Download Chemistry Final Study Guide

Chemistry Final Study Guide
Name _________________________________ Period ________
Directions: Take out your McDougal Littell textbooks (Matter and Energy and Chemical Interactions). Work with your
small group to complete the chemistry final study guide.
Chapter 1 Matter & Energy – on AIMS
Compound
mass
mixture
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element
gas
pure substance
volume
motion
liquid
atom
solid
molecule
__________ is a measure of how much matter an object contains.
__________ is the measure of the amount of space matter occupies.
An __________ is the smallest basic unit of matter.
A __________ is two or more atoms bonded together.
Atoms and molecules are always in __________.
A __________ __________ cannot be broken down by ordinary physical means.
A __________ contains two or more pure substances.
A __________ has a fixed volume and a fixed shape.
A __________ has a fixed volume but no fixed shape.
A __________ has no fixed volume and no fixed shape.
An __________ is a pure substance made of only one type of atom.
A __________ is made of two or more different atoms bonded together in a specific ratio.
Chapter 2 Matter & Energy – on AIMS
condensation
sublimation
substance
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melting point
boiling
new
melting
density
state
freezing
boiling point
magnetic
freezing point evaporation
physical
chemical
solubility
A __________ property can be observed without changing the substance.
Physical changes can change some physical properties but do not change the __________.
__________ properties describe how substances form new substances.
Chemical changes create __________ substances.
Changes in __________ are physical changes.
The process by which a solid becomes a liquid is called __________.
The lowest temperature at which a substance begins to melt is called its __________ __________.
__________ is the process by which a liquid becomes a solid.
The temperature at which a specific liquid becomes a solid is called the __________ __________ of the
substance.
__________ is the process by which a liquid becomes a gas.
When a solid changes directly to a gas, the process is called __________.
__________ is another process by which a liquid becomes a gas.
Boiling can occur only when the liquid reaches a certain temperature, called the __________ __________.
The process by which a gas changes its state to become a liquid is called __________.
Physical properties can be used to identify a substance, such as __________, __________, and __________
properties.
Chapter 4 Matter & Energy
Kinetic theory of matter
gases
solids
heat
temperature
liquids
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The kinetic theory of matter states that all of the particles that make up matter are constantly in motion.
Temperature is a measure of the average kinetic energy of all of the particles in an object.
Heat is a flow of energy from an object at a higher temperature to an object at a lower temperature.
Particles in solids are held tightly together but are always in motion.
Particles in liquids slide by one another and are always in motion.
Particles in gases are completely free to move and are always in motion.
Chapter 1 Chemical Interactions (online Chemistry Booknotes Chapter 5) – Some topics on AIMS
half-life
valence electrons
atomic mass number
alkali metals
half-life
period
isotope
proton
halogens
Electron cloud
group
nonmetal
neutron
transition
two
ion
metals
electrons
rare earth
one
radioactivity periodic table
metalloids
Metalloids
nucleus
atomic number
alkaline earth metals noble
electron
34. Atoms are made of positive __________, neutral __________, and negative __________.
35. The protons and neutrons are located in the __________, while the electrons are found in an __________
__________.
36. The number of protons identifies an element and is called the __________ __________.
37. The number of protons plus neutrons is the __________ __________ __________.
38. When an atom has a different number of neutrons it is called an __________.
39. An __________ forms when an atom gains or loses electrons.
40. Elements are organized by atomic number on the __________ __________.
41. The vertical columns are called __________, and elements within each of these have similar properties.
42. The horizontal rows are called __________, and each of these indicates what energy level is being filled with
electrons.
43. The three major categories of elements on the periodic table are the __________, __________, and
__________.
44. The first group on the periodic table is called the __________ __________, and they are very reactive due to the
fact that they tend to lose one __________.
45. Electrons in the outer energy level are called __________ __________.
46. The second group on the periodic table is called the __________ __________ __________, and they tend to lose
__________ electrons.
47. The elements in Groups 3-12 are called the __________ metals.
48. The two detached rows at the bottom of the periodic table are called the __________ __________ elements
because they were hard to isolate in pure form.
49. The elements in Group 17 are called the __________, and are very reactive nonmetals.
50. Group 18 elements are called the __________ gases because they almost never react with other elements.
51. __________ are elements that have properties of both metals and nonmetals.
