Inorganic Chemistry Cumulative

To study for the inorganic chemistry extra credit quiz and final

Who discovered spectroscopy with Hydrogen?

Swedish physicist and astrologer Angers Angstrom

Who discovered the mathematical equation to accurately predict the wavelength of visible lines in hydrogen’s spectrum?

Johann Balmer and Johannes Rydberg

In excited states, electron is (__) from the positive nucleus, and it is (__) in energy

Further from the positive nucleus and higher in energy

In ground state, the electron is (__) to the positive nucleus and is (__) in energy

Closest to the positive nucleus and lowest in energy

The Bohr model of hydrogen says what?

The Bohr model says that electrons are held in orbit around the nucleus by a balance of electrostatic attraction and centripetal force. Each energy level (n) refers to an allowed orbit

What is the main problem with the Bohr model?

If it were true, as electrons lost energy they would move more slowly and collapse into the electrostatic pull of the nucleus. All atoms with orbiting electrons would collapse within picoseconds.

Electrons show (__), a wave property

diffraction

What did de Broglie propose?

He proposed wave-particle duality for electrons

What does Heisenberg’s uncertainty principle apply to?

It applies to all wave-like systems

Quantum mechanics says that electrons exist in (___) described entirely by a (__)

Quantum mechanics says that electrons exist in orbitals described entirely by a wavefunction

How is the wave function for a certain energy level in hydrogen determined?

By solving the Schrödinger Equation
A wavefunction is a solution if it returns itself multiplied by an energy value when the Hamiltonian operator is conducted on the function

The square of the wave function amplitude at certain coordinates gives the (__________)

The square of the wave function amplitude at certain coordinates gives the probability of finding the electron at that position.

Valid wavefunctions must have what five things

Ψ is single-valued for a certain combo of coordinates
Ψ must be continuous
Ψ must approach 0 as r (distance from the nucleus) approaches infinity

∫Ψ² (over all space) = 1

• 100% probability of finding it in space somewhere

∫Ψ_aΨ_b (over all space) = 0

• orthogonal

Each wavefunction can be broken down into what two components?

Radial and angular components

Each wavefunction has (__) quantum numbers

Each wavefunction has three quantum numbers

n is the (____) quantum number and it means (___) and has (___) as possible values

n is the principal quantum number, defines the energy level, and has 1-infinity possible values

L is the (___) quantum number, with (____) as possible values, and it means (____)

L is the angular momentum with possible values being 0-(n-1). It gives us the orbital shape in space and is equal to the number of angular/planar nodes.
l=0 is s
l=1 is p
l=2 is d

m_L is the (___) quantum number, with (___) as possible values, and it means (___).

m_L is the magnetic quantum number with +L thru -L as possible values. It indicates the orientation of the orbital in space, which effects the magnetism of the electrons.

Total m_L values = total orbitals of the same shape

What are the n and L quantum numbers for a 4d orbital?

n=4
L=2

What are the possible m_L values for a 4d orbital? What does each value represent and what does the number of total possible values mean?

m_L = -2, -1, 0, 1, 2
They represent the different directions those orbitals could be pointing.

Name the orbital (z-axis is up, x is out of the page and y is into the page)

S orbital

Name the orbital (z-axis is up, x is out of the page and y is into the page)

p_x orbital

Name the orbital (z-axis is up, x is out of the page and y is into the page)

p_y orbital

Name the orbital (z-axis is up, x is out of the page and y is into the page)

p_z orbital

Name the orbital (z-axis is up, x is out of the page and y is into the page)

d_xy orbital

Name the orbital (z-axis is up, x is out of the page and y is into the page)

d_xz orbital

Name the orbital (z-axis is up, x is out of the page and y is into the page)

d_yz orbital

Name the orbital (z-axis is up, x is out of the page and y is into the page)

d_x²-y² orbital

Name the orbital (z-axis is up, x is out of the page and y is into the page)

d_z² orbital

The radial part of the wavefunction holds into on changes with (___)

distance from the nucleus

Radial probability function =

probability of finding an electron at r in a shell at all angles

For a 3s orbital, n = …

n=3

a₀ is the ___

Bohr radius

Z is the …

nuclear charge

The Aufbau principle says…

electrons fill the lowest energy orbitals first

Pauli’s exclusion principle says…

Electrons in the same orbital have opposite spin quantum numbers (+1/2 -1/2) so that no two electrons have identical sets of quantum numbers

Hund’s Rule says…

When filling degenerate orbitals (i.e. same energy), electrons fill any empty orbital before pairing

Electrons in degenerate half-filled orbitals have the have “unpaired” spin which…

maximizes exchange energy

In neutral atoms, one “s” electron can move to the (_____) “d” orbitals if a half filled or completely filled d shell would result

higher

Why is 3d higher than 4s?

