Deck 35: Praxis II Elementary Education Content Knowledge

Question 1

Which of the following is NOT a city in North America?

A)Mexico City
B)Buenos Aires
C)Anchorage
D)Toronto

Answer 1

Buenos Aires

Question 2

Which of the following events is believed by many to be a cause of the Great Depression?

A)Black Tuesday
B)World War I
C)The Roaring Twenties
D)Prohibition

Answer 2

Black Tuesday

Question 3

According to the US Standard system, which of the following would be used to measure the volume of water in a bath tub?

A)Gallons
B)Liters
C)Cups
D)None of the above

Answer 3

Gallons

Question 4

A second-grade teacher asks a student to read several written words and then to read a paragraph containing each word. While assessing the student's reading skills, she notices he does better reading the paragraph than he does reading the words individually. Which of the following best describes the student's reading abilities? Choose all that apply.

A)The student has poor individual word decoding skills
B)The student does well recognizing context cues
C)The student does not recognize semantic cues
D)None of the above

Question 5

Which of the following instructional materials can teachers use as visual aids to encourage language acquisition for second-language learners?

A)Picture dictionaries
B)Board games
C)Computer games
D)All of the above

Question 6

Given that the atomic mass of chlorine is 35.5 grams/mol, approximately what is the weight of an individual chlorine atom?

A)5)8 x 10-23 grams
B)1)1 x 10-25 grams
C)10.5 x 10-8 grams
D)0)355 grams
E)2)6 x 10-23 grams

Question 7

If one mole of potassium reacts with one mole of chlorine to form potassium chloride, (KCl), how many moles of product will there be?

A)5
B)4
C)3
D)2
E)1

Question 8

Sachin has retrieved a lump of iron oxide (Fe2O?), and finds that its mass is 160.7 grams. How many moles of iron are in the lump?

A)1
B)2
C)2)5
D)3
E)3)5

Question 9

Which of the following best defines the concept of a limiting reagent?

A)A reagent that limits the rate at which a reaction can occur.
B)A reagent that has the highest activation energy.
C)A reagent that is present in the lowest concentration and limits the amount of product formation.
D)A reagent that limits the solubility of the product in water.
E)All of the above can be defined as a limiting reagent.

Question 10

By mass, calcium hydroxide (Ca(OH)2) is 54% calcium. What is the mole percent of calcium in calcium hydroxide?

A)25%
B)33%
C)50%
D)75%
E)54%

Question 11

Alex received a cool gift from his grandmother, a 1-ounce bar of gold! How many moles of gold did his grandma just give him?

A)0)14
B)0)53
C)1)1
D)1
E)0)005

Question 12

Given the following reaction, what is the correct balanced chemical reaction equation? Ca(OH)₂ + HCl ? CaCl₂ + H?O

A)Ca(OH)₂ + 2HCl ? CaCl₂ + 2H?O
B)2Ca(OH)₂ + HCl ? 2CaCl₂ + H?O
C)2Ca(OH)2 + HCl ? CaCl2 + 2H?O
D)Ca(OH)2 + 3HCl ? 2CaCl2 + H?O
E)The original equation is correct.

Question 13

Charlie is using a catalyst to turn rust (iron oxide) back into iron and unstable carbon trioxide. The unbalanced equation is seen below. If he has 1 mole of rust, how many grams of carbon does he need for the reaction to proceed completely? Fe2O? + C ? Fe + CO?

A)1 gram
B)5 grams
C)10 grams
D)12 grams
E)14 grams

Question 14

In fireworks displays, magnesium reacts with oxygen to produce bright white light. Which of the following could be the product of this reaction?

A)MgO
B)MgO?
C)Mg2O5
D)Mg2O?
E)MgOMgO

Question 15

Which of the following elements would be considered 'semi-metallic'?

A)Chlorine
B)Iron
C)Oxygen
D)Gold
E)Germanium

Question 16

A newly discovered compound has been found to be 16.2% magnesium, 18.9% nitrogen, and 64% oxygen by weight. What is a possible formula for this compound?