52. The process by which atoms produce energy and particles is called __________.
53. The amount of time that it takes for one-half of the atoms in a particular sample to decay is called the
__________ of the isotope.
Chapter 2 Chemical Interactions (online Chemistry Booknotes Chapter 6)
metallic bond
covalent bond
ionic bond
subscript
chemical formula
bond structure
polar covalent bond
54. The name of a compound or molecule is written in a __________ __________.
55. The __________ tells how many atoms are in the compound.
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In an __________ __________ the electrons are transferred.
In a __________ __________ the electrons are shared.
In a __________ __________ __________ the electrons are shared unequally, as in water.
__________ __________ form between metals; electrons are shared in all directions.
Carbon takes on different forms due to a change in the __________ ___________.
Chapter 3 Chemical Interactions (online Chemistry Booknotes Chapter 7)
Bond energy conservation of mass law
coefficient
reactants
respiration
catalyst
precipitate forms
Synthesis
combustion
increasing concentration
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chemical equation
endothermic
color change
gas forms
decomposition
arrow
respiration
exothermic
products
photosynthesis
temperature change
adding a catalyst
increasing surface area
yields
balanced
Chemical reactions are described in __________ __________.
__________ are on the left side of a chemical equation, while __________ are on the right.
The __________ indicates the direction of the reaction and is read as __________.
Evidence for a chemical reaction includes __________ __________, __________ __________, __________
__________, and __________ __________.
A __________ speeds up the rate of a reaction but is not used up in the reaction.
The _______________ _____ _________ _________ states that mass is neither created nor destroyed.
__________ chemical equations show the conservation of mass.
A __________ is used to balance chemical equations and it changes the number of molecules.
_________ ___________ is the energy the is required to break or form bonds.
In an __________ reaction more energy is released and the temperature increases.
In an __________ reaction more energy is absorbed and the temperature decreases.
An example of an important endothermic reaction is __________, where plants make glucose using carbon
dioxide, water, and sun light.
An example of an important exothermic reaction is __________, which is how living organisms break down
glucose into carbon dioxide, water, and usable energy.
In a __________ reaction, simple reactants combine to form a more complex product.
In a __________ reaction, a complex reactant is broken down into simpler products.
In a __________ reaction, oxygen is always a reactant and energy is always produced.
The rate of a chemical reaction can be increased by __________ ___________ __________, __________
___________ __________, or _______________ _______________.
Chapter 4 Chemical Interactions (online Chemistry Booknotes Chapter 8 – pH scale, Acids and Bases on AIMS)
Acids
solution
solubility
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bases
solute
molecules
pH scale
solvent
ions
neutral
soluble
acidic
saturated
basic
dilute
alloys
concentration
A __________ is a type of mixture in which one or more solutes are dissolved in a solvent.
A __________ dissolves in a __________.
Ionic compounds dissolve by forming __________, while covalent compounds for individual __________.
The amount of dissolved solute determines a solution’s __________.
The more __________ a substance is, the more of it will dissolve in a solution.
A solution that has a low concentration of solute is called a __________ solution.
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A solution that contains as much solute that can be dissolved in a solvent is called __________.
__________ donate protons (H+) in solutions, and__________ accept protons.
Acid/base strength is measured on the __________ __________.
A pH of 1-6 is considered __________, a pH of 7 is considered __________, and a pH of 8-14 is considered
__________.
88. Metal __________ are solid mixtures.
History of the Atom – Illustrate how the model of an Atom has changed over time
Democritus (460 BC – 370 BC)
Antoine Lavoisier (1743 – 1794)
John Dalton (1766 – 1844)
Draw these scientists’ Atomic Model(s) below:
J.J. Thomson (1856 – 1940)
Draw this scientist’s Atomic Model below:
Ernest Rutherford (1871 – 1937)
Draw this scientist’s Atomic Model below:
Niels Bohr (1885 – 1962)
Draw this scientist’s Atomic Model below:
Erwin Schrodinger (1887-1961)
Draw this scientist’s Atomic Model below:
James Chadwick (1891 – 1974)
Draw this scientist’s Atomic Model below:
Awesome Job completing the chemistry final study guide! Review through the information as a small group to prepare
for the chemistry final exam. 