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Eddie - IGCSE Chemistry > Solids, liquids, and gases > Flashcards

Solids, liquids, and gases Flashcards

(74 cards)

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1
Q

What are the four state symbols

A

Aqueous (aq), Liquid (l), Gas (g), solid (s)

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2
Q

Describe structure of a solid

A

Particles arranged in a fixed lattice
Particles can vibrate

Properties - 
Fixed shape
Fixed volume
Do not flow
Higher density than liquids/ gases
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3
Q

Describe structure of a liquid

A

Particles close together
Particles can move about

Properties - 
Shape can change
Fixed volume
Can flow
Higher density than gas, lower than solids
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4
Q

Describe structure of a gas

A

Particles far apart
Particles move quickly

Properties - 
Shape can change
Volume can change
Can flow
Lower density than solid/ liquid
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5
Q

Definition of melting

A

Solid changes into liquid (at the melting point)

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6
Q

Definition of boiling

A

Liquid changes into a gas (at the boiling point)

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7
Q

Definition of freezing

A

Liquid changes into solid (at the freezing point)

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8
Q

Definition of condensation

A

Gas changes into liquid (at the boiling point)

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9
Q

Definition of sublimation

A

Solid changes into gas (without going through liquid state)

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10
Q

Definition of diffusion

A

The process by which particles in liquids and gases mix together or spread out by colliding with each other.

Particles move down a concentration gradient rom a high concentration to a low concentration.

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11
Q

What factors affect rate of diffusion

A

Tempurature - faster diffusion with higher temp

Molecular mass - higher molecular mass = slower diffusion

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12
Q

What is an experiment to demonstrate diffusion

A

There is a tube which at one end had cotton wool soaked in HCl and at the other soaked in Ammonia solution. a white ring of ammonia chloride forms where the two gases meet showing one has diffused quicker than the other

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13
Q

What is Brownian motion

A

The random movement of large particles in a gas or suspended in a liquid.

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14
Q

What causes Brownian motion

A

Caused by collision of molecules in the surrounding gas or liquid with the large particles

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15
Q

What evidence is there for Brownian motion

A

Pollen grains move randomly in water when observed under microscope
Dust particles move randomly in the air

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16
Q

What is an atom made up of

A

Protons, electrons and neutrons

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17
Q

What is a proton

A

Mass - 1
Charge - +1
Location - nucleus

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18
Q

What is a neutron

A

Mass - 1
Charge - 0
Location - nucleus

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19
Q

What is an electron

A

Mass - 1/2000
charge - -1
location - Shells orbiting the nucleus

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20
Q

What is the nucleon number

A

Total number of protons and neutrons

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21
Q

What is the proton number

A

Number of protons

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22
Q

What are valency electrons

A

The electrons in the most outer shell

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23
Q

How is the stability of atoms related to their electronic structure

A

Atoms with a full outer shell are stable

this is achieved by losing or gaining electrons

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24
Q

What is an atom

A

The smallest particle of a chemical element, which cannot be broken down any further (by chemical means)

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25
What is an element
A group of atoms which all have the same number of protons
26
What are isotopes
Atoms with the same number of protons but different numbers of neutrons
27
what is a compound
A substance in which two or more elements are chemically combined
28
What is a mixture
A combination of two or more substances that are not chemically combined
29
What is an ion
An atom where the number of electrons is different from the number of protons, so it has an overall charge Cation - A positively charged ion Anion - A negatively charged ion
30
What is an allotrope
Different forms of the same element e.g. diamond and graphite
31
Radioisotopes
Unstable isotopes which give out radiation when they decay, They can be used for Tracers, Radiotherapy, Sterilisation
32
What is ionic bonding
Occurs between metal and non-metal | Attraction between positive metal ions and negative non-metal ions
33
How are ions formed
Metals lose electrons to form positive ions | Non-metals gain electrons to form negative ions
34
What is covalent bonding
Occurs between non-metals | Covalent bonds are a shared pair of electrons
35
What are two types of covalent structure
Simple molecular | Giant covalent lattice
36
What is a molecule
a group of atoms being held together by covalent bonds
37
What are intermolecular forces
weak forces between covalently bonded molecules
38
Name three covalent macromolecules
Diamond, Graphite, Silicon (IV) Oxide
39
Properties of diamond
Hardest known substance, Does not conduct electricity, very high melting point, cut diamonds sparkle
40
Properties of Graphite
Soft and slippery, conducts electricity, dark in colour
41
Properties of silicon (IV) dioxide
Hard (can scratch things), doesn't conduct electricity, ,light passes through it, high melting point
42
What is metallic bonding
Occurs in metallic elements, The attraction between +ve metal ions and -ve electrons
43
Describe properties of metals
``` High mp and bp malleable and ductile good electrical conductors good heat conductors insoluble in water ```
44
What is an alloy
A mixture of a metal with other elements
45
Why are alloys more useful than pure metals
harder and stronger than pure metals, some are more resistant to corrosion
46
Define exothermic reaction
Reaction that gives out energy (temp increase)
47
Define endothermic reaction
Reaction that take in energy from surroundings (temp decrease)
48
What is bond energy
The energy required the break a particular bond
49
Equation for calculating energy change of reaction
Total energy of bonds broken - total energy of bonds formed
50
What four ways can energy be released
Burning fuels, nuclear fuels, fuel cells, electrochemical cells
51
What are "Photochemical reactions"
reactions which obtain the energy they need from light
52
What is a reversible reaction
A reaction that can take place in both directions
53
What is meant by equilibrium
The forward and backward reactions that take place at the same rate. No overall change in conc.
54
How is equilibrium affected by concentration, tempurature, pressure
equilibrium moves to the products side if reaction conc. increases, the product concentration decreases. If temp increases it becomes a endothermic reaction. If pressure increases equilibrium position moves to the side.
55
How is yield related by equilibrium position
The yield will be higher if the equilibrium if closer to the products side
56
Define "rate of reaction"
amount of reactant used up per unit time
57
what factors affect rate of reaction
increase the concentration, increase the tempurature, increase surface area, use a cataylst
58
What is "collision theory"
Where for two particles to react successfully they must collide with sufficient energy to break the necessary bonds
59
What is "empirical formula"
Shows the simplest ratio in which atoms combine to form a compound
60
What is "molecular formula"
shows the actual numbers of atoms that combine to form a molecule
61
What is "structural formula"
shows how the atoms are arranged in the molecule
62
What is "relative atomic mass"
The average mass of naturally occurring atoms of an element relative to the mass of carbon-12
63
What is "Relative formula mass"
the sum of the relative atomic masses
64
What is a "mole"
the amount of a substance that contains the same number of particles as the number of carbon atoms in 12g of carbon-12
65
What is "Avogadro constant"
The number of particles in one mole of an element or compound
66
What is "molar solution"
A solution that contains 1-mole of solute per dm3 of solution, written as 1mol/dm3
67
What is "molar volume of gas"
1 mole of gas occupies 24dm3 at room tempurature and pressure
68
What is the equation for number of moles
mass/molecular mass
69
What is the equation for concentration
molar concentration = amount of solute(g)/volume of solution mass conc. = amount of solute(mol)/ volume of solution
70
What is the equation for moles of a gas
volume of a gas (in dm3)/24dm3
71
What is the equation for percentage yield
actual mass obtained/ theoretical mass
72
What is the equation for percentage composition
total Ar of element in compound/ mr of compound x 100
73
What is the equation for percentage purity
mass of substance in mixture/total mass of mixture x 100
74
What does aqueous mean
Dissolved in water

Eddie - IGCSE Chemistry (5 decks)

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