Chem 1 Test 1

Front 1

Atoms

Back 1

Submicroscopic particles that constitute the fundamental building blocks of ordinary matter.

Front 2

Molecules

Back 2

Two or more atoms joined in a specific geometric arrangements

Front 3

Three states of matter (Classification according to state)

Back 3

Solids

Liquid

Gas: compressible, take up shape and volume of container.

Front 4

Two types of solids

Back 4

Crystalline: atoms/molecules are arranged in patterns with long-range, repeating order

Amorphous: Atoms/molecules don't have long range order.

Front 5

Classification according to composition

Back 5

Matter -- Broken down into 2 kinds (Does the sample differ from one sample to another?)
a) Pure substances

b) Mixtures

Pure substances -- Broken down into 2 parts (Does the sample differ from one area of sample to another?)
a) Elements

b) Compounds

Mixtures -- Broken down into 2 parts
a) Homogeneous

b) Heterogeneous

Front 6

Physical Change

Back 6

Changes that only alter the state or appearance, not the composition. Ex. Boiling of water

Front 7

Chemical Change

Back 7

Changes that alter chemical composition. Ex. Decomposition of iron atoms in an Iron by oxygen molecules in the air, to form iron oxide.

Front 8

Physical properties

Back 8

Physical: It's the property a substance can display without changing its composition. Ex. odor, taste, color, appearance, melting point, boiling point, density

Front 9

Chemical properties

Back 9

Chemical: It's a property a substance displays ONLY by changing its composition via a chemical change. Ex. corrosives, flammability, acidity, toxicity.

Front 10

Kinetic/Potential

Back 10

Kinetic energy: energy associated with motion

Potential energy: energy associated with position or composition.

Front 11

Matter

Back 11

Anything that occupies space and has mass.

Can be classified according to its state or composition

Front 12

Substance

Back 12

It is a specific instance of matter, such as air, water, or sand.

Front 13

Three important atomic laws

Back 13

1) Law of conservation of mass

2) Law of definite proportions

3) Law of multiple proportions

Front 14

Law of conservation of mass

Back 14

In a chemical reaction, matter is neither created nor destroyed.

Total mass of the substances involved in a reaction does not change.

Front 15

Law of definite proportions

Back 15

All samples of a given compound, regardless of their source or how they were prepared, have the same proportions of their constituent elements.

Compounds occur in fixed proportions, while components of a mixture could be present in any proportion.

Front 16

Law of multiple proportions

Back 16

When two elements, A and B, with two different compounds, the masses of element B combine with 1g of element A can be expressed as a ratio of small whole numbers.

So when 2 elements combine, their ratio can be expressed in small, whole number ratios. CO2

Front 17

Difference between "Law of definite proportions" and "Law of multiple proportions"

Back 17

Definite: Two or more samples of sample compounds, and states the ratio of one element to another is always the same

Multiple:Two different compounds containing same elements.

Front 18

Atomic Theory

Back 18

a) Each lement is composed of tiny, indestructible particles called atoms

b) All atoms of a given element have same mass and other properties that distinguish them from the atoms of a different element

c) atoms combine in simple, whole numbers to form compounds

d) atoms of one elements cannot change into atoms of another element. In a chemical reaction, atoms only change they way they are bound to another atoms to form a new substance.

Front 19

J. J. Thomson

Back 19

Discovered electrons by the use of Cathode Rays in a Cathode Tube.

Front 20

Robert Miller

Back 20

Discovered charge of a single electron.

Front 21

Radioactivity

Back 21

The emission of small energetic particles from the core of certain unstable atoms. Three different types discovered, Alpha (positive, most massive), Gamma, and Beta.