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Chemistry GRE > Inorganic > Flashcards

Inorganic Flashcards

1
Q

Binding energy

A

Energy used to bind the nucleus of an atom and overcome the proton-proton repulsion

This energy is the reason that the atomic mass of an atom is slightly less than the sum the masses of its constituent protons, neutrons, and electrons

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2
Q

Mass Number (A)

A

The total number of protons and neutrons in the nucleus

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3
Q

Atomic Number (Z)

A

Total number of protons in the nucleus

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4
Q

Alpha particle

A

4/2 He

Or helium nucleus

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5
Q

Normal beta particle

A

An electron ejected from neutron

A neutron is converted to a proton and an electron

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6
Q

Electron capture

A

A proton and an electron fuse to make a neutron

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7
Q

Positron Emission

A

Proton breaks down into a neutron and a positron

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8
Q

Gamma emission

A

And excited atom releases a Gamma Ray Photon

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9
Q

Transmutation

A

Process where one element is transformed into another

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10
Q

Primary quantum number, n

A

The energy level or shell of an orbital

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11
Q

Secondary quantum number, l

A

The angular momentum of an electron in an orbital. This describes the shape of an orbital

l = 0, s orbital

l = 1, p orbital

l = 2, d orbital

l = 3, f orbital

l = 4+, proceed in alphabetical order after f

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12
Q

Magnetic quantum number, ml

A

The subshells of a particular orbital are further divided into electron orbitals

s orbitals have 1

p orbitals have 3

d orbitals have 5

f orbitals have 7

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13
Q

Spin quantum number, ms

A

Each orbital can hold two electrons, the two electrons will have opposite spins given by the Spin Quantum Number.

ms = +1/2 or -1/2

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14
Q

Pauli exclusion principle

A

The principle states that no two electrons of the same atom will have completely identical quantum numbers (n, l, ml, ms).

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15
Q

Aufbau principal

A

To find the correct ground state electric configuration of an atom, always completely fill the lower energy orbitals before filling any higher energy orbitals.

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16
Q

Hund’s rule

A

When feeling degenerate orbitals for p, d, or f subshells always put one electron in all available orbitals, before pairing two electrons in the same subshell.

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17
Q

Exceptions to Aufbau principle and transition metal ions

A

The Aufbau principle can be violated as extra stabilization can be achieved when a d orbital is half or completely filled. (s electrons may be promoted to d orbital)

Transition metals will lose valence s electrons before losing any d electrons.

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18
Q

N-type conductor

A

A semiconductor that is doped with atoms that contain an extra e-

e- can be released which initiates a current

D-band is slightly below the Conductor Band

Group 5: P
Group 7: At

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19
Q

P-type conductor

A

A semiconductor that is doped with atoms that contain an empty p-orbital

e- can be accepted which initiates a current

A-band is slightly above the Valence Band

Group 3: B, Ga

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20
Q

Intrinsic semiconductor

A

A material where the CB is at a higher E level that the VB. Heat may be applied to cause an e- in the VB to jump to the CB.

Applying a current will cause e- to flow through the material as e- will move to fill the holes.

21
Q

Extrinsic semiconductor

A

A material that is normally an insulator, that was made to be a semiconductor by doping the crystal lattice

22
Q

Coulomb’s Law

A

F = (kQ1Q2)/r^2

k = 9.010^9 N(m^2)/(C^2)

If:
F<0, force is attractive.
F>0, force is repulsive.

23
Q

Repulsive forces

A

e- cloud repulsion (or steric hindrance)

24
Q

Cohesive forces

A
  • ionic forces
  • dipole forces (force is proportional to Q1*Q2)
  • london dispersion forces (results from two instantaneous dipoles of atoms in close proximity)
25
Q

Unit cell

A

The smallest repeating unit of a crystal lattice

26
Q

Lattice energy (U)

A

The energy of electrostatic interactions of a crystal

27
Q

Ionic solids

A

A solid composed of cations and anions

28
Q

Covalent solids

A

Solid composed of atoms that are held together by very strong covalent bonds

29
Q

Molecular solids

A

A solid composed of neutral molecules

Ex: H2O, sucrose, I2, P4

30
Q

Metallic solids

A

Solid composed of a closely packed metal element

31
Q

T-hole

A

An atom fills this void to make a tetrahedron

32
Q

O-hole

A

An atom fills this void to make an octahedron

33
Q

Cubic closest packed

A

Length = 2r

Volume = 8(r^3)

34
Q

Body centered cubic cell

A

Length = 4/(sqrt(3))*r

Volume = 64/3(sqrt(3))*(r^3)

35
Q

Face centered cell

A

Length = 4/(sqrt(2))*r

Volume = 32/(sqrt(2))*(r^3)

36
Q

Radius of the nucleus

A

r = (1.33•10^-13)(A^(1/3)) cm

  • A = mass number
37
Q

Consequences of lattice energy

A

1) Thermal stability
- Generally large cations are stabilized by large anions and vice versa

2) High ox. #s and small ions
- Cations with high ox. #s are stabilized by small anions (allows for shorter bond length)

3) Solubility
- In general, compounds that contain ions with widely different radii are generally soluble in H2O (MgSO4, and BaOH are water soluble)

38
Q

Le Chatelier’s Principal

A

The eq point can be disturbed by:

1) Concention
- add to reactance equals shift to products
- remove reactance equals shift to reactants

2) Pressure
- Increase pressure equals shift to the side with less gas molecules
- Decrease Pressure equals shift two the side with more gas molecules

3) Temperature
- If DeltaH > 0, heat is a reactant. Increase or reduce temperature fix EQ as rule #1
- Changing T is the only way to change EQ constant (K)

39
Q

Amphoteric molecule/ion

A

A molecule/ion that will act either as an acid or a base, depending on the conditions of the solution that it is in

HCO3
Acidic: HCO3 + H -> H2CO3
Basic: HCO3 + OH -> CO3 + H2O

40
Q

Strong acids

A 
HCl
HBr
HI
HNO3
H2SO4
HClO4
41
Q

Strong bases

A

LiOH
NaOH
KOH

42
Q

pH equations

A

pH + pOH = 14

pH = pKa + log([A-]/[HA])

pOH = pKb + log([HA]/[A-])

43
Q

pH calculations

A

If the [acid] or [base] is 3 orders of magnitude greater than the Ka or Kb value, then you can exclude x from the denominator

K = (x^2)/(M - x) -> (x^2)/M

44
Q

When do acid-base indicators change color?

A

At pH +/- 1 of their pka

H-Indicator —> H+ + Indicator-
Red) (Yellow

45
Q

At what point of a titration curve does the pH = pKa?

A

Halfway to the equivalence point.

[HA] = [A-], so..

Henderson Hasselbach: pH = pKa

46
Q

Borane classes:

A

Closoboranes: BnHn

Nidoboranes: BnH(n+4)

Arachnoboranes: BnH(n+6)

47
Q

Most reactive noble gas

A

Xenon

XeF2 XeF4 XeF6

Xe is also know to bond with C, N, and O.

48
Q

Solubility in H2O

MgCO3 vs BaCO3

MgOH vs BaOH

A

MgCO3 is more soluble in water then BaCO3
- Ba has a more similar radius to CO3(-2) so it is not water soluble

BaOH is more soluble in water than MgOH

Chemistry GRE (3 decks)

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