Vocab

Vocabulary

Day 1

• Density= mass/volume
• Beaker- holds solids or liquids that will not release gases when reacted or unlikely to splash
• Erlenmeyer Flask- holds solids or liquids that may release gases when reacted or likely to splash
• Graduated Cylinder- used to measure volumes of liquids
• Spot Plates- used when we want to perform many small scale reactions at one time
• Watch Glass- used to hold a small amount of a solid (remember the thingy that looked like a huge contact lens?)
• Glass stir rod- used to manually stir solutions (better than metal because it does not react)
• Medicine dropper- used to transfer a small amount of liquid
• Wash bottle- delivers a wash solution to a specific area (only distilled water)
• Weighing boat- a kind of scale (looks like a lil boat)
• Spatulas- used to dispense solid chemicals from their containers (long, evil looking metal spoons)
• Crucible- used for heating certain solids (like metals) to very high temperatures
• Ringstands- a safe and convenient way to perform reactions that require heating using a Bunsen burner
• Iron rings- connect to ringstand to hold containers
• Pressed fiber pads- provides a surface for heat
• Meniscus- the curved surface of the water when reading a graduated cylinder
• Parallax Errors- misreading the meniscus from an angle
• Ductile- can be drawn into wires
• Luster- are shiny and reflect light
• Physical Properties- properties that can be determined without altering the chemical makeup of the material
• Physical Change- the material remains the same, even though its form appears to have changed
• Chemical Properties- relate to any kind of chemical change it undergoes, often determine its usefulness
• Chemical Change- when a substance changes into one or more new substances 

Day 2

• Particulate Level- the level of atoms and molecules in a material
• Matter- anything that occupies space and has mass
• Atoms- the building blocks of matter
• Element- matter that is made up of only one kind of atom
• Compound- a substance composed of atoms of two or more elements linked together chemically in certain fixed proportions
• Substance- has a uniform and definite composition as well as distinct properties
• Molecule- a collection of atoms that move and act together as a single entity 
• Chemical Bonds- holds together atoms of a molecule
• Chemical Symbols- the "letters" in the "chemical language"
• Chemical Formula- represents chemical compounds
• Subscript- (a small number written below the normal line of letters) indicates how many atoms of the element just to the left of the subscript are in one unit of the compound
• Chemical Equations- summarize the details of a particular chemical reaction
• Chemical Reactions- entail the breaking and forming of chemical bonds, causing atoms to become rearranged into new substances
• Reactants- the original (starting) substances in a chemical reaction 
• Products- the new substance or substances formed from the rearrangement of the reactant atoms
• Balanced Chemical Equation- the total number of each type of atom is the same for both reactants and products

Day 3

• Macroscopic- large-scale readily observed things
• Models- representations
• Metals-includes elements such as iron, tin, zinc and copper
• Nonmetals- carbons and oxygen
• Metalloids- have properties that are intermediate to those of metals and nonmetals, exhibit both metallic and nonmetallic properties
• Conductor- electricity is able to flow through the material
• Nonconductor- electricity is not able to flow through the material
• Malleable- it flattens without shattering when struck
• Brittle- it shatters into pieces

Day 5

• Periodic Table- placing elements with similar properties near one another in a chart
• Mendeleev- a Russian chemist, published a periodic table in 1869 (table we use today)
• Noble Gases- unreactive gases
• Protons- positively charged particles
• Electrons- negatively charged particles
• Neutrons- electrically neutral particles 
• Combining Capacity- how an element combines with other elements

Day 6

• Atomic Number- number of protons
• Nucleus- a concentrated region of positive charge (due to protons) in the center of an atom
• Mass Number- the total number of protons and neutrons in the nucleus of an atom 
• Isotopes- atoms with the same number of protons but different number of neutrons/ atoms of the same element with different mass numbers 

Day 7

• Periods- horizontal rows on the periodic table
• Periodic Relationship- when elements are listed in order of increasing atomic numbers and grouped according to similar properties
• Group/Family- columns on the periodic table
• Alkali Metal Family- 6 elements, all of which are highly reactive metals that form a chloride compound with a 1:1 alkali metal atom to chlorine atom ratio and an oxide with a 2:1 (alkali metal atom to oxygen atom) ratio
• Noble Gas Family- consists of very unreactive (or even chemically inert) elements
• Halogen Family- highly reactive and readily form binary compounds with hydrogen
• Halide Compound- when elements in the halogen group form compounds
• Periodic Properties- chemical or physical properties that vary among elements according to trends that repeat as atomic number increases

Day 8

• Ionic Compounds- substances that are composed of positive and negative ions
• Ions- are electrically charged atoms or groups of atoms
• Crystal- a 3-D network
• Anion- a negatively charged ion
• Cation- a positively charged ion
• Formula Unit- the simplest unit of an ionic compound
• Polyatomic Ions- group of bonded atoms with an electrical charge
• Monatomic Ions- one atom with an electrical charge
• Activity Series- ranking elements in order of their chemical reactivity

Day 9

• Relative Reactivities
• Metal Reactivities

Day 10

• Resources-
• Atmosphere- provides nitrogen, oxygen, neon, and argon 
• Hydrosphere- provides water and some dissolved minerals
• Lithosphere- the solid part of the Earth, provides the greatest variety of chemical resources
• Ore- a naturally occurring rock or mineral that can be mined, and from which it is profitable to extract a metal or other material
• Deposits- naturally occurring collections of ores in the lithosphere
• Minerals- naturally occurring solid compounds containing the element or group of elements of interest
• Percent Composition- the percent by mass of each component found in a sample such as a coin (can be found by dividing the mass of each constituent metal by the mass of the penny and multiplying by 100%).

