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Claudine Recena

Claudine R.

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Ronald Prasad verified

Numerade educator

13. An atom whose electronic configuration is 4p³ describes the electron of the atom having __________ a. n = 4 ? = 0 m? = -2 ms = +½ b. n = 4 ? = 1 m? = -1 ms = -½ c. n = 4 ? = 1 m? = +1 ms = -½ d. n = 4 ? = 1 m? = +1 ms = +½

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Ronald Prasad verified

Numerade educator

what electronic configuration is not possible?a.) 1s² 2s³ 2p³ b.) 1s² 2s² 2p³ c.)1s² 2s² 2p² d.) 1s² 2s²

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The maximum number of electons that can occupy a single orbital is?

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1. Which of the following statement about quantum theory is incorrect? a. When filling orbitals with the same \( n \) and \( \ell \) quantum numbers, two electrons will fill the same \( m_{\ell} \) before filling a new \( m_{\ell} \). b. Lower energy orbitals are filled-up with electrons first before the higher energy orbitals are filled-up. c. No two electrons in the same atom can have the same four quantum numbers. d. Electrons fill-up the orbitals according to increasing energies.

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Write the electronic configuration, distribution of electrons in the main energy level, last sublevel configurations, orbital diagram of LSC, quantum numbers, and magnetic property of the following elements. 84Po

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Write the electronic configuration, distribution of electrons in the main energy level, last sublevel configurations, orbital diagram of LSC, quantum numbers, and magnetic property of the following elements. 36Kr

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Write the electronic configuration, distribution of electrons in the main energy level, last sublevel configurations, orbital diagram of LSC, quantum numbers, and magnetic property of the following elements. 78Pt

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Write the electronic configuration, distribution of electons in the main energy level, last sublevel configurations orbital diagram of LSC, quantum numbers, and magnetic property of the following elements. 1. 20Ca

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D. Write the electronic configuration, distribution of electrons in the main energy level, last sublevel configurations, orbital diagram of LSC, quantum numbers, and magnetic property of the following elements. 1. \( { }_{20} \mathrm{Ca} \) 2. \( { }_{78} \mathrm{Pt} \) 3. \( { }_{17} \mathrm{Cl} \) 4. \( { }_{36} \mathrm{Kr} \) 5. \( { }_{84} \mathrm{Po} \)

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B. Wavelength In \( \mathrm{nm} \), calculate the wavelength of a photon emitted by \( \mathrm{H} \) atom when an electron drops from \( n_{1}=5 \) to the \( n_{f}=2 \). If the wavelength is in the visible region, what color can be observed (use the figure below to determine the color)? Visilble Region 303 anin \( 500 \mathrm{nnin} \) 600 nim 700 nin \( \quad 780 \mathrm{~nm} \)

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