Module I Flashcards
Extensive property
A property that depends on how much matter you have
Intensive property
A property that does not depend on its quantity
Absolute error =
Measured value - True value
Relative error =
Absolute error / True value
What is absolute error?
The difference between a measured value and a true value
What is relative error?
The proportion of the absolute error relative to the measured value
Standard state of metals
Solid (except for mercury, a liquid)
Standard state of nonmetals
Solid
Standard state of diatomic nonmetals
Gas
Exceptions to diatomic nonmetal standard states
Iodine (solid) and Bromine (liquid)
Standard state of phosphorus
P4(s)
Standard state of sulfur
S8(s)
Definition of precision
How closely clustered together the measurements are
Definition of accuracy
How close to the true value the measurement is
When will charge items not interact?
When they are infinitely far apart
Quantum number n
Principle quantum number, shell number
Roughly describes the distance from the nucleus
Fully describes energy in single electron systems
Quantum number L
Shape of orbitals
s, p d, f
s = 0 … f = 3
Max value = n-1
Quantum number m(L)
Magnetic quantum number
Orientation of orbital
-L <= m(L) <= L
Quantum number m(S)
Spin quantum number
Property of the electron itself, not its orbital
Either +1/2 or -1/2
Which electrons are best at screening?
The electrons closest to the nucleus are best at screening the nucleus’s charge from outer electrons
Why is there no 1p orbital?
Because p indicates that L=1, therefore n must equal 2
Effective nuclear charge
The pull exerted on a specific electron by the nucleus, notated as Z(eff)
What makes a group of atoms and/or ions isoelctronic?
Sharing the same electron configuration
Ionization energy
The amount of energy required to remove the most loosely bound electron (cation formation)
Electron affinity
The energy change for the process of adding an electron to form an anion. Can be endothermic or exothermic.
A compound made of nonmetals only is usually…
Molecular
A compound made of metals and nonmetals is usually…
Ionic
Determinate error
Causes the mean of a data set to differ from the accepted value
Indeterminate error
Causes data to be scattered roughly symmetrically around a mean value (also called random error)
Dalton’s atomic theory
- Elements consist of indivisible small particles
- All atoms of the same elements are identical
- Atoms can neither be created nor destroyed
What subshells do electons fill first?
The ones with the lowest available energy
You calculate that two of an atoms electrons share the same set of four quantum numbers. Is this correct?
No. The Pauli Principle states that no two electrons in an atom can have an identical set of four quantum numbers. You likely made a mistake somewhere.
Hund’s rule
All orbits will be singly occupied before any is doubly occupied
Empirical formula
Simplest whole number ratio of atoms found in a compound/molecule
Simplest whole number ratio of atoms found in a compound/molecule
Empirical formula
How to calculate the total number of orbital nodes:
n - 1
n being the first quantum number, referring to an electron’s shell (think Bohr model)
How to calculate the total number of angular/planar nodes:
L
L being the second quantum number, corresponding to the s p d f orbital shapes
How to calculate the total number of radial/spherical nodes:
n - 1 - L
For the smartasses, just subtract the number of angular/planar nodes from the total number of orbital nodes
What is light’s/photons ability to excite and eject an electron dependent on?
The frequency of the photon wave, NOT its intensity!
This is because energy is quantized (smallest divisible particle is a photon). It’s not continuous