Day 11

• Mole- counting unit that is useful in calculating the metal content of ores and solving similar problems (6.02 x 10^23)
• Molar Mass- the mass of one mole of any substance
• Refined- the removal of impurities from a desired material
• Reduction- any chemical change in which a reactant can be considered to gain one or more electrons
• Oxidation- the reverse reaction in which an ion or other reactant can be considered to lose one or more electrons
• Oxidation-Reduction Reactions/ Redox Reactions- whenever one reactant loses electrons, another reactant must simultaneously gain them
• Reducing Agent- a reactant that provides electrons
• Electrometallurgy- involves using an electric current to supply electrons to metal ions, thus reducing them
• Pyrometallurgy- involves treating metals and their ores with thermal heat
• Hydrometallurgy- involves treating ores and other metal-containing materials with reactants in water solution

Day 12

• Electron-Dot Structure/Dot Structure
• Oxidizing Agent- the reactant involved in removing electrons from the oxidized reactant
• Electroplating- uses direct-current (DC) electricity, causes redox reactions to occur
• Half-Reactions- separately represent the reduction and oxidation parts of a redox process
• Cathode- where reduction occurs
• Anode- the ultimate source of elections in any electrochemical process
• Material's Life Cycle

Day 15

• Diatomic Molecules- exist as two bonded atoms of the same element
• The Law of Conservation of Matter- in a chemical reaction, matter is neither created nor destroyed
• Balanced Chemical Equation- the number of atoms of each element is the same on the reactant and product sides
• Coefficients- indicate the relative number of units of each substance involved in the chemical reaction

Day 16

• Alloy- a solid combination of atoms of two or more metals
• Superconductivity- the ability to conduct an electric current without any electrical resistance
• Sustainability- preserving the ability of future generations to thrive and meet their resource needs on a habitable Earth
• Renewable Resources- natural cycles are not disturbed too much, maintained indefinitely (water, air, soil, plants, animals)
• Nonrenewable Resources- cannot be readily replenished (metals, natural gas, coal, petroleum)
• Brass- alloy made of copper and zinc

Day 18

• Viscosity- resistance to flow
• Hydrocarbons- molecular compounds that contain only atoms of the elements hydrogen and carbon
• Crude Oil- petroleum pumped from underground 
• Fossil Fuels- petroleum, natural gas, coal
• Reserves- resources that can be tapped by available technology at costs consistent with current market prices

Day 19

• Distillation- the separation of liquid substances according to their differing boiling points.
• Distillate- condensed liquid component
• Fractal Distillation- the refining process does not separate each compound in crude oil, it produces several distinctive mixtures
• Fractions- several distinctive mixtures from fractal distillation
• Bottoms- substances with the highest boiling points that never vaporize

Day 20

• Alkanes- each carbon atom in an alkane shares electrons with four other atoms
• Tetrahedron- a pyramid w/ a triangle as its base
• Condensed Formulas- ex. CH3CH2CH3

Day 21

• Extrapolation- the process of estimating a value beyond a known range of data points
• Straight Chain Alkanes- each carbon atom is only linked to one or two other carbon atoms
• Branched Chain Alkanes- one carbon atom can be linked to three or four other carbon atoms
• Structural Isomers- molecules that have molecular formulas but different arrangements of atoms

Day 22:

• Organic Chemistry- hydrocarbons and their derivatives, including polymers, are the focus
• Carbon Chain- carbon atoms are joined to form a backbone 
• Shell- separate energy levels in space surrounding the nucleus
• Valence Electrons- those electrons within an atom's unfilled outer shell
• Covalent Bond- the sharing of two or more valence electrons between two atoms
• Lewis Structures- dots surrounding each element's symbol represent the valence electrons for that atom
• Structural Formula- a chemical formula showing the arrangement of atoms and covalent bonds in a molecule, in which each electron pair in a covalent bond is represented by a line between the symbols of two atoms
• Petrochemicals- compounds produced from oil or natural gas
• Double Covalent Bond- a bond in which four electrons are shared between two adjacent atoms
• Addition Reaction- a reaction at the double or triple bond within an organic molecule
• Addition Polymer- a polymer formed by repeated addition reactions at double or triple bonds within monomer units

Day 23

• Potential Energy- energy of position (or condition)
• Kinetic Energy- energy related to motion 
• Chemical Energy- a different form of potential energy, stored in chemical compounds
• Thermal Energy- energy released as heat
• Endothermic- a process that requires the addition of energy
• Exothermic- a process that involves the release of energy
• Law of Conservation of Energy- states that energy is neither created nor destroyed in any mechanical, physical, or chemical processes
• Heat of Combustion- the quantity of thermal energy given off when a certain amount of a substance burns 
• Molar Heat of Combustion- if the amount of substance burned is one mole, the quantity of thermal energy involved 

Day 26

• Mixture- when two or more substances combine yet retain their individual properties
• Heterogeneous Mixtures- composition is not the same throughout
• Suspension- if the solid particles are large enough to settle out or can be separated by using filtration
• Colloid- small, solid particles are in the water
• Tyndall Effect- the scattering of light indicating the particles
• Homogeneous- uniform throughout
• Solution- a homogeneous mixture
• Solute- the dissolved substance
• Solvent- the dissolving agent
• Surface Water- water supply originating in a lake, river, or other body of water
• Groundwater- water supply originating in a well
• Aquifer- a water-bearing layer of rock, sand, or gravel
• Filtration- solid particles are separated from a liquid by passing the mixture through a material that retains the solid particles and allows the liquid to pass through
• Filtrate- the liquid collected after it has been filtered
• Adsorbs- attracts and holds on its surface
• Adhesive Forces- attract molecules of different substances to one another
• Percent Recovery- the percent of original foul water recovered as purified water