Chem #1

Front 1

macroscopic

Back 1

shows us the physical things large enough to be examine by the naked eye.

Front 2

microscopic

Back 2

shows us things that cannot be seen with the naked eye. (what the macroscopic world is made of)

Front 3

forensic chemistry - interdisciplinary

Back 3

relates to branches of science such as biology, geology, physics, and psychology

Front 4

states of matter

Back 4

solid, liquid, gas

Front 5

solid

Back 5

-particles are closely packed
-limits motion
-cannot be compressed
highest potential energy, lowest kinetic energy

Front 6

liquid

Back 6

-particles are slightly apart
-moves with more freedom
-hard to compress
-little potential energy, high kinetic energy

Front 7

gas

Back 7

-particles are far apart
-moves very freely
-easily compressed
-least potential energy, most kinetic energy

Front 8

scientific method

Back 8

techniques to examine things. observation, hypotheses, experiment

Front 9

chemical properties

Back 9

ability to change to different substance

Front 10

physical properties

Back 10

characteristics of a substance when no chemical change occurs

Front 11

penny

Back 11

-changes in compositions.

Front 12

positive slope

Back 12

direct relationship, y =kx

Front 13

negative slope

Back 13

indirect relationship, y=k/x

Front 14

horizontal line

Back 14

slope = 0

Front 15

vertical line

Back 15

undefined, x doesn't change

Front 16

independent variable

Back 16

x

Front 17

dependent variable

Back 17

y

Front 18

Aluminium (Al)

Back 18

solid, atomic number = 13, boron group (metal), insoluble in water, recyclable, nonmagnetic, nonsparking, never found in its element state

Front 19

weight

Back 19

mass + gravity

Front 20

mass

Back 20

quantity of matter (kg, g, lbs..) <-- units

Front 21

matter

Back 21

anything that has volume and mass

Front 22

gravity

Back 22

force of attraction between all matter

Front 23

inertia

Back 23

resistance to change

Front 24

potential energy

Back 24

energy associated with position
energy stored
(mgh)
chemical bonds are a source of potential energy

Front 25

kinetic energy

Back 25

energy in motion
KE = 1/2 mv2 (mvsquared)

Front 26

distillation

Back 26

a method of separating mixtures based on differences in their temperature in a boiling liquid mixture

Front 27

evaporation

Back 27

the slow vaporization of a liquid and the reverse of condensation. A type of phase transition, it is the process by which molecules in a liquid become gaseous.

Front 28

filtration

Back 28

used to separate particles and fluid, where the fluid can be a liquid or a gas.

Front 29

chromatography

Back 29

a process used for separating mixtures by differences in absorbency

Front 30

protons

Back 30

subatomic particle with positive electric charge

Front 31

electrons

Back 31

subatomic particle with negative electric charge

Front 32

neutrons

Back 32

neutral. found in the atomic nuclei

Front 33

subatomic particles

Back 33

particles that make up atoms

Front 34

atom

Back 34

basic building block of matter
elements are made of atoms
small particle of an element that has the properties of that element.

Front 35

elements

Back 35

simplest pure substance
cannot be changed into simpler substance by heating or any chemical process.

Front 36

compounds

Back 36

pure substances that are the unions of two or more elements. they can be broken into simpler substances by chemical means

Front 37

allotropes

Back 37

a structurally different form of an element; "graphite and diamond are allotropes of carbon"

Front 38

do all elements combine the same way?

Back 38

no.

Front 39

water

Back 39

oxygen is bigger, therefore the electrons are pulled towards it (gravity).
the solid form of water is less dense than the liquid.

Front 40

diatomic

Back 40

a molecule made up of two atoms

Front 41

molecule

Back 41

smallest part of a compound that retains the properties of that compound

Front 42

molecular compound

Back 42

a compound held together by covalent bonds (sharing of electrons between atoms)

Front 43

ionic compound

Back 43

when ions are held together by ionic bonds (transfer of electrons)

Front 44

noble gases

Back 44

a group of chemical elements with very low chemical reactivity.
they have a full shell of electrons, therefore then don't bond, they're on their own.

Front 45

volume

Back 45

takes up space and has mass
how much space an object occupies
use water to measure unusual shapes

Front 46

homogeneous mixture

Back 46

A mixture that is uniform throughout, and has only one phase. one sample is like the rest

Front 47

heterogeneous mixture

Back 47

a mixture where the substances aren't equally distributed. samples are different to each other.

Front 48

alloys

Back 48

metal dissolved in metals

Front 49

physical changes

Back 49

change in one or more physical properties. no change in composition

Front 50

chemical changes

Back 50

change in the fundamental components of substances. given substance changes into different substances. "reactions"

Front 51

chemical properties

Back 51

ability to change to different substance

Front 52

physical properties

Back 52

characteristics of a substance when no chemical change occurs.

Front 53

mixtures

Back 53

two or more substances that are not chemically combined with each other and can be separated by chemical means. The substances in a mixture retain their individual properties.

Front 54

solutions

Back 54

one substance dissolves into another. best mixed of all mixtures. always has a substance that is dissolved (solute) and another that does the dissolving (solvent)

Front 55

universal solvent

Back 55

water

Front 56

air

Back 56

solution of oxygen and other gases dissolved in nitrogen.

Front 57

colloids

Back 57

particles are mixed together but not dissolved. particles are constantly colliding, conducting light and seem cloudy.