Download Chemistry Unit Test Study Guide (2012-2013)

Name _______________________________________________
Period __________ Date ______________ Test Date: ________________
Chemistry Unit Test Study Guide (2012-2013)
1. Chemistry Basics
a.
b.
c.
d.
e.
Atom (def.) ___________________________________________________________________________________________
Element (def.) _________________________________________________________________________ Ex. ____________
Compound (def.) ________________________________________________________________________Ex. ____________
Molecule (def.) _________________________________________________________________________ Ex. ____________
Mixture (def.) __________________________________________________________________________ Ex. ____________
2. Periodic Table
a.
b.
c.
This person developed the first useful periodic table: _____________________________________.
Properties
 Elements are arranged by increasing ____________________.
 The atomic mass of an element is determined by _______________________________________.
 The atomic number of an element represents ________________________________________.
 Metals are found on the left / right side of the staircase on the periodic table.
 Nonmetals are found on the left / right side of the staircase on the periodic table.
 The majority of the elements on the periodic table are metals / non-metals.
 Elements in the same group or family (column) have similar physical and chemical properties based on the number
of _________________ in their _______________ shell.
Matching Section:
1) Elements that share some properties with metals, and some with non-metals.
2) Column of elements in the periodic table that have similar physical or chemical properties.
3) An element that has a shiny luster, is a good conductor of heat and electricity, is malleable and ductile.
A) Halogens
B) Metal
C) Noble Gases
4) Elements in groups 3-12, like gold and silver.
5) Element that is usually a gas or brittle, solid at room temperature, and does not conduct heat and electricity
well.
6) Group 17 elements, such as F, Cl, and Br are known as this.
7) The most reactive elements in the periodic table are found in this group.
8) Elements in this group do not form compounds.
D) Metalloid
E) Transition
Element
F) Group 1
G) Non-metal
H) Group 2
3. Acids and Bases
a.
b.
c.
d.
e.
f.
The pH of a substance can be determined using ____________________ paper
Neutral substances have a pH of __________. An example of a common neutral substance is ____________.
Acids- Name 3 properties (ex: feel, taste, uses, etc.): 1. _______________ 2. _______________ 3. _____________
a. pH range for acids: ____________
Bases- Name 3 properties (ex: feel, taste, uses, etc.): 1. _______________ 2. _______________ 3. _____________
a. pH range for bases: ____________
True / False. Strong Acids and Strong Bases are both corrosive, which means they eat away at body tissue and dissolve
other objects, and should always be handled with care.
Interpreting a pH scale diagram:
a. Identify the strongest acid shown on the pH scale below: __________________
b. Identify the strongest base shown on the pH scale below: __________________
c. Identify the weakest acid shown on the pH scale below: __________________
d. Identify the weakest base shown on the pH scale below: __________________
e. Identify the neutral substance shown on the pH scale below: __________________
Stomach acid
lemon
grapes tomatoes bananas milk
water
eggs baking soda soap ammonia bleach
oven cleaner
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4. Mixtures
a.
b.
c.
d.
e.
Mixture (def.) ________________________________________________________
Heterogeneous (def.) ___________________________________________________
 Give 3 examples of a heterogeneous mixture: 1. ________________ 2. _________________ 3. ________________
Homogeneous (def.) ____________________________________________________
 Give 3 examples of a homogeneous mixture: 1. _________________ 2. _________________ 3. ________________
Separating Mixtures
 Name & give a brief description of the 4 ways that a mixture can be separated (some of which we did in class!)
1. _________________________________________________________________________________
2. _________________________________________________________________________________
3. _________________________________________________________________________________
4. _________________________________________________________________________________
Solutions
 Solute (def.) ____________________________________________________________________________
 Solvent (def.) ___________________________________________________________________________
 Solubility (def.) __________________________________________________________________________
 In Kool-Aid, identify the solute: ___________________ and the solvent: _______________
 TRUE / FALSE. When a solid dissolves in water, each particle becomes surrounded by water molecules.
5. Model of the Atom: Evolution of the Atomic Theory
Atoms are so small that scientists create models to describe them. Complete the table below for each of the scientists that
have contributed to the evolution of the atomic model.
Scientist
Discovery
Name of atomic model
Year
1
2
3
4
5
6
6. Parts of an Atom
a.
Shown below is the Bohr model of the atom, proposed by scientist Niels Bohr. Scientists create models to describe atoms,
because __________________________________.
Subatomic
Mass
Location in the
Charge
Particle
(in amu)
atom
Proton
Electron
Neutron
Nucleus
The atom is made up of mostly ___________ ____________.
d.
e.
f.
b. The greatest number of valence electrons an atom can have is ______.
c. The majority of the mass of an atom is found ____________________.
This atom has ______ valence electrons, and has _______ electrons that would be involved in bonding.
