That whole fucking chem GCSE in a nutshell 🙂

Question 1

What did newlands do for periodic table

Answer 1

• arranged elements in order of atomic mass

- left no spaces

Question 2

Why was Mendeleev periodic table BETTER THAN newlands

Answer 2

• left spaces
• predicted properties
• atomic mass

Question 3

Reactivity increases as you go down GROUP 1 because….

Answer 3

• elements are bigger ( more shells of electrons)
• outer shell electron further from nucleus- attraction decreases
• electron more easily lost
• MORE shielded

Question 4

Group 1 in water…

Answer 4

• fizz, release hydrogen gas
• move around, float
• eventually sink
• make water purple when universal indicator added to it, meaning it alkali

Question 5

Metal+ COLD water———>

Answer 5

Metal hydroxide+ hydrogen

Question 6

Metal+ steam———->

Answer 6

Metal oxide+ hydrogen

Question 7

Why do group 7 elements become less reactive as you go down group

Answer 7

• elements are larger
• harder to gain electron
• outer shell electron is further from nucleus and more shielded

Question 8

Properties of halogens

Answer 8

• LOW boiling points

- poor conductors

Question 9

Properties of transition metals

Answer 9

• GOOD conductors of heat and electricity
• hard
• strong
• high density
• high MELTING points

Question 10

Describe the properties of transition metal compounds

Answer 10

• coloured
• catalysts
• multiple ions

Question 11

When does ionic bonding occur

Answer 11

Between metals and non metals

Question 12

When does covalent bonding occur

Answer 12

Between non metals only

Question 13

Covalent bonding is…….

Answer 13

A shared pair of electrons

Question 14

Ionic bonding is…..

Answer 14

Strong forces of attraction between oppositely charged ions

Question 15

Why do ionic structures have such high MELTING points?

Answer 15

• strong forces of attraction between oppositely charged ions
• require lots of energy to break

Question 16

Why are ionic structures brittle?

Answer 16

• when force is applied ions with the same charge end up next to each other
• like charges repel
• structure falls apart

Question 17

Structure of metals….

Answer 17

• positive ions

- surrounded by a sea of delocalised electrons

Question 18

Alloy?

Answer 18

Mixture of two or more metals

Question 19

Why are alloys harder than individual metals?

Answer 19

• ions of different sizes

- more difficult for layers to slide over each other

Question 20

Why does DIAMOND have such a high MELTING point

Answer 20

• giant covalent structure
• EACH carbon atom is bonded to four others
• many strong covalent bonds
• require lots of energy to break

GRAPHITE IS THE SAME JUST BONDED TO THREE OTHERS NOT FOUR

Question 21

Why does graphite conduct electricity

Answer 21

• EACH carbon atom is only bonded to three others

- 4th electron free to move

Question 22

Why is graphite used as a lubricant

Answer 22

• Carbon atoms arranged in layers
• layers are held together by weak intermolecular forces
• does not require a lot of energy to break
• layers slide off each other

Question 23

Define polymer

Answer 23

A large molecule formed of many small monomers which JOIN together

Question 24

Define Thermosetting polymer

Answer 24

Can’t be heated and then RE shaped

Question 25

Define thermosoftening polymer

Answer 25

Can be heated and RE shaped CHAINS ARE HELD TOGETHER BY WEAK INTERMOLECULAR FORCES WHICH ARE EASY TO RE SHAPE

Question 26

SOME examples of nanoscience in industry

Answer 26

- glass coated in nanoparticles. Sunshine triggers reaction which breaks down dirt - sunscreen contains nano particles which are better blockers of UV rays - nanoparticles in face creams are absorbed deeper into the skin

Question 27

Method of titration 100% copied this off bitesize, its got it all there friends

Answer 27

Use the pipette and pipette filler to add 25 cm3 of alkali to a clean conical flask. Add a few drops of indicator and put the conical flask on a white tile (so you can see the colour of the indicator more easily). Fill the burette with acid and note the starting volume. Slowly add the acid from the burette to the alkali in the conical flask, swirling to mix. Stop adding the acid when the end-point is reached (the appropriate colour change in the indicator happens). Note the final volume reading. Repeat steps 1 to 5 until you get consistent readings The same method works for adding an alkali to an acid - just swap around the liquids that go into the conical flask and burette.

Question 28

Less than 100% yield in titration (or I guess other reactions idrk) because........

Answer 28

- SOME product is lost - reversible reaction - reactant form unexpected products

Question 29

Reactivity series

Answer 29

``` POTASSIUM SODIUM LITHIUM CALCIUM MAGNESIUM ALUMINIUM CARBON ZINC IRON HYDROGEN COPPER SILVER GOLD ```

Question 30

TEST for hydrogen

Answer 30

Lighted splint | Squeaky pop

Question 31

Hydrochloric acid+ sodium hydroxide-----> Acid+ base= Salt+ WATER

Answer 31

Sodium chloride+ water GET THE NAME OF THE SALT, IN THIS CASE SODIUM AND THEN PUT THE END OF THE ACID NEXT TO THE SALT... HYDROCHLORIC= CHLORIDE SO SODIUM CHLORIDE

Question 32

Metal+ acid= Salt+ hydrogen Nitric acid+ magnesium------->

Answer 32

Magnesium nitrate + hydrogen

Question 33

Acid+ metal oxide------->

Answer 33

Salt+ WATER

Question 34

Acid+metal carbonate------->

Answer 34

Salt+ WATER + carbon dioxide

Question 35

PANIC

Answer 35

Positive anode | Negative is cathode