EP ESSENTIAL ORG.CHEM.-MOD.MASTERING
3rd Edition
ISBN: 9780133858501
Author: Bruice
Publisher: PEARSON CO
expand_more
expand_more
format_list_bulleted
Videos
Textbook Question
Chapter 1.9, Problem 21P
Put a number in each of the blanks:
- a. ___ s orbital and ___ p orbitals form ____ sp3 orbitals.
- b. ___ s orbital and ___ p orbitals form ____ sp2 orbitals.
- c. ___ s orbital and ___ p orbitals form ____ sp orbitals.
Expert Solution & Answer
Want to see the full answer?
Check out a sample textbook solution
Students have asked these similar questions
Put a number in each of the blanks:a. ___ s orbital and ___ p orbitals form ____ sp3 orbitals.b. ___ s orbital and ___ p orbitals form ____ sp2 orbitals.c. ___ s orbital and ___ p orbitals form ____ sp orbitals.
What is the maximum number of electrons that can be placed into each of the following.
a. 1s orbital
b. 2p orbital
c. 2p subshell
d. n=2 shell
e. 3d subshell
f. 4f subshell
Which statement is an example of the Pauli Exclusion Principle?
a. Atoms with a full octet shell have more stability.
b. When filling orbitals with the same energy levels, electrons fill them singly first, and then form pairs when every orbital has a single electron.
c. Two electrons in an orbital must have opposite spins
d. Electrons must fill the lowest energy levels first
Chapter 1 Solutions
EP ESSENTIAL ORG.CHEM.-MOD.MASTERING
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
Find more solutions based on key concepts
Problem 11.1 Neopheliosyne B is a novel acetylenic fatty acid isolated from a New Caledonian marine sponge. (a)...
Organic Chemistry
Write the electron configurations far each of the following elements: (a) Sc. (b) Ti. (c) Cr. (d) Fe. (e) Ru
Chemistry by OpenStax (2015-05-04)
For each of the following 2-dimensional shapes, determine the highest order rotation axis of symmetry.
Inorganic Chemistry
Give one example from main group chemistry that illustrates each of the following descriptions: (a) Covalent ne...
General Chemistry: Atoms First
Classify each example of molecular art as a pure element, a pure compound, or a mixture.
General, Organic, and Biological Chemistry - 4th edition
22.102 Write the structures of the cis and tram isomers, if any, for the following compounds:
Chemistry: The Molecular Nature of Matter
Knowledge Booster
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.Similar questions
- What are the differences between the :math>2s orbital and the 1s orbital of hydrogen? How are they similar?arrow_forwardChemistryarrow_forward5. What is quantum-mechanical model of the atom? A. Describes an electron probability distribution that determines the most likely location of an electron. B. Is the currently accepted atomic model. C. Makes predictions based on Schrodinger's wave equation. D. All of the above 6. In the quantum-mechanical model of the atom, which of the following is NOT one of the four quantum numbers needed to specify the probable location of an electron? A. Principal quantum number (n) which describes the energy level/distance from the nucleus. B. Heisenberg number (H) which describes the electron's position and momentum. C. Angular quantum number (I) which describes the shape of an electron's orbital. D. Magnetic quantum number (ml) which describes the orbitals orientation in space. 7. Which of the statement below best explains Heisenberg Uncertainty Principle? A. Assumes that the electrons take positions predicted by Bohr's theory. B. States that the position of an electron can be found by…arrow_forward
- 8. In the quantum-mechanical model of the atom, how orbit is being defined? A. Region of the most probable proton location. B. Region of the most probable electron location. C. Circular path traveled by an electron around an orbital. D. Circular path traveled by a proton around an orbital. A.31 D. 2P U. 20 120 19. Which of the orbitals below do not exist due to the constraints upon the angular quantum number? A.3d B. 3p C. 3s D. 3f 20. Which one of the following is an incorrect orbital notation? C. 3s D.2p A.4f B.2darrow_forwardWhat is the Pauli Exclusion Principle? * a. An atomic orbital can only hold a maximum of 2 electrons, each with opposite spins b. An atomic orbital can hold a minimum of 6 electrons, each with opposite spins c. An atomic orbital can hold a maximum of 6 electrons, each with the same spin d. An atomic orbital can hold a minimum of 2 electrons, each with opposite spinsarrow_forwardQuiz time Write your answers on your blank page and be prepared to upload a photo to this Quiz Assignment. 