A)Mg(NO?)₂
B)MgO?
C)MgNO
D)Mg2NO?
E)Mg2(NO)₃

Question 17

In the following reaction, 2 moles of silver nitrate are reacted with an excess of calcium chloride. If the reaction has a 90% yield, how many grams of silver chloride are formed? 2AgNO? + CaCl2 ? Ca(NO?)2 +2AgCl

A)284
B)256
C)511
D)568

Question 18

The elements in the 18th group in the periodic table, such as helium and neon, are not very reactive because:

A)Their atomic mass is too great to allow them to easily interact with other atoms
B)They have no electrons
C)Their valence shell is full, so there are no free electrons for reaction
D)They have a full d-shell of electrons
E)They are not found on Earth, so don't react well with other elements

Question 19

On the periodic table, which group of elements will have the highest first ionization energy? Ionization energy is the energy required to remove an electron from the atom.

A)Group 3
B)Group 18
C)Group 2
D)Group 1
E)Group 10

Question 20

Chris has discovered a curious element that is metallic in nature, rusts easily when exposed to oxygen, and seems heavier than iron. Which of the following elements could this not be?

A)Palladium
B)Nickel
C)Zinc
D)Sodium
E)Silver

Question 21

As we approach the upper left hand corner of the periodic table, which of the following is true?

A)The elements become less and less reactive.
B)The elements become more and more reactive.
C)The elements become larger and larger in atomic radius.
D)The elements become smaller and smaller in atomic radius.
E)The elements become more and more metallic.

Question 22

A student wishes to produce magnesium bromide and water using a reaction based around magnesium hydroxide. Which other reactant is he or she missing?

A)Magnesium bromide
B)Magnesium iodide
C)Hydrogen bromide
D)Bromochloroform
E)Sodium bromide

Question 23

If a car burns one gallon of gasoline (C8H18) in a standard combustion reaction, how much water is produced? Gasoline weighs 2.75 kg per gallon.

A)3)91 kg
B)2)75 kg
C)1)82 kg
D)4)21 kg
E)5)52 kg

Question 24

The reaction seen below can be categorized as which kind of reaction mechanism? NH?NO? N2O + H?O

A)Replacement
B)Production
C)Double replacement
D)Decomposition
E)Precipitation

Question 25

The rate of a reaction can usually be increased by all of the following except:

A)Increasing the temperature.
B)Adding a chemical catalyst.
C)Increasing the surface area available for a solid reactant.
D)Increasing the amount of water present in an aqueous reaction.
E)Increasing the concentration of the reactants.

Question 26

Which of the following is an example of a heterogeneous reaction?

A)Iron rusting.
B)Methane and oxygen combusting.
C)Dye being poured into water.
D)Water evaporating.
E)None of the above is a heterogeneous reaction.

Question 27

What will an exothermic reaction do?

A)Turn products into reactants.
B)Turn intermediates into products.
C)Create energy or heat.
D)Consume energy or heat.
E)Reduce entropy.

Question 28

Lillian has discovered a new 2-step reaction that can produce aluminum hydride. Reaction 1 operates very slowly however; about 5 times slower than Reaction 2. Reaction 1 likely has a:

A)Volatile intermediate.
B)Higher activation energy.
C)Heterogeneous interaction problem.
D)Reduced surface area.
E)Van der Waals reduction effect.

Question 29

The reaction rate constant can be determined by:

A)Boltzmann's equation.
B)Arrhenius' equation.
C)Darwin-Bolling's equation.
D)Van der Waal's ignoble equation.
E)Brussel's equation.

Question 30

10 grams of potassium is placed into a solution of hydrochloric acid. After 20 seconds, 4.4 grams of potassium remained. What was the average rate of reaction?

A)0)12 grams/sec
B)0)19 grams/sec
C)0)28 grams/sec
D)0)34 grams/sec
E)0)50 grams/sec

Question 31

If the rate law of a reactant is zero, then this means that:

A)There is no appreciable concentration of the reactant.
B)Increasing the concentration of the reactant will not increase the rate.
C)Decreasing the concentration of the reactant will increase the rate.
D)The reaction of this reactant consumes product.
E)This reaction produces no products.

Question 32

In the following reaction, which chemical species is a reaction intermediate? Step 1: H?O? (aq) + Br- (aq) ? H?O (aq) + OBr- (aq)
Step 2: H?O? (aq) + OBr- (aq) ? H?O (aq) + Br- (aq) + O? (g)

A)H?O?
B)O?
C)H?O
D)OBr-
E)H?

