(a)
Interpretation:
The elements that are
Concept Introduction:
Diamagnetic: When atoms or ions with all electrons are paired their magnetic field effectively cancels each other. Substances with paired electrons are called diamagnetic. They are weakly repelled by magnetic fields.
Paramagnetic: Atoms or ions with unpaired electrons are attracted to magnetic field. Substances with unpaired electrons are called paramagnetic.
(b)
Interpretation:
The elements with
Concept Introduction:
Refer to part (a)
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Chapter 5 Solutions
OWLv2 for Moore/Stanitski's Chemistry: The Molecular Science, 5th Edition, [Instant Access], 1 term (6 months)
- What is the electron configuration of the Ba3+ ion? Suggest a reason why this ion is not normally found in nature.arrow_forwardConsider the Mg2+, Cl-, K+, and Se2- ions. The four spheresbelow represent these four ions, scaled according to ionic size.(a) Without referring to Figure 7.8, match each ion to its appropriatesphere. (b) In terms of size, between which of the sphereswould you find the (i) Ca2+ and (ii) S2- ions?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
- Write the electron configuration and orbital diagram for each ion and predict whether each will be paramagnetic or diamagnetic.(a) Co2+ (b) N3- (c) Ca2+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) 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_forwardWrite the formula and name of the compound formed fromthe following ionic interactions: (a) The 2 ion and the 1 ion are both isoelectronic with the atoms of a chemically unreactive Period 4 element. (b) The 2 ion and the 2 ion are both iso-electronic with the Period 3 noble gas. (c) The 2ion is thesmallest with a filled d subshell; the anion forms from the small-est halogen. (d) The ions form from the largest and smallest ion-izable atoms in Period 2.arrow_forward
- Consider the Mg2+, Cl-, K+, and Se2- ions. The four spheresbelow represent these four ions, scaled according to ionic size.(a) Without referring to Figure 7.8, match each ion to its appropriatesphere. (b) In terms of size, between which of the sphereswould you find the (i) Ca2 + and (ii) S2 - ions? [Section 7.3]arrow_forward11)Explain the given ionization energy for each pair using electron configurations. (12(Be)l1(B), I1(N)>l1(O) ).arrow_forward7. Which element has the smallest first ionization energy? (a) Cs (b) Ga (c) K (d) Bi (e) As 8. Which element has the smallest second ionization energy? (a) Mg (b) Li (c) S (d) O (e) Ca 9. Which of the following sets contain all linear molecules? (a) H2S, HCN, CO2. (b) HCN, O2, CO2 (c) H2O, CO, Cl2. (d) H2S, CO, CO2. (e) BF3, Cl2, O2 10. The molecular geometry of SnCl3-ion is: (a) trigonal planar (b) T-shaped. (c) trigonal pyramidal. (d) Tetrahedral (e) see-saw 11. The geometry of the molecule SPC13 is best described as: (a) square planar (b) trigonal pyramidal (c) trigonal bipyramidal. (d) octahedral (e) tetrahedral 12. The O-S-Cl bond angles in O2SCl2 are expected to be approximately: (a) 90° (b) 109.5° (c) 120° (d)180 ° (e) 90° and 120°arrow_forward
- Nitrogen (N), phosphorus (P), and arsenic (As) are three elements that almost universally form ions with –3 charge when they form compounds with metals. First, (i) write the full and core electron configurations for N, P, and As. Then, using those configurations, (ii) explain why those three elements all form ions with the same charge.arrow_forward10. Which of the following element has paramagnetic property? (a) Mg (b) P (c) Ne (d) Hg 11. Which of the following element is a main group (representative group) element? (a) Zn (b) S (c) Cu (d) Co 12. The energy required to remove an electron from an atom in its ground state is called (a) atomic number (b) electronegativity (c) electron affinity (d) ionization energyarrow_forwardWhat is meant by the term nuclear charge? How does the effective nuclear charge experienced by the valence electrons of an atom vary going from left to right across a period of the periodic table? 3. If each core electron was totally effective in shielding the valence electrons from the full charge of the nucleus and the valence electrons provided no shielding effect for each other, what would be the effective nuclear charge acting on a valence electron in (a.) K (B.) Br 4. what is the general relationship between the size of an atom and its first ionization energy? 5. which element in the periodic table has the largest ionization energy? Which has the smallest?arrow_forward
- Chemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage LearningChemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage Learning
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