Inorganic Exam 1

What is the Pauli Exclusion Principle?

No two electrons can have identical quantum numbers

Why did the discovery of Argon pose a problem for Mendeleev's periodic table?

Noble gases didn't exist so it didn't fit into a group. Also, because Mendeleev's table was based on measured atomic mass, argon (39.9) should have been placed between potassium (39.1) and calcium (40.1).

Define polar covalent

Two atoms with a large difference in electronegativity

What are the only two radioactive elements to exist in significant quantities on earth?

Uranium and thorium

BP = 2, LP = 1

V

BP = 2, LP = 2

V

Potential units

V (joules/coloumb)

scan rate

V/s

IMF's/Solubility of small covalent molecules

Weak IMF's, soluble is many solvents but not water

Why is iron the highest number formed in stellar processes?

With nuclei up to 26 protons, nuclear fusion is an exothermic process and is thus favored. Beyond this point, fusion is endothermic and requires the energy from a supernova explosion to happen.

Why is the radius of Germanium almost the same as silicon?

With the poorly shielding 3d orbitals having been filled corresponding to the added protons, the effective nuclear charge on the outer (4p) electrons will be increased; hence the covalent radius will decrease.

Zeff formula

Z - σ

_____ is a measure of how much of the positive charge of the nucleus is felt by each e⁻

Zeff

How to find Q

[products] / [reactants]

Weak metal characteristics

a little less metallic?

Bronsted-lowry base definition

accepts H+

Lewis Acid definition

accepts electrons

Examples of Polar Aprotic Solvents

acetonitrile, dimethylsulfoxide, dimethylformamide, "ionic liquids".

Add (acid/water) to (acid/water)

acid to water

As charge increases, aquo ligands become more ___________.

acidic

Most non-metal oxides are ________.

acidic

define zwitterion

adjacent charges

Group 1's name

alkali metals

Group 2's name

alkaline earth metals

Possible n values

an integer value (1,2,3....n)

What is l?

angular momentum quantum number

Acidity trend between anions and cations

anion < neutral < cation (most acidic)

Dative bonds sometimes represented with _______

arrows

What defines the type of element?

atomic number / protons

Negative potentials are good/bad

bad

Most metal oxides are _______.

basic

Why do we have to take metals to 3D conductivity?

because graphite is a good electrical conductor in 2D

Ionic properties

brittle, high melting points, conduct electricity, typically soluble in water, and involves very strongly and weakly electronegative elements

The only liquid non-metal at SATP

bromine

Group 16's name

chalcogens

charge density formula

charge / volume

No band gap =

conductor

One advantage and one disadvantage of the long form of the periodic table

correct order but too long

what is l=2's shape?

d

Electrostatic interactions sometimes represented with ___________.

dashed lines

As cation size __________, aquo ligands become more acidic.

decreases

Bronsted-lowry acid definition

donates H+

Lewis base definition

donates electrons

Metal characteristics

ductility (stretchable), malleability (squishible), and highly conductive

When Zeff increases, it's (easier/harder) to add an electron

easier

metallic

electron sea/gas

What is the aufbau Principle?

electrons fill in the lowest energy orbital first

Semi-metal characteristsics

even less metallic - tend to form small molecules rather than metallic sheets

What is l=3's shape?

f

VSEPR limitations

fails for isoelectronic species an fails to accurately predict geometries for transition metal complexes

Non-polar solvents are good at dissolving _____ and ______. (Hint: think dry cleaning)

fats and oils

∆G < 0 Rxn moves _________

forward

extreme steric bulk

frustrated lewis pairs

What is l=4's shape?

g

Define what weak nuclear force does

governs how things decary

Define what gravity does

governs particle attraction based on mass - doesn't rely on charge

Elements in the same ______ have similar properties.

group

What is l=5's shape?

h

Covalent radius

half distance between the nuclei of two atoms of the same element

Van der waals Radius

half distance between the nuclei of two neighboring atoms

Group 17's name

halogens

When Zeff increases, it's (easier/harder) to remove an electron

harder

Examples of non-polar solvents

hexane, diethyl ether, benzene, toluene, chloroform, xenon(!)

