Essential Organic Chemistry (3rd Edition)
3rd Edition
ISBN: 9780321937711
Author: Paula Yurkanis Bruice
Publisher: PEARSON
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Textbook Question
Chapter 1.3, Problem 5P
- a. Find potassium (K) in the periodic table and predict how many valence electrons it has.
- b. What orbital does the unpaired electron occupy?
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3. Is this arrangement of electrons possible, why or why not?
4. What would happen, eventually, to the electron in the highest energy level in Model 1?
5. Write the electronic configuration corresponding to the electronic arrangement
6. Write out the ground state electron configuration for this atom.
The electrons in an atom are good grouped based on their shell, subshell, and orbital. What are the shells? List them. How many subshells are there per shell? List those for the first four shells. How many orbitals are in each subshell? How many electrons can be fit in an orbital? What is the total number of electrons per shell?
The electrons in an atom are grouped based in their shell, subshell, and orbital. What are the shells? List them. How many subshells are there per shell? List those for the first four shells. How many orbitals are in each subshell? How many electrons can be fit in a n orbital? What is the total number of electrons per shell?
Chapter 1 Solutions
Essential Organic Chemistry (3rd Edition)
Ch. 1.1 - Oxygen has three isotopes, 16O, 17O, and 18O. The...Ch. 1.2 - Prob. 2PCh. 1.2 - How many valence electrons do chlorine, bromine,...Ch. 1.2 - Look at the relative positions of each pair of...Ch. 1.3 - a. Find potassium (K) in the periodic table and...Ch. 1.3 - Which bond is more polar?Ch. 1.3 - Which of the following has a. the most polar bond?...Ch. 1.3 - Use the symbols + and to show the direction of...Ch. 1.3 - After examining the potential maps for LiH, HF,...Ch. 1.4 - An atom with a formal charge does not necessarily...
Ch. 1.4 - Prob. 12PCh. 1.4 - a. Draw two Lewis structures for C2H6O. b. Draw...Ch. 1.4 - Draw the lone-pair electrons that are not shown in...Ch. 1.4 - Prob. 16PCh. 1.4 - Which of the atoms in the molecular models in...Ch. 1.4 - Prob. 18PCh. 1.7 - What orbitals are used to form the 10 sigma bonds...Ch. 1.9 - Put a number in each of the blanks: a. ___ s...Ch. 1.11 - Predict the approximate bond angles in a. the...Ch. 1.11 - According to the potential map for the ammonium...Ch. 1.12 - Prob. 25PCh. 1.13 - a. Predict the relative lengths and strengths of...Ch. 1.13 - Prob. 28PCh. 1.14 - Which of the bonds in a carbonoxygen double bond...Ch. 1.14 - Caffeine is a natural insecticide, found in the...Ch. 1.14 - a. What is the hybridization of each of the carbon...Ch. 1.14 - Prob. 33PCh. 1.14 - Describe the orbitals used in bonding and the bond...Ch. 1.15 - Account for the difference in the shape and color...Ch. 1.15 - Which of the following molecules would you expect...Ch. 1 - Draw a Lewis structure for each of the following...Ch. 1 - Prob. 38PCh. 1 - What is the hybridization of all the atoms (other...Ch. 1 - Prob. 40PCh. 1 - Draw the condensed structure of a compound that...Ch. 1 - Prob. 42PCh. 1 - Prob. 43PCh. 1 - Draw a Lewis structure for each of the following...Ch. 1 - Prob. 45PCh. 1 - List the bonds in order from most polar to least...Ch. 1 - What is the hybridization of the indicated atom in...Ch. 1 - Write the Kekul structure for each of the...Ch. 1 - Assign the missing formal charges.Ch. 1 - Predict the approximate bond angles for the...Ch. 1 - Prob. 51PCh. 1 - a. Which of the indicated bonds in each compound...Ch. 1 - In which orbitals are the lone pairs in nicotine?...Ch. 1 - Draw the missing lone-pair electrons and assign...Ch. 1 - Rank the following compounds from highest dipole...Ch. 1 - Prob. 56PCh. 1 - a. Which of the species have bond angles of 109.5?...Ch. 1 - Prob. 58PCh. 1 - Sodium methoxide (CH3ONa) has both ionic and...Ch. 1 - a. Why is a H 8 H bond (0.74 ) shorter than a C 8...Ch. 1 - Which compound has a larger dipole moment, CHCl3...Ch. 1 - Which compound has a longer C 8 Cl bond?Ch. 1 - Prob. 63PCh. 1 - The following compound has two isomers. One isomer...
Additional Science Textbook Solutions
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- Compare the configurations below with two electrons located in p orbitals. Which would be the most stable (have the lowest energy)? Which would be the least stable? Explain your answers.arrow_forward1) Give the electronic configuration of Silver and Silver (2+). Note that Silver (2+) means that it has lost 2 of its valence electrons.arrow_forwardDefine an atomic orbital, how many orbitals do we have? and how many electrons can they hold?arrow_forward
- What values are needed to determine the energy of an electron in a many‑electron atom? ?? ? ?? ? What information is most important in determining the size of an orbital? ? ?? ? ?? What information is needed to determine the orientation of an orbital? ?? ?? ? ? What information is needed to determine the general shape of an orbital? ? ?? ?? narrow_forwardThe total number of electrons, valence electrons, and valency of He, C, and N? Thank you!arrow_forwardCompare the configurations below with two electrons located in p orbitals. Which would be the most stable (have the lowest energy)? Which would be the least stable? Explain your answers.</o:p> </v:imagedata> </v:shape></o:p>arrow_forward
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