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Year 11 - Chemistry > Module 3 - Reactive Chemistry > Flashcards

Module 3 - Reactive Chemistry Flashcards

Main definitions and notes on Chemistry - Module 3

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1
Q

What is Decomposition?

What are the three types?

A

A compound is broken down into two or more other substances, which may be elements or other compounds.
Types: Thermal, Electrolysis, photolysis

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2
Q

Oxygen test

A

Glowing splint -

Oxygen gas inside the test tube relights the glowing splint

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3
Q

What is Thermal Decomposition?

Also, state a common example of thermal decomposition (CuCO3).

A

Breaking up a chemical substance with heat into at least two chemical substances.

A common example is Copper Carbonate, causing a colour change from green to black.

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4
Q

What are Spectator Ions?

Which ‘Ionic’ equation are they not included in?

A

Ions that do not take part in a chemical reaction and are found in solution both before and after the reaction. Removed in NET IONIC equations.

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5
Q

What type of reaction is Combustion?

State the equations for Complete
& Incomplete combustion.

A

An exothermic reaction of compounds burning in oxygen at extremely high temperatures.

Incomplete (Insufficient Oxygen) =
Carbon monoxide / soot + water
Complete (Excess oxygen) =
Carbon dioxide + water.

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6
Q

What is formed from a ‘precipitation’ reaction, and the specific solution required for a ‘precipitate’ to form?

What occurs with the ions?

A

An insoluble, ionic precipitate is formed when two aqueous solutions, containing different salts are mixed.

Cations and Anions of different solutions pair together to form the precipitate (insoluble salt) and an aqueous solution.
E.g: Sr(NO3)2 (aq) + LiOH (aq) –> Sr(OH)2 (s) + LiNO3 (aq)

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7
Q

What is the Net Ionic Equation?

Ions/Compounds, Charge/No charge, Connected/Separate?

A

Shows reactant IONS AND COMPOUNDS that undergo the reaction/relevant to precipitate. Ions/compounds are SEPARATE, shows CHARGES but no spectator ions.

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8
Q

What takes place during Synthesis?
What is a common example?
(Hint: Mg/Copper + O, converting Ammonia)

A

The formation of a more complex, chemical compound from two or more, simpler substances. Decreasing Entropy.
E.g: Ionic reaction of Magnesium & Copper reacting with Oxygen, conversion of ammonia into fertiliser (NH3).

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9
Q

State Oxidation Reaction and Acronyms.

Where is 2e- placed?

A

The loss of electrons from a substance involved in a redox reaction. 2e- is placed on RHS, as the product. (OIL) & (AN OX) - Oxidation no. increases.

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10
Q

How do higher temperatures affect the rate of reaction?

Collision frequency increase/decrease?

A

INCREASE in Rate of Reaction -

Molecules gain higher kinetic energy and move around faster = Collision frequency increases

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11
Q

What is the Complete Ionic equation?
Ions/Compounds, Charge/No charge, Connected/Separated?
What is always shown? (P____)

A

Shows ALL reactant IONS that are present in the reaction, SEPARATED equation and shows spectator ions. CHARGES are shown and the precipitate is always shown.

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12
Q

Explain the process of Electrolysis and the process with water.

A

Electrical decomposition of a liquid/aqueous solution.

E.g.: Water - intermolecular and intramolecular bond between Hydrogen and Oxygen are broken.

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13
Q

What equation is formed by the Acid-Carbonate Reaction? (Hint: 3 products)

What are 2 everyday examples?
(CaCO3) + (NaHCO3)

A

acid + carbonate –> salt + water + carbon dioxide

Example 1: Calcium Carbonate added to soil to neutralise the acidity.
Example 2: Sodium Bicarbonate and Tartaric Acid heated to cause a rise in bread due to Carbon Dioxide being produced.

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14
Q

Explain what a Galvanic Cell is and its energy process? (Produces and releases?)

State the components of a galvanic cell equation.
(A__ | A___ S___ || C__ S___ | C__)

A

Electrochemical cell powered by a spontaneous redox reaction that produces an electric current flow. Involves an exothermic reaction (Produces and releases energy)

Zn(s) | ZnSO4(aq) || CuSO4(aq) | Cu(s)

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15
Q

Carbon Dioxide Test

A

Limewater -

Turns it from clear and colourless to white and milky

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16
Q

State Reduction Reaction and Acronyms.
Where is 2e- placed?

How does this impact Oxidation no.?

A

The gain of electrons from a substance involved in a redox reaction. 2e- is placed on LHS as the reactant. (RIG) & (RED CAT).
Oxidation no. decreases as electrons are lost.