1. a. Write the Electron Configuration for Phosphorus b. Draw the Orbital Diagram for Phosphorus c. In your own words, and referencing to the Electron Configuration & Orbital Diagram for Phosphorus, describe how you used the Aufbau Principle, Hund's Rule and the Pauli Exclusion Principle. Include enough detail that would help to explain these concepts to someone for the first time. Take a picture of your work and upload to this form. * 1 Add file Send me a cony of my responsesarrow_forward
- Look at the relative positions of each pair of atoms listed here in the periodic table. How many core electrons does each have? How many valence electrons does each have?a. carbon and siliconb. oxygen and sulfurc. nitrogen and phosphorusd. magnesium and calciumarrow_forwardmultiple choicearrow_forwardConsider the electron configuration for fluorine (F) and the electron configuration for chlorine (CI). What is different about the valence electrons in these two atoms? 1.There are different numbers of valence electrons. II.The valence electrons have different energies. III. The valence electrons are in different types of orbitals (s, p, d, f). IV.The valence electrons are in different size orbitals. O I only O I and III OII and IV O II only O IV onlyarrow_forward
- How many electrons are present in each shell, subshell, or orbital? a. a 2 p orbital b. the 3 d subshell c. a 3 d orbital d. the third shellarrow_forwarda. What is the maximum number of electrons that can go into the first shell? The second shell?b. How many electrons are present in an atom with its 1s, 2s and 2p subshells completely filled?c. How many subshells are in the 3rd shell?d. How many orbitals are there in the third principal energy level?arrow_forwardPlease help with question 5arrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
Chemistry & Chemical ReactivityChemistryISBN:9781133949640Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage Learning
Chemistry & Chemical ReactivityChemistryISBN:9781337399074Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage Learning
Chemistry: Matter and ChangeChemistryISBN:9780078746376Author:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl WistromPublisher:Glencoe/McGraw-Hill School Pub Co
Introductory Chemistry: A FoundationChemistryISBN:9781337399425Author:Steven S. Zumdahl, Donald J. DeCostePublisher:Cengage Learning
World of Chemistry, 3rd editionChemistryISBN:9781133109655Author:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCostePublisher:Brooks / Cole / Cengage Learning
Living By Chemistry: First Edition TextbookChemistryISBN:9781559539418Author:Angelica StacyPublisher:MAC HIGHER
Chemistry & Chemical Reactivity
Chemistry
ISBN:9781133949640
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:Cengage Learning
Chemistry & Chemical Reactivity
Chemistry
ISBN:9781337399074
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:Cengage Learning
Chemistry: Matter and Change
Chemistry
ISBN:9780078746376
Author:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom
Publisher:Glencoe/McGraw-Hill School Pub Co
Introductory Chemistry: A Foundation
Chemistry
ISBN:9781337399425
Author:Steven S. Zumdahl, Donald J. DeCoste
Publisher:Cengage Learning
World of Chemistry, 3rd edition
Chemistry
ISBN:9781133109655
Author:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCoste
Publisher:Brooks / Cole / Cengage Learning
Living By Chemistry: First Edition Textbook
Chemistry
ISBN:9781559539418
Author:Angelica Stacy
Publisher:MAC HIGHER
Quantum Numbers, Atomic Orbitals, and Electron Configurations; Author: Professor Dave Explains;https://www.youtube.com/watch?v=Aoi4j8es4gQ;License: Standard YouTube License, CC-BY
QUANTUM MECHANICAL MODEL/Atomic Structure-21E; Author: H to O Chemistry;https://www.youtube.com/watch?v=mYHNUy5hPQE;License: Standard YouTube License, CC-BY