12. What are the exceptions to the periodic trends in ionization energy? a) Exceptions occur with elements Li, Na, and K in group 1A and Be, Mg, and Ca in group 2A. b) Exceptions occur with elements Be, Mg, and Ca in group 2A and B, Al, and Ga in group 3A. c) Exceptions occur with elements B, Al, and Ga in group 3A and C, Si, and Ge in group 4A. d) Exceptions occur with elements C, Si, and Ge in group 4A and N, P, and As in group 5A. e) Exception occurs with elements N, P, and As in group 5A and O, S, and Se in group 6A f) Exception occurs with elements O, S, and Se in group 6A and F, Cl, and Br in group 7A g) Exception occurs with elements F, Cl, and Br in group 7A and Ne, Ar, and Kr in group 8A

12. What are the exceptions to the periodic trends in ionization energy? a) Exceptions occur with elements Li, Na, and K in group 1A and Be, Mg, and Ca in group 2A. b) Exceptions occur with elements Be, Mg, and Ca in group 2A and B, Al, and Ga in group 3A. c) Exceptions occur with elements B, Al, and Ga in group 3A and C, Si, and Ge in group 4A. d) Exceptions occur with elements C, Si, and Ge in group 4A and N, P, and As in group 5A. e) Exception occurs with elements N, P, and As in group 5A and O, S, and Se in group 6A f) Exception occurs with elements O, S, and Se in group 6A and F, Cl, and Br in group 7A g) Exception occurs with elements F, Cl, and Br in group 7A and Ne, Ar, and Kr in group 8A

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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In general, the ionization energy increases as you move from left to right in the periodic table, as can be seen in the figure below. 2500 He Noble gases Ne 2000 Ar * 1500 Kr Period 4 transition elements Period 5 Хе transition elements 1000 500 Li Na K Rb Alkali metals 0+ 10 20 30 40 50 Atomic number However, the ionization energy of boron lower than that of beryllium, and the ionization energy of aluminum is lower than that f magnesium.
Which of the following statements are TRUE? a) The third ionization energy (IE3) of magnesium is less than the second ionization energy (IE2) of magnesium. b) An atom of beryllium will have a longer atomic radius than an atom of magnesium. Oc) An atom of fluorine will have a greater ionization energy than an atom of nitrogen. O d) An atom of calcium will have a greater ionization energy than an atom of potassium.
(a) Give each element's full name. A: B: C: D: (b) Put these four elements in order from smallest size to largest size: Smallest... ...Largest A B C D A B C D A B C D A B C D (c) Put these four elements in order from smallest ionization energy to largest ionization energy: Smallest... ...Largest A B C D A B C D A B C D A B C D
a This question uses He to explore the ability of one electron to shield another from the positive charge of the nucleus. The ionization of an atom not experiencing shielding can be calculated from Bohr's equation for the electron energy. E = - (N₁Rhc) (Z²/n² where N₁ Rhc = 1312 kJ/mol and Z is the atomic number. Use this approach to calculate a possible ionization energy for helium assuming the electrons of the He experience the full 2+ nuclear charge. This gives us the upper limit for the ionization energy. Ionization energy = kJ/mol
A space probe identifies a new element in a sample collected from an asteroid. Successive ionization energies, in attojoules per atom, for the new element are given in the table. I4 Is 5.074 8.294 0.507 1.017 4.108 6.147 7.903 To what family of the periodic table does this new element probably belong? 16 (6A) 2 (2A) 18 (8A) 17 (7A) O 1 (IA) О 13 (ЗА) 14 (4A) 15 (5A)
30. How do ionization energies change (a) down a group of elements in the periodic table? (b) from left to right across a period of elements?
The continuation of this problem is Ar: n=1 n=2 n=3 n=4 Same thing with Ca And lastly, “What is The neutral atom that has its first two energy levels filled, has one electron in its third energy level, and has no other electrons? Enter the name of the element, not the abbreviation”
When looking at the list of electron configurations of elements up to Z = 103. Some do not follow the Aufbau principle. What do these elements have in common? A) They are all transition metals. B) They all have at least one half-filled shell. C) They all end in d5 or d10. D)They do not have anything in common
Sort each of the following elements from smallest to largest first ionization energy, IE,: Si , S, Cl, Al, P, Mg , Na, Ar D.
Arrange atoms C, K, Ge, Cs in order of:decreasing atomic size: biggest size – ___ > ___ > ___ > ___ – smallest size
An element with the valence electeon configuration 4s1 would form a monatomic ion with a charge of _____. In order to form this ion, the element gain or lose how many electrons from or into the ____ subshell(s). An element with the valence electeon configuration 2s22p3 would form a monatomic ion with a charge of _____. In order to form this ion, the element gain or lose how many electrons from or into the ____ subshell(s).
3. A student was asked to write the electron configuration for a number of elements on an exam. Here is a sample of some of their answers: a) Ne s2 b) 1s²25³ c) [Kr] 4s1 Select any 2 of the answers above, and explain what is wrong. What element do you think they were describing? Write the correct electron configuration for that element.