Chapters 6 & 7 Flashcards by Abby Kreisler

electronic structure (of atoms)

arrangement and energy of electrons

How well did you know this?

Not at all

Perfectly

Electromagnetic radiation (radiant energy)

carries energy through space
- moves at speed of light (c)

How well did you know this?

Not at all

Perfectly

C =

c = λv
c = 3.00 x 10^8 m/s

How well did you know this?

Not at all

Perfectly

wavelength (λ)

distance b/w 2 wave peaks
- meters (or nm)

How well did you know this?

Not at all

Perfectly

Frequency(v)

of complete cycles (wavelengths) that pass a given point/second
- v = 1 s^-1

How well did you know this?

Not at all

Perfectly

Electromagnetic Spectrum

electromagnetic radiation arranged in increasing wavelength

How well did you know this?

Not at all

Perfectly

blackbody radiation

emission of light from hot objects

How well did you know this?

Not at all

Perfectly

photoelectric effect

emission of electrons from metal surfaces which light in shone

How well did you know this?

Not at all

Perfectly

emission spectra

emission of light from electronically excited gas atoms

How well did you know this?

Not at all

Perfectly

Quantum physics

physics to describe atoms

How well did you know this?

Not at all

Perfectly

Quantum theory

to describe electronic structure of atoms

How well did you know this?

Not at all

Perfectly

Photoelectric effect

every metal has diff energy level which ejects e-

How well did you know this?

Not at all

Perfectly

Planck’s constant: E=

E = hv
- to calculate the energy required to remove an electron

How well did you know this?

Not at all

Perfectly

Emission spectra

observed energy emitted when electric current is passed thru
- radiation–>component wavelengths

How well did you know this?

Not at all

Perfectly

Continuous spectrum

(the “rainbow”) from white light source

How well did you know this?

Not at all

Perfectly

Line spectrum

radiation of only specific wavelengths; discrete wavelengths observed
- each element = unique line spectrum

How well did you know this?

Not at all

Perfectly

Rydberg formula

1/λ = (RH)x((1/n1^2) - (1/n2^2))
- RH = 1.096 x 10^7 m^-1

How well did you know this?

Not at all

Perfectly

Bohr equation

∆E = Ef-Ei
- ∆E = (-2.18 x 10^-18 J)(1/n^2-1/n^2)

How well did you know this?

Not at all

Perfectly

ground state

lowest energy state of atom
- n=1

How well did you know this?

Not at all

Perfectly

excited state

higher energy state of atom
- n=2+

How well did you know this?

Not at all

Perfectly

λ =

h / mv

How well did you know this?

Not at all

Perfectly

Heisenberg Uncertainty Principle

can’t know both momentum and position of a particle

How well did you know this?

Not at all

Perfectly

Wave functions

describes the electron (orbital) and its energy

How well did you know this?

Not at all

Perfectly

electron density

probability e- can be found in specific location

orbitals

hold 2 electrons

electron shell (n)

orbitals w/ same n value - ex: all orbitals w/ n=3 = third orbital

subshell

diff orbital types w/in shell

s orbital

L = 0 - spherical

p orbital

L = 2 - 2 lobes w/ 1 node

f orbital

L = 3

degenerate orbitals

orbitals at same energy level; n =

electron spin

describes magnetic field; (+/-) 1/2

pauli exclusion principle

each electron in atom must have distinct quantum numbers; need image to describe

electron configurations

way electrons are distributed in an atom - orbitals filled in order of increasing energy - n = energy level - letter = type of orbital - superscript = number of electrons in orbitals

ground state

most stable organization at lowest possible energy

orbital diagram

each orbital denoted by box and electron by half arrow

Hund’s rule

"sharing is caring" - there must be 1 e- (w/ same spin) per orbital before pairing with 2nd opposite spin

Valence electrons

same group (↓) have same # of e- in outer shell; part after [ ]

core electrons

filled inner-shell electrons; part in [ ]

transition elements

10 elements touching step-line - d-block

Lanthanide elements

Actinide elements

Periodicity

repetitive pattern of property for elements based on atomic number

effective nuclear charge (Zeff)

Zeff = Z – S feel pull of nucleus more: - changes w/ # of protons - increase Zeff = increase nucleus size = incr. pull - decrease Zeff = decr. nucleus size = decr. pull

Slater's Rules

ignore all outer e- beyond one of interest

Nonbonding radius (van der Waals radius)

½ shortest distance separating 2 nuclei during collision of atoms

Bonding atomic radius (covalent radius)

½ distance b/w nuclei in a bond - Can’t get any closer bc of core e- repulsion - Bonding radius < nonbonding radius

cations

- smaller than parent atoms - e- removed - repulsions b/w e- = reduced

anions

- larger than parent atoms - e- added - repulsions b/w e- = increased

isoelectronic series

ions have the same # e-, diff # of protons - calculate number of ions and compare

Ionization energy

energy required to remove 1 e- from ground state of a gaseous atom or ion - larger ionization energy # = more difficult to remove e-

first ionization energy

- removing e- from gaseous element ex: Al (g) --> e- + Al+ (g)

Electron affinity

measures attraction/affinity of atom for added electron

Ionization energy measures energy change when atom __ e-

loses

Electron affinity measures energy change when atom __ e-

gains

increasing atomic radius

Increasing: - right to left - top to bottom (same as increasing metallic character)

increasing ionization energy

Increasing: - left to right - bottom to top (same as increasing electron affinity)

increasing electron affinity

Increasing: - left to right - bottom to top (same as increasing ionization energy)

increasing metallic character

Increasing: - right to left - top to bottom (same as increasing atomic radius)