Term
|
Definition
| The study of the properties and behavior of matter. |
|
|
Term
|
Definition
| anything that has mass and occupies space. |
|
|
Term
|
Definition
| Any characteristic that allows us to recognize a particular type of matter to distinguish it from other types. |
|
|
Term
|
Definition
about 100 very basic substances
- Cannot be decomposed into simpler substances. |
|
|
Term
|
Definition
| The most infitesimally small building blocks of matter. |
|
|
Term
|
Definition
- which two or more atoms are joined together in specific shapes
- 1.Minor differences in the composition of molecules can lead to big differences in their chemical properties. |
|
|
Term
|
Definition
|
|
Term
|
Definition
| has no fixed volume or shape, it conforms to the volume and shape of its container. Spaced far apart and moving at high speeds |
|
|
Term
|
Definition
| Has a distinct volume independent of its container but has no specific shape.The molecules are packed tightly but are moving rapidly, and can slide over each other. |
|
|
Term
|
Definition
- Distinct shape and volume.
- Molecules can only wiggle slightly in their rather fixed positions. |
|
|
Term
| Pure Substance (Substance) |
|
Definition
| matter hat has distinct properties and a composition that does not vary from sample to sample. |
|
|
Term
|
Definition
| substances composed of two or more elements; they contain two or more kinds of atoms. |
|
|
Term
|
Definition
| combinations of two or more substances in which each substance retains its own chemical identity. |
|
|
Term
|
Definition
| two-atom molecules, like oxygen and hydrogen. |
|
|
Term
| Law of Constant Composition |
|
Definition
| The elemental composition of a pure compound is always the same. |
|
|
Term
|
Definition
| Has the same appearance and composition of molecules throughout the mixture. |
|
|
Term
|
Definition
| can be observed without changing the identity or composition of the substance. |
|
|
Term
|
Definition
| describe the way a substance may change or react, to form other substances. E.g. flammability, the ability of a substance to burn in the presence of oxygen. |
|
|
Term
|
Definition
| Some properties such as temperature, melting point, and density. THey do not depend on the amount of the sameple being examined and are particularly useful in chemistry because many lf these properties can be used to IDENTIFY substances |
|
|
Term
|
Definition
| depend on the quantity of the sample, with two examples being mass and volume. Extensive properties relate to the AMOUNT of substance present. |
|
|
Term
|
Definition
| a substance is transformed into a chemically different substance. |
|
|
Term
|
Definition
| a substance changes its physical appearance but not its composition. |
|
|
Term
|
Definition
| Mixtures can be seperated by taking advantages of the properties of the different molecules. For example, in a gold and iron mixture, the iron could get pulled out with a magnet, or an acid could dissolve one of the two. |
|
|
Term
| How many sig figs in one number? |
|
Definition
1.Zeros between nonzero digits are always significant e.g 1005 or 1.03.
2.Zeros at the beginning of a number are never significant, they indicate the position of the decimal point; .02 grams has one sig fig, .0026 g has 2 sig figs.
3.Zeros at the end of a number are significant if the number contains a decimal point. |
|
|
Term
|
Definition
1.We have 1.01 L of water, + 1 L
2.We can only use the lowest number of decimal places in our answer, in this case it is 1. This means we have 2 L as our answer. |
|
|
Term
|
Definition
1.We only care about the number of sig figs, not decimal places.
2.So 2.04 x 3.1 = 2.262, but only 2 sig figs because of 3.1, so its 2.3 |
|
|
Term
|
Definition
| A factor that is equal to 1 that you can multiply a unit by to get the equivalent amount in a different unit. |
|
|
Term
| Law of Definite Proportions |
|
Definition
1.If two elements A and B combine to form more than one compound, then the masses of B that can combine with a given mass of A are in the ratio of small whole numbers.
There cannot be fractions of atoms. |
|
|
Term
| John Dalton Atomic Theory |
|
Definition
1. Elements are composed of tiny particles called atoms (True)
2. All atoms of a given element are identical to the other ones (Not True; isotopes.
3. Atoms of one element cannot be changed into other elements, no creation or destruction (Not true, radiation, Hadron Collider.
4. Atoms combine to form compounds, a given compound has the same relative number of atoms. |
|
|
Term
|
Definition
| Greek for "indivisible or uncuttable" Democritus bypothesized that the world was made of these more than a thousand years ago. |
|
|
Term
| J. J. Thompson Experiments |
|
Definition
| Used cathode ray tubes to deduce the charge of electrons, and that they had a mass. Finding either the charge or the mass would yield the other. |
|
|
Term
| Millikan's Oil Drop Experiment |
|
Definition
| Suspended a drop of oil between two charged plates. FOund that charge of a single electron to be 1.602 * 10^-19 Coulombs, and the charge to mass ratio to be 1.76 *10^8 C/g |
|
|
Term
|
Definition
| Spontaneous emission of high-energy radiation, Lead Marie Curie and her husband to isolate the radioactive components of the compound. |
|
|
Term
| Alpha, Beta, Gamma Particles |
|
Definition
| High energy particles investigated by Rutherford. Alpha particles are essentially protons and the nucleus, beta particles are the electrons, and gamma particles are the neutrons. |
|
|
Term
|
Definition
| Shot alpha particles through a thin gold foil. Most passed through, many were bent, and some even shot right back. This showed that the nucleus of the atom was very dense with a large electron cloud. Nucleus was positive and extremely dense. |
|
|
Term
| Charge and Mass of Protons, Neutrons, Electrons |
|
Definition
Proton - Positive (+1) charge, 1.0073 amu.
Neutron - No charge, neutral, 1.0087 amu.
Electron - Negative (1-), 5.486 *10^-4 amu. |
|
|
Term
| amu to gram conversion factor |
|
Definition
|
|
Term
|
Definition
| Number of protons in an element |
|
|
Term
|
Definition
|
|
Term
|
Definition
Same protons, different # of neutrons.
The different isotopes of an atom are what composes the ATOMIC WEIGHT on the PERIODIC TABLE. |
|
|
Term
|
Definition
| Made form a metal and a nonmetal, two ions, like ZnO or NiCl2 |
|
|
Term
|
Definition
| Ions that have gained electrons, usually nonmentals. |
|
|
Term
|
Definition
| Ions that have lost an electron, usually metals. |
|
|
Term
| Molecular/Empirical Formula |
|
Definition
| Molecular formula is how everything binds and shows more accurate composition, Emprical formula is basically the lowest common factor of the molecular formula. |
|
|
Term
|
Definition
| Bonds between Nonmetals, follow a specific naming pattern. |
|
|
Term
| Covalent Bond Nomenclature |
|
Definition
| It has the prefixes mono-, di-, tri-, tetra-, etc. |
|
|
Term
|
Definition
Periods are the horizontal rows.
Groups are the vertical rows |
|
|
