Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

Chemistry Igcse > C1 + C2 > Flashcards

C1 + C2 Flashcards

You may prefer our related Brainscape-certified flashcards:
AP® Chemistry flashcards Periodic Table flashcards Chemistry 101 flashcards Organic Chemistry 101 flashcards
1
Q

What is the definition of matter?

A

Substance that occupies space and has mass

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

What are the three states of matter? What are their distinguishing properties?
Pressure
Volume
Density
Shape
Flow

A

Solid
Unaffected by change in pressure
Fixed volume
High density
Definite shape
Does not flow

Liquid
Slightly affected by change in pressure
Fixed volume
Moderate-high density
No definitely shape
Flows easily (generally)

Gas
Easily compressed
No fixed volume
Low density
No definitely shape
Flows easily

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

What are the particle structures of solids, gases and liquids?

A

Gas
Arranged irregularly
Spread far apart (relatively)
Able to move randomly

Liquid
Closely packed
Irregular arrangement
Able to move past each other

Solid
Pack close together
Regular arrangement
Cannot move freely (only vibrate)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

Name the changes in state.

A

Melting, boiling, evaporation, freezing, condensation

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

Define atom

A

The smallest part of an element (element- substance that is made of only one type of atom)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

Define molecule

A

More than 2 atoms
Can be formed by 2 of the same element or 2 different ones

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

Define Ion.

A

An atom (or group of atoms) that have a charge as a result of losing or gaining an electron
Cations -> lose electrons -> positive
Anions -> gain ions -> negative

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

Define melting point (including particle theory and energy change)

A

When a pure substance turns into a liquid
Endothermic -> particles heat up and move/spread out
Energy change -> absorb energy -> cooler surroundings

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

Define freezing point (including particle theory)

A

Liquid cooled down -> freezing point
Exothermic -> particles cool down, move less/ closer together
Energy change -> release energy -> surrounding hotter

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

Define evaporation (particle theory and energy change)

A

Liquid is left with surface exposed to air -> evaporation (gas)
Energy change -> absorb energy to become warmer -> cooler surroundings (endothermic)
Particles -> heat and spread

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

Define boiling (particle theory and energy change)

A

Gas forms inside a liquid -> boiling
Energy change -> absorb energy and warm -> surroundings are cooler (endothermic)
Particles -> heat and move

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

Define condensation (particle theory and energy change)

A

Gas cooled or pressure increased -> condensation (liquid)
Energy change -> release energy become cold -> hotter surroundings (exothermic)
Particles -> cool and move less

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

Define sublimation (energy change and particle theory)

A

Some solids do not melt when heated (at normal pressure) instead goes directly into gas -> sublimation (Called the same thing when the other way around)
Energy change -> releases or absorbs (direction of reaction)
Particles -> cool down or heat up (depends on direction of reaction)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

What the boiling point and freezing point of water (°C)? How can this be converted into Kelvin scale?

A

Boiling -> 100°
Freezing -> 0°
Kelvin -> add 273 to Celsius

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

Define particles. How does kinetic energy effect the particles?

A

All substances are made of particles
Particles move -> kinetic energy
More heat -> more kinetic energy

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

Define diffusion

A

The net movement of particles from a region of high concentration to a region of low concentration down a concentration gradient, as a result of their random movement

Passive process
Diffuse until equilibrium

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

What are some factors that effect diffusion?

A

Distance to travel, temp, concentration, state of matter (slow/nonexistent in solids, increased in liquids, fast in gases) , size of particles/molecules (slower diffusion)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

What is the cause of pressure?

A

Particles of gas colliding with the sides of the container, exerting force and keeping it expanded
Size of container and concentration of particles -> change pressure

19
Q

How are intervals of time measured?

A

Stopwatch

20
Q

How is temperature measured?

A

Thermometer

21
Q

How is mass measured?

A

Balances

22
Q

How are volumes and liquids measured?

