Acids and Bases Study Guide (Chapter 7)

Acids, Bases, and Neutrals Test

Study Guide  - Chapter 7

Vocabulary to Know

Acid

Base

Neutral

H+ ion  (Hydrogen Ion)

OH- ion  (Hydroxide Ion)

Salt

Neutralization and Neutralization Reaction

pH and pH scale

indicator

litmus paper

Concepts to Know

1.     What are the characteristics of acids, bases and neutrals?

2.     What is pH?  What is the pH of acids, bases and neutrals?  What do we use to measure or determine pH?

3.     What are examples of acids, bases and neutrals?

4.     What happens when you put acids and bases together?  What do they form?  What is a neutralization reaction?

5.     What are some common indicators of acids, bases and neutrals and how do they work?

Chapter 6 Study Guide

Chapter 6 Study Guide

Chemical Reactions

1.     You should know how to write a chemical formula using your valence sheet.

Example:  Sodium chloride     Na ⁺¹   Cl ^-1   =     NaCl

       2.  A chemical change is when two or more substances react, or one substance

           decomposes.  In both cases something new is formed.  Evidence of a chemical

           change: 

         -  Temperature change (exothermic or endothermic)

         -  Color change

         - Precipitate forms

         - Gas produced (bubbles)

         - Fire/Explosion

3.     A physical change is a change in matter that does not produce a new substance like cutting paper or mixing salt and pepper.

4.     You should know the structure of a chemical formula.  Be able to label reactants, products, yields sign, subscripts and coefficients.

5.     Know that subscripts tell us the number of atoms of an element and coefficients tell us the number of molecules of a substance.

6.     Law of Conservation of Mass:  Matter is not created nor destroyed.

7.     You should know how to balance chemical equations.

8.     You should be able to identify the four major types of chemical reactions: Synthesis, Decomposition, Single Replacement,  Double Replacement, and Combustion.

9.     A catalyst is a substance that speeds up a reaction but is not involved in the chemical reaction.  Be able to identify the catalyst in a reaction.

Chapter 2 Study Guide (Version 2)

Chapter 2 Chemistry (pages 58 -77)

Review all Homework, Labs, Vocabulary, and Notes

I.               Review Properties of Matter Notes

II.             Know the following vocabulary words:

Matter, Substance, Physical Property, Chemical Property, Element, Atom, Chemical Bond, Molecules, Compound, Chemical Formula, Mixture, Heterogeneous Mixture, Homogeneous Mixture, Solution, Physical Change, Chemical Change, Precipitate, Law of Conservation of Matter, Energy, Temperature, Thermal Energy, Endothermic Reaction, Exothermic Reaction, Chemical Energy, Electromagnetic Energy, Electrical Energy, Electrolysis.

III.           Know examples of all of the vocabulary words above

IV.           Labs:

A.     Know how to identify the physical properties of a substance.

B.     Know how to identify a physical change of matter.

C.     Know how to tell if a chemical change has occurred.

D.    Know what a precipitate is and how you can tell if a precipitate has formed.

E.     Know how to tell if an endothermic or exothermic reaction has occurred.  Know why they occur.

F.     Know what electrolysis is and be able to explain what happened in the electrolysis lab.

Chapter 4 Study Guide

Study Guide

Chapter 4 – The Periodic Table

Study Classroom Notes:

Introduction to Atoms

Atomic Structure and Energy Levels

Reading the Periodic Table

Periodic Table Squares Practice (Finding Protons, Neutrons, and Electrons and Drawing Bohr Models)

Study Labs:

It’s Elemental

Periodic Puzzle

Flame Test Lab

Metals Vs. Nonmetals

Review Text pages 124-155

Know:

Atomic Number if given the name, symbol, # of protons, or # of electrons

Number of Protons if given the name, symbol, atomic #, or # of electrons

Number of Electrons if given the name, symbol, atomic #, or #of protons

Atomic Mass (weight) if given the name or symbol

Element Symbol if given the element name

Element Name if given the symbol, atomic #, # of protons, or #of electrons

Period Number if given the symbol, atomic #, or # of protons or electrons

Number of Energy Levels if given the name, symbol, atomic #, or period

Group/Family if given the name, symbol, or atomic number

Number of Valence Electrons if given the name, symbol, or group/family

Properties and Valence Electrons for Alkali Metals, Alkaline Earth Metals, Halogens and Noble (Inert Gases)

Dmitri Mendeleev

Know where to find metals, nonmetals, and synthetic elements on the Periodic Table

Know that semimetals (metalloids) are good semiconductors because they can conduct electricity but not as well as metals (example: silicon)

Periods are horizontal rows that tell us the number or energy levels

Know major properties of metals and nonmetals

Bohr Models:  Be able to draw Bohr models for all elements up to 20.

