Developing a Nuclear Model of the Atom

Question 1

what is John Dalton known for?

Answer 1

creating a new way to describe, explain and visualize the nature of matter

named atoms atoms

Question 2

what is Joseph John known for?

Answer 2

first to discover that an atom is made of smaller components of an atom called electrons

discovers that cathode rays are streams of negatively charges particles called electrons

created an atomic model called the plum pudding which illustrated atoms as positively charged spheres where negatively charged electrons are floating inside

Question 3

what did Henri Becquerel, Marie, and Pierre Curie discover?

Answer 3

discovered that certain elements are radioactive
meaning they naturally emit positive particles/alpha particles, negative particles/beta particles and electromagnetic energy (gamma rays)

Question 4

Explain rutherfords gold foil experiment

Answer 4

the discovery that properties of radioactive emissions student in rutherfords class aimed particles at extremely thin sheets of gold foil

gold foil was surrounded by a zinc sulphide coated screen that produced a flash of light whenever it was struck by an alpha particle

purpose: by noting where the flashes occurred researches could determine if the atoms on the gold foil deflected the particles

Question 5

what is a nuclear model?

Answer 5

a model of the atom in which electrons move around and extremely small positively charged nucleus

this is called the planetary model because the electrons resemble planets in motion

Question 6

what did James Chadwick discover

Answer 6

discovered the neutron

Question 7

what is electromagnetic radiation?

Answer 7

energy in the form of light

oscillating (swinging back and forth), perpendicular (a straight line at an angle of 90° to a given line, plane, or surface) electric (worked by electricity), and magnetic fields, moving through space as waves

Question 8

what is wavelength defined as?

Answer 8

the shortest distance between equivalent points

expressed in meters or nanometres
(1 nm=1 times 10^-9)

as wavelength decreases the frequency increases

amplitude a wave represents intensity and represents that amount of brightness

Question 9

what is frequency in terms of waves?

Answer 9

the number of wave cycles that pass a given point in the unit of time

Question 10

how are wave and frequency related?

Answer 10

are inversely proportional (when one goes up, the other goes down)

Question 11

what are the components of the speed of light?

Answer 11

a product of frequency and wavelength

Question 12

what are photons?

Answer 12

a packet electromagnetic energy

when electromagnetic waves interact with matter they do so in individually separate quantums of energy called photons

Question 13

electromagnetic radiation

Answer 13

a kind of radiation including visible light, radio waves, gamma rays, and X-rays, in which electric and magnetic fields vary simultaneously.

Question 14

radiation

Answer 14

the release of energy as waves that are electromagnetic or as moving particles that are subatomic, mostly high-energy particles that cause ionization (when the number of electrons and protons stop being equal)

Question 15

ionization

Answer 15

ionization, in chemistry and physics, any process by which electrically neutral atoms or molecules are converted to electrically charged atoms or molecules

Question 16

fλ = c

Answer 16

Frequency (f) and wavelength (λ) are joined together fλ = c, where c is the speed of light.

Question 17

What is the value of h in E HV?

Answer 17

h is Planck’s Constant which is 6.626 x 10-34 Js

Question 18

emission spectrum

Answer 18

a series of separate colours of light released by atoms as they lose excited energy

Question 19

quantized

Answer 19

to subdivide something, such as energy into small but measurable increments

Question 20

radii

Answer 20

a straight line from the center to the circumference of a circle or sphere

Question 21

ground state

Answer 21

energy level closest to the nucleus

Question 22

how can an atom absorb energy according to Bohr?

Answer 22

it can clash with a highly energetic particle such as an electron in, a stream of charged particles called an electric current

it can absorb a photon that has an amount of energy equal to the difference between the energy of the orbit it occupies and the higher energy above it

Question 23

orbit

Answer 23

An orbit is a not able to be changed path along which electrons revolve around the nucleus of the atom

Question 24

what is the quantum mechanical model of the atom?

Answer 24

an atomic model in which electrons are treated as having wave characteristics

Question 25

what is the meaning of the word atomic?

Answer 25

relating to an atom or atoms

Question 26

what is atomic orbital?

Answer 26

the space around the nucleus that corresponds to a distinct wavelength

Question 27

what are quantum numbers?

Answer 27

a value used when describing an energy level available to atoms and molecules

an electron in an atom or an ion has four electron numbers to describe its state

Question 28

what is the principal quantum number?

Answer 28

The principal quantum number is (n) which describes the size of the orbital. The principal quantum number therefore indirectly describes the energy of an orbital. The value of n ranges from 1 to the shell containing the outermost electron of that atom.

Question 29

what is a shell?

Answer 29

the main energy level uses to the given value of n (the principal quantum number)

Question 30

what does orbital shape quantum number l stand for?

Answer 30

an integer describes the shape of an atomic orbital within each principal energy level

Question 31

what is a sublevel?

Answer 31

an energy subshell associated with the given value of l (the orbital shape quantum number)
is found in each energy level
designated by letters s p d f
has the same shape but increases the volume at a higher energy level

Question 32

what is volume?

Answer 32

the amount of space that is filled by something

Question 33

what does the magnetic quantum number stand for

Answer 33

uses the integer m to indicate the orientation of the orbital in space around the nucleus

Question 34

what does quantum mean?

Answer 34

the smallest possible discrete unit of any physical property, such as energy or matter

Question 35

physical property

Answer 35

a characteristic you can observe without changing or trying to change the composition of the substance

Question 36

paul exclusion principle

Answer 36

a principle that states that a maximum of two electrons can occupy an orbital and that the electrons must have opposite spines

Question 37

paramagnetic

Answer 37

elements that contain unpaired electrons

Question 38

diamagnetic

Answer 38

elements that contain only paired electrons

Question 39

what does l represent?

Answer 39

represents the shape a region of the electron

Question 40

Quantum Numbers

Answer 40

a number used when defining the energy levels that atoms have

there are four quantum numbers

Question 41

what are the four quantum numbers and what do they stand for?

Answer 41

n, l, ml, ms
n describes the energy level
l describes the sublevels
ml describes the orbital of the subshell
ms describes the spin

Question 42

what are the four sublevel orbitals and what are their shapes

Answer 42

s, p,d,f
s is the shape of a sphere
p is a balloon shape can fit in quadrants 1 and 3, on the x axis, and on the y axis

Question 43

orbitals

Answer 43

circle around the nucleus where electrons are held

Question 44

spin quantum number

Answer 44

the quantum number is represented using ms, and it specifies the orientation of the axis on which the electron is spinning (up or down using 1/2)

if arrow is facing down, it is -1/2

if arrow is facing up, it is 1/2

Question 45

Pauli Exclusion Principle

Answer 45

a principle that exclaims that a maximum of two electrons can occupy an orbital and each orbital block representing the spin of the electrons clockwise and counterclockwise must have opposite spins