Chemical Reactions Flashcards

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1
Q

Distinguishing Between Physical and Chemical Changes:

A

Physical changes involve a change in appearance, state, or form of matter without altering its chemical composition. Chemical changes involve the formation of new substances with different chemical properties.

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2
Q

Definition of a Chemical Reaction:

A

A chemical reaction is a process in which one or more substances (reactants) are converted into one or more different substances (products), with the formation of new chemical bonds and the rearrangement of atoms.

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3
Q

Word Equation of Reactions of Metals with Oxygen, Acid, and Water:

A

Metal + Oxygen → Metal Oxide
Metal + Acid → Salt + Hydrogen gas
Metal + Water → Metal Hydroxide + Hydrogen gas

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4
Q

Signs/Indicators of a Chemical Reaction:

A

Formation of gas, change in color, formation of precipitate (solid), release or absorption of heat or light, and production of odor.

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5
Q

Salts Produced with Acid and Metal Reactions:

A

Salts produced depend on the metal and acid involved in the reaction, such as zinc chloride, copper sulfate, or magnesium nitrate.

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6
Q

Reactivity Series of Metals:

A

A list of metals arranged in order of their reactivity, with the most reactive metals at the top and the least reactive at the bottom.

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7
Q

Displacement Reaction:

A

A displacement reaction occurs when a more reactive element displaces a less reactive element from its compound.

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8
Q

Single Displacement Reactions Between Metal and Metal Oxides:

A

Metal + Metal Oxide → Metal Oxide + Metal

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9
Q

Predicting Reactions Using the Reactivity Series:

A

A metal higher in the reactivity series can displace a metal lower in the series from its compound.

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10
Q

Factors Increasing the Rate of Reaction:

A

Temperature, concentration of reactants, surface area, presence of catalysts, and pressure (for gaseous reactions).

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11
Q

Activation Energy:

A

The minimum amount of energy required for a chemical reaction to occur.

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12
Q

Endothermic and Exothermic Reactions:

A

Endothermic reactions absorb heat from the surroundings, while exothermic reactions release heat to the surroundings.

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13
Q

Examples of Endothermic and Exothermic Reactions:

A

Endothermic: Melting ice, evaporation of water, and baking soda reacting with vinegar.
Exothermic: Burning wood, rusting of iron, and neutralization reactions.

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14
Q

Interpreting Reaction Profiles, Calculating ΔH, and Determining Endo/Exothermic Reactions:

A

Endothermic reactions have a positive change in enthalpy (ΔH), while exothermic reactions have a negative ΔH. Reaction profiles show the energy changes during a reaction.

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15
Q

Bond Breaking and Bond Forming:

A

Breaking bonds requires energy and is endothermic, while forming bonds releases energy and is exothermic.

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16
Q

Effects of Catalysts on Rates of Reaction - Using Elephant’s Toothpaste:

A

Catalysts speed up chemical reactions by providing an alternative reaction pathway with a lower activation energy. In the breakdown of hydrogen peroxide, a catalyst like potassium iodide (KI) or yeast is used to catalyze the decomposition of hydrogen peroxide into water and oxygen, producing foam (elephant’s toothpaste).