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Types of Reaction > types of reactions > Flashcards

types of reactions Flashcards

1
Q

the formulae and combining powers of carbonate

A

formulae: CO3
combining power: -2

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2
Q

the formulae and combining powers of nitrate

A

formulae: NO3
acid:HNO3
combining power: -1

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3
Q

the formulae and combining powers of sulfate

A

formulae: SO4
acid:HSO4
combining power: -2

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4
Q

the formulae and combining powers of hydroxide

A

formulae: OH
combining power: -1

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5
Q

the formulae and combining powers of ammonium

A

formulae: NH4
combining power: +1

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6
Q

Definition of oxidation

A

addition of oxygen

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7
Q

Definition of reduction

A

removal of oxygen

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8
Q

What is the formula for Hydrochloric acid

A

HCL

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9
Q

what is the definition of neutralisation

A

an acid and a base make salt and water

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10
Q

what is the definition of decomposition

A

a reaction when a substance breaks apart into two or more substances

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11
Q

what is the definition of precipitation

A

a reaction where two solutions make a solid

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12
Q

what is the definition of displacement

A

a reaction where less reactive element is replaced with a more reactive element in a compound

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13
Q

how can you identify if a substance is an acid

A

acid always starts with H and bases

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14
Q

How do you use reduction to extract metal

A

you can use reduction by reacting a metal oxide with a reducing agent

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15
Q

Recall the colors of universal indicator

A

red, orange, yellow, green, blue, purple

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16
Q

Recall the colors of phenolphthalein

A

pink/ magnate colour for base and transparent for all others

17
Q

how do you measure rate of reaction using vol of gas

A

Collect the gas in a gas syringe and measure how much gas was collected within 20s.

18
Q

Describe how neutralisation can be used to prepare a salt by titration

A

Measure HCL (conical flask) add 3 drops phenolphthalein, mixture will turn colourless. using pipette add drops of NaOH slowly into acid until turns permanent pink colour. Record volume of NaOH required for neutralisation. re-measure HCL and add reaquired NaOH (with no indicator), heat solution until most water is evaporated. Leave solution to crystallise

19
Q

recall the general equation for the decomposition of metal carbonate

A

metal carbonate (+ energy) –> metal oxide + carbon dioxide

20
Q

recall the patterns in thermal stability of metal carbonates

A

group 2 metal carbonates are unstable (decompose)
group 1 metal carbonates are stable (do not decompose)

21
Q

Describe how salts can be prepared through precipitation

A

react 2 aqueous salts. they will produce a insoluble salt which can be filtered out.

22
Q

what is the chemical test for hydrogen?

A

test: buring splint
result: expoldes

23
Q

chemical test for Oxygen

A

glowing splint, will reignite

24
Q

metal carbonate -

A

metaloxide + carbondioxide

25
Q

define ‘endothermic’

A

a reaction that absorbs heat energy (temperature decreases)

26
Q

define ‘exothermic’

A

a reaction that releases heat energy (temperature increases)

27
Q

what is the chemical test for carbon dioxide?

A

test: lime water
result: turns cloudy

28
Q

What observations can be used to measure the rate of reaction

A

effervescing, solid disappearing, mass change, colour change

29
Q

what methods can be used to change the rate of reaction?

A

1.surface area
2.concentration (of solution)
3. Temperature
4. Catalyst

30
Q

What is the test for chlorine

A

test: damp universal indicator paper result: yellow - red - white

31
Q

metal + acid

A

salt + hydorgen

32
Q

what is the chemical test for oxygen

A

test: Glowing splint
Result: Splint reignites

33
Q

What chemicals are acids? (name and formula)

A

Hydrochloride (HCL)
Nitric (HNO3)
Sulfuric (H2SO4)
non-metal oxide

34
Q

describe the requirements for particles to react during collisions

A

sufficient energy and the correct orientation

35
Q

explain how surface area affects the rate of reaction

A

greater surface area -> particles more frequently in the correct orientation -> react more frequently-> rate or reaction increases

36
Q

explain how concentration affects the rate of reaction

A

greater concentration -> more particles dissolved in water ->more collisions (react more frequently)-> rate or reaction increases

37
Q

explain how temperature affects the rate of reaction

A

greater temperature -> particles more often have sufficient energy -> react more frequently-> rate or reaction increases

38
Q

define the term catalyst

A

a chemical which speeds up the rate of reaction without being used up.
catalysts are specific to individual reactions

Types of Reaction (1 decks)

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