Atomic Theory Definitions Chapter 3

Question 1

A positively charged subatomic particle found in the nucleus of atoms

Answer 1

Proton

Question 2

A variety of atoms of an element, Atoms of this variety have the same number of protons as all atoms of the element, but a different number of neutrons

Answer 2

Isotope

Question 3

A neutral(unchanged) subatomic particle present in the nucleus of atoms

Answer 3

Neutron

Question 4

the release of electrons from a substance due to light striking the surface of a metal

Answer 4

Photoelectric Effect

Question 5

A small discrete, invisible quantity(Plural quanta); A quantum of light is a photon; a burst of some energy

Answer 5

Quantum

Question 6

A quantum of light energy, A stream of energy packets(quanta)

Answer 6

Photon

Question 7

A technique for analyzing spectra; the spectra may be visible light, infrared, ultraviolet, x-ray, and other types

Answer 7

Spectroscopy

Question 8

A series of bright lines of light produced or emitted by a gas excited by heat or electricity

Answer 8

Bright-Line/Emission Spectrum

Question 9

A series of dark lines of a continuous spectrum; is produced by placing a gas between the continuous spectrum source and the observer; also known as a dark line spectrum

Answer 9

Absorption Spectrum

Question 10

A stable energy state of an atomic system that does not involve any emission of radiation

Answer 10

Stationary State

Question 11

The jump of an electron from one stationary state to another

Answer 11

Transition

Question 12

Electrons do not radiate energy while orbiting the nucleus

Answer 12

Bhor’s First Postulate

Question 13

Electrons can change energy by undergoing a transition from one stationary state to another

Answer 13

Bhor’s Second Postulate

Question 14

A region of space around a nucleus where an electron is most likely to be found

Answer 14

Orbital

Question 15

Main energy level, number n(quantum numbers), corresponds to the periodic table for s and p groups

Answer 15

Shell

Question 16

Orbitals of different shapes and energies, given by the quantum number

Answer 16

Subshell

Question 17

when electrons are added to an atom, they go into the lowest energy available and fill the levels in order of increasing energy level until electrons run out

Answer 17

Aufbau Principle

Question 18

No two electrons in an atom can have the same 4 numbers(quantum); no two electrons in the same orbital have the same spin; only two electrons with opposite spins can occupy an orbital

Answer 18

Pauli Exclusion Principle

Question 19

states that one electron occupies each of several orbitals at the same energy level before a second electron can occupy the same orbital

Answer 19

Hund’s Rule

Question 20

A method for communicating the location and number of electrons in electron energy levels

Answer 20

Electron Configuration

Question 21

The metals and non-metals in the main blocks, S and P blocks

Answer 21

Representative Elements

Question 22

The metals in groups 3-12; elements filling d-orbitals with electrons

Answer 22

Transition Elements

Question 23

The 14 metals in each of periods 6 and 7 that range in atomic numbers 57-70 and 89-102 respectively; elements filling f-block

Answer 23

Lanthanides and Actinides

Question 24

It is impossible to simultaneously know the exact position and speed of a particle

Answer 24

Heisenberg Uncertainty Principle

Question 25

The current theory of atomic structure based on wave properties of electrons; Also known as wave mechanics

Answer 25

Quantum Mechanics

Question 26

A mathematical or graphical representation of the chance of finding an electron in a given space

Answer 26

Electron Probability Density

Question 27

Created the plum pudding model aka the Raison Bun model, atoms make up of electrons scattered unevenly within an elastic sphere surrounded by a soup of positive charges to balance the electron’s charge

Answer 27

J J Thomson

Question 28

Performed the gold foil experiment to discover a positively charged nucleus, and concluded that the atom’s nucleus consists of positively charged subatomic particles, called protons. Used alpha particles in the experiment.

Answer 28

Ernest Rutherford

Question 29

introduced the idea that particles such as electrons could be also described as waves. “If a wave can behave like a particle, then a particle can behave as a wave.”

Answer 29

De Brogile

Question 30

hypothesized that energies from oscillating atoms in the heated object were multiples of a small quantity of energy. The light was emitted in bursts of energy in waves rather than as a continuous stream

Answer 30

Planck

Question 31

Electrons can change(gain or lose energy) their energy by undergoing a transition from one transition state to another

Answer 31

Bhor

Question 32

the electron can only have certain(quantized) energies because of the requirements for only whole numbers of wavelengths of the electron. Suggested the energy of hydrogen electrons was quantized because of its specific orbit. Therefore since electron energy has certain values, changes in energy also have certain values.

Answer 32

Schrodinger

Question 33

-Weak attraction to magnetic fields
-Unable to retain magnetic properties when a field is removed
-Domains are randomly oriented
-Examples: Oxygen, Lithium, Chlorine…

Answer 33

Paramagnetisim

Question 34

-Strong attraction to magnetic fields
-Able to retain magnetic properties when a field is removed
-Domains are lined up creating a “permanent magnet”
-Examples: Iron, Cobalt, Nickel

Answer 34

Ferromagnetism

Question 35

Anything under Copper and Chromium, Has half-filled shells for example copper has 4s1 and chromium has 4s1. The other electron is promoted to the 3d orbital

Answer 35

Anomalus