WorksheetsPeriod 11 Final Review
Total questions: 123
Worksheet time: 2hrs 5mins
Name
Class
Date
1.
Anything that has mass and volume is ______.
a)
matter
b)
mass
c)
density
d)
water
2.
An exothermic reaction _________.
a)
releases heat
b)
absorbs heat
3.
A ________ can be observed or measured without changing the composition.
a)
physical property
b)
physical change
c)
chemical property
d)
chemical change
4.
The smallest unit of an element that retains properties properties of that element is a(n) _____.
a)
atom
b)
mixture
c)
cell
d)
molecule
5.
_______ Is where the identity or composition of the substance does not change whereas a ____ is where the identity or composition of a substance changes and at least one new substance forms.
a)
physical change, chemical change
b)
physical property, chemical property
c)
physical change, physical property
d)
chemical change, physical change
6.
_____ is how compact a substance is the ratio of mass to volume.
a)
density
b)
weight
c)
matter
d)
atoms
7.
An endothermic reaction ______.
a)
absorbs heat
b)
releases heat
8.
Mass is the amount of _______in an object.
a)
matter
b)
volume
c)
weight
d)
density
9.
Weight is ______.
a)
affected by Gravity
b)
NOT affected by Gravity
10.
______ is a property that is observed as a substance undergoes a chemical change.
a)
chemical property
b)
physical property
c)
chemical change
d)
physical change
11.
What is the smallest fundamental unit of a chemical compound?
a)
a molecule
b)
an element
c)
an atom
d)
a cell
12.
What is matter that is composed of only one type of an atom that cannot be broken down into simpler substances?
a)
element
b)
mixture
c)
atom
d)
matter
13.
What is a type of pure substance that has definite physical and chemical properties?
a)
compound
b)
mass
c)
weight
d)
atom
14.
What is two or more elements or compounds that are physically combined?
a)
mixture
b)
atom
c)
solution
d)
solvent
15.
What is energy?
a)
The ability to change color
b)
The ability to ionise a metal
c)
The capacity to do work
d)
The capacity of gas that a container can hold
16.
What is NOT considered kinetic energy?
a)
Electrical
b)
Heat
c)
Motion
d)
Chemical energy
17.
What is the difference between potential energy and kinetic energy?
a)
KE is stored energy or chemical energy, whereas potential energy is the energy of motion
b)
KE is the energy of motion, whereas potential energy is stored energy or chemical energy
c)
There is no difference
d)
None of the above
18.
The Law of Conservation says that Energy can be both created and destroyed
a)
True
b)
Not enough information given
c)
False
d)
None of the above
19.
What is an exothermic reaction?
a)
A reaction which emits energy
b)
A reaction that neither emits or absorbs energy
c)
A reaction that can only happen in water
d)
A reaction that absorbs energy
20.
What is an endothermic reaction?
a)
A reaction which causes a colour change from red to blue of the substance
b)
A reaction that absorbs energy
c)
A reaction that emits energy
d)
a reaction which produces only soaps
21.
True or False: Activation energy is the minimum amount of energy required to start a reaction.
a)
True
b)
Not enough information
c)
Neither
d)
False
22.
True or False: Activation energy is the minimum amount of energy required to start a reaction. (This is lowered by the addition of a catalyst)
a)
True
b)
Not enough information
c)
Neither
d)
False
23.
What is heat?
a)
a measure of average potential energy of particles in an object
b)
The point of which water reaches its boiling point
c)
Energy that is transferred between objects that are at different temps
d)
None of the answers are correct
24.
True or False: Kinetic energy can be electrical energy, sound, heat, and motion.
a)
False
b)
True
c)
Not enough information
d)
None of the answers are correct
25.
J.J.Thomson discovered the electron using what?
a)
Cathode Ray Tube
b)
The gold foil experiment
c)
The planetary model
d)
Dalton's atomic theory
26.
Rutherford discovered the positively charged nucleus using what?
a)
Cathode Ray Tube
b)
The gold foil experiment
c)
The planetary model
d)
Dalton's atomic theory
27.
The Greek word "atomos" translates to "indivisible".
a)
True
b)
False
28.
