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Phamistry IB Prep

Total questions: 98

Worksheet time: 25hrs 30mins

Name
Class
Date
1.

Na2S2O3 (aq) +HCl (aq) → S (s) +SO2 (g)+NaCl (aq)+H2O (l)Na_2S_2O_3\ \left(aq\right)\ +HCl\ \left(aq\right)\ \rightarrow\ S\ \left(s\right)\ +SO_2\ \left(g\right)+NaCl\ \left(aq\right)+H_2O\ \left(l\right) What is the sum of the coefficients when the equation is balanced with the lowest whole number ratio?

a)

8

b)

16

c)

5

d)

7

2.

What is the number of atoms of Oxygen in 2 moles of Na2CO3∘ 10 H2ONa_2CO_3\circ\ 10\ H_2O

(You will need Avogadro's number and flow chart for stoichiometry calculations)

a)

1.6 ×10251.6\ \times10^{25} atoms (O)

b)

13 atoms (O)

c)

4 atoms (O)

d)

3.6 ×10233.6\ \times10^{23} atoms (O)

3.
11.
LiOH + KCl → LiCl + KOH 

b)  I actually produced 6 grams of lithium chloride and I began this reaction with 20 grams of lithium hydroxide. What is my percent yield?
a)
16.9%
b)
5.91%
c)
1.88%
d)
12.3%
4.
CH4 + 2 O2 → CO2 + 2 H2O
How many moles of carbon dioxide are produced from the combustion of 110 g of CH4?
a)
13.7 mol
b)
2.75 mol
c)
6.11 mol
d)
6.85 mol
5.
N2 +  3H2 → 2NH3 
How many moles of hydrogen are needed to react with 2 moles of nitrogen?
a)

6 mol H

b)

2 mol H

c)

3 mol H

d)

1 mol H

6.
9. Complete the equation for the percent yield of a chemical reaction:
Percent yield=(________)÷(________)×100%
a)
actual yield; theoretical yield
b)
theoretical yield; actual yield
7.
What is the molar mass of C6H12O6?
a)

180.18 g/mol

b)

180.12 g/mol

c)

180.24 g/mol

d)

180.06 g/mol

8.
What is the measured amount of a product obtained from a chemical reaction?
a)
mole ratio
b)
theoretical yield
c)
percentage yield
d)
actual yield
9.
 SiO2 + 3C → SiC + 2CO
I need to add 8 moles of Carbon to the reaction. How many grams of Carbon should I weigh?
a)
96 g
b)
0.67 g
c)
2.67 g
d)
48 g
10.
An aqueous solution of MgSO4 is added to an aqueous solution of BaCl2 to form BaSO4 and MgCl2. If 1.75 g of MgSO4 and 2.75 g of BaCl2 are used, calculate the mass of BaSO4 produced after the reactant has completed. [Mr MgSO4 = 120.4; BaCl2 = 208.3; BaSO4 = 233.4; MgCl2 = 95.3]
a)

2.03 g

b)

1.96 g

c)

3.08 g

d)

1.50 g

11.
Balance the following equation in acidic medium
aMnO4-(aq) + bC2O42-(aq) →cMn2+(aq) + dCO2(g) + eH2O(l)
The sum of the coefficient a+b+c+d+d
a)
43
b)
27
c)
29
d)
25
12.

How many mL of 0.5M HNO3 would be needed to react with 85mL of 0.75M KOH?

a)

127.5mL

b)

0.1275mL

c)

31.9mL

d)

0.031875mL

13.

What would the molarity of the solution be if 0.475 mol of KNO3 were formed in this reaction and the final volume of the solution was 595mL

a)

0.798M

b)

1.25M

c)

282.6M

d)

7.98x10-4M

14.

What is this subatomic particle that has positive charge?

a)

Electron

b)

Neutron

c)

Proton

d)

Megatron

15.

What is the atomic model proposed by J.J Thompson, and suggest that negatively-charged electrons were embedded in a kind of cloud or soup of positive charge?

a)

Asia's Next Top Model

b)

Quantum Atomic Model

c)

Plum Pudding Model

d)

Nuclear Model

16.
Where is most of the mass in an atom located?
a)
in the nucleus
b)
in the protons
c)
in the neutrons
d)
in the electrons
17.
What is the atomic number of the atom pictured? 
a)
9
b)
10
c)
18
d)
19
18.

