Chemistry: Principles and Practice
3rd Edition
ISBN: 9780534420123
Author: Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher: Cengage Learning
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Chapter 20, Problem 20.26QE
Interpretation Introduction
Interpretation:
Reason has to be given for the monomeric and relatively nonreactive nature of Group 8A elements.
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Pick any four non metallic elements from Group 3A - 8A.
Group_A Element:
a) Discuss one benefit or hazard of the element. b) Discuss one commercial application of element
A Element:
Group
a) Discuss one benefit or hazard of the element. b) Discuss one commercial application of element
Group_A Element:
a) Discuss one benefit or hazard of the element. b) Discuss one commercial application of element
Group_A Element:
a) Discuss one benefit or hazard of the element. b) Discuss one commercial application of element
Consider these statements about an element E in Group 4A:
• The most important modern use of E is as an ultrapure semiconductor used to make microelectronic chips.
• E has two main allotropes: a shiny silvery-white metal at room temperature, and a brittle gray powdery form at colder temperatures.
• Although E is not a common element on the Earth's crust, deposits of the mineral EO₂ are widely found, and this ore can be reduced to E with moderate
heating and charcoal.
• Under standard conditions, E is a metal.
Are all of these statements true about the same Group 4A element?
If you said yes, what is E? Enter its chemical symbol:
O
O
0
yes
no
X
S
Using the following thermodynamic data, calculate the lattice enthalpy of lithium
oxide:
Li(g) → Li*(g) + e* AH₁= 540 kJ /mol
Li(s) → Li(g) AHS= +146 kJ/mol
O₂(s) → 20(g) AH₂= +488 kJ /mol
O(g) + 1e →→ O(g) AHA1= -142 kJ /mol
O` (g) + 1e¯ → 0²-(g) AHÃ₂= +844 kJ /mol
2Li(s) + 1/2O₂(g) → Li₂O(s) AH₁= -586 kJ /mol
NOTE: Give your answer in kJ mol-¹
Chapter 20 Solutions
Chemistry: Principles and Practice
Ch. 20 - Prob. 20.1QECh. 20 - Prob. 20.2QECh. 20 - Prob. 20.3QECh. 20 - Prob. 20.4QECh. 20 - Prob. 20.5QECh. 20 - Prob. 20.6QECh. 20 - Prob. 20.7QECh. 20 - Prob. 20.8QECh. 20 - Prob. 20.9QECh. 20 - Prob. 20.10QE
Ch. 20 - Prob. 20.11QECh. 20 - Prob. 20.12QECh. 20 - Prob. 20.13QECh. 20 - Prob. 20.14QECh. 20 - Prob. 20.15QECh. 20 - Prob. 20.16QECh. 20 - Prob. 20.17QECh. 20 - Prob. 20.18QECh. 20 - Prob. 20.19QECh. 20 - Prob. 20.20QECh. 20 - Prob. 20.21QECh. 20 - Prob. 20.23QECh. 20 - Prob. 20.24QECh. 20 - Prob. 20.25QECh. 20 - Prob. 20.26QECh. 20 - Prob. 20.27QECh. 20 - Prob. 20.28QECh. 20 - Prob. 20.30QECh. 20 - Prob. 20.31QECh. 20 - Prob. 20.32QECh. 20 - Prob. 20.33QECh. 20 - Prob. 20.34QECh. 20 - Prob. 20.35QECh. 20 - Prob. 20.36QECh. 20 - Prob. 20.37QECh. 20 - Prob. 20.38QECh. 20 - Prob. 20.39QECh. 20 - Prob. 20.40QECh. 20 - Prob. 20.41QECh. 20 - Prob. 20.42QECh. 20 - Prob. 20.43QECh. 20 - Prob. 20.44QECh. 20 - Prob. 20.46QECh. 20 - Prob. 20.47QECh. 20 - Prob. 20.49QECh. 20 - Prob. 20.50QECh. 20 - Prob. 20.51QECh. 20 - Prob. 20.52QECh. 20 - Prob. 20.53QECh. 20 - Prob. 20.54QECh. 20 - Prob. 20.55QECh. 20 - Prob. 20.56QECh. 20 - Prob. 20.57QECh. 20 - Prob. 20.58QECh. 20 - Prob. 20.59QECh. 20 - Prob. 20.60QECh. 20 - Prob. 20.61QECh. 20 - Prob. 20.62QECh. 20 - Prob. 20.63QECh. 20 - Prob. 20.64QECh. 20 - Prob. 20.65QECh. 20 - Prob. 20.66QECh. 20 - Prob. 20.67QECh. 20 - Prob. 20.68QECh. 20 - Prob. 20.69QECh. 20 - Prob. 20.70QECh. 20 - Prob. 20.71QECh. 20 - Prob. 20.72QECh. 20 - Prob. 20.73QECh. 20 - Prob. 20.74QECh. 20 - Prob. 20.75QECh. 20 - Prob. 20.76QECh. 20 - Prob. 20.77QECh. 20 - Prob. 20.78QECh. 20 - Prob. 20.79QECh. 20 - Prob. 20.80QECh. 20 - Prob. 20.82QECh. 20 - Prob. 20.83QECh. 20 - Prob. 20.84QE
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- Explain the theoretical aspect of the separation of Group IIA cations from Group IIB.arrow_forwardUse Born-Mayer equation to calculate the lattice energy for PbS (it crystallizes in theNaCl structure). Then, use the Born–Haber cycle to obtain the value of lattice energy for PbS.You will need the following data following data : ΔH Pb(g) = 196 kJ/mol; ΔHf PbS = –98kJ/mol; electron affinities for S(g)→S- (g) is -201 kJ/mol; ) S- (g) →S2-(g) is 640kJ/mol. Ionizationenergies for Pb are listed in Resource section 2, p.903. Remember that enthalpies of formationare calculated beginning with the elements in their standard states (S8 for sulfur). Diatomicsulfur, S2, is formed from S8 (ΔHf: S2 (g) = 535 kJ/mol. Can you just do the Born-Haber part?arrow_forwardUntil the early 1960s the group 8A elements were called the inert gases; before that they were called the rare gases. The term rare gases was dropped after it was discovered that argon accounts for roughly 1% of Earth’s atmosphere. (a) Why was the term inert gases dropped? (b) What discovery triggered this change in name? (c)What name is applied to the group now?arrow_forward
- The oxygen and nitrogen families have some obvious sim-ilarities and differences.(a) State two general physical similarities between Group5A(15) and 6A(16) elements. (b) State two general chemical similarities between Group5A(15) and 6A(16) elements.(c) State two chemical similarities between P and S.(d) State two physical similarities between N and O.(e) State two chemical differences between N and O.arrow_forwardGive a description of the kinds of ions that are expected to form by group : 1A, 2A, 6A, 7A elements.arrow_forwardElement Y reacts with oxygen to form the compound Y2O and has the lowest ionization energy of any Period 4 element on the periodic table. Identify this element.arrow_forward
- What correlation, if any, exists for the Period 2 elements between group number and the number of covalent bonds the element typically forms? How is the correlation different for elements in Periods 3 to 6?arrow_forwardWhy is Group I elements known as the most electropositive element?arrow_forwardWhich element does NOT exhibit paramagnetism?arrow_forward
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