Ap Chemistry Mid Term

Front 1

Matter

Back 1

Anything that takes up space and has mass

Front 2

Mass

Back 2

Makes up matter

Front 3

Energy

Back 3

Ability to do work or cause change

Front 4

Law of conservation of energy

Back 4

No energy is created nor destroyed in a chemical reaction

Front 5

Mixture

Back 5

two or more substances which have been combined such that each substance retains its own chemical identity.

Front 6

Solution

Back 6

a liquid mixture in which the minor component (the solute) is uniformly distributed within the major component (the solvent).

Front 7

Density

Back 7

Mass/ volume

Front 8

Kelvin

Back 8

Celsius + 273

Front 9

Prefixes

Back 9

Giga 10(9)
Mega 10(6)
Kilo 10(3)
Deci 10(-1)
Centi 10(-2)
Milli 10(-3)
Micro 10(-6)
Nano 10(-9)
Pico 10(-12)

Front 10

Accuracy

Back 10

How many times you hit a certain target

Front 11

Precision

Back 11

How close or far away your aim is from one another

Front 12

Compound

Back 12

two or more chemical elements are chemically bonded together

Front 13

Physical properties

Back 13

Changes the identity of the substance
Extensive properties:
Mass
Volume
Length
Shape
Intensive properties:
Color
Taste
Melting/boiling point
Density
Luster
Hardness

Front 14

Chemical properties

Back 14

Doesn't change the identity of substance
How it reacts with:
Air
Water
Acid
Bases
Other chemicals

Front 15

Significant figures

Back 15

Significant if:
Non zero numbers
Zeros between non zeros
Trailing zeros after the decimal
Not significant if:
Leading zeros
Adding/ subtracting:
Keep the lowest amount
Multiplying/ dividing:
Keep the smallest decimal

Front 16

Scientific notation

Back 16

1.4 X 10(2)
*add the exponents

Front 17

Democritus

Back 17

Formulated the atomic theory

Front 18

John dalton

Back 18

Atomic theory

Front 19

Lavoisier

Back 19

Father of modern chemistry

Front 20

Law of conservation of mass

Back 20

Mass of the reactants equals the mass of the products

Front 21

Law of definite proportions

Back 21

Law stating that every pure substance always contains the same elements combined in the same proportions by weight

Front 22

Law of multiple proportions

Back 22

law stating that when two elements can combine to form more than one compound the amounts of one of them that combines with a fixed amount of the other will exhibit a simple multiple relation

Front 23

Cathode Ray

Back 23

JJ Thomson
tube used by Thomson is a sealed glass container in which two electrodes are separated by a vacuum. When a voltage is applied across the electrodes, the rays are generated, creating a glowing patch where they strike the glass at the opposite end of the tube. Through experimentation, Thomson discovered that the rays could be deflected by an electric field (in addition to magnetic fields, which was already known). He concluded that these rays, rather than being waves, were composed of negatively charged particles he called "corpuscles" (they would later be renamed electrons by other scientists).

Front 24

Millikens oil drop expieriment

Back 24

The experiment entailed balancing the downward gravitational force with the upward drag and electric forces on tiny charged droplets of oil suspended between two metal electrodes. Since the density of the oil was known, the droplets' masses, and therefore their gravitational and buoyant forces, could be determined from their observed radii. Using a known electric field, Millikan and Fletcher could determine the charge on oil droplets in mechanical equilibrium. By repeating the experiment for many droplets, they confirmed that the charges were all multiples of some fundamental value

Front 25

Gold-foil experiment

Back 25

Rutherford
Shot delta rays through a piece of gold foil and the ray bounced everywhere showing that there isn't a pool of electrons but they are in orbitals

Front 26

Plum pudding

Back 26

Protons and electrons are spread around like a blueberry muffin

Front 27

Nuclear

Back 27

The nucleus is positively charged with electrons surrounding it

Front 28

The amount if protons

Back 28

How can you tell elements from one another

Front 29

A- mass number
X- chemical symbol
Z- atomic number

Back 29

A
ZX

Front 30

Elements

Back 30

Protons=electrons
Mass number= protons/electrons + neutrons
Neutrons= mass number - protons/ electrons

Front 31

Isotopes

Back 31

Different number of neutrons

Front 32

Ions

Back 32

Different number of electrons

Front 33

Mendeleev

Back 33

Crested the periodic table by atomic mass

Today it is in atomic number

Front 34

Mole

Back 34

6.022 x 10(23) atoms, particles, molecules/ 1 mol of a substance

Front 35

Molar mass

Back 35

1 mol of a substance
Mol----> mass
Mass----> mol

Front 36

Ionic compounds

Back 36

Have at least one metal

Front 37

Molecular compounds

Back 37

Prefixes in the nomenclature

Front 38

Transition metals

Back 38

They get the Roman numerals in their names

Front 39

Formula mass

Back 39

CH(4) ---> 12 + 4 = 16

Front 40

Percent composition

Back 40

CH (4)
12/16 x 100 = 75%

Front 41

Synthesis

Back 41

A + B ---> AB

Front 42

Decomposition

Back 42

AB ---> A + B

Front 43

Combustion

Back 43

C (x) H (y) + O (2) ---> CO (2) + H(2)O

Front 44

Acid / Base

Back 44

Acid + Base ---> salt + H(2)O

Front 45

Single replacement

Back 45

Al +NaCl ---> AlCl (3) + 3Na

Front 46

Double replacement

Back 46

AB + CD ---> AD + CB