What is this subatomic particle that has no charge?

a)

Electron

b)

Neutron

c)

Proton

d)

Megatron

19.
What element is represented in this Bohr Model? 
a)

Carbon

b)

Hydrogen

c)

Aluminum

d)

Lithium

20.

How is the molar mass found?

a)

It's the same as the atomic mass (polyatomic particles are the addition of all atoms)

b)
21.
Subatomic particle that has a negative charge and is located outside of the nucleus.
a)
Electron
b)
Proton
c)
Neutron
d)
Voltron
22.

What makes a valence electron more attracted to the nucleus?

a)

less distance between the nucleus and having less protons

b)

less distance between the nucleus and having more protons

c)

more distance between the nucleus and having less protons

d)

more distance between the nucleus and having more protons

e)

less distance and having more valence electrons

23.

Where are the elements that are usually silver, lustrous, conduct electricity and react with acid?

a)
b)
c)
24.

Where are the elements that are solids?

a)
b)
c)
25.

Elements that don't react.

a)
b)
c)
d)
26.

Samples of four Group 15 elements, antimony,

arsenic, bismuth, and phosphorus, are in the gaseous

phase. An atom in the ground state of which element

requires the least amount of energy to remove its

most loosely held electron?

a)

As

b)

Bi

c)

P

d)

Sb

27.

The diagram shows how a property of Period 3 elements varies across the period. What is the property?

a)

Atomic radius

b)

Electronegativity

c)

First ionisation energy

d)

Melting point

28.

Nitrogen will gain _ ve- to have a charge of _.

a)

5 , -5

b)

3, +3

c)

3, -3

d)

5, +5

29.

Which element has the lowest first ionization energy? (The letters are not the actual symbol of the elements

a)

11M

b)

12Q

c)

13R

d)

19L

30.

A full valence shell is considered having _ ve-.

a)

0

b)

2

c)

6

d)

8

31.

The ions P+, Q2+ , R3- and L2- have same electron configuration as nobel gas, argon. Which of the following statement is true about these ions. (The letters are not the actual symbol of the elements)

a)

They have the same of ionic size

b)

They are from the same period.

c)

The valence electrons in all ions experience the same effective nuclear charge.

d)

They have same number of valence electrons

32.
a)

A

b)

B

c)

C

d)

D

33.
a)

A

b)

B

c)

C

d)

D

34.

Another way to judge the tendency of two elements to form an ionic compound is by looking at electronegativity values. If the electronegativity difference is greater than 1.8, then it forms ionic bonds. Which of the following pairs will be most likely to form an ionic bond.

a)

Be and F

b)

Si and O

c)

N and Cl

d)

K and S

35.
a)

A

b)

B

c)

C

d)

D

36.

Which of the following molecules are polar molecule?

a)

HCl

b)

H2O

c)

CH4

d)

NH3

37.

Which of the following elements has the capability to form expanded octet?

a)

Hydrogen

b)

Carbon

c)

Sulfur

d)

Oxygen

38.

Which sub-atomic particle is involved in chemical bonding?

a)

Proton

b)

Neutron

c)

Electron

d)

Valence Electron

39.

Diagram show the reaction of

a)

Precipitation

b)

Displacement

c)

Neutralisation

d)

Combustion

40.
What kind of graph is this?
a)
endothermic
b)
exothermic
41.
Thermal energy always moves:
a)
From a high temperature object to a lower temperature object.
b)
From a lower temperature object to a higher temperature object.
c)
From an object with lower kinetic energy to an object with higher kinetic energy.
d)
From an object of higher mass to an object of lower mass.
42.

The energy diagram for the combustion of ethanoic acid, C2H4O2 is shown.

a)

The enthalpy of combustion for ethanoic acid is – 1360 kJ mol-1

b)

The enthalpy of formation of water is – 286 kJ mol-1

c)

The enthalpy of combustion for carbon is – 394 kJ mol

43.

Which metal would you expect to require the MOST energy to increase in temperature by 25°C?

