09 CHAPTER: HW
Name an element in the fourth period of the periodic table with 5 valence electrons.
Arsenic
Select the element(s) that will have one unpaired electron in the p orbital.
B & Br
Arrange the colors of light in the visible spectrum in order of decreasing frequency. Highest to lowest frequency blue green orange red indigo violet yellow
Highest frequency→lowest frequency violet indigo blue green yellow orange red
What is the maximum number of electrons that can occupy the n=3 quantum shell?
18 electrons
How many valence electrons are in each of the following elements? Ba Al Be Se
2 3 2 6
Arrange the elements in decreasing order of the number of valence electrons.?
F = 7 valence electrons Ba = 2 valence electrons I = 7 valence electrons Ar = 8 valence electrons Cl = 7 valence electrons C = 4 valence electrons P = 5 valence electrons Be = 2 valence electrons B = 3 valence electrons Li = 1 valence electron K = 1 valence electron N = 5 valence electrons Ne = 8 valence electrons S = 6 valence electrons Mg = 2 valence electrons
Name an element in the fourth period of the periodic table with a complete outer shell
Krypton
Which electron is, on average, closer to the nucleus: an electron in a 2s orbital or an electron in a 3s orbital?
On average, the 2s electron is closer to the nucleus
Name an element in the fourth period of the periodic table with a total of 4 4p electrons.
Selenium
Match each emission wavelength of the Balmer series to the corresponding transition. 434nm 396nm 656nm 486nm 410nm
So here they are from the table in the link: n = 3 and the emission is 656 nanometers (Red Light) n = 4 and the emission is 486 nanometers (Blue Light) n = 5 and the emission is 434 nanometers (Violet Light) n = 6 and the emission is 410 nanometers (Violet Light) n = 7 and the emission is 397 nanometers (Violet Light verging on Near UltraViolet Light)
List the four possible sub shells in the quantum-mechanical model, the number of orbitals in each subshell, and the maximum number of elections that can be contained in each subshell
Subshells: S, P, D, F Orbitals. : 1, 3, 5, 7 Electrons: 2, 6, 10, 14
According to the quantum-mechanical model for the hydrogen atom, which of the following electron transitions would produce light with longer wavelength: 2p to 1s or 3p to 1s?
The 2p to 1s transition would produce light with longer wavelength
Two of the emission wavelengths in the hydrogen emission spectrum are 410 nm and 434 nm. One of these is due to the n=6 to n=2 transition, and the other is due to the n=5 to n=2 transition. Which wavelength goes with which transition?
The 410 nm wavelength corresponds to the n=6 to n=2 transition, the 434 nm wavelength corresponds to the n=5 to n=2 transition.
Which type of electromagnetic radiation has the shortest wavelength? a) radio waves b) microwaves c) infrared d)ultraviolet
Ultraviolet
Name an element in the fourth period of the periodic table with a total of 3 3d electrons.
Vanadium
1) Te 2) Br 3) I 4) Cs
[Kr]5s^24d^105p^4 [Ar]4s^23d^104p^5 [Kr]5s^24d^105p^5 [Xe]6s^1
Four of the wavelengths of the Balmer series occur in the visible spectrum (656 nm, 486 nm, 434 nm, and 410 nm). In which region of the electromagnetic spectrum does the fifth line, with a wavelength of 397 nm, occur? a) X rays b) gamma rays c) radio waves d) ultraviolet e) visible light f) infrared g) microwaves
d) ultraviolet
What is the relationship between the wavelength of light and the amount of energy carried by its photons?
inverse relationship
When an electron makes a transition from the n=4 to the n=2 hydrogen atom Bohr orbit, the energy difference between these two orbits (4.1×10−19J) is given off in a photon of light. The relationship between the energy of a photon and its wavelength is given by E=hc/λ , where E is the energy of the photon in J, h is Planck's constant (6.626×10−34J⋅s), and c is the speed of light (3.00×108m/s).
λ = 4.8×10−7 m