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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the number of electrons of the ions will be odd numbers the number of electrons of the ions will be even numbers Question 16: Choose the correct trend in ionization energy. ionization energies decrease going across a row in the periodic table from left to right; it increases going down a column ionization energies increase going across a row in the periodic table from left to right; it increases going down a column ionization energies decrease going across a row in the periodic table from left to right; it decreases going down a column ionization energies increase going across a row in the periodic table from left to right; it decreases going down a column Question 17: What is the maximum number of electrons that can occupy the n = 2 quantum shell? 10 8 6 2 Question 18: 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 smaller amount of energy per photon a longer wavelength a shorter wavelength a lower frequency Question 19: Which property decreases as you move down a column in the periodic table? metallic character ionization energy none of the above (all decrease as you move down a column). atomic size Question 20: How are X-rays used? to heat substances that contain water to transmit the signals used by AM and FM radio to sterilize surgical instruments to image internal bones and organs Question 21 The quantum-mechanical orbitals represent____A ___. Each orbital has a region of highest ___B ___. roughly corresponding to its ___C ___ . The farther from this region, the ___D___ the

probability of finding the electron, but the probability never quite reaches ___E ___. This produces a fuzzy effect. A regions in space where electron is statistically most likely to be found B density C shape D lower E zero Question 22: Which electron is, on average, closer to the nucleus: an electron in a 2s orbital or an electron in a 3s orbital? On average, the 3s electron is closer to the nucleus. they have the same distance from nucleus On average, the 2s electron is closer to the nucleus. Question 23: The element magnesium forms an ion with what charge? 2+ 2- 1+ 1- Question 24: Order the elements Sr, Ca, and Se in order of decreasing atomic size. Se> Sr> Ca Se> Ca> Sr Sr> Ca> Se Ca> Se> Sr Question 25: Which property increases as you move from left to right across a row in the periodic table? ionization energy metallic character atomic size

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