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.

Chapter 1 - Study Guide

Study Guide – Test Chapter 1

Scientific Inquiry, Density, and Buoyancy

  

I.               Scientific Inquiry and Data

A.    Hypothesis – what is it?

B.     What are variables in an experiment?

C.    What is a manipulated/independent variable?

D.    What is a controlled experiment?

E.     Why is it important that an experiment be controlled?

F.     What is the responding/dependent variable in an experiment?

G.   What are Qualitative and Quantitative Data?

H.    Why is data important when writing conclusions?

I.       Be prepared to analyze a scientific experiment to identify parts of the experiment.

II.              Measurement

A.    Metric Unit of Length is a meter

B.     Weight is a measure of force (your weight is a force on the Earth).  The units are pounds and Newtons.

C.    Weight is determined by mass and gravity.

D.    Why would weight change as you move from Earth to space to the Moon but mass would not?

E.     Mass is the amount of matter in an object.  Mass is measured in grams on a balance.

F.     Volume is the amount of space something takes up.

G.   Volume of a regular object (length x width x height) cm³

H.    Volume of an irregular object (water displacement) milliliters

I.       Read a graduated cylinder at the bottom of the meniscus (curvature)

J.     Metric Conversions using a metric conversion line

III.            Equipment

IV.           Graphing

a.    Know the parts of a graph.

b.    Know how to read a graph to obtain data.

c.    Know how to construct a graph to show data

     d. Know how to find errors or missing information on a graph.