Essay, Pages 7 (1544 words)

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The wavelength of some green light is 530.0 nm. What is the frequency of this green light?

5.66 x 10^14 hz

Microwave radiation vs. UV radiation

Which has a longer wavelength?

Which has a greater frequency?

Which has greater energy?

Microwave

UV

UV

Microwave ovens emit microwave energy with a wavelength of 12.1 cm. What is the energy of exactly one photon of this microwave radiation?

1.66 x 10 ^-24 J

A certain shade of blue has frequency of 7.32 x 10^14 Hz. What is the energy of exactly one photon of this light?

4.85 x 10^-19

Light from hydrogen can be emitted at the wavelength of 486.0 nm. What is the energy of one photon of light?

4.09 x 10^-19

Calculate the energy for one mole of photons (an einstein) for light absorbed at 685 nm

1.75 x 10^5 J

Blue light vs. Red light

Which has longer wavelength?

Which has a greater frequency?

Which has the greater energy?

Red

Blue

Blue

Blue

Blue

Arrange from longest to shortest wavelength.

Green light, X ray photon, red photon, high frequency UV radiation, low frequency UV radiation

Red photon

Green light

low frequency UV radiation

high frequency UV radiation

x ray photon

Green light

low frequency UV radiation

high frequency UV radiation

x ray photon

Arrange the following from lowest to highest frequency.

infrared radiation, gamma ray radiation, short wavelength X-rays, blue light, long wavelength X-rays

infrared radiation

blue light

long wavelength X rays

short wavelength X rays

gamma ray radiation

blue light

long wavelength X rays

short wavelength X rays

gamma ray radiation

The existence of quantized energy levels in an atom can be inferred from…

atomic spectral lines

Will a jump from n=1 to n=3 be absorption or emission?

absorption

Would a jump from n=2 to n=1 be emission or absorption?

emission

Calculate the energy of a photon emitted when an electron in a hydrogen atom undergoes a transition from n=3 to n=1.

1.94 x 10^-18

What information is needed to determine the energy of an electron in a many-electron atom? Select all that apply.

l and n

What information is most important in determining the size of an orbital?

n

What information is needed to determine the orientation of an orbital?

Ml

What information is needed to determine the general shape of an orbital?

l

How many sub shells are in the n=5 shell?

5

How many orbitals are in the n=2 shell?

4

In the n=3 level…

How many sub levels?

How many orbitals?

How many electrons?

3

9

18

9

18

Which sub shell is designated by each set of quantum numbers?

1. n=2, l=1

2. n=5, l=4

3. n=4, l=0

4. n=3, l=1

1. 2p

2. 5g

3. 4s

4. 3p

2. 5g

3. 4s

4. 3p

How many electrons in an atom could have these sets of quantum numbers?

1. n=2

2.n=5, l=0

3. n=7, l=3, ml=-1

1. 8

2. 2

3. 2

2. 2

3. 2

If l=2, what can you deduce about n?

n is greater than 2

If ml = 4, what can you say about l?

l is greater than or equal to 4

What are the possible magnetic quantum numbers (m?) associated with each indicated value of ??

l = 2

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

Identify the generic outer electron configuration for the noble gases.

ns^2 np^6

What are the chemical symbols for the following electron configurations?

1. 1s2 2s2 2p3

2. 1s3 2s2 2p6 3s2 3p6 4s2 3d10 4p6

3. 1s2 2s2 2p6 3s2 3p6

4. 1s2 2s2 2p6 3s2 3p3

1. N

2. Kr

3. Ar

4. P

2. Kr

3. Ar

4. P

Determine the element of lowest atomic number that contains a complete d subshell in the ground state.

Cu

Which of the following experiments provided evidence that the electrons in atoms are arranged in distinct energy levels?

the observation of line spectra from gas discharge tubes

Assume n1 and n2 are two adjacent energy levels of an atom. The emission of radiation with the longest wavelength would occur for which two values of n1 and n2?

8,7

Use the Rydberg formula for atomic hydrogen to calculate the wavelength of the photon emitted in the transition of an electron from n=4 to n=2.

What is the name given to the spectroscope series to which the transition described in question 3 belongs?

In what region of light will the photons emitted in question 3 lie?

486 nm

Balmer series

visible blue light

The graph below shows the radial distribution plots for the 1s wavefunctions for H and He+. Which plot (A or B) is the 1s wavefunction for the He+ ion?

A

What is the maximum number of electrons that can have the quantum number n=2 in an atom?

8

The three quantum numbers for an electron in a hydrogen atom in a certain state are n=4, ℓ=2, and mℓ=1. The electron is located in what type of orbital?

