Organic Chemistry
8th Edition
ISBN: 9781305580350
Author: William H. Brown, Brent L. Iverson, Eric Anslyn, Christopher S. Foote
Publisher: Cengage Learning
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Textbook Question
Chapter 1, Problem 1.21P
Identify the atom that has each ground-state electron configuration.
- (a) 1s2 2s2 2p6 3s2 3p4
- (b) 1s2 2s2 2p4
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Identify the atom that has each ground-state electron configuration.
(a) 1s 2 2s 2 2p6 3s 2 3p4
(a) Identify the following neutral elements by their condensed electron configurations. (Enter the chemical symbol or name of the element.)
(i) [Ar] 4s2 3d3 (ii) [Kr] 5s2 4d10 5p3 (iii) [Ar] 4s2 3d10 4p4
Give the ground-state electron configuration for each of the
following elements. After each atom is its atomic number in
parentheses.
(a) Boron (5)
(b) Hydrogen (1)
Chapter 1 Solutions
Organic Chemistry
Ch. 1.1 - Prob. 1.1PCh. 1.2 - Prob. 1.2PCh. 1.2 - Judging from their relative positions in the...Ch. 1.2 - Classify each bond as nonpolar covalent or polar...Ch. 1.2 - Using the symbols and +, indicate the direction...Ch. 1.2 - Draw Lewis structures showing all valence...Ch. 1.2 - Draw Lewis structures for these ions and show...Ch. 1.3 - Draw Lewis structures and condensed structural...Ch. 1.3 - Prob. 1.9PCh. 1.3 - Prob. 1.10P
Ch. 1.3 - Prob. 1.11PCh. 1.3 - Prob. 1.12PCh. 1.4 - Predict all bond angles for these molecules. (a)...Ch. 1.5 - The geometry of carbon in diamond is tetrahedral,...Ch. 1.5 - Because of their spherical shape, C60 molecules...Ch. 1.5 - What best describes the CCC bond angles in C60? 1....Ch. 1.5 - Prob. 1.14PCh. 1.7 - Describe the bonding in these molecules in terms...Ch. 1.8 - Prob. 1.16PCh. 1.8 - Prob. 1.17PCh. 1.8 - Prob. 1.18PCh. 1.9 - Draw three contributing structures of the...Ch. 1.9 - What is the hybridization state of the circled...Ch. 1.9 - The molecule shown on the right in the example in...Ch. 1.9 - Prob. CQCh. 1.9 - The following structure is called imidazolium....Ch. 1 - Write the ground-state electron configuration for...Ch. 1 - Identify the atom that has each ground-state...Ch. 1 - Define valence shell and valence electron.Ch. 1 - How many electrons are in the valence shell of...Ch. 1 - Prob. 1.24PCh. 1 - Prob. 1.25PCh. 1 - Prob. 1.26PCh. 1 - Write Lewis structures for these compounds. Show...Ch. 1 - Write Lewis structures for these ions. Show all...Ch. 1 - Prob. 1.29PCh. 1 - Some of these structural formulas are incorrect...Ch. 1 - Following the rule that each atom of carbon,...Ch. 1 - Following are several Lewis structures showing all...Ch. 1 - Which statements are true about electronegativity?...Ch. 1 - Why does fluorine, the element in the upper right...Ch. 1 - Arrange the single covalent bonds within each set...Ch. 1 - Using the values of electronegativity given in...Ch. 1 - Prob. 1.37PCh. 1 - Use VSEPR to predict bond angles about each...Ch. 1 - Use VSEPR to predict bond angles about each atom...Ch. 1 - Use VSEPR to predict the geometry of these ions....Ch. 1 - Prob. 1.41PCh. 1 - Prob. 1.42PCh. 1 - What is the meaning of the term tertiary (3) when...Ch. 1 - What is the meaning of the term tertiary (3) when...Ch. 1 - Draw structural formulas for (a) The four primary...Ch. 1 - Draw structural formulas for the three tertiary...Ch. 1 - Prob. 1.47PCh. 1 - Identify the functional groups in each compound.Ch. 1 - Draw a three-dimensional representation for each...Ch. 1 - Tetrafluoroethylene, C2F4, is the starting...Ch. 1 - Which statements are true about resonance...Ch. 1 - Prob. 1.52PCh. 1 - Prob. 1.53PCh. 1 - Prob. 1.54PCh. 1 - Are