ORGANIC CHEMISTRY-W/S.G+SOLN.MANUAL
8th Edition
ISBN: 9780134595450
Author: Bruice
Publisher: PEARSON
expand_more
expand_more
format_list_bulleted
Textbook Question
Chapter 1.3, Problem 7P
a. Find potassium (K) in the periodic table and predict how many valence electrons it has.
b. What orbital does the unpaired electron occupy?
Expert Solution & Answer
Want to see the full answer?
Check out a sample textbook solutionStudents have asked these similar questions
1. The rule stating that elements need 8 valence electrons in
order to become stable:
A.Lewis Rule
B.Pauli's Rule
C.Hund's Rule
D.Octet Rule
2. The Main Energy Level is composed of
P, d, and f.
A.Pauli's Exclusion Principle
B. Hund's Rule
C. Subshell
D. Valence Electron
3. It is important to learn about quantum mechanies
because:
which are S,
A. This information tells us why certain elements may be
very reactive while others may be relatively non- reactive.
B.This information tells us how atoms grow to become
larger molecules.
C.This information tells us why certain elements are found
as gases at room temperature.
D.This information allows us to undersstand why some
chemicals are colorful and others are dull and muted.
13. Draw the Lewis dot symbol for oxygen, O, how many unpaired electrons are there?
A. 4
B. 0
C. 2
D. 3
A. Given the following elements: N and O
1.Write the electronic configuration of each atom in their Ground and Excited States
2.Identify the valence electrons and the covalency numbers (GS & ES)
3.Write the Lewis Dot Structure of these atoms (GS & ES)
4.Identify the pure orbitals occupied by the valence electrons (GS & ES)
Chapter 1 Solutions
ORGANIC CHEMISTRY-W/S.G+SOLN.MANUAL
Ch. 1.1 - Oxygen has three isotopes, 16O, 17O, and 18O. The...Ch. 1.1 - a. How many protons do the following species...Ch. 1.1 - Chlorine has two isotopes, 35Cl and 37Cl; 75.77%...Ch. 1.2 - Prob. 4PCh. 1.2 - a. Write the ground-state electronic configuration...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? a. b. c. d.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 - Explain why HCL has a smaller dipole moment than...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. 16PCh. 1.4 - a. Draw two Lewis structure for C2H6O. b. Draw...Ch. 1.4 - Draw the lone-pair electrons that are not shown in...Ch. 1.4 - Prob. 20PCh. 1.4 - Which of the atoms in the molecular models in...Ch. 1.4 - Prob. 22PCh. 1.4 - Prob. 23PCh. 1.5 - Draw the following orbitals: a. 3s orbital b. 4s...Ch. 1.6 - Prob. 25PCh. 1.6 - Indicate the kind of molecular orbital (, , , or )...Ch. 1.7 - What orbitals are used to form the 10 sigma bonds...Ch. 1.7 - Explain why a bond formed by overlap of s orbital...Ch. 1.9 - Put n number in each of the blanks: a. __ s...Ch. 1.9 - For each of the given species: a. Draw its Lewis...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. 35PCh. 1.13 - a. What are the relative lengths and strengths of...Ch. 1.13 - Prob. 38PCh. 1.14 - Describe the orbitals used in bonding and the bond...Ch. 1.15 - Which of the bond in a carbon-oxygen double bond...Ch. 1.15 - Would you expect a CC bond formed by sp2sp2...Ch. 1.15 - Caffeine is a natural insecticide found in the...Ch. 1.15 - a. What is the hybridization of each of the carbon...Ch. 1.15 - Predict the approximate bond angles for a. the CNC...Ch. 1.16 - What of the following molecules would you expect...Ch. 1.16 - Account for the difference in the shape and color...Ch. 1.16 - If the dipole moment of CH3F is 1.847 D and the...Ch. 1 - Draw a Lewis structure for each of the following:...Ch. 1 - Prob. 50PCh. 1 - What is the hybridization of all the atoms (other...Ch. 1 - Draw the condensed structure of a compound that...Ch. 1 - Predict the approximate bond angles: a. the CNH...Ch. 1 - Prob. 54PCh. 1 - Draw a Lewis structure for each of the following:...Ch. 1 - What is the hybridization of each of the carbon...Ch. 1 - Rank the bonds from most polar. a. CO, CF, CN b....Ch. 1 - Draw a Lewis structure