Essay Topics: (be prepared for the following topics):

-       Be able to explain what is unique about the inert (noble) gas region of the periodic table.

-       Be prepared to discuss similarities and differences of metals and nonmetals with examples.

Chapter 9 Study Guide

Study Guide – Chapter 9 Motion

Key Terms are underlined and in bold.  You need to know the definitions and examples/explanations for all key terms.

1.     Describing Motion (Pages 338 – 341)

A.     What is motion?

B.     What is a reference point?  Why is it important for the reference point to be a stable object?

C.     If objects are moving together (like you when you drive home from school with your parents or a carpool) are they in motion relative to each other (relative motion)?

D.     What are distance and displacement (a vector)?  Be able to label on a map.

2.     Speed and Velocity (pages 342 – 347)

A.     What is speed?  Know that speed is calculated with the formula

speed = distance/time.  Be able to solve speed problems.

B.     Average speed is the total distance covered divided by the total time covered.

C.     Velocity is speed in a direction.  The formula for calculating velocity is the same as for speed but you need to add a direction.  Velocity is a Vector Quantity.

D.     Be able to read graphs showing Time and Distance like the graphs on pages 346 and 347.  You need to be able to describe the motion at each point.

E.     On distance and time graphs, the steeper the slope, the faster the object is moving.  The shallower the slope, the slower the object is moving.

3.     Acceleration (pages 352- 355)

A.     Acceleration is the rate at which velocity changes.  If speed changes (faster or slower) OR direction changes, then an object has accelerated.

B.     Be able to read a distance vs. time graph for acceleration like the one on page 355.

C.     Be able to calculate the acceleration of an object given the velocities and total time like the acceleration lab in class.  See page 353 for practice.

4.     Energy (pages 358 – 363)

A.     Energy is the ability to do work.  Work is what is required to put an object in motion.

B.     Potential Energy is stored energy.  Be able to describe chemical, elastic and gravitational potential energy in real-life situations.

C.     Gravitational potential energy depends on the height of an object and its weight.  The more massive the object and the height of the object will determine the amount of potential energy.

D.     Kinetic Energy  is energy of motion.  As an object falls is gains kinetic as it loses potential.  Energy is transformed.  Kinetic energy depends upon mass and speed but speed really affects the moving energy of an object. 

E.     The Law of Conservation of Energy says that energy cannot be created or destroyed, it only changes form.  Be able to apply this law to the roller coasters we build in class, to how a pendulum moves, and also to explain why the pendulum CAN’T hit you in the face if you let it go from the tip of your nose.

F.      Using the Law of Conservation of Energy, describe how energy changes form given a certain scenario like Sun -à Plant --à Person -àMarathon Run.  Radiant Energy from the Sun transforms into Chemical Potential Energy (stored energy) which the person eats (Chemical Energy) to transform into Mechanical Energy and Thermal Energy.

Chapter 10 Study Guide

Study Guide:  Chapter 10 Forces

1.    Forces

A.     A force is a push or a pull.

B.     Net force is a combined force.

C.    Unbalanced and Balanced forces

D.    Force as a vector quantity

E.     Force is measured in Newtons.  A Newton is equal to about .22 pounds or 102 grams.

2.    Friction Force

A.     Friction is a force that acts opposite to a push or a pull.

B.     When one surface interacts with another surface.

C.    Four types of friction

D.    Know what type of friction is being used in a situation and if you are trying to increase or decrease friction.

3.    Elastic Force

A.     Tension is a pulling elastic force

B.     Compression is a pushing elastic force

4.    Gravity

A.     Gravity is a property of matter. The more matter and the closer you are to the matter, the greater the gravitational pull.  The denser the object, the more gravitational pull.

B.     Gravity is the force that pulls all objects toward Earth.

C.    Free fall is when the only force accelerating an object is gravity.  The acceleration due to gravity on Earth is 9.8 m/s2.

D.    All objects fall at the same rate on Earth (as long as air friction is removed).

E.     Monkey and the Hunter – Gravity is separate from forward motion so a shot object and a dropped object will fall at the same rate.  Think running off a cliff vs. stepping off a cliff.

Chapter 5 Study Guide

Chapter 5 Study Guide

Chemical Bonding

Review Notes, Labs, Homework, and the Textbook.

1.    Using the Periodic Table, you should be able to draw the electron dot diagram for all of the elements covered in class.

