Meniscus- the curved surface of a liquid
Filtration- separation of particles: retains solid particles allowing liquid to pass through
Filtrate- liquid collected after filtration
Adsorbs- attracts and holds on its surface
Percent Recovery- how much water you purified (ex. 90% was purified)
Histogram- shows the percent recovery obtained by all groups
Range- difference between largest and smallest values in a set of data
Average (or mean)- add and divide by total number of values
Median- middle value
Electrical conductivity- the presence of dissolved, electrically charged particles
Hydrologic cycle- remaining water flows back into the water cycle
Direct water use- directly measured water
Indirect water use- hidden uses of water that you may never have considered
Gaseous state- water vapor in the air
Liquid state- how water is most easily identified
Solid state- ice is a common example
Surface water- water from rivers or other bodies of water; contains dissolved minerals
Groundwater- water from wells pumped to the surface
Aquifer- a water-bearing layer of rock, sand, or gravel
Unit 1B:
Boiling point- 100 degrees c
Melting point- 0 degrees c
Surface tension- force that holds water molecules
together
ex. objects that float on liquids that are in fact denser than the actual liquids
ex. objects that float on liquids that are in fact denser than the actual liquids
Unit 1B:
Matter- anything that occupies space and has mass
ex. solids, liquids, gases
ex. solids, liquids, gases
Physical properties- measured without a change in the chemical makeup
ex. color, size, density
ex. color, size, density
Density- mass within volume
Freezing point- 0 degrees c
Aqueous (aqua) solution- a water-based solution
ex. river water, salt water, rain water, orange juice, coffee
ex. river water, salt water, rain water, orange juice, coffee
Distilled water- contains dissolved gasses from the atmosphere
Pure water- clear, colorless, odorless, and tasteless
Mixture- two substances combine yet retain their individual properties
Heterogeneous mixture- composition is not uniform throughout
ex. foil water because its not the same throughout (coffee grounds sank to bottom)
ex. foil water because its not the same throughout (coffee grounds sank to bottom)
Suspension- solid particles separated by filtration
ex. water and coffee grounds
ex. water and coffee grounds
Tyndall effect- the scattering of light, proving the small particles in the water
Colloid- a cloudy mixture containing small particles dispersed in the water; heterogenous
ex. milk (butterfat particles not visible to the human eye)
ex. milk (butterfat particles not visible to the human eye)
Homogenous- uniform throughout
ex. salt and water
ex. salt and water
Solutions- homogenous mixtures consisting of few solutes and a solvent
ex. salt in water; sugar in water
ex. salt in water; sugar in water
Solute- the dissolved substance
ex. salt
ex. salt
Solvent- the dissolving agent
ex. water
ex. water
Elements- one type of atom
Compounds- two or more types of atoms chemically bonded
Chemical Formulas- the
representation of compounds and
elements
Substance- an
element or a compound; a material with a uniform, definite composition and
distinct properties
Molecule- the
smallest unit of a molecular compound that retains the properties of that
substance
Unit 2 B.1 Vocabulary
Atmosphere: provides nitrogen, oxygen, argon, neon
Hydrosphere: layer of water (oceans, clouds, ice caps, glaciers, lakes, rivers, underground water supplies) and some dissolved minerals
Lithosphere: solid part of Earth, provides the greatest variety of chemical resources like petroleum and metal-bearing ores
Ore: naturally occurring rock or mineral that can be mined and from which it is possible to extract metal or other minerals
Minerals: naturally occurring solid compounds containing the element or group of elements of interest
Unit 2 A.6-A.11 Vocabulary
Atomic number: the number of proton in an atom; distinguishes atoms of different elements
Nucleus: positively charged central region of an atom that contains protons and neutrons
Mass number: the sum of the number of protons and neutrons in the nucleolus of an atom of a particular isotope
Isotopes: atoms with the same number of protons but different number of neutrons
Periods: horizontal row in the periodic table; elements are listed in order of increasing atomic numbers and grouped according to similar properties
Periodic relationship: regular patterns among chemical and physical properties of elements arrayed in the periodic table
Group/ Family: vertical row in the periodic table (column); contains elements with similar properties
Alkali metal family: first column on the left side; highly reactive metal that forms an ECl chloride and E2O oxide
Noble gas family: right most group of the periodic table; consists of very unreactive (chemically inert) elements
Halogen family: form 1- ions; group containing fluorine, chlorine, and bromine in a column to the left of the noble gases
Unit 2 A.5 Vocabulary
Combustion: chemical reaction with oxygen gas that produces thermal energy and light; burning
Conductor: a material that allows electricity (thermal energy) to flow through it
o Conducts electricity à light bulb is on
Nonconductor: a material that does not allow electrical current (or thermal energy) to flow through it
o Doesn’t conduct electricityà light bulb off
Malleable: flattens without shattering when struck
Brittle: shatters into pieces
Unit 2 A.1-A.4 Vocabulary
Physical properties: a property that can be observed or measured without changing the identity of the sample of matter
o Color, density, odder
Physical change: a material stays the same, but its form appears to have changed
