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Overreacting

Total questions: 87

Worksheet time: 1hrs 25mins

Name
Class
Date
1.

How many Al atoms are in this compound? 4Al2O3

a)

2

b)

8

c)

6

d)

4

2.
How many F atoms are in this compound?
6MgF2 
a)
2
b)
6
c)
8
d)
12
3.
The Law of Conservation of Mass states
a)
that matter exists in all states and reacts the same
b)
that matter can only be changed into new substances by introducing a catalyst
c)
that matter exists in the same state throughout any chemical change
d)
that matter cannot be created or destroyed and that the mass of the products must equal the mass of the reactants
4.

Is this chemical equation balanced? Why or why not? Choose the BEST answer.

a)

Yes, the amount of atoms for each element are equal on both the reactant and product side.

b)

No, the carbons are not the same number on both the reactant and product side.

c)

No, neither the carbons or hydrogens are the same amount on both the reactant and product side.

d)

No, none of the elements (carbon, hydrogen, or oxygen) are the same amount on both the reactant and product side.

5.
What are the correct coefficients when this equation is balanced?
KClO3  --> KCl  +  O2
a)
2,2,2
b)
2,2,3
c)
1,2,3
d)
3,3,3
6.
Which is the name of the kind of solid substance formed in this figure?  
a)
aqueous 
b)
precipitate
c)
acid
d)
synthesis 
7.
Which type of reaction takes place in the presence of oxygen and produces carbon dioxide and water?
a)
double replacement 
b)
decomposition 
c)
combustion 
d)
single replacement
8.
Predict the following reaction 
NaCl   +   Ca(NO3)2 --> 
a)
no reaction both products are aqueous 
b)
Calcium chloride and sodium nitrate are produced  
c)
sodium nitrate is a solid formed 
d)
calcium chloride is the solid formed
9.

Why are chemical equations always balanced? Select ALL that apply.

a)

Matter cannot be created.

b)

Matter cannot be destroyed.

c)

Matter can only be rearranged/conserved.

d)

Matter doesn't matter.

10.
Balancing this reaction: ____ CH4 + ____ O2 ---> ____ CO2 + ____ H2O
a)
2,1,3,1
b)
1,2,1,2
c)
1,2,2,1
d)
2,1,1,2
11.

What charge do electrons have?

a)

positive

b)

negative

c)

neutral

12.

Subatomic particles with a negative charge

a)

Electrons

b)

Neutrons

c)

Protons

d)

Quarks

13.

An atom has 10 protons and 11 neutrons. What is the atomic number

a)

10

b)

11

c)

21

d)

22

14.
an atom or molecule which has gained or lost one or more of its valence electrons
a)
Covalent Bond
b)
Chemical Formula
c)
Ion
d)
Compound
15.
Value representing the number of protons in an element
a)
Atomic Mass
b)
Mass Number
c)
Valence Electrons
d)
Atomic Number
16.

Which of the following elements is a metal?

a)

Sodium

b)

Oxygen

c)

Hydrogen

d)

Argon

17.

An atom has a mass of 35 and an atomic number of 17. How many neutrons does this atom have?

a)

35

b)

17

c)

18

d)

52

18.
What is the electron configuration of sodium?
a)
2.8
b)
2.8.2
c)
2.8.1
d)
11
19.
Which element has an electron configuration of 2.5?
a)
Oxygen
b)
Nitrogen
c)
Phosphorus
d)
Carbon
20.