for each of the following:...Ch. 1 - Prob. 59PCh. 1 - What is the hybridization of the indicated atom in...Ch. 1 - Predict the approximate bond angles for the...Ch. 1 - Prob. 62PCh. 1 - Draw the missing lone-pair electrons and assigns...Ch. 1 - a. Which of the indicated bonds in each molecule...Ch. 1 - For each of the following molecules, indicate the...Ch. 1 - Draw a Lewis structure for each of the following:...Ch. 1 - Prob. 67PCh. 1 - Rank the following compounds from highest dipole...Ch. 1 - In which orbitals are the lone pairs in nicotine?Ch. 1 - Prob. 70PCh. 1 - Prob. 71PCh. 1 - a. Which of the species have bond angles of 109.5?...Ch. 1 - Prob. 73PCh. 1 - Which compound has a larger dipole moment: CH3Cl...Ch. 1 - Prob. 75PCh. 1 - Explain why CH3Cl has a greater dipole moment than...Ch. 1 - a. Draw a Lewis structure for each of the...Ch. 1 - There are three isomers with molecular formula...
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 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_forwardWhich 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 firstarrow_forward12. Draw the Lewis dot symbol for boron, B, how many unpaired electrons are there? A. 1 B. 2 C. 4 D. 3arrow_forward
- 4. Write the (ground state) electronic configuration for each of the following. a. antimony b. lead C. xenon d. selenide ion e. cobalt (II) ion f. cobalt (III) ion g. palladium (II) ion h. ruthenium (III) ion i. zincionarrow_forwardChemistryarrow_forwardDo question 14 and 15. This is not graded. This is a study guide.arrow_forward
- 4. Consider this chemical equation: Br + e > Br + energy Which concept does this chemical equation correspond with? A. atomic radius B. ionization energy C. electron affinity D. electronegativity E, metal reactivityarrow_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_forwardPredict how the 1st ionization energy of neon would compare to the 2nd ionization energy of sodium and give a reason for why you made your prediction. a. Which ionization has a larger value or are they similar?b. Provide an explanationarrow_forward
- Metals have high melting point because a. the electrons are mobile b. of close-packed arrangement of atoms c. of the strength of the electrostatic attraction between the metal ions and electrons d. when heat touches the metal, the loosely bonded electron vibrate easily and radiate the heat with the same frequency and wavelength. Which substance has mobile electron cloud as a binding force? a. salt b. ice c. dry ice d. Cu wirearrow_forwardDue to inert pair effect, the elements of group IV having electronic configuration ns’, np? will form A. M" cation i. B. M" cation c. M' cation D. M²" cation ii. Which of the following is not an alternative ozone depleting Chlorofluorocarbon (CFCS)? A. Hydrocarbons B. CO, C. Hydrofluorocarbons D. Perfluorocarbons(PFCS) iii. Double bond is formed as a result of: A. Addition Reaction B. Polymerization Reaction C. Substitution Reaction D. Elimination Reaction iv. Which region of electromagnetic spectrum is involved in NMR spectroscopy? A. Radio waves B. Ultraviolet C. Visible D. Microwaves v. Which of the following oxide is used as a Catalyst in Contact process? C. Fe,O3 Which of the following alcohols will be most easily dehydrated to give an alkene? B. 2-methyl 2-prepanol Which of the following can undergo Aldol Condensation reaction? A. V,0; В. Р.0, D. Mn;03 vi. A. 3- Propanol С. 1-prepanol D.2-prepanol vii. A. Benzaldehyde B. Trimethylacetaldehyde C. Formaldehyde D. Acetaldehyde…arrow_forward1. How many unpaired electrons are in the beryllium atom? This atom is A. Paramagnetic B. Diamagnetic 2. How many unpaired electrons are in the iron atom? This atom is A. Paramagnetic B. Diamagneticarrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
- Living By Chemistry: First Edition TextbookChemistryISBN:9781559539418Author:Angelica StacyPublisher:MAC HIGHER
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