o Melting, boiling, bending
Chemical properties: properties only observed or measured by changing the chemical identity of a sample of matter
Chemical change: when a substance changes to one or more new substances
o Burning wood, formation of a gas/solid
Luster: shinny and reflect light
Ductile: can be drawn into wires
Metals: a material possessing such as luster, ductility, conductivity, and malleability
o Iron (Fe), tin (Sn), copper (Cu), zinc (Zn)
Nonmetals: a material possessing properties such as brightness, lack of luster, and nonconductivity; nonmetals are often insulators
o Carbon (C) and oxygen (O)
Metalloids: a material with properties intermediate between those of metal and nonmetals
o Silicon (Si) and germanium (Ge)
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Unit 1 C.8- C.13 Vocabulary
Heavy-metal ions: their atoms have greater masses than those of essential metallic elements, and can be harmful to humans or other organisms
o Lead
o Mercury
Green Chemistry: design that prevents pollution by eliminating the production and use of hazardous substances, related to heavy metal pollution
o To prevent heavy metals from getting into water à producing and using alternate materials that do not contain theses ions
pH scale: a way to measure and report the acidic, basic, or chemically neutral character of a solution
o Solution with pH values lower than 7 = Acidic
o Solutions with pH value greater than 7 = Basic
Alkaline: another name for a basic solution. Contains an excess of hydroxide ions (OH-)
Acids: ions or compounds that produce hydrogen ions (H+) or hydronium ions (H3O+) when dissolved in water
o Hydrochloric acid (HCl)
Bases: ions or compounds that produce hydroxide ions (OH-) ions when dissolved in water
o Sodium hydroxide (NaOH)
Chemically neutral: a substance that displays neither acidic nor basic characteristics
Molecular substances: a substance composed of molecules
o H2O
o CH4
Electronegativity: the ability of an elements atom to attract shared electrons when bonding within a compound (difference in electron attraction)
“like dissolves like”: the pattern or solubility behavior- polar substances dissolve in polar solvents and nonpolar substances dissolve in nonpolar solvents
Insoluble: refers to substances that are very, very slightly soluble in water
Gas-bubble trauma: when the total amount of dissolved gases (oxygen and nitrogen) reaches a state of supersaturation
o Causes gas bubbles to form in the blood and tissue of fish
C.4 + C.6 Vocabulary
Particulate level- atomic and molecular phenomena that cannot be easily observed
Polar molecule- a molecule with regions of partial positive and negative charge resulting from the uneven distribution of electrical charge
Concentration- refers to how much solute is dissolved in a specific quantity of a solvent or solution
Percent- another way to express concentration
Parts per million (ppm)- an expression of concentration; the number of units of solute found in one billion units of solution
Parts per billion (ppb)- an expression of concentration; the number of units of solute found in one billion units of a solution
Unit 1 C.1- C.2 Vocabulary
Saturated- is when a solvent has dissolved as much solute as it can retain at a specific temperature, and therefore the solute settles at the bottom of the container because it cant dissolve anymore; even stirring the mixture will not make the crystals dissolve
Solubility- the maximum quality of a substance that will dissolve in a certain quality of water (solvent) to form a saturated solution at a specific temperature
Solubility curve- a graph indicating the solubility of a particular solute at different temperatures
Saturated solution- a solution in which the solvent contains as much dissolved solute as it normally can at that temperature (maxed out amount)
Unsaturated solution- a solution that contains less dissolved solute than the amount that the solvent can normally hold at that temperature
Supersaturated solution- an unstable solution; that contains more solute than can normally be dissolved at that temperature
o Heat up a solvent, then cool it down and slightly tap the beaker or add a drop of a chemical à solid forms
Precipitate- when the extra solute appears as solid crystals and settles to the bottom of the beaker
Unit 1 B.8- B.11 Vocabulary
Protons- positively charged particles
Electrons- negatively charged particles
Electron cloud- a group of electrons (negative charge) revolving around the nucleus of an atom
Neutrons- electrically neutral particles
Ions- electrically charged atoms or groups of atoms
Ionic compounds- substances that are composed of positive and negative ions
o always neutral because positive and negative electrical charges offset each other
Crystal- NaCl consists of positive and negative ions arranged in a three- dimensional network
o in solids, ionic compounds (table salt) ions are held together in crystals by attractions among negative and positive charges
Anion- negatively charged ion
Cation- positively charged ion
Polyatomic ion- an ion consisting of a group of bonded atoms
Confirming tests- tests that confirms that ions are present
Precipitate- insoluble solid substance that has separated from a solution
Qualitative tests- tests that identify the presence or absence of a particular substance in a sample
Quantitative tests- determines the amount of a specific substance present in a sample
Reference solution- a solution of known composition used as a comparison
Unit 1B.5- B.6 Vocabulary listUnit 1B.5- B.6 Vocabulary list
Macroscopic- a world filed with large scale (macro) readily observed things
Models- representations of atoms and molecules
Chemical symbols- an abbreviation of an element’s name.