How are ions formed?

a)

Gaining or losing protons

b)

Gaining or losing neutrons

c)

Gaining or losing electrons

d)

Gaining of losing mass

21.
Atoms of the same element with a different number of neutrons
a)
Ion
b)
Gluons
c)
Isotope
d)
Quarks
22.
Subatomic particles that are neutral in charge
a)
Neutrons
b)
Protons
c)
Nucleus 
d)
Electrons
23.
The only element with no neutrons in its nucleus.
a)
Oxygen
b)
Helium 
c)
Hydrogen
d)
Lithium
24.
Calculation used to find the number of neutrons in an atom
a)
Atomic Mass - Atomic Number
b)
Atomic Number - Atomic Mass
c)
Atomic Mass - Electrons
d)
none of these
25.
The word "atom" comes from a Greek word that means
a)
Invisible
b)
Indivisible
c)
Undivided
26.
Discovered the nucleus of the atom through the Gold Foil Experiment
a)
Rutherford
b)
Chadwick
c)
Thomson
d)
Dalton
27.
Created the Planetary Model of the atom
a)
Bohr
b)
Dalton
c)
Rutherford
d)
Chadwick
28.
Discovered the neutron within the atom
a)
Democritus
b)
Thomson
c)
Rutherford
d)
Chadwick
29.
How did Rutherford discover the proton?
a)
Cathode tube ray experiment
b)
Gold Foil Experiment
c)
Planetary Model
d)
Plum Pudding Model
30.
The scientist responsible for "discovering" the nucleus is:
a)
Bohr
b)
Rutherford
c)
Schroedinger
d)
Einstein
31.
What scientist is best known for his "Plum Pudding" model of the atom?
a)
J.J. Thomson
b)
Ernest Rutherford
c)
John Dalton
d)
Democritus
32.
What contribution did John Dalton make to atomic theory? 
a)
He discovered that every atom was positively charged. 
b)
He discovered that every element consisted of one type of atom that couldn't be divided. 
c)
He discovered that atoms had nuclei. 
d)
He discovered that atoms could be divided into smaller parts. 
33.
Rutherford's gold foil experiment provided evidence that...
a)
negative and positive charges are spread evenly throughout the atom.
b)
alpha particles have a positive charge.
c)
gold is not a dense as previously thought.
d)
there is a dense positively charged nucleus at the center of an atom.
34.
Who came up with the model of an atom pictured?
a)
J.J. Thompson
b)
Ernest Rutherford
c)
Neils Bohr
d)
James Chadwick
35.
Place the following scientists in order, from earliest to latest: 
Rutherford, Dalton, Bohr, Thomson
a)
Dalton, Rutherford, Bohr, Thomson
b)
Thomson, Dalton, Rutherford, Bohr
c)
Dalton, Thomson, Rutherford, Bohr
d)
Bohr, Dalton, Rutherford, Thomson
36.
He discovered the electron using cathode ray tube experiment.
a)
Joseph Thomson
b)
John Dalton
c)
Ernest Rutherford
d)
Robert Millikan
37.
What makes something radioactive?
a)
elements with an atomic number above 81
b)
an unstable nucleus
c)
contaminated sewage
d)
It decays over time
38.

An isotope of an element has the same number of _________, but a different number of _________.

a)

Protons, electrons

b)

Protons, neutrons

c)

Electrons, neutrons

d)

Neutrons, protons

39.
In the symbol 20682Pb what does 206 stand for?
a)
Mass number
b)
Atomic number
c)
Atomic mass
d)
Number of protons
40.
In order of most to least penetrating radiation we have
a)
Alpha , Beta,  Gamma
b)
Beta , Gamma , Alpha
c)
Gamma, Beta, Alpha
d)
Gamma, Alpha, Beta
41.

Which type of radiation releases an electron?

a)

Alpha radiation

b)

Beta radiation

c)

Gamma radiation

d)

Theta radiation

42.

What particle is released when an unstable isotope undergoes alpha radiation?

a)

a helium nucleus

b)

an electron

c)

a photon of light

d)

a neutron

43.
Which type of radioactive decay is occurring in this equation? 
a)
Alpha decay
b)
beta decay
c)
gamma decay
d)
positron emission
44.