In order Protons,electrons,and neutrons have what charges?
a)
Negative,positive, and no charge
b)
no charge,positive, and negative
c)
Positive,Negative, and no charge
29.
The D sublevel has how many orbitals?
a)
1
b)
7
c)
5
d)
3
30.
The electron spin +1/2 indicates a....
a)
clockwise spin
b)
counter clockwise spin
31.
The further from the nucleus an e orbital is, the less energy it has.
a)
true
b)
False
32.
What is the lowest energy state of an e- ?
a)
Up state
b)
Bottom state
c)
Ground state
d)
low state
33.
Frequency and wavelength are inversely proportional.
a)
False
b)
True
34.
Energy is measured in what?
a)
Joules
b)
Inches
c)
Volts
d)
Gigawatts
35.
What is the major region to the far left (group 1) of the Periodic Table called?
a)
Alkali Metals
b)
Metalloids
c)
Alkaline Earth Metals
d)
Halogens
36.
What is the major region in group 2 of the Periodic Table called?
a)
Electronegativity
b)
Carbon
c)
Alkaline Earth Metals
d)
Noble Gases
37.
What is the major region in the center (Groups 3-12) of the Periodic Table called?
a)
Gases
b)
Transition Metals
c)
Protons
d)
Alkali Metals
38.
What is the major region in group 17 of the Periodic Table called?
a)
Noble Gases
b)
Alkaline Earth Metals
c)
Electron Affinity
d)
Halogens
39.
What is the major region to the far right (group 18) of the Periodic Table called?
a)
Endothermic
b)
Alkali Metals
c)
Noble Gases
d)
Oxygen
40.
What are the Rare-Earth elements #57-70 classified as?
a)
Lanthanides
b)
Sig Figs
c)
Actinides
d)
Halogens
41.
What are the Rare-Earth elements #89-102 classified as?
a)
Ionization Energy
b)
Lanthanides
c)
Actinides
d)
Transition Metals
42.
What are the substances with properties of metals and nonmetals classified as? (Found on the Step Line in Periodic Table)
a)
Alkaline Earth Metals
b)
Covalent Bonds
c)
Alkali Metals
d)
Metalloids
43.
What is the measure of the ability of an atom in a compound to attract electrons called?
a)
Ionization Energy
b)
Electron Affinity
c)
Electronegativity
d)
Nucleus
44.
What is the measure of the energy change when an electron is added to a neutral atom to form a negative ion?
a)
Neutrons
b)
Ionization Energy
c)
Electron Affinity
d)
Atomic Radius
45.
What is the energy required to remove an electron from a neutral atom?
a)
Electronegativity
b)
Law of Gases
c)
Atomic Radius
d)
Ionization Energy
46.
What is the distance from the center of the nucleus to the valence shell?
a)
Atomic Radius
b)
Electronegativity
c)
Electron Affinity
d)
Ionic Bonding
47.
What is it called when a very heavy nucleus splits into smaller nuclei and one or more neutrons?
a)
Nuclear Fusion
b)
Nuclear Fission
48.
What is it called when two smaller nuclei combine to form a larger, more stable nucleus?
a)
Nuclear Fission
b)
Nuclear Fusion
49.
Charged atom
a)
Electron
b)
Transition metals
c)
Ion
d)
Anion
50.
May have more than one charge
a)
Transition metals
b)
Monatomic Ion
c)
Ionic bonds
d)
Polyatomic Ions
51.
Atoms react to achieve full valence shells
a)
Empirical formula
b)
Molecular formula
c)
Octet Rule
d)
Ionic bonds
52.
Ion made from a single atom
a)
Polyatomic Ion
b)
Monatomic Ion
c)
Ion
d)
Cation
53.
Ion made up of 3 or more atoms
a)
diatomic ion
b)
Monatomic Ion
c)
Ionic bonds
d)
Polyatomic Ion
54.
Forms between a cation and an anion
a)
Ionic bonds
b)
Octet Rule
c)
Polyatomic Ion
d)
Ion
55.
Percent by mass of each element in a cmpd
a)
Percent Composition
b)
Empirical Formula
c)
Ionic Bonds
d)
Molecular Formula
56.
A formula that shows the composition of a cmpd in the simplest raito
a)
Molecular Formula
b)
Octet Rule
c)
Percent Composition
d)
Empirical Formula
57.
