On the basis of electron configuration explain why: a) Sulphur has a lower electron affinity than chlorine. (2) b) Phosphorous has a higher ionization energy than sulphur.
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1. On the basis of electron configuration
explain why:
a) Sulphur has a lower
chlorine. (2)
b) Phosphorous has a higher ionization
energy than sulphur.
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- Give the group number and the general valence electron configuration of an element with the following electron-dot symbol. (For example, type ns2 np6 for ns²np°, which is the valence configuration of all group 8A elements.) (a) group number electron configuration (b) group number electron configurationExplain why boron (B) has a higher ionization energy than fluorine (F).Among the elements B, Al, C and Si(a) Which has the highest first ionization enthalpy?(b) Which has the largest atomic radius?
- 5. Which of the following alkali metal halides has the larger lattice energy, and which has the smaller lattice energy? Explain. (a) (b)Given the following elements: Si, Sr, Cu, Ti, S (a) which of those elements would have the larget atomic radius? (b) which of those elements would have the highest ionization energy? (c) which of those elements would have the lowest electronegativity?The oxygen and nitrogen families have some obvious similarities and differences.(a) State two general physical similarities between Group 5A(15) and 6A(16) elements.(b) State two general chemical similarities between Group 5A(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.
- Why fluorin has low electron affinity as compared to chlorine?Until 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?Explain why Be and Mg form metallic hydrides instead of ionic hydrides like the other elements in Groups 1 and 2?
- Assuming normal filling rules write the full name and abbreviated electron configurations as well as the Lewis structure for; (a) silicon (b) fluorine (c) selenium (d) xenonThe 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.(a) List four physical characteristics of a solid metal. (b) List two chemical characteristics of a metallic element.