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Chem summed > Summarised > Flashcards

Summarised Flashcards

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1
Q

What group are noble gases

A

0

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2
Q

Name the 5 noble gases and their uses

A

Helium - balloons
Neon - lights
Argon - lightbulbs
Krypton- high efficiency miners lamps
Radon - radioactive research

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3
Q

What group are alkali metals and name them

A

Group 1, lithium, sodium, potassium, calcium, francium

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4
Q

Why does reactivity increase down the alkali metal group?

A

Reactivity increases as the negative electron in the valence is further away from the positive nucleus. It is therefore less attracted and can be lost easily.

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5
Q

What are the observations of placing lithium, sodium, potassium and rubidium in water?

A

Lithium - fizzing, moving as well
Sodium - small spark and more fizzing
Potassium - bigger explosion lilac flame
Rubidium- huge explosion

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6
Q

What group are the halogens

A

7

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7
Q

What happens to the reactivity down the halogens and why?

A

The reactivity decreases down the group as the attraction of the nucleus to the outer shell is weaker, making it harder to gain an electron in outer shell

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8
Q

What are endothermic reactions?

A

This is when energy is taken in from surroundings

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9
Q

What are exothermic reactions?

A

This is when energy is released to surroundings

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10
Q

State 2 examples of endothermic reactions

A

Thermal decomposition and sport injury packs

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11
Q

State 3 examples of exothermic reactions

A

Combustion, many oxidation reactions, neutralisation

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12
Q

What is ionic bonding?

A

This occurs between a non metal and a metal, the metal loses electrons and the non metal gains electrons

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13
Q

What is covalent bonding?

A

This occurs between 2 non metals where they share electrons. It forms molecules.

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14
Q

What is the difference between small and large covalent structures

A

Small - tend to be gases, have less elements, lower melting points and weak intermolecular forces.
Large - tend to have more elements with lots more bonds. Higher melting points and higher intermolecular forces.

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15
Q

State the properties of silicon dioxide ( sand )

A

Each bond is joined to 4 other silicon elements, insoluble, doesn’t conduct electricity, high melting point.

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16
Q

State the properties of graphite.

A

Carbon atoms are joined to 3 other atoms in hexagonal columns, these are layered, conducts electricity and has a high melting point

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17
Q

Why can graphite conduct electricity

A

Graphite has delocalised electrons, just like metals. These electrons are free to move between the layers in graphite, conducting electricity.

18
Q

State the properties of diamond

A

Each carbon atom is bonded to 4 others, hard, doesn’t conduct electricity, high melting point

19
Q

What is a fullerene

A

This is 60 carbon atoms joint in a spherical structure.

20
Q

What is the first fullerene known as?

A

Buckminsterfullerene

21
Q

What is a graphene?

A

This is 1 layer of graphite in a hexagonal structure.

22
Q

What forces are between ionic bonds’

A

Electrostatic

23
Q

What forces are between covalent bonds?

A

Intermolecular

24
Q

If an element is below carbon in the reactivity series what happens?

A

Carbon displaced it.

25
Q

What is the configuration for chloride?

A

Cl-

26
Q

What is the configuration for sulfate?

A

SO4 ²-

27
Q

What is the configuration for nitrate?

A

NO3-

28
Q

What is the configuration for hydrochloric acid?

A

HCl

29
Q

What is the configuration for nitric acid?

A

HNO ³

30
Q

What is the configuration of sulphuric acid?

A

H ² SO ⁴

31
Q

Equation for overall energy change?

A

Energy needed to break bonds (reactants) — energy released from bonds (products)

32
Q

Equation for moles?

A

Moles = mass (g) / Mr

33
Q

Equation for concentration (g/dm ³)

A

Mass (g) / volume (dm ³)

34
Q

Equation for concentration (mol/ dm ³)

A

Moles / volume (dm ³)

35
Q

How to convert from dm ³ to cm ³?

A

X1000

36
Q

What is avogrados constant?

A

6.02 x 10 ²³

37
Q

What is the pneumonic for the reactivity series?

A

People Say Little Children Make A Zebra Ill However Constantly Sniffing Giraffes.

38
Q

What are the steps to electrolysis and state the conclusions that would occur

A
  1. Place 50cm ³ of acid into a beaker
  2. Insert 2 non-touching carbon electrodes
  3. Attach crocodile leads to electrodes and connect to power, turning on.
  4. Cations discharged at cathode ( reduction )
    Anions discharged at anode. ( oxidation )
  5. Repeat to avoid error
39
Q

What are the rules for electrolysis?

A

Hydrogen is produced at cathode if metal is more reactive. Metal produced if not. Halide ions discharged as halogen gases at anode or hydroxide ions (Oh-) given off as oxygen gas

40
Q

What is the experiment for making salts? ( 6 steps)

A
  1. Fill beaker with fixed volume of sulphuric acid
  2. Gently heat acid until almost boiling + add small amounts of metal with spatula
  3. Stir solution with glass rod and keep adding metal until in excess
  4. Filter excess using filter paper and place solution in evaporating basin + head to evaporate water
  5. Leave for 24 hours in a cool place for crystals to form
  6. Scrape crystals onto tissue paper and pat them to dry, gently
41
Q

What is the practical involving temperature changes? (6 steps)

A
  1. Measure 30cm ³ of dilute Hcl in beaker
  2. Transfer to polystyrene cup and measure initial temperature using thermometer
  3. Measure 5cm ³ of sodium hydroxide solution and transfer to cup
  4. Place thermometer in lid hole and stir gently; record highest temperature reached
  5. Rinse cup out and repeat, increasing sodium hydroxide 5cm ³ more each time until 40cm ³
  6. Repeat whole experiment again and calculate means
42
Q
A

Chem summed (1 decks)

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