A formula that shows the exact number & kinds of atoms in a molecule (not always the simplest ratio)
a)
Empirical Formula
b)
Molecular Formula
c)
Ionic Bonds
d)
Percent Composition
58.
Losing e- produces a (+) charge
a)
Ion
b)
Cation
c)
Transition Metals
d)
Anion
59.
Gaining e- produces a (-) charge
a)
Anion
b)
Ion
c)
Transition Metals
d)
Cation
60.
What is the formula for Cesium nitride
a)
CuO
b)
Cs3N
c)
ClO
d)
CH
61.
What is the formula for Copper (ll) oxide
a)
CuO
b)
ClH
c)
CaCl
d)
CuH
62.
What is the formula for Barium carbonate
a)
Bel2
b)
BrO
c)
BaCO3
d)
BaO
63.
What is the name of Bel2
a)
Beryllium Oxide
b)
Beryllium lodide
c)
Barium carbonate
d)
Bromine Sulfate
64.
What is the name of NiCl3
a)
Nickel (lll)
b)
Nickel (lll) Chloride
c)
Nickel (ll) Chloride
d)
Iron (lll) Chloride
65.
What is the name of (NH4)2Cr207
a)
Nickle (lll) Chloride
b)
Sodium Nitrate
c)
Aluminum Dichromate
d)
Ammonium Dichromate
66.
What is the percent of the element Na in NaCl?
a)
39.34%
b)
49.34%
c)
59.47%
d)
78.12%
67.
What is the percent of Cl in NaCl?
a)
30.44%
b)
70.99%
c)
60.66%
d)
80.77%
68.
What is the empirical formula for:
36.50 g(Na)
25.40 g(S)
38.10 g(O)
36.50 g(Na)
25.40 g(S)
38.10 g(O)
a)
NaSO
b)
Na2SO3
c)
NO
d)
NiCl3
69.
How many electrons are in the second valence shell?
a)
2
b)
4
c)
6
d)
8
70.
Covalent bonding is __________________.
a)
Sharing of electrons between atoms
b)
Donating of electrons between atoms
71.
What is a polar bond?
a)
e- are shared equally between atoms
b)
unequal sharing of e- between atoms
c)
transfer of e- between atoms
72.
Covalent bonds are between ___________.
a)
Metals and nonmetals
b)
Transition and nonmetals
c)
Two nonmetals
d)
Two metals
73.
Which type of bond is the weakest?
a)
Polar covalent
b)
Nonpolar covalent
c)
Ionic
74.
When does a resonance structure occur?
a)
When a molecule only has one possible Lewis structure
b)
When a molecule only has two or more possible Lewis structures
75.
What is a dipole?
a)
Same as an ion
b)
A molecule with a partial charge
c)
A molecule with no charge
76.
What are intermolecular forces?
a)
Attractive forces between molecules
b)
Attractive forces within molecules
c)
Repulsive forces between molecules
d)
Repulsive forces within molecules
77.
Written form of a chemical reaction
a)
Decomposition Reaction
b)
Chemical Equation
c)
Synthesis Reaction
d)
Coefficients
78.
Numbers in front of each product; used to balance equations
a)
Coefficients
b)
Net Ionic Equations
c)
Synthesis Reaction
d)
Double Replacement
79.
Oxygen reacts with a compound (CH or CHO) to form water & carbon dioxide
a)
Single Replacements (Displacement)
b)
Synthesis Reaction
c)
Combustion Reactions
d)
Net Ionic Equations
80.
2 or more substances combine to form One product
a)
Synthesis Reaction
b)
Combustion Reaction
c)
Chemical Equation
d)
Single Replacement (Displacement)
81.
A single reactant breaks down into 2 or more products
a)
Coefficients
b)
Double Replacement
c)
Combustion Reactions
d)
Decomposition Reactions
82.
A more reactive element replaces a less reactive element in a compund
a)
Coefficients
b)
Single Replacement (Displacement)
c)
Double Replacement
d)
Synthesis Reaction
83.
Anions and Cations of 2 molecules switch places, forming 2 new compounds
a)
Double Replacement
b)
Single Replacement (Displacement)
c)
Combustion Reaction
d)
Chemical Equation
84.