2.    Ionic Bonds

A.    Know that an ion is a charged atom or group of atoms

B.    A polyatomic ion is what we call a charged group of atoms

C.    Atoms become charged when the gain or lose electrons.

D.   Atoms have positive charges when the lose electrons (mostly metals) and negative charges when they gain electrons (mostly nonmetals).

E.    Ionic Bonds form when electrons are transferred from one atom to another resulting in ions.  The opposite charges of the ions attract each other.  This is a very strong bond.

F.    You should know how to write chemical formulas using ion charges.  You should know how to name compounds using the chemical formula.  I will give you an ion list to use on the test.

G.    You should know the characteristics of ionic compounds:

1)   Ionic compounds form crystals because of the regular repeating pattern of ions.

2)   Conduct electricity when dissolved in water.

3)   High melting points

4)   Not flammable

5)   Almost all ionic compounds (salts) are formed from

a metal and a nonmetal bonding.

3.    Covalent Bonds

A.    Know that covalent bonds form when atoms share electrons.

B.    Usually form when nonmetals bond to other nonmetals.

C.    Sometimes atoms have to share lots of electrons when they bond (example: Nitrogen gas forms with a triple bond).

D.   Covalent molecules often have low melting points and burn easily (more flammable).

E.    Most covalent compounds do not conduct electricity in water like ionic compounds do.

F.    If electrons are not shared equally between all atoms, the molecule is said to be polar.  A polar bond makes one part of the molecule more positive and another part of the molecule more negative.  An example is water where the Hydrogen atoms are more positive and the oxygen is more negative because the electrons like the oxygen better.

Chapter 2 Study Guide

Chapter 2 Test Study Guide

Properties of Matter

To study for this test please use your brown notes on the Properties of Matter and Exothermic/Endothermic Reactions vs. Changes.  Also use labs on Physical Properties, Chemical Properties, Chemical Changes, Endothermic and Exothermic reactions, and Solutions.  Also study Density and Buoyancy.  Use homework assignments and the graphic organizer on physical and chemical changes and your textbook pages 58 – 77 as well.

Vocabulary to Know:

Energy   Matter    Properties of Matter     Physical Properties

Chemical Properties    Element     Atom      Molecule    Compound  

Mixture      Homogeneous Mixture     Heterogeneous Mixture

Solution     Solute    Solvent       Dilute Solution      

Super-Saturated Solution       Physical Change        Chemical Change    

Law Of Conservation of Matter        Thermal Energy

Temperature       Endothermic Reaction      Exothermic Reaction

Indicators of a Chemical Change         Precipitate

Density     Mass     Volume     Buoyant Force  Archimedes’ Principle

Concepts to Know:

1.    Everything is either energy or matter.

2.    Properties of matter are characteristics of a substance that help to identify that substance.  Physical properties are characteristics that can be observed and measured without breaking bonds or changing the substance chemically.  

Examples:  Color, shape, density, boiling point

Chemical properties can only be observed when a substance is changes chemically.

Examples: Reactivity with other chemicals, flammability

3.    An element is a pure substance that cannot be broken down into any other substance.  There are 92 naturally occurring elements in the universe.  Elements are organized on the Periodic Table of the Elements. 

4.    Atoms are the smallest particle of an element.

5.    Molecule – Two or more atoms chemically bonded.  Examples:  NaCl, CaCl₂, O₂, H₂O, H₂

6.    Compound – Two or more DIFFERENT types of atoms chemically bonded.  Example:  All of the examples for molecules BUT H₂.  H₂ is only made of one thing, Hydrogen.

7.    A mixture is two or more things combined together that have not been chemically bonded.  Solutions are a type of mixture where one thing dissolves into another. Examples: trail mix, salt water

8.    Heterogeneous Mixture – You can see the parts of the mixture

9.    Homogeneous Mixture – You can’t see the parts of the mixture.  A Solution is a type of Homogeneous Mixture.  In a solution a Solvent dissolves a Solute.  A “watered-down” solution is called Dilute.  A solution where there is too much solute is called Super-Saturated.

10.                  A physical change is a change in a substance that does not alter a substance chemically.  It’s still the same substance.

11.                  A chemical change is a change where bonds are broken and new substances are formed.  Example: Burning wood, reacting Sulfuric Acid and Sugar.

12.                  Law of Conservation of Matter says that whatever matter goes into a chemical reaction has to come out.

13.                  Thermal Energy is the measure of the amount of movement of molecules in a substance.  The more movement, the more thermal energy, the higher the temperature.  Temperature is a measure of the thermal energy of an object.  We measure thermal energy (temperature) with a thermometer.

14.                  Know the indicators of a chemical change and that a precipitate is a solid formed from a chemical reaction between two or more substances.