1. Consider the first ionization energy for two atoms: Nitrogen (N) and Oxygen (O). Which one has the higher ionization energy and why? 1. Nitrogen 2. Oxygen Because 1. It lies further to the right within the same row of the periodic table. 2. It is a smaller atom 3. Electrostatic repulsion means it is harder to remove an electron from a singly occupied orbital vs. a doubly occupied one. O 2,1 ο ο ο ο ο ο O 2,3 O 1,3 O 1,2 O 1.1 O 2,2

1. Consider the first ionization energy for two atoms: Nitrogen (N) and Oxygen (O). Which one has the higher ionization energy and why? 1. Nitrogen 2. Oxygen Because 1. It lies further to the right within the same row of the periodic table. 2. It is a smaller atom 3. Electrostatic repulsion means it is harder to remove an electron from a singly occupied orbital vs. a doubly occupied one. O 2,1 ο ο ο ο ο ο O 2,3 O 1,3 O 1,2 O 1.1 O 2,2

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...

See similar textbooks

Similar questions

7. An atomic orbital is defined by a) the first three quantum numbers (n, I, m) b) the principle quantum number only (n) c) all four quantum numbers (n, I, mi, m,) d) the first two quantum numbers (n, I)
a. Write the electron configuration for Ba²+. (Express your answer as a series of orbitals, in order of increasing orbital energy. For example, the electron configuration of Li would be entered as 1s²2s¹ or [He]2s¹.) b. Write the electron configuration for Ca²+. (Express your answer as a series of orbitals, in order of increasing orbital energy. For example, the electron configuration of Li would be entered as 1s²2s¹ or [He]2s¹.) c. Write the electron configuration for P³-. (Express your answer as a series of orbitals, in order of increasing orbital energy. For example, the electron configuration of Li would be entered as 1s²2s¹ or [He]2s¹.) d. Write the electron configuration for Te²-. (Express your answer as a series of orbitals, in order of increasing orbital energy. For example, the electron configuration of Li would be entered as 1s²2s¹ or [He]2s¹.)
Fill Table 1 with full electron configuration and number of unpaired electrons with the configurations. To get number of unpaired electrons, draw orbital diagram of the outermost shell, and fill the orbitals with electrons following Aufbau Rule, Hund's Rule, and Pauli Exclusion Principle, then count how many electrons are left unpaired. Table 1: Electron Configurations of Atoms and lons Element Atomic Unpaired Full Electron Configuration Symbol Number Electrons S 1s° 2s° 2p° 3s° 3p* 16 CI Na Li F Fe Fe2+ Fe+ K* P3- O2- Mg**
How can we find the value for hydrogen?
6a. Which type of ions – cations or anions – have smaller radii than the corresponding neutral atoms? Explain why the ion radii are larger. b. Which would be smaller? Li or Li+? Explain why. c. Which would be smaller? Cl or Cl-? Explain why. d. Write the complete electron configuration for Cl atom. Please answer all parts of question.
One way to measure ionization energies is photoelectron spectroscopy (PES), a technique based on the photoelectric effect. In PES, monochromatic light is directed onto a sample, causing electrons to be emitted. The kinetic energy of the emitted electrons is measured. The difference between the energy of the photons and the kinetic energy of the electrons corresponds to the energy needed to remove the electrons (that is, the ionization energy). Suppose that a PES experiment is performed in which mercury vapor is irradiated with ultraviolet light of wavelength 58.4 nm. (Figure 1) Figure lonization energy (kJ/mol) 2500 2000 1500 1000 500 0 419 Rb 403 496 1A 2A 549 Ha 509 H 1312 $20 M Na 738 Be 899 Ca 990 801 Al 786 Sa 709 558 PD 11 710 Ga 762 Ge 947 941 579 S 1012 1000 BE 703 Sb 834 O 1402 1314 Po 812 Increasing ionization energy s 1251 Te 1008 SAY 1681 Kr Se 1140 Be 1351 Xo 1170 Rn 1037 3A 4A SA 6A 7A SA He Increasing ionization energy
Consider the element Zn. Which of the following statements is true regarding the electrons in the ground state electron configuration. I. Eight electrons occupy orbitals that have one radial node (and any number of angular nodes). II. Five electrons occupy orbitals that have two angular nodes (and any number of radial nodes). III. 15 electrons will have a magnetic spin of +1/2. IV. Six electrons occupy orbitals that have a magnetic quantum number of -1.
7. The following shapes each represent an orbital of an atom in a hypothetical universe. The small circle is the location of the nucleus in each orbital. a) If you placed an electron in each orbital, which one would be higher in energy? b) When an electron makes a transition from the orbital represented on the right to the orbital on the left, would you expect energy to be absorbed or released? c) Draw a sketch of an orbital of the same type that would be higher in energy than either of the two pictured orbitals.
4. Which of the following should be the larger atom? Why? Sodium vs. Chlorine- Lithium vs. Cesium 5. Which is larger? Why? The hydrogen 1s orbital The lithium 1s orbital 6. Which is lower in energy? Why? The hydrogen 1s orbital The lithium 1s orbital
Which of these statements referring to ionization energy is INCORRECT? A. For Na, I2 < 11 B. lonization is an endothermic process C. Helium has the highest ionization energy of all the noble gases. D. Of the elements Rb, Sr, Sb and Cs, lonization energies increase in the order: Cs < Rb < Sr < Sb O B OC A.
#7: describe the orbitals that make up n=3, describe the orbitals and their energy levels and how they are filled.
B. Given the following information of the three electrons: Quantum Number Electron A Electron B Electron C in 4 4 m, -2 1 m, + ½ + 2 - ½ 1. Which electron has the highest energy? Why? 2. Which electron has the lowest energy? Why? 3. Describe the electrons based on their quantum numbers.