Question 33

Edward conducts the following set of experiments to determine the reaction order of hydrogen in the reaction. What is the reaction order of hydrogen in this reaction? Br Concentration, H? Concentration , Initial rate
0)10.1 0.10.1 2.38 x 10-2
0)20.2 0.10.1 2.38 x 10-2
0)10.1 0.20.2 4.41 x 10-2

A)0
B)1
C)2
D)3
E)4

Question 34

The reaction rate constant is usually described using which of the following units in a first order reaction?

A)s^-1
B)mol•L^-1•s^-2
C)mol/L
D)L/mol²
E)mol^-1

Question 35

When a chemical reaction is at equilibrium, the reaction quotient is what percentage of the equilibrium constant?

A)0%
B)25%
C)50%
D)75%
E)100%

Question 36

Jenny has carried out a reaction in her lab to equilibrium. She tells her friend, Joe, that there are no longer any reactions occurring in the solution. Joe tells her she is wrong, because:

A)A reaction at equilibrium has no reactants left.
B)A reaction at equilibrium has reactions occurring, just at equal forward and backward rates.
C)The reaction is still occurring, just moving forward a little slower than before.
D)The reaction is not occurring anymore, but still can occur if you shake the solution.
E)Joe is wrong as well, and none of the above answers is correct.

Question 37

If the following reaction is in equilibrium, what would a graph representing the concentration of H? look like? 2NH?(g) ? N2(g) + 3H?(g)

A)A line with a negative slope.
B)A line with a positive slope.
C)An exponential curve going toward infinity.
D)A flat horizontal line.
E)An exponential curve going toward zero.

Question 38

If a reaction has proceeded to completion, then what does this mean?

A)All reactants have reacted.
B)Equilibrium has been reached.
C)The reaction is now proceeding very slowly.
D)The reaction has produced some intermediates.
E)The phase change of the reactants is beginning.

Question 39

Kelley measured the concentrations of a reaction in progress, and stated them below. What is the current equilibrium constant for this reaction? 2S(s) + 3O?(g) 2SO?(g)
S: 1.5 mols
O?: 4 mols
SO?: 2.9 mols

A)2)1
B)1)4
C)5)5
D)3)9
E)4)1

Question 40

A catalyst will usually make a reaction proceed much faster. How do catalysts work? I. Puts reactants close together
II) Reduces activation energy
III) Increases the temperature

A)I only.
B)I and II.
C)I and III.
D)I, II, and III.
E)II and III.

Question 41

If the reaction quotient is greater than the reaction equilibrium, that means:

A)Intermediates are becoming products
B)Reactants are becoming products
C)Products are becoming reactants
D)The products and reactants are equal in concentration
E)There is more product than reactant in the system

Question 42

Which of the following is not a state function?

A)Mass
B)Moles
C)Energy
D)Pressure
E)Volume

Question 43

Which of these statements regarding chemical thermodynamics is not correct?

A)A thermodynamically favorable process will always occur quickly.
B)A negative ?G value means the process is thermodynamically favorable.
C)Exothermic reactions have a negative ?G.
D)The enthalpy is equal to U + PV.
E)Processes with positive ?G require energy to proceed.

Question 44

Sean wants to determine the amount of energy released by the combustion of butane. Which instrument should he use?

A)Pipette
B)Scale
C)Calorimeter
D)Gel chromatography
E)Thermometer

Question 45

When ionic compounds, such as NaCl or KOH, enter water, they will:

A)Lose electrons.
B)Precipitate.
C)Oxidize.
D)Dissociate.
E)Reduce.

Question 46

Which of the following pairs of solutions will be miscible, in that they will mix easily with one another?

A)Water and hexane.
B)Benzene and methanol.
C)Ethanol and water.
D)Acetic acid and benzene.
E)None of the above are miscible with each other.

Question 47

Which of the following is not a colligative property?

A)Elevation of boiling point.
B)Osmotic pressure.
C)Generated heat of mixing.
D)Relative lowering of vapor pressure.
E)Depression of freezing point.

Question 48

Which of the following compounds would, if dissolved in water, create the greatest difference in boiling point?

A)HCl
B)NaCl
C)KOH
D)MgCl₂
E)HCN

Question 49

Jamie has a flask containing 1 liter of water at 50°C. If she adds 1 mole of C6H14O? to the water, what will happen to the vapor pressure of the water?

