Calculate the energy associated with one mole of radiation of wavelength 560 mm.

Question

Calculate the energy associated with one mole of radiation of wavelength 560 mm. How many electrons in an atom can have the following quantum numbers? (a) n = 3, t = 2 (b) n = 4, t = 1, m_t = 0 Is the following combination allowed? If not, show one way to correct it. 9a n = 3, t = 1, m_t = 2 (b) n = 2, t = 0, m_t = -1. Write a full set of quantum numbers for the outermost electron in a sodium atom. (a) Draw the Lewis structures for the carbonate ion. (b)What is the bond angle and what is the shape of the carbonate ion? What is the formal charge on the S in the sulfur dioxide molecule? Is the sulfur dioxide molecule polar or nonpolar?

Explanation / Answer

(1)

wave length = 560 nm = 560 * 10-9 m

Formula, E = n h c / wave length

E = 6.02*1023*6.*10-34*3.00*108/(560*10-9)

E = 1.94 * 105 J/mol

(2)

n = 3, l= 2 => 3d subshell, so no.of electrons = 10 e (because d has five orbitals, 2 * 5 = 10)

n = 4, l = 1, ml = 0 => 4py orbital, so number of electrons = 2

(3)

n = 3, l = 1, ml = 2 is not allowed combination. Because for a given 'l' value, 'ml' has the values from +l to -l only. So, for l = 1 , ml has the values +1, 0 , -1 only.

n = 2, l= 0 , ml = -1 is not allowed combination. Because for a given 'l' value, 'ml' has the values from +l to -l only. So, for l = 0 , ml has the values 0 only.

(4)

Na(Z=11) outermost electronic configuration is 3s1

Quantum numbers: n = 3, l = 0, ml = 0, s = +1/2

(5)

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