Module I Flashcards
(39 cards)
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)