A)It will increase slightly.
B)It will decrease slightly.
C)It will increase significantly.
D)It will decrease significantly.
E)It will not change at all.

Question 50

Given that the boiling point constant(Kb) of water is 0.512, what will be the boiling point of 2 liters of water that has 200 grams of CaCl2 added?

A)100 °C
B)100.7 °C
C)101.4 °C
D)101.9 °C
E)102.5 °C

Question 51

Alexander is hiking up Mt. Everest, and recently reached the base camp at 12,000 feet. While there, he decides to make some tea, and puts a thermometer in the boiling water. To his surprise, the thermometer tells him the water is boiling at 96 °C. Why is this happening?

A)Water boils more quickly when you watch it.
B)The thermometer is broken.
C)The pressure is lower at higher elevations, and results in a lower boiling temperature.
D)The number of solutes in the air is higher at higher elevations, resulting in boiling point depression.
E)Alex is suffering from oxygen deprivation, and is reading the thermometer incorrectly.

Question 52

Ming needs to add some salt solution to his algae culture to emulate seawater conditions. The only salt solution he has is 20% (w/v) of salt. He wants to make 5 liters of 1 molar salt solution. How much 20% salt solution should he add?

A)0)78 liters
B)1)12 liters
C)1)46 liters
D)2)08 liters
E)2)45 liters

Question 53

What is the primary difference between a molecular solution and an ionic solution?

A)Molecular solutions dissociate and ionic solutions do not.
B)Ionic solutions dissociate and molecular solutions do not.
C)Molecular solutions are able to conduct electricity.
D)Ionic solutions have a higher pH than molecular solutions.
E)Molecular solutions and ionic solutions are the same thing.

Question 54

Which of the following compounds is completely insoluble in water?

A)Magnesium chloride
B)Silver chloride
C)Potassium hydroxide
D)Phosphate
E)Ammonium hydroxide

Question 55

Which of the following nitrate compounds is insoluble in water?

A)Sodium nitrate
B)Calcium nitrate
C)Iron nitrate
D)Lead nitrate
E)All of these compounds are soluble

Question 56

Amanda is trying to determine the solubility of nickel chloride (NiCl2) in water. She finds that her 1 liter saturated solution has 0.55 M of chloride ions. What is the solubility of nickel chloride?

A)23.8 g/L
B)31.7 g/L
C)35.5 g/L
D)41.3 g/L
E)52.1 g/L

Question 57

If an oxidation reaction has occurred:

A)A precipitation reaction must also have occurred.
B)A reduction reaction must also have occurred.
C)The oxidized species must have gained a charge.
D)The oxidized species must have become more acidic.
E)The reaction is not reversible.

Question 58

For the following reaction, what is the oxidation half reaction? O? + H?O + SO? ? SO?2- + O? + 2H+

A)O? + H?O + SO? ? 2e-
B)H?O + 2e- ? SO?2-
C)O? + SO? + 2e- + O ? SO?2- + O?
D)H?O ? 2H+ + 2e- + O
E)O? + H?O + SO? ? SO?2- + O? + 2H+

Question 59

In the following reaction, which species is becoming oxidized? CO?(g) + H?(g) CO(g) + H?O(g)

A)CO?
B)H?
C)CO
D)H?O
E)This is not a redox reaction.

Question 60

A battery is a standard example of an electrochemical cell. Which part of a battery is being reduced when a battery is used?

A)Positive end.
B)Negative end.
C)Middle.
D)Outer shell.
E)Both the positive and negative end.

Question 61

For an oxidation reduction reaction to occur spontaneously, which of the following needs to be true?

A)The electrochemical potential of reduction needs to be greater than that of oxidation.
B)The electrochemical potential of oxidation needs to be greater than that of reduction.
C)The del-G of the reaction needs to be positive.
D)The enthalpy of the reaction needs to be near zero.
E)The difference in electrochemical potentials of oxidation and reduction needs to be greater than zero.

Question 62

Which of the following species has a covalent bond type?

A)FeO
B)CH?
C)NaCl
D)HCl
E)H?PO?

Question 63

Which one of the following chemical compounds is incorrectly matched with its chemical name?