When ionic compounds dissolve in water, ions separate from each other. This equation only shows the ions that participate in the reaction
a)
Synthesis Reaction
b)
Net Ionic Equations
c)
Decomposition Reactions
d)
Combustion Reactions
85.
Identify the Double Replacement Reaction
a)
Fe + CuSO4 ➝ FeSO4 + Cu
b)
NaCl + AgNO3 ➝ NaNO3 + AgCl
c)
C10H18 + O2 ➝ CO2 + H2O
86.
Identify the Synthesis Reaction
a)
Na + Cl2 ➝ 2NaCl
b)
CaCO3 ➝ CaO + CO2
c)
C10H18 + O2 ➝ CO2 + H2O
87.
Balance this Equation:
___ Fe + ___ S ➝ ___ Fe2S3
___ Fe + ___ S ➝ ___ Fe2S3
a)
Fe + S ➝ Fe2S3
b)
2 Fe + 3 S ➝ Fe2S3
c)
Fe + 3 S ➝ Fe2S3
d)
2 Fe + S ➝2Fe2S3
88.
Balance this Equation:
___ C6H6 + ___ O2 ➝ ___ CO2 + ___ H2O
___ C6H6 + ___ O2 ➝ ___ CO2 + ___ H2O
a)
2 C6H6 + 15 O2 ➝ 12 CO2 + 6 H2O
b)
C6H6+ 7 O2➝6 CO2 + 3 H2O
c)
2 C6H6 + O2 ➝ CO2 + 6 H2O
d)
4 C6H6 + 15 O2➝ 6 CO2 + 12 H2O
89.
What is STP?
a)
Science, Technology and Performance
b)
Standard Temperature and Pressure
c)
Scientifically Treated Petroleum
90.
What is a Combustion Reaction?
a)
2 or more substances combine to form one product
b)
A more reactive element replaces a less reactive reactive element in a compound
c)
Oxygen reacts with a compound to form water & carbon dioxide
d)
A single reactant breaks down into 2 or more products
91.
What is a Decomposition Reaction?
a)
2 or more substances combine to form one product
b)
A more reactive element replaces a less reactive reactive element in a compound
c)
Oxygen reacts with a compound to form water & carbon dioxide
d)
A single reactant breaks down into 2 or more products
92.
What type of reaction is this?
Fe + CuSO4 ➝ FeSO4 + Cu
Fe + CuSO4 ➝ FeSO4 + Cu
a)
Double Replacement
b)
Decomposition Reaction
c)
Synthesis Reaction
d)
Single Replacement
93.
What type of reaction is this?
C10H18 + O2 ➝ CO2 + H2O
C10H18 + O2 ➝ CO2 + H2O
a)
Single Replacement
b)
Double Replacement
c)
Combustion Reaction
d)
Synthesis Reaction
94.
Define Theoretical Yield
a)
The amount of product produced in the lab
b)
Maximum amount of product that can be produced if everything works perfectly
c)
The amount of reactants required in a reaction
95.
Actual yield is defined as the amount of product that is actually produced from the reaction
a)
False
b)
True
96.
Cl2 & H2 form HCl. You obtain a 98% yield and you started with 3.00 moles of H2 and excess Chlorine, what amount of HCl was actually produced?
a)
214.6 grams
b)
215 grams
c)
420 grams
d)
214.62 grams
97.
A reaction is supposed to produce 200.0 grams of NaCl. After the lab, the NaCl is measured and there are 178 grams. How efficient is the reaction?
a)
90%
b)
89%
c)
88%
d)
86%
98.
15.0 g of K reacts with 15.0 g of iodine. Find the limiting reactant, excess reactant, and how much product is made in grams.
2K + I2 →2KI
2K + I2 →2KI
a)
LR = K; ER = I2; 19.6 g KI
b)
LR = I2; ER = K; 19.6 g KI
c)
LR = I2; ER = K; 19.66 g KI
d)
LR = K; ER = I2; 20 g KI
99.
How many mol of NaCl will be produced if 2.6 mol Cl2 react with an excess of Na? 2Na + Cl2 → 2NaCl
a)
5.2 g NaCl
b)
5.2 mol NaCl
c)
5,2 mol NaCl
d)
5.22 mol NaCl
100.
