Concept explainers
(a)
Interpretation:
The wavelength of an electron wave in its ground state and first excited state are to be calculated.
Concept introduction:
There are mainly two types of waves; travelling waves and standing waves. A travelling wave is a wave that propagates through space. For example,
(b)
Interpretation:
The number of nodes in first excited state of the given electron is to be calculated.
Concept introduction:
There are mainly two types of waves; travelling waves and standing waves. A travelling wave is a wave that propagates through space. For example, electromagnetic radiation. A standing wave originates in a place where physical boundary is present. For example, guitar string which has fixed ends.
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Principles of Modern Chemistry
- Schrodinger and de Broglie suggested a ‘Wave—particle duality" for small particles—that is, if electromagnetic radiation showed some particle-like properties, then perhaps small punicles might exhibit same wave-like properties. Explain. How does the wave mechanical picture of the atom fundamentally differ from the Bohr model? How do wave mechanical arbitals differ from Bohr’s orbits? What does it mean to say that an orbital represents a probability map for an electron?arrow_forward10. Consider two hydrogen atoms. The electron in the first one is in n=1 state, whereas in the second the electron is in the n=3 state. (a) which atom is in the ground state configuration? Why? (b) Which orbital has a larger radius? (c) Which electron is moving faster and why? (d) Which electron has a lower potential energy? (e) Which atom has higher ionization energy? Hint: assume that the radius of the n=3 orbital is =5 rBarrow_forward(1)Draw a ground state energy level diagram for a silicon atom that shows where all of the electrons would be (n, L, ml and show spin up or spin down with an arrow). (2) Determine the values of L and S for the ground state using Hund's rule. (3) For chlorine, repeat steps 1 and 2.arrow_forward
- do thisarrow_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(i) What do you understand by the dual nature of light? Explain clearly in few sentences. (ii)What is the difference between an emission and an absorption spectra? (iii) What is meant by Heisenberg uncertainty principle? Explain clearly in as simple a language as possible. (iv)What are the quantum numbers? How many are there ? What are their symbols and what do they signify? (v)What do you mean by periodic properties? What are the different trends seen in a periodic table and how can you explain them in at least two to three simple sentences for each of them?arrow_forward
- (a) What are the similarities of and differences between the1s and 2s orbitals of the hydrogen atom? (b) In what sensedoes a 2p orbital have directional character? Compare the“directional” characteristics of the px and dx2 - y2 orbitals.(That is, in what direction or region of space is the electrondensity concentrated?) (c) What can you say about the averagedistance from the nucleus of an electron in a 2s orbital ascompared with a 3s orbital? (d) For the hydrogen atom, listthe following orbitals in order of increasing energy (that is,most stable ones first): 4f, 6s, 3d, 1s, 2p.arrow_forwardA gold nucleus is located at the origin of coordinates, andan electron is brought to a position 2 Å from the origin inthe 1y direction.(a) Calculate the force on the gold nucleus exerted by theelectron giving its components Fx and Fy.(b) Calculate the potential energy of the gold nucleus andthe electron.arrow_forward(a) How does the Bohr model differ from the quantum mechanical model of the atom? Describe at least 2 differences.(b) Define each of the 4 quantum numbers (n, l, ml, ms) and what they physically represent about the orbital and/or electron.(d) How many quantum numbers are needed to completely define a specific orbital? Provide the quantum numbers for the 2s orbital.(d) How many quantum numbers are needed to completely define a specific electron? Provide the quantum numbers for the second electron to fill into a 2s orbital.arrow_forward
- It takes 163./kJmol to break an nitrogen-nitrogen single bond. Calculate the maximum wavelength of light for which an nitrogen-nitrogen single bond could be broken by absorbing a single photon. Be sure your answer has the correct number of significant digits.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_forwardIt takes 157./kJmol to break a nitrogen-oxygen single bond. Calculate the maximum wavelength of light for which a nitrogen-oxygen single bond could be broken by absorbing a single photon. Be sure your answer has the correct number of significant digits.arrow_forward
- Principles of Modern ChemistryChemistryISBN:9781305079113Author:David W. Oxtoby, H. Pat Gillis, Laurie J. ButlerPublisher:Cengage LearningIntroductory Chemistry: A FoundationChemistryISBN:9781337399425Author:Steven S. Zumdahl, Donald J. DeCostePublisher:Cengage Learning