chapter 3 electronic structure midterm review

what is the relationship between light and energy

energy in light is directly related to frequency, short wavelengths=high frequency=high energy

how do you calculate the energy of electromagnetic radiation given its wavelength and vice versa

E=hv and c=wavelength times v

how do line spectra occur

when electrons transition btw quantized energy levels of electrons in an atom, each specific energy transition btw different electron energy levels indicates, higher to lower

what is the concept of wave-particle duality in regards to electromagnetic radiation and electrons

electromagnetic particles exhibit wave like behavior, but give off photons that are considered particles. have both characteristics depends on the situation

how do electromagnetic particles give off photons?

when the electron returns to a lower energy, it gives off electromagnetic energy, releasing photons

how did the photoelectric effect confirm the wave-particle duality of light photons

since only certain frequencies of light are able to cause ejection of electrons, this confirms that light behaves like particles when interacting with electrons

how do you calculate the threshold frequency/wavelength for a substance

wavelength = hc/work function
frequency = work function/h
E=hv

how does the wave-particle nature of electrons capture the limitations of the Bohr model of the atom

it portrays electrons as particles orbiting the nucleus in fixed patterns, but neglects the wavelength behavior since electrons cannot be precisely located in space

what is the concept of wave functions in relation to its probability

its wavelike behavior and its probability of finding electrons at a specific location

what is the concept of atomic orbitals

the region of space where the electron is found in

what are the types of atomic orbitals

s, p, d, and f

what are the quantum numbers (l) associated with the different types of atomic orbitals, s

0

what are the quantum numbers (l) associated with the different types of atomic orbitals, p

1

what are the quantum numbers (l) associated with the different types of atomic orbitals, d

2

what are the quantum numbers (l) associated with the different types of atomic orbitals, f

3

how many electrons can s orbitals hold

2

how many electrons can p orbitals hold

6

how many electrons can d orbitals hold

10

how do you determine the set of 4 quantum numbers for any given electron in an atom

using the last valence electron in the electron config, find n and l from that, using the quantum numbers, fill in the electrons according to the orbitals and electron number, then use that to find ml and whether it is up or down, find ms

how do you write short hand electron configs

use previous noble gas and account for everything after the noble gas

how do you know that an ion is positive using the electron configuration

if the valence shell has few electrons, remove to form a positive ion with the same electron configuration as preceding noble gas

how do you know that an ion is negative using the electron configuration

if the valence shell is nearly full, add to complete, forming negative ion

describe the relationship between periodic nature of periodic table and building up of atomic orbitals/electron configs

building is known as aufbau principle, that electrons added to orbitals in order of increasing energy with each row new electron shell filled

what do the different blocks on the periodic table correspond to

the different types of orbitals being filled

using the concept of effective nuclear charge explaining how atomic radius, ionization energy, and electron affinity change across a period of elements and down a group of elements, what occurs in the periodic table: __________ across group and _____________ down a group

decreases, increases

what does across the period mean: _____________ a nuclear change, ___________ atomic radius, ___________ ionization energy, ____________ electron affinity charge

increasing, decreasing, increasing, increasing

what does down the group mean: _____________ atomic radius, _____________ ionization, ____________ electron affinity

increasing, decreasing, decreasing