THE BOHR ATOM

Question 1

Although the Bohr model is not completely accurate, it can be used to explain

Answer 1

absorption and emission

Question 2

Electrons move from low energy to higher energy orbits by

Answer 2

absorbing energy

Question 3

Electrons move from high energy to lower energy orbits by

Answer 3

emitting energy

Question 4

Electron energy is

Answer 4

quantized

Question 5

the higher the wavelength, the lower the energy

Answer 5

the higher the energy, the lower the wavelength

Question 6

n

Answer 6

principal quantum numbers

Question 7

describes the energy level on which the orbital residue
- numbers greater than 0

Answer 7

Quantum Numbers

Question 8

this quantum number defines the shape of the orbital
- allowed values of ranging 0 to n − 1

Answer 8

Azimuthal Quantum Number (l)

Question 9

describes the three-dimensional orientation of the orbital
- values of integers ranging from -l to l

Answer 9

Magnetic Quantum Number (ml)

Question 10

electrons in the same orbital do not have the same energy.
- upward or downward

Answer 10

Spin Quantum Number (ms)

Question 11

sphere around the nucleus

Answer 11

1s orbital

Question 12

the one that tells you that the electron is in the orbital closest to the nucleus

Answer 12

1s orbital

Question 13

similar to 1s except the electron is most likely in the region farther from the nucleus

Answer 13

2s orbital

Question 14

at the first energy level, there is only the 1s orbital, after the second energy level there are

Answer 14

2p orbitals

Question 15

look like dumbells

Answer 15

p orbitals

Question 16

distribution of all electrons in an atom

Answer 16

electron configurations

Question 17

4p^5

what is 5?

Answer 17

superscript denoting the number of electrons in those orbitals

Question 18

4p^5

what is p?

Answer 18

letter denoting the type of orbital

Question 19

4p^5

what is 4?

Answer 19

number denoting the energy level

Question 20

“For degenerate orbitals, the lowest energy is attained when the number of electrons with the same spin is maximized.”

Answer 20

Hund’s Rule

Question 21

Filling Rules of Electron Orbitals

Electrons are added one at a time to the lowest energy orbitals available until all the electrons of the atom have been accounted for.

Answer 21

Aufbau Principle

Question 22

Filling Rules for Electron Orbitals

An orbital can hold a maximum of two electrons, to occupy the same orbital, two electrons must spin in opposite directions

Answer 22

Pauli Exclusion Principle

Question 23

Filling Rules for Electron Orbitals

Electrons occupy equal-energy orbitals so that a maximum number of unpaired electrons results.

Answer 23

Hund’s Rule

Question 24

when n = 1?
what are the possible values of l, subshell designation, ml, numbers of orbitals in subshell, total numbers of orbitals?

Answer 24

l = 0
subshell designation = 1s
ml = 0
numbers of orbitals in shell = 1
total number of orbs = 1

Question 25

when n = 2? what are the possible values of l, subshell designation, ml, numbers of orbitals in subshell, total numbers of orbitals?

Answer 25

l = 0,1 subshell designation = 2s, 2p ml = 0 1, 0 , -1 numbers of orbitals in shell = 1, 3 total number of orbs = 4

Question 26

when n = 3? what are the possible values of l, subshell designation, ml, numbers of orbitals in subshell, total numbers of orbitals?

Answer 26

l = 0,1,2 subshell designation = 3s 3p 3d ml = 0 1, 0, -1 2, 1, 0, -1, -2 numbers of orbitals in shell = 1, 3, 5 total number of orbs = 9

Question 27

when n = 4? what are the possible values of l, subshell designation, ml, numbers of orbitals in subshell, total numbers of orbitals?

