Term
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Definition
-Small simple substances without carbon
-Groups are: water, simple salts, simple bases, simple acids |
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Term
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Definition
-Carbon-containing compounds (Carbon: associated with life processes/existence)
-Generally large and complex
-Examples: carbohydrates, lipids, protein, and nucleic acids |
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Term
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Definition
| Substances that can't be broken down into simpler substances by ordinary chemical reactions |
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Term
| Important Roles of Elements O, C, H, and N |
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Definition
-Most abundant in organisms: 96% of mass
Oxygen: Required for cellular respiration; present in most
organic compounds
Carbon: Forms backbone of organic molecules; each carbon atom can form four bonds with other atoms
Hydrogen: Present in most organic compounds; component of water
Nitrogen: Component of proteins and nucleic acids + chlorophyll in plants |
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Term
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Definition
| The smallest unit of an element that retains that element's chemical properties |
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Term
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Definition
| Proton (+), Neutron (0), Electron (-) |
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Term
| Atomic Number and Atomic Mass |
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Definition
| -Number of Protons and number of Neutrons + Protons |
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Term
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Definition
-Atoms of the same element with varying atomic masses/number of neutrons
-e.g. hydrogen, duterium (2 amu, 1 neutron), tritium (3 amu, 2 neutrons) |
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Term
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Definition
| Unstable isotope that emits radiation that emits radiation that can be detected by autoradiography on photographic film |
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Term
| Practical Applications of Radioisotopes |
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Definition
| Archaeological dating, agricultural plant studying, smoke detectors |
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Term
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Definition
| -Atoms of different elements combined in a fixed ratio |
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Term
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Definition
-Between non-metals
-Covalent bonds |
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Term
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Definition
Describes chemical composition: what types of atoms are present and how many
-e.g. glucose- C6H1206 |
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Term
| Chemical Reactions (how they are described) |
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Definition
By chemical equations!
Reactant (C6H1206) + Reactant (602) ---> Products (6C02 + 6H20 + Energy) |
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Term
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Definition
Represents a certain amount of chemical energy
-Formation of chemical bond: energy stored
-Break of chemical bond: release of energy |
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Term
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Definition
-Atoms share valence electrons
-Strong bond
-Non-polar covalent bonding: H2 |
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Term
| Covalent Bonds in Biologically Important Molecules |
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Definition
| -Hydrogen (H): 1. Oxygen: 2. Carbon: 4. Nitrogen: 3. Sulfur: 2 |
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Term
| Polar Covalent Bond / Non-Polar Covalent Bonds |
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Definition
Polar: Bonds between atoms that differ in electronegativity .
Non-polar: No differ in electronegativety (almost mostly same element) |
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Term
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Definition
The measure of at atom's attraction for electrons in chemical bonds
-Higher in oxygen, then sulfur, then hydrogen |
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Term
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Definition
| Electrically-charged atom or group of atoms. Anion: (-), Cation: (+). |
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Term
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Definition
| Formed by the attraction between the charges of an anion and a cation |
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Term
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Definition
-Hydrogen (H) combines with an electronegative atom
-Generally weak bonds, but important in living organisms
-When bonds are collective, very strong, e.g. water. In water, polarity allows water molecules to form hydrogen bonds with each other |
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Term
| Van Der Waals Interactions |
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Definition
| -A weak attractive force between atoms or molecules caused by an instantaneous dipole moment of one atom or molecule that induces a similar temporary dipole moment in adjacent atoms or molecules. |
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Term
| Water Molecule Importance |
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Definition
-All living organisms require water
-Cells are surrounded by water
-Cells are 70%-95% water |
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Term
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Definition
| -Cohesion (similar molecules sticking together), Surface Tension, -Adhesion (dissimilar molecules sticking together) and cappilary action |
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Term
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Definition
| Occurs because of inter-molecular attractive forces between the liquid and solid surrounding surfaces. If the diameter of the tube is sufficiently small, then the combination of surface tension (which is caused by cohesion within the liquid) and adhesive forces between the liquid and container act to lift the liquid |
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Term
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Definition
-Allows liquid to resist external force
-Molecules at water's surface produce a strong layer as they are pulled downward by the attraction (cohesion) of the water molecules below |
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Term
| Specific Heat/Water's Specific Heat |
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Definition
The amount of heat that must be absorbed or lost for 1g. of that substance to change it's temperature by 1 degree C
-Specific heat of water higher than usual; heat absorbed when hydrogen bond break, heat is released when bond forms |
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Term
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Definition
| The heat a liquid must absorb for 1 g. to be converted into gas |
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Term
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Definition
-Ice has more stable hydrogen bonds
-Less dense
-Rings with holes in it cause it to take up more volume |
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Term
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Definition
Base: H+ < OH-. Acid: H+ > OH-.
Bases donate OH or accept H in aqueous solutions, acids donate H+ in aqueous solutions |
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