How many grams of chlorine are required to react completely with 5.00 moles of sodium? 2Na + Cl2 → 2NaCl
a)
177 mol Cl2
b)
177 g Cl2
c)
177 g Na
d)
177.1 g Cl2
101.
How many moles of oxygen are required to make 10.0 g or aluminum oxide? (Write the balanced equation)
a)
.15 mol O2
b)
.147 mol O2
c)
.1477 mol O2
d)
1 mol O2
102.
What is the formula for the ideal gas law?
a)
PV=nRT
b)
√M2/M1
c)
P1T2=P2T1
d)
V1T2=V2T1
103.
What is the combined gas law?
a)
Combination of Boyle's, Charles & Lussac's laws
b)
Relationship between all four variables of gases
c)
None of these
d)
Combination of ideal gas law and Avogadro's law
104.
What is the definition of Dalton's law?
a)
Relationship between volume and pressure
b)
Relationship between pressure and temperature
c)
Comparison between a solid and a liquid
d)
Gas exerts pressure as if it were the only gas
105.
What is the definiton for Boyle's law?
a)
Relationship between volume and pressure
b)
Compares rate of diffusion for different gases
c)
None of these
d)
Gase rates of diffusion are inveresly proportional
106.
The relationship between temperature and volume is the definition for Charles law.
a)
False
b)
True
107.
Gay-Lussac's law is the relationship between volume and temperature.
a)
True
b)
False
108.
How do you convert temperature from Celsius to Kelvin?
a)
Subtract 273
b)
Add 273
c)
Add 210
d)
Subtract 210
109.
What are the conditions of STP?
a)
273 degrees C and 1 atm
b)
0 degrees C and 3 atm
c)
0 degrees C and 1 atm
d)
10 degrees C and 1 atm
110.
The greenhouse effect is a warming of Earth's surface and the air above it and is caused by gases in the air that trap energy from the sun.
a)
True
b)
False
111.
What are the greenhouse gases?
a)
Nitrogen, hydrogen, and carbon dioxide
b)
Carbon dioxide, oxygen, and hydrogen
c)
Methane, propane, and ethane
d)
Water vapor, carbon dioxide, and methane
112.
What happens to a substance as it changes state from a liquid to a gas?
a)
Energy goes directly to increasing the kinetic energy and temperature.
b)
Energy goes directly to changing the phase
113.
What is the formula for dilutions?
a)
Mol solute/ L solution
b)
M1M2 = V1V2
c)
M1V1 = M2V2
d)
PV = nRT
114.
What is the general rule of solubility?
a)
Like dissolves unlike
b)
Liquids dissolves solids
c)
Liquids dissolves liquids
d)
Like dissolves like
115.
True or False?
A solute is a substance in the greatest quantity?
A solute is a substance in the greatest quantity?
a)
False
b)
True
116.
Oil and water are miscible
a)
true
b)
false
117.
How many grams of NaOH are needed to make 750.0 mL of a 6.00 M solution of NaOH?
a)
18.0 g
b)
180. g
c)
98.23 g
d)
67 g
118.
What are C and D considered in the Keq equation?
a)
Reactants in a balanced equation
b)
Reactants in a stoichiometry equation
c)
Products in a balanced equation
d)
Products in a stoichiometry equation
119.
What is NOT a step in order to prepare a solution?
a)
Place solute into volumetric flask of desired volume
b)
Put cap on flask and shake to mix
c)
Fill the entire flask up with distilled water
d)
Measure out mass of solute needed
120.
What are the units placed after solving an Keq equation?
a)
Grams
b)
No units
c)
Mol
d)
Liters
121.
What side is favored when adding CO to the equation?
2 C (g) + O2 (g) ↔ 2 CO (g)
2 C (g) + O2 (g) ↔ 2 CO (g)
a)
Forward
b)
Reverse
c)
Neither
122.
A reverse reaction points to what direction?
a)
Left
b)
Right
123.
What type of reaction is this?
A + B ↔ C + D + Heat
A + B ↔ C + D + Heat
a)
Endothermic
b)
Exothermic
100 %
