unit 3

Question 1

Nucleon

Answer 1

A particle that exists in the nucleus (protons and neutrons.)

Question 2

Nuclear charge

Answer 2

The net positive charge of the nucleus, equal to the number of protons in the nucleus.

Question 3

Ion

Answer 3

A charged atom or group of atoms formed by the gain or loss of
electrons. Protons and electrons are a different number.

Question 4

Anion vs Cation

Answer 4

A negatively charged ion vs A positively charged ion

Question 5

Emission Spectrum

Answer 5

the spectrum of frequencies of electromagnetic radiation emitted due to an atom or molecule making a transition from a high energy state to a lower energy state. The frequencies can be used to determine the identity of an element.

Question 6

Excited State vs. Ground State

Answer 6

A condition where and atom’s electrons occupy higher energy levels than
they normally would due to absorption of energy vs A condition where an atom’s electrons are occupying the lowest possible
energy states

Question 7

Orbital Notation

Answer 7

Also called “box diagrams”, these schematics describe the location and
spin of every electron in an atom

Question 8

Photon

Answer 8

An infinitesimally small particle that travels in a wave-fashion that is released when electrons fall from the excited state into the ground state.
It is also known as a packet of light-energy or quanta

Question 9

Planck’s Constant (h)

Answer 9

A proportionality constant that converts Hz (frequency) to J (energy). It is
6.63 X 10-34 J . sec

Question 10

Quantum Numbers

Answer 10

A four-digit series of numbers that identifies the location of a specific
electron around the nucleus based on PEL, sublevel, orbital and spin.

Question 11

Sublevel

Answer 11

Regions of space that electrons occupy making up a principal energy level. Number of orbitals will determine sublevel type

Question 12

Stable octet

Answer 12

An electron configuration that is reached when atoms gain, lose or share
electrons in an attempt to get a noble gas electron configuration of eight valence electrons. Helium is an exception to this “Rule of Eight”.

Question 13

Wavelength (λ)

Answer 13

The distance from one peak to the next in a wave. Measured in nanometers.

Question 14

Frequency

Answer 14

The number of wavelengths that pass a fixed point per second.

Question 15

Democritus

Answer 15

thought atoms were small hard spheres, infinite in number, and called them Atomos(uncuttable).

Question 16

Aristotle

Answer 16

Opposed Democritus’ model and thought everything was made out of four elements (earth, water, fire, air). He thought atoms were wrong because they were uncuttable (even by gods), and that opposed the idea that gods could do anything. His theories were more accepted.

Question 17

John Dalton

Answer 17

Revived Democritus’ ideas, and had the same model, but his theory was what counted (Dalton’s atomic theory).

Question 18

Dalton’s Atomic Theory

Answer 18

All matter is made of tiny invisible particles called atoms
atoms of the same element are identical
different atoms combine in whole # ratios to form new compounds
Chemical reactions involve the REARRANGEMENT of atoms

Question 19

Joseph John Thompson

Answer 19

discovered the first subatomic particle, the electron, while studying cathode rays. His magnet both attracted while negative and pushed away while positive, meaning that there must be smaller particles that attract and repel. Also discovered that the electron was 2000x smaller than atom

Question 20

Ernie Rutherford

Answer 20

was a student of Thompson, and wanted to expand on his theories. Used the gold foil experiment to find out that most of an atom was empty space, but w/ a small & hard nucleus (w/ a positive charge).

Question 21

Gold foil experiment

Answer 21

Rutherford’s experiment that proved the existence of the nuclear atom He shot positive alpha particles at gold foil, with most passing through. He proved: 1. existence of the nucleus 2. The positive charge of the nucleus 3. The atom is mostly empty space

Question 22

Neils Bohr Model

Answer 22

used light and photon experiments, and found that electrons moved around the nucleus in fixed PELs.

Question 23

Erwin Schrodinger

Answer 23

Realized that Bohr’s model was slightly incorrect, as the exact place of electrons can’t be measured, but have areas of high probability called ORBITALS/probability clouds. They appear in the wave particle/quantum mechanical model/electron cloud model, and have different energy levels.

Question 24

Valence electrons

Answer 24

electrons in the outermost PEL’s S/P sublevels

Question 25

atomic mass / AMUs

Answer 25

1/12 the mass of a C-12 atom, the approximate mass of protons and
neutrons.

Question 26

Isotopes

Answer 26

an atom with a non-typical amount of neutrons in its nucleus (which changes atomic mass but not charge)

Question 27

SPDF sublevel notations

Answer 27

A reflect the modern atom model, which include regions of probability and sublevels within orbitals (S, P, D, F). the number of PELs tells you how many orbitals it has.

Question 28

principle quantum #

Answer 28

The energy level that an electron is in, represented with n. e.g. n=1, n=2, etc

Question 29

Aufbau Principle

Answer 29

shows that the lower PELs and sublevels fill before the next ones, and shown in a graph form that should be WRITTEN ON EVERY TEST

Question 30

Noble Notations

Answer 30

the most recent noble gas in [] + the extra PELs in SPDF notation

Question 31

The Hund Rule

Answer 31

all orbitals of a sublevel must be occupied before doubling up

Question 32

Pauli Exclusion Principle

Answer 32

electrons occupying the same orbital must spin in opposite directions

Question 33

Electron Maximums

Answer 33

the max number of electrons that an orbital can hold

Question 34

Spectral line patterns

Answer 34

patterns emitted by photons of a certain pattern. A spectral line pattern can be used to identify which elements the substance contains because all the spectral lines will match up with the element(s) it contains.

Question 35

red wavelength nm

Answer 35

700

Question 36

orange wavelength nm

Answer 36

620

Question 37

yellow wavelength nm

Answer 37

570

Question 38

green wavelength nm

Answer 38

520

Question 39

blue wavelength nm

Answer 39

470

Question 40

indigo wavelength nm

Answer 40

420

Question 41

violet wavelength nm

Answer 41

400