4s is always ______ in energy than 3d in ions

higher

HOMO

highest occupied molecular orbital

Frost Diagram: high and on the left of the plot =

highly oxidizing

Frost Diagram: high and on the right of the plot =

highly reducing

Define what strong nuclear force does

holds the nuclei together

Periodic table study websites

http://www.sporcle.com/games/g/elements http://www.ilpi.com/genchem/periodicquiz.html

∆E =

hv

Secondary coordination sphere:

hydrogen-bonding interactions similar to bulk water, stabilizing an acid.

What is l=6's shape?

i

Impurity band =

impurity semi-conductor

More negative charge will _________ the affinity for a positively charged proton.

increase

Arrhenius-Oswald acid definition

increase the [H+] in aqueous solution

Arrhenius-Oswald base definition

increase the [OH-] in aqueous solution

Large band gap =

insulator

Small band gap =

intrinsic semi-conductor

Zeff and radius are (directly/inversely) proportional.

inversely

More polar solvents, especially polar protic solvents: good at solubilizing _______.

ions

∆G = 0 Rxn _________

is at equilibrium

Entropy formula

klnw (k = boltzmann constant, w = # of possible states)

Beyond the 126 protons of _______, the number of positive charges in the nucleus becomes too large to maintain nuclear stability.

lead

Elements above ____ are unstable.

lead

Zeff increases from ____ to ____ on the period table

left to right

increasing electron affinity goes from

left to right and bottom to top

increasing ionization energy goes from

left to right and bottom to top

Heavier elements are _______ abundant

less - many are radioactive

BP = 2, LP = 0

linear

LUMO

lowest unoccupied molecular orbital

What is ml?

magnetic quantum numbers

Ionic

mainly electrostatic (large differences in electronegativity)

Covalent

mainly through orbital overlap

What is Hund's Rule?

maximize total spin and orbital angular momentum

Current x time =

moles of e- and Faraday's constant

Elements with even atomic numbers are _____ abundant.

more

higher diaelectric constant =

more polar

Primary coordination sphere:

most dramatic impact on reactivity and properties

Non-polar solvents, especially aprotic solvents: good for solubilizing ______________.

neutral small molecules

What defines the isotope of the element?

neutrons

∆H>0, ∆S<0: ∆G>0

never spontaneous

Group 18's name

noble gases

Non-metal characteristics

non-conducting and often liquids or gases

Types of solvents

non-polar, polar aprotic, polar protic

What is the atomic number made of?

number of protons in the nucleus (aka number of electrons)

Possible l Values

o to (n-1)

6 bonding pairs geometry

octahedral

BP = 6, LP = 0

octahedral

Elements with (even/odd) numbers of protons have an abundance of about 1/10th that of their (even/odd)-numbered neighbors.

odd; even

Know the different radiuses

okay

Know the name of the groups and regions of the table

okay

Look at powerpoint for calculation of Zeff

okay

Look up relationship between element names and symbols

okay

Look up the differences between the dirac and schrodinger wave equations

okay

what is l=1's shape?

p

The behavior of an unpaired electron is named _________.

paramagnetism

Elements in the same _____ have different properties, but have related orbital structure with different numbers of protons and electrons.

period

What period often exceeds the octet rule?

period 3

Group 15's name

pnictogens

What is n?

principle quantum numbers

Secondary coordination sphere can play a huge role in chemistry:

protein reactions are often dramatically influenced.

What two things are in the nucleus?

protons and neutrons

F =

q/n (charge / electrons)

Solubility is based on

reactant solvation and reactant IMF's

∆G > 0 Rxn moves _________

reverse

Atomic radius increases from _____ to _____ and from ____ to _____.

right to left; top to bottom

what is l=0's shape?

s

BP = 4, LP = 1

seesaw

Does a period go up and down or side to side?

side to side

SOMO

singly occupied molecular orbital

What is ms?

spin quantum number

∆H<0, ∆S>0: ∆G<0

spontaneous at any temperature

BP = 4, LP = 2

square planar

BP = 5, LP = 1

square-based pyramidal

Would you rather have s² and f₉ or s¹ and f¹⁰?

s¹ and f¹⁰

Would you rather have s² and f⁴ or s¹ and f⁵?

s¹ and f⁵

4 bonding pairs geometry

tetrahedral

BP = 4, LP = 0

tetrahedral

What is Z?

the actual nuclear charge

What happens when bound-water protons become more acidic?

they deprotonate!

