Chapter 2&3 Vocab-AP Bio-Neidermeyer
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missvalerieann on October 10, 2009
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46 terms
Terms | Definitions |
|---|---|
 Matter | that which has mass and occupies space |
| Element | A substance that cannot be broken down into simpler substances by chemical reactions. |
| Neutrons | subatomic particle with no charge |
| Protons | a subatomic particle with a positive charge |
| Electrons | a subatomic particle that has a negative charge; orbits the nucleus |
| Atomic Nucleus | area where protons and neutrons are tightly packed together at the center of an atom. |
| Atomic Number | number of protons |
| Mass Number | the sum of protons and neutrons in an atom |
| Isotopes | atoms of the same element that have different numbers of neutrons |
| Energy | the ability to cause changes in matter; the ability to do work |
| Potential Energy | the energy that matter possesses because of its location or structure. |
| Chemical Bonds | atoms staying close together by attraction |
| Covalent Bonds | the sharing of a pair f valence electrons by two atoms |
| Molecule | two or more atoms held together by covalent bonds |
| Ionic Bond | occurs whentwo atoms are so unequal in their attraction for valence electrons that the more electronegative atom strips an electron completely away from its partner. |
| Ion | a charged atom |
| Nonpolar Covalent Bond | a bond in which electrons are shared equally |
| Cation | positively charged atom |
| Anion | negatively charged atom |
| Hydrogen Bond | forms when a hydrogen atom covalently bonded to one electronegative atom is also attracted to another electronegative atom. |
| Polar Covalent Bond | A covalent bond between atoms that differ in electronegativity. The shared electrons are pulled closer to the more electronegative atom, making it slightly negative and the other atom slightly positive. |
| Polar Molecule | unequal distribution of electrons |
| Cohesion | when hydrogen bonds hold a substance together. |
| Adhesion | the clinging of one substance to another |
| Surface Tension | a measure of how difficult it is to stretch or break the surface of a liquid. |
| Kinetic Energy | the energy of motion. |
| Heat | a form of energy. |
| Temperature | a measure of heat intensity that represents the averagekinetic energy of the molecules. |
| Specific Heat | of a substance; the amount of heat that must be absorbed or lost for 1g of that substance to change its temperature by 1 degree C. |
| Solution | a liquid that is a completely homogeneous mixture of two or more substances |
| Solute | substance that is dissolved |
| Solvent | the dissolving agent of a solution |
| Evaporative Cooling | occurs because the "hottest" molecules, those with the greatest kinetic energy, are the most likely to leave as a gas. |
| Hydrophilic | a substance that has an affinity for water |
| Hydrophobic | substances that are nonionic and nonpolar that repel water |
| Acid | a substance that increases the hydrogen ion concentration of a solution. |
| Heat of Vaporization | the quantity of heat a liquid must absorb for 1g of it to be converted from the liquid to the gaseous state. |
| Hydrogen Ions | a single proton with a charge of 1+ |
| Hydroxide Ions | single proton with a charge of 1- |
| Base | a substance that reduces the hydrogen ion concentration of a solution. |
| Buffers | substances that minimize changes in the concentrationof H+ and OH- in a solution. |
| Acid Precipitation | rain, snow, or fog with a pH lower (more acidic) than pH 5.2. |
| pH Scale | In any aqueous solution at 25 degrees C, the product of the H+ and OH- concentrations is constant at 10-(14) |
| Compound | a substance consisting of two or more different elements combined in a fixed ratio. |
| Trace Elements | elements required by an organism in only minute quantities. Some are needed by all forms of life, others are needed by only certain species |
| Atom | the smallest unit having the properties of its element |
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