1. Dec 13th & 15th Midterm Specifications – Comp III Science ADV
Standard # of Questions Topic_____________________________
SC.8.N.1.1 4
SC.8.N.1.2 1
SC.8.P.8.1 7
SC.8.P.8.3 5
SC.8.P.8.4 8
SC.8.P.8.7
SC.8.P.9.2 3
SC.8.P.8.5
SC.8.P.8.6 6
SC.8.P.8.8 2
SC.8.P.8.9
SC.8.P.9.3
SC.912.P.8.1
SC.912.P.8.2
SC.912.P.8.4
SC.912.P.8.5
SC.912.P.8.7
Define a problem from the eighth grade curriculum using appropriate reference materials to support scientific understanding, plan and carry out scientific investigations of various types, such as systematic observations or experiments, identify variables, collect and organize data, interpret data in charts, tables, and graphics, analyze information, make predictions, and defend conclusions.
Design and conduct a study using repeated trials and replication.
Explore the scientific theory of atoms (also known as the atomic theory) by using models to explain the motion of particles in solids, liquids & gases.
Explore & describe the densities of various materials through measurement of their masses and volumes.
Classify and compare substances on the basis of characteristic physical properties that can be demonstrated or measured: for example: density, thermal or electrical conductivity, solubility, magnetic properties, melting and boiling points, and know that these properties are independent of the amount of the sample
Explore the scientific theory of atoms (also known as the atomic theory) by recognizing that atoms are the smallest unit of an element & are composed of sub-atomic particles (electrons surrounding a nucleus containing protons & neutrons)
Differentiate between physical changes and chemical changes.
Recognize that there are a finite number of elements and that their atoms combine in a multitude of ways to produce compounds that make up all of the living and nonliving things that we encounter.
Recognize that elements are grouped in the periodic table according to similarities of their properties.
Identify basic examples of and compare and classify the properties of compounds, including acids, bases, and salts.
Distinguish among mixtures (including solutions) and pure substances.
Investigate and describe how temperature influences chemical changes.
Differentiate among the four states of matter
Differentiate between physical and chemical properties and physical and chemical changes of matter.
Explore the scientific theory of atoms (also known as atomic theory) by describing the structure of atoms in terms of protons, neutrons and electrons, and differentiate among these particles in terms of their mass, electrical charges and locations within the atom.
Relate properties of atoms and their position in the periodic table to the arrangement of their electrons.
Interpret formula representations of molecules and compounds in terms of composition and structure.

2. A: Scientific inquiry is a multifaceted activity; The processes of science include the formulation of scientifically investigable questions, construction of investigations into those questions, the collection of appropriate data, the evaluation of the meaning of those data, and the communication of this evaluation.
B: The processes of science frequently do not correspond to the traditional portrayal of "the scientific method."
C: Scientific argumentation is a necessary part of scientific inquiry and plays an important role in the generation and validation of scientific knowledge.
D: Scientific knowledge is based on observation and inference; it is important to recognize that these are very different things. Not only does science require creativity in its methods and processes, but also in its questions and explanations.
A. All objects and substances in the world are made of matter. Matter has two fundamental properties: matter takes up space and matter has mass which gives it inertia. B. Objects and substances can be classified by their physical and chemical properties. Mass is the amount of matter (or "stuff") in an object. Weight, on the other hand, is the measure of force of attraction (gravitational force) between an object and Earth. The concepts of mass and weight are complicated and potentially confusing to elementary students. Hence, the more familiar term of "weight" is recommended for use to stand for both mass and weight in grades K-5. By grades 6-8, students are expected to understand the distinction between mass and weight, and use them appropriately.
A. Matter can undergo a variety of changes. B. When matter is changed physically, generally no changes occur in the structure of the atoms or molecules composing the matter. C. When matter changes chemically, a rearrangement of bonds between the atoms occurs. This results in new substances with new properties. Clarification for grades K-5: The target understanding for students in the elementary grades should focus on Big Ideas A and B. Clarification for Grades 6-8: The target understanding for students in the middle grades should begin to transition the focus to: C. When matter changes chemically, a rearrangement of bonds between the atoms occurs. This results in new substances with new properties.
A. A working definition of matter is that it takes up space, has mass, and has measurable properties. Matter is comprised of atomic, subatomic, and elementary particles.
B. Electrons are key to defining chemical and some physical properties, reactivity, and molecular structures. Repeating (periodic) patterns of physical and chemical properties occur among elements that define groups of elements with similar properties. The periodic table displays the repeating patterns, which are related to the atom's outermost electrons. Atoms bond with each other to form compounds.
C. In a chemical reaction, one or more reactants are transformed into one or more new products. Many factors shape the nature of products and the rates of reaction.
D. Carbon-based compounds are building-blocks of known life forms on earth and numerous useful natural and synthetic products.