Chemical formula- a symbolic expression representing the elements contained in a substance, together with subscripts that indicate the relative numbers of atoms of each element
Subscript- the number printed below the normal line of letters; indicates how many atoms of the element there are
Reactants- starting materials in a chemical reaction
Products- substances formed in a chemical reaction
Diatomic Molecules- a molecule made up of two atoms (two bonded atoms of the same element)
Atmosphere: provides nitrogen, oxygen, argon, neon
Hydrosphere: layer of water (oceans, clouds, ice caps, glaciers, lakes, rivers, underground water supplies) and some dissolved minerals
Lithosphere: solid part of Earth, provides the greatest variety of chemical resources like petroleum and metal-bearing ores
- Contains the crust (band of soil and rock that obtain the raw materials needed to build homes and more), mantle, and core
Ore: naturally occurring rock or mineral that can be mined and from which it is possible to extract metal or other minerals
Minerals: naturally occurring solid compounds containing the element or group of elements of interest
Unit 2 A.6-A.11 Vocabulary
Atomic number: the number of proton in an atom; distinguishes atoms of different elements
- 12 protons: magnesium
- 6 protons: carbon
Nucleus: positively charged central region of an atom that contains protons and neutrons
Mass number: the sum of the number of protons and neutrons in the nucleolus of an atom of a particular isotope
- protons + neutrons= mass number
Isotopes: atoms with the same number of protons but different number of neutrons
Periods: horizontal row in the periodic table; elements are listed in order of increasing atomic numbers and grouped according to similar properties
Periodic relationship: regular patterns among chemical and physical properties of elements arrayed in the periodic table
Group/ Family: vertical row in the periodic table (column); contains elements with similar properties
Alkali metal family: first column on the left side; highly reactive metal that forms an ECl chloride and E2O oxide
- a group of elements consisting of lithium, sodium, potassium, rubidium, cesium, and francium
Noble gas family: right most group of the periodic table; consists of very unreactive (chemically inert) elements
Halogen family: form 1- ions; group containing fluorine, chlorine, and bromine in a column to the left of the noble gases
Unit 2 A.5 Vocabulary
Combustion: chemical reaction with oxygen gas that produces thermal energy and light; burning
Conductor: a material that allows electricity (thermal energy) to flow through it
o Conducts electricity à light bulb is on
Nonconductor: a material that does not allow electrical current (or thermal energy) to flow through it
o Doesn’t conduct electricityà light bulb off
Malleable: flattens without shattering when struck
Brittle: shatters into pieces
Unit 2 A.1-A.4 Vocabulary
Physical properties: a property that can be observed or measured without changing the identity of the sample of matter
o Color, density, odder
Physical change: a material stays the same, but its form appears to have changed
o Melting, boiling, bending
Chemical properties: properties only observed or measured by changing the chemical identity of a sample of matter
Chemical change: when a substance changes to one or more new substances
o Burning wood, formation of a gas/solid
Luster: shinny and reflect light
Ductile: can be drawn into wires
Metals: a material possessing such as luster, ductility, conductivity, and malleability
o Iron (Fe), tin (Sn), copper (Cu), zinc (Zn)
Nonmetals: a material possessing properties such as brightness, lack of luster, and nonconductivity; nonmetals are often insulators
o Carbon (C) and oxygen (O)
Metalloids: a material with properties intermediate between those of metal and nonmetals
o Silicon (Si) and germanium (Ge)
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Unit 1 C.8- C.13 Vocabulary
Heavy-metal ions: their atoms have greater masses than those of essential metallic elements, and can be harmful to humans or other organisms
o Lead
o Mercury
Green Chemistry: design that prevents pollution by eliminating the production and use of hazardous substances, related to heavy metal pollution
o To prevent heavy metals from getting into water à producing and using alternate materials that do not contain theses ions
pH scale: a way to measure and report the acidic, basic, or chemically neutral character of a solution
o Solution with pH values lower than 7 = Acidic
o Solutions with pH value greater than 7 = Basic
Alkaline: another name for a basic solution. Contains an excess of hydroxide ions (OH-)
Acids: ions or compounds that produce hydrogen ions (H+) or hydronium ions (H3O+) when dissolved in water