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17
Q

Which Soluble Ionic compounds are involved in the SNAAP Rule?

How does it determine which precipitate is formed first?

A

Soluble ionic compounds: (These salts always dissolve):
- Sodium: Na+, Nitrate: NO3-, Ammonium: NH4+, Acetate: CH3COOH-, Potassium: K+

The salt which is not any of these will form as a precipitate, these will dissolve.

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18
Q

What is an Anode? What is its purpose during
a Galvanic Cell process?
State how it is determined in a Galvanic Cell.

A

A negatively charged Electrode where OXIDATION occurs, anions are attracted to Anodes. From a Galvanic Cell, it is the more reactive metal.
(AN OX)

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20
Q

What happens to Reaction Rate in effect to
greater Surface Area?

Collision frequency increase/decrease?

A

INCREASE in Rate of Reaction -
More solute particles exposed to solvent particles. Greater chances for correct orientation to occur
= Collision frequency increases

21
Q

State the Collision Theory and the 2

factors required to initiate a reaction.

A

For a reaction to occur, the particles must collide with sufficient energy (Activation Energy) and correct, molecular orientation.

22
Q

Spontaneous Reaction - Info and what are the requirements

A

Reaction that forms products when the Electrochemical value is positive (E > 0 = Spontaneous reaction, E < O = (No reaction).

23
Q

What is the Complete formula equation? Ions/Compounds, Charge/No charge, Connected/Separate?

A

Shows COMPOUNDS used for the reaction which are connected WITHOUT CHARGES. CONNECTED equation.

E.g.: NO + HNO3 –> H2O + NO2

24
Q

Hydrogen Test

A

‘Popping Test’ -

Pop sound occurs when lit splint is over the test tube.

24
Q

How does Increased Concentration impact
Reaction Rate?

Collision frequency increase/decrease?

A

INCREASE in Rate of Reaction - More Solvent particles available, greater chances for correct molecule orientation
= Collision frequency increases

25
Q

How does Metal Activity Series affect the displacement of metals?

Higher-up Metal = ? (O & A)
Lower-down Metal = ? (R & C)

A

Metals higher in the activity series displace less-reactive metals.

'Higher'-Metal = Oxidised (Anode)
'Lower'-Metal = Reduced (Cathode)

E.g.: K(s) + FeSO4(aq) –> KSO4(aq) + Fe(s)

26
Q

What is Photolysis and what bonds are broken?

What is a common example? (Hint: AgCl)

A

Light decomposition - Intermolecular bonds are broken due to (Direct & Indirect) transfer of light energy.
E.g.: Silver Chloride changes colour from white to purple, then black. (Ag + Cl2)

27
Q

What is Ionisation Energy?
Do Anions/Cations have ↑ or ↓ Ionisation Energy?

State its Periodic table trend.
(Up a group=? Left to right=?)

A

The energy required to remove one electron from an atom. Determines chemical activity (Anions- Lower IE, Cations- Higher IE)

Up a group = Increases,
Left to Right = Increases

28
Q

What is a salt bridge and why is it required for a Galvanic Cell to properly function?

Where do the +ve and -ve electrons move? (Anode/Cathode).

A

Neutral device transferring anion and cations between two connected half-cells without reacting. Generally soaked in KNO3 / KCl.

Purpose: To remove excess positive ions in one solution and excess negative ions in the other solution.
-ve (Anions) move into the anode.
+ve (Cations) move into the cathode

29
Q

What happens to Reaction Rate when Pressure increases?

Collision frequency increase/decrease?

A

INCREASE in Rate of Reaction - Forces molecules closer together = Collision frequency increases.

30
Q

What is Electronegativity?
Explain its periodic table trend?
(Up a group=? Left to right=?)
Which elements does it not include?

A

Ability to attract shared electrons to form negative/positive ions. (Does not include Noble gases)

Up a group = Increase
Left to right = Increase.

31
Q

What is the Core Charge of an atom?
How is it calculated?
Periodic Table Trend?
(Down a group? Left to right=?)

A

The attractive force between the valence electrons and the nucleus of the atom.
Calculated by: no. of protons - no. of inner-shell electrons. (Always positive)

Down a group = No change
Left to right = Increases

32
Q

What is an Electrode?

Which parts of a Galvanic Cell is it connected to?

A

Cell conductors (generally metals) connected to an external circuit and also connected to the solution of one half-cell of a galvanic cell.

E.g.: Platinum, gold, zinc, copper.

33
Q

Metal Reactivity INCREASES when:

Ionisation Energy - ↑ / ↓?
Electronegativity - ↑ / ↓?
Atomic Radius - ↑ / ↓?

