Chapter 7 Homework Flashcards Preview

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Flashcards in Chapter 7 Homework Deck (20)
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1
Q

An incandescent light bulb gives off much more heat than a fluorescent light bulb, but appears dimmer than the fluorescent light bulb. Based on this information, what can you conclude about the fluorescent light bulb?

A

It emits less infrared light than the incandescent bulb.

2
Q

A radio wave has a period of 4.76 × 10^−7 s. What is its wavelength?

A

143 m

3
Q

A solution absorbs light with frequencies between 6.17 × 10^14 s−1 to 5.98 × 10^14 s−1. What can you conclude about the solution based on this information and the following table?

A

The solution absorbs blue-green light.

4
Q

Suppose you are in a room in which the only light source emits wavelengths of green light and no other colors. What color will an apple that appears red in white light will appear in this room?

A

black

5
Q

An aqueous solution is used in an absorption experiment. 1 mL of the solution absorbs 50% of the red light shined through it. How will this percentage be affected if enough water is added to reduce the concentration of the solution by half?

A

1 mL of the diluted solution will absorb less than 50% of the red light shined through it, but greater than 0%.

6
Q

What process at the atomic level is responsible for the production of incandescent light from a hot metal?

A

Vibrating nuclei within the atom create electromagnetic radiation.

7
Q

What wavelength of light will be emitted from a hydrogen atom when its electron drops from an energy level of n = 4 to an energy level of n = 3?

A

1.88 × 10^−6 m

8
Q

A beam of neutrons is used in an experiment. If the minimum error in knowing the position of the neutrons is 1.1 × 10−12 m, what is the minimum error in knowing the momentum of the neutrons?

A

4.8 × 10^−23 kg • m / s

9
Q

Which experimental observation below cannot be predicted by the Bohr model of the hydrogen atom?

A

The exact frequency at which light is emitted by the Li atom.

10
Q

What is the wavelength of an electron with a velocity of 6.7 × 10^7 m / s?
(The mass of an electron is 9.109 × 10^−31 kg.)

A

1.1 × 10^−11 m

11
Q

How would a 2s orbital most likely be affected if the angular part of its wave function were to change?

A

The orbital would probably no longer be spherical.

12
Q

Which of the following symbols represents the probability of finding the electron?

A

Ψ^2

13
Q

What does the angular solution to the Schrodinger equation disclose?

A

The shape of electron orbitals.

14
Q

What must occur for an electron to move from a 2s orbital to a 3s orbital?

A

It must absorb a photon.

15
Q

What is the physical meaning of the square of the wave function, ψ^2?

A

The square of the wave function is related to the probability of finding a particle at a certain point in space.

16
Q

Which of the following diagrams is a plot of the 2p orbitals?

A

This drawing represents the p orbitals.

17
Q

Which of the following best defines ionization energy?

A

Ionization energy is the energy required to remove an electron from an atom

18
Q

Determine the wavelength of light having energy of 2.25 × 10^−19 J.

A

8.83 × 10^−7 m

19
Q

What frequency of light would cause the electron of a Li 2+ ion to be ejected from the 1s orbital? The energy needed to remove this electron is 1.96 × 10^−17 J.

A

2.96 × 10^16 s−1

20
Q

Why doesn’t Schrödinger’s equation for the hydrogen atom work for the lithium atom?

A

Schrödinger’s equation for the hydrogen atom only works for single electron species. It does not take into account the interaction between the electrons in multi-electron species.

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