Electronic Structure (PHY, GC)

Question 1

The electrons closer to the nucleus are at ___ energy levels, while those that are further out (in higher electron shells) have ____ energy.

Answer 1

lower, higher

Question 2

Valence electrons have the ___ interactions with the surrounding environment and the ____ interactions with the nucleus.

Answer 2

strongest, weakest

Question 3

Valence electrons are much more likely to become involved in bonds with other atoms because they experience the ___ electrostatic pull from their own ____.

Answer 3

least, nucleus

Question 4

A positively charged ion

Answer 4

cation

Question 5

A negatively charged ion

Answer 5

anion

Question 6

The atomic mass of an atom (in amu) is nearly equal to the _____, which is the sum of the protons and neutrons

Answer 6

mass number

Question 7

Atoms of the same element with varying mass numbers are called

Answer 7

isotopes

Question 8

Isotopes differ in their number of ___

Answer 8

neutrons

Question 9

Atomic weight

Answer 9

The weighted average of the different isotopes and is the number reported on the periodic table

Question 10

Avogadro’s number

Answer 10

6.02 x 10 ^ 23

Question 11

What does Avagadro’s Number represent?

Answer 11

The number of “things” (atoms, ions, molecules) in 1 mole

Question 12

As electrons go from a lower energy level to a higher energy level, they get AHED

Answer 12

A: absorb light
H: higher potential
E: excited
D: distant (from nucleus)

Question 13

When an electron returns to ground state,

Answer 13

it emits a photon with wavelength of energy it undergoes

Question 14

The electromagnetic energy of photons equation

Answer 14

E = hc/λ 
where 
h = Planck's constant
c = speed of light (3.0 x 10^8 m/s)
λ = wavelength of radiation

Question 15

The energy of the emitted photon corresponds to the difference in energy between the _____-energy ___ state and the ___-energy ___ state

Answer 15

higher-energy initial state, lower-energy final state

Question 16

a positive E corresponds to ___ and a negative E corresponds to ____

Answer 16

(+) E = emission

(-) E = absorption

Question 17

According to the Pauli Exclusion Principle,

Answer 17

no 2 electrons in a given atom can possess the same set of 4 quantum numbers

Question 18

Heisenberg Uncertainty Principle

Answer 18

It is impossible to simultaneously determine, with perfect accuracy, the momentum and the position of an electron

Question 19

The principle quantum number, n: the larger the integer value of n, the ____ the energy level and radius of the electron’s shell

Answer 19

higher

Question 20

Maximum number of electrons within a shell (equation)

Answer 20

2n^2

Question 21

The difference in energy between two shells ____ as the distance from the nucleus increases

Answer 21

decreases

Question 22

angular momentum, l

Answer 22

refers to the shape and number of subshells

value of l ranges from 0 to (n-1)

Question 23

l = 0 subshell is _
l = 1 subshell is _ 
l = 2 subshell is _
l = 3 subshell is _

Answer 23

s, p, d, f

Question 24

Maximum number of electrons within a subshell (equation)

Answer 24

4l +2

Question 25

magnetic quantum number, ml

Answer 25

specifies the particular orbital within a subshell where an electron is most likely to be found at a given moment in time.

Question 26

each orbital can hold a maximum of ___ electrons

Answer 26

two

Question 27

The possible values of ml are the integers between ___ and ___, including 0

Answer 27

-l and +l

Question 28

spin quantum number, ms

Answer 28

two spin orientations designated by +1/2 and -1/2

Question 29

Whenever two electrons are in the same orbital, they must have ____ spins

Answer 29

opposite

Question 30

Every element has a ____ atomic absorption and emission line spectrum

Answer 30

unique

Question 31

An _______ is the pattern of line formed when a light passes through a prism to separate it into the different frequencies of light it contains - each of these spectral lines corresponds to a different electron transition from a ___ energy state to a ___ energy state

Answer 31

atomic emission spectrum - higher, lower

Question 32

The n+l rule, used to rank subshells by ____ energy.

