Chemistry Definitions Test Questions – Flashcards
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| What does WHIMIS stand for ? |
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| Workplace Hazardous Materials Information System |
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| Workplace Hazardous Materials Information System (WHIMIS) |
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| System of easy-to-see warning symbols on hazardous materials, designed to help protect people who use hazardous materials at work. |
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| What does MSDS stand for ? |
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| Material Safety Data Sheets. |
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| Material Safety Data Sheets (MSDS) - |
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| Information sheet on a hazardous product used in workplaces, including schools; identifies the chemical and physical hazards associated with the product. |
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| Physical Properties |
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| Properties that describe the physical appearance and composition of a substance. |
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| Chemical Properties |
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| Properties that describe the reactivity of a substance. |
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| Pure Substances |
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| Substances in which all the particles are identical. |
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| Element |
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| Pure substance that cannot be broken down into other substances; substances made up of only one atom. |
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| Compound |
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| Chemical combination of two or more elements in a specific ratio. |
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| Mixture |
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| Combination of pure substances. |
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| Mechanical Mixture |
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| Mixture in which the different substances are visible. |
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| Heterogeneous Mixture |
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| Mixture in which the different substances are visible. |
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| Homogeneous Mixture |
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| Mixture in which the different substances are not visible. |
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| Suspension |
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| Mechanical mixture in which the components are in different states. |
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| Colloid |
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| Mechanical mixture in which the suspended substance cannot be easily separated from the other substances in the mixture. |
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| Solution |
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| Mixture in which the separate components are not visible. |
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| Chemical Reaction |
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| Process that occurs when a substance or substances react to form a different substance or substances. |
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| Physical Change |
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| Change to a substance in which the composition of a substance stays the same. |
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| Chemical Change |
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| Change to a substance that always results in the formation of a different substance or substances. |
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| Salting |
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| Method of drying food to preserve it; salt draws water out of the food. |
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| Fermentation |
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| Biochemical preservation technique involving bacteria. |
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| Atom |
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| Smallest part of an element that still has the properties of the element. |
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| Law of Conservation of Mass |
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| Total mass of the reactants in a chemical reaction equals the total mass of the products. |
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| Electron |
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| Negatively charged particle in the atom that occupies energy levels around the nucleus. |
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| Nucleus (In Atoms) |
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| Positively charged centre of the atom made up of protons and neutrons. |
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| Nucleon |
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| Subatomic particles in the nucleus of the atom; protons and neutrons. |
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| Proton |
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| Positively charged particle in the nucleus of an atom. |
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| Neutron |
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| Neutral particle in the nucleus of an atom. |
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| Metal |
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| Shiny, malleable, ductile element. |
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| Ductile |
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| Description of a substance that can be drawn or stretched into long wires. |
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| Inert |
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| Unreactive with all but the most corrosive of acids. |
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| Non-Metal |
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| One of the 17 elements with varying properties that are completely different from metals. |
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| Molecule |
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| Group of non-metallic atoms bound together by covalent bonds; can be made up of atoms of the same element or atoms of different elements. |
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| Metalloid |
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| Element with properties intermediate between metals and non-metals. |
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| Period |
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| Horizontal line or row in the periodic table; numbered 1-7. |
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| Group |
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| Vertical column of elements in the periodic table; numbered from 1-18; also called family. |
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| Family |
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| Vertical column of elements in the periodic table; numbered from 1-18; also called group. |
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| Alkali Metals |
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| Soft, shiny, silvery elements, very reactive with water; group 1 in the periodic table. |
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| Alkaline-Earth Metals |
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| Shiny, silvery metals, not as soft as the alkali metals; group 2 in the periodic table. |
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| Noble Gases |
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| Extremely unreactive non-metals; group 18 in the periodic table. |
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| Halogens |
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| Non-metals in group 17 in the periodic table; fluorine, chlorine, bromine, and iodine. |
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| Salts |
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| Compound produced in a neutralization reaction between an acid and a base. |
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| Atom |
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| Smallest part of an element that still has the properties of the element. |
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| Energy Level |
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| Region of space near an atom's nucleus that may be empty or may contain electrons; electrons in energy levels nearest the nucleus have the lowest energy. |
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| Atomic Number |
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| Number of protons in an atom; can be used to specify an element. |
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| Isotopes |
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| Atoms of the same element containing different numbers of neutrons. |
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| Mass Number |
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| Integer equal to the toal number of protons and neutrons in the nucleus of an atom. |
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| Atomic Molar Mass |
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| Average molar mass of an element's atoms, including those of all the element's different isotopes. |
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| Ionization |
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| Process of an atom gaining or losing electrons. |
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| Ion |
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| Electrically charged atom or group of atoms. |
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| Cations |
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| Positively charged ion. |
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| Anions |
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| Negatively charged ion. |
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| Valence Electrons |
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| Electron in the outermost energy level of an atom. |
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| Valence |
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| Tendency of an atom to gain or lose electrons. |
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| Valence Number |
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| Number of electrons an element can gain or lose to combine with other elements. |
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| Atomic Number |
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| Number of protons in an atom; can be used to specify an element. |
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| Isotopes |
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| Atoms of the same element containing different numbers of neutrons. |
