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Chemistry 11 > Chapter 4 Test > Flashcards

Chapter 4 Test Flashcards

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1
Q

Chemical Reaction

A

The changes or transformations of various kinds of matter into other substances with different compositions, structures and properties described using chemical equations

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2
Q

Evidence/observations of a chemical reaction

A 
Change in temperature
Evolution of a gas
Formation of a Precipitate
Change in colour
Formation of an odour
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3
Q

3 Laws a Chemical Reaction Must Follow

A
  1. Conservation of Mass
  2. Conservation of Charge
  3. Conservation of Energy
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4
Q

Conservation of Mass

A

The total mass of the reactants equals the total mass of the products

balance equation

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5
Q

Conservation of Charge

A

Since the total # of electrons and protons after a chemical reaction is the same as before the reaction, the # of positive and negative charges remains constant

Charge of reactant = charge of product

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6
Q

Conservation of Energy

A

The total amount of energy after a chemical reaction equals the total amount of energy before the reaction

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7
Q

What does a chemical reaction require?

What is the rate of reaction determined by?

A

A chemical reaction requires a collision between reactant particles

The rate of a reaction is determined by measuring the amount of products formed

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8
Q

5 Factors Affecting the Rate of a Chemical Reaction

A
  1. Temperature
  2. Catalysts/Enzymes
  3. Concentration and Surface Area
  4. Pressure
  5. Reversiblity
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9
Q

Temperature

A

An increase causes an increase in in the rate of the chemical reaction

An increase in temperature results in an increase in the kinetic energy (movement of the particles) of the reactants; this causes the reactants to collide faster, harder and more often, increasing the chances to form bonds

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10
Q

Catalysts/ Enzymes

A

A chemical which speeds up a reaction but is itself unaffected

A catalyst lowers the initial energy “kick”/ activation energy required to start a reaction

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11
Q

Concentration and Surface Area

A

An increase in the concentration of reactants and an increase in the surface area increases the rate of reaction.

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12
Q

Pressure

A

It has no effect on the volume of a solid or liquid, therefore, no effect on the rate of the reaction
→ an increase in the pressure exerted on a gas will decrease the volume which in turn increases the concentration, therefore, an increase in the rate

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13
Q

Reversibility

A

Does not influence the rate of a chemical reaction, however, not all reactants are converted to products

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14
Q

Chemical equation

A

A shorthand description of a chemical change using symbols and formulas to indicate the substances involved in the change

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15
Q

Reactant

A

A substance that undergoes a chemical reaction

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16
Q

Product

A

A substance that is formed in a chemical reaction

17
Q

Endothermic

A

Energy is absorbed (feels cold) +△H

18
Q

Exothermic

A

Energy is given off (feels hot) -△H

19
Q

Precipitate

A

An insoluble solid that forms when 2 liquids are mixed

20
Q

Synthesis Reaction

A + B → AB

A

Atoms and molecules join together directly to produce larger molecules

Combustion and corrosion are synthesis reactions

21
Q

Decomposition

AB → A + B

A

The exact opposite of synthesis reactions

22
Q 
Special Synthesis and Decomposition Reactions:
metal oxide (basic oxide) + water
A

Metal oxide (basic oxide) + water→base

_____ hydroxide OH

Ex: MgO + H2O → Mg(OH)2
Mg(OH)2 →MgO + H2O

23
Q

Special Synthesis and Decomposition Reactions:

Non-metal oxide(acidic oxide)+ water

A

Non-metal oxide(acidic oxide)+ water→ acid

______ic acid H oxyacid can be used too

Ex: CO2 + H2O → H2CO3(aq)
H2CO3(aq) → CO2(g) + H2O

24
Q

Special Synthesis and Decomposition Reactions:

Metal oxide + Non-metal oxide

A

Metal oxide + non-metal oxide → metal oxyanion

EX: MgO +CO2 →MgCO3
MgCO3 → MgO + CO2

25
Q

Complete Combustion:

A

Sufficient supply of oxygen

CH(g) + O2(g) → CO2(g) + H20(g) + energy (exothermic)
Hydrocarbon + oxygen→ carbon dioxide + water vapour + energy

26
Q

Incomplete Combustion

A

Insufficient supply of oxygen

CH(g) + O2(g)→ CO2(g) + H2O(g) + CO(g) + C(s) + energy

Hydrocarbon + oxygen → carbon dioxide + water vapour + carbon monoxide + carbon + energy

27
Q

Danger of Incomplete Combustion

A

Carbon monoxide gas is dangerous because of its physical properties. It is a gas, odourless and non-combustible. It has the same configuration as oxygen so it competes with oxygen to bind to the hemoglobin sites in the RBC’s. But unlike oxygen, the binding to hemoglobinis permanent. The somatic cells will eventually starve of oxygen and die. High CO in the body is lethal

28
Q

Symptoms of CO poisoning

A 
Dizziness
Headache
Nausea
Vomiting
Shortness of breath
Loss of consciousness
29
Q

Visible signs of incomplete combustion

A

Yellow flame instead of blue flame

Formation of soot

30
Q

Soot

A

Carbon monoxide + Carbon

31
Q

To determine a type of gas during gas test

A

OXYGEN: use a glowing splint and it will burst into flames

CARBON DIOXIDE: a burning splint will have its flame extinguish OR use limewater and the water will turn from clear→ cloudy

HYDROGEN: you will hear a ‘pop’ from a burning splint

32
Q

any time carbonic acid or ammonium hydroxide is formed as a product, it decomposes further

A

Carbonic acid: H2CO3 (aq)
→ H2O (l) + CO2 (g)

Ammonium hydroxide:NH4OH (aq)
→H2O (l) + NH3 (g)

33
Q

NO REACTION: single displacement

A

If the 1st metal is less reactive than the 2nd metal

Use activity series chart

34
Q

NO REACTION: double displacement

A

If the 1st metal is less reactive than the 2nd metal

If neither soluble ionic compounds precipitates out

35
Q

Group 17: if halogen (standalone) is higher than the halogen in the compound, a reaction will take place

A

Yes

Chemistry 11 (5 decks)

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