chapter 5

Question 1

region of high probability of finding an electron

Answer 1

atomic orbital

Question 2

each orbital has at most two electrons

Answer 2

Pauli exclusion principle

Question 3

discrete bundle of electromagnetic energy

Answer 3

photon

Question 4

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

Answer 4

quantum

Question 5

number of wave cycles passing a point per unit of time

Answer 5

frequency

Question 6

distance between wave crests

Answer 6

wavelength

Question 7

separation of light into different wavelengths

Answer 7

spectrum

Question 8

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

Answer 8

energy

Question 9

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

Answer 9

7

Question 10

sub-level

Answer 10

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

Question 11

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

Answer 11

5

Question 12

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

Answer 12

3

Question 13

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

Answer 13

8

Question 14

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

Answer 14

absorbs a quantum of energy

Question 15

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

Answer 15

energy sublevel

Question 16

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

Answer 16

counterclockwise

Question 17

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

Answer 17

4s

Question 18

According to the aufbau principle,

Answer 18

electrons enter orbitals of lowest energy first

Question 19

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

Answer 19

6

Question 20

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

Answer 20

one electron in each orbital

Question 21

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

Answer 21

2

Question 22

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

Answer 22

1

Question 23

What is the basis for exceptions to the aufbau diagram?

Answer 23

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

Question 24

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

Answer 24

4f14

Question 25

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

Answer 25

The speeds are the same

Question 26

Which color of visible light has the shortest wavelength?

Answer 26

violet

Question 27

How are the frequency and wavelength of light related?

Answer 27

They are inversely proportional to each other.

Question 28

Emission of light from an atom occurs when an electron

Answer 28

drops from a higher to a lower energy level

Question 29

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

Answer 29

increase

Question 30

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

Answer 30

n = 5 to n = 1

Question 31

Which variable is directly proportional to frequency?

Answer 31

energy

Question 32

relation between wavelength, frequency, and energy

Answer 32

λ↑V↓E↓ λ↓V↑E↑

Question 33

The quantum mechanical model of the atom

Answer 33

involves the probability of finding an electron in a certain position

Question 34

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

Answer 34

Louis de Broglie

Question 35

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

Answer 35

velocity

Question 36

How can the position of a particle be determined?

Answer 36

by analyzing its interactions with another particle

Question 37

The wavelike properties of electrons are useful in

Answer 37

magnifying objects

Question 38

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

Answer 38

direction with respect to the nucleus

Question 39

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

Answer 39

.

Question 40

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

Answer 40

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.

Question 41

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

Answer 41

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.

Question 42

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

Answer 42

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.

Question 43

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

Answer 43

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.

Question 44

What is the quantum mechanical model?

Answer 44

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.

Question 45

Explain what is meant by the Heisenberg uncertainty principle.

Answer 45

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.

Question 46

Principal Quantum Number

Answer 46

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

Question 47

Aufbau principle

Answer 47

electrons enter the lowest energy first

Question 48

Pauli Exclusion Principle

Answer 48

- at most 2 electrons per orbital - different spins

Question 49

energy level

Answer 49

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

Question 50

first energy level

Answer 50

Has only s orbital only 2 electrons

Question 51

second energy level

Answer 51

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

Question 52

third energy level

Answer 52

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

Question 53

fourth energy level

Answer 53

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