A

Ionisation Energy= ↓
Electronegativity= ↑
Atomic Radius= ↑

34
Q

What is Atomic Radius?
Periodic table trend?
(Down a group=? Left to right=?)

A

The distance from nucleus to the valence electrons. “Outer shell electrons readily lost due to long distance from nucleus.”

Down a group = Increases
Left to Right = Decreases.

35
Q

What are Cathodes? What is its purpose during a Galvanic Cell process?
State how it is determined in a Galvanic Cell.

A

Positively charged electrode where REDUCTION occurs as it gains electrons. It is the less-reactive metal in a Galvanic Cell.
(RED CAT)

36
Q

What are Electrolytes? What is produced from it and what is conducted?
Provide a common example of electrolytes in a galvanic cell.
(Hint: Salt bridge - Strong/Weak electrolyte)

A

A substance that produces ions in a solution when dissolved. These ions conduct electricity for a redox reaction to occur.

More ions = Greater conductivity
(Stronger electrolytes)
KCl is a strong electrolyte as it ionizes extremely fast. (Ionic electrolyte).

37
Q

What is the difference (energy specifically) between Spontaneous vs Non-Spontaneous reactions?
Provide an example for each.

A

Spontaneous - Electrical energy produced from the reaction. Only occurs if Anode is more reactive than Cathode in a Galvanic Cell.

Non-Spontaneous -
No energy produced, must be provided externally.
(Electrolytic Cell)

38
Q

Outline the 3 steps to calculate reduction potential (voltage) of two agents.
(Note: 3rd step = Reaction Type)

A

1) Higher-up agent is oxidised (switch sign)
E.g.: negative (Reduction) to positive (Oxidation)
2) Add both voltages of oxidation and reduction agents.
3) if value is +ve = Spontaneous
If value is -ve = Non-Spontaneous

39
Q

Outline the 4 ways Rate of Reaction can be observed.

State the measuring device used for the first 3.

A

1) Volume of gas produced over a period of time (gas syringe)
2) Mass lost over a period of time (electronic balance)
3) Change in temperature over a period of time (thermometer)
4) Change in colour/turbidity over time (only for precipitations)

40
Q

During a reaction, what does Activation Energy refer to and what bond does it break?

A

The minimum amount of energy required for a reaction to occur.
Breaks the intermolecular bonds in the reactants, to then form products.

  • If energy is > Ea, a spontaneous reaction will occur
41
Q

State what molecular orientation during collision is.

What happens when correct orientation occurs? (Bonds)

A

Must collide in the favourable orientation for a spontaneous reaction to occur.

  • Correct orientation is required to both break and form intermolecular bonds.
42
Q

How does solubility rules affect precipitation reactions?

A

The product formed which is insoluble will be the precipitate, whereas the product that is soluble will be dissolved in the aqueous solution.

43
Q

State the solubility rule mnemonic NAG SAG.

State which groups/elements are excluded?
PMS | Castro Bear

A 
Soluble: NAG SAG
Nitrates, Acetates, Group 1 (Li, Na, etc.
Sodium, Ammonium, Group 17 (F, Cl, etc.)
Excluded: PMS, CAStRo BeAr
Pb (lead), Hg (Mercury), Silver (Ag)
Ca, Sr, Ba
44
Q

Explain the 3 chemical processes that occur when detoxifying Cycads.
(T___ D___, F___, L___).
What is produced from F___ as well?

A

1) Thermal Decomposition: Kernel is heated, causing the intermolecular bonds between toxins and cycad to be broken. Toxins become soluble and leached off.
2) Fermentation: Stored in a warm environment for a long time, where bacteria and fungi dissolve the toxins. Carbon dioxide is produced, and seeds are then used after washing it.
3) Leaching - The surface area of the Cycad increases as it is crushed up, able to be dissolved faster.

45
Q

Explain what Galvanising and Electroplating are.

What are the differences between both types of Chemical reactions? (Hint: Coating, energy)

A

Galvanising - Process of applying zinc coating to a more noble metal to prevent corrosion (rusting).
Electroplating - Process of plating one metal onto another by hydrolysis, onto another metal surface.

Galvanising does not require energy, while electroplating requires electrical energy for the plates to combine/stick.

46
Q

What is the general structure for an Ionic and Net Ionic equation for Galvanic Cells?

A

Ionic: Anode + Cathode Solution –> Anode Solution + Cathode

Net Ionic: Anode + Cathode Solution (No SI) –> Anode Solution (No SI) + Cathode

Year 11 - Chemistry (4 decks)

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