4d

The number that describes the main energy level of an electron in an atom is…

the principal quantum number, n

Can an electron in an atom be in an energy level described by the set of quantum numbers n=5, ℓ=3, mℓ=-2?

yes

An electron in a 3d orbital could have which of the following quantum numbers?

n=3, l=2, ml=0

How many p electrons does Se (atomic number 34) possess?

16

For which H-atom wavefunction are you most likely to find the electron farthest from the nucleus?

4p

The transition metals are elements with partially filled…

d subshells

Which element is predicted to have the ground-state electron configuration shown below?

[Ne] 3s2 3p4

sulfur

Which of the following is the valence electronic structure for a halogen?

ns2 np5

In the Aufbau order of occupancy of electronic energy levels, the level occupied just after 5p is…

6s

The electron configuration for the Mn atom is…

1s2 2s2 2p6 3s2 3p6 4s2 3d5

The ground state electron configuration of a neutral silver atom is [Kr] 5s1 4d10 instead of [Kr] 5s2 4d9. This observation can be explained (theoretically) by the fact that…

an enhanced stability is associated with filled sets of equivalent orbitals

How many s electrons does P (atomic number 15) possess?

6

How many values of the quantum number ℓ are possible when n=5?

5

How many values of mℓ are allowed for an electron in a 5f subshell?

7

How many values of mℓ are allowed for an electron in a 2s subshell?

1

How many subshells are there in the shell with n=3?

3

What is the frequency of light with a wavelength of 4.0 x 10-7 m?

7.5 x 10^14

What is the correct order of increasing frequency?

UV radiation, visible light, radio waves, infrared radiation

radio waves, infrared radiation, visible light, UV radiation

Light with a frequency of 7.30 x 1014 Hz lies in the violet region of the visible spectrum. What is the wavelength of this frequency of light?

411 nm

When an electron beam strikes a block of copper, x-rays of frequency 1.97 x 1019 Hz are emitted. What is the wavelength of these x-rays?

15.2 pm

Wavelength is..

the distance between successive peaks in a wave

Frequency is…

the number of waves passing a fixed point in one second

It takes light with a wavelength of 212 nm to break the N‒H bond in ammonia. What energy is required per photon to break this bond? What is the N‒H bond strength in terms of kJ per mole?

9.4 x 10^-22 kJ/photon; 565 kJ/mol

In 1 sec, a 60 W bulb emits 11 J of energy in the form of infrared radiation (heat) of a corresponding wavelength of 1850 nm. How many photons of infrared radiation does the lamp generate in 1 sec?

1.02 x 10^20

A photon has a frequency of 223 MHz. What is the energy of this photon?

1.48 x .10^-25

Carbon emits photons at 745 nm when exposed to blackbody radiation. How much energy would be obtained if 44g of carbon were irradiated? Assume each carbon atom emits one photon.

5.9 x 10^5 J

A 200 nm photon has ______ times the energy of a 700 nm photon.

3.5

If a photon’s wavelength is 663 µm, what is its energy?

3.00 x 10^-22

Sodium vapor lamps, used for public lighting, emit yellow light of a wavelength of 570 nm. How much energy is emitted by an excited sodium atom when it generates a photon?

3.5 x 10^-19 J

Consider the sodium vapor lamps described in question 13. How much energy is emitted by 45.8 mg of sodium atoms emitting light at this wavelength? Assume each sodium atom emits one photon.

420 J

A particular metal has a work function of 1.05 eV. A light is shined onto this metal with a corresponding wavelength of 324 nm. What is the maximum velocity of the photoelectrons produced? (Hint: 1eV = 1.6022 x 10-19 J, mass of an electron = 9.11 x 10-31 kg)

9.89 x 10^5 m/s

A particular metal has a work function of 3.05 eV. A light is shined onto this metal with a corresponding wavelength of 524 nm. What is the maximum velocity of the photoelectrons produced? (Hint: 1eV = 1.6022 x 10-19 J, mass of an electron = 9.11 x 10-31 kg)

no photoelectrons are produced

Max Planck’s theory averted the so called “UV Catastrophe” of classical mechanics. Which of the following best describes how Planck’s theory avoided the “UV Catastrophe”?

radiation given off by blackbody radiators can only be emitted in quantized amounts

The de Broglie equation was important for a number of reasons, not least of which was that it demonstrated that _______.

all objects have a wavelength. however, in the case of macroscopic objects, these wavelengths are so small that they can be ignored

An atom of which element, moving at 240 m/s, would possess a de Broglie wavelength of 1.40 x 10‒11 m?

Sn

Which quantum number tells you orbital, subshell, and shell? What are each of these things?

n – shell

l – subshell

ml – orbital

l – subshell

ml – orbital

What does each quantum number tell you?

n – distance from the nucleus/energy level

l – shape

ml – orientation

ms – direction of spin

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