1 1 s 2 2 s 2 2 p 6 3 s 2 3 p 6 4 s 2 3 d 10 4 p 6 5

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1. 1 s 2 2 s 2 2 p 6 3 s 2 3 p 6 4 s 2 3 d 10 4 p 6 5 s 2 4 d 1 correct 2. 1 s 2 2 s 2 2 p 6 3 s 2 3 p 6 3 d 10 4 s 2 4 p 6 5 s 2 5 p 1 3. 1 s 2 2 s 2 2 p 6 3 s 2 3 p 6 3 d 10 4 s 2 4 p 6 5 s 3 4. 1 s 2 2 s 2 2 p 6 3 s 2 3 p 6 3 d 10 4 s 2 4 p 6 4 d 3 5. 1 s 2 2 s 2 2 p 6 3 s 2 3 p 6 4 s 2 4 p 6 3 d 10 3 f 3 Explanation: 013 10.0 points A comparison of the electron configurations of cobalt (Co) and chromium (Cr) indicates that 1. Cr has 2 fewer d electrons and the same
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Patel (ap29737) – Homework 2 – Sutcliffe – (50985) 4 number of s electrons as Co. 2. Cr has 2 fewer d electrons and one less s electron than Co. correct 3. Cr has 3 fewer d electrons and the same number of s electrons as Co. 4. Cr has 3 fewer d electrons and one less s electron than Co. 5. Cr has 3 fewer d electrons and one more s electron than Co. Explanation: Cr is an exception. It is more stable when it has a half filled d -orbital. One of its 4 s electrons is elevated into the 3 d orbital, giving it one 4 s electron and five 3 d electrons. 014 10.0 points The Group IIIA elements through the Group VIIIA elements form an area of the periodic table where the electron sublevels being filled are 1. s and p orbitals. 2. f orbitals. 3. d orbitals. 4. p and d orbitals. 5. p orbitals. correct Explanation: s d p f 015 10.0 points The addition of 2 electrons to a neutral atom of sulfur would produce an ion having the same ground state electronic configuration as a neutral atom of 1. Ar. correct 2. S. 3. Cl. 4. P. 5. Si. Explanation: S 2 - has 18 electrons. The neutral Ar also has 18 electrons. 016 10.0 points According to the general trends of the peri- odic table, which of the following elements has the largest atomic radius? 1. Ca 2. Kr 3. K 4. Cs correct Explanation: Following the general pattern, which is that atomic sizes are largest in the bottom left- handcorner and smallest in the top right-hand corner of the periodic table, the largest atomic radius would belong to Cs in this group. 017 10.0 points Due to the screening effect, the 3 s electrons of magnesium (Mg) feel an effective nuclear charge (Z eff ) of 1. +1 2. - 2 3. +12 4. +2 correct
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Patel (ap29737) – Homework 2 – Sutcliffe – (50985) 5 5. +4 Explanation: The two 3 s electrons are partially shielded from the 12 protons in the nucleus by the 10 electrons in the lower energy orbitals. The lower energy electrons cancel out 10 of the positive charges from the protons in the nu- cleus, leaving only two positive charges to act on the two 3 s electrons. Thus the 3 s electrons feel an effective nuclear charge (Z eff ) of +2. Effective nuclear charge: Z eff = # of protons in the nucleus - # of lower energy electrons (not in the outer shell). 018 10.0 points The first ionization potential of the elements B, C, and N (atomic numbers 5, 6, and 7) steadily increases, but that of O is less than that of N. The best interpretation of the lower value for O is that 1. the ionization potential of N is a maxi- mum and the values decrease steadily for the elements O, F, and Ne.
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