Oxidation And Reduction Reactions Quiz! Trivia
Below is an Oxidation and reduction reactions quiz trivia. Oxidation is the process where electrons are lost while reduction is the transfer of electrons between substances. Oxygen is either lost or gained in the reactions. In this quiz you will test out what you know about different compounds and substances and what happens when they undergo this process. Do give it a shot and see how well you do!
- 1.
The terms Oxidation and Reduction both have direct polar opposite definitions. what is each term defined as?
- A.
Oxidation- the loss of electrons by atom or ion/ the gain of oxygen, Reduction- the loss of oxygen/ the gain of said electrons.
- B.
Oxidation- the gain of electrons by an atom or ion/ loss of oxygen, Reduction- the gain of oxygen/ the loss of electrons by atom or ion.
- C.
Oxidation- something having to do with oxide, i don't care -__- Reduction- something's being reduced, but i don't know what.
Correct Answer
A. Oxidation- the loss of electrons by atom or ion/ the gain of oxygen, Reduction- the loss of oxygen/ the gain of said electrons.Explanation
polar opposite would mean that one has the exact opposite meaning of the other.Rate this question:
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- 2.
Can oxidation and reduction occur without one another?
- A.
They are interdependent
- B.
They are not interdependent.
Correct Answer
A. They are interdependentExplanation
what does interdependent mean?Rate this question:
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- 3.
What, in simplified terms, does Redox mean?
- A.
Its a combination of Reduction and Oxidation, when one occurs, the other does not.
- B.
It is not a combination of reduction and oxidation , when one occurs, the other must occur as well.
- C.
Its a combo of both REDuction and OXidation. one reaction cannot occur without the other.
Correct Answer
C. Its a combo of both REDuction and OXidation. one reaction cannot occur without the other.Explanation
Redox refers to a combination of both reduction and oxidation. In a redox reaction, one substance is reduced (gains electrons) while another is oxidized (loses electrons). These two processes always occur together and are interconnected. Therefore, one reaction cannot occur without the other in a redox reaction.Rate this question:
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- 4.
What does LEO say GER stand for?
- A.
LEO- Loss of Electrons is Oxygen, GER- Gain of Electrons is Red
- B.
LEO- Loss of Elections is Oxidation, GER- Gain of Electrons is Reduction
- C.
LEO- Loss of Electrons is Oxidation, GER- Gain of Electrons is Reduction
Correct Answer
C. LEO- Loss of Electrons is Oxidation, GER- Gain of Electrons is ReductionExplanation
The correct answer explains the acronym LEO as "Loss of Electrons is Oxidation" and GER as "Gain of Electrons is Reduction". This is a commonly used mnemonic in chemistry to remember the processes of oxidation and reduction. In an oxidation reaction, a substance loses electrons (LEO), while in a reduction reaction, a substance gains electrons (GER).Rate this question:
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- 5.
Credit given only to those who show all work!! what are the oxidation numbers of the atoms in HNO3?
- A.
H: +1, N: +5 , O: -2
- B.
H: 1, N: 5, O: 2
- C.
H: +1, N: -5, O: +2
Correct Answer
A. H: +1, N: +5 , O: -2Explanation
The oxidation number of an atom is the charge it would have in a compound if electrons were completely transferred. In HNO3, hydrogen (H) typically has an oxidation number of +1, nitrogen (N) has an oxidation number of +5, and oxygen (O) has an oxidation number of -2. This is because hydrogen usually has an oxidation number of +1 in compounds, nitrogen typically has an oxidation number of +5 in compounds, and oxygen typically has an oxidation number of -2 in compounds. Therefore, the correct answer is H: +1, N: +5, O: -2.Rate this question:
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- 6.
The sum of the oxidation numbers in all compounds is equal to 1.
- A.
True
- B.
False
Correct Answer
B. FalseExplanation
The sum of the oxidation numbers in all compounds is not necessarily equal to 1. The oxidation number of an element is a hypothetical charge assigned to that element in a compound, and it is used to track the electron transfer in chemical reactions. The sum of the oxidation numbers in a compound must always equal the overall charge of the compound, which can be positive, negative, or even zero. Therefore, the statement that the sum of the oxidation numbers in all compounds is equal to 1 is false.Rate this question:
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- 7.
The sum of the oxidation numbers in all compounds is equal to 0.
- A.
True
- B.
False
Correct Answer
A. TrueExplanation
The statement is true because in a compound, the sum of the oxidation numbers of all the elements must be equal to zero. This is because oxidation numbers are assigned to each element in a compound to represent the distribution of electrons. The sum of these oxidation numbers represents the overall charge of the compound, and since compounds are electrically neutral, the sum must be zero.Rate this question:
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- 8.
The sum of the oxidation numbers in the polyatomic ions must be equal to the charge on the ion.
- A.
True
- B.
False
Correct Answer
A. TrueExplanation
Think of the rules for assigning oxidation numbers....Rate this question:
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- 9.
In which substance does phosphorus have a +3 oxidation state
- A.
P4O10
- B.
PCl5
- C.
Ca3(PO4)2
- D.
KH2PO3
Correct Answer
D. KH2PO3Explanation
Phosphorus typically exhibits a +5 oxidation state in most compounds, but in KH2PO3, it has a +3 oxidation state. This is because hydrogen (H) has a +1 oxidation state, and oxygen (O) has a -2 oxidation state. Since there are two hydrogen atoms bonded to phosphorus, the overall charge contributed by hydrogen is +2. Therefore, in order to balance the charges, phosphorus must have a +3 oxidation state in KH2PO3.Rate this question:
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- 10.