What type of decay is shown here

23892U ---> 23490Th + 42He.

a)

alpha

b)

beta

c)

gamma

45.
The half-life of strontium-90 is 25 years. How much strontium-90 will remain after 100 years if the initial amount is 4.0 g?
a)
3.0g
b)
0.25mg
c)
0.3g
d)
0.25g
46.
Which process involves the splitting of large nuclei?
a)
alpha decay
b)
nuclear fusion
c)
beta decay
d)
nuclear fission
47.
The rate at which a radioactive element decays is its ____.
a)
quarter life
b)
whole life
c)
wonderful life 
d)
half life
48.
Where does radioactivity have application in our lives?
a)
Medicine
b)
Energy (electricity)
c)
Agriculture
d)
All of the above
49.

Name the ionic compound, CaCO3

a)

calcium carbide

b)

calcium carbon trioxide

c)

calcium carbon oxide

d)

calcium carbonate

50.

Name the ionic compound, FeBr3

a)

Iron (II) bromide

b)

Iron (III) bromide

51.

What is the name for AlBr3?

a)

aluminum bromide

b)

aluminum tribromide

c)

aluminum bromine

d)

monoaluminum tribromide

52.

In a chemical reaction, if the reactants are heated, the reaction usually happens

a)

slower

b)

faster

c)

at the same rate

d)

in a smaller volume

53.
Raising the temperature of a chemical reaction would make the reaction __________________.
a)
happen slower
b)
happen faster
c)
stop completely
d)
proceed as normal
54.

What does it mean for a reaction to be endothermic? Choose 2 of the following.

a)

When two substances react, the temperature of the mixture decreases.

b)

When two substances react, the temperature of the mixture increases.

c)

There is less energy going into the reactant to break the bond than there is energy leaving the product.

d)

There is more energy going into the reactant to break the bond than there is energy leaving the product.

e)

The amount of energy entering and leaving is the same.

55.
Increasing the concentration of a reactant in a chemical reaction will _____________.
a)
decrease the rate of the reaction
b)
stop the reaction from happening
c)
increase the rate of the reaction
d)
have no effect on the rate of the reacion
56.

What does it mean for a reaction to be exothermic? Choose 2 of the following.

a)

When two substances react, the temperature of the mixture decreases.

b)

When two substances react, the temperature of the mixture increases.

c)

There is less energy going into the reactant to break the bond than there is energy leaving the product.

d)

There is more energy going into the reactant to break the bond than there is energy leaving the product.

e)

The amount of energy entering and leaving is the same.

57.
type of chemical reaction where two compounds react, and the positive ions (cation) and the negative ions (anion) of the two reactants switch places, forming two new compounds or products
a)
Double Displacement
b)
Single Displacement
c)
Synthesis
d)
Decomposition
58.

If the temperature at which a reaction occurs increases, the number of collisions decreases.

a)

True

b)

False

59.
The rate of a chemical reaction is NOT affected by which of the following:
a)
temperature
b)
concentration
c)
particle size (surface area)
d)
All of these affect reaction rates
60.

Orientation of molecules during a reaction does not affect the production of products.

a)

True

b)

False

61.
Products will form faster if____________
a)
the particle size of the reactants are larger.
b)
temperature is decreased.
c)
concentration of the reactants are increased.
d)
the reaction is not stirred.
62.
Catalysts permit reactions to proceed along a ___________energy path.
a)
lower
b)
higher
63.

Predict the precipitate when you mix silver nitrate and sodium chloride:

a)

AgNO3

b)

No precipitate

c)

AgCl

d)

NaNO3

64.

When you mix magnesium nitrate and sodium hydroxide

a)

No precipitate

b)

NaOH

c)

NaNO3

d)

Mg(OH)2

65.

