Chemistry

Front 1

Can be observed without changing the composition of the material (color, size, shape, transparency, density, hardness, texture, melting point, boiling point, ect.)
Do not produce a new material

Back 1

Physical (Property of Matter)

Front 2

Can only be observed by changing the composition of the material (iron rust, hydrogen explodes in oxygen to form water, zinc reacts with acids to produce hydrogen gas)
Do produce a new material

Back 2

Chemical (Property of Matter)

Front 3

One that has a uniform composition throughout and always has a single phase; also called a solution
--clear

Back 3

Homogenous Mixture

Front 4

one that does not have a uniform composition and in which the individual substances remain distinct
not clear ( has particles)

Back 4

Heterogeneous Mixture

Front 5

~ Length- meter- m
~ Mass- kilogram- kg
~ Time- Second- s
~ Thermodynamic Temp.
~ Kelvin- K
~ Amount of Substance- mole- mol
~ Luminous Intensity- Candela- cd

Back 5

SI Units- Fundamental Units

Front 6

|error| /accepted value x 100

Back 6

Percent error

Front 7

was the first person to propose the idea that matter was not infinitely divisible, but made up of individual particles called atomos

Back 7

Democritus

Front 8

revived the idea of the atom in the early 1800s based on numerous chemical reactions

Back 8

Dalton

Front 9

conservation of mass in a reaction as the result of the combination, separation, or rearrangement of atoms

Back 9

Daltons Atomic Theory

Front 10

measured the effects of both magnetic and electric fields on the cathode ray to determine the change- to- mass ratio of charged particles, then compare it to known values

Back 10

Thomson

Front 11

Received the Nobel prize in 1906 for identifying the first subatomic particle- the electron

Back 11

Thompson

Front 12

Studied how positively charged alpha particles interacted with solid matter

Back 12

Rutherford

Front 13

Used the oil-drop apparatus to determine the charge of an electron

Back 13

Millikan

Front 14

Received a Nobel prize in 1935 for discovering the existence of neutrons

Back 14

Chadwick

Front 15

A fundamental principle of classical physics that matter cannot be created or destroyed in an isolated system

Back 15

Laws of Conservation of Matter

Front 16

radiation that originates from the cathode and travels to the anode of a cathode- ray tube

Back 16

Cathode Ray

Front 17

the primary factor in determining an atom’s stability is its ratio of neutrons and protons

Back 17

Nuclear Stability

Front 18

 The radiation that was deflected toward the negatively charged
 Two protons and two neutrons (2+)

Back 18

Alpha Radiation

Front 19

 The radiation that was deflected toward the positively charged plate
 Electron (1-)

Back 19

Beta Radiation

Front 20

 High-energy radiation that possesses no mass

Back 20

Gamma Radiation

Front 21

the splitting of nuclei

Back 21

Fission

Front 22

the combining of nuclei

Back 22

Fusion

Front 23

is the minimum amount of energy that can be lost or gained by an atom

Back 23

Quantum

Front 24

the phenomenon in which electrons are emitted from a metal’s surface when light of a certain frequency shines on it

Back 24

Photoelectric Effect

Front 25

states that it is impossible to know both the velocity and the position of a particle at the same time

Back 25

Heisenberg Uncertainly Principle

Front 26

originally applied to the hydrogen atom, it led to the quantum mechanical model of the atom

Back 26

Schrodinger wave equation

Front 27

the modern model of the atom that treats electrons as waves

Back 27

Quantum Mechanical Model of the Atom

Front 28

the lowest allowable energy state of an atom

Back 28

Photon

Front 29

A figure indicating the relative sizes and energies of atomic orbital

Back 29

Principal Quantum Number

Front 30

elements from group 1, 2, and 13-18 in the modern periodic table, possessing a wide range of chemical and physical properties

Back 30

Representative Elements

Front 31

the energy required to remove an electron from a gaseous atom

Back 31

Ionization Energy

Front 32

indicates the relative ability of an element’s atoms to attract electrons in an chemical bond

Back 32

Electro Negativity

Front 33

proposed an explanation for atoms react with other to form certain kinds of ions and molecules- octet rule

Back 33

Gilbert Lewis

Front 34

both atoms share electrons- but not equally

Back 34

Polar Covalent

Front 35

both atoms share electrons- somewhat equally or equally

Back 35

Nonpolar Covalent