(All samples are the same mass)

a)

Titanium

b)

Iron

c)

Copper

d)

Gold

44.

Which metal below would be the best conductor of energy? The Specific Heat values are in the table.

a)

Iron

b)

Copper

c)

Titanium

d)

Silver

45.
A reaction is performed in a beaker with a temperature probe recording the temperature changes of the reaction.  If the temperature began at 15.0 degrees Celsius and ended at 27.5 degrees Celsius.  If the reaction is our system, is the system endothermic or exothermic?
a)
Exothermic
b)
Endothermic
46.

How will the presence of a catalyst affect the Maxwell Boltzmann distribution curve below?

(a)  

47.

Which of the following are true of reaction rates?

I. The overall rate law is determined by the fastest step of a reaction

II. The presence of a catalyst will increase the number of molecules entering the transition state

III. An increase in temperature will increase the rate of a reaction

IV. Decreasing the concentration of reactants will increase the rate at which products yield

a)

II+III+IV

b)

I+IV

c)

II + III

d)

I+II+III

48.

Which of the following plots will show a linear relationship for a second order reaction?

a)

[A] vs time

b)

1/[A] vs time

c)

ln[A] vs time

d)

[A]2 vs time

49.
Find the order for F2 and CIO2 using data shown below.
a)
(F2 - 2nd order) (CIO2 - 1st order)
b)
(F2 - 1st order) (CIO2 - 1st order)
c)
(F2 - 1st order) (CIO2 - 2nd order)
d)
(F2 - 2nd order) (CIO2 - 2nd order)
50.
Grinding a seltzer tablet into powder increases the rate of reaction due to...
a)
increased concentration of reactants
b)
increased surface area
c)
increased speed of particles.
d)
better orientation of reactants
51.

The following data were measured for the reaction

BF3(g) + NH3(g) ⟶ F3BNH3(g)

What is the rate when [BF3] = 0.100 M and [NH3] = 0.500 M ?

a)

.01704 M/s

b)

.0852 M/s

c)

.1704 M/s

d)

.852 M/s

52.
a)

a

b)

b

c)

c

d)

d

53.

Catalysts are agents that increase reaction rates without themselves being used up.

a)

True

b)

False

54.

List four factors that affects the rate of a reaction

a)

temperature

b)

concentration

c)

surface area

d)

volume

e)

catalysts

55.
a)

A

b)

B

c)

C

d)

D

56.
What are [A] and [B]?
a)
concentration of reactants
b)
concentration of products
c)
energy of reactants
d)
energy of products
57.
a)

A

b)

B

c)

C

d)

D

58.
At what time the reaction reached equilibrium?
a)
t1
b)
t2
c)
t3
d)
t4
59.
This symbol indicates that a reaction is ____________
a)
reversible
b)
irreversible
60.
Which is the reactant - and why?
a)
A, as concentration decreases
b)
B, as concentration decreases
c)
A, as concentration increases
d)
B, as concentration increases
61.

What are [C] and [D]?

a)

concentration of reactants

b)

concentration of products

c)

energy of reactants

d)

energy of products

62.

Is the following substance an acid or a base? H2(SO4)

a)

Acid

b)

Base

63.

Is the following substance an acid or a base? Ca(OH)2

a)

Acid

b)

Base

64.

Neutral solutions have a pH of _______________.

a)

below 7

b)

above 7

c)

exactly 7

65.
Barium hydroxide
a)
BaOH
b)
Ba2OH
c)
Ba(OH)2
66.

What specific substance has the ability to act as an acid or base

a)

Hydronium Ion

b)

Hydroxide Ion

c)

Water

d)

Ammonia

67.

What is the Acid in the reaction below:

C2O42– + HC2H3O2 → HC2O4– + C2H3O2–

a)

C2O42–

b)

HC2H3O2

c)

HC2O4–

d)

C2H3O2–

68.

Which represents a hydroxide ion?

a)

H+

b)

OH-

c)

Na+

d)

Cl-

69.

What is the Conjugate Acid in the reaction below:

C2O42– + HC2H3O2 → HC2O4– + C2H3O2–

a)

C2O42–

b)

HC2H3O2

c)

HC2O4–

d)

C2H3O2–

70.

