Chapters 6 & 7

Question 1

electronic structure (of atoms)

Answer 1

arrangement and energy of electrons

Question 2

Electromagnetic radiation (radiant energy)

Answer 2

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

Question 3

C =

Answer 3

c = λv
c = 3.00 x 10^8 m/s

Question 4

wavelength (λ)

Answer 4

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

Question 5

Frequency(v)

Answer 5

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

Question 6

Electromagnetic Spectrum

Answer 6

electromagnetic radiation arranged in increasing wavelength

Question 7

blackbody radiation

Answer 7

emission of light from hot objects

Question 8

photoelectric effect

Answer 8

emission of electrons from metal surfaces which light in shone

Question 9

emission spectra

Answer 9

emission of light from electronically excited gas atoms

Question 10

Quantum physics

Answer 10

physics to describe atoms

Question 11

Quantum theory

Answer 11

to describe electronic structure of atoms

Question 12

Photoelectric effect

Answer 12

every metal has diff energy level which ejects e-

Question 13

Planck’s constant: E=

Answer 13

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

Question 14

Emission spectra

Answer 14

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

Question 15

Continuous spectrum

Answer 15

(the “rainbow”) from white light source

Question 16

Line spectrum

Answer 16

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

Question 17

Rydberg formula

Answer 17

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

Question 18

Bohr equation

Answer 18

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

Question 19

ground state

Answer 19

lowest energy state of atom
- n=1

Question 20

excited state

Answer 20

higher energy state of atom
- n=2+

Question 21

λ =

Answer 21

h / mv

Question 22

Heisenberg Uncertainty Principle

Answer 22

can’t know both momentum and position of a particle

Question 23

Wave functions

Answer 23

describes the electron (orbital) and its energy

Question 24

electron density

Answer 24

probability e- can be found in specific location

Question 25

orbitals

Answer 25

hold 2 electrons

Question 26

electron shell (n)

Answer 26

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

Question 27

subshell

Answer 27

diff orbital types w/in shell

Question 28

s orbital

Answer 28

L = 0
- spherical

Question 29

p orbital

Answer 29

L = 2
- 2 lobes w/ 1 node

Question 30

f orbital

Answer 30

L = 3

Question 31

degenerate orbitals

Answer 31

orbitals at same energy level; n =

Question 32

electron spin

Answer 32

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

Question 33

pauli exclusion principle

Answer 33

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

Question 34

electron configurations

Answer 34

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

Question 35

ground state

Answer 35

most stable organization at lowest possible energy

Question 36

orbital diagram

Answer 36

each orbital denoted by box and electron by half arrow

Question 37

Hund’s rule

Answer 37

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

Question 38

Valence electrons

Answer 38

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

Question 39

core electrons

Answer 39

filled inner-shell electrons; part in [ ]

Question 40

transition elements

Answer 40

10 elements touching step-line
- d-block

Question 41

Lanthanide elements

Answer 41

4f

Question 42

Actinide elements

Answer 42

5f

Question 43

Periodicity

Answer 43

repetitive pattern of property for elements based on atomic number

Question 44

effective nuclear charge (Zeff)

Answer 44

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

Question 45

Slater’s Rules

Answer 45

ignore all outer e- beyond one of interest

Question 46

Nonbonding radius (van der Waals radius)

Answer 46

½ shortest distance separating 2 nuclei during collision of atoms

Question 47

Bonding atomic radius (covalent radius)

Answer 47

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

Question 48

cations

Answer 48

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

Question 49

anions

Answer 49

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

Question 50

isoelectronic series

Answer 50

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

Question 51

Ionization energy

Answer 51

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

Question 52

first ionization energy

Answer 52

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

Question 53

Electron affinity

Answer 53

measures attraction/affinity of atom for added electron

Question 54

Ionization energy measures energy change when atom __ e-

Answer 54

loses

Question 55

Electron affinity measures energy change when atom __ e-

Answer 55

gains

Question 56

increasing atomic radius

Answer 56

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

Question 57

increasing ionization energy

Answer 57

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

Question 58

increasing electron affinity

Answer 58

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

Question 59

increasing metallic character

Answer 59

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