Answer 32

increasing This rule states that the lower the sum of the values of the first and second quantum numbers, n + l, the lower the energy of the subshell. --> if 2 subshells possess the same n+l value, the subshell with the lower n value has a lower energy and will fill with electrons first.

Question 33

The n+l rule in action, | Which will fill first, the 5d subshell or the 6s subshell?

Answer 33

The 6s will fill first 5d: n=5 + l=2 = 7 6s: n=6 + l=0 = 6

Question 34

The lowest s subshell is __, the lowest p subshell is __, the lowest d subshell is ___, and the lowest f subshell is ___

Answer 34

1s, 2p, 3d, 4f

Question 35

What is the electron configuration of osmium (Z = 76)? | *use noble gas abbreviation

Answer 35

[Xe]6s24f145d6

Question 36

What is the electron configuration of Fe3+?

Answer 36

[Ar]3d5

Question 37

Hund's rule tells us that ___ and ___ orbitals have ___ energies (___ stability) than other states

Answer 37

half-filled, fully filled, lower energies, higher stability

Question 38

Hund's rule creates 2 notable exceptions to electron configuration, chromium (and the other elements in its group) and copper (and the other elements in its group). What are the electron configurations of Chromium (Z=24) and Copper (Z=29)?

Answer 38

Chromium: [Ar]4s13d5 Copper: [Ar]4s13d10

Question 39

Paramagnetic of diamagnetic? Materials composed of atoms with unpaired electrons will orient their spins in alignment with a magnetic field, thus be weakly attracted to the magnetic field

Answer 39

paramagnetic --> mnemonic: PARAmagnetic means that a magnetic field with cause PARAllel spins in unpaired electrons and thus cause an attraction

Question 40

Paramagnetic or diamagnetic? | Materials consisting of atoms that have only paired electrons will be slightly repelled by a magnetic field

Answer 40

diamagnetic

Question 41

The ____ ____ of an atom are those electrons that are in its _____ energy shell, are ____ ____ removed, and are available for _____.

Answer 41

valence electrons, outermost, most easily, bonding

Question 42

All elements in period ____ (starting with ___) and below may accept electrons into their d subshell, which allows them to hold more than eight electrons in their valence shell --> this allows them to violate the ___ ____.

Answer 42

three, sodium, octet rule

Question 43

The ____ is the net positive charge experienced by an electron in a multi-electron atom.

Answer 43

effective nuclear charge (Zeff)

Question 44

The _____ describes the ___ in the attraction between an electron and the nucleus in any atom with more than 1 electron shell.

Answer 44

shielding effect, decrease

Question 45

The more electron shells there are, the __ the shielding effect experienced by the outermost electrons.

Answer 45

greater

Question 46

The effective nuclear charge on an electron is given by the following equation:

Answer 46

Zeff = Z-S Z is the number of protons in the nucleus (atomic #) S is the number of electron between the nucleus and the electron in question (the number of non-valence electrons)

Question 47

The shielding effect explains why ____ electrons are ______ removed from the atom

Answer 47

valence-shell, more easily

Question 48

When light strikes materials, it can ____ electrons from them. This is called the ____ _____.

Answer 48

eject. photoelectric effect

Question 49

In the photoelectric effect, electrons are ____ from matter as a consequence of their _____ from electromagnetic radiation of high frequency (_____ wavelength), such as UV radiation.

Answer 49

emitted, absorption of energy, short

Question 50

If the energy of the light is such that the electron is ___ above ____ associated with the atom, the electron can break free from the atom leading to ____ of the atom. These escaping electrons are called ___.

Answer 50

excited, energy levels, ionization, photons

Question 51

Energy of a photon equation:

Answer 51

E = hf h is Planck's constant f is the frequency of EM wave

Question 52

The energy required to knock off an electron is called the _____.

Answer 52

Ionization energy