Homework 3 (Chapter 9)

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Homework 3 (Chapter 9) Question 1: How many 3d electrons are in an atom of each element? Fe six 3d electrons Zn ten 3d electrons K zero 3d electrons As ten 3d electrons Question 2: You need to draw the periodic table from memory (do not look at a table to do this). First of all, how many rows would you draw? 9 18 7 10 Question 3: The element magnesium forms an ion with what charge? 2+ 2- 1- 1+ Question 4: The nearest star is Alpha Centauri, at a distance of 4.3 light-years from Earth. A light-year is the distance that light travels in one year (365 days). (a) How far away, in kilometers, is Alpha Centauri from Earth? l=1.57x10^12 km l=4.1×10^13 km l=4.1×10^12 km l=1.57x10^13 km Question 5: In one transition, an electron in a hydrogen atom falls from the n = 3 level to the n = 2 level. In a second transition, an electron in a hydrogen atom falls from the n = 2 level to the n = 1 level. Compared to the radiation emitted by the first of these transitions, the radiation emitted by the second has: a longer wavelength a lower frequency a shorter wavelength a smaller amount of energy per photon Question 6: The electron configuration of calcium is 1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 In its reactions, calcium tends to form the Ca2+ ion. Which electrons are lost upon ionization? all of the 3s electrons all of the 4s electrons two of the 3p electrons the 1s electrons

Question 7: In the Bohr model, what happens when an electron makes a transition between orbits? energy increases or decreases energy only increases energy does not change energy only decreases Question 8: How are X-rays used? to image internal bones and organs to transmit the signals used by AM and FM radio to heat substances that contain water to sterilize surgical instruments Question 9: Which orbital diagram corresponds to chlorine Cl? A C B D Question 10: How many valence electrons does selenium have? 6 34 16 4 Question 11: When sodium forms an ion, it loses electrons. How many electrons does it lose, and which orbitals do the electrons come from? one electron from 3s the orbital three electrons: one from the 3s orbital and two from the 2s orbital five electrons from the 3p orbital three electrons: two from the 3s orbital and one from the 3p orbital

Question 12: Which pair of elements has the same total number of electrons in its p orbitals? P and N Ar and Ca K and Kr Na and K Question 13: What is the Pauli exclusion principle? The maximum number of electrons in an orbital is eight. The chemical properties of elements are largely determined by the number of valence electrons they contain. When filling orbitals of equal energy, electrons fill them singly first, with parallel spins. The maximum number of electrons in an orbital is two. Question 14: Write full electron configurations for Kr. 1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^10 4p^6 1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^10 4p^3 1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^5 4p^11 1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 4d^10 4p^6 Question 15: Explain the difference between a Bohr orbit and a quantum-mechanical orbital. The quantum-mechanical model orbital s best described as a region that has the greatest probability for the location of an electron. The Bohr model orbit maps the exact path an electron would make around a nucleus. Question 16: Which of the listed elements has the highest ionization energy? S Si Ne In Question 17: Explain why Group 1 elements tend to form 1+ ions and Group 7 elements tend to form 1- ions. the number of electrons of the ions will be even numbers the number of electrons of the ions will be odd numbers the electron configuration of the ions will match that of a noble gas the electron configuration of the ions will match that of a halogen Question 18: What is the maximum number of electrons that can occupy the n=4 quantum shell? 16 8

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4 32 Question 19: Choose the correct explanation why a blue object appears blue. It appears blue because the object absorbs the wavelength corresponding to blue and reflects all of the other wavelengths from the white light that illuminated the object. It appears blue because the object reflects the wavelength corresponding to blue and absorbs all of the other wavelengths from the white light that illuminated the object. It appears blue because the object absorbs and reflects the wavelength corresponding only to blue. No answer text provided. Question 20: Give the electron configuration of magnesium. [Ne]4s^2 [Ne]3s^6 [Ne]3s^2 [Ar]3s^2 Question 21: Indicate the number of unpaired electrons in neutral atom of Krypton 2 0 unpaired electrons 3 1 Question 22: What purposes does Bohr model serve? explain how protons are arranged within the atomic structure explain how electrons are arranged within the atomic structure explain how neutrons affect the chemical and physical properties of each element explain how electrons affect the chemical and physical properties of each element Question 23: Choose the element with the larger atoms from each of the following pair: Al or In Al Cannot determine In Question 24: Which element has the fewest valence electrons? Ga O K B Ca Question 25: Which of the listed elements is most metallic? Al

O N H

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