That whole fucking chem GCSE in a nutshell 🙂 Flashcards by Pilar Thorley-Saiz | Brainscape

Q

What did newlands do for periodic table

A

arranged elements in order of atomic mass

- left no spaces

How well did you know this?

1

Not at all

2

3

4

5

Perfectly

Q

Why was Mendeleev periodic table BETTER THAN newlands

A

left spaces
predicted properties
atomic mass

How well did you know this?

1

Not at all

2

3

4

5

Perfectly

Q

Reactivity increases as you go down GROUP 1 because….

A

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

How well did you know this?

1

Not at all

2

3

4

5

Perfectly

Q

Group 1 in water…

A

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

How well did you know this?

1

Not at all

2

3

4

5

Perfectly

Q

Metal+ COLD water———>

A

Metal hydroxide+ hydrogen

How well did you know this?

1

Not at all

2

3

4

5

Perfectly

Q

Metal+ steam———->

A

Metal oxide+ hydrogen

How well did you know this?

1

Not at all

2

3

4

5

Perfectly

Q

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

A

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

How well did you know this?

1

Not at all

2

3

4

5

Perfectly

Q

Properties of halogens

A

LOW boiling points

- poor conductors

How well did you know this?

1

Not at all

2

3

4

5

Perfectly

Q

Properties of transition metals

A

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

How well did you know this?

1

Not at all

2

3

4

5

Perfectly

Q

Describe the properties of transition metal compounds

A

coloured
catalysts
multiple ions

How well did you know this?

1

Not at all

2

3

4

5

Perfectly

Q

When does ionic bonding occur

A

Between metals and non metals

How well did you know this?

1

Not at all

2

3

4

5

Perfectly

Q

When does covalent bonding occur

A

Between non metals only

How well did you know this?

1

Not at all

2

3

4

5

Perfectly

Q

Covalent bonding is…….

A

A shared pair of electrons

How well did you know this?

1

Not at all

2

3

4

5

Perfectly

Q

Ionic bonding is…..

A

Strong forces of attraction between oppositely charged ions

How well did you know this?

1

Not at all

2

3

4

5

Perfectly

Q

Why do ionic structures have such high MELTING points?

A

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

How well did you know this?

1

Not at all

2

3

4

5

Perfectly

Q

Why are ionic structures brittle?

A

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

Q

Structure of metals….

A

positive ions

- surrounded by a sea of delocalised electrons

Q

Alloy?

A

Mixture of two or more metals

Q

Why are alloys harder than individual metals?

A

ions of different sizes

- more difficult for layers to slide over each other

Q

Why does DIAMOND have such a high MELTING point

A

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

Q

Why does graphite conduct electricity

A

EACH carbon atom is only bonded to three others

- 4th electron free to move

Q

Why is graphite used as a lubricant

A

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

Q

Define polymer

A

A large molecule formed of many small monomers which JOIN together

Q

Define Thermosetting polymer

A

Can’t be heated and then RE shaped

Q

Define thermosoftening polymer

A

Can be heated and RE shaped

CHAINS ARE HELD TOGETHER BY WEAK INTERMOLECULAR FORCES WHICH ARE EASY TO RE SHAPE

Q

SOME examples of nanoscience in industry

A

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

Q

Method of titration

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

A

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.

Q

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

A

SOME product is lost
reversible reaction
reactant form unexpected products

Q

Reactivity series

A

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

Q

TEST for hydrogen

A

Lighted splint

Squeaky pop

Q

Hydrochloric acid+ sodium hydroxide—–>

Acid+ base= Salt+ WATER

A

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

Q

Metal+ acid= Salt+ hydrogen

Nitric acid+ magnesium——->

A

Magnesium nitrate + hydrogen

Q

Acid+ metal oxide——->

A

Salt+ WATER

Q

Acid+metal carbonate——->

A

Salt+ WATER + carbon dioxide

Q

PANIC

A

Positive anode

Negative is cathode