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| Anything that occupies space and has mass. |
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| Cannot be divided by ordinary chemical processes into another substance. |
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| Each element is referred to by its chemical symbol, derived from its name in English, Latin or Greek. |
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| Smallest unit of an element that retains the unique properties of the element. |
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| Has an atomic mass of one and a positive charge. |
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| Has an atomic mass of one and a neutral charge. |
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| Protons and neutrons grouped in the center of the atom. |
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| Protons and neutrons together determine the atomic weight of an atom. |
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| These have a negative charge and remain in constant motion around the nucleus of the atom. |
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| Equal to the number of protons in the atom. |
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| An atom that has developed a positive or negative charge by gaining or losing an electron. |
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| An atom that has a positive electrical charge such as sodium. |
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| An atom that has a negative electrical charge such as chloride. |
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| Atoms that exist that contain a different number of neutrons. |
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| This isotope spontaneously emits particles of energy at a constant rate and, therefore, changes into a stable, nonradioactive element. |
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| The area around the nucleus of an atom where the electrons have their most likely position. |
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| Atoms joined together by chemical bonds. The smallest unit of a compound (ie. table salt or NACl) that retains the properties of that compound. |
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Definition
| Occurs between two atoms that are sharing or transferring electrons between them. |
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| The bond formed when atoms share electrons. Single bonds are formed when atoms share one electron, double bonds are formed when atoms share two electrons, and triple bonds are formed when atoms share three electrons. |
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Definition
| The bond formed when electrons are transferred from one atom to another. |
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| Two atoms drawn to each other by their respective electrical charges. |
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| The bond between hydrogen atoms already covalently bonded in a molecule to oppositely charged particles. A type of weak ionic bond that is weaker than covalent or ionic bonding. |
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Definition
| The formation and breaking of chemical bonds. |
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Definition
| The way in which a reaction is described in writing. Shows the molecular formula of the reactants (X and Y) and the products (Z) and the direction of the reaction (shown by an arrow). X+Y --> Z |
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Definition
| A new more complex chemical is made from multiple, simple chemicals. O+O --> O2 |
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| A single complex chemical is broken into multiple, simpler chemicals. 2 H2O --> 2H2 + O2 |
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Definition
| Atoms are exchanged between molecules. It is a combination of a synthesis and decomposition reaction. NaHCO3 + HCl --> NaCl + H2O + CO2 |
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| The energy required for a chemical reaction to happen. |
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| Special proteins that hold reactants together so they may interact. |
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| Molecules that do not contain hydrocarbon groups and often have ionic bonding. They include water, salts, acids and bases. |
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| Molecules that contain hydrocarbon groups and are usually covalently bonded. They include carbohydrates, lipids, proteins, and nucleic acids. |
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| Chemicals added to a solvent. |
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| The result of combined solutes and a solvent. |
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| What solutes are added to. Water is the universal solvent. |
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| Chemicals that dissolve or mix well in water. |
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| Molecules that do not mix well with water. |
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| Mineral compounds that have ionic bonds. |
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| Salts in their ionic form that have the ability to transmit an electrical charge. |
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