Other than blood, the body structures of living organisms are made up of tissues. What is the role of tissues? Take up the quiz below on tissue level of organization to find out this and more.
Redox
Reflox
Remox
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Same
Increase
Reduction
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electropositive
electronegative
electronuetral
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Nuetrons
Protons
Electrons
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Protons
Nuetrons
Electrons
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True about oxidation and reduction.
True about electrons in redox reactions.
True about the rate of corrosion.
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Oxygen
Hydrogen
Carbon dioxide
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+2
+1
-1
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True about Aluminum oxide
True about hydrogen
True about oxidation
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O
R
N
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Charcoal (carbon)
Redox reaction
Covalent compounds
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Water
Oxygen
Iron
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Redox reactions involve a shift of nuetrons between reactants.
Redox reactions involve a shift of protons between reactants.
Redox reactions involve a shift of electrons between reactants.
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Billions
Millions
Trillions
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Oxidation originally meant the combination of an element with oxygen to produce oxides.
Oxidation originally meant the combination of an compound with oxygen to produce oxides
Oxidation originally meant the combination of an element with oxygen to produce water.
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Carbon combines with oxygen from the coal(III) oxide to form carbon dioxide.
Carbon combines with oxygen from the iron(III) oxide to form carbon dioxide.
Carbon combines with oxygen from the lead(III) oxide to form carbon dioxide.
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Oxygen
Water
Hydrogen
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Iron atoms slowly combine with oxygen in moist air to produce compounds such as iron(III) oxide.
Methane and oxygen are combining to produce carbon dioxide and water vapor and a great deal of heat.
When iron oxide is reduced to metallic iron, it gains oxygen.
Aluminum oxide forms a tightly packed protective layer that does not admit water. Because iron(III) oxide is not tightly packed, it allows water to penetrate and attack the metal below.
Sodium oxide forms a tightly packed protective layer that does not admit water. Because iron(III) oxide is not tightly packed, it allows water to penetrate and attack the metal below.
Patrolium oxide forms a tightly packed protective layer that does not admit water. Because iron(III) oxide is not tightly packed, it allows water to penetrate and attack the metal below.
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+1
0
-1
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0 0 +1-2 H3(g) + O2(g) ____> H3O
0 0 +1-2 H2(g) + O2(g) ____> H2O
0 0 +1-2 H3(g) + O2(g) ____> H2O
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The oxidation and reduction equations are balanced separately.
The oxidation and reduction equations are balanced together.
The oxidation and reduction equations are not balanced.
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O
R
N
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Because gold and platinum are very resistant to gaining their electrons through corrosion
Because gold and platinum are very resistant to losing their electrons through corrosion
Because gold and platinum are very resistant to keeping their electrons through corrosion
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The reaction is a redox reaction.
Decrease in the oxidation number of an element
Electrons contributed by the hydrogen atoms
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-1
-2
+2
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Iron atoms slowly combine with oxygen in moist air to produce compounds such as iron(III) oxide.
When iron oxide is reduced to metallic iron, it gains oxygen.
Iron atoms slowly combine with oxygen in moist air to produce compounds such as iron(III) oxide.
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Carbon combines with oxygen from the iron(III) oxide to form carbon zioxide.
Carbon combines with oxygen from the iron(III) oxide to form carbon monoxide.
Carbon combines with oxygen from the iron(III) oxide to form carbon dioxide.
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Early Iron Age people knew how to reduce iron ore to metallic iron by heating the ore with charcoal.
Early Iron Age people knew how to increase iron ore to metallic iron by heating the ore with charcoal.
Early Iron Age people knew how to keep the same iron ore to metallic iron by heating the ore with charcoal.
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Nothing is oxidized; nothing is reduced.
Oxygen is oxidized;hydrogen is reduced.
Hydrogen is oxidized; oxygen is reduced.
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Early Iron Age people knew how to keep the same amount of iron ore to metallic iron by heating the ore with charcoal.
Early Iron Age people knew how to increase iron ore to metallic iron by heating the ore with charcoal.
Early Iron Age people knew how to reduce iron ore to metallic iron by heating the ore with charcoal.
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Two-replacement reactions and acid–base reactions are not redox reactions.
Triple-replacement reactions and acid–base reactions are not redox reactions.
Double-replacement reactions and acid–base reactions are not redox reactions.
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Electron reactions in solution
Ionic reactions in solution
Proton reactions in solution
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0
1
2
Quiz Review Timeline (Updated): Mar 21, 2023 +
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