the structures in each set valid contributing...Ch. 1 - State the orbital hybridization of each...Ch. 1 - Describe each highlighted bond in terms of the...Ch. 1 - Following is a structural formula of the...Ch. 1 - Draw a Lewis structure for methyl isocyanate,...Ch. 1 - What is the hybridization of the highlighted atoms...Ch. 1 - Using cartoon representations, draw a molecular...Ch. 1 - In what kind of orbitals do the lone-pair...Ch. 1 - Draw the delocalized molecular orbitals for the...Ch. 1 - Prob. 1.64APCh. 1 - Each compound contains both ions and covalent...Ch. 1 - Predict whether the carbon-metal bond in these...Ch. 1 - Prob. 1.67APCh. 1 - Phosphorus is immediately under nitrogen in the...Ch. 1 - Draw a Lewis structure for the azide ion, N3. (The...Ch. 1 - Cyanic acid, HOCN, and isocyanic acid, HNCO,...Ch. 1 - In Chapter 6, we study a group of organic cations...Ch. 1 - Many reactions involve a change in hybridization...Ch. 1 - Following is a structural formula of benzene,...Ch. 1 - Following are three contributing structures for...Ch. 1 - (a) Draw a Lewis structure for the ozone molecule,...Ch. 1 - The following two compounds are isomers; that is,...Ch. 1 - In future chapters, we will encounter...Ch. 1 - Prob. 1.78AP
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- Write the ground-state electron configuration for each atom. After each atom is its atomic number in parentheses. (a) Sodium (11) (b) Magnesium (12) (c) Oxygen (8) (d) Nitrogen (7)arrow_forwardUse the noble-gas notation and write the ground-state electronic configurations of the following ions:(a) Ca2+ (b) Ga3+ (c) Cr3+arrow_forward2) What is the electron geometry of the indicated atoms? A- C D Atom A = Atom B = Atom C = Atom D = Barrow_forward
- Which species, has the following ground state electron configuration: 1s2 2s2 2p6 3s2 3p6 4s0 3d8 (a) Fe+ (b) Ni (c) Ni2+ (d) Cu2+arrow_forwardIdentify all the possible elements that have the following valence electronic configuration. a) S2d1 T1 A1 b) S2p6 T1 A1arrow_forwardFor each pair, identify the orbital in which an electron possesses more energy. (a) 4s or 5s; (b) 5p or 5darrow_forward
- How many valence electrons does each of the following atoms have? (a) Oxygen (b) Magnesium (c) Fluorinearrow_forwardpart 1: Given an electron configuration: 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p5 Give the electron configuration of the most stable ion of this element: ???????? part 2: Given an electron configuration: 1s2 2s2 2p6 3s2 3p6 4s2 3d10 Give the electron configuration of the most stable ion of this element: ???????? Please answer part 1 and part 2. Thank youarrow_forwardQ25. Identify the following atoms or ions from their electron configurations: (a) W: 1s 2 2s 2 2p6 3s 2 3p6 4s 2 3d10 4p6,5s1 (b) X-: 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 (c) Y++: 1s2 2s2 2p6 3s 2 3p6 4s 2 3d10 4p6 5s2 4d10 5p6 (d) Z: 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2 4f 11arrow_forward
- Using complete subshell notation (1s^22s^22p^6, and so forth), predict the electron configurations of the following ions. (a) N3– (b) Ca2+ (c) S– (d) Cs2+ (e) Cr2+ (f) Gd3+arrow_forwardThe electron configuration of a cation M3+ is [Ar] 3d3. What is the electron configuration of the original atom M? (M is not a real chemical symbol of an element.) (A) [Ar] 4s1 3d5 (B) [Ar] 4s2 3d4 (C) [Ar] 3d6 (D) [Ar] 3d4 4p2arrow_forward54.Using complete subshell notation (1s22s22p6, and so forth), predict the electron configurations of the following ions. (a) N3– (b) Ca2+ (c) S– (d) Cs2+ (e) Cr2+ (f) Gd3+arrow_forward
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