5 bonding pairs geometry

trigonal bipyramidal

BP = 5, LP = 0

trigonal bypyramidal

3 bonding pairs geometry

trigonal planar

BP = 3, LP = 0

trigonal planar

BP = 3, LP = 1

trigonal pyramidal

Define pure covalent

two atoms with similar electronegativity

Paramagnetic behavior in a magnetic field indicates the presence of ________.

unpaired electrons

Does a group go up and down or side to side?

up and down

IMF's/Solubility of metals and network covalent

very strong bonding forces, not typically soluble

Examples of polar protic solvents

water, alcohols (methanol, ethanol), amines (ammonia, methylamine)

Define unstable

when left alone, the pure elemental material decomposes — usually occurs by radioactive decay.

Polar Aprotic Solvents

• Solvation through dispersion forces, polarization, and cation stabilization. • Good for some polar covalent small molecules and some ionic lattices.

VSEPR Theory (Gillespie-Nyholm Theory)

•Minimize formal charges (FC = nvalence - (nnon-bonded - nbonds)) • Ensure full octets (if possible) • Don't exceed an octet (unless d-orbitals are available) • Minimize overall charge • Avoid adjacent charges (zwitterions)

∆G formula

∆G = ∆G° + RtlnQ

Bond Order Formula

(# of bonding e - # of antibonding e)/2

Possible ms values

+1/2 and -1/2

Possible ml values

-1, 0, 1

Define what electromagnetic force is/does

-Combination of Electric, and magnetic effects (relationship between electric and magnetic fields) -Relies on sign and magnitude of charge -Electric attraction/repulsion are responsible for holding molecules together

Polar Protic Solvents

-Solvation through polarization, cation stabilization, and anion stabilization (H bond). • Good for ionic lattices, sometime unable to dissolve non-polar small molecules. • Good for hydrophilic materials

E =

-∆G° / nF

If you're calculating Zeff for a 1s electron, when n=n you subtract ____.

0.3

How many nodes does a p orbital have?

1

Slater's Rules

1. Each electron in orbitals of greater principle quantum number (in shells beyond the shell of interest) contributes 0. 2. (a) If e- of interest is in a s- or p-orbital, each e- with the same principle quantum number contributes 0.35. (b) If e- of interest is in a d or f orbital, the d or f e-'s contribute 0.35 but the s and p e⁻'s (of same quantum number) contribute 1.0. 3. (a) If e- of interest is in a s or p orbital, each e- in the (n-1) quantum level contributes 0.85. (b) If e- of interest is in a d or f orbital, then they contribute 1.0. 4. Each e- in an orbital of smaller principle quantum number contributes 1.0.

Predicting metal acidity rules:

1. Smaller cations = more acidic 2. More highly charged cations = more acidic 3. electronegativity

Find the potential using free energies instead of just standard potentials

1. ∆G° = nFE° 2. Add the two 3. Plug back into -∆G°FV/nF

The highest atomic number for which stable isotopes exist

126 (lead)

How many nodes does a d orbital have?

2

Completed quantum levels contain how many electrons? (List all the possibilities)

2, 10, 18, 36, 54, and 86

List the most stable nuclear configurations "magic numbers"

2, 8, 20, 28, 50, 82, 126

Suggest the number of neutrons in the most common isotope of Calcium

20 - doubly magic

All ionic transition metal complexes fill in order ___, ___, ____.

3d, 4s, 4p

Yttrium, element 39, exists in nature with only one isotope. What do you think the number of neutrons is?

50 - neutrons > protons and 50 is closest "magic" number above 39

How many stable elements are there?

80

What is the highest atomic number for which stable isotopes exist?

