Chapter 6- Electronic Structure & Periodic Table

Question 1

electromagnetic radiation

Answer 1

radiation consisting of electric and magnetic waves that travel at the speed of light

Question 2

wavelength

Answer 2

• distance between two consecutive peaks in a wave

- unit: m

Question 3

frequency

Answer 3

• number of waves (cycle) per second that pass a given point in space
• unit: 1/s = hertz (Hz)
• frequency = speed of light (c)/ wavelength

Question 4

Max Planck’s Quantum Theory

Answer 4

• light must be emitted and absorbed in discrete amounts

- light was before considered as a continuous electromagnetic wave

Question 5

Equation for light

Answer 5

• E = hv
• h = 6.63 x 10^-34 J-s
  v = frequency

Question 6

de Broglie’s wave equation

Answer 6

wavelength = h / mv (mass x velocity)

Question 7

Lyman’s Series

Answer 7

• results in ultraviolet emission of lines

- electron goes from n>=2 to n=1

Question 8

Balmer series

Answer 8

• results in visible emission of lines

- electron goes from n>=3 to n=2

Question 9

Paschhen series

Answer 9

• results in infrared emission of lines

- electron goes from n>=4 to n=3

Question 10

Brackett series

Answer 10

• results in infrared emission of lines

- electron goes from n>= 5 to n=4

Question 11

Schrodinger Equation

Answer 11

predicts analytically and precisely the probability of events or outcome, predicts the probability of finding the particle

Question 12

Heisenberg Uncertainty Principle

Answer 12

it is impossible to calculate both the momentum and the speed of an electron in an atom, only possible to calculate the probability of finding an electron

Question 13

orbital

Answer 13

indicates electron’s probable location

Question 14

node

Answer 14

an area of an orbital having zero electron probability

Question 15

ground state

Answer 15

lowest possible energy state of an atom or molecule

Question 16

excited state

Answer 16

any state of a particle or system of particles that has a higher energy than that of its ground state

Question 17

Pauli Exclusion Principle

Answer 17

no two electrons can have the same set of four quantum numbers

Question 18

Aufbau Principle

Answer 18

electrons fill orbitals starting at the lowest available energy state before filling higher states

Question 19

Hund’s Rule

Answer 19

single electron with the same spin must occupy each equal energy orbital before additional electrons with opposite spins can occupy the same orbital

Question 20

paramagnetic

Answer 20

• atom has unpaired electrons

- attracted to a magnetic field due to unpaired electron

Question 21

diamagnetic

Answer 21

• all electrons are paired

- weakly repelled by magnetic fields

Question 22

principal quantum number (n)

Answer 22

as n increases, the orbital becomes larger- electron has a higher energy level and is less tightly bounded to the nucleus

Question 23

angular momentum number (l)

Answer 23

• values from 0 to n-1
• defines shape of orbitals
• 0 is S. 1 is P, 2 is D, and 3 is F

Question 24

magnetic quantum number

Answer 24

• determines orientation of orbital

- values from -l to +l

Question 25

spin quantum number

Answer 25

either -1/2 or +1/2

Question 26

atomic radius

Answer 26

• increases as you move down

- decreases as you move right

Question 27

shielding effect

Answer 27

lessening of attractive electrostatic charge difference between the nuclear protons and valence electrons by partially or fully filled inner shells

Question 28

effective nuclear charge

Answer 28

attractive positive charge of nuclear protons acting on valence electrons

Question 29

anion radius

Answer 29

• larger than respective atoms

- electron electron repulsion forces them to spread further apart

Question 30

cation radius

Answer 30

• smaller than respective atoms

- less electron electron repulsion, come closer together

Question 31

first ionization energy

Answer 31

energy required to remove the most loosely bound electron from a neutral atom in its GASEOUS state

Question 32

ionization energy

Answer 32

• decreases as you move down (larger atomic radius)

- increases as you move right (smaller atomic radius)

Question 33

electron affinity

Answer 33

• energy released when an atom gains an electron and becomes a negative ion
• decreases as you move down (atomic radius increases)
• increases as you move right (atomic radius decreases)
• greater electron affinity = more negative