Quantum Chemistry

Question 1

Wavelength is inversely proportional to Frequency, Energy, and Wavenumber

Question 2

Phenomenon in which electrons are emitted from surface of a metal when light strikes it.

Answer 2

Photoelectric effect

Question 3

Equation that describes spectral line emissions of hydrogen atom

Answer 3

Rydberg Equation

Question 4

Quantum number that descirbes the distance of electrons from nucleus (energy level)

Answer 4

Principal

Question 5

Describes energy subshells and shape of orbitals

Answer 5

Azimuthal

Question 6

Describes the number of orbitals in subshells and their possible orientation in space

Answer 6

Magnetic

Question 7

Describes the movement of electron around it’s own axis

Answer 7

Spin

Question 8

Probability of finding no electron

Answer 8

Node

Question 9

What principle states “ orbitals filled with electrons in increasing energy”

Answer 9

Aufbau

Question 10

What principle states that “the moste stable arrangement of electron in subshells ins the one with the most number of parallel spins”

Answer 10

Hunds rule of maximum multiplicity

Question 11

Principle that states that “An orbital must contain a max of 2 electron with opposite signs”

Answer 11

Pauli’s Exclusion Principle

Question 12

Lowest energy arrangements of electrons

Answer 12

Graound state electron configuration

Question 13

In a configuration, electrons with highest principal quantum number are the ____

Answer 13

Valence electron

Question 14

Species with same electron configuration is called ____

Answer 14

Isoelectronic

Question 15

As more orbitals, subshells and energy levels are filled up with electrons, the energy differences between subshells become smaller

Question 16

Measure of nuclear attraction for an electron

Answer 16

Effective nuclear charge

Question 17

Used to compute for shielding constant

Answer 17

Slater’s Rule

Question 18

Significant decrease in size from left to right among lanthanide metals, where outer electrons filled the 4f orbital.

Answer 18

Lanthanide contraction

Question 19

Minimum energy required to remove an electron from a gaseous atom in it’s ground state

Answer 19

Ionization Energy

Question 20

As the charge of species become more positive, inner electrons are more tightly held by the nucleus resulting in increase in successive ionization energies.

Question 21

Energy change associated with the addition of electron to a gaseous atom

Answer 21

Electron affinity

Question 22

Electron affinity is ____ when energy is released, ____ when energy is required, and ____ when the process is energetically neutral

Answer 22

Negative, positive, zero

Question 23

Chemical property that describes the tendency of atom or functional group to attract electrons towards itself

Answer 23

Electronegativity

Question 24

Equation used in determining electronegativity values

Answer 24

Mulliken equation
X=(IE+EA)/2

Question 25

Ability to be distorted by an electric field

Answer 25

Polarizability

Question 26

Summarizes the factors that affects polarization

Answer 26

Fajans Rule

Question 27

Fajans Rule
1. Small, highly charged cations have polarizing ability
2. Large, highly charged anions are easily polarized
3. Cations without noble gas electron configuration are easily polarized

Question 28

Bond type when theres a low charge on ions and the size of cation is large while that of the anion is small?

Answer 28

Ionic bond

Question 29

Bond type when theres a high charge on ions and the size of cation is small while that of the anion is large?

Answer 29

Covalent bond