Homework Answers
a)
Both these elements are in same group.
In is below Al in the group.
Ionisation energy decreases as we move down a group in periodic table. This is because atomic size increases and hence nuclear force on outermost electron is less.
This means ionisation energy of Al is more than In
Answer: Al
b)
Both these elements are in same period.
Ge is to the right of K in the period.
Ionisation energy increases as we move from left to right in a period in periodic table. This is because atomic size decreases and hence nuclear force on outermost electron is more.
This means ionisation energy of Ge is more than K
Answer: Ge
c)
Both these elements are in same group.
Se is below S in the group.
Ionisation energy decreases as we move down a group in periodic table. This is because atomic size increases and hence nuclear force on outermost electron is less.
This means ionisation energy of S is more than Se
Answer: S
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7. Choose the element with the higher ionization energy in each pair: Al or In а. b. K or Ge S or Se С.
73. Choose the element with the higher first ionization energy from each pair. a. Br or Bi b. Na or Rb c. As or At...
73. Choose the element with the higher first ionization energy from each pair. a. Br or Bi b. Na or Rb c. As or At d. Por Sn 74. Choose the element with the higher first ionization energy from each pair. POD a. Por I b. Si or C1 c. Por Sb d. Ga or Ge
Highest ionization energy Lowest ionization energy Answer Bank Ca Br Ge Kr Ga K Se As
Highest ionization energy Lowest ionization energy Answer Bank Ca Br Ge Kr Ga K Se As
4) Which element has the highest electronegativity? A) Ge B) O C) B D) Ca 5)...
4) Which element has the highest electronegativity? A) Ge B) O C) B D) Ca 5) Which element has the highest electron affinity? A) Ge В) 0 С) в D) Ca E)K 6) of the 3 elements fluorine, bromine, and calcium, has the highest ionization energy and _has the lowest ionization energy. (Note that we are considering the first ionization energy). A) bromine; calcium B) calcium; fluorine C) fluorine; bromine D) fluorine; calcium E) none of these 7) Based upon...
Predict which element in each of the following pairs has the larger ionization energy K or...
Predict which element in each of the following pairs has the larger ionization energy K or Br S or Te Ga or Se Ne or Sr
Which of the following atoms would have the smallest ionization energy? A. Se B. K C....
Which of the following atoms would have the smallest ionization energy? A. Se B. K C. Br D. As E. Ge What volume of ammonia gas, measured at 617.7 mmHg and 31.1 °C, is required to produce 2.41 g of ammonium sulfate (132.14 g/mol) according to the following balanced chemical equation? 2NH3(g) + H2SO4(aq) → (NH 4)2SO4(s) A. 1.12 L OB. 4.35 L OC. 0.000297 L OD. 0.00119 L OE. 0.280 L
a. Write the following in order of increasing atomic radius: C, Ge, Si b. Write the following in order of increasing atomic radius: Al, B, Mg c. Write the following in order of increasingly negative...
a. Write the following in order of increasing atomic radius: C, Ge, Si b. Write the following in order of increasing atomic radius: Al, B, Mg c. Write the following in order of increasingly negative electron affinity: Ar, Cl, K d. Write the following in order of increasing first ionization energy: C, Ge, Si e. Write the following in order of increasing first ionization energy: Al, Be, Mg
a. Write the following in order of increasing atomic radius: C, Ge,...
Which element is most metallic? a. Sn b. S c. Si d. F Circle the largest atom in each pair. a. C or O b. Rb or Na c...
Which element is most metallic? a. Sn b. S c. Si d. F Circle the largest atom in each pair. a. C or O b. Rb or Na c. C or Al d. For Se
For each pair, choose the Compound with the higher lattice energy. CaO or CaS BaO or SrO (select) (select)
For each pair, choose the Compound with the higher lattice energy. CaO or CaS BaO or SrO (select) (select)
7. Which element has the following electron configurations? lon: [Ar]3d10 lon (-1 charge): [Kr]5s4d105p6 8. Write t...
7. Which element has the following electron configurations? lon: [Ar]3d10 lon (-1 charge): [Kr]5s4d105p6 8. Write the following in order of increasing size As O Br Br Na Rb Te²- F- 02- 9. Arrange these elements in order of decreasing first ionization energy: CI, S, Sn, Pb 10. Choose the element with a more negative (exothermic) electron affinity in each pair: K or Cs Si or P Ga or Br Mg or s 11. a) Which has a higher ionization...
B. Element X has a higher metallic character than element Y. Choose the correct statement: A...
B. Element X has a higher metallic character than element Y. Choose the correct statement: A Element X could be cesium and element Y could be francium. Element X would have a lower first ionization energy than element Y. A d-electron in element X would experience a much higher effective nuclear charge than a d-electron in element Y. D. Element X would have a higher electron affinity than element Y. E. Element X would have a lower electron affinity and...
73. Choose the element with the higher first ionization energy from each pair. a. Br or Bi b. Na or Rb c. As or At d. Por Sn 74. Choose the element with the higher first ionization energy from each pair. POD a. Por I b. Si or C1 c. Por Sb d. Ga or Ge
Highest ionization energy Lowest ionization energy Answer Bank Ca Br Ge Kr Ga K Se As
4) Which element has the highest electronegativity? A) Ge B) O C) B D) Ca 5) Which element has the highest electron affinity? A) Ge В) 0 С) в D) Ca E)K 6) of the 3 elements fluorine, bromine, and calcium, has the highest ionization energy and _has the lowest ionization energy. (Note that we are considering the first ionization energy). A) bromine; calcium B) calcium; fluorine C) fluorine; bromine D) fluorine; calcium E) none of these 7) Based upon...
Which of the following atoms would have the smallest ionization energy? A. Se B. K C. Br D. As E. Ge What volume of ammonia gas, measured at 617.7 mmHg and 31.1 °C, is required to produce 2.41 g of ammonium sulfate (132.14 g/mol) according to the following balanced chemical equation? 2NH3(g) + H2SO4(aq) → (NH 4)2SO4(s) A. 1.12 L OB. 4.35 L OC. 0.000297 L OD. 0.00119 L OE. 0.280 L
a. Write the following in order of increasing atomic radius: C, Ge, Si b. Write the following in order of increasing atomic radius: Al, B, Mg c. Write the following in order of increasingly negative electron affinity: Ar, Cl, K d. Write the following in order of increasing first ionization energy: C, Ge, Si e. Write the following in order of increasing first ionization energy: Al, Be, Mg
a. Write the following in order of increasing atomic radius: C, Ge,...
Which element is most metallic? a. Sn b. S c. Si d. F Circle the largest atom in each pair. a. C or O b. Rb or Na c. C or Al d. For Se
For each pair, choose the Compound with the higher lattice energy. CaO or CaS BaO or SrO (select) (select)
7. Which element has the following electron configurations? lon: [Ar]3d10 lon (-1 charge): [Kr]5s4d105p6 8. Write the following in order of increasing size As O Br Br Na Rb Te²- F- 02- 9. Arrange these elements in order of decreasing first ionization energy: CI, S, Sn, Pb 10. Choose the element with a more negative (exothermic) electron affinity in each pair: K or Cs Si or P Ga or Br Mg or s 11. a) Which has a higher ionization...
B. Element X has a higher metallic character than element Y. Choose the correct statement: A Element X could be cesium and element Y could be francium. Element X would have a lower first ionization energy than element Y. A d-electron in element X would experience a much higher effective nuclear charge than a d-electron in element Y. D. Element X would have a higher electron affinity than element Y. E. Element X would have a lower electron affinity and...
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