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EQ: How does energy flow and matter cycling affect climate change one earth?
Standard: SEV1 Investigate the flow of energy and cycling

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EQ: Compare and contrast mixtures and solutions
Standards: SC4 Use the organization of the Periodic Table to predict properties of elements

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1.Unsaturated hydrocarbons react very rapidly with halogens.
2.The replacement of a hydrogen atom in a hydrocarbon with chlorine or other atoms is called substitution.
3.Addition involves the adding of atoms to molecules of unsaturated organic compounds.
4.The added atoms are placed on the carbons containing double bonds.
5.The energy necessary to break the double bond is very small and therefore the addition reaction is very rapid.

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1.Carbon atoms can form chains thousands of atoms long or rings of various sizes.
2.Understanding the delicate balance of nature has its foundation in the study of organic chemistry.
3.Natural gas, petroleum, and coal are the largest sources of carbon compounds.
4.Although many of these materials are used as they are, many compounds from these sources are used as raw materials for synthesizing new compounds.
5.Natural gas is about 90% methane, CH₄. Natural gas is found in certain porous rock formations.

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1.A method that is often used to find the concentration of an acid-base system is called titration.
2.A titration is adding an acid or base of known concentration to an acid or base of unknown concentration.
3.An indicator signals when the concentration of acid and base is equal.
4.When the condition of [H⁺] = [OH⁻] is reached, this state is called the equivalence point.
5.Any change in ion charge depends upon the transfer of electrons.

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1.Dissolving and dissociating is the mechanical separation of the ions or molecules that make up the solute.
2.The attraction of the solvent for solute particles and the diffusion-dilution process cause the dissolving to proceed away from the solute source until a equilibrium is established.
3.If during the process of dissolving, the mass action expression of the products < Ksp, the solution is unsaturated.
4.If the mass action expression of the products > Ksp, the solution is supersaturated and precipitation will occur.
5.Compounds which yield (H⁺) ions or increase the (H⁺) concentration when dissolved in water are acids.

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1.A mole of any substance is equal to the sum of the atomic masses of the elements in the substance expressed in grams.
2.A balanced equation is one that has the same number of atoms of each kind on both sides of the reaction.
3.A balanced equation shows a Conservation of Mass.
4.The coefficients of each component in a chemical equation represent the number of molecules, or the relative number of moles, of each component which reacts with each other.
5.A homogeneous mixture or solution consists of a single phase.

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equilibrium Equilibrium is a dynamic state where two opposing forces are in balance, where two opposite events are occurring at equal rates.
solute The substance dissolved in a solution.
solvent That component of a solution which dissolves the solute.

1.The ratio of the number of moles of one component to the TOTAL number of moles in the solution.
2.The number of moles of solute per liter of solution is designated a capital "M."
3.The number of moles of solute per 1,000 g of solvent is designated with lowercase "m."
4.Once a solution is prepared to a given concentration, the concentration remains constant regardless of the quantity being used.
5.Whether one drop or 100 mL of a 0.1 M solution is used, the concentration remains 0.1 M.

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endothermic A reaction that absorbs energy.

enthalpy The energy in atoms and molecules that hold the substances together.
exothermic A reaction that releases energy.
heat of reaction The amount of heat released or absorbed by a reaction.
precipitate The solid formed as a result of chemicals reacting together from a solution.

1.A change intemperature is an indication of energy transfer.
2.Every chemical reaction involves an energy change because the bonds are changed.
3.Energy tied up in the bonds of atoms, molecules, ions, and the rest of the chemical system is called enthalpy.
4. The absolute amount of this energy cannot be measured, but the change in enthalpy from the reactants to products can be measured.
5.If the energy is lost (given off), the reaction is exothermic; if energy is gained (absorbed), the reaction is endothermic.

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EQ: How is the periodic table or elements significant?
Standards: SC4 use the organization of the periodic table to predict properties of elements/

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covalent bond A chemical bond between atoms with similar electronegativities, usually nonmetals; valence electrons are shared.
electronegativity A measure of the ability of atoms to attract electrons within a chemical bond.
ion chargeThe electron charge an atomic particle carries.
ionic bond A bond between atoms of greatly differing electronegativities, usually a metal and a nonmetal; a transfer of one or more valence electrons from one atom (low electronegativity) toward another (high electronegativity); bonds exist between unlike electrical charges (+ and - ions).
metallic bondThe bond formed in metals, holding metals together; delocalized bond with very fluid, mobile electrons; electron mobility accounts for ease of electrical conductivity.

1.Scientists found that all atoms in the combined state show varying degrees of attraction for the electrons of the other atom(s) of the compound.
2.When ions combine, the product is electrically neutral.
3.This process means that the number of (+) charges will equal the number of (-) charges.
4.Remember that ionization energy is the energy necessary to remove valence electrons from atoms.
5.Ionic bonds occur when it appears that valence electrons from one atom are completely transferred to another.

