The chemical reactions that occur inside the human body are extremely complex. One of the main reactions that occurs is the metabolism of glucose, and another reaction is the liver’s detoxification. The metabolism of glucose is one of the main factors that affect the levels of insulin that are generated by the liver. The metabolism of glucose is also related to a person’s risk of developing type 2 diabetes.
The human body produces a lot of glucose. This excess glucose is quickly transported to the cells in the body by the bloodstream and is rapidly processed into glucose. When the body is in an energy deficit, it will try to use any glucose it can find.
The liver then converts the glucose into the ketone body acetoacetate, which has a very powerful detoxifying effect on the body. In addition to the normal conversion process, the liver also produces other substances such as urea, bile salts, and purine.
Chemistry Chapter 11 Chemical Reactions Answer Key
| Term | Definition |
|---|---|
| chemical equation | a symbolic way of describing a chemical reaction |
| skeleton equation | a chemical equation that does not indicate the amounts of substances involved |
| catalyst | a substance that speeds up the rate of a reaction |
| coefficients | numbers used to balance a chemical equation |
| balanced equation | an equation in which each side has the same number of atoms of each element |
| reactants | substances that undergo chemical change |
| products | new substances formed in a chemical reaction |
| combination reaction | a reaction in which two or more substances combine to form a single substance |
| decomposition reaction | reaction in which a single compound is broken down into two or more products |
| single-replacement reaction | reaction in which atoms of one element replace atoms of a second element in a compound |
| combustion reaction | reaction of a compound with oxygen to produce energy |
| complete ionic equation | equation that shows dissolved ionic compounds as free ions |
| spectator ions | ions that do not participate in a reaction |
| net ionic equation | equation that indicates only the particles that take part in a reaction |
| precipitate | solid product of reaction in solution |
| aqueous reaction | reaction that occurs in water |
| ionic solubility rules | used to predict whether a precipitate will form in an aqueous reaction |
| soluble salts | salts of alkali metals and ammonia; nitrate and chlorate salts; sulfate salts (except with Pb2+, Ag+, Hg22+, Ba2+, Sr2+, Ca2+); chloride salts (except with Ag+, Pb2+, Hg22+) |
| insoluble compounds | carbonates, phosphates, chromates, sulfides, hydroxides |
| Avogadro’s Number | another name for mole |
| 6.02×10^23 | mole (in number form) |
| atomic mass | the mass of an element as listed on the periodic table |
| molar mass | number of grams in 1 mole (=to the numerical value of the atomic mass); the mass of a mole of an element |
| standard temperature pressure (STP) | STP |
| molecular formula | gives the exact number of atoms present in a molecule |
| empirical formula | tells the ratio of different elements in a molecule |
| chemical reactions | reactions that involve chemical changes in matter resulting in new substances |
| hv | light symbol |
| shock | mechanical symbol |
| elec | electrical symbol |
| triangle | heat symbol |
| evidence of a chemical change | color change, gas, emission of light, emission of heat, formation of precipitate |
| synthesis | A + B → AB |
| decomposition | AB → A + B |
| single displacement | A + BC → AC + B |
| double displacement | AB + CD → AD + BC |
| synthesis reaction | when two or more reactants combine together to make one product |
| decomposition reaction | one reactant breaks down into two or more products |
| single replacement reaction | one atom displaces another and replaces it in a compound |
| double replacement reaction | two ionic compounds exchange ions |
| combustion reaction | reactant + oxygen → energy released + oxygen-containing products |
| representative particle | atoms, molecules, or formula units in a substance |
| avogadro’s hypothesis | equal volumes of gases at the same temperature and pressure contain equal numbers of particles |
| molar volume | the volume of a mole of an element (22.4 liters) |
| percent composition | the relative amounts of the elements in a compound (not empirical formula) |
Pearson Chemistry: Describing Chemical Reactions
Here is a summary of key terms and concepts related to chemical equations:
- Chemical equation: Symbolic representation of a chemical reaction. Shows the reactants, products, direction of reaction, and relative amounts (coefficients).
- Skeleton equation: Shows only chemical formulas of reactants and products without coefficients.
- Catalyst: Substance that increases the reaction rate but is not consumed.
- Coefficients: Numbers placed in front of chemical formulas in an equation to balance the number of atoms.
- Balanced equation: Equation where the number of atoms of each element is the same on both sides.
- Reactants: Starting substances in a chemical reaction.
- Products: Substances formed by a chemical reaction.
- Combination reaction: Two or more reactants form one product.
- Decomposition reaction: One reactant breaks down to form multiple products.
- Single-replacement reaction: One element replaces another element in a compound.
- Combustion reaction: Reactant combines with oxygen, releasing energy.
- Ionic solubility rules: Used to predict if precipitate will form when mixing aqueous ionic solutions.
- Avogadro’s number: 6.02 x 10^23 items/mole.
- Molar mass: Grams per mole of a substance.
- Empirical formula: Simplest whole number ratio of elements in a compound.
- Chemical change: Bonds are broken and formed, accompanied by energy changes.
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