(a)
Interpretation:
The reason for the atomic radius of anion to be always larger than that of the atom from which it is derived is to be explained.
Concept Introduction:
Atomic radius is half the distance between two molecules of an atom. Cation is formed by removal of electron/s from an atom and anions are formed by addition of electron/s in an atom. For same atoms, cationic radius is always less than that of the neutral atom and anionic radius is always greater than that of the neutral atom.
(b)
Interpretation:
The reason for the atomic radius of cation to be always smaller than that of the atom from which it is derived is to be explained.
Concept Introduction:
Atomic radius is half the distance between two molecules of an atom. Cation is formed by removal of electron/s from an atom and anions are formed by addition of electron/s in an atom. For same atoms, cationic radius is always less than that of the neutral atom and anionic radius is always greater than that of the neutral atom.
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Chapter 2 Solutions
Introduction to General, Organic and Biochemistry
- 2-59 You are presented with a Lewis dot structure of element X as X.. To which two groups in the Periodic Table might this element belong?arrow_forward2-67 Account for the fact that the first ionization energy of oxygen is less than that of nitrogen.arrow_forward2-89 Assume that a new element has been discovered with atomic number 117. Its chemical properties should be similar to those of astatine (At). Predict whether the new element’s ionization energy will be greater than, the same as, or smaller than that of: (a)At (b)Raarrow_forward
- 2-69 (Chemical Connections 2A) Why does the body need sulfur, calcium, and iron?arrow_forward2-99 A 7.12 g sample of magnesium is heated with 1.80 g of bromine. All the bromine is used up, and 2.07 g of magnesium bromide is produced. What mass of magnesium remains unreacted?arrow_forward2-47 Which element in each pair is more metallic? (a) Silicon or aluminum (b) Arsenic or phosphorus (c) Gallium or germanium (d) Gallium or aluminumarrow_forward
- 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_forwardQ2. This question is about the periodicity of the Period 3 elements. (a) State and explain the general trend in first ionisation energy across Period 3. Give one example of an element which deviates from the general trend in first (b) ionisation energy across Period 3. Explain why this deviation occurs. Page 3 of 12 (c) The table shows successive ionisation energies of an element Y in Period 3. lonisation number 1 2 3 4 5 6 7 8 lonisation energy kJ mol- 1000 2260 3390 4540 6990 8490 27 100 31 700 Identify element Y Explain your answer using data from the table. (d) Identify the Period 3 element that has the highest melting point. Explain your answer by reference to structure and bonding.arrow_forward
- Before Mendeleev published his periodic table, Döbereiner grouped elements with similar properties into “triads,” in whichthe unknown properties of one member could be predicted byaveraging known values of the properties of the others. To test this idea, predict the values of the following quantities:(a) The atomic mass of K from the atomic masses of Na and Rb(b) The melting point of Br₂ from the melting points of Cl₂(-101.0°C) and I₂(113.6°C) (actual value -7.2°C)arrow_forward(b) A new element, "X", is discovered and found to have 2 electrons in its outer level. Is X a metal or non-metal? Predict the formula its ion would have in any ionic compounds it forms.arrow_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) 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?arrow_forward
- Introduction to General, Organic and BiochemistryChemistryISBN:9781285869759Author:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar TorresPublisher:Cengage LearningChemistry & Chemical ReactivityChemistryISBN:9781337399074Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage LearningChemistry & Chemical ReactivityChemistryISBN:9781133949640Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage Learning