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energy level The broad bands or regions located around the nucleus where the electrons are found.
group A vertical columns of the periodic table; groups have similar valence electron structure and similar chemical and physical properties.
ion Atom or group of atoms with a net charge caused by unequal numbers of electrons and protons.
ionization energy The energy necessary to overcome the attractions of electrons to the nucleus of an atom so as to remove electrons from the atom.
period A horizontal row in the periodic table.

1.You have probably used the periodic table before to determine the atomic number and average atomic weights of the elements.
2.However, the general arrangement of the table itself highlights the repeating order and similarities of the elements.
3.Each horizontal row is called a period.
4.As you read across the table from left to right, the atomic numbers of the elements increase.
5.In each period the properties of the elements gradually change from the properties of metals on the left to nonmetals on the right.

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alpha particle Helium nucleus emitted from the nucleus of a decaying isotope.
beta particle An electron or particle similar to an electron emitted from the nucleus of a radioactive element.
daughter The nuclide produced from a radioactive decay.
mass number The number of protons plus neutrons in the nucleus.
electron A negative particle basic to matter; located outside the nucleus.

1.Dalton formulated his own law of multiple proportions in 1803, based on his observation that the same elements combine in different proportions to produce different substances.
2.After many years of research, Rutherford and Bohr concluded that electrons move in orbits around the atomic nucleus.
3.As long as an electron remains in a given orbit, no energy is radiated.
4.However, a suitable energy source can cause the electron to jump to an orbit of high erenergy.
5.When the electron returns to the lower orbit, the extra energy is liberated as a single quantum (specified quantity) of light or other form of radiation.

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Avogadro's hypothesis A hypothesis that equal volumes of gas under equal conditions have equal numbers of molecules.
Avogadro's numberThe number of particles in a mole of a substance. Equals 6.02 x 1023 particles per mole.
Boyle's LawThe inverse relationship between pressure and volume of gases such that as pressure increases, volume decreases by the same fraction of change Temperature and number of molecules remain constant.
Charles' LawThe direct relationship between temperature and volume of gases such that as temperature (absolute scale) increases, volume increases by the same fraction of change. Pressure and volume remain constant.
Combined Gas LawThe mathematical relationship which contains the three variables of pressure, volume, and temperature. This law is derived from combining Boyle's and Charles' Laws into one.

1.One characteristic that distinguishes solids, liquids, and gases from each other is their shape.
2. Solids have a fixed shape and volume.
3.iquids assume the shape of their container and also have a fixed volume.
4.Gases expand to fill whatever volume is available.
5.Air pressure is explained in terms of continually moving particles.

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3-12 Pre Test....TU,3/11 & WED,3/12

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atom The simplest unit of an element that still retains the properties of that element.
colloid A uniform dispersion, heterogeneous in nature, between two or more substances.
compound Two or more elements chemically joined together such that the elements have lost their individual identity in favor of a new set of properties.
element A primary substance that cannot be divided into separate substances; one of about 112 different basic varieties of matter making up the universe.
heterogeneous Composed of dissimilar parts which can be separated easily and which are unevenly distributed in the mixture.

1.One of the easiest ways to identify a particular element is by its physical properties.
2.These properties include such things as color, specific gravity, hardness, boiling point, melting point, density, magnetic properties, crystalline shape, and ability to conduct electricity and heat.
3.Theoretically, all elements can also be classed by their chemical properties.
4.As with physical properties, more than one chemical property marker is necessary to verify the identity of any particular element sample.
5.Chemical properties involve the ability of an element to react with another element or particular substance, such as oxygen or an acid or base.

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deductive reasoning A prediction made or conclusion drawn from insight gained from an established principle.
direct relationship When two variables change in the same direction, one remaining larger than the other by the same factor.
hypothesisAn initial proposed explanation for the phenomenon.
inverse relationship When one variable becomes larger by a given factor and the other variable becomes smaller by the same factor.
law A relationship that is accepted as true and no longer needs to be tested and verified.

1.If a theory consistently fails to confirm the expected predictions after extensive research, it is probably unreliable.
2.Scientific predictions are not made up from imagination, subjective conclusions, or presuppositions.
3.They need to be made in an objective way.
4.Predictions are generated from deductive reasoning.
5.The process of hypothesizing is one in which we systematically collect evidence and at some point develop a logical explanation or "educated guess" as to why the evidence is as it is.

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accuracy The correctness of a measurement when compared to the actual value.
length The measure of the distance from one point to another.
mass A measure of the quantity of matter in an object.

precision How spread out the results of an experiment are or, how repeatable measurements are; often dependent on the certainty with which an estimation can be made.
volume Space occupied by a quantity of matter.

1.Science and scientists have used the metric system of measurement for almost two hundred years.
2.The metric system is used in nearly all countries in the world for the standard units of measurement.
3.Length is the measure of the distance from one point to another.
4.It can be measured in large units like light years or small units like angstroms.
5.All of our measurements of length and volume derive from this standard.