Electron Configurations

Question 1

Electromagnetic Spectrum

Answer 1

The range of all types of electromagnetic radiation (light)

Question 2

Speed of light

Answer 2

C = 3.0 x 10^8 m/s

Question 3

Wavelength

Answer 3

The distance between two peaks of a wave, specifically electromagnetic radiation. (𝝺, measured in m)

Question 4

frequency

Answer 4

How often a peak occurs while a wave passes a specific point. (f, measured in Hz or s^-1)

Question 5

Equation for the wavelength and frequency of light

Answer 5

C = f * 𝝺

Question 6

Energy of light

Answer 6

Energy = 1/𝝺

Question 7

continuous spectrum

Answer 7

How we experience light, it appears as a continuous series of colors with no gaps.

Question 8

emission spectrum

Answer 8

The spectrum of light produced when a gaseous element is exposed to high voltage (or heat) and electrons are energized.

Question 9

absorption spectrum

Answer 9

The spectrum of light produced when a gaseous element that has been heated and cools, and electrons return to lower energy.

Question 10

Line spectra

Answer 10

The emission spectra specific to an element, where only certain wavelengths are emitted.

Question 11

Quantization

Answer 11

Electromagnetic radiation comes in discrete packets or quanta. Quanta are represented only by integers, (think of steps vs a ramp)

Question 12

Photon

Answer 12

a quantum of electromagnetic radiation energy

Question 13

Energy of a photon

Answer 13

E = h x f

Question 14

Planck’s constant

Answer 14

h = 6.63 x 10^-34 j/s

Question 15

Energy levels

Answer 15

fixed distances from the nucleus of an atom where electrons may be found

Question 16

Energy of a orbital

Answer 16

En = -Rh (1/n^2)

Question 17

Rydberg constant

Answer 17

Rh = 2.18 x 10^-18 j

Question 18

Quantum numbers

Answer 18

All of the values used to describe the energy of an electron

Question 19

Principal quantum number

Answer 19

n, the distance and energy of an orbit

Question 20

Ground state

Answer 20

the most stable formation for an atom, where electrons are at their lowest energy level

Question 21

excited state

Answer 21

when an electron moves up one or more orbitals

Question 22

Number of electrons in n=1

Answer 22

2

Question 23

Number of electrons in n=2

Answer 23

8

Question 24

Number of electrons in n=3

Answer 24

18

Question 25

Number of electrons in n=4

Answer 25

32

Question 26

Heisenberg uncertainty principle

Answer 26

states that it is impossible to precisely know the location and speed of an electron simultaneously

Question 27

Schrodinger’s wave function

Answer 27

used to describe the electrons in an atom based on a probability density function. Electron’s have a high likelihood of occupying a region in space called an atomic orbital.

Question 28

Atomic orbital

Answer 28

An area where electrons have a high likelihood of occupying a region in space

Question 29

S orbital

Answer 29

sphere shaped, can hold 2 electrons

Question 30

p orbital

Answer 30

dumbbell shaped, there are 3 p orbitals per energy level, each can hold 2 electrons for a total of 6.

Question 31

d orbital

Answer 31

flower shaped, there are 5 orbitals per energy level, each can hold 2 electrons for a total of 10.

Question 32

Degenerate orbitals

Answer 32

Orbitals with the same energy are degenerate (same principal quantum number and orbital shape).

Question 33

Orbital diagrams

Answer 33

Electrons represented by arrows, in orbitals represented by boxes.

Question 34

Electron confirgurations

Answer 34

A way to represent the location of electrons in an atom, either as a diagram or written out.

Question 35

Pauli exclusion principle

Answer 35

Electrons also must have opposite spins if they are in the same orbital so one arrow is up and the other down to represent this

Question 36

Hund’s rule

Answer 36

every degenerate orbital in a sublevel is singly occupied and all electrons in singly occupied orbitals have the same spin

Question 37

Aufbau principle

Answer 37

electrons are added to an atom’s lowest energy orbital first. You will only need to know up to 4p!

Question 38

Condensed electron configuration

Answer 38

A short hand representing inner core electrons with the noble gas from the row above

Question 39

Exceptions to the Aufbau rule

Answer 39

Transition metals will fill or half fill 3d before 4s. Cu: 4s13d10 and Cr: 4s13d5

Question 40

Period

Answer 40

the rows of the periodic table

Question 41

Group

Answer 41

column of the periodic table

Question 42

Isoelectronic species

Answer 42

Atoms with identical electron configurations, will be a series of cations, an element and anions.

Question 43

Metal

Answer 43

generally have three or fewer valence electrons, which are delocalized

Question 44

Nonmetal

Answer 44

generally have four or more valence electrons, which are NOT delocalized

Question 45

Metalliod

Answer 45

show hybrid metallic and non-metallic character. The touch the zig-zag line shown on the table.