A

Pipette (small amount)
-> digital pipette for extra precision
Burette
Volumetric flask
Gas syringe
Measuring cylinder

23
Q

What are the criteria of a pure substance?

A

It contains only one substance, containing no impurities
-> definite melting and boiling points
Ex: elements and compounds

24
Q

Define mixture

A

Impure -> contain more than two elements/compounds that aren’t chemically bonded

25
Q

Connection between pure substances and rising temps when melting

A

When a pure substance melts, the temperature will stop rising
-> because it is an endothermic process

(Unlike wax -> impure -> melts over a range of temps)

26
Q

What is paper chromatography?

A

Used to separate mixture of soluble substances by running a solvent through the mixture, causing the substances to move (they move at different rates)
Stationary phase -> paper
Mobile phase-> solvent

NEED TO BE SOLUBLE

27
Q

What is the Rf value?

A

The ratio of the distanced moved (from the origin)

28
Q

What is the equation of Rf value?

A

Rf=distance moved by substance/distance moved by solvent (solvent front)

Solvent always travel farther -> Rf<1

29
Q

What is ‘unique’ about pure compounds in chromatographs?

A

Pure compounds only produce one spot in ALL solvents

30
Q

Why is purity important in everyday life?

A

Medicinal drugs -> as pure as possible -> contamination could lead to harmful side effects
Colored dyes -> highly regulated -> many have harmful side effects

31
Q

What is ‘unique’ about the melting and boiling points of mixtures?

A

Each part of mixture boil at different temperatures and will melt/boil over a range of temps

32
Q

How can boiling and melting points be used to determine purity?

A

If the substance is pure the temp of the substance will stop increasing while boiling/melting -> definitive melting and boiling point

33
Q

How can different mixtures be separated?
Solid + solid (powder)
Suspension of solid in liquid
Liquid + liquid (not homogenous)
Solution of solid in liquid
Two or more liquids mixed together
Solution of two+ solids in liquids

A

Solid + solid (powder)
-> difference in property (magnetism, solubility, sublimation, density)

Suspension of solid in liquid
-> filtration or centrifugation

Liquid + liquid (not homogenous)
-> separating funnel or decantation

Solution of solid in liquid
->crystallization (for solid)
->distillation (liquid)

Two or more liquids mixed together
-> fractional distillation

Solution of two+ solids in liquids
-> chromatography

34
Q

Explain solubility (as a method of seperation)

A

Add mixture of solids to a solvent -> only one is soluble in
Pour liquid out (decant)
Repeat until solid is obtained

35
Q

Explain filtration

A

Solid material is collected in filter paper -> liquid passes through

36
Q

Explain centrifugation

A

Spin sample of solution very quickly -> solid goes to bottom because of higher density -> liquid decanted

37
Q

Explain crystallization

A

Solvent evaporated, leaving behind solute -> cools -> crystals

38
Q

Explain distillation

A

Separation of solute and solvent -> solvent evaporates at boiling point -> travels down condescending tube (tube surrounded by cool water) -> comes out as pure substance

39
Q

Explain fractional distillation

A

Separation by boiling point -> volatile liquids (evaporates at normal temps) travel up fractional column as well as water vapor -> volatile liquid vapor passes to the condenser (temp in column is above boiling point) -> water vapor condenses in the column (glass rods (more surface area) and cooler at top) -> flows back into flask

40
Q

Define solution

A

Made of a solvent (the liquid which it dissolves in) and solute (solid which dissolves)

41
Q

Define a concentrated and dilute solution

A

Concentrated-High proportion of solute
Dilute-low proportion of solute

42
Q

Define saturated solution

A

No more solid can be dissolved at this temperature

43
Q

Define solubility

A

The ability of a solute to dissolve in a solvent

44
Q

Define compound

A

More than 2 elements/compounds that are chemically combined

Chemistry Igcse (10 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2024 Bold Learning Solutions. Terms and Conditions