Term
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Definition
| the energy stored in chemical bonds |
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Term
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Definition
| a chemical reaction in which a substance reacts rapidly with oxygen (o2) often producing heat and light |
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Term
| double replacement reactions |
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Definition
| a chemical reaction in which two compounds exchange positive ions and form two new compounds |
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Term
| oxidation reduction reactions |
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Definition
| (redox) a chemical reaction in which electrons are transferred from one reactant to another |
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Term
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Definition
| substances that undergo change in a chemical reaction |
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Term
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Definition
| a representation of a chemical reaction in which the reactants ad products are expressed as formulas |
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Term
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Definition
| In a chemical reaction mass can be neither created nor destroyed |
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Term
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Definition
| a chemical reaction that absorbs energy from its surroundings |
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Term
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Definition
| a covalently bonded group of atoms that has a positive or negative charge and acts as a unit |
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Term
| single replacement reaction |
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Definition
| a chemical reaction in which one element takes the place of another element in a compound |
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Term
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Definition
| numbers that appear before a formula in a chemical equation to show the relative proportions of each reactant and product |
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Term
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Definition
| a chemical reaction in which a compound breaks down into two or more simpler substances |
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Term
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Definition
| a chemical reaction that releases heat to its surroundings |
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Term
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Definition
| new substances formed as the result of a chemical reaction |
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Term
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Definition
| a chemical reaction in which two or more substances react to form a single substance |
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Term
| What information do the name and formula of an ionic compound provide? |
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Definition
| The name of an ionic compound must distinguish the compound from other ionic compounds containing the same elements. The formula of an ionic compound describes the ratio of the ions in the compound |
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Term
| What information do the name and fomrula of a molecular compound provide? |
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Definition
| The name and formula of a molecular compound describe the type and number of atoms in a molecule of the compound |
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Term
| What is the law of conservation of mass? |
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Definition
| Mass cannot be created nor destroyed in a chemical reaction |
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Term
| Why must chemical equations be balanced? |
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Definition
| In order for mass to be conserved, the reaction must be balanced. |
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Term
| Why do chemists use the mole? |
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Definition
Because chemical reactions often involve large numbers of small particles, chemists use a counting unit called te mole to measure amounts of a substance.
1 mole = 6,02x10^23 atoms = Avagadros Num |
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Term
| How can you calculate the mass of a reactant or product in a chemical reaction? |
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Definition
| By using a balanced chemical equation and molar masses of the reactants and products. |
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Term
| What are the general types of chemical reactions? (5) |
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Definition
Synthesis
Decomposition
Single Replacement
Double Replacement
Combustion |
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Term
| How did the discovery of subatomic particles affect the classification of reactions? |
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Definition
| It enabled scientists to classify certain reactions as a transfer of electrons between atoms. |
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Term
| What happens to chemical bonds during a chemical reaction? |
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Definition
| Some are broken (reactants) and some new ones are formed (products) |
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Term
| What happens to energy during a chemical reaction? |
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Definition
| Energy is either released or absorbed. If the energy of te bonds formed is less than the energy of the bonds broken, it is exothermic. If the bonds of the products have more energy than the bonds of the reactants, it is endothermic. |
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