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53 Cards in this Set
- Front
- Back
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Define Atom
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the smallest particle of any element that retains the properties of the element.
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Define Element
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a substance that cannot be broken down by chemical means. Elements are defined by the number of protons they possess.
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Define Proton
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Subatomic particles that have a positive (1+) electric charge.
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Define Neutron
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Subatomic particles that do not have an electric charge.
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Electron
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Subatomic particles that have a negative electric charge.
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Oribtal
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Electron cloud having an energy state described by given values of the n, ℓ, and mℓ quantum numbers. An orbital can contain two electrons with paired spins and is often associated with a specific region of an atom.
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Nucleus
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The positively charged central core of an atom, containing most of its mass.
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Charge
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Usually refers to electric charge, which is a conserved property of certain subatomic particles that determines their electromagnetic interaction.
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Combining capacity
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The number of electrons it needs to gain or lose in order to be a stable ion.
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Symbol
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A notation for one of the chemical elements, consisting of letters; for e.
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Atomic number
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The number of protons in the nucleus of an atom, which identifies the element which the atom belongs to.
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Mass Number
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the total number of protons and neutrons found in a nucleus of an atom.
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Family
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Refers to a group of elements with similar chemical properties. Chemical families tend to be associated with the vertical columns on the periodic table.
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Period
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The elements in a horizontal row of the periodic table.
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Alkali metal
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Any of the elements found in Group IA of the periodic table. Alkali metals are very reactive chemical species which readily lose their one valence electron to form ionic compounds with nonmetals.
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Alkaline earth metal
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An element belonging to group 2 of the periodic table. The alkaline earth metals, as a group, share charactertic properties.
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Halogens
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A element located in Group VIIA of the periodic table. Halogens are reactive nonmetals having seven valence electrons.
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Noble gases
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Any of the elements found in Group 8 at the far right of the Periodic Table.
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Inert
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Stable and unreactive under specified conditions.
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Transition Metals
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Any of the metallic elements within Groups 3 to 12 in the Periodic Table that have an incomplete inner electron shell and that serve as transitional links between the most and the least electropositive in a series of elements. They are characterized by multiple valences, colored compounds, and the ability to form stable complex ions. Also called transition metal.
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Bohr Model Diagrams
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An early model of atomic structure in which electrons travel around the nucleus in a number of discrete stable orbits determined by quantum conditions.
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Ions
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An atom or a group of atoms that has acquired a net electric charge by gaining or losing one or more electrons.
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Isotopes
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One of two or more atoms having the same atomic number but different mass numbers.
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Chemical Properties
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property used to characterize materials in reactions that change their identity
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Physical Properties
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any property used to characterize matter and energy and their interactions
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Acid
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Any of a class of substances whose aqueous solutions are characterized by a sour taste, the ability to turn blue litmus red, and the ability to react with bases and certain metals to form salts. (H)
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Base
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Any of a class of compounds whose aqueous solutions are characterized by a bitter taste, a slippery feel, the ability to turn litmus blue, and the ability to react with acids to form salts. (OH)
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Salt
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salts are ionic compounds that can result from the neutralization reaction of an acid and a base. (neither)
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Ionic Compound
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a chemical compound in which ions are held together in a lattice structure by ionic bonds
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Ionic Bond
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a chemical bond in which one atom loses an electron to form a positive ion and the other atom gains an electron to form a negative ion.
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Covalent Compound
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a molecule formed by covalent bonds, in which the atoms share one or more pairs of valence electrons
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Covalent Bond
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a chemical link between two atoms in which electrons are shared between them.
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Binary Ionic Compounds
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A binary ionic compound is a salt consisting of only two elements in which both elements are ions, a cation and an anion
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Co-effiecent
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A coefficient is a number placed in front of a term in a chemical equation to indicate how many molecules (or atoms) take part in the reaction.
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Synthesis Reaction
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one of the most common types of chemical reactions. In a synthesis reaction two or more chemical species combine to form a more complex product.
A + B → AB The combination of iron and sulfur to form iron (II) sulfide is an example of a synthesis reaction: 8 Fe + S8 → 8 FeS |
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Decomposition Reaction
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one of the most common types of chemical reactions. In a decomposition reaction a compound is broken into smaller chemical species.
AB → A + B The electrolysis of water into oxygen and hydrogen gas is an example of a decomposition reaction: 2 H2O → 2 H2 + O2 |
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Combustion
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when all substances in a compound are combined with oxygen, which then produces carbon dioxide and water
CxHy + O2 --> CO2 + H2O |
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Single Replacement Reaction
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one reactant is exchanged for one ion of a second reactant.
Single displacement reactions take the form A + BC → B + AC |
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Double Replacement Reaction
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two reactant ionic compounds exchange ions to form two new product compounds with the same ions.
Double replacement reactions take the form: A+B- + C+D- → A+D- + C+B- AgNO3 + NaCl → AgCl + NaNO3 |
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Acid/Base Neutralization
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A neutralization is a type of double replacement reaction. A salt is the product of an acid-base reaction and is a much broader term then common table salt as shown in the first reaction.
The following are some examples of neutralization reactions to form salts. a. HCl + NaOH --> NaCl + HOH b. H2SO4 + 2 NH4OH --> (NH4)2SO4 + 2 HOH c. 2 NaOH + H2CO3 --> N2CO3 + 2 NaOH |
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pH indicator
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either a weak acid or weak base that exhibits a color change as the concentration of hydrogen (H+) or hydroxide (OH-) ions changes in an aqueous solution
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Inorganic
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Of, relating to, or denoting compounds that are not organic (broadly, compounds not containing carbon)
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Organic
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Compounds containing carbon
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Catalyst
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A substance that increases the rate of a chemical reaction without itself undergoing any permanent chemical change.
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Surface Area
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If you pound a solid sample in a pestle and mortar before reacting it with a liquid you drastically increase it's surface area and it reacts or dissolves many times faster than if you placed the solid lump in the test tube. The same thing happens when you crunch a sweet in your mouth,you get a sudden increase in flavour and the sweet disappears really quickly.
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Temperature
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Rate of reaction increases with temperature increase
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Concentration
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the number of collisions and hence the activated collisions between the reactant molecules increase with increase in concentration.
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Radiation
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The emission of energy as electromagnetic waves or as moving subatomic particles.
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Alpha Particle
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A helium nucleus emitted by some radioactive substances, originally regarded as a ray
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Beta Particle
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A fast-moving electron emitted by radioactive decay of substances. (The emission of beta particles was originally regarded as a ray.).
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Gamma Wave
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Electromagnetic radiation emitted by radioactive decay and having energies in a range from ten thousand (104) to ten million (107) electron volts.
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Radioactive Decay
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decay: the spontaneous disintegration of a radioactive substance along with the emission of ionizing radiation.
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Half-Life
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the time required for something to fall to half its initial value
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