The collision theory states that atoms, ions, and molecules must collide in order to react.

a)

True

b)

False

66.
An acid reacts with metal to produce 
a)
Carbon dioxide 
b)
Hydrogen gas
c)
Hydrogen gas and water 
d)
Salt and hydrogen gas 
67.
A neutralisation reaction produces 
a)
An acid 
b)
A neutral substance 
c)
Only water 
d)
Salt and water 
68.
What type of reaction is the following: 
HCl  + Zn --> ZnCl2 + H2
a)
Neutralisation
b)
Acid and a metal 
c)
Acid and a carbonate 
d)
Ionic 
69.
Complete the following reaction:
Hydrochloric acid + magnesium hydroxide --> 
a)
Magnesium chloride + water 
b)
Magnesium + water
c)
Magnesium chloride + hydrogen gas 
d)
Magnesium chloride + water + carbon dioxide 
70.
Incomplete combustion is when there is a limited amount of oxygen.
a)
True
b)
False
71.
Complete combustion is when there is plenty of oxygen to react with. 
a)
True
b)
False
72.

In heat transfer, heat always flows from the _______________ substance to the _______________ substance.

a)

Hotter to colder

b)

Colder to hotter

c)

Hotter to hotter

d)

Colder to colder

73.

Look at the solubility curve - as a GENERAL rule (that means there are exceptions, as always, in science) what trend can be states about how temperature affects the solubility of the compounds shown.

a)

Temperature has NO affect.

b)

The relationship is inversely proportional - as temperature increases, the solubility decreases.

c)

The relationship is directly proportional - as temperature increases, the solubility increases.

d)

It varies - the solubility will increase and then decrease when it reaches a certain temperature.

74.

You can buy salt in different forms - granulated (like what you have on your table), course ground (kosher salt) and rock salt (for making ice cream).


If you used the rock salt as the solute in a rate of dissolving investigation, which of the following WOULD NOT increase the rate at which the rock salt would dissolve?

a)

Crushing the solute.

b)

Stirring the solution.

c)

Heating the solution.

d)

Increasing the amount of solute.

75.
What type of reaction occurs in a hand warmer
a)
exothermic
b)
endothermic
76.
A student mixed two chemicals to allow them to react. The temperature before the reaction was 25 ° C. The temperature after the reaction was 18° C. Which of the following is true? 
a)
The temperature changed 
b)
It is an endothermic reaction
c)
It is an exothermic reaction 
d)
Two of the answers are correct 
77.
Iron rust in the presence of:
a)
Vacuum
b)
Moisture
c)
Oxygen
d)
Moisture and Oxygen
78.

Which diagram shows the most favourable conditions for rust to appear on the nail?

a)

A

b)

B

c)

C

d)

D

79.

Which of the following is / are examples of sacrificial protection against rusting?

(1) Iron object coated with tin

(2) Underground iron pipes connected to magnesium bars

(3) Iron railings coated with paint

a)

(1) only

b)

(2) only

c)

(1) and (3) only

d)

(2) and (3) only

80.

Galvanizing is a process of:

a)

Applying a Zinc coating to bare steel

b)

Washing the body with the phosphate coating

c)

dipping a body in E-COAT

d)

Chemically etching primer to steel

81.

What is the chemical nature of rust?

a)

iron (II) oxide

b)

hydrated iron (II) oxide

c)

iron (III) oxide

d)

hydrated iron(III) oxide

82.

What conditions are required for rusting?

a)

water only

b)

oxygen only

c)

water and oxygen

83.

Which metal is more reactive than calcium?

a)

magnesium

b)

potassium

c)

silver

d)

aluminum

84.
What will be the result of :  Zn + AuCl2->
a)
ZnCl2 +Au
b)
ZnAu + Cl2
c)
no reaction
d)
ClAu + Zn
85.
Will silver react with magnesium chloride solution?
a)
yes
b)
no
86.

The correct equations for dissolving a salt is

a)

NaOH(s) --> Na+(aq) + OH-(aq)

b)

NaOH(s) --> Na(aq) + OH(aq)

c)

NaOH --> Na + OH

87.

The simplified equation for corrosion:

a)

Fe + O2 -> Fe3O2

b)

Fe + O -> FeO

c)

Fe + O2 -> Fe2O3

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