Ch.5 - Periodicity & Electronic Structure of Atoms
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Problem 1
Which wave corresponds to higher energy radiation? (LO 5.1) (a)
(b)
- What is the energy (in kJ) of one mole of photons of ultraviolet light with a wavelength of 85 nm? (LO 5.3) (a) 1.4 * 10-6 kJ (b) 1.4 * 103 kJ (c) 2.4 * 1014 kJ (d) 2.4 * 10-15 kJ
Problem 3
- Which type of electromagnetic radiation will cause the greatest number of electrons to be ejected from zinc metal with a work function of 350 kJ/mol? (LO 5.4, 5.5) (a) Dim light with a wavelength of 320 nm (b) Dim light with a wavelength of 360 nm (c) Bright light with a wavelength of 360 nm (d) Bright light with a wavelength of 375 nm
Problem 4
Problem 6
When a copper salt such as Cu(NO3)2 is burned in a flame, a blue-green color is emitted. Which figure represents the emission spectrum for the element copper? (LO 5.6)? (a)
(b)
(c)
(d)
- Which arrow in the energy diagram for an atom represents the absorption of light with the shortest wavelength? (LO 5.7)
Problem 7
- Calculate the wavelength in nm of the light emitted when an electron makes a transition from an orbital in n = 5 to an orbital in n = 2 in the hydrogen atom. (LO 5.8) (a) 2.31 * 10-3 nm (b) 4.34 * 10-2 nm (c) 231 nm (d) 434 nm
Problem 8
- What are the possible values of n, l, and ml for an electron in a 5p orbital? (LO 5.12)
Problem 10
- What are the possible values of n, l, and ml for the orbital shown? (LO 5.13)
Problem 11
Problem 26a
Two electromagnetic waves are represented below. (
(a) Which wave has the greater intensity?
Problem 26c
Two electromagnetic waves are represented below.
(c) Which wave represents yellow light, and which represents infrared radiation?
- Identify each of the following orbitals, and give n and l quantum numbers for each. (a)
Problem 28
(b)
- Where on the blank outline of the periodic table do elements that meet the following descriptions appear? (c) Elements with electrons whose largest principal quantum number is n = 4
Problem 29