3. Midterm Vocab – Comp III
Independent (Test, Manipulated) Variable – What YOU purposely change during an experiment
Dependent (Responding, Outcome) Variable – What is expected to change as a result
Variables Held Constant – Things that are controlled or kept the same as not to influence the outcome
Trials – Repeating a procedure from the beginning
Samples – The amount or variety of something tested, measured, or changed
Replication – Someone else recreating your experiment with the very same procedures (for comparison)
Repetition – Doing something over again (trials) to eliminate errors and establish an average
Hypothesis – What you predict will happen (based on prior knowledge)
Conclusion – What patterns exist in your results with evidence towards likely causes and explanations
Applications – How findings can connect, function or be significant in a practical (non laboratory) way
Qualitative Data – Information that is “descriptive” or subjective in nature. Ex: Warm
Quantitative Data – Information represented with numbers (which can be compared) Ex: 30 degrees
Solid – Doesn’t flow or change shape. Fixed volume. Lower energy and slower, more closely packed particles
Liquid – Fluid (changes shape) with fixed volume and looser, more energetic particles than a solid
Gas – Fluid with no fixed volume and very free and active particles
Plasma – An energized gas with unique magnetic and electrical properties. Most matter is the universe is plasma (In stars)
Freezing Point – The temperature at which something turns to a solid
Melting Point – The temperature at which something turns from a solid to a liquid
Boiling Point – The temperature at which something turns into a gas. Related to Evaporation.
Sublimation – When something turns from a solid directly to a gas (skipping the liquid state)
Condensation – A gas turning “back” to a liquid
Heat – a thermal energy transfer from a hotter area to a colder area
Volume – How much space something takes up
Mass – How much matter something contains
Weight – How much something is pulled “down” by gravity. Proportional to mass, but can change according to location
Temperature – The energy of particles in a substance
Density – How much matter in a given space. Mass divided by Volume. This figure does not change when the amount of the sample changes
Conductance – How well something allows energy like heat or electricity to pass into it or through it
Physical Properties – Characteristics of a substance that can be directly observed or measured. Ex: Density, Melting Point, Conductance,
magnetism, solubility. Note: These figures will NOT change based on the amount of the substance.
Chemical Properties – Hidden characteristics of a substance that can only be potentially “unlocked” when interacting with another substance (Chemical reaction). Ex: Flammability, pH, Toxicity
Chemical Change – A reaction occurs that changes the composition and identity resulting in a new substance. Ex: Cooking, Rusting. If
temperature is increased, the reaction rate increases too (and the opposite).
Physical Change – Some aspect of the substance changes, but no reaction has taken place (leaving the same substance). Ex: Boiling, Dissolving
Atom – The smallest unit of matter. Each element on the periodic table has unique atoms (based on the number of sub-atomic particles
inside the atom.)
Nucleus – the core of an atom, where the mass is contained
Proton – Positively charged sub-atomic particle, found in the nucleus, has a mass of 1
Neutron – No charge, found in the nucleus, has a mass of 1
Electron – Negative charge, found in orbit outside of the nucleus, essentially no mass
Elements – Found on their own or bound with other elements to make up all matter that exists (both living and non-living). We know which elements are which by the number of protons they have.
Compounds – More than one element chemically connected in a molecule. Ex: CO2, H2O
2Pure Substance – Contains only one type of atom, molecule or compound. Every sample taken from it will be identical (homogenous) and only
a chemical reaction can separate it. Ex: The Mercury in a thermometer, the distilled water in a jug, the sugar in a bag.
Mixture – Can be either homogenous or heterogeneous but can always be separated mechanically (by hand, filter, magnet, etc.) These contents
are not locked together chemically, so they can be taken apart according to their physical properties. Ex: Salad, Coffee, Soil
Solution – A mixture which every sample taken from it will be the same (uniform, homogenous). The variety of atoms, molecules, or compounds
are not bound chemically together but are so well mixed that it may be more difficult than a typical mixture to separate. Ex: Coffee, Air, Brass
Periodic Table – Orders elements by atomic mass, or number of protons. Elements that have common characterizes are found near each other. Ex: A vertical group may belong to the same “series” like the soft and very reactive group 1; Alkali Metals. A group (1-18) also tells
us about electron configuration. This allows predictions about how reactive an element will be and what bonds might easily form.
Acid – A low number on the 14 point pH scale. Tastes sour, reacts with metal. Ex: Vinegar: pH = 3
Base – A high number on the pH scale. Slippery and bitter. Ex: Soap: pH = 8 Salt – A neutral compound (more than one element – ionic bonded) formed from an acid and a base. Ex: NaCl (table salt); Na (sodium) is a base and Cl (chlorine) is an acid. Neutral pH is around 7.