Atomic Structure

Question 1

Name the group of elements highlighted below

Answer 1

Alkali Metals

Question 2

Name the group of elements highlighted below

Answer 2

Noble Gases

Question 3

Name the group of elements highlighted below

Answer 3

Halogens

Question 4

Name the group of elements highlighted below

Answer 4

Alkaline Earth Metals

Question 5

Name the group of elements highlighted below

Answer 5

Lanthanides

Question 6

Which orbital is shown below?

Answer 6

d_xy orbital

Question 7

Which orbital is shown below?

Answer 7

d_xz orbital

Question 8

Which orbital is shown below?

Answer 8

d_yz orbital

Question 9

Which orbital is shown below?

Answer 9

d_x²-_y² orbital

Question 10

Predicting Oxidation State from Bond lengths

As a general rule, the size of an ion will decrease by____Å by going from high spin to low spin.

Answer 10

>0.09 Å

Question 11

Predicting Oxidation State from Bond Lengths

As a general rule, the size of an ion will decrease by ______ Å per increase in positive charge

(Important: Spin state change leads to deviations from this rule of thumb.)

Answer 11

0.03-0.07 Å

Question 12

The size of an ion of the same charge will increase by_____ Å per increase in bound ligand.

Answer 12

0.05-0.1 Å

Question 13

Periodic Table Trends

Electron Affinity

Answer 13

Up a group: Increases

Left to Right Row: Increases

Question 14

Periodic Table Trends

Ionization Energy

Answer 14

Up a group: Increases

Left to Right Row: Increases

Question 15

Particles in nucleus

Answer 15

Protons and Neutrons

Question 16

Important Subatomic Particles for Chemists.

Particles in an atom

Answer 16

Proton, neutron, electron

Question 17

Electronegativity

Answer 17

The power of an atom in a molecule to attract

electrons to itself.

Question 18

Electronegativity

“Mulliken’s Definition”

Answer 18

χ=1/2(IE+EA)

Casted in terms of average of the Ionization Energy (IE) and Electron Affinity (EA)

Question 19

The sign of the wavefunction as an electronwave goes through a nodal plane

Answer 19

Changes Sign

Question 20

Hund’s Rule

Answer 20

The state of the highest spin multiplicty is lowest in energy

Question 21

The magnetic quantum number symbol is given by____.

Answer 21

m_l

Question 22

This quantum number can take on the following values:

x > 0, where x is an integer

Answer 22

n

Question 23

This quantum number can take on the following values:

-l ≤ __≤ l

Answer 23

m_l

Question 24

This quantum number can take on the following values:

0 ≤ __≤n-1

Answer 24

ℓ

Question 25

This quantum number can take on the following values:

±½​

Answer 25

m_s

Question 26

The angular quantum number symbol is given by____.

Answer 26

ℓ

Question 27

The spin quantum number symbol is given by____.

Answer 27

m_s

Question 28

The principal quantum number symbol is given by____.

Answer 28

n

Question 29

“Periodic Table Trends”

e^- + M —> M^-

Answer 29

Electron Affinity

Question 30

Name the group of elements highlighted below

Answer 30

Transition metals

Question 31

It contains 2 protons and 2 neutrons

Answer 31

An α-particle ​

Question 32

Parts of a Wavefunction

Characterizes the number of angular nodes and shape of an atomic orbital.

Answer 32

Angular Wavefunction

Question 33

Parts of the Wavefunction

Characterizes the number of radial nodes and the size of an atomic orbital.

Answer 33

Radial Wavefunction

Question 34

This experiment reveled that every atom has a nucleus composed of positive charge(s) and that it is where most of the atom’s mass is concentrated.

Answer 34

Rutherford Gold foil experiment

Question 35

Same number of protons, different number of neutrons

Answer 35

Isotope​

Question 36

Number of angular nodes for d orbitals

Answer 36

2

Question 37

Number of angular nodes for p orbitals

Answer 37

1

Question 38

Number of angular nodes for s orbital

Answer 38

0

Question 39

Heisenberg Uncertainty Principle

Answer 39

Δx Δp > h/4π​

Question 40

Einstein Energy

Relationship

Answer 40

E = mc²

Question 41

Wave Particle Duality

(De Broglie)

Answer 41

λ=h/(mv)

Question 42

Pauli Exclusion Principle

Answer 42

No two electrons can simultaneously occupy the same quantum state (quantum number)

Question 43

Based on the electronegative values (Hoffmann et al) of the nitrogen and hydrogen atom, what is the best description of hydrogen in Borane (BH₃)?

B - 11.4 eV e^−1​

H - 13.6 eV e^−1​

Answer 43

It has H- character

Question 44

Based on the electronegative values (Hoffmann et al) of the nitrogen and hydrogen atom, what is the best description of hydrogen in ammonia (NH₃)?

N - 16.9 eV e^−1​

H - 13.6 eV e^−1​

Answer 44

It has H+ character

Question 45

Based on the electronegative values (Hoffmann et al) of the carbon and hydrogen atom, what is the best description of hydrogen in methane (CH₃)?

C - 13.9 eV e^−1​

H - 13.6 eV e^−1​​

Answer 45

It has H^.character

Question 46

Electronegativity

“Pauling’s Definition “

Answer 46

Casted in terms of bond energies

A_2(g) + B_2(g) –> 2AB_(g)

ΔE(AB)=E(AB)_exp – ½[E(AA)+E(BB)]

|χ_A – χ_B|=bond polarity=0.208√(ΔE(AB)

Question 47

Slater’s Rules

“If calculating for d or f orbital electrons”

All electrons to the left shield

Answer 47

1.0 per electron

Question 48

Slater’s Rules

“For an ns or np electron”

All electrons n-1

Answer 48

0.85 per electron

Question 49

Slater’s Rules

“For an ns or np electron”

All electrons less than or equal to n-2

Answer 49

1.0 per electron

Question 50

Slater’s Rules

Electrons in the same “group”

Answer 50

0.35 per electron