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Perryland Chemistry Theory - 2015 Standards > Theory - Unit 5 - Chemical Reactions > Flashcards

Theory - Unit 5 - Chemical Reactions Flashcards

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1
Q

Le Chatlier’s Principle

A
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2
Q

Symbols used in writing chemical equations

A
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4
Q

Law of Conservation of Mass

A

Mass is neither created or destroyed during a chemical reaction - it is conserved.

Mass Reactants = Mass Products

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6
Q

Coefficients

A

The large numbers in front of chemical formulas. Represents the number of molecules of the substance.

2Al

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7
Q

Diatomic Molecules

A

If these elements appear by themselves in an equation, the must be in pairs with the subscript 2.

(H₂, N₂, O₂, F₂, Cl₂, Br₂, I₂)

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8
Q

Reactants

A

Substances being mixed in a chemical reaction. The left side of the equation.

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9
Q

Products

A

Substance(s) being made. Right side of the equation.

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10
Q

Synthesis or Combination

A

Two or more elements combine to make one product.

A + B –> AB

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11
Q

Decomposition Reaction

A

One reactant breaks down into two or more elements.

AB –> A + B

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12
Q

Single Replacement

A

An element and a compound are located on each side of the equation. The Activity Series must be checked to determine if the reaction will occur. If the reaction occurs, the element on the reactant side switches with the similarly charged ion within the compound on the reactant side.

A + BC –> AC + B

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13
Q

Double Displacement

A

There are two compounds on each side of the equation. During a DD Reaction the positively charged cations in each compound switch places. Also known as Precipitate Reaction. For the reaction to occur a precipitate must be formed. The solubility rules or table are used to confirm this.

AB + CD –> AD + CB

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14
Q

Precipitate

A

Formation of a solid in a solution.

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15
Q

Definition of a balanced chemical equation:

A

no atoms are lost or gained

the number of reacting atoms is equal to the number of product atoms

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16
Q

Predict the products and write a balanced equation from the following word statement:

Methane (CH₄) plus Oxygen Gas forms:

A
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17
Q

How to PREDICT PRODUCTS of the 4 Main Types of Chemical Reactions.

A
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18
Q

Predict the products of and write a balanced equation from the following word statement:

Methane (C3H8) reacts with Oxygen gas to form __________.

A
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20
Q

Subscript

A

Small numbers to the lower right of chemical symbols. Represent the number of atoms of each element in a molecule.

O₂

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30
Q

Combustion

A

Any compound formed from only Carbon an Hydrogen (fuel) added to Oxygen to produce Carbon Dioxide and Water.

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34
Q

Write a chemical equation from the following word equation:

Magnesium reacts with oxygen to form magnesium oxide.

A

2Mg + O₂ –> 2MgO

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35
Q

Write a chemical equation from the following word equation:

Magnesium reacts with aluminum chloride to form magnesium chloride and aluminum.

A

3Mg + 2AlCl₃–> 3MgCl₂ + 2Al

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36
Q

Write a chemical equation from the following word equation:

Sodium reacts with fluorine to form sodium fluoride

A

2Na + F₂–> 2NaF

37
Q

Write a chemical equation from the following word equation:

Lithium chloride reacts with magnesium nitrate to form lithium nitrate and magnesium chloride.

A

2LiCl + Mg(NO₃)₂ –> 2Li(NO₃) + MgCl₂

38
Q

Write a chemical equation from the following word equation:

Water decomposes into hydrogen gas and oxygen gas:

A

2H₂O → 2H₂ + O₂

39
Q

Predict the products of and write a balanced equation from the following statement:

C₄H₆ + O₂ →

A

2C₄H₆ + 7O₂ →4CO₂ + 6H₂O

Combustion

40
Q

How would temperature and pressure affect the equilibrium of the following reaction?

N2 + 3H2 ⇔ 2NH3 + heat

A
41
Q

How would removing ammonia, NH3, affect the equilibrium of the following reaction?

N2 + 3H2 ⇔ 2NH3 + heat

A
42
Q

Predict the products of and write a balanced equation from the following statement:

Mg + I₂ →

A

Mg + I₂ →MgI₂

Synthesis

43
Q

Predict the products of and write a balanced equation from the following statement:

CuCl₂ + H₂S →

A

CuCl₂ + H₂S →CuS + 2HCl

Double Replacement

44
Q

Predict the products of and write a balanced equation from the following statement:

HCl + Zn →

A

2HCl + Zn →ZnCl₂ + H₂

Single Replacement

45
Q

Predict the products of and write a balanced equation from the following statement:

H₂O₂ →

A

H₂O₂ → H₂ + O₂

DECOMPOSITION

46
Q

Balance the following chemical equation:

__Al₂(SO₄)₃ + __Ca(OH)₂ → __Al(OH)₃ + __CaSO₄

A

Al₂(SO₄)₃ + 3Ca(OH)₂ → 2Al(OH)₃ + 3CaSO₄

47
Q

Balance the following chemical equation:

__C₂H₆ + __O₂ → __CO₂ + __H₂O

A

2C₂H₆ + 7O₂ → 4CO₂ + 6H₂O

48
Q

Balance the following chemical equation:

__C + __O₂ → __CO₂

A

1C + 1O₂ → 1CO₂

49
Q

C₄H₆ + O₂ →

A

2C₄H₆ + 7O₂ →4CO₂ + 6H₂O Combustion

50
Q

Mg + I₂ →

A

Mg + I₂ →MgI₂ Synthesis

51
Q

CuCl₂ + H₂S →

A

CuCl₂ + H₂S →CuS + 2HCl Double Replacement

52
Q

NaOH + HClO₄ →

A

NaOH + HClO₄ →NaClO₄+ H₂O Double Replacement

53
Q

HCl + Zn →

A

2HCl + Zn →ZnCl₂ + H₂ Single Replacement

54
Q

Na + MgCl₂ →

A

2Na + MgCl₂ →2NaCl + Mg Single Replacement

55
Q

CaCl₂ + K₂CO₃ →

A

CaCl₂ + K₂CO₃ →CaCO₃ + 2KCl Double Replacement

56
Q

K + Cl₂ →

A

2K + Cl₂ →2KCl Synthesis

59
Q

How does a reaction at equilibrium shift when more reactants are added?

A

Reaction shifts to the right to make more product.

60
Q

How does a reaction at equilibrium shift when reactants are removed?

A

Reaction shifts to the left to make more reactant.

61
Q

How does a reaction at equilibrium shift when more products are added?

A

Reaction shifts to the left to make more reactant.

62
Q

How does a reaction at equilibrium shift when products are removed?

A

Reaction shifts to the right to make more product.

63
Q

What happens to an endothermic reaction when temperature is increased?

A

Heat is a reactant, so the reaction will shift to the right to make more product.

64
Q

What happens to an endothermic reaction when temperature is lowered?

A

Heat is a reactant, so the reaction will shift to the left to make more reactant.

65
Q

What happens to an exothermic reaction when temperature is increased?

A

Heat is a product, so the reaction shifts to the left to make more reactant.

66
Q

What happens to an exothermic reaction when temperature is lowered?

A

Heat is a product, so the reaction shifts to the right to make more product.

67
Q

What happens when the pressure of a reaction at equilibrium is increased?

A

It depends if there are gases present. If there ARE gases present, reaction will shift to the side with the lower number of moles of gas.

68
Q

What happens when the pressure of a reaction at equilibrium is increased?

A

It depends if there are gases present. If there ARE gases present, reaction will shift to the side with the greater number of moles of gas.

Perryland Chemistry Theory - 2015 Standards (12 decks)

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