Answer 27

l = 0, 1, 2, 3 subshell designation = 4s 4p 4d 4f ml = 0 1, 0, -1 2, 1, 0, -1, -2 3, 2, 1, 0, -1, -2, -3 numbers of orbitals in shell = 1, 3, 5, 7 total number of orbs = 16

Question 28

It is the grouping of electrons that is not at the lowest possible energy state

Answer 28

Excited state

Question 29

It is the grouping of electrons that is at the lowest possible energy state

Answer 29

Ground state

Question 30

Atoms return to ground state by

Answer 30

emitting radiation

Question 31

To understand the electronic structure of atoms, one must understand the nature of

Answer 31

electromagnetic radiation

Question 32

The number of waves passing a given point per unit of time is the

Answer 32

frequency (v)

Question 33

For waves traveling at the same velocity, the _____the wavelength, the ______the frequency

Answer 33

longer , smaller

Question 34

in, E = hv, what is h?

Answer 34

Planck's constant (6.626 x 10 J*s)

Question 35

One does not observe a continuous spectrum, as one gets from a white light source.

Answer 35

Only a line spectrum of discrete wavelengths is observed.

Question 36

developed a mathematical treatment into which both the wave and particle nature of matter could be incorporated.

Answer 36

Erwin Schrödinger quantum mechanics

Question 37

is the amount of energy needed to move from one energy level to another

Answer 37

quantum

Question 38

The wave equation is designated with a

Answer 38

lower case Greek psi ()

Question 39

gives a probability density map of where an electron has a certain statistical likelihood of being at any given instant in time

Answer 39

square of the wave equation, 2

Question 40

* Describes the three-dimensional orientation of the orbital

Answer 40

Magnetic Quantum Number, ml

Question 41

Distribution of Electrons No two electrons in the same atom can have exactly the same energy

Answer 41

Pauli Exclusion Principle

Question 42

no two electrons in the same atom can have identical sets of .

Answer 42

quantum numbers

Question 43

Distribution of Electrons Electrons occupy the positions of the lowest energy

Answer 43

Aufbau Principle

Question 44

Distribution of Electrons Electrons in the same sublevel occupy empty orbitals rather than pair up

Answer 44

Hund’s Rule

Question 45

no two electrons in an atom have the same four quantum number’s

Answer 45

Pauli exclusion principle

Question 46

Electrons are added one at a time to the lowest energy orbitals available until all the electrons of the atom have been accounted for.

Answer 46

Aufbau Principle

Question 47

An orbital can hold a maximum of two electrons.To occupy the same orbital, two electrons must spin in opposite directions. Type of principle

Answer 47

Pauli Exclusion Principle

Question 48

Electrons occupy equal-energy orbitals so that a maximum number of unpaired electrons results.

Answer 48

Hund’s Rule

Question 49

Electrons behave as

Answer 49

particle and wave

Question 50

describes the probability of the location of the electrons

Answer 50

Shapes and Orientations of Orbitals

Question 51

are useful way of the describing the elements.

Answer 51

Electronic Configuration

Question 52

adopted Planck’s assumption and explained these phenomena in this way

Answer 52

Niels Bohr

Question 53

The Nature of Energy

Answer 53

1. Electrons in an atom can only occupy certain orbits 2. Electrons in permitted orbits have specific, “allowed” energies; these energies will not be radiated from the atom. 3. Energy is only absorbed or emitted in such a way as to move an electron from one “allowed” energy state to another; the energy is defined by E = hv

Question 54

RH is the

Answer 54

Rydberg constant, 2.18 x 10^−18 J

Question 55

posited that if light can have material properties, the matter should exhibit wave properties.

Answer 55

Louis de Broglie

Question 56

Louis de Broglie demonstrated that the relationship between mass and wavelength was

Answer 56

λ =h/mv

Question 57

Chromium can be detected in atomic absorption spectroscopy by monitoring the absorbance of UV light at a wavelength of 357.8 nm ➢ What is the energy of a photon of this light?

Question 58

replaced the Bohr model of the atom

Answer 58

Quantum mechanical model

Question 59

Quantum mechanical model depicts electrons as waves spread out or delocalized through a region of space called

Answer 59

orbital

Question 60

Wave behavior was described using a wave function, called as the

Answer 60

Schrödinger equation