AP Biology Chapter 2 Keyterms
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shareberry18 on October 1, 2009
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All the key terms in bold. From AP bio Campbell/Reece 7th edition
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41 terms
Terms | Definitions |
|---|---|
 Element | a substance that can not be broken down to other substances by chemical reactions. |
| Compound | A substance consisting of two ore more different elements combined in a fixed ratio. |
| Trace Elements | Required by an organism in only small quantities. |
| Atom | The smallest unit of matter that still retains the properties of an element. |
| Proton | A subatomic particle with a single positive electrical charge, found in the nucleus of an atom. |
| Neutron | an electrically neutral particle found in the nucleus of an atom. |
| Electron | A subatomic particle with a single negative charge. One or more electrons move around the nucleus of an atom. |
| Atomic Nucleus | The center of an atom where the protons and neutrons are located. |
| Dalton | A unit of measurement used for atoms and subatomic particles/molecules. It is named after John Dalton who helped develop the atomic theory in the 1800s. |
| Atomic Number | The atomic # is made up of protons and written as a subscript to the left of the symbol of the element. Tells us both number of protons and electrons. |
| Atomic Mass Number | The sum of protons plus neutrons in the nucleus of an atom. It's written as a subscript to the left of the symbol on top. (23/11 Na; 11 protons/electrons and 12 neutrons) |
| Isotopes | When some atoms have more neutrons than protons in the same element and have greater mass. Behave the same in chemical reactions. |
| Radioactive Isotope | When the nucleus decays spontaneously, giving off particles and energy. |
| Energy | Defined as the capacity to cause change such as work. |
| Potential Energy | The energy that matter possesses because of its location or structure. |
| Energy Levels | The different states of potential energy that electrons have in an atom. It's correlated with distance from nucleus |
| Electron Shells | An energy level represented as the distance of an electron from the nucleus of an atom. |
| Valence Electron | The outermost electrons in the outermost shell. |
| Valence shell | The outermost shell. |
| Orbital | The three-dimensional space where an electron is found 90% of the time. |
| Chemical Bonds | An attraction between two atoms to complete its outer shell, by either sharing or transferring electrons to one another. |
| Covalent bond | Sharing of a pair of valence electrons by two atoms. |
| Molecule | Two or more atoms held together by covalent bonds. |
| Single Bond | A pair of shared electrons. H—H |
| Structural Formula | The notation of H—H, represents both atoms and bonding. |
| Molecular Formula | Example...H little two. Means two atoms of hydrogen have bonded... |
| Double Bond | a double covalent bond so when the two atoms form a molecule by sharing two pairs of valence electrons. |
| Electro negativity | The attraction of a particular kidn of atom for the electrons of a covalent bond. |
| Nonpolar Covalent Bond | When two atoms are equally electronegative and the electrons are shared equally. |
| Polar Covalent Bond | When one atom is bonded to a more electronegative atom and the electrons of the bond are not shared equally. |
| Ionic Bond | When opposite charges, cations and anions, attract each other. |
| Ion | A charged atom/molecule |
| Cation | when the charge is positive |
| Anion | When the charged atom is negative. |
| Ionic Compounds/salts | Compounds formed by ionic bonds. |
| Hydrogen Bond | It forms when a hydrogen atom covalently bonds to one electronegative atom that is also attracted to another electronegative atom. |
| Van Der Waals interactions | Weak attractions between molecules or parts of molecules that are brought about by localized charge fluctuations. |
| Chemical Reactions | The making and breaking of chemical bonds that lead to changes in the composition of matter. |
| Reactants | The starting materials of a chemical reaction |
| Products | The end result of a chemical reaction |
| Chemical Equilibrium | The point at which the reactions offset one another exactly. |
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