Chem Chapter 7

Select the acceptable sets of quantum numbers in an atom.

(4‚ 3‚ −2‚ +1/2) (3‚ 0‚ 0‚ +1/2)

The electron configurations described in this chapter all refer to gaseous atoms in their ground states. An atom may absorb a quantum of energy and promote one of its electrons to a higher-energy orbital. When this happens, we say that the atom is in an excited state. The electron configurations of some excited atoms are given. Select the configuration that would correspond to an excited state of As.

(d) [Ar]4s13d104p4

Select the quantum numbers associated with the 2p orbital. Possible magnetic quantum numbers (mell)

-1,0,1

Select the quantum numbers associated with the 5d orbital. Possible magnetic quantum numbers (mell)

-2,-1,0,1,2

Select the quantum numbers associated with the 3s orbital. Possible magnetic quantum numbers (mell)

0

Select the quantum numbers associated with the 3s orbital. Angular momentum quantum number(ell)

0

Select the quantum numbers associated with the 2p orbital. Angular momentum quantum number(ell)

1

Select the quantum numbers associated with the 2p orbital. Principal quantum number (n)

2

Select the quantum numbers associated with the 5d orbital. Angular momentum quantum number(ell)

2

Select the quantum numbers associated with the 3s orbital. Principal quantum number (n)

3

Photodissociation of water H2O(l) + hν → H2(g) + (1/2) O2(g)

418nm and no

Select the quantum numbers associated with the 5d orbital. Principal quantum number (n)

5

How many orbitals do the possible sub shells have? If a listed orbital is not possible, place a zero in the answer blank. when n= 6

6s=1 6p=3 6d=5 6f=7 6g=9 6h=11

Element X reacts with hydrogen gas at 200°C to form compound Y. When Y is heated to a higher temperature, it decomposes to the element X and hydrogen gas in the ratio of 559 mL of H2 (measured at standard temperature and pressure) for 1.00 g of X reacted. X also combines with chlorine to form a compound Z, which contains 63.89 percent by mass of chlorine. Deduce the identity of X.

Ca

Portions of orbital diagrams representing the ground-state electron configurations of certain elements are shown here: Which violate the Pauli exclusion principle?

a, f

An electron in a hydrogen atom is excited from the ground state to the n = 5 state. Decide if the following statements are true or false. (a) n = 5 is the first excited state. (b) It takes more energy to ionize (remove) the electron from n = 5 than from the ground state. (c) The electron is farther from the nucleus (on average) in n = 5 than in the ground state. (d) The wavelength of light emitted when the electron drops from n = 5 to n = 1 is longer than that from n = 5 to n = 2. (e) The wavelength the atom absorbs in going from n = 1 to n = 5 is the same as that emitted as it goes from n = 5 to n = 1.

a= false b=false c= true d-false e=true

Which orbital in each of the following pairs is lower in energy in a many-electron atom?

a=2s b=3s c=4s

Portions of orbital diagrams representing the ground-state electron configurations of certain elements are shown here: Which violate Hund's rule?

b,d,e

A photoelectric experiment was performed by separately shining a laser at 450 nm (blue light) and a laser at 560 nm (yellow light) on a clean metal surface and measuring the number and kinetic energy of the ejected electrons. (Assume that the same amount of energy is delivered to the metal surface by each laser and that the frequencies of the laser exceed the threshold frequency.) (b) Which light would eject electrons with greater kinetic energy?

blue

An electron in a certain atom is in the n = 2 quantum level. Select the possible values of l and ml that it can have. l= & ml=

l = 0, 1 ml= -1,0,1

An electron in an atom is in the n = 3 and ell = 1 quantum level l= ml=

l= -1, 0, 1 ml= 0, 1,2

Give all the possible values of the four quantum numbers of an electron in the following orbitals: (c) 3d n= l= ml= ms=

n=3 l=2 ml= -2,-1,0,1,2 ms=both

Give all the possible values of the four quantum numbers of an electron in the following orbitals: (a) 3s n= l= ml= ms=

n=3, l=0 ml=0 ms= both

Give all the possible values of the four quantum numbers of an electron in the following orbitals: (b) 4p n= l= ml= ms=

n=4, l=1, ml= -1,0,1 ms=both

A photoelectric experiment was performed by separately shining a laser at 450 nm (blue light) and a laser at 560 nm (yellow light) on a clean metal surface and measuring the number and kinetic energy of the ejected electrons. (Assume that the same amount of energy is delivered to the metal surface by each laser and that the frequencies of the laser exceed the threshold frequency.) (a) Which light would generate more electrons?

yellow