Inorganic Chemistry Exam Correctly
Answered
Various Isotopes of Hydrogen - ✅✅ Atoms of the same element have the same
atomic number (Z= 1), but may have varying mass numbers (A= 1, 2, 3,)
Atomic Number - ✅✅ - Number of Protons
- Number of Protons = Number of Electrons (in a neutral atom)
Atomic Mass Number - ✅✅ - Protons + Neutrons
- Electrons are not included in mass calculations because they are much smaller.
(1/2000) that of a proton.
Atomic Weight - ✅✅ Weighted average of the naturally occurring isotopes of an
element.
Molar Mass - ✅✅ Grams per mol (g/mol)
Planck Relation - ✅✅ - Quanta: Energy emitted as electromagnetic radiation
from matter comes in discrete bundles.
- E = hf
- h= 6.626*10^-34 J*s
- Energy is inversely proportional to wavelength
,Speed of Light - ✅✅ c= 3 * 10^8 m/s
Angular Momentum of an electron orbiting - ✅✅ - n is the principal quantum
number
- h is planck's constant = 6.626*10^-34 J*s
- Part of Bohr Model
- L = n-1
Energy of the electron - ✅✅ - E is the energy of the electron
- RH: Rydberg unit of energy; 2.18*10^-18 J/electron
- n: Principal quantum number
- Due to the negative sign, (E) is directly proportional to the principal quantum
number (n)
- Positive E: Emission of energy (electrons move to orbits of lower energy)
- Negative E: Absorption (color we see is the light that is not absorbed by the
compound)
- Part of Bohr Model
Ground State of an atom - ✅✅ - State of lowest energy (n=1), in which electrons
are in the lowest possible orbitals.
- Bohr's Nobel prize winning model
Heisenberg uncertainty principle - ✅✅ It is impossible to simultaneously
determine, with perfect accuracy, the momentum and the position of an electron
, Bohr model of the atom - ✅✅ A dense positively charged nucleus is surrounded
by electrons revolving around the nucleus in orbits with distinct energy levels.
Quantum - ✅✅ - Energy difference between energy levels. First described by
Planck.
- Electrons can only exist at certain energy levels.
- The energy of an electron increases the further it is from the nucleus.
Atomic Absorption Spectrum - ✅✅ - For each element is unique
- For an element to jump from a lower energy to a higher one, it must absorb an
amount of energy precisely equal to the energy difference between the two levels.
Atomic Emission Spectrum - ✅✅ - When electrons return from the excited state
to the ground state, they emit an amount of energy that is exactly equal to the
energy difference between the two levels.
Quantum Mechanical Model - ✅✅ - Electrons do not travel in defined orbits, but
rather localized in orbitals
- Orbitals: A region of space around the nucleus defined by the probability of
finding an electron in that region of space.
Heisenberg Uncertainty Principle - ✅✅ - States that is it is impossible to know
both an electron's position and its momentum exactly at the same time.
Quantum Numbers - ✅✅ - Describe any electron in an atom
- Principal Quantum number, n: average energy of a shell.
- Azimuthal quantum number, l: describes sub shells within a given principal
energy level (s, p, d, f)
Answered
Various Isotopes of Hydrogen - ✅✅ Atoms of the same element have the same
atomic number (Z= 1), but may have varying mass numbers (A= 1, 2, 3,)
Atomic Number - ✅✅ - Number of Protons
- Number of Protons = Number of Electrons (in a neutral atom)
Atomic Mass Number - ✅✅ - Protons + Neutrons
- Electrons are not included in mass calculations because they are much smaller.
(1/2000) that of a proton.
Atomic Weight - ✅✅ Weighted average of the naturally occurring isotopes of an
element.
Molar Mass - ✅✅ Grams per mol (g/mol)
Planck Relation - ✅✅ - Quanta: Energy emitted as electromagnetic radiation
from matter comes in discrete bundles.
- E = hf
- h= 6.626*10^-34 J*s
- Energy is inversely proportional to wavelength
,Speed of Light - ✅✅ c= 3 * 10^8 m/s
Angular Momentum of an electron orbiting - ✅✅ - n is the principal quantum
number
- h is planck's constant = 6.626*10^-34 J*s
- Part of Bohr Model
- L = n-1
Energy of the electron - ✅✅ - E is the energy of the electron
- RH: Rydberg unit of energy; 2.18*10^-18 J/electron
- n: Principal quantum number
- Due to the negative sign, (E) is directly proportional to the principal quantum
number (n)
- Positive E: Emission of energy (electrons move to orbits of lower energy)
- Negative E: Absorption (color we see is the light that is not absorbed by the
compound)
- Part of Bohr Model
Ground State of an atom - ✅✅ - State of lowest energy (n=1), in which electrons
are in the lowest possible orbitals.
- Bohr's Nobel prize winning model
Heisenberg uncertainty principle - ✅✅ It is impossible to simultaneously
determine, with perfect accuracy, the momentum and the position of an electron
, Bohr model of the atom - ✅✅ A dense positively charged nucleus is surrounded
by electrons revolving around the nucleus in orbits with distinct energy levels.
Quantum - ✅✅ - Energy difference between energy levels. First described by
Planck.
- Electrons can only exist at certain energy levels.
- The energy of an electron increases the further it is from the nucleus.
Atomic Absorption Spectrum - ✅✅ - For each element is unique
- For an element to jump from a lower energy to a higher one, it must absorb an
amount of energy precisely equal to the energy difference between the two levels.
Atomic Emission Spectrum - ✅✅ - When electrons return from the excited state
to the ground state, they emit an amount of energy that is exactly equal to the
energy difference between the two levels.
Quantum Mechanical Model - ✅✅ - Electrons do not travel in defined orbits, but
rather localized in orbitals
- Orbitals: A region of space around the nucleus defined by the probability of
finding an electron in that region of space.
Heisenberg Uncertainty Principle - ✅✅ - States that is it is impossible to know
both an electron's position and its momentum exactly at the same time.
Quantum Numbers - ✅✅ - Describe any electron in an atom
- Principal Quantum number, n: average energy of a shell.
- Azimuthal quantum number, l: describes sub shells within a given principal
energy level (s, p, d, f)
