Master Deck Flashcards
How many kilograms is 1 dalton?
1.66x10-27kg
What is another unit for the atomic mass unit (amu)?
dalton
What is the exact charge of an electron?
1.6 x 10-19
Which is the considered the identity of an element: protons, neutrons, or electrons?
proton
What is the mass number of an element?
protons + neutrons
What is the atmoic number of an element?
number of protons
Which of these can change: atomic number or mass number?
mass number (isotopes)
What are the 3 isotopes for hydrogen?
hydrogen (0 neutrons), dueterium (1 neutron), tritium (2 neutron)
What is atomic weight?
the average mass of all isotopes of an atom
What do the suffixes -ous and -ic mean in the context of ions?
-ous means lesser charge (Fe+2), -ic means greater charge (Fe+3)
What does the suffix -ide mean in the context of ions?
monoatomic anions
What does the suffix -ite and -ate mean with respect to oxyanions?
-ite= fewer oxygens; -ate=greater oxygens
Does oxide have a negative or positive charge?
-ide indicates an anion, which is negatively charged
Which has more electrons, chlorate or chlorite? What about nitrate vs nitrite?
the suffix -ate tells you that chlorate and nitrate have more electrons
What does the prefix “hypo” mean in the context of anions?
This means 1 less electron than the -ite form
What does the prefix “per” mean in the context of anions?
This means 1 more electrons than the -ite form
What letter represents the atomic number?
Z
What is the lowest energy level for an electron?
n=1
The energy emitted or absorbed from an electron is is in the form of _________.
electromagnetic radiation
What is the equation describing the amount of energy emitted from an electron when excited?
E=hf
h=Planck’s constant; f=frequency of light
What is the equation for the frequency of light?
f=c/lambda
c=speed of light; gamma=wavelength
Can also be:
E=h(c/lambda)
When electrons jump energy levels, the energy of the photon is emitted or absorbed in discrete energy amount, called _____
quanta
What are atomic emission/absorption spectra?
a set of distinct lines that each represent the quantized amount of energy emitted/absorbed when an electron falls to a lower energy level. ; these are unique for each element
How do you use the Rydberg formula for the MCAT?
See whether the initial energy>final energy. If so, we have a positive amount of energy, meaning energy was absorbed to get this electron to a higher state
What is the Heisenberg Uncertainty Principle?
It is impossible to know both the exact position and speed of an electron at the same time
What is the Pauli Exclusion Principle?
no two electrons in an atom can have the same four quantum numbers
(“can’t have the same address”)
What is the order of quantum numbers in order of most broad to most specific?
Electron shell, subshell, orbital, electron
What symbol represents the principal quantum number? what values can it have?
n; 1-5…
What does n represent in quantum numbers? What values can it have?
the quantum number; 1-5…
What does the symbol “l” represent in quantum numbers?
angular momentum, or azimuthal number
What is the azimuthal number?
angular momentum, “l”
What symbol represents angular momentum?
l; angular momentum is also called the azimuthal number.
What does the azimuthal number/angular momentum tell us about the electron?
the shape of the orbital: s, l=0, p, l=1, d, l=2 f, l=3
How do you calculate the azimuthal number?
n-1
n=quantum number
If n=2, what is l? Given the number and letter for orbital
1, p
What is the magnetic quantum number?
spatial orientation of the electron; for l=2, m=-2,-1,0,+1,+2
What is the spin quantum number?
specifies negative half or positive half spin; -1/2, +1/2
What is the difference between shell, subshell, and orbital?
shell=broadest term; principal quantum number; the path of an electron around the nucleus
sub shell= s, p, d, f; most likely to find electron
orbital=unique spatial orientation; 2 electrons
How many electrons can exist at an energy level of n=4?
(4^2)x2=32
True or False: Each subshell can hold up to two electrons, regardless of the energy level, subshell shape, or subshell orientation.
True
True or False: The number of electrons that a given subshell can accommodate is dependent on the orbital the electron is in.
False; Each subshell can hold up to two electrons, regardless of the energy level, subshell shape, or subshell orientation.
What is the Aufbau Principle?
electrons fill orbitals in order of lowest to highest energy