o Hydrochloric acid (HCl)
Bases: ions or compounds that produce hydroxide ions (OH-) ions when dissolved in water
o Sodium hydroxide (NaOH)
Chemically neutral: a substance that displays neither acidic nor basic characteristics
Molecular substances: a substance composed of molecules
o H2O
o CH4
Electronegativity: the ability of an elements atom to attract shared electrons when bonding within a compound (difference in electron attraction)
“like dissolves like”: the pattern or solubility behavior- polar substances dissolve in polar solvents and nonpolar substances dissolve in nonpolar solvents
Insoluble: refers to substances that are very, very slightly soluble in water
Gas-bubble trauma: when the total amount of dissolved gases (oxygen and nitrogen) reaches a state of supersaturation
o Causes gas bubbles to form in the blood and tissue of fish
C.4 + C.6 Vocabulary
Particulate level- atomic and molecular phenomena that cannot be easily observed
Polar molecule- a molecule with regions of partial positive and negative charge resulting from the uneven distribution of electrical charge
Concentration- refers to how much solute is dissolved in a specific quantity of a solvent or solution
Percent- another way to express concentration
Parts per million (ppm)- an expression of concentration; the number of units of solute found in one billion units of solution
Parts per billion (ppb)- an expression of concentration; the number of units of solute found in one billion units of a solution
Unit 1 C.1- C.2 Vocabulary
Saturated- is when a solvent has dissolved as much solute as it can retain at a specific temperature, and therefore the solute settles at the bottom of the container because it cant dissolve anymore; even stirring the mixture will not make the crystals dissolve
Solubility- the maximum quality of a substance that will dissolve in a certain quality of water (solvent) to form a saturated solution at a specific temperature
Saturated solution- a solution in which the solvent contains as much dissolved solute as it normally can at that temperature (maxed out amount)
Unsaturated solution- a solution that contains less dissolved solute than the amount that the solvent can normally hold at that temperature
Supersaturated solution- an unstable solution; that contains more solute than can normally be dissolved at that temperature
o Heat up a solvent, then cool it down and slightly tap the beaker or add a drop of a chemical à solid forms
Precipitate- when the extra solute appears as solid crystals and settles to the bottom of the beaker
Unit 1 B.8- B.11 Vocabulary
Protons- positively charged particles
Electrons- negatively charged particles
Electron cloud- a group of electrons (negative charge) revolving around the nucleus of an atom
Neutrons- electrically neutral particles
Ions- electrically charged atoms or groups of atoms
Ionic compounds- substances that are composed of positive and negative ions
o always neutral because positive and negative electrical charges offset each other
Crystal- NaCl consists of positive and negative ions arranged in a three- dimensional network
o in solids, ionic compounds (table salt) ions are held together in crystals by attractions among negative and positive charges
Anion- negatively charged ion
Cation- positively charged ion
Polyatomic ion- an ion consisting of a group of bonded atoms
Confirming tests- tests that confirms that ions are present
Precipitate- insoluble solid substance that has separated from a solution
Qualitative tests- tests that identify the presence or absence of a particular substance in a sample
Quantitative tests- determines the amount of a specific substance present in a sample
Reference solution- a solution of known composition used as a comparison
Unit 1B.5- B.6 Vocabulary listUnit 1B.5- B.6 Vocabulary list
Macroscopic- a world filed with large scale (macro) readily observed things
Models- representations of atoms and molecules
Chemical symbols- an abbreviation of an element’s name.
- Such as N for nitrogen
- Fe for iron
Chemical formula- a symbolic expression representing the elements contained in a substance, together with subscripts that indicate the relative numbers of atoms of each element
Subscript- the number printed below the normal line of letters; indicates how many atoms of the element there are
- For example: H 2O, the subscript 2 indicates the total of H atoms
- 2H2(g) + O2(g) à 2H2O(g)
Reactants- starting materials in a chemical reaction
Products- substances formed in a chemical reaction
Diatomic Molecules- a molecule made up of two atoms (two bonded atoms of the same element)
- chlorine gas- Cl2
- hydrogen gas- H2
- Oxygen gas- O 2
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