A)MgCl₂ - Magnesium chloride
B)PbI₂ - Lead di-iodide
C)CuSO? - Copper sulfite
D)NiO - Nickel oxide
E)KCl - Potassium chloride

Question 64

Andy is telling his friend that sulfur dioxide, SO?, has a bi-linear planar VSEPR geometry. Unfortunately, Andy is wrong. Why?

A)Sulfur dioxide has a tetrahedral geometry.
B)Sulfur dioxide has a linear geometry.
C)The bi-linear planar VSEPR geometry does not exist.
D)Sulfur dioxide is not a real compound.
E)Sulfur dioxide has an octahedral geometry.

Question 65

On the periodic table, which group of elements is it not possible to form an ionic bond with?

A)Group 4
B)Group 8
C)Group 11
D)Group 16
E)Group 18

Question 66

In the VSEPR geometry theory, how should electrons be represented?

A)As a bonding pair.
B)Electrons are not represented.
C)As two bonding pairs.
D)As a circulating shell.
E)As an electron cloud.

Question 67

What is the molecular shape of NH?, according to VSEPR theory?

A)Bent
B)Linear
C)Tetrahedral
D)Trigonal pyramidal
E)Octagonal

Question 68

Which of the following molecules possesses sp² hybridization?

A)CO?
B)FeO
C)BCl₃
D)CCl₄
E)NaCl

Question 69

Which of the following is the best definition for a covalent bond?

A)A weak bond that occurs due to electrostatic forces.
B)A bond that is formed by sharing of electrons between atoms.
C)A bond that is formed through a charge difference between two atoms.
D)A bond that has significant dipole moment, resulting in strong bonding forces.
E)A weak polar bond formed through interaction of electronegativity.

Question 70

Diprotic acids, such as H?SO?, are able to donate two protons to a solution. However, the dissociation constant for the second proton is usually much lower than for the first. This is because:

A)After the first proton reaches equilibrium, no more protons can dissociate.
B)Diprotic acids are able to give two protons.
C)The second proton is a weak acid, so it dissociates faster.
D)The 2nd proton's dissociation is affected by the presence of protons already in solution.
E)None of the above are correct.

Question 71

Which of the following acids is not a strong acid?

A)HCl
B)HBr
C)H?SO?
D)HNO?
E)HCOOH

Question 72

Tracy dissolves 2.5 grams of hydrochloric acid (HCl) into 1 liter of water. What is the pH of the solution?

A)1)1
B)1)6
C)1)9
D)2)5
E)3)1

Question 73

Oh no! Becky has spilled 4.8 liters of 5 M nitric acid (HNO?) on the ground! How many grams of sodium hydroxide should be used to neutralize this acid spill?

A)960 grams
B)999 grams
C)1,150 grams
D)2,300 grams
E)2,589 grams

Question 74

According to the Arrhenius definition of acids and bases, what product is always formed when an acid and base neutralize each other?

A)OH-
B)H?O
C)HCOOH
D)CO?
E)There is no defined product for the neutralization of an acid and base.

Question 75

Which of the following can be used to determine the pH of a solution? I. Methyl orange indicator
II) Litmus paper
III) pH probe

A)I only.
B)II only.
C)I and II.
D)I, II, and III.
E)III only.

Question 76

Water, as well as many other substances, can act as either an acid or a base. The correct name for these kinds of compounds is:

A)Duality compounds.
B)Reconciliant compounds.
C)Amphoteric compounds.
D)Diprotic compounds.
E)Dibasic compounds.

Question 77

Which acid-theory defines an acid as a compound which donates a proton to a corresponding base?

A)Arrhenius
B)Lewis
C)Brønsted-Lowry
D)Darwinian
E)Pascal

Question 78

Barney has discovered a new acid. Upon adding 15 grams of the new acid to water, he discovers that 4 grams of the acid dissociates. What should Barney classify this acid as?

A)Strong acid
B)Amphoteric acid
C)Buffer
D)Weak acid
E)Soluble acid

Question 79

Which of the following is not a functional group that exists?

A)Hydroxyl (-OH)
B)Carboxylic (-COOH)
C)Methyl (-CH?)
D)Amino (-NH?)
E)All of these functional groups exist.

Question 80

In the Earth's atmosphere, which element is the most common?

A)Oxygen
B)Carbon
C)Nitrogen
D)Helium
E)Hydrogen