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Chem Midterm
| Term | Definition |
|---|---|
| Element | A pure substance of atoms with the same number of protons |
| Compound | A pure substance made of two or more different elements that are chemically combined in a fixed ratio |
| Homogenous Mixture | A single-phase mixture with a uniform composition |
| Heterogeneous mixture | A non-uniform mixture of two or more ingredients or phases |
| Chemical property | A characteristic of matter that becomes evident during or after a chemical change or reaction |
| Physical property | A characteristic that can be observed and measured without changing the chemical identity of a substance |
| Chemical change | A process in which one or more substances are altered into one or more new and different substances |
| Conductivity | The degree to which a specified material conducts electricity is calculated as the ratio of the current density in the material to the electric field that causes the flow of current |
| Density | The mass of substance per unit volume. The amount of “stuff” in a given amount of space |
| Malleable | Able to be hammered or pressed permanently out of shape without breaking or cracking |
| Ductile | The ability of an element to be drawn into a wire |
| Volatile | Easily transitions from a liquid to a gas |
| Aqueous | A solution in which the solvent is water |
| Systematic error | A consistent bias in measurement that leads to results deviating from the true value in a predictable manner |
| Random error | Inconsistent error caused by chance differences that occur when taking repeated measurements |
| Accuracy | How close a measurement is to the true accepted value |
| Precision | The consistency of a set of measurements or results |
| Wafting | A technique used to safely detect the smell of a chemical without directly inhaling it |
| Ion | An atom or molecule with a net electric charge due to the loss or gain of one or more electrons |
| Ionic bond | A type of chemical bond formed due to the electrostatic attraction between oppositely charged ions in a chemical compound |
| Covalent bond | A type of chemical bond that involves the sharing of electron pairs between atoms |
| Isotope | Each of two or more forms of the same element that contain equal numbers of protons but different numbers of neutrons in their nuclei, and hence differ in relative atomic mass but not in chemical property |
| Average atomic mass | The weighted average of the masses of the naturally occurring isotopes of a chemical element |
| Binary compound | A chemical compound that consists of exactly two different elements |
| Polyatomic ion | An ion composed of two or more covalently bonded atoms |
| Transition metal | Any of the set of metallic elements occupying a central block in the periodic table |
| Oxidation numbe r | A positive or negative charge assigned to an atom to indicate its degree of oxidation or reduction |
| Alkali metal | A chemical compound that neutralizes or effervesces with acids and turns litmus blue |
| Alkali earth metal | Any of the six chemical elements in Group 2 of the periodic table |
| Halogen | Reactive nonmetallic elements that form strongly acidic compounds with hydrogen; occupy Group 17 of the periodic table |
| Noble Gas | any of the gaseous elements helium, neon, argon, krypton, xenon, and radon, occupying Group 0 (18) of the periodic table. They were long believed to be totally unreactive, but compounds of xenon, krypton, and radon are now known. |
| Metal | a class of substances characterized by high electrical and thermal conductivity as well as by malleability, ductility, and high reflectivity of light. |
| Non Metal | Nonmetals are elements that do not have typical metal properties such as conductivity, hardness, and ductility. |
| Metalloid | chemical elements whose physical and chemical properties fall in between the metal and non-metal categories. Boron, germanium, silicon, antimony, arsenic, tellurium and pollanium are the seven most widely recognized metalloids |
| Law of conservation of mass | in a chemical reaction, the mass of the products equals the mass of the reactants |
| Coefficient | a numerical value placed directly in front of a chemical formula within a balanced chemical equation. |
| Subscript | small numbers or symbols written below and to the right of a chemical element or formula, which indicate the number of atoms of that element present in a compound |
| Charge balancing | The principle of electroneutrality, where the sum of positive charges must equal the sum of negative charges in a solution |
| Synthesis reaction | a chemical reaction that combines two or more simple elements or compounds to form a more complex product. A + B → AB |
| Decomposition reaction | a chemical reaction with a single reactant that forms two or more products. AB → A + B |
| Single replacement reaction | a chemical reaction where one element replaces another in a compound. It is also known as a single displacement reaction. A + BC → B + AC |
| Double replacement reaction | a chemical reaction in which two reactants exchange ions to form two new compounds. Double displacement reactions typically result in precipitate formation. AB + CD → AD + CB |
| Neutralization reaction | a chemical reaction between an acid and a base that forms a salt and water as products |
| Oxidation reduction reaction | any chemical reaction in which the oxidation number of a molecule, atom, or ion changes by gaining or losing an electron. |
| Oxidation | the loss of electrons during a reaction by a molecule, atom or ion. |
| Reduction | any of a class of chemical reactions in which the number of electrons associated with an atom or a group of atoms is increased |
| Activity series | a list of elements in decreasing order of their reactivity. |
| Molar mass | The mass of one mole of a substance |
| Mole | 6.02214076 × 10^ 23 |
| Avogadro’s number | number of units in one mole of any substance, equal to 6.02214076 × 10 23 |
| Percent composition | the ratio of the amount of each element to the total amount of all individual elements that are available in the given compound and then multiplied by 100 |
| Empirical formula | The simplest whole number ratio of elements present in a compound |
| Molecular formula | formula giving the number of atoms of each of the elements present in one molecule of a specific compound |
| Limiting reactant | The substance that is completely consumed during a chemical reaction, thus determine the maximum amount of product that can be formed |
| Concentration | The amount of substance (solute) dissolved in a specific volume of another substance(solvent) to form a solution |
| Solubility | The degree to which a substance dissolves in a solvent to form a solution |
| Solution | A homogenous mixture of two or more substances where one substance is dissolved in another |
| Solute | Substance that is dissolved in a solvent |
| solvent | A substance, usually a liquid, that dissolves a solute to form a solution |
| Molarity | The number of moles of solute per liter of solution |
| Acid | A substance that donates hydrogen ions or protons in a solution |
| Base | A substance that can accept protons or donate electron pairs |
| pH | A measure of the concentration of hydrogen ions in a solution, indicating whether it is acidic, basic, or neutral |
| pOH | A measure of hydroxide ion concentration in a solution |
| pH indicator | A compound that changes color in response to the acidity or alkalinity of a solution, typically over a narrow range of pH values |
| Salt | A compound form from positively charged ions and negatively charged ions, held together by ionic bonds |
| Weak acid | An acid that partially dissociates in solution meaning there are lower concentration of hydrogen ions compared to strong acids, which fully dissociates |
| Weak base | A base that does not completely dissociate in water, resulting in a solution that contains a small proportion of hydroxide ions and a large proportion of undissociated molecules |
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