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GCSE Science > Chemistry Y9 > Flashcards

Chemistry Y9 Flashcards

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1
Q

What is an isotope?

A

Atoms of the same element and same number of protons but different number of neutrons

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2
Q

How many electrons would be in the outer shell of an element in group 7?

A

7 electrons in the outer shell

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3
Q

What is a molecule?

A

Two or more atoms of the same or different elements chemically bonded

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4
Q

Why is rubidium more reactive than potassium?

A

Rubidium is larger so the negative outer shell of electrons is further away from the positive nucleus. Therefore the electrostatic attractions weakens so its easier to lose electrons- therefore it’s more reactive

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5
Q

What did Rutherford conclude in the Alpha Scattering experiment?

A

Most of the particles went through - mostly empty space

Some were repelled - repelled by something positive

Some rebounded fully - Hit something small, dense and positive (nucleus)

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6
Q

What is the mass of protons, neutrons and electrons

A

Proton: 1
Neutron: 1
Electron: 0

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7
Q

What are the charges of electrons, protons and neutrons?

A

Proton: positively charged
Electron: negatively charged
Neutron: no charge

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8
Q

What is solubility?

A

A measure of how much a substance dissolves

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9
Q

What is a solvent?

A

A liquid that dissolves a substance

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10
Q

What is a solution?

A

Formed when a solid dissolves in a liquid

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11
Q

What is a solute?

A

A substance that dissolves in a liquid

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12
Q

What is retention Factor (Rf)

A

Measure of solubility

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13
Q

What is the law of the conservation of mass?

A

Mass of reactants = Mass of products
(No mass added or removed)
Exception:
If one of the reactants or one of the products is a gas then mass can appear to be gained or lost.

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14
Q

What are the properties of the transitional metals?

A

hard and strong
high melting and boiling point
form multiple ions
for coloured compounds
7 electrons in outer shell (group 7)
shiny
ductile
malleable
sononrous
central in the periodic table

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15
Q

What are the properties of the alkali metals?

A

soft to cut
low melting and boiling points
more reactive going down group
one electron in outer shell (group 1)
ductile
shiny
malleable
sonorous
metal

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16
Q

Properties of metals

A

Hard / strong
Conduct heat / electricity
High mpts
Malleable

17
Q

What are the giant covalent structures?

A

Diamond (SiO2)
Graphite
Graphene
Fullerene
Nanotube

18
Q

Metal + oxygen = ?

A

Metal oxide

19
Q

Metal + water =

A

Metal hydroxide + hydrogen

20
Q

Metal + acid = ?

A

Metal salt + hydrogen

21
Q

Properties of giant covalent structures?

A

High mpt + bpt (strong covalent bonds = lots of energy to overcome)
Hard and strong (e.g diamond)
Insoluble in water

22
Q

What is an alloy?

A

Mixture (not bonded) of two or more elements, at least one of which is a metal

23
Q

Why are alloys harder than pure metals?

A

Different sizes atoms disrupt the regular crystal lattice structure of a metal so the layers can no longer slide and the structure becomes harder

24
Q

How are covalent bonds formed?

A

By atoms sharing electrons

25
Q

Why do giant covalent structures have high melting points?

A

It takes a lot of energy to break the strong covalent bonds between the atoms

26
Q

Why does graphite conduct electricity?

A

The delocalized electrons can move through the graphite

27
Q

Explain why graphite is soft

A

Layers do not have strong covalent bonds so can slide over each other

28
Q

Give two properties of graphene

A

Strong
Conducts electricity

29
Q

Give two properties of nanotubes

A

High tensile strength
Conduct electricity

30
Q

Why do small covalent molecules have low melting points?

A

Only a small amount of energy is needed to overcome the weak intermolecular forces

31
Q

Describe the structure and bonding of polymers

A

Many identical molecules joined together by strong covalent bonds in a long chain, with weak intermolecular forces between the chains

32
Q

Why do ionic substances have high melting and boiling points?

A

Electrostatic attraction between positive metal ions and negative non metal ions is strong and requires lots of energy to overcome

33
Q

Properties of pure metals

A

Malleable
High melting + boiling points
Conduct electricity
Conduct thermal energy

34
Q

Why are alloys harder than pure metals

A

Different sizes atoms disturb the layers, preventing them from sliding over eachother

GCSE Science (2 decks)

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