Homework 2 (Chapter 9)

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Homework 2 (Chapter 9) Question 1: 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? 7 9 10 18 Question 2: Choose the element with the larger atoms from each of the following pair: Al or In In Al Cannot determine Question 3: Choose the 1 s orbital. A C B Question 4: Why is it important when writing orbital diagrams? It is important in order to indicate the order in which orbitals fill. It is important in order to write all electrons with parallel spins. It is important in order to write the correct number of paired and unpaired electrons. It is important in order to write the correct number of total electrons.

Question 5: 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? the 1s electrons all of the 4s electrons two of the 3p electrons all of the 3s electrons Question 6: How many valence electrons are in each of the following elements? O 6 valence electrons S 6 valence electrons Br 7 valence electrons Rb 1 valence electrons Question 7: How are wavelength and frequency of light related? logarithmic relationship direct relationship inverse relationship exponential relationship Question 8: Give the electron configuration of magnesium. [Ne]3s^6 [Ne]3s^2 [Ne]4s^2 [Ar]3s^2 Question 9: How many 2p electrons are in an atom of each element? C two 2p electrons N three 2p electrons F five 2p electrons P six 2p electrons Question 10: Which set of wavelengths for light are arranged in order of increasing frequency? 480 nm; 500 nm; 520 nm 520 nm; 500 nm; 480 nm 520 nm; 480 nm; 500 nm 480 nm; 520 nm; 500 nm Question 11: 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 12: What is the Pauli exclusion principle? The maximum number of electrons in an orbital is two. The chemical properties of elements are largely determined by the number of valence electrons they contain. The maximum number of electrons in an orbital is eight. When filling orbitals of equal energy, electrons fill them singly first, with parallel spins. Question 13: Write full electron configurations for B. 1s^2 2s^2 2p^2 1s^2 3s^2 2p^1 1s^1 2s^2 2p^1 1s^2 2s^2 2p^1 Question 14 The trends shown in the given figure reflect the tendency of ___A ___ elements to form ions that will have an identical electron configuration to that of a noble gas. The elements of groups 1A, 2A, and 3A shown in the figure ___B ___ electrons to form ____C ___ charged ions. The elements of groups 5A, 6A, and 7A normally ___D ___ electrons to form ___E ___charged ions. The ___F ___ series represents the filling of core orbitals, and the number of ___G ___ electrons is mostly constant. A main-group B lose C positively D gain E negatively F transition G outermost Question 15: Explain why Group 1 elements tend to form 1+ ions and Group 7 elements tend to form 1- ions. 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

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