Chemistry: Principles and Reactions
8th Edition
ISBN: 9781305079373
Author: William L. Masterton, Cecile N. Hurley
Publisher: Cengage Learning
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Textbook Question
Chapter 6, Problem 56QAP
Which of the four atoms Na, P, Cl, or K
(a) has the largest atomic radius?
(b) has the highest ionization energy?
(c) is the most electronegative?
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Students have asked these similar questions
Boron, 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) Drawthe orbital diagram for an atom of 11B. Which electrons are the valence electrons? (c) Indicate three ways in which the 1s electrons inboron differ from its 2s electrons. (d) Elemental boron reacts with fluorine to form BF3, a gas. Write a balanced chemical equation forthe reaction of solid boron with fluorine gas. (e) ΔHf° for BF31g2 is -1135.6 kJ>mol. Calculate the standard enthalpy change in thereaction 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?
Arrange the following chemical species in order of increasing atomic radius. Explain your arrangement in each case.
(a) K, Mg, Ca, Al
(b) F–, S2–, Cl–.
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 mass
Chapter 6 Solutions
Chemistry: Principles and Reactions
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Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.Similar questions
- Boron, 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_forwardArrange the following chemical species in order of increasing atomic radius. Explainyour arrangement in each case.(a) K, Mg, Ca, Aℓ(b) F–, S2–, Cℓ–.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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