Interpretation: The energy of the 3s atomic orbital of an H atom is to be calculated and the energy of the hydrogen 3p atomic orbital the same as or different from that of the 3s orbital is to be explained.
Concept Introduction:
Atomic orbitals are regions of space around the nucleus of an atom where an electron is likely to be found and it describes the wave like behavior of one electron or pair of electron in an atom.
The most commonly filled orbitals are s, p, d, and f. Each such orbital can filled by a maximum of two electrons, each with opposite spin.
Each atomic orbital may be uniquely labelled by a set of four quantum numbers: n, l,
Want to see the full answer?
Check out a sample textbook solutionChapter 1 Solutions
Inorganic Chemistry
- 2. Consider a helium atom. (a) Sketch the system and write the Hamiltonian. Denote the term(s) in the operator that make(s) the Schrödinger equation unsolvable. (b) Given an excited-state configuration 1s 2s', express all possible excited-state wavefunctions in terms of spatial and spin functions for the two electrons. For each, denote the symmetry of the overall wavefunction, the spatial component, and the spin component with respect to exchange.arrow_forwardState the orbital degeneracy of the levels in a hydrogenic atom (Z in parentheses) that have energy (i) −4hcR᷉N, (2); (ii) −1/4hcR᷉N (4), and (iii) −hcR᷉N (5).arrow_forward(a) The nitrogen atom has one electron in each of the 2px,2py and 2pz orbitals. By using the form of the angularwave functions, show that the total electron density,c2(2px) +c2(2py) +c2(2pz), is spherically symmetric(that is, it is independent of the angles u and f). Theneon atom, which has two electrons in each 2porbital, is also spherically symmetric.(b) The same result as in part (a) applies to d orbitals,thus a filled or half-filled subshell of d orbitals isspherically symmetric. Identify the spherically symmetric atoms or ions among the following: F=, Na, Si,S2-, Ar+, Ni, Cu, Mo, Rh, Sb, W, Au.arrow_forward
- State the orbital degeneracy of the levels in a hydrogen atom that have energy (i) −hcR᷉H; (ii) − 1/9hcR᷉H; (iii) − 1/25hcR᷉H.arrow_forward(a) Look very carefully at the pictures below: Picture 1 and Picture 2. What does each of the pictures represent? Give FULL EXPLANATIONS for your answer. (1) (2) (b) Look very carefully at the picture below. Give the relevant quantum numbers. Explain your answer. у-аxis (c) (i) What is a wavefunction? (ii) What are the two parts of a wavefunction? (iii) What is the importance of squaring a wavefunction? (iv) Where is a wavefunction obtained from?arrow_forward5. (a) Use the hydrogen-like model z2 (in eV) En --13.6 to calculate the total energy of the three electrons of lithium (Li), which has the electron configuration: 1s? 2s'. The three ionization energies for Li(g) are: IE, = 5.392 ev; IE2 = 75.64 eV; IE = 122.5 ev. With the help of Koopman's theorem, what is the total energy of ropulsion between lithium's three electrons (in kJ mol')?arrow_forward
- 7. State the orbital degeneracy of the levels in the hydrogen atom that have the following energies: (i) (ii) (iii) -hcRH -hcRH -hcRHarrow_forwardConsider an electron in the N shell. (a) What is the smallest orbital angular momentum it could have? (b) What is the largest orbital angular momentum it could have? Express your answers in terms of h and in SI units. (c) What is the largest orbital momentum this electron could have in any chosen direction? Express your answers in terms of h and in SI units. (d) What is the largest spin angular momentum this electron could have in any chosen direction? Express your answers in terms of h and in SI units. (e) For the electron in part (c), what is the ratio of its spin angular momentum in the z-direction to its orbital angular momentum in the z direction? E and d no answerarrow_forwardTrue or false? The 4d orbital does not exist in the carbon atom. Justify your answer in 1 sentence or 2.arrow_forward
- (1) (2) (b) Look very carefully at the picture below. Give the relevant quantum numbers. Explain your answer. y-axis (c) (1) What is a wavefunction? (ii) What are the two parts of a wavefunction?arrow_forwardQ.1(a) What were the important advance (s) as a result of which, idea of an electron orbitmovement was swapped by, the notion of probability of finding electron in an orbital?What name was given to the transformed atomic model? Also explain its variouspostulates.(b) Which quantum numbers revel information about the shape, energy, orientation, andsize of the orbitals? How many orbitals are possible for n=4? Which of these may bedescribed as gerade?(c) The signs of the unsquared wave functions are usually shown in plots of the squaredfunctions. Why do you think this practice exists? Give values of angular nodes andplane of 3p, 4d, 2p, 4f, 4s.(d) Predict the trend in values of slater’s constant of the every first element of each groupof p-block elements.arrow_forward2.) Neglecting electron-electron repulsion, write down the singlet and triplet excited states of with the electron configuration, 1s^ 1 2s^ 1 . Make sure the wave function including spin and space parts) is antisymmetric under the interchange of the two electrons. What are the energies of the singlet and triplet states? What are the term symbols for the singlet and triplet states?arrow_forward
- ChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage LearningChemistryChemistryISBN:9781259911156Author:Raymond Chang Dr., Jason Overby ProfessorPublisher:McGraw-Hill EducationPrinciples of Instrumental AnalysisChemistryISBN:9781305577213Author:Douglas A. Skoog, F. James Holler, Stanley R. CrouchPublisher:Cengage Learning
- Organic ChemistryChemistryISBN:9780078021558Author:Janice Gorzynski Smith Dr.Publisher:McGraw-Hill EducationChemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage LearningElementary Principles of Chemical Processes, Bind...ChemistryISBN:9781118431221Author:Richard M. Felder, Ronald W. Rousseau, Lisa G. BullardPublisher:WILEY