In order for an equation to be a REDOX equation, you must recognize it as a..?
Correct Answer
single replacement reactionExplanation
A single replacement reaction is a type of chemical reaction where an element replaces another element in a compound. In a redox equation, there is a transfer of electrons between the reactants and products. In a single replacement reaction, one element is being oxidized (loses electrons) while another element is being reduced (gains electrons). Therefore, recognizing an equation as a single replacement reaction is crucial in determining if it is a redox equation.Rate this question:
- 11.
Which equation represents an oxidation-reduction reaction?
- A.
HCl + KOH yields KCl + H2O
- B.
4HCl + MnO2 yields MnCl2 + 2H2O +Cl2
- C.
2HCl +CaCO3 yields CaCl2 + H2O +CO2
- D.
2Hcl + FeS yields FeCl2 +H2S
Correct Answer
B. 4HCl + MnO2 yields MnCl2 + 2H2O +Cl2Explanation
In this equation, manganese (Mn) undergoes a change in oxidation state from +4 in MnO2 to +2 in MnCl2, indicating oxidation and reduction processes are occurring simultaneously. The hydrogen chloride (HCl) is oxidized to chlorine gas (Cl2), while manganese dioxide (MnO2) is reduced to manganese chloride (MnCl2). This demonstrates the transfer of electrons, characteristic of oxidation-reduction reactions.Rate this question:
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- 12.
When a Substance is oxidized, it
- A.
Loses protons
- B.
Gains protons
- C.
Acts like a reducing agent
- D.
Acts as an oxidizing agent
- E.
Its gets oxyclean. xD
Correct Answer
C. Acts like a reducing agentExplanation
When a substance is oxidized, it acts like a reducing agent. This means that it donates electrons to another substance, causing a reduction in its own oxidation state. By donating electrons, the substance helps to facilitate the reduction of another substance, which is why it is referred to as a reducing agent.Rate this question:
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- 13.
What do you call the substance being reduced?
Correct Answer
the oxidizing agentExplanation
The substance being reduced is called the oxidizing agent. In a redox reaction, the oxidizing agent is the species that gains electrons and gets reduced. It causes the oxidation of another species by accepting electrons from it. Therefore, the oxidizing agent is the substance that is responsible for the reduction process in the reaction.Rate this question:
- 14.
What do you call the substance being oxidized?
Correct Answer
the reducing agent.Explanation
The substance being oxidized is referred to as the reducing agent. In a redox reaction, the reducing agent donates electrons to another substance, causing itself to be oxidized. The reducing agent is responsible for the reduction half-reaction, where it loses electrons. This transfer of electrons allows the other substance to be reduced. Therefore, the correct answer is "the reducing agent."Rate this question:
- 15.
Consider the Following Equation. 2Fe3+ + Sn2+ yields 2Fe2++Sn4+ who is the oxidizing agent?
- A.
Fe3+
- B.
Sn2+
- C.
Fe2+
- D.
Sn4+
Correct Answer
A. Fe3+Explanation
In the given equation, Fe3+ is being reduced to Fe2+, which means it is gaining electrons and undergoing a reduction reaction. The species that causes another species to undergo reduction is known as the oxidizing agent. Therefore, Fe3+ is the oxidizing agent in this equation.Rate this question:
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- 16.
If the number changes from high oxidation to low, then it has been oxidized.
- A.
True
- B.
False
Correct Answer
A. TrueExplanation
If a number changes from high oxidation to low oxidation, it means that it has lost electrons and has been oxidized. Oxidation is the process in which a substance loses electrons, and this statement correctly states that if a number changes from high oxidation to low, it has indeed been oxidized. Therefore, the answer "True" is correct.Rate this question:
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- 17.
In the Equation MnO2 + 4HCl yields MnCl2 + Cl2 + 2H2O what is the Reducing Agent and is the Oxidizing Agent?
Correct Answer
Mn4+ : oxidizing Agent Cl- : reducing agentExplanation
In the given equation, MnO2 is being reduced from Mn4+ to Mn2+, which means it is gaining electrons and undergoing a reduction reaction. Therefore, MnO2 is the oxidizing agent. On the other hand, Cl- is being oxidized from -1 to 0, which means it is losing electrons and undergoing an oxidation reaction. Therefore, Cl- is the reducing agent.Rate this question:
- 18.
Oxidation-Reduction Reactions occur because of the competition between particles for
- A.
Neutrons
- B.
Elections
- C.
Positrons
- D.
Electrons
Correct Answer
D. ElectronsExplanation
Oxidation-Reduction Reactions occur because of the competition between particles for electrons. In these reactions, one species loses electrons (oxidation) while another species gains electrons (reduction). This transfer of electrons allows for the formation of new chemical bonds and the conversion of one substance into another. The competition for electrons is what drives these reactions, as particles strive to achieve a more stable electron configuration by either gaining or losing electrons.Rate this question:
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- 19.
What must ALWAYS occur in REDOX reactions?
Correct Answer
both the gain and loss of electrons.Explanation
In REDOX reactions, which stands for reduction-oxidation reactions, both the gain and loss of electrons must always occur. Reduction refers to the gain of electrons, while oxidation refers to the loss of electrons. These reactions involve the transfer of electrons from one species to another, resulting in the reduction of one species and the oxidation of another. Therefore, it is essential for both processes to happen simultaneously in order for a REDOX reaction to take place.Rate this question:
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Mar 13, 2024Quiz Edited by
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Apr 25, 2011Quiz Created by
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