpretation:
The element that has a high electron affinity from Bi and Cl should be predicted.
Concept Introduction:
The amount of energy required to add an electron to the atom to form negative ion is known as electron affinity. The factors affecting electron affinity are shown below:
- It is inversely proportional to the size of an atom.
- It is directly proportional to the effective nuclear charge.
- It is inversely proportional to the stable electronic configuration.
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Principles of Modern Chemistry
- Q1. This question is about atomic structure. (a) Write the full electron configuration for each of the following species. CH Fe2+ (b) Write an equation, including state symbols, to represent the process that occurs when the third ionisation energy of manganese is measured. (c) State which of the elements magnesium and aluminium has the lower first ionisation energy Explain your answer. (d) A sample of nickel was analysed in a time of flight (TOF) mass spectrometer. The sample was ionised by electron impact ionisation. The spectrum produced showed three peaks with abundances as set out in the table. m/z Abundance /% 58 61.0 60 29.1 61 9.9 Give the symbol, including mass number, of the ion that would reach the detector first in the sample. Calculate the relative atomic mass of the nickel in the sample. Give your answer to one decimal place. Page 2 of 12 Symbol of ion Relative atomic massarrow_forwardBoron, atomic number 5, occurs naturally as two isotopes, 10B and 11B, with natural abundances of 19.9% and 80.1%, respectively. (a) In what ways do the two isotopes differ from each other? Does the electronic configuration of 10B differ from that of 11B? (b) Draw the orbital diagram for an atom of 11B. Which electrons are the valence electrons? (c) Indicate three ways in which the 1s electrons in boron differ from its 2s electrons. (d) Elemental boron reacts with fluorine to form BF3, a gas. Write a balanced chemical equation for the reaction of solid boron with fluorine gas. (e) ΔHf° for BF3(g) is -1135.6 kj/mol. Calculate the standard enthalpy change in the reaction of boron with fluorine. (f) Will the mass percentage of F be the same in 10BF3 and 11BF3? If not, why is that the case?arrow_forward5. The atoms and ions Ne, N³-, F, Mg2+, and Si4+ are part of an isoelectronic series. (a) Which of these will have the smallest effective nuclear charge acting on the outermost electron? (b) Which one possess the greatest effective nuclear charge? (c) Which ion will be the largest in size? Explain why.arrow_forward
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