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Chapter 1-3
Chm101, Test 1, Scruggs, ASU, Ch 1-3
| Term | Definition |
|---|---|
| Matter | anything that occupies space and has mass |
| Matter classifications | 1. pure substances 2. mixtures. |
| Pure Substances | have the same composition throughout, and from sample to sample. can be further classified as either elements or compounds. |
| Elements | a substance that cannot be broken down into simpler substances even by a chemical reaction. |
| Compound | a pure substance composed of two or more elements combined chemically in definite proportions...has properties that are different from those of its component elements. |
| Mixtures | combination of two or more elements or compounds...differs from pure compounds in that their components can be separated by physical processes. ie: Pencil lead, Salt water, Air |
| Mixture Classifications | homogeneous and heterogeneous. Homogeneous mixtures have the same composition throughout. Heterogeneous mixtures do not. |
| Representations of Matter | Macroscopic – we can see with our eyes Microscopic level – a magnification using a microscope. (Down to cell level) Molecular level – a magnification to a level that shows atoms and molecules Atom – the smallest unit of an element; represented as a sin |
| States of Matter | solid, liquid, or gas. |
| physical property of matter | a characteristic that we can observe without changing the composition of a substance. ie. qualitative properties = Color & Odor quantitative properties = Mass, Volume, Density Temperature |
| Physical Changes | a process that changes the physical properties of a substance without changing its chemical composition. Phase changes are physical changes. |
| chemical change | a process where one or more substances are converted into one or more new substances. (Also called a chemical reaction). ie. Pennies tarnishing |
| Chemical Properties | descriptions of the ability of a substance to undergo a chemical change. ie Hydrogen burns easily with oxygen |
| Energy Changes | When chemical or physical changes occur, energy changes also occur. |
| Kinetic energy | energy of motion |
| Potential energy | energy possessed by an object because of its position; stored energy |
| Density | mass/volume |
| Law of Conservation of Mass | Mass is not gained or lost in a chemical reaction |
| Law of Definite Proportions | A compound always has the same relative amounts of the elements that compose it. ie when water is broken down by electrolysis into oxygen and hydrogen, the mass ratio is always 8 to 1. |
| Dalton’s Atomic Theory | All matter is composed of small, indivisible particles, called atoms. All atoms of a given element are identical both in mass and in chemical properties. Atoms are not created or destroyed in chemical reactions. Atoms combine in simple, fixed, whole-numb |
| scanning tunneling microscope | invented in 1981, allows us to create images of matter at the atomic level. |
| Subatomic Particles | Atoms are composed of subatomic particles. The three most important are: Proton Neutron Electron |
| Electron | In 1897 J. J. Thomson’s experiments with cathode-ray tubes showed that matter is composed of negatively charged particles. |
| protons | Scientists reasoned that if atoms have negatively charged particles, they must also have positively charged particles (protons). |
| Nuclear Model of the Atom | In 1907, Earnest Rutherford’s gold foil experiment unintentionally showed that the positively charged protons are located in a tiny core in the very center of the atom, now called the nucleus. The experiment showed that the nucleus of the atom contains mo |
| Neutron | Because the protons in the atom were found to account for only about half the mass of most atoms, scientists knew there was another heavy particle in the nucleus. The neutron, a particle with about the same mass as a proton, but with no charge, was detec |
| Subatomic particles relative charge | Electron= 1- Proton= 1+ Neutron= 0 |
| Atomic Number | The number of protons in an atom of an element |
| Isotopes | An isotope of an element is an atom that contains a specific number of neutrons.Mass Number = # protons + # neutrons |
| Isotope symbols | top left of element symbol |
| Ions | Ions differ from atoms in that they have a charge; the number of electrons is either greater than, or less than, the number of protons. |
| Cations | positively charged. They have fewer electrons than in the neutral atom. |
| Anions | negatively charged. They have more electrons than in the neutral atom. |
| Atomic Mass | We can use mass number to compare the approximate relative masses of different isotopes.the mass number is NOT an actual mass |
| Determination of Atomic Mass | The individual masses of the isotopes of an element can be determined by mass spectrometry. |
| AMU Scale | 1 amu = 1/12 mass of 1 C-12 atom = 1.66061024 g. This means that carbon-12 has a mass of exactly 12 amu. |
| Relative Atomic Mass | The average mass of the individual isotopes of an element, taking into account the natural-occurring relative abundance of each. |
| Periodic Table | shows elements in order of increasing atomic number (#protons), Elements in the same column have similar properties, and are called a group or family. A horizontal row of elements is a period. Elements in the same period have properties that tend to vary |
| Diatomic Molecules | Most elements, except for the noble gases, do not exist as single atoms. |
| Materials | Metals, Semiconductors (Electronics), Polymers (rubber bands, plastics, etc..), Ceramics, Liquid Crystals, Ferrofluids. |
| Ionic Compound | Consists of oppositely charged cations and anions. Usualy the cation is a metal and the anion is a nonmetal or a group of nonmetals. |
| Molecular Compound | Consist of two or more different nonmetals. It exists as a discrete unit of atoms. |
| Polyatomic Ions | Consists of a group of atoms with an overall net charge. |
| Oxoanions | Contain oxygen attached to some other element. |
| Nitrate | NO3 |
| Bicarbonate | HCO3 |
| Bromate | BrO3 |
| Chlorate | ClO3 |
| Iodate | IO3 |
| Cyanide | CN |
| Hydroxide | OH |
| Acetate | C2H3O2 |
| Chromate | CrO42 |
| Sulfate | SO42 |
| Carbonate | CO32 |
| Peroxide | O22 |
| Phosphate | PO43 |
| Ammonium | NH4+ |
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