. (a) Draw the shape of the atomic valence orbitals formed by the overlaping of two fluoride 2p atomic orbitals. (b) Draw the molecular orbital diagrams for F2 and F2*. Identify their bond order and magnetic properties. (c) An unstable nucleus exhibit radioactivity. (i) Explain how the number of protons and neutrons in a radioactive nucleus can be used to predict its probable decay. (ii) Illustrate your answer in (1) with a schematic graph.

. (a) Draw the shape of the atomic valence orbitals formed by the overlaping of two fluoride 2p atomic orbitals. (b) Draw the molecular orbital diagrams for F2 and F2*. Identify their bond order and magnetic properties. (c) An unstable nucleus exhibit radioactivity. (i) Explain how the number of protons and neutrons in a radioactive nucleus can be used to predict its probable decay. (ii) Illustrate your answer in (1) with a schematic graph.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

(a) Draw the Lewis structure for hydrogen peroxide, H2O2.(b) What is the weakest bond in hydrogen peroxide? (c) Hydrogenperoxide is sold commercially as an aqueous solution inbrown bottles to protect it from light. Calculate the longestwavelength of light that has sufficient energy to break theweakest bond in hydrogen peroxide.
Write the chemical formulas for the following compounds:(a) Silver cyanide(b) Calcium hypochlorite(c) Potassium chromate(d) Gallium oxide(e) Potassium superoxide(f) Barium hydrogen carbonate
(a) What are trihalomethanes (THMs)? (b) Draw the Lewisstructures of two example THMs.
Each of the chemically active Period 2 elements forms sta-ble compounds that have bonds to fluorine.(a) What are the names and formulas of these compounds?(b) Does ΔEN increase or decrease left to right across the period?(c) Does percent ionic character increase or decrease left to right?(d) Draw Lewis structures for these compounds.
Which molecule would you expect to be a free radical?(a) CO (b) CO2 (c) N2O (d) ClO
The strength of a covalent bond depends upon the size of the atoms and the bond order. In general short bonds are strong bonds. For each pair of covalently bonded atoms, choose the one expected to have the higher bond energy.(A) C≡N(B) C=N ...... (A,B) fill in the blank 1(C) N-N(D) N=N ...... (C,D) fill in the blank 2
From their Lewis structures, determine the number of sand p bonds in each of the following molecules or ions:(a) CO2; (b) cyanogen, 1CN22; (c) formaldehyde, H2CO;(d) formic acid, HCOOH, which has one H and two O atomsattached to C.
The length of a covalent bond depends upon the size of the atoms and the bond order. For each pair of covalently bonded atoms, choose the one expected to have the shortest bond length.(A) C≡N(B) C=N ...... (A,B) fill in the blank 1(C) N-N(D) N=N ...... (C,D) fill in the blank 2
Which molecule would you expect to be a free radical?(a) CO(b) CO2(c) N2O(d) NO2
In 1995, Mario Molina, Paul Crutzen, and F. SherwoodRowland shared the Nobel Prize in chemistry for their work onatmospheric chemistry. One of several reaction sequences pro-posed for the role of chlorine in the decomposition of strato-spheric ozone is (1) Cl(g) +O3(g)→ ClO(g) +O₂(g) (2) ClO(g) +ClO(g)→ Cl₂O₂(g) (3) Cl₂O₂→ (g)2Cl(g)+ O₂(g).Over the tropics, O atoms are more common in the stratosphere:(4) ClO(g) +O(g)→ Cl(g) +O₂(g).(a) Which, if any, of these are oxidation-reduction reactions?(b) Write an overall equation combining reactions 1–3
In regard to the greenhouse effect, which statement is not true? (a) Ultraviolet and visible radiation are converted to infrared radiation at the surface of Earth. (b) Approximately one-third of the radiation of the Sun does not enter the atmosphere of Earth. (c) Infrared radiation is absorbed by greenhouse gases. (d) Greenhouse gases were not historically present in the atmosphere. (e) Ultraviolet radiation is absorbed by ozone.
QUESTION 5 (31 MARKS) (a) (i) Draw a pz orbital and a d?-y² orbital. (4) (ii) What are the differences between a 5pz orbital and a 4d,- orbital in the H atom? (6) (b) (i) Draw the Lewis structure of methanol, CH3OH(8). (3) (ii) Show with a simple diagram how methanol dissolves in water. Explain. (2) (c) How does the energy and length of the carbon-oxygen bond in CH3OH(e) compare with the carbon-oxygen distance in carbon monoxide? Explain. (5) (d) Chemical bonds can be classified as polar covalent, according to and (3) (e) Chemical bonds can also be classified as single or number of according to the (2) (f) Draw the Lewis structure(s) for SO3F. Explain the structure which you have drawn. (6)