C4 - Predicting and identifying reactions and products Flashcards

1
Q

What name do the Group 1 metals have?
Why do they have this name?

A
  • Alkali metals
  • They form alkaline solutions in water.
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2
Q

Group 1 metals properties compared to other metals (Similarities and comparisions)

A

Similarly:
- Shiny when freshly cut
- Good conductors of metals

However:
- Soft enough to cut with a knife
- More reactive than other metals

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3
Q

Trends shown by the Group 1 metals as you go down

A
  • They become softer.
  • Melting & boiling points decrease.
    (delocalised electrons are closer to atomic nucleus, so electrostatic forces of attraction are greater)
  • Density generally increases (sodium is the exception).
  • Reactivity increases.
    (it is easier to loose valence shell electrons with more shells; further for nuclei, weaker forces of attraction)
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4
Q

Alkali metals and water reaction word equation

A

Alkali Metal + Water –> Metal Hydroxide + Hydrogen

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5
Q

How do the different alkali metals react with water?

A
  • Lithium fizzes and slowly disappears
  • Sodium melts to form a silvery ball, fizzes vigorously, and quickly disappears.
  • Potassium quickly ignites, burns with a lilac flame, and very quickly disappears.
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6
Q

How do the different halogens exist at room temperature?

A
  • Fluorine (Fl2) is a pale yellow gas.
  • Chlorine (Cl2) is a green gas.
  • Bromine (Br2) is an orange-brown liquid that vaporises easily.
  • Iodine (I2) is a shiny grey-black crystalline solid that sublimes to form a purple vapour.
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7
Q

Trends shown by the Group 7 halogens

A

As you go down:
- Density increases.
- Melting points and boiling points increase.
(larger molecules, stronger IM forces)
- Reactivity decreases.
(easier to gain electrons when the valence shell is closer to the atomic nuclei; stronger electrostatic forces of attraction)

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8
Q

Why are the noble gases so unreactive?

A

They have full outer shells of electrons, so they have no tendency to lose/gain electrons.

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9
Q

Trends shown by the Group 8 Noble Gases

A

They are monoatomic.

As you go down:
- The attractive forces between atoms gets stronger.
- Their boiling point increases.
- Density increases.

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10
Q

Why do noble gases have low densities?

A
  • Their atoms are far apart in the gas state.
  • There is very little mass in a given volume.
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11
Q

Transition metals properties

A
  • Shiny when freshly cut
  • Good conductors of electricity
  • Strong
  • Malleable (they can be bent/hammered into shape)
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12
Q

Compared to the alkali metals, transitions metals are:

A
  • Stronger and harder
  • Have higher densities
  • Have higher melting points (except for Mercury at liquid state)
  • Less reactive (more useful for everyday activities)
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13
Q

Chemical properties of the transition metals

A
  • Iron reacts slowly with water and oxygen to produce rust (hydrated iron (II) oxide)
  • Gold, platinum, and iridium do not react with water or oxygen at all.
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14
Q

What colour ionic compounds of the different metals? (Transition vs Alkali)

A
  • Alkali metals produced white or coloured ionic compounds.
  • Transition metals produce coloured ionic compounds.
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15
Q

What charge do metal ions have? (Transition vs Alkali)

A
  • Alkali metal ions have a single positive charge, as they lose one electron.
  • Transition metals can form more than one type of ions.
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16
Q

Which metals are good catalysts?

A

Transition metals

17
Q

How do metals react with water and dilute acids?

A

Water:
- Produces a metal hydroxide and hydrogen
- Calcium + Water –> Calcium Hydroxide + Hydrogen

Dilute acid:
- Produces a salt and hydrogen.
- Calcium + Hydrochloric acid –> Calcium Chloride + Hydrogen

18
Q

Detecting carbon dioxide

A
  • Limewater (calcium hydroxide solution)
  • Bubble carbon dioxide through limewater and it will turn cloudy.
  • This is because the calcium hydroxide reacts with carbon dioxide to form water and a white precipitate of calcium carbonate.
19
Q

Detecting Chlorine

A
  • Dampened piece of blue litmus paper.
  • Hold it near the gas.
  • It turns red then bleaches white.
20
Q

Why does the litmus paper have to be dampened when testing for chlorine?

A
  • Chlorine dissolves in the water to form an acidic solution which bleaches the litmus paper.
21
Q

How to perform flame test

A
  • Clean nichrome wire loop in hydrochloric acid, then distilled water.
  • Put it over bunsen burner to ensure it’s clean.
  • Dip clean loop into test powder/solution.
  • Place under blue roaring flame.
22
Q

Flame test results (Lithium, Sodium, Potassium, Calcium, Copper)

A
  • Lithium: Red
  • Sodium: Yellow
  • Potassium: Lilac
  • Calcium: Orange-red
  • Copper: Green-blue
23
Q

Hydroxide precipitate tests (Iron2, Iron3, Copper2, Calcium, Zinc)

A
  • Iron(II): Green
  • Iron(III): Orange-brown
  • Copper(II): Blue
  • Calcium: White
  • Zinc: White

Add few drops sodium hydroxide solution to the solution containing the ions.

24
Q

Detecting sulphate ions

A
  • Add few drops of dilute hydrochloric acid
  • Add few drops of barium chloride solution
  • White precipitate SHOULD form.
25
Q

Detecting carbonate ions

A
  • Add few drops of dilute hydrochloric acid.
  • Bubbles of gas should produce (carbon dioxide).
  • Confirm this is CO2 but bubbling it through limewater.
26
Q

Detecting halide ions

A
  • Add few drops of dilute nitric acid
  • Add few drops of silver nitrate solution
  • Chloride: White
  • Bromide: Cream
  • Iodide: Yellow
27
Q

Advantages of instrumental methods of analysis

A
  • Sensitivity: They can analyse very small amounts of substances.
  • Accuracy: They are very accurate and can be calibrated to a universally accepted standard.
  • Speed: They run all the time and analyse quickly.