In an atom which has an equal number of protons and electrons, the atom’s charge would be _______________.
An atom is made up of mostly ______________ space.
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7. Properties of Atoms
Fill in the blanks for the elements in this chart. When completing this chart, round all atomic masses to the nearest whole number.
Reminder: Atomic mass = # of ____________ + # of ______________; Atomic number = # of ________________
Element
Atomic
Symbol
Group
#
# of Valence
Electrons
# of protons
# of
neutrons
# of
electrons
Atomic
mass #
Atomic
number
Sodium
Carbon
Oxygen
Phosphorus
Hydrogen
Nitrogen
Chlorine
8. Gaining or Losing Electrons
a.
b.
c.
d.
e.
f.
g.
An atom that has gained or lost an electron is called a(n) _________________________
What is a cation? ____________________________________
What is an anion? ____________________________________
The charge becomes positive when what has happened?
___________________________________________________________________
The charge becomes negative when what has happened?
___________________________________________________________________
If an atom in group 16 gains 2 electrons, how many valence electrons will it have? _______ What will its charge be?
_______
What charges attract to each other? _______________________________________
9. Bonding
Circle the word that makes each of the sentences below correct.
a. Atoms are held together in molecules by physical / chemical bonds.
b. Which electrons (name and location) are involved in chemical bonding? __________________________________________
c. Ionic bonds:
 Metal/non-metal OR non-metal/non-metal bond together in ionic bonds and electrons are shared / transferred.
d. Covalent bonds
 Metal/non-metal OR non-metal/non-metal bond together in covalent bonds and electrons are shared / transferred.
e. Classify the following compounds as ionic or covalent:
 KCl _________________
CO2 _________________
NaCl ________________ CH4 _________________
f. Molecules such as H2, N2, O2, and Cl2 are called ______________ molecules.
g. Draw the following molecules:
i) Nitrogen triiodide
Formula: _________
(Lewis Structure)
(Structural Formula)
ii) Mg3N2
Name: _____________________
(Use arrows to draw how Magnesium and Nitrogen ionically bond.)
10. Naming Chemical Formulas
a.
Naming Covalent Molecules
 Prefixes: 1 atom-_______; 2 atoms-_____; 3 atoms______; 4 atoms-_______; 5 atoms-_______; 6 atoms-_______
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 Write names for the following covalent chemical formulas:
HBr _____________________
SCl4 _____________________
N2O4 ___________________
SO3 ____________________
b. Naming Ionic Molecules
 What is written first? Positive ion (cation) / negative ion (anion)
 The 2nd word is the first syllable of the 2nd, with the suffix (ending) _________.
 Ionic compounds use prefixes like mono-, di-, and tri-. True / False
NaCl _________________________
Li2O _________________________
CaF2 _________________________
MgO _________________________
Pb3N4 _________________________
Mn(CO3)2 _________________________
c. Common Names of Molecules- Complete the chart!
Formula
Chemical Name
Common Name
C6H12O6
Dihydrogen monoxide
Table Salt
Carbon dioxide
Carbon dioxide
Table Sugar
11. Physical and Chemical Changes
a.
c.
The Law of Conservation of Mass states that: _______________________________________________________________
Physical change (def.) ___________________________________________________________________________________
 List 3 pieces of evidence that a physical change has occurred: ___________________________________________
Chemical change (def.) __________________________________________________________________________________
 List 9 pieces of evidence that a chemical change has occurred: __________________________________________
_____________________________________________________________________________________________
Compare the physical and chemical properties of Salt with the properties of the elements that bond when it forms.
d.
Classify the following as a physical or chemical change:
b.
Example
Using electricity to break
H2O into H and O
Dissolving salt
in water
Rust forming
on a fence
Water
boiling
Burning
paper
Baking
cookies
Heating table
sugar
Physical
Chemical
e. Chemical Reactions
 The left side of a chemical reaction is made up of reactants / products, the right side is reactants / products.
f. Energy Transfer- Forms of energy: ___________________ ____________________
 A change that gives off energy is called ________________________________ Example _____________________
 A change that absorbs energy is called _________________________________ Example _____________________
g. TRUE / FALSE. The appearance of the reactants predicts the appearance of the products.
h. Identify which of the following equations are balanced; if it is not balanced, balance it:
 _1_ Na3PO4 + _3_ KOH  _3_ NaOH + _1_ K3PO4
 ___ P4 + ___ O2  _2_ P2O3

___ MgF2 + ___ Li2CO3  ___ MgCO3 + ___ LiF

i.
Identify the reactants and products from the following equation: ____ N2 + ____ H2  ____ NH3
2 RbNO3 + __ BeF2  __ Be(NO3)2 + 2 RbF
12. DNA
a. Name the five atoms found in the DNA molecule:
i. ______
ii. _____
iii. _____
vi. _____
v. _____
True/False questions: If false, re-write the corrected statement.
b. TRUE / FALSE. DNA is a micromolecule. ____________________________________________________________________
c. TRUE / FALSE. DNA’s shape is a single helix. _________________________________________________________________
d. TRUE / FALSE. A-T and G-C are base pairs in DNA. ____________________________________________________________
e. TRUE / FALSE. DNA has a sugar-phosphate backbone. _________________________________________________________
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