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chemistry > chapter 5 > Flashcards

chapter 5 Flashcards

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1
Q

region of high probability of finding an electron

A

atomic orbital

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2
Q

each orbital has at most two electrons

A

Pauli exclusion principle

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3
Q

discrete bundle of electromagnetic energy

A

photon

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4
Q

energy needed to move an electron from one energy level to another

A

quantum

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5
Q

number of wave cycles passing a point per unit of time

A

frequency

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6
Q

distance between wave crests

A

wavelength

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7
Q

separation of light into different wavelengths

A

spectrum

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8
Q

In the Bohr model of the atom, an electron in an orbit has a fixed

A

energy

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9
Q

What is the maximum number of f orbitals in any single energy level in an atom?

A

7

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10
Q

sub-level

A

like theater seats arranged in sections: letters s, p, d, and f

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11
Q

What is the maximum number of d orbitals in a principal energy level?

A

5

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12
Q

What is the maximum number of orbitals in the p sublevel?

A

3

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13
Q

What is the maximum number of electrons in the second principal energy level?

A

8

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14
Q

When an electron moves from a lower to a higher energy level, the electron

A

absorbs a quantum of energy

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15
Q

The shape (not the size) of an electron cloud is determined by the electron’s

A

energy sublevel

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16
Q

If the spin of one electron in an orbital is clockwise, what is the spin of the other electron in that orbital?

A

counterclockwise

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17
Q

What is the next atomic orbital in the series 1s, 2s, 2p, 3s, 3p?

A

4s

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18
Q

According to the aufbau principle,

A

electrons enter orbitals of lowest energy first

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19
Q

What is the number of electrons in the outermost energy level of an oxygen atom?

A

6

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20
Q

If three electrons are available to fill three empty 2p atomic orbitals, how will the electrons be distributed in the three orbitals?

A

one electron in each orbital

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21
Q

How many unpaired electrons are in a sulfur atom (atomic number 16)?

A

2

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22
Q

How many half-filled orbitals are in a bromine atom?

A

1

23
Q

What is the basis for exceptions to the aufbau diagram?

A

Filled and half-filled energy sublevels are more stable than partially-filled energy sublevels.

24
Q

Which electron configuration of the 4f energy sublevel is the most stable?

A

4f14

25
Q

How does the speed of visible light compare with the speed of gamma rays, when both speeds are measured in a vacuum?

A

The speeds are the same

26
Q

Which color of visible light has the shortest wavelength?

A

violet

27
Q

How are the frequency and wavelength of light related?

A

They are inversely proportional to each other.

28
Q

Emission of light from an atom occurs when an electron

A

drops from a higher to a lower energy level

29
Q

As changes in energy levels of electrons increase, the frequencies of atomic line spectra they emit

A

increase

30
Q

Which of the following quantum leaps would be associated with the greatest energy of emitted light?

A

n = 5 to n = 1

31
Q

Which variable is directly proportional to frequency?

A

energy

32
Q

relation between wavelength, frequency, and energy

A

λ↑V↓E↓
λ↓V↑E↑

33
Q

The quantum mechanical model of the atom

A

involves the probability of finding an electron in a certain position

34
Q

Who predicted that all matter can behave as waves as well as particles?

A

Louis de Broglie

35
Q

According to the Heisenberg uncertainty principle, if the position of a moving particle is known, what other quantity CANNOT be known?

A

velocity

36
Q

How can the position of a particle be determined?

A

by analyzing its interactions with another particle

37
Q

The wavelike properties of electrons are useful in

A

magnifying objects

38
Q

In an s orbital, the probability of finding an electron a particular distance from the nucleus does NOT depend on

A

direction with respect to the nucleus

39
Q

What is the energy of a microwave photon that has a frequency of 1.12 10 Hz? (h = 6.63 10 Js)

A

.

40
Q

Explain why the 4s sublevel fills before the 3d sublevel begins to fill as electrons are added.

A

Electrons occupy orbitals in a definite sequence, filling orbitals with lower energies first. Generally, orbitals in a lower energy level have lower energies than those in a higher energy level. But, in the third level the energy ranges of the principal energy levels begin to overlap. As a result, the 4s sublevel is lower in energy than the 3d sublevel, so it fills first.

41
Q

Describe the different principles that govern the building of an electron configuration.

A

The aufbau principle states that electrons enter the orbitals of lowest energy first. The Pauli exclusion
principle states that each orbital can hold only two electrons. Hund’s rule states that electrons first enter separate orbitals of the same energy, with each electron having the same spin, before pairing with electrons that have opposite spins.

42
Q

What is the explanation for the discrete lines in atomic emission spectra?

A

Atoms absorb energy, causing electrons to be raised from one orbital to an orbital of higher energy. When these excited electrons fall back to lower energy levels, they emit light. The lines result from the fact that the electrons can move only between discrete energy levels. Emissions of specific frequencies of light correspond to these energy changes.

43
Q

Why are you unable to observe the wavelike motion of a soccer ball as it is kicked toward a goal?

A

The mass of an object must be very small in order to observe its wavelength. Classical mechanics describes the motions of objects much larger than atoms. The motion of objects with sizes in the atomic range and smaller are best described (and are detectable) as waves.

44
Q

What is the quantum mechanical model?

A

It is a model that describes subatomic particles and atoms as waves. Schrodinger applied a mathematical model of the wave/particle nature of matter to hydrogen. Solutions to the Schrodinger equation determine the energies an electron can have and how likely it is to find the electron in various locations.

45
Q

Explain what is meant by the Heisenberg uncertainty principle.

A

The measurement of the speed or position of a moving particle necessarily involves an interaction with the particle. Therefore, the position or the speed of the particle is changed as a result of the measurement. As a consequence, accurate measurements of both these variables cannot be made at the same time.

46
Q

Principal Quantum Number

A

(n) the energy level of the electron: 1, 2, 3, etc.

47
Q

Aufbau principle

A

electrons enter the lowest energy first

48
Q

Pauli Exclusion Principle

A
  • at most 2 electrons per orbital
  • different spins
49
Q

energy level

A

analogous to the rungs of a ladder
electrons cannot exist between levels

50
Q

first energy level

A

Has only s orbital
only 2 electrons

51
Q

second energy level

A

Has s and p orbitals available
2 in s, 6 in p

52
Q

third energy level

A

Has s, p, and d orbitals
2 in s, 6 in p, and 10 in d

53
Q

fourth energy level

A

Has s, p, d, and f orbitals
2 in s, 6 in p, 10 in d, and 14 in f

chemistry (6 decks)

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