82 - lead

Faraday's constant

96485 C/mol

effective nuclear charge definition

Actual nuclear charge experienced by an electron in an atom.

k =

Ae^(-Ea/RT) (A = frequency factor)

Valence bond theory

Assumes that covalent bonds are formed when atomic orbitals on different atoms overlap and electrons are shared.

Semi-metals

B, Si, Ge, As, Sb, Te

Weak Metals

Be, Al, Zn, Ga, Sn, Pb, Bi, and Po

What are the eight chemically weak metals?

Beryllium, Aluminum, Zinc, Gallium, Tin, Lead, Bismuth, and polonium.

Suggest why polonium-210 and astatine-211 are the isotopes of those elements with the longest half-lives?

Both polonium-210 and astatine-211 have 126 neutrons, the filled-shell value, giving additional stability to the isotopes.

What is the only liquid nonmetal at SATP?

Bromine

Why s, p, d, f?

Derived from atomic spectral lines of alkali metals

Why is thermal conductivity a poor guide to determining metals?

Diamond, a carbon (nonmetal) allotrope, has the highest thermal conductivity of all substances.

Father of the periodic table

Dmitri Medeleev

rare earth metals

Elements scandium, yttrium, and lanthanum through lutetium

What makes something a metalloid?

Elements with some chemical and/or physical properties that resemble metals and others that resemble nonmetals. Alternative answer: elements with properties that are intermediate between those expected for a metal and those expected for a nonmetal

Define Bertrand's Rule

For almost all essential elements, there is an optimum amount for intake. Above or below this amount typically causes harmful effects.

What is the best criterion for metal?

High three-dimensional electrical conductivity

Covalent properties

Rely on matching orbital energy, orbital overlap, and symmetry

What are the rare earth metals?

Sc, Y, La-Lu

Why is metallic luster a poor guide to determining metals?

Several nonmetals, such as iodine, and some compounds, such as FeS2 fool's gold, have metallic lusters

What does s, p, d, and f stand for?

Sharp, Principle, Diffuse, Fundamental

Non-polar solvents

Solvation through dispersion forces, Good for non-polar covalent small molecules, and Hydrophobic or lypophilic substances

IMF's/Solubility of ionic lattices

Strong IMF's and soluble in water

What are the 4 fundamental forces?

Strong nuclear force, weak nuclear force, gravity and electromagnetic force

BP = 3, LP = 2

T

What is the only transition metal for which no stable isotopes are known?

Technetium

Only transition metal for which no stable isotopes are known

Telhnetium

Explain why the atomic mass of cobalt is greater than that of nickel even though the atomic number of cobalt is less than that of nickel

The common isotope of cobalt has more neutrons than that of nickel

Why is the atomic mass of cobalt bigger than nickel's?

The common isotope of cobalt has more neutrons than that of nickel, hence the atomic mass will be higher. In fact, the only natural isotope of cobalt has 32 neutrons, while nickel has two common isotopes, one with 30 neutrons (68 percent), the other with 32 neutrons (26 percent).

Why must the heavy elements on this planet have been formed from the very early supernovas that exploded?

The only way in which high-atomic-number elements can be formed is by means of the energy from supernova explosions (iron is the highest atomic-number element that is formed exothermically by fusion reactions). Hence these elements on this planet must have been formed from such an explosion billions of years ago.

What is σ?

The screening constant

Why does Hund's rule work?

The two electrons paired and occupying the same orbital would be least favorable, because the pairing energy would be necessary to overcome the repulsive forces. Paired but in different orbitals also comes with an energy cost because there is a finite probability that the electrons will occupy the same volume of space, again resulting in a repulsive energy factor. With parallel spins there is zero probability that the electrons will occupy the same volume of space; hence this is the lowest energy condition

Two reasons why the discovery of argon posed problems for the original mendeleev table

There was no space for argon because it did not fit into any of the then known groups (the noble gas group was then unknown). Also, because Mendeleev's table was based on measured atomic mass (atomic number was unknown at the time), argon (39.9) should have been placed between potassium (39.1) and calcium (40.1).