Unit 3 (Atomic Theory)

Front 1

What are subatomic particles

Back 1

Protons

Neutrons

Electrons

Front 2

Protons

Back 2

Charge of +1

Mass of 1 amu

Found in nucleus

Front 3

What is amu

Back 3

Atomic mass unit

Front 4

Electrons

Back 4

Charge of -1

Mass of 0 amu (1/1800)

Found in the space outside a nucleus

Front 5

Neutrons

Back 5

Charge of 0

Mass of 1 amu

Found in nucleus

Front 6

What is the atomic number

Back 6

The number of protons found in the nucleus of an atom

(Also electrons)

Front 7

Isotopes

Back 7

Atoms of the same element, with the same number of protons, but different numbers of neutrons

Front 8

Atomic mass

Back 8

Protons + Neutron

Front 9

Ions

Back 9

When an atom loses or gains an electron

Front 10

Radioactivity

Back 10

When substances spontaneously wmit radiation

Front 11

Nuclear reactions

Back 11

Reactions that involve a change in the atom's nucleus

The atom the one element can change into the atom of another element

Front 12

Radiation

Back 12

The Ray's and particles emitted by the radioactive material

Front 13

radioactive decay

Back 13

unstable nuclei lose energy by emitting radiation in a spontaneous process (doesn't require energy)

Front 14

alpha radiation

Back 14

radiation that is positive

Front 15

alpha particles

Back 15

contains 2 protons and 2 neutrons, 2+ charge

Front 16

nuclear equation

Back 16

show the atomic number and mass number of particles involved

Front 17

Beta radiation

Back 17

Radiation that deflects towards the positively charged plate

Front 18

Beta particles

Back 18

Radiation that consists of fast-moving electrons called beta radiation

Electron with -1 charge

Front 19

Gamma radiation

Back 19

Gamma rays are high-energy radiation that possess no mass

No electrical charge

not deflected by electric or magnetic fields

Front 20

Nuclear stability

Back 20

An atom's stability is determined by its ratio of neutrons to protons

Front 21

Electromagnetic radiation

Back 21

Form of energy that exhibits wavelike Behavior as a travels through space

Front 22

Examples of electromagnetic radiation

Back 22

Visible light, microwaves, x-rays, radio, television waves

Front 23

Wavelength

Back 23

Shortest distance between equivalent points on a continuous wave

Front 24

Units of wavelength

Back 24

Meters, centimeters, nanometers

Front 25

Frequency

Back 25

The number of waves that pass a given point per second

Front 26

Amplitude

Back 26

The waves height from the original to Crest or from origin to a trough

Front 27

Electromagnetic spectrum

Back 27

Encompasses all forms of electromagnetic radiation with the only differences in the types of radiation being their frequencies and wavelengths

Front 28

Quantum theory

Back 28

The description of the properties of atoms using wave properties

Based on the idea that we can only predict the probability of finding an electron in a particular position

Front 29

Who's model is this and what is it called

Back 29

Dalton's model

Marble model

Front 30

What what Dalton's theory (marble model)

Back 30

All matter is made of indivisible and indestructible atoms

Atoms of a given element are identical in their properties

Atoms of different elements have different properties

Law of multiple proportions

Front 31

Law of multiple proportions

Back 31

Atoms of different elements combine in simple whole number ratios to form compounds

Front 32

What was Dalton's conclusion (marble model)

Back 32

Law of conservation of mass

Front 33

Law of conservation of mass

Back 33

Atoms cannot be subdivided, created, or destroyed when they are combined, separated or arranged in chemical reactions

Front 34

Who's model is this and what is it called?

Back 34

J. J. Thompson's model

Plum Pudding model

Front 35

What was J.j. Thompson's conclusion

Back 35

Negatively charged electrons embedded and ball positive positive charge

Front 36

Robert a millikan

Back 36

Used Thompson's work to determine the exact charge and mass of an electron

Front 37

Ernst Rutherford experment?

Back 37

Gold foil experienment

Front 38

Ernst Rutherford theory

Back 38

The positive particles would deflect as they Struck the positive spheres of the plum pudding model atom

Front 39

Ernst Rutherford conclusion

Back 39

Most of the atom is empty space

Adams have a solid core called the nucleus

Nucleus are positively charged

They measure the approximate size of the nucleus

Front 40

Back 40

Rutherford model

Front 41

Back 41

Bohr model

Front 42

Neil Bohr

Back 42

Electrons would be found only in specific energy levels, similar to the rungs on a ladder

Energy levels closer to the nucleus have a lower energy from those further away

The difference in energy between anyone level and the next called a Quantum

Front 43

atom

Back 43

basic unit of matter

Front 44

elements

Back 44

a substance in which all the atoms are exactly the same