3d electrons have a higher Z_eff but feel higher repulsion than 4s electrons

• 3d orbitals put electrons in the same region as 3s, 3p, and even 2p orbitals. Due to high repulsion, 3d fills after 4s in neutral atoms

When a half filled shell is possible, (______) is maximized so a half filled 3d shell becomes more favorable than filling 4s first

exchange energy

On the periodic table, rows are called

periods

On the periodic table, columns are called

groups

Metals easily form…

cations

Transition metals form…

cations

Transition metals are all what state of matter at room temp

All solid except Hg

Effective Nuclear Charge (Z_eff) is…

The net attraction an electron actually feels from the nucleous after repulsions from other electrons are considered

Z_eff = (_______)

Z_eff = Z - S

Z_eff increases from (_____) on the periodic table

left to right

Metallic radius is defined as ___

half the distance between the centers of neighboring atoms in a pure metal solid

Non-polar covalent radius method is defined as ___

Atomic radius is half of the bond length for two identical atoms in a non-polar covalent molecule

Atomic radius _____ from left to right

decreases

Atomic radius _____ from top to bottom

increases

Atomic radius initially _____ from left to right

increases

For late transition metals, radius ______ down a group after period 5 due to _______

does not increase
lanthanide contraction

Cations are ____ than their neutral atoms because _____

cations are smaller than their neutral atoms because electrons have been lost

Anions are ____ than their neutral atoms because _____

Anions are larger than their neutral atoms because electrons have been added

Ionization energy _____ up a group

increases

Ionization energy ____ from left to right

increases

Electron affinity is defined as …

The energy required to remove an electron from the gaseous anion (-1 charge) of an element

Electron affinity _____ from left to right

increases

Electron affinity _____ from top to bottom

decreases

Electronegativity is defined as…

The ability of an atom to attract electron density

Name how the following periodic trends align with the periodic table:
Atomic radius
Electronegativity
Electron affinity
Ionization energy
Metallic character
Nonmetallic character

Bonds form to achieved what

Bonds form to achieve favored full shell electron configurations

In ionic bonds, electrons are …

fully transferred from one atom to another

In ionic bonds, resulting ions are held together by …

electrostatic attraction between opposite charges

Ionic bonding occurs between a ____ and a ____

metal and a nonmetal

The overall charge on a salt is ___

neutral

Salts exist as extended lattice of …

repeating pairings of ions

What is the simplest repeating structure within a lattice?

The unit cell

Unit cells with atoms at their corners are called ____

primitive

What lattices are common unit cells for salts?

The 7 primitive Bravais lattices

Covalent bonding occurs between ____ and _____

nonmetals and nonmetals/metalloids

What is a formal charge?

A formal charge is the difference between a neutral atom’s valence electron count and the number of electrons assigned to the atom in a structure.
Formal charge = Neutral atom valence electrons - lewis dot electrons

How do you calculate bond order?

number of bonds / number of bonding pairs in resonance

Correct this Gen. Chem half truth: Boron can fall short of the octet in Lewis structures

Structures where boron does not have an octet are so unstable that they will react with anything having lone pairs or will dimerize.

This electron geometry is…

Linear

This electron geometry is…

Trigonal Planar

This electron geometry is…

Tetrahedral

This electron geometry is…

Trigonal Bipyramidal

This electron geometry is…

Octahedral

The seesaw molecular geometry involves…

4 atoms and 1 lone pair

The square pyramidal molecular geometry involves…

5 atoms and 1 lone pair

Trigonal planar angle:

120

Tetrahedral angle:

109.5

Trigonal bipyramidal angle:

120 and 90

Molecular geometry can be used to determine…

polarity

Polarity determines…

Solubility
like dissolves like

Polar substances experience ____ intermolecular forces

stronger

The ratio of ions contained in one unit cell must match the ratio in ____

the salt’s formula

In order for MOs to form, what four things must occur?

1. Atoms must approach closely

2. Atomic orbitals (AOs) must have correct symmetry to overlap

3. AOs must be similar in energy

   1. AOs with an energy difference larger than 14eV cannot interact

4. Orbitals must be conserved so #AOs combined = #MOs formed

For naming MOs, orbitals representing head-on overlap along the bonding axis connecting 2 nuclei = ___

sigma

For naming MOs, subscript g means …

gerade, and it indicated that the MO is symmetry to inversion through a central point

Paramagnetic means ___ and occurs when ___

attraction to a magnetic field, occurs with unpaired electrons

Diamagnetic means ___ and occurs when ___

little response to magnetic field, occurs when electrons are paired

Photoelectron spectroscopy (PES) relies on what

the photoelectric effect

A symmetry operation is defined as…

action like rotation or reflection which can be conducted without changing the object’s original appearance (due to balance in the object)

A symmetry element is defined as…

physical marker like an axis or mirror plane around which a symmetry operation is conducted

C_n stands for ____ where n represents ____

The proper rotation symmetry operation, where n represents the number of times you divide 360 degrees by to acquire the angle at which you can rotate the molecule and still achieve symmetry to the original form.