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| Mass Number |
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| Integer equal to the toal number of protons and neutrons in the nucleus of an atom. |
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| Atomic Molar Mass |
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| Average molar mass of an element's atoms, including those of all the element's different isotopes. |
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| Ionization |
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| Process of an atom gaining or losing electrons. |
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| Ion |
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| Electrically charged atom or group of atoms. |
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| Cations |
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| Positively charged ion. |
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| Anions |
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| Negatively charged ion. |
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| Valence Electrons |
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| Electron in the outermost energy level of an atom. |
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| Valence |
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| Tendency of an atom to gain or lose electrons. |
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| Valence Number |
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| Number of electrons an element can gain or lose to combine with other elements. |
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| Octet Rule |
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| Atoms bond in such a way as to have eight electrons in the valence energy level; also called the rule of eight. |
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| Another name for Octet Rule. |
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| Another name for Rule of Eight. |
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| Crystal Lattice |
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| Organized array of ions. |
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| Formula Unit |
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| Smallest amount of an ionic compound with the composition shown by the chemical formula; number of positive and negative ions in the smallest whole-number ratio that results in a neutral unit in the crystal lattice of a compound. |
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| Ionic Bond |
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| Type of bond formed when electrons transfer between metals and non-metals. |
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| Multivalent Element |
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| Element with more than one stable ion. |
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| Polyatomic Ion |
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| Charged particle made up of several non-matallic atoms joined together. |
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| Covalent Bond |
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| Bond formed when non-metallic atoms share electrons; atoms in a molecule are bound together by covalent bonds. |
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| Molecule |
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| Group of non-metallic atoms bound together by covalent bonds; can be made up of atoms of the same element or atoms of different elements. |
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| Molecular Element |
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| Element that forms molecules made up of only of its own atoms. |
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| Diatomic Molecule |
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| Molecule composed of two atoms of the same element. |
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| Polar |
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| Description of an object that has a positive electric charge at one end and a negative charge at the other; water molecules are slightly _____. |
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| Electrolyte |
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| Solution that conducts electricity; ionic compounds are excellent electrolytes. |
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| Precipitate |
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| Solid with a low solubility that forms a solution. |
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| Precipitation (In Solutions) |
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| Process of forming a solid from a solution. |
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| Acid |
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| Substance that produces hydrogen ions (H+) when disolved in water; compound that dissolves in water to form a solution with a pH lower than 7 (at 25?C). |
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| Base |
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| Substance that produces hydroxide ions (OH-) in water; compound that dissolves in water to form a solution with a pH greater than 7 (at 25?C). |
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| pH |
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| Measure of the number of hydrogen ions in a solution; indicates how acidic or basic a substance is. |
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| Buffer |
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| Substance that keeps the pH of a solution nearly constant despite the addition of a small amount of acid or base. |
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| Universal Indicator |
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| Mixture of several indicators that change colour as the acidity of a solution changes. |
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| Neutral |
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| Description of a substance that is neither acidic nor basic; solution with a pH of 7 (at 25?C) |
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| Neutralization |
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| Process in which acids and bases react with each other so that the H+ ion and OH- ion combine to make a single water molecule; both acidic and basic properties disappear. |
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| Addiction |
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| Physical dependance on a drug. |
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| Reactant |
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| Substance that reacts in a chemical reaction to form another substance or substances. |
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| Product |
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| New substance produced in a chemical reaction. |
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| Exothermic Reactions |
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| Chemical reaction that releases energy, usually in the form of heat, light or electricity. |
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| Combustion |
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| Exothermic chemical reaction that occurs when oxygen reacts quickly with a substance to form a new substance or substances. |
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| Endothermic Reaction |
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| Chemical reaction that absorbs energy. |
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| Law of Conservation of Mass |
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| Total mass of the reactants in a chemical reaction equals the total mass of the products. |
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| Chemical Equation |
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| Record of a chemical reaction using chemical symbols and formulas; shorthand way of showing the results of a chemical reaction. |
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| Formula Equation |
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| Chemical equation that uses the chemical formulas of reactants and products in a chemical equation to represent a chemical reaction. |
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| Skeleton Equation |
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| Formula equation showing the identify of each substance involved in a chemical reaction; does not show the correct proportions of the reactants and the products. |
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| Formation Reaction |
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| Chemical reaction in which two elements combine to form a compound; also known as a synthesis reaction. |
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| Synthesis Reaction |
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| Chemical reaction in which two elements combine to form a compound; also known as a formation reaction. |
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| Skeleton Equation |
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| Formula equation showing the identify of each substance involved in a chemical reaction; does not show the correct proportions of the reactants and the products. |
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| Decomposition Reaction |
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| Chemical reactions in which a compound breaks apart into its elements. |
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| Hydrocarbon |
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| Compound that contains hydrogen and carbon; common hydrocarbons include the main components of gasoline (a mixture of many liquid hydrocarbons) and many plastics. |
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| Single Replacement Reactions |
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| Chemical reaction in which a reactive element reacts with an ionic compound. |
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| Double Replacement Reactions |
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| Chemical reaction between two ionic compounds in solution that often results in the formation of at least one precipitate. |
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| Mole |
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| Quantity that chemists use to measure elements and compounds; symbol: mol; Avogadro's number is the number of particles in a mole. |
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| Avogadro's Number |
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| Number of atoms in 1 mol; approximately 6.02 X 10^23; symbol: N^^A. |
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| Molar Mass |
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| Mass od one mole of a substance. |
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| Atomic Molar Mass |
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| Average molar mass of an element's atoms, including those of all the element's different isotopes. |