Which of these pH values represent an acid?

a)

4

b)

8

c)

10

d)

12

71.

How do you name Group I and Group II ions?

a)

The Stock System

b)

element name + "ide"

c)

element name + "ion"

d)

None of the above

72.

phosphate

a)

P-3

b)

PO3-3

c)

PO4-3

73.

Ionic compounds are bonds between a metal and a nonmetal elements? Which pair will form an ionic compound?

a)

potassium and calcium

b)

flourine and oxygen

c)

strontium and sulfur

d)

nitrogen and bromine

74.

What is the correct name of the anion in the ionic compound: NH3N?

a)

ammonium

b)

hydride

c)

nitride

d)

nitrate

75.

What is the name of this ion: O2-

a)

Oxygen ion

b)

Oxygen (II) ion

c)

Oxide ion

d)

Oxygen

76.

How many ions can vanadium form?

a)

2

b)

3

c)

4

d)

5

77.

What does an ionic compound consist of?

CHOOSE ALL THAT APPLY

a)

Anions

b)

positive & negative ions

c)

Cations

d)

None of these

78.

Ions made of more than one element are called

a)

dual elements

b)

polyatomic ions

c)

monoatomic ions

d)

dual ions

79.

How is a molecular compound held together?

a)

covalent bonds

b)

ionic bonds

c)

duct tape

d)

with the will of an atom

80.

When is the crossover method used to get the formula of a compound?

a)

When two polyatomic ions have different charges

b)

When two monoatomic ions have different charges

c)

When two polyatomic ions have the same charges

d)

When two monoatomic ions have the same charges

81.

Name P2O5

a)

Phosphorus pentaoxide

b)

Diphosphorus oxide

c)

Diphosphorus pentoxide

d)

Phosphorus oxide

82.

How do you name a nonmetal when it forms an ion?

a)

element name + "ion"

b)

element name + "ide"

c)

By identifying the elements

d)

You can't name nonmetal ions

83.
a)

IO-, because it was used as a reactant in an earlier step and reproduced in a subsequent step

b)

I-, because it was used as a reactant in an earlier step and reproduced in a subsequent step

c)

IO-, because it was produced in an earlier step and used up in a subsequent step

d)

I-, because it was produced in an earlier step and used up in a subsequent step

84.
a)

0; 2; 2

b)

1; 2; 3

c)

1; 2; 2

d)

0; 1; 1

85.
What is the volume of the rock after water displacement?
a)

1.8mL

b)

.6mL

c)

1.1mL

d)

1.2mL

86.

How many Hydrogen are in 4H2O + 2CH4?

(a)  

87.
___________________ are the elements or compounds that are formed in a chemical
reaction.
a)
Polymers
b)
Bonds
c)
Reactants
d)
Products
88.

What physical state symbol should be included for oxygen?

a)

(s) - solid

b)

(l) - liquid

c)

(g) - gas

d)

(aq) - aqueous

89.
Is this equation balanced?
a)
yes
b)
no
c)
Not enough information
90.
What are the larger numbers that you CAN CHANGE in a chemical equation? 
a)
Coefficient 
b)
Products
c)
Reactants
d)
Subscripts
91.

Which side of an equation is referred to as the “reactant”?

a)

The right side

b)

The arrow in the center

c)

The left side

d)

None of the provided answers

92.
What are the smaller numbers that you CANNOT change in a chemical equation? 
a)
Coefficient
b)
Products
c)
Reactants
d)
Subscript
93.

Which of the following is the only thing you should change when balancing an equation?

a)

Subscript

b)

Atom

c)

Coefficient

d)

Atom

94.

What is the missing coefficient needed to balance the equation below?

_ H₃PO₄ →  H₄P₂O₇ +  H₂O

a)

Already balanced

b)

3

c)

2

d)

6

95.
Is NaCl (table salt) a Organic or Inorganic Compound?
a)
Inorganic
b)
Organic
96.
Name this alkane.
a)
propane
b)
octane
c)
hexane
d)
butane
97.
Is this hydrocarbon saturated or unsaturated? 
a)
saturated
b)
unsaturated
98.

What is the name of the alkane shown here?

a)

Methane